2
1
3
The diagrams show particles in a container.
Cambridge International Examinations
Cambridge International General Certificate of Secondary Education (9–1)
4
1
2
In which atom is the number of protons equal to the number of neutrons?
40
A
3
5
Ar
Paper 1 Multiple Choice (Core)
May/June 2018
Which two diagrams show the process of evaporation?
*9935813517*
Multiple Choice Answer Sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
1→2
A
READ THESE INSTRUCTIONS FIRST
2
B
1→3
2→3
C
D
C
23
Na
alloy
pure metal
non-metal
carbon
copper
B
brass
copper
carbon
C
copper
brass
carbon
D
copper
carbon
brass
A
45 minutes
Additional Materials:
F
brass
0971/11
CHEMISTRY
19
B
D
16
O
Which row identifies an alloy, a pure metal and a non-metal?
3→1
Which piece of apparatus is used to measure exactly 26.3 cm3 of a liquid?
Write in soft pencil.
Do not use staples, paper clips, glue or correction fluid.
Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless
this has been done for you.
DO NOT WRITE IN ANY BARCODES.
A
B
C
6
D
A covalent molecule Q contains exactly six shared electrons.
What is Q?
A
ammonia, NH3
B
There are forty questions on this paper. Answer all questions. For each question there are four possible
answers A, B, C and D.
Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.
chlorine, Cl 2
C
methane, CH4
D
water, H2O
Read the instructions on the Answer Sheet very carefully.
7
Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
Any rough working should be done in this booklet.
A copy of the Periodic Table is printed on page 16.
Electronic calculators may be used.
3
The ‘lead’ in a pencil is made of a mixture of graphite and clay.
The melting points and boiling points of pure substances W, X and Y are shown.
W
X
Y
melting point / °C
–114
115
–101
boiling point / °C
78
445
–34
‘lead’
When the percentage of graphite is increased, the pencil slides across the paper more easily.
The substances are chlorine, ethanol and sulfur.
Which statement explains this observation?
Which row identifies W, X and Y?
A
Graphite has a high melting point.
W
X
Y
B
Graphite is a form of carbon.
A
chlorine
ethanol
sulfur
C
Graphite is a lubricant.
B
ethanol
sulfur
chlorine
D
Graphite is a non-metal.
C
sulfur
chlorine
ethanol
D
sulfur
ethanol
chlorine
This document consists of 14 printed pages and 2 blank pages.
IB18 06_0971_11/FP
© UCLES 2018
[Turn over
© UCLES 2018
4
8
© UCLES 2018
0971/11/M/J/18
5
The equation for the reaction between magnesium and dilute sulfuric acid is shown.
6
12 The diagram shows a rate of reaction experiment.
15 Dilute nitric acid is added to a solid, F.
The Mr of MgSO4 is 120.
A gas, G, is produced which is denser than air and extinguishes a burning splint.
Mg + H2SO4 → MgSO4 + H2
What are F and G?
hydrogen
Which mass of magnesium sulfate is formed when 12 g of magnesium completely reacts with
dilute sulfuric acid?
A
9
5g
B
10 g
C
60 g
D
120 g
negative electrode
Increasing the concentration of the acid and increasing the temperature both affect the rate of
reaction.
bubbles of a colourless gas
bubbles of a brown gas
B
bubbles of a colourless gas
bubbles of a colourless gas
C
shiny grey liquid
bubbles of a brown gas
D
shiny grey liquid
bubbles of a colourless gas
10 Which gas is used as a fuel?
argon
hydrogen
C
nitrogen
D
oxygen
solid F
gas G
A
calcium
hydrogen
B
calcium carbonate
carbon dioxide
C
calcium hydroxide
hydrogen
D
calcium oxide
carbon dioxide
Which row is correct?
positive electrode
A
B
excess dilute
hydrochloric acid at 25 °C
magnesium
What is observed at each electrode when molten lead(II) bromide is electrolysed using platinum
electrodes?
A
16 Which statement about oxides is correct?
increase the concentration
of acid
increase the temperature
A
A solution of magnesium oxide has a pH less than pH 7.
A
decrease rate of reaction
decrease rate of reaction
B
A solution of sulfur dioxide has a pH greater than pH 7.
B
decrease rate of reaction
increase rate of reaction
C
Magnesium oxide reacts with nitric acid to make a salt.
C
increase rate of reaction
decrease rate of reaction
D
Sulfur dioxide reacts with hydrochloric acid to make a salt.
D
increase rate of reaction
increase rate of reaction
17 Which methods are suitable for preparing both zinc sulfate and copper(II) sulfate?
13 Water is added to anhydrous copper(II) sulfate.
1
What happens during the reaction?
A
The copper(II) sulfate turns blue and the solution formed gets colder.
B
The copper(II) sulfate turns blue and the solution formed gets hotter.
11 Burning fuels is an exothermic reaction.
C
The copper(II) sulfate turns white and the solution formed gets colder.
What is meant by the term exothermic?
D
The copper(II) sulfate turns white and the solution formed gets hotter.
A
A gas is produced.
B
Energy is released.
C
Heat is absorbed.
A
C + O2 → CO2
D
The mass of the fuel decreases.
B
CaCO3 → CaO + CO2
A
reacting the metal oxide with warm dilute aqueous sulfuric acid
2
reacting the metal with dilute aqueous sulfuric acid
3
reacting the metal carbonate with dilute aqueous sulfuric acid
1, 2 and 3
B
1 and 2 only
C
1 and 3 only
C
CaO + 2HCl → CaCl 2 + H2O
D
N2O4 → 2NO2
© UCLES 2018
0971/11/M/J/18
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0971/11/M/J/18
7
© UCLES 2018
9
21 Which row shows the catalytic activity of transition elements and their compounds?
The table shows the results.
test
X
catalytic activity of
transition elements
catalytic activity of compounds of
transition elements
A
good
good
B
good
poor
C
poor
good
D
poor
poor
Y
a few drops of aqueous
sodium hydroxide are added
green precipitate
formed
red-brown
precipitate formed
a few drops of dilute nitric acid and
a few drops of barium nitrate are added
no change seen
white precipitate
formed
a few drops of dilute nitric acid and
a few drops of silver nitrate are added
white precipitate
formed
no change seen
24 Three metals, X, Y and Z, were reacted with water.
The oxides of the same three metals were also heated strongly with carbon.
The results are shown.
A
Noble gases are diatomic molecules.
Y
B
Noble gases are unreactive gases.
A
iron(II) chloride
iron(III) sulfate
C
Noble gases have full outer electron shells.
B
iron(III) chloride
iron(III) sulfate
D
The noble gas argon is used in lamps.
C
iron(II) sulfate
iron(III) chloride
reaction of the metal with water
X
vigorous reaction
with cold water
no reaction
Y
no reaction
metal and
carbon dioxide produced
Z
no reaction observed with cold water
but reaction observed with steam
no reaction
What is a correct conclusion about X, Y and Z?
23 The following statements are made about the metals copper, iron, magnesium and zinc.
iron(III) chloride
19 Which element is in the same period of the Periodic Table as silicon?
1
Their oxides are acidic.
2
They all conduct electricity in the solid state.
germanium
3
They all have high melting points.
B
scandium
4
They all react with dilute acids to form hydrogen.
C
sodium
Which statements are correct?
D
strontium
A
B
1 and 4
A sample of bromine reacts with potassium chloride solution.
B
A sample of bromine reacts with potassium iodide solution.
C
A sample of chlorine has a higher density than a sample of bromine.
D
A sample of chlorine is a darker colour than a sample of bromine.
© UCLES 2018
0971/11/M/J/18
X is sodium and Y is magnesium.
B
X is the least reactive and Y is the most reactive.
C
Z is less reactive than Y.
D
Z is magnesium and Y is copper.
Compound R is formed. Compound R then reduces the iron ore to iron.
Which equation shows the formation of compound R?
C
2 and 3
20 Which statement about the halogens is correct?
A
A
25 In a blast furnace, iron ore is mixed with coke and limestone, and heated in hot air.
A
1 and 2
reaction of the metal oxide
with carbon
metal
22 Which statement about the noble gases is not correct?
What are X and Y?
iron(III) sulfate
2 and 3 only
0971/11/M/J/18
8
18 Two salt solutions, X and Y, are tested.
X
D
14 Which equation shows an oxidation reaction?
© UCLES 2018
D
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0971/11/M/J/18
D
3 and 4
A
C + O2 → CO2
B
CO2 + C → 2CO
C
CaCO3 → CaO + CO2
D
CaO + SiO2 → CaSiO3
26 Which statement explains why aluminium is used in the manufacture of aircraft?
[Turn over
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0971/11/M/J/18
A
It conducts heat well.
B
It has a low density.
C
It is a good conductor of electricity.
D
It is easy to recycle.
© UCLES 2018
0971/11/M/J/18
[Turn over
10
11
27 Dry air is passed over hot copper until all the oxygen has reacted.
dry air
12
31 Which statement is correct?
copper
35 What is not the correct use of the fraction named?
A
Atmospheric carbon dioxide is not a cause of climate change.
B
Atmospheric methane is produced by respiration.
C
Burning natural gas decreases the level of carbon dioxide in the atmosphere.
D
Decomposition of vegetation causes an increase in atmospheric methane.
heat
The volume of gas at the end of the reaction is 120 cm .
What is the starting volume of dry air?
132 cm3
152 cm3
B
180 cm3
C
D
570 cm3
28 A steel bicycle which had been left outdoors for several months was starting to rust.
What would not reduce the rate of corrosion?
making waxes
B
gas oil
fuel in diesel engines
C
kerosene
jet fuel
D
naphtha
making chemicals
A
Sulfur dioxide is used as a food preservative.
B
Sulfur dioxide turns acidified aqueous potassium manganate(VII) from purple to colourless.
C
Sulfur forms a basic oxide.
D
Sulfur is used in the manufacture of sulfuric acid.
36 Four organic compounds are listed.
ethane
ethanoic acid
ethanol
ethene
33 Which process is used to convert limestone (calcium carbonate) into lime?
A
Remove the rust and paint the bicycle.
B
Remove the rust and store the bicycle in a dry shed.
C
Remove the rust and wipe the bicycle with a clean, damp cloth.
D
use
fuel oil
32 Which statement about sulfur and its compounds is not correct?
3
A
name of fraction
A
Remove the rust and wipe the bicycle with an oily cloth.
Which bond do all four compounds contain?
A
electrolysis
B
fractional distillation
C
incomplete combustion
D
thermal decomposition
A
C–C
B
C–H
C
F
29 Which statements about water are correct?
34 Lime is used to treat an industrial waste.
1
Household water contains dissolved salts.
2
Water for household use is filtered to remove soluble impurities.
3
Water is treated with chlorine to kill bacteria.
4
Water is used in industry for cooling.
A
1, 2, 3 and 4
B
1, 2 and 3 only
C
1, 3 and 4 only
D
2, 3 and 4 only
untreated
waste
Which change occurs in the treatment?
Which elements in the soil are replaced by adding fertilisers?
Ca, P, O
B
K, O, S
C
© UCLES 2018
N, K, P
D
treated waste
A
acidic
→
B
alkaline
→
acidic
C
alkaline
→
neutral
D
neutral
→
© UCLES 2018
neutral
acidic
[Turn over
0971/11/M/J/18
13
39 Which reaction is used to make ethanol?
A
O–H
C
F
F
F
F
C
C
F
F
F
F
F
F
F
C
C
C
F
F
F
F
A
because they contain fluorine and carbon atoms
B
because they have saturated bonds
C
because they have the same functional group
D
because they react differently from each other
38 Which substances can be obtained by cracking hydrocarbons?
N, O, S
0971/11/M/J/18
D
Why do these molecules represent a homologous series?
treated
waste
lime
30 Farmers use fertilisers to replace minerals in the soil that have been removed by the crops they
grow.
A
F
F
untreated waste
C–O
37 The first three members of a homologous series are shown.
A
ethanol and ethene
B
ethanol and hydrogen
C
ethene and hydrogen
D
ethene and poly(ethene)
© UCLES 2018
0971/11/M/J/18
14
15
BLANK PAGE
BLANK PAGE
adding steam to ethene
B
addition polymerisation
C
fractional distillation of petroleum
D
reacting ethene with aqueous bromine
40 Polymers are long-chain molecules made from small molecules linked together.
Four polymers or types of polymer are listed.
1
carbohydrates
2
nylon
3
proteins
4
Terylene
Which of these polymers or types of polymer are synthetic?
A
1 and 3
B
1 and 4
C
2 and 3
D
2 and 4
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
International Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at
www.cie.org.uk after the live examination series.
Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local
Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2018
0971/11/M/J/18
© UCLES 2018
0971/11/M/J/18
© UCLES 2018
0971/11/M/J/18
A student investigated the diffusion of ammonia gas, NH3, and hydrogen chloride gas, HCl.
–
Np
neptunium
–
U
The volume of one mole of any gas is 24 dm at room temperature and pressure (r.t.p.).
Lr
lawrencium
–
No
nobelium
Md
mendelevium
–
–
fermium
Fm
Es
einsteinium
–
–
Cf
californium
45 minutes
apparatus 1
Multiple Choice Answer Sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
apparatus 2
How long does it take for the damp blue litmus paper to change colour in apparatus 2?
READ THESE INSTRUCTIONS FIRST
Write in soft pencil.
Do not use staples, paper clips, glue or correction fluid.
Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless
this has been done for you.
DO NOT WRITE IN ANY BARCODES.
There are forty questions on this paper. Answer all questions. For each question there are four possible
answers A, B, C and D.
Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.
A
64 seconds
B
30 seconds
C
21 seconds
D
2
The blue litmus paper would not change colour.
Chromatography is a technique used to separate coloured dyes.
Which dye has an Rf value of 0.7?
Read the instructions on the Answer Sheet very carefully.
Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
Any rough working should be done in this booklet.
A copy of the Periodic Table is printed on page 16.
Electronic calculators may be used.
solvent front
baseline
A
B C
dyes
D
This document consists of 13 printed pages and 3 blank pages.
IB18 06_0971_21/FP
© UCLES 2018
damp blue
litmus paper
The damp red litmus paper in apparatus 1 changed colour after 30 seconds.
–
Bk
berkelium
curium
Cm
–
–
Am
americium
source of
hydrogen chloride gas
May/June 2018
3
231
Pa
232
–
protactinium
Th
thorium
Ac
actinium
actinoids
damp red
litmus paper
0971/21
CHEMISTRY
Additional Materials:
238
Pu
Two sets of apparatus were set up as shown at room temperature and pressure.
source of
ammonia gas
Paper 2 Multiple Choice (Extended)
–
103
Cambridge International Examinations
Cambridge International General Certificate of Secondary Education (9–1)
uranium
plutonium
175
102
71
Lu
lutetium
173
70
Yb
101
169
Tm
thulium
69
68
Er
167
erbium
100
99
165
Ho
holmium
67
66
163
Dy
dysprosium
98
97
159
Tb
terbium
65
64
96
157
Gd
gadolinium
95
152
Eu
europium
62
94
150
Sm
–
93
92
samarium
61
Pm
promethium
144
60
Nd
59
91
90
89
Pr
140
139
141
58
Ce
cerium
57
La
lanthanoids
lanthanum
praseodymium
neodymium
63
ytterbium
–
–
livermorium
Lv
Fl
flerovium
–
–
copernicium
Cn
Rg
roentgenium
–
–
darmstadtium
Ds
Mt
meitnerium
–
–
Hs
–
–
hassium
Bh
bohrium
Sg
seaborgium
–
Db
dubnium
–
–
–
Rf
Ra
radium
Fr
francium
rutherfordium
86
Rn
radon
–
85
At
astatine
–
116
Po
polonium
84
83
Bi
209
bismuth
lead
114
207
Pb
82
81
Tl
thallium
204
112
201
Hg
mercury
80
79
111
gold
197
Au
Pt
110
195
platinum
78
77
Ir
109
192
iridium
76
108
107
190
Os
186
106
osmium
75
Re
rhenium
184
74
W
tungsten
73
181
105
Hf
0971/11/M/J/18
178
72
55
Ta
actinoids
88
87
tantalum
104
89–103
137
133
hafnium
57–71
lanthanoids
56
Ba
barium
Cs
caesium
54
84
131
Xe
127
128
36
xenon
I
iodine
Te
tellurium
122
Sb
antimony
tin
Sn
119
115
indium
In
Cd
cadmium
112
108
silver
Ag
Pd
palladium
106
103
Rh
rhodium
101
Ru
–
96
ruthenium
Tc
technetium
Mo
molybdenum
Nb
niobium
93
91
zirconium
Zr
Y
88
85
89
Sr
strontium
Rb
rubidium
yttrium
53
80
79
52
51
75
73
50
49
70
65
48
47
64
59
46
45
59
44
43
42
56
55
52
51
41
40
37
48
39
40
38
39
45
40
Kr
krypton
Br
bromine
Se
selenium
As
arsenic
germanium
Ge
Ga
gallium
zinc
Zn
Cu
copper
nickel
Ni
Co
cobalt
iron
Fe
Mn
manganese
Cr
chromium
vanadium
V
Ti
Sc
Ca
calcium
K
20
19
potassium
24
23
titanium
18
27
26
25
23
21
magnesium
sodium
9
12
Mg
7
11
Na
22
name
atomic symbol
Be
beryllium
Li
lithium
relative atomic mass
atomic number
4
24
1
hydrogen
Key
3
scandium
35
34
33
32
28
29
30
31
20
Ar
neon
argon
35.5
chlorine
sulfur
32
31
phosphorus
silicon
28
27
aluminium
Ne
F
17
19
Cl
fluorine
16
16
O
oxygen
S
P
14
N
nitrogen
15
14
C
Si
carbon
12
11
B
13
Al
boron
2
4
6
5
III
Group
1
The Periodic Table of Elements
H
II
I
© UCLES 2018
2
1
*6954491355*
IV
7
V
8
VI
9
10
He
VIII
VII
helium
16
[Turn over
© UCLES 2018
0971/21/M/J/18
3
3
4
Which piece of apparatus is used to measure exactly 26.3 cm3 of a liquid?
A
B
C
5
5
Chlorine exists as two common isotopes, 35Cl and 37Cl.
9
Which statement about this solution is correct?
Information about these two isotopes is shown.
D
number of
neutrons
number of
electron shells
B
30 g of ethanoic acid is dissolved in 250 cm3 of water.
35
17
18
3
C
60 g of ethanoic acid is dissolved in 1 dm3 of water.
37
17
20
3
D
120 g of ethanoic acid is dissolved in 2 dm3 of water.
Cl
Which statement explains why the two isotopes are of the same element?
The ‘lead’ in a pencil is made of a mixture of graphite and clay.
6
‘lead’
A
Both have the same number of electron shells.
B
Both have the same number of protons.
C
Both have 7 outer shell electrons.
D
37
A
Graphite has a high melting point.
B
Graphite is a form of carbon.
C
Graphite is a lubricant.
D
Graphite is a non-metal.
Which statement is correct?
Which substance is not a macromolecule?
A
A reduction reaction occurs at the positive electrode.
B
The blue colour of the solution becomes darker.
C
The concentration of copper ions in the solution decreases.
D
The mass of the negative electrode increases.
diamond
B
When the percentage of graphite is increased, the pencil slides across the paper more easily.
Which statement explains this observation?
10 Aqueous copper(II) sulfate is electrolysed using copper electrodes.
Cl has 2 more neutrons than 35Cl.
A
11 Dilute sulfuric acid is electrolysed using inert electrodes.
graphite
C
silicon(IV) oxide
D
sulfur
What are the ionic half-equations for the reactions that take place at each electrode?
A
7
Copper is a metallic element.
Which statements about copper are correct?
A
8
1
Copper is malleable because layers of ions are in fixed positions and cannot move.
2
The structure of copper consists of negative ions in a lattice.
3
Copper conducts electricity because electrons can move through the metal.
4
Electrons hold copper ions together in a lattice by electrostatic attraction.
1 and 2
B
2, 3 and 4
C
2 and 3 only
D
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0971/21/M/J/18
B
24 dm3
C
© UCLES 2018
12 dm3
bond energy
in kJ / mol
less energy is released making bonds than is absorbed to break bonds
B
endothermic
more energy is released making bonds than is absorbed to break bonds
C
exothermic
less energy is released making bonds than is absorbed to break bonds
D
exothermic
more energy is released making bonds than is absorbed to break bonds
8
20 Which methods are suitable for preparing both zinc sulfate and copper(II) sulfate?
1
reacting the metal with dilute aqueous sulfuric acid
A
chlorine
iodide ions
D
iodine
H–H
+436
–263 kJ / mol
increasing concentration
increasing temperature
more collisions per second only
more collisions per second only
B
more collisions per second and more
collisions with sufficient energy to react
more collisions per second only
more collisions per second only
more collisions per second and more
collisions with sufficient energy to react
more collisions per second and more
collisions with sufficient energy to react
1, 2 and 3
A
germanium
B
scandium
A
A solution of magnesium oxide has a pH less than pH 7.
C
sodium
B
A solution of sulfur dioxide has a pH greater than pH 7.
D
strontium
C
Magnesium oxide reacts with nitric acid to make a salt.
D
Sulfur dioxide reacts with hydrochloric acid to make a salt.
A sample of bromine reacts with potassium iodide solution.
0.1 mol / dm3 ammonia solution
C
A sample of chlorine has a higher density than a sample of bromine.
D
A sample of chlorine is a darker colour than a sample of bromine.
A
3
B
0.1 mol / dm ethanoic acid
C
0.1 mol / dm3 lithium hydroxide
23 Which row shows the catalytic activity of transition elements and their compounds?
0.1 mol / dm3 nitric acid
D
Which row describes the solubility of the salts?
Which conditions produce the highest equilibrium yield of sulfur trioxide?
soluble
insoluble
A
silver nitrate
barium chloride, barium nitrate
and silver chloride
pressure
temperature
B
silver nitrate and barium chloride
barium nitrate and silver chloride
high
high
C
silver nitrate, barium chloride
and barium nitrate
silver chloride
D
silver nitrate, barium chloride
and silver chloride
barium nitrate
high
low
C
low
high
D
low
low
catalytic activity of
transition elements
catalytic activity of compounds of
transition elements
A
good
good
B
good
poor
C
poor
good
D
poor
poor
24 The following statements are made about the metals copper, iron, magnesium and zinc.
1
© UCLES 2018
0971/21/M/J/18
Their oxides are acidic.
2
They all conduct electricity in the solid state.
3
They all have high melting points.
4
They all react with dilute acids to form hydrogen.
Which statements are correct?
A
© UCLES 2018
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0971/21/M/J/18
9
1 and 2
B
1 and 4
© UCLES 2018
C
2 and 3
D
3 and 4
0971/21/M/J/18
10
25 Silver is a less reactive metal than cadmium.
2 and 3 only
A sample of bromine reacts with potassium chloride solution.
2AgNO3 + BaCl 2 → 2AgCl + Ba(NO3)2
B
D
B
The forward reaction is exothermic.
A
1 and 3 only
A
The equation is shown.
2SO3(g)
C
18 Which solution has the lowest pH?
The equation is shown.
2SO2(g) + O2(g)
1 and 2 only
22 Which statement about the halogens is correct?
19 A student mixes silver nitrate and barium chloride to form a white precipitate of silver chloride.
15 The formation of sulfur trioxide is a reversible reaction.
B
21 Which element is in the same period of the Periodic Table as silicon?
17 Which statement about oxides is correct?
D
reacting the metal oxide with warm dilute aqueous sulfuric acid
reacting the metal carbonate with dilute aqueous sulfuric acid
C
–103 kJ / mol
[Turn over
0971/21/M/J/18
3
B
more collisions per second and more
collisions with sufficient energy to react
explanation
endothermic
chloride ions
+193
A
D
type of
energy change
A
A
+366
14 Which row describes the effects of increasing both concentration and temperature on the
collisions between reacting particles?
C
2H+ + 2e– → H2
2
H–Br
C
4OH– + 4H+ → 4H2O
What is the oxidising agent?
Br–Br
+103 kJ / mol
2H+ + 2e– → H2
D
Cl 2 + 2I– → I2 + 2Cl –
What is the energy change for the reaction?
B
4OH– → 2H2O + O2 + 4e–
© UCLES 2018
16 Chlorine displaces iodide ions from potassium iodide.
2HBr(g) → H2(g) + Br2(g)
+263 kJ / mol
2H + 2e → H2
C
7
The bond energies are shown in the table. The reaction is endothermic.
A
4OH– + 4H+ → 4H2O
B
6 dm3
0971/21/M/J/18
6
13 Hydrogen bromide decomposes to form hydrogen and bromine. The equation is shown.
bond
D
–
Which row describes and explains the energy change that occurs?
2C2H6 + 7O2 → 4CO2 + 6H2O
48 dm3
negative electrode
4OH– → 2H2O + O2 + 4e–
+
3 and 4 only
The equation for the combustion of ethane is shown.
A
positive electrode
2H+ + 2e– → H2
12 Plant cells use energy from sunlight for photosynthesis.
Which volume of carbon dioxide, at room temperature and pressure, is formed when 0.5 moles of
ethane burn?
© UCLES 2018
20 g of ethanoic acid is dissolved in 10 cm3 of water.
A
number of
protons
Cl
4
A solution of ethanoic acid, CH3COOH, has a concentration of 2 mol / dm3.
11
29 A steel bicycle which had been left outdoors for several months was starting to rust.
33 Which statement about sulfur and its compounds is not correct?
Cadmium is a less reactive metal than barium.
What would not reduce the rate of corrosion?
A
Sulfur dioxide is used as a food preservative.
Which statement is correct?
A
Remove the rust and paint the bicycle.
B
Sulfur dioxide turns acidified aqueous potassium manganate(VII) from purple to colourless.
A
Barium does not react when heated with silver oxide.
B
Remove the rust and store the bicycle in a dry shed.
C
Sulfur forms a basic oxide.
B
Cadmium displaces barium from a solution of barium chloride.
C
Remove the rust and wipe the bicycle with a clean, damp cloth.
D
Sulfur is used in the manufacture of sulfuric acid.
C
Cadmium displaces silver from a solution of silver nitrate.
D
Remove the rust and wipe the bicycle with an oily cloth.
D
Cadmium reacts when heated with barium oxide.
34 Which process is used to convert limestone (calcium carbonate) into lime?
A
electrolysis
Household water contains dissolved salts.
B
fractional distillation
2
Water for household use is filtered to remove soluble impurities.
C
incomplete combustion
3
Water is treated with chlorine to kill bacteria.
D
thermal decomposition
4
Water is used in industry for cooling.
30 Which statements about water are correct?
26 Aluminium metal is extracted from aluminium oxide using electrolysis.
1
Which statement about the extraction process is not correct?
A
A large amount of electricity is required.
B
Molten cryolite is used to dissolve the aluminium oxide.
C
Oxygen gas is released which reacts to form carbon dioxide.
A
1, 2, 3 and 4
D
The negative electrodes burn away and have to be replaced.
B
1, 2 and 3 only
C
1, 3 and 4 only
D
2, 3 and 4 only
27 Which statement explains why aluminium is used in the manufacture of aircraft?
A
35 What is not the correct use of the fraction named?
It conducts heat well.
31 Ammonia is manufactured by reacting hydrogen with nitrogen in the Haber process.
B
It has a low density.
C
It is a good conductor of electricity.
D
It is easy to recycle.
Which row describes the sources of hydrogen and nitrogen and the conditions used in the
manufacture of ammonia in the Haber process?
source of
hydrogen
source of
nitrogen
temperature of
reaction / °C
A
air
natural gas
250
2
B
air
natural gas
250
200
C
natural gas
air
450
2
D
natural gas
air
450
200
28 Dry air is passed over hot copper until all the oxygen has reacted.
dry air
copper
pressure of
reaction / atm
heat
32 Which statements about the carbon cycle are correct?
The volume of gas at the end of the reaction is 120 cm3.
What is the starting volume of dry air?
A
132 cm3
B
152 cm3
C
180 cm3
D
570 cm3
A
© UCLES 2018
0971/21/M/J/18
[Turn over
1
Carbon dioxide is added to the atmosphere by respiration.
2
Carbon dioxide is added to the atmosphere by combustion of coal.
3
Carbon dioxide is removed from the atmosphere by photosynthesis.
1, 2 and 3
© UCLES 2018
name of fraction
use
fuel oil
making waxes
B
gas oil
fuel in diesel engines
C
kerosene
jet fuel
D
naphtha
making chemicals
A
B
1 and 2 only
C
1 and 3 only
0971/21/M/J/18
D
36 Which reaction is not a reaction which alkenes undergo?
A
bromination
B
hydration
C
hydrogenation
D
hydrolysis
37 Which substances can be obtained by cracking hydrocarbons?
A
ethanol and ethene
B
ethanol and hydrogen
C
ethene and hydrogen
D
ethene and poly(ethene)
2 and 3 only
© UCLES 2018
0971/21/M/J/18
[Turn over
12
38 Ethanol is produced by fermentation or from ethene.
13
14
BLANK PAGE
BLANK PAGE
What is a disadvantage of producing ethanol by fermentation?
A
Distillation is needed to purify the ethanol produced.
B
Fermentation uses glucose from plants.
C
Fermentation is catalysed by enzymes in yeast.
D
Fermentation occurs at a low temperature and pressure.
39 Which structural formula represents methyl propanoate?
A
CH3CH2COOCH3
B
CH3COOCH2CH2CH3
C
CH3CH2CH2COOCH3
D
HCOOCH2CH2CH3
40 Which row describes addition polymerisation and condensation polymerisation?
addition polymerisation
condensation polymerisation
A
monomers have a C=C double bond
and the polymer is the only product
monomers have a C=C double bond
and the polymer is the only product
B
monomers have a C=C double bond
and the polymer is the only product
the monomers react to form the
polymer and a small molecule
C
the monomers react to form the
polymer and a small molecule
monomers have a C=C double bond
and the polymer is the only product
D
the monomers react to form the
polymer and a small molecule
the monomers react to form the
polymer and a small molecule
© UCLES 2018
0971/21/M/J/18
© UCLES 2018
0971/21/M/J/18
15
© UCLES 2018
0971/21/M/J/18
16
0971/21/M/J/18
© UCLES 2018
–
Candidates answer on the Question Paper.
No Additional Materials are required.
Write your Centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
The volume of one mole of any gas is 24 dm at room temperature and pressure (r.t.p.).
Lr
–
lawrencium
No
nobelium
–
Fm
–
–
Es
einsteinium
–
–
Cf
californium
–
curium
–
–
Bk
berkelium
Cm
Am
americium
Pu
plutonium
Np
neptunium
–
238
U
1 hour 15 minutes
Answer all questions.
Electronic calculators may be used.
A copy of the Periodic Table is printed on page 12.
You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
231
232
–
Pa
Th
thorium
Ac
actinium
protactinium
3
uranium
May/June 2018
Paper 4 Theory (Extended)
READ THESE INSTRUCTIONS FIRST
actinoids
62
fermium
Md
102
mendelevium
71
103
173
101
175
Lu
70
Yb
ytterbium
169
69
Tm
thulium
68
Er
167
erbium
100
99
165
67
Ho
holmium
66
98
163
97
96
Dy
159
157
95
94
dysprosium
65
Tb
terbium
64
Gd
gadolinium
152
150
63
Eu
europium
Sm
samarium
–
61
Pm
promethium
93
92
144
Nd
neodymium
60
59
91
90
89
Pr
140
139
141
58
Ce
cerium
57
La
lanthanum
praseodymium
0971/41
CHEMISTRY
This document consists of 12 printed pages.
IB18 06_0971_41/FP
© UCLES 2018
[Turn over
0971/21/M/J/18
2
1
lanthanoids
Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local
Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2018
lutetium
–
–
livermorium
Lv
Fl
flerovium
–
–
Cn
copernicium
–
–
–
–
Rg
roentgenium
Ds
darmstadtium
Mt
meitnerium
Hs
hassium
–
bohrium
Bh
Sg
seaborgium
–
–
Db
dubnium
–
–
–
76
Rf
Ra
radium
Fr
francium
rutherfordium
Rn
radon
86
–
85
At
–
116
astatine
84
Po
polonium
209
83
Bi
bismuth
lead
114
207
Pb
82
81
204
Tl
thallium
80
112
201
Hg
mercury
111
79
gold
197
Au
78
110
Pt
195
109
108
platinum
192
190
77
Ir
iridium
Os
osmium
75
107
186
rhenium
Re
W
106
184
tungsten
74
73
181
105
Hf
178
72
55
Ta
actinoids
88
87
tantalum
104
89–103
137
133
hafnium
57–71
lanthanoids
56
Ba
barium
Cs
caesium
54
84
131
Xe
xenon
I
127
128
122
iodine
Te
tellurium
Sb
tin
119
115
In
indium
108
112
Cd
silver
106
103
101
Ag
Pd
palladium
Rh
rhodium
Ru
Tc
–
96
molybdenum
Mo
Nb
niobium
93
91
Zr
zirconium
80
Y
88
85
yttrium
Sr
strontium
Rb
rubidium
89
technetium
ruthenium
cadmium
Sn
antimony
52
51
36
53
79
75
73
50
49
70
48
47
65
64
46
45
44
59
59
56
55
43
42
52
51
41
40
37
48
39
40
38
39
45
40
krypton
Kr
Br
bromine
Se
selenium
As
arsenic
Ge
zinc
germanium
Ga
gallium
Zn
Cu
copper
Ni
iron
nickel
Co
cobalt
Fe
manganese
Mn
Cr
chromium
vanadium
V
Ti
Sc
Ca
calcium
K
20
19
potassium
24
23
titanium
27
26
25
24
23
21
magnesium
sodium
9
12
Mg
7
11
Na
22
name
atomic symbol
Be
beryllium
Li
lithium
relative atomic mass
atomic number
4
3
Key
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
International Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at
www.cie.org.uk after the live examination series.
scandium
18
35
28
29
30
31
32
34
20
Ar
neon
argon
33
35.5
32
chlorine
sulfur
31
28
27
aluminium
silicon
phosphorus
Ne
F
17
S
P
19
16
15
Cl
16
14
fluorine
O
oxygen
N
nitrogen
14
C
Si
carbon
12
11
B
13
Al
6
5
boron
2
4
9
8
7
10
He
VIII
VI
III
1
hydrogen
Group
1
The Periodic Table of Elements
H
II
I
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
Cambridge International Examinations
Cambridge International General Certificate of Secondary Education (9 –1)
*4799018190*
IV
V
VII
helium
BLANK PAGE
4
3
(i)
Substances can be classified as elements, compounds or mixtures.
(a) What is meant by the term compound ?
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [2]
2
Apparatus X needs to have cold water flowing through it.
●
Draw an arrow on the diagram to show where the cold water enters apparatus X.
●
Name apparatus X.
(ii)
●
Draw on the diagram the part of the fractionating column which is missing.
●
xplain why the experiment will not work with this part of the fractionating column
E
missing.
Give the order and the correct scientific term for the physical processes used to separate the
common salt from the mixture.
. ............................................................................................................................................
1 .................................................................................................................................................
. ............................................................................................................................................
[2]
(iii)
3 .................................................................................................................................................
[4]
A
B
C
D
boiling point / °C
56
78
122
160
.............................................................................................................................................. [1]
(b) In which period of the Periodic Table is flerovium?
.............................................................................................................................................. [1]
(c) Predict the number of outer shell electrons in an atom of flerovium.
.............................................................................................................................................. [1]
Suggest why a Bunsen burner is not used to heat the flask.
(d) Two isotopes of flerovium are 286Fl and 289Fl. The nuclei of both of these isotopes are unstable
and emit energy when they split up.
A hot water bath cannot be used to separate alcohols C and D.
(i)
State the term used to describe isotopes with unstable nuclei.
(ii)
omplete the table to show the number of protons, neutrons and electrons in the atoms of
C
the isotopes shown.
. ...................................................................................................................................... [1]
Explain why.
. ............................................................................................................................................
. ............................................................................................................................................
(c) A
student suggested that the apparatus shown could be used to separate the mixture of
alcohols.
isotope
. ...................................................................................................................................... [2]
The nucleus of one atom of plutonium combined with the nucleus of one atom of element Z.
his formed the nucleus of one atom of flerovium.
T
Suggest the identity of element Z.
. ...................................................................................................................................... [1]
(iv)
The boiling points of four different alcohols, A, B, C and D, are shown.
alcohol
●●
●●
Part of the fractionating column is missing. This means that the experiment will not work.
sequence of physical processes can be used to separate common salt (sodium chloride)
A
from a mixture containing sand and common salt only.
2 .................................................................................................................................................
(a) F
lerovium was made by bombarding atoms of plutonium, Pu, atomic number 94, with atoms of
element Z.
. ............................................................................................................................................
[2]
(b) Mixtures can be separated by physical processes.
Flerovium, Fl, atomic number 114, was first made in research laboratories in 1998.
[Total: 13]
286
Fl
289
Fl
number of protons
number of neutrons
number of electrons
[2]
(e) O
nly a relatively small number of atoms of flerovium have been made in the laboratory and the
properties of flerovium have not yet been investigated.
X
fractionating column
It has been suggested that flerovium is a typical metal.
(i)
Suggest two physical properties of flerovium.
1 . .........................................................................................................................................
hot water
2 . .........................................................................................................................................
[2]
mixture of
alcohols
A, B, C and D
(ii)
electric heater
Suggest one chemical property of flerovium oxide.
. ...................................................................................................................................... [1]
© UCLES 2018
0971/41/M/J/18
© UCLES 2018
0971/41/M/J/18
[Turn over
© UCLES 2018
[Total: 9]
0971/41/M/J/18
6
5
3
This question is about iron.
4
(a) T
hree of the raw materials added to a blast furnace used to extract iron from hematite are
coke, hematite and limestone.
7
(d) A 1.68 g sample of phosphorus was burned and formed 3.87 g of an oxide of phosphorus.
This question is about masses, volumes and moles.
(a) Which term is defined by the following statement?
Calculate the empirical formula of this oxide of phosphorus.
The average mass of naturally occurring atoms of an element
on a scale where the 12C atom has a mass of exactly 12 units.
Name one other raw material added to the blast furnace.
.............................................................................................................................................. [1]
.............................................................................................................................................. [1]
(b) A series of reactions occurs in a blast furnace during the extraction of iron from hematite.
(b) Butane, C4H10, has a relative molecular mass of 58.
Potassium fluoride, KF, has a relative formula mass of 58.
escribe these reactions.
D
Include:
●● one chemical equation for the reduction of hematite
●● one chemical equation for the formation of slag.
xplain why the term relative molecular mass can be used for butane but cannot be used for
E
potassium fluoride.
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [2]
....................................................................................................................................................
....................................................................................................................................................
empirical formula = ............................. [4]
(e) A
nother oxide of phosphorus has the empirical formula P2O3.
One molecule of this oxide of phosphorus contains four atoms of phosphorus.
(c) A 0.095 g sample of gaseous element Y occupies 60.0 cm3 at room temperature and pressure.
....................................................................................................................................................
●●
Determine the number of moles of element Y in 60.0 cm3.
●●
Calculate the relative molecular mass of element Y and hence suggest the identity of
element Y.
Calculate the mass of one mole of this oxide of phosphorus.
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [5]
moles of element Y = ............................. mol
(c) The iron extracted from hematite using a blast furnace is impure.
mass = ............................. g [2]
[Total: 12]
Identify the main impurity in this iron and explain how it is removed in the steel‑making process.
main impurity ..............................................................................................................................
how it is removed .......................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
[3]
[Total: 9]
© UCLES 2018
[Turn over
0971/41/M/J/18
relative molecular mass = .............................
identity of element Y = .............................
[3]
© UCLES 2018
0971/41/M/J/18
8
5
[Turn over
0971/41/M/J/18
9
(a) T
he table gives some chemical properties of transition elements and their compounds, and of
Group I elements and their compounds.
(i)
© UCLES 2018
chemical property
transition elements
Group I elements
ability to act as catalysts
yes
no
exist as coloured compounds
yes
no
(d) The reaction between zinc and dilute sulfuric acid can be catalysed by the addition of aqueous
copper(II) sulfate.
Cambridge International Examinations
Cambridge International General Certificate of Secondary Education (9 –1)
On the diagram, add the energy profile for the catalysed reaction.
What is meant by the term catalyst?
energy Zn(s) + H2SO4(aq)
. ............................................................................................................................................
. ...................................................................................................................................... [2]
(ii)Give one other chemical property shown by transition elements which is not shown by
Group I elements.
progress of reaction
[1]
(e) A student electrolyses aqueous copper(II) sulfate using the apparatus shown.
. ...................................................................................................................................... [1]
power supply
*9567793711*
. ............................................................................................................................................
0971/61
CHEMISTRY
May/June 2018
Paper 6 Alternative to Practical
1 hour
Candidates answer on the Question Paper.
No Additional Materials are required.
READ THESE INSTRUCTIONS FIRST
(b)Give two physical properties shown by transition elements which are not shown by Group I
elements.
–
+
1 .................................................................................................................................................
2 .................................................................................................................................................
[2]
Write your Centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
carbon electrodes
aqueous
copper(II) sulfate
(c) T
he energy level diagram shows the energy profile for the reaction between zinc and dilute
sulfuric acid.
Answer all questions.
Electronic calculators may be used.
You may lose marks if you do not show your working or if you do not use appropriate units.
Oxygen gas forms at the positive electrode (anode).
(i)
Write an ionic half‑equation for the reaction at the negative electrode (cathode). Include
state symbols.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
. ...................................................................................................................................... [3]
energy Zn(s) + H2SO4(aq)
(ii)
Describe what the student observes at the negative electrode.
. ...................................................................................................................................... [1]
(iii)Give two other observations which the student makes during the electrolysis.
progress of reaction
1 . .........................................................................................................................................
(i)
Complete the diagram by adding the formulae of the products. Include state symbols. [3]
(ii)
Draw an arrow on the diagram to represent the activation energy.
(iii)
Is the reaction endothermic or exothermic? Explain your answer.
[1]
2 . .........................................................................................................................................
[2]
(iv)
. ............................................................................................................................................
. ...................................................................................................................................... [1]
© UCLES 2018
0971/41/M/J/18
hat difference would the student observe at the positive electrode if the aqueous
W
copper(II) sulfate were replaced by concentrated aqueous copper(II) chloride?
This document consists of 11 printed pages and 1 blank page.
. ...................................................................................................................................... [1]
[Total: 18]
© UCLES 2018
0971/41/M/J/18
2
IB18 06_0971_61/FP
© UCLES 2018
4
3
1The volume of dilute nitric acid that reacts with 25.0 cm3 of aqueous potassium hydroxide can be
found by titration using the apparatus shown.
(d)The equation for the reaction taking place in the titration is shown.
HNO3 + KOH
2
A student investigated the rate of reaction between dilute hydrochloric acid and aqueous
sodium thiosulfate. When these chemicals react they form a precipitate which makes the solution
go cloudy. The formation of this precipitate can be used to show how fast the reaction proceeds.
KNO3 + H2O
The student concluded that the aqueous potassium hydroxide was more concentrated than the
dilute nitric acid.
...........................................
[Turn over
[Turn over
Five experiments were done using the apparatus shown.
eye
Explain whether or not the student’s conclusion was correct.
.....................................................................................................................................................
10 cm3 of dilute hydrochloric acid
.....................................................................................................................................................
dilute nitric acid
............................................................................................................................................... [2]
250 cm3 conical flask
[Total: 8]
aqueous sodium thiosulfate
25.0 cm of aqueous
potassium hydroxide
with indicator
3
printed sheet of paper
(a)Complete the box to name the apparatus.
printed words
[1]
(b)Name a suitable indicator that could be used.
............................................................................................................................................... [1]
A student did the titration four times and recorded the following results.
(c) (i)
titration number
volume of dilute nitric acid / cm3
1
18.1
2
18.9
3
18.3
4
18.2
Which one of the results is anomalous?
........................................................................................................................................ [1]
(ii)Suggest what might have caused this result to be anomalous.
........................................................................................................................................ [1]
(iii)Use the other results to calculate the average volume of dilute nitric acid that reacted with
the aqueous potassium hydroxide.
........................................................................................................................................ [2]
© UCLES 2018
0971/61/M/J/18
© UCLES 2018
0971/61/M/J/18
[Turn over
© UCLES 2018
0971/61/M/J/18
6
5
●
●
●
large measuring cylinder was used to pour 50 cm3 of aqueous sodium thiosulfate into a
A
250 cm3 conical flask. The conical flask was placed on a printed sheet of paper.
10 cm3 of dilute hydrochloric acid was added to the solution in the conical flask. A timer was
started immediately and the mixture was swirled.
The time taken for the printed words to disappear from view was measured.
7
(a)Record the volumes of distilled water used in the table. Use the stop-clock diagrams to record
the results in the table.
Experiment 1
experiment
volume of
aqueous sodium
thiosulfate / cm3
volume of
distilled water
/ cm3
stop-clock diagram
Experiment 2
●
●
●
0
210
180
1
45 15
50
5
10
15
minutes
30
Experiment 3
●
240
time taken for
the printed words
to disappear
from view / s
seconds
0
The large measuring cylinder was used to pour 40 cm3 of aqueous sodium thiosulfate into a
conical flask, followed by 10 cm3 of distilled water. The conical flask was placed on the printed
sheet of paper.
10 cm3 of dilute hydrochloric acid was added to the solution in the conical flask. The timer was
started immediately and the mixture was swirled.
The time taken for the printed words to disappear from view was measured.
(b)Plot the results from Experiments 1–5 on the grid. Draw a smooth line graph.
150
time taken for
the printed words
to disappear
from view / s
120
0
0
xperiment 2 was repeated but using 35 cm3 of aqueous sodium thiosulfate and 15 cm3 of
E
distilled water.
2
40
45 15
5
15
Experiment 4
●
10
xperiment 2 was repeated but using 30 cm3 of aqueous sodium thiosulfate and 20 cm3 of
E
distilled water.
0
Experiment 5
●
90
30
0
xperiment 2 was repeated but using 10 cm3 of aqueous sodium thiosulfate and 40 cm3 of
E
distilled water.
3
35
60
45 15
5
15
30
10
30
0
0
0
4
30
45 15
5
10
0
20
30
40
50
volume of aqueous sodium thiosulfate / cm3
15
[3]
10
30
(c) (i)
From your graph, deduce the time taken for the printed words to disappear from view
if Experiment 2 were repeated using 20 cm3 of aqueous sodium thiosulfate and 30 cm3 of
distilled water.
0
0
Show clearly on the grid how you worked out your answer.
5
10
45 15
5
15
.............................. s [2]
10
30
[3]
© UCLES 2018
0971/61/M/J/18
[Turn over
© UCLES 2018
0971/61/M/J/18
8
3
1
time taken
Solid B was zinc carbonate.
tests on solution A
Complete the expected observations.
(c)Dilute nitric acid was added to solid B. The gas produced was tested.
observations
observations ...............................................................................................................................
Solution A was divided into three equal portions
in three test-tubes.
In which experiment, 1, 2, 3, 4 or 5, was the rate of reaction greatest?
........................................................................................................................................ [1]
(ii)
tests on solid B
Some of the tests and observations are shown.
........................................................................................................................................ [1]
(d) (i)
10
Two substances, solution A and solid B, were analysed.
tests on solution A
Calculate the rate of reaction using your answer from (c)(i).
Explain, in terms of particles, why the rate of reaction was greatest in this experiment.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(e)Give the name of a more accurate piece of apparatus for measuring volumes than a measuring
cylinder.
............................................................................................................................................... [2]
test 1
The pH of the first portion of solution A was
tested.
The zinc nitrate solution formed in the test in (c) was divided into two portions in two test‑tubes.
pH = 1
(d) (i)
Magnesium ribbon was added to the second
portion of solution A.
The gas produced was tested.
(ii)
An excess of aqueous sodium hydroxide was then added to the mixture.
effervescence
observations .................................................................................................................. [1]
gas ‘popped’ with a lighted splint
(e) (i)
Drops of aqueous ammonia were added to the second portion of the zinc nitrate solution.
test 3
observations .................................................................................................................. [1]
Dilute nitric acid and aqueous barium nitrate
were added to the third portion of solution A.
white precipitate formed
(ii)An excess of aqueous ammonia was then added to the mixture.
.....................................................................................................................................................
............................................................................................................................................... [2]
rops of aqueous sodium hydroxide were added to the first portion of the zinc nitrate
D
solution.
observations .................................................................................................................. [2]
test 2
............................................................................................................................................... [1]
(f)Suggest the effect on the results of using a 100 cm3 conical flask instead of a 250 cm3 conical
flask. Explain your answer.
[Turn over
0971/61/M/J/18
9
(ii)The rate of reaction can be calculated using the equation shown.
rate of reaction =
© UCLES 2018
observations .................................................................................................................. [1]
(a)Identify the gas produced in test 2.
[Total: 10]
............................................................................................................................................... [1]
(g)Sketch on the grid the graph you would expect if all of the experiments were repeated at a
lower temperature. Clearly label your graph.
[1]
[Total: 16]
© UCLES 2018
0971/61/M/J/18
(b)Identify solution A.
............................................................................................................................................... [2]
© UCLES 2018
0971/61/M/J/18
11
12
4Potassium chloride is a salt that dissolves in water.
The solubility of a salt is the mass in grams of the salt that dissolves in 100 cm3 of water at a
particular temperature.
BLANK PAGE
[Turn over
© UCLES 2018
0971/61/M/J/18
Cambridge Assessment International Education
Cambridge International General Certificate of Secondary Education (9–1)
Plan an investigation to determine the solubility of potassium chloride in water at 40 °C.
You are provided with potassium chloride and common laboratory apparatus.
0971/11
CHEMISTRY
............................................................................................................................................................
Paper 1 Multiple Choice (Core)
............................................................................................................................................................
May/June 2019
45 minutes
Additional Materials:
*5786315246*
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
Multiple Choice Answer Sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
READ THESE INSTRUCTIONS FIRST
Write in soft pencil.
Do not use staples, paper clips, glue or correction fluid.
Write your name, centre number and candidate number on the Answer Sheet in the spaces provided unless
this has been done for you.
DO NOT WRITE IN ANY BARCODES.
There are forty questions on this paper. Answer all questions. For each question there are four possible
answers A, B, C and D.
Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.
...................................................................................................................................................... [6]
[Total: 6]
Read the instructions on the Answer Sheet very carefully.
Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
Any rough working should be done in this booklet.
A copy of the Periodic Table is printed on page 16.
Electronic calculators may be used.
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable
effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will
be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International
Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after
the live examination series.
Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local
Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2018
0971/61/M/J/18
[Turn over
© UCLES 2018
0971/61/M/J/18
This document consists of 15 printed pages and 1 blank page.
IB19 06_0971_11/FP
© UCLES 2019
[Turn over
2
1
3
Sodium chloride is a liquid at 900 °C.
4
motion of particles
regular
vibrate about a fixed point
A
B
2
regular
8
Which chromatogram shows an insoluble colour?
How are the particles arranged and how do the particles move in sodium chloride at 900 °C?
arrangement of particles
4
The colours in four dyes are separated using chromatography.
A
Which statement describes graphite?
B
C
D
move randomly
C
random
vibrate about a fixed point
D
random
move randomly
9
baseline
2.00 g of powdered calcium carbonate is added to 50.0 cm3 of hydrochloric acid.
3
Which statement about an atom of fluorine, 199 F, is correct?
balance
burette
A
B
balance
thermometer
B
It contains a total of 28 protons, neutrons and electrons.
C
pipette
burette
C
Its isotopes contain different numbers of protons.
D
pipette
thermometer
D
Its nucleus contains 9 neutrons.
6
Sodium chloride is soluble in water but not in hexane.
Sand is insoluble in both water and hexane.
What is required to separate the sand from the sodium chloride?
A
1
filter paper
2
fractionating column
3
hexane
4
water
1 and 3
B
7
1 and 4
C
© UCLES 2019
2 and 3
D
It contains more protons than neutrons.
Different metal oxides are added to four of the test-tubes and the height of the foam formed after
1 minute is measured. The results are shown.
D
172
substance
anode product
A
concentrated aqueous sodium chloride
hydrogen
cathode product
chlorine
chlorine
oxygen
oxygen
hydrogen
What happens when a calcium ion forms during this reaction?
D
molten lead bromide
lead
bromine
A
The calcium atom gains one electron.
B
The calcium atom gains two electrons.
C
The calcium atom loses one electron.
D
The calcium atom loses two electrons.
11 Dissolving ammonium chloride in water is an endothermic change.
Which row shows the energy change and temperature change of the mixture during the
dissolving of ammonium chloride?
Which row describes the formation of single covalent bonds in methane?
A
atoms share a pair of electrons
both atoms gain a
noble gas electronic structure
B
atoms share a pair of electrons
both atoms have the same number
of electrons in their outer shell
C
electrons are transferred from one
atom to another
both atoms gain a
noble gas electronic structure
D
electrons are transferred from one
atom to another
both atoms have the same number
of electrons in their outer shell
energy change
temperature change
A
energy is absorbed
decrease
B
energy is absorbed
increase
C
energy is released
decrease
D
energy is released
increase
12 Which process is a physical change?
[Turn over
0971/11/M/J/19
A
burning wood
B
cooking an egg
C
melting an ice cube
D
rusting iron
© UCLES 2019
0971/11/M/J/19
7
18 How could crystals of a pure salt be prepared from dilute sulfuric acid?
15 In a blast furnace, iron is extracted when iron(III) oxide reacts with carbon monoxide.
The equation is shown.
Fe2O3 + 3CO → 2Fe + 3CO2
Which substance is oxidised and which is reduced?
oxidised
reduced
CO
Fe2O3
A
add an excess of aqueous sodium hydroxide, filter, evaporate the filtrate to crystallisation
point
B
add an excess of copper(II) carbonate, filter, evaporate the filtrate to dryness
C
add an excess of copper metal, filter, evaporate the filtrate to crystallisation point
D
add an excess of zinc oxide, filter, evaporate the filtrate to crystallisation point
A
no metal oxide added
0.1
B
CO2
Fe
aluminium oxide
0.1
C
Fe
CO2
test
observation
calcium oxide
0.2
D
Fe2O3
CO
add ammonia solution
green precipitate formed
copper(II) oxide
2.3
add dilute nitric acid followed
by aqueous barium nitrate
white precipitate formed
manganese(IV) oxide
5.4
19 The results of two tests on a solution of compound Q are shown.
16 Four different solutions are separately tested with blue litmus and with methyl orange. Each
solution is known to be either acidic or alkaline. The results are shown.
Metal oxides do not affect the rate of this reaction.
solution
result with
blue litmus
result with
methyl orange
All metal oxides increase the rate of this reaction and act as catalysts.
1
red
red
C
Manganese(IV) oxide is the best catalyst of the four metal oxides tested.
2
red
yellow
D
Only transition element oxides increase the rate of this reaction.
3
blue
yellow
4
blue
yellow
14 When blue-green crystals of nickel(II) sulfate are heated, water is produced and a yellow solid
remains. When water is added to the yellow solid, the blue-green colour returns.
Which process describes these changes?
reversible reaction
148
dilute sulfuric acid
B
D
C
concentrated hydrochloric acid
A
neutralisation
134
C
Which conclusion can be drawn from these results?
corrosion
B
height of
foam / cm
metal oxide
C
86
6
Five test-tubes are half filled with hydrogen peroxide solution. A drop of liquid detergent is added
to each one.
B
The compound magnesium nitrate has the formula Mg(NO3)2.
B
5
combustion
It has no free electrons, so does not conduct electricity.
Calcium reacts with chlorine to produce calcium chloride.
© UCLES 2019
13 Hydrogen peroxide solution decomposes very slowly at room temperature to produce oxygen
gas. This gas forms a rising foam when liquid detergent is added.
A
It has layers, which can slide over each other.
D
Which row describes the electrode products?
2 and 4
0971/11/M/J/19
It has four strong covalent bonds between each carbon atom.
C
10 Four substances are electrolysed using inert electrodes.
A
Rock salt is a mixture of sand and sodium chloride.
It has a strong, rigid three-dimensional structure.
B
A
5
hydrochloric acid
A
What is the relative formula mass of magnesium nitrate?
Which apparatus is used to measure the calcium carbonate and the hydrochloric acid?
calcium carbonate
Diamond and graphite have giant covalent structures of carbon atoms.
What is Q?
iron(II) chloride
A
iron(II) sulfate
B
C
iron(III) chloride
D
iron(III) sulfate
20 The properties of an element are shown.
Which statement is correct?
A
Solutions 1 and 4 are acidic.
B
Solutions 1 and 2 are alkaline.
C
Solutions 3 and 4 are alkaline.
D
Solutions 3 and 4 are acidic.
electrical conductivity
density
reaction with water
high
low
reacts violently with cold water
Which element has these properties?
17 The positions of elements W, X, Y and Z in the Periodic Table are shown.
A
B
C
D
W
21 Which statement about elements in Group I and Group VII of the Periodic Table is correct?
Y
Z
X
Which elements form basic oxides?
A
© UCLES 2019
[Turn over
0971/11/M/J/19
W, X and Y
B
W and X only
© UCLES 2019
C
Y only
D
Z only
Iodine is a monoatomic non-metal.
C
Lithium has a higher melting point than potassium.
D
Sodium is more reactive with water than potassium.
10
25 The reactions of three metals, P, Q and R, are shown.
28 Water can be treated by filtration then chlorination.
melting
point
density
forms coloured
compounds
metal reacts with
dilute hydrochloric acid
metal reacts
with water
A
high
low
no
P
yes
no
B
high
high
yes
Q
no
no
C
low
low
no
R
yes
yes
D
low
low
yes
Which uses do not need water of this quality?
1
A
water for cooling in industry
2
water for washing clothes
3
water for drinking
1, 2 and 3
B
1 and 2 only
A
They all have a full outer shell of electrons.
B
They all react with Group I elements to form ionic compounds.
C
They are all diatomic molecules.
D
They are all liquids at room temperature.
24 The diagrams show the structure of two substances used to make electrical conductors.
Y
most
reactive
X is a pure metal and Y is a compound.
B
X is a pure metal and Y is an alloy.
C
X is a solid and Y is a liquid.
D
X is harder and stronger than Y.
© UCLES 2019
1 and 3 only
Q
1
burning fossil fuels containing sulfur
R
2
nitrogen reacting with oxygen in car engines
P
3
incomplete combustion of carbon fuels
P
4
adding lead compounds to petrol
A
P
B
Q
R
C
R
Q
D
R
P
Q
2 and 3 only
D
3 and 4
Which sources produce acid rain?
A
26 Iron is extracted from its ore in a blast furnace.
Hematite, coke, limestone and hot air are added to the furnace.
1 and 2
B
1 and 3
C
P
A
Coke burns and produces a high temperature.
B
Hematite is the ore containing the iron as iron(III) oxide.
C
Hot air provides the oxygen for the burning.
D
Limestone reduces the iron(III) oxide to iron.
2 and 3
30 The diagram shows an experiment to investigate how paint affects the rusting of iron.
Q
iron
painted iron
air
water
27 Why is aluminium used to make containers for storing food?
0971/11/M/J/19
D
29 Four sources of air pollution are listed.
least
reactive
Which explanation is not correct?
A
C
What is the order of reactivity of the metals?
23 Which statement about elements in Group VIII of the Periodic Table is correct?
Which statement correctly describes X and Y?
[Turn over
0971/11/M/J/19
9
22 Which row describes the properties of a transition element?
X
Bromine reacts with potassium chloride to produce chlorine.
B
© UCLES 2019
0971/11/M/J/19
8
A
A
It conducts electricity.
B
It has a high melting point.
C
It is resistant to corrosion.
D
It is strong.
© UCLES 2019
What happens to the water level in tubes P and Q?
tube P
0971/11/M/J/19
[Turn over
tube Q
A
falls
rises
B
no change
rises
C
rises
falls
D
rises
no change
© UCLES 2019
0971/11/M/J/19
11
12
31 A mixture of two substances, R and S, is heated.
13
33 The diagram represents a lime kiln used to heat limestone to a very high temperature.
The damp red litmus paper turns blue.
35 Which fuel could be gasoline?
waste gases
damp red
litmus paper
Is it obtained
from petroleum?
lime kiln
yes
no
limestone
Is it used as
fuel for cars?
R and S
fuel in
yes
gentle heat
air in
air in
X
S
A
a basic oxide
ammonium chloride
B
a basic oxide
sodium nitrate
A
calcium carbonate
C
an acidic oxide
ammonium chloride
B
calcium hydroxide
D
an acidic oxide
sodium nitrate
C
calcium oxide
D
calcium sulfate
What leaves the kiln at X?
name of W
H
H
H
C
C
H
C
B
H
H
H
H
C
C
H
H
D
H
H
H
C
O
C
H
H
OH
H
H
C
C
H
H
C
C
H
H
H
H
H
C
C
H
H
ethane
B
OH
H
H
ethene
C
H
H
C
C
H
H
C
C
H
ethene
D
[Turn over
0971/11/M/J/19
© UCLES 2019
15
16
© UCLES 2019
0971/11/M/J/19
© UCLES 2019
0971/11/M/J/19
© UCLES 2019
Cambridge Assessment International Education
Cambridge International General Certificate of Secondary Education (9–1)
0971/21
CHEMISTRY
Paper 2 Multiple Choice (Extended)
May/June 2019
45 minutes
Additional Materials:
*4098257922*
Multiple Choice Answer Sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
2
A
Ammonia expands to occupy all of the space available.
B
Ammonia has a smaller relative molecular mass than hydrogen chloride.
C
Ammonia is an alkali and hydrogen chloride is an acid.
D
Ammonia molecules diffuse in all directions at the same time.
2.00 g of powdered calcium carbonate is added to 50.0 cm3 of hydrochloric acid.
4
5
Write in soft pencil.
Do not use staples, paper clips, glue or correction fluid.
Write your name, centre number and candidate number on the Answer Sheet in the spaces provided unless
this has been done for you.
DO NOT WRITE IN ANY BARCODES.
There are forty questions on this paper. Answer all questions. For each question there are four possible
answers A, B, C and D.
Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.
3
balance
burette
B
balance
thermometer
C
pipette
burette
D
pipette
thermometer
The measurements from a chromatography experiment using substance F are shown. The
diagram is not drawn to scale.
Read the instructions on the Answer Sheet very carefully.
6
solvent front
Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
Any rough working should be done in this booklet.
A copy of the Periodic Table is printed on page 16.
Electronic calculators may be used.
–
The volume of one mole of any gas is 24 dm at room temperature and pressure (r.t.p.).
lawrencium
Lr
No
nobelium
–
–
mendelevium
Md
Fm
fermium
–
–
einsteinium
Es
Cf
californium
–
–
Bk
berkelium
curium
Cm
–
–
americium
Am
Pu
plutonium
–
–
neptunium
Np
U
238
uranium
3
231
Pa
232
–
protactinium
Th
thorium
Ac
actinium
actinoids
71
175
Lu
103
102
173
Yb
ytterbium
70
69
101
169
thulium
Tm
Er
167
erbium
100
99
165
Ho
holmium
68
66
163
Dy
dysprosium
98
97
159
Tb
terbium
65
64
157
Gd
gadolinium
96
95
152
Eu
europium
63
62
94
Sm
samarium
150
–
61
Pm
promethium
93
92
144
Nd
neodymium
60
59
91
90
Pr
140
89
141
58
Ce
cerium
57
praseodymium
67
A
It contains more protons than neutrons.
B
It contains a total of 28 protons, neutrons and electrons.
C
Its isotopes contain different numbers of protons.
D
Its nucleus contains 9 neutrons.
Which row describes the formation of single covalent bonds in methane?
hydrochloric acid
A
139
Which statement about an atom of fluorine, 199 F, is correct?
Which apparatus is used to measure the calcium carbonate and the hydrochloric acid?
calcium carbonate
La
3
Which statement explains why ammonia gas, NH3, diffuses at a faster rate than
hydrogen chloride gas, HCl ?
READ THESE INSTRUCTIONS FIRST
lanthanum
0971/11/M/J/19
2
1
lanthanoids
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
lutetium
–
Lv
livermorium
–
–
flerovium
Fl
Cn
copernicium
–
–
roentgenium
Rg
Ds
darmstadtium
–
–
meitnerium
Mt
Hs
hassium
–
–
bohrium
Bh
Sg
seaborgium
–
–
Db
dubnium
–
–
–
Rf
Ra
radium
Fr
francium
rutherfordium
Rn
radon
86
85
At
astatine
–
–
116
Po
polonium
84
83
Bi
209
bismuth
lead
114
207
Pb
82
81
Tl
thallium
204
112
201
Hg
mercury
80
79
111
gold
197
Au
78
Pt
110
195
platinum
77
Ir
192
iridium
109
108
190
Os
osmium
76
75
107
186
rhenium
Re
W
106
184
tungsten
74
73
181
105
72
Hf
178
lanthanoids
57–71
Ta
88
87
tantalum
104
actinoids
137
133
hafnium
89–103
56
Ba
barium
55
Cs
caesium
54
84
Xe
xenon
36
131
127
iodine
I
Te
tellurium
128
122
Sb
antimony
tin
119
Sn
In
indium
115
112
Cd
cadmium
silver
Ag
108
106
palladium
Pd
Rh
rhodium
103
101
ruthenium
Ru
Tc
technetium
–
96
molybdenum
Mo
Nb
niobium
93
91
zirconium
Zr
Y
89
88
yttrium
Sr
strontium
80
53
52
79
75
51
50
73
49
70
65
48
47
64
59
46
45
59
56
44
43
55
52
42
41
51
48
40
39
37
45
40
38
39
40
krypton
Kr
Br
bromine
selenium
Se
As
arsenic
germanium
Ge
Ga
gallium
zinc
Zn
Cu
Mn
Cr
V
Ti
Sc
20
19
copper
18
24
23
22
21
magnesium
sodium
9
12
Mg
7
11
Na
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
nickel
Ni
Co
35
34
29
atomic symbol
Be
beryllium
Li
lithium
23
atomic number
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
cobalt
3 and 4
4
2 and 3
3
C
Key
1 and 4
II
B
Ca
proteins
calcium
4
1 and 2
I
A
K
salts
potassium
nylon
3
24
2
iron
D
complex carbohydrates
25
1
Fe
2 and 4
manganese
D
chromium
1 and 4
vanadium
C
titanium
1 and 3
40 Which naturally occurring polymers are found in foods?
scandium
B
33
30
Ethanoic acid has a pH lower than pH 7.
28
4
1 and 2
27
Ethanoic acid turns Universal Indicator paper blue.
26
Ethanoic acid reacts with carbonates to produce hydrogen.
3
Group
Ethanoic acid contains the functional group –COOH.
2
The Periodic Table of Elements
A
32
20
Ar
neon
argon
39 Which statements about aqueous ethanoic acid are correct?
1
31
35.5
chlorine
sulfur
32
31
phosphorus
silicon
28
27
aluminium
Ne
F
19
Cl
fluorine
17
16
16
O
oxygen
S
P
14
N
nitrogen
15
14
12
C
Si
10
9
8
7
6
carbon
11
B
13
Al
boron
2 and 3 only
name
D
relative atomic mass
1 and 3 only
5
C
III
1 and 2 only
2
It burns in air and can be used as a fuel.
B
4
It is an unsaturated compound.
IV
It can be made by fermentation.
3
1, 2 and 3
He
VIII
VI
V
38 Which statements about ethanol are correct?
A
helium
VII
Ethanol contains the same functional group as other alcohols but propane does not.
1
Ethanol is a liquid but propane is a gas.
D
hydrogen
Ethanol can be made from ethene but propane is obtained from petroleum.
C
1
Ethanol has two carbon atoms per molecule but propane has three.
B
H
A
2
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BLANK PAGE
37 Why is ethanol a member of the homologous series of alcohols but propane is not?
1
H
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0971/11/M/J/19
14
H
H
H
© UCLES 2019
H
85
It dissolves in water to form acid rain.
ethane
A
Rb
It can be used to manufacture sulfuric acid.
D
structure of W
rubidium
It can be used to kill bacteria in food.
C
D
W decolourises bromine water.
A
B
no
C
What is the name of W and what is its structure?
34 What is the structure of ethanol?
It can be used as a bleach when making wood pulp.
yes
B
36 A hydrocarbon W burns to form carbon dioxide and water.
32 Which statement describes a disadvantage of sulfur dioxide?
A
no
A
What are R and S?
R
Is it used as
fuel for cars?
fuel in
A
atoms share a pair of electrons
both atoms gain a
noble gas electronic structure
B
atoms share a pair of electrons
both atoms have the same number
of electrons in their outer shell
C
electrons are transferred from one
atom to another
both atoms gain a
noble gas electronic structure
D
electrons are transferred from one
atom to another
both atoms have the same number
of electrons in their outer shell
Which statement describes the structure of an ionic compound?
A
It is a giant lattice of oppositely charged ions.
B
It is a giant lattice of positive ions in a ‘sea’ of electrons.
C
It is a giant molecule of oppositely charged ions.
D
It is a simple molecule of oppositely charged ions.
distance moved by F
7
Propane burns in oxygen.
100 mm
90 mm
55 mm
C3H8 + xO2 → 3CO2 + yH2O
Which values of x and y balance the equation?
A
15 mm
baseline
What is the Rf value of F?
A
0.55
B
0.61
C
0.90
D
1.64
x
y
5
4
B
7
4
C
10
8
D
13
8
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4
8
5
A tablet contains 0.080 g of ascorbic acid (Mr = 176).
What is the concentration of ascorbic acid when one tablet is dissolved in 200 cm3 of water?
9
A
9.1 × 10–5 mol / dm3
B
–4
4.5 × 10 mol / dm
C
9.1 × 10–2 mol / dm3
D
2.3 × 10–3 mol / dm3
6
12 Nitrogen reacts with hydrogen to produce ammonia.
15 The graph shows how the yield of product in a reversible reaction changes as the temperature
and pressure are changed.
N2 + 3H2 → 2NH3
All reactants and products are gases.
The reaction is exothermic. The bond energies are shown in the table.
reactants
3
bond
bond energy
in kJ / mol
Which statement about the electrolysis of copper(II) sulfate solution using carbon electrodes is
correct?
N≡N
945
H–H
436
N–H
390
A
A colourless gas is produced at the anode.
What is the energy change for this reaction?
B
A colourless gas is produced at the cathode.
A
–1473 kJ / mol
C
The colour of the electrolyte remains the same.
B
–87 kJ / mol
D
The mass of both electrodes remains constant.
C
87 kJ / mol
D
1473 kJ / mol
yield of
product
pressure
Which row is correct for this reversible reaction?
13 Which change in reaction conditions increases both the collision rate and the proportion of
molecules with sufficient energy to react?
ionic half-equation
electrode
A
addition of a catalyst
A
2O2– → O2 + 2e–
anode
B
increasing the concentration of a reactant
B
Al 3+ + 3e– → Al
anode
C
increasing the surface area of a reactant
D
increasing the temperature of the reaction
2–
C
2O
–
cathode
D
Al 3+ + 3e– → Al
cathode
→ O2 + 4e
A
Chemical energy is converted into electrical energy.
B
Hydrogen is oxidised.
C
The reaction that takes place is endothermic.
D
Water is the only product.
side of reaction
with fewer moles
forward
reaction
A
reactant
exothermic
B
reactant
endothermic
C
product
endothermic
D
product
exothermic
16 Which changes represent oxidation?
1
2I– → I2 + 2e–
2
Cr(VI) → Cr(III)
3
Fe(II) → Fe(III)
1 and 2
B
14 When blue-green crystals of nickel(II) sulfate are heated, water is produced and a yellow solid
remains. When water is added to the yellow solid, the blue-green colour returns.
11 Which statement about the hydrogen fuel cell is not correct?
Which process describes these changes?
A
combustion
B
corrosion
C
neutralisation
D
reversible reaction
300 °C
100 °C
10 Aluminium metal is extracted from aluminium oxide by electrolysis.
Which ionic half-equation describes a reaction that occurs at the named electrode?
products
A
1 and 3
C
1 only
D
2 only
17 Nitrogen(I) oxide, N2O, nitrogen(II) oxide, NO, and carbon monoxide, CO, are all non-metal
oxides.
They do not react with acids or bases.
Which statement is correct?
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7
Y
B
W and X only
C
Y only
D
Z only
Hydrochloric acid is a strong acid.
Which statements are correct?
0971/21/M/J/19
24 Three metal compounds, P, Q and R, are heated using a Bunsen burner.
Bromine reacts with potassium chloride to produce chlorine.
B
Iodine is a monoatomic non-metal.
P
colourless gas produced, which relights a glowing splint
C
Lithium has a higher melting point than potassium.
Q
colourless gas produced, which turns limewater milky
D
Sodium is more reactive with water than potassium.
R
no reaction
The results are shown.
A
They all have a full outer shell of electrons.
P
Q
B
They all react with Group I elements to form ionic compounds.
A
magnesium carbonate
potassium carbonate
potassium nitrate
C
They are all diatomic molecules.
B
magnesium carbonate
potassium nitrate
potassium carbonate
D
They are all liquids at room temperature.
C
potassium nitrate
magnesium carbonate
potassium carbonate
D
potassium nitrate
potassium carbonate
magnesium carbonate
Ethanoic acid molecules are partially dissociated into ions.
X
1.0 mol / dm3 ethanoic acid has a higher pH than 1.0 mol / dm3 hydrochloric acid.
3
Ethanoic acid is always more dilute than hydrochloric acid.
4
Ethanoic acid is a proton acceptor.
B
1 and 3
C
R
D
density
high
3 and 4
Which statement correctly describes X and Y?
reaction with water
low
25 Zinc is extracted from its ore, zinc blende, using two chemical reactions.
Y
1
2ZnS + 3O2 → 2ZnO + 2SO2
2
2ZnO + C → 2Zn + CO2
Which substance is reduced in reactions 1 and 2?
2 and 4
20 The properties of an element are shown.
electrical conductivity
Which row shows the identity of P, Q and R?
23 The diagrams show the structure of two substances used to make electrical conductors.
2
1 and 2
They are neutral oxides.
© UCLES 2019
A
22 Which statement about elements in Group VIII of the Periodic Table is correct?
19 Ethanoic acid is a weak acid.
A
They are basic oxides.
D
Z
X
Which elements form basic oxides?
1
They are amphoteric oxides.
C
9
21 Which statement about elements in Group I and Group VII of the Periodic Table is correct?
W
W, X and Y
They are acidic oxides.
B
8
18 The positions of elements W, X, Y and Z in the Periodic Table are shown.
A
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A
reacts violently with cold water
reaction 1
reaction 2
A
X is a pure metal and Y is a compound.
A
O2
C
B
X is a pure metal and Y is an alloy.
B
O2
ZnO
C
X is a solid and Y is a liquid.
C
ZnS
C
D
X is harder and stronger than Y.
D
ZnS
ZnO
Which element has these properties?
A
B
C
D
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10
11
26 Four metals, zinc, M, copper and magnesium, are reacted with aqueous solutions of their
nitrates.
12
29 Oxides of nitrogen are formed in car engines and are a source of air pollution.
32 The carbon cycle is shown.
To decrease this pollution, catalytic converters are fitted to car exhausts.
atmospheric
carbon dioxide
The results are shown.
What happens to the oxides of nitrogen in the catalytic converter?
metal
magnesium
nitrate
M
nitrate
copper
nitrate
zinc
nitrate
key
= no reaction
magnesium
zinc
M
copper
= reacts
A
combustion
B
cracking
C
oxidation
D
reduction
A
copper → zinc → M → magnesium
copper → M → zinc → magnesium
C
magnesium → M → zinc → copper
D
magnesium → zinc → M → copper
It conducts electricity.
B
It has a high melting point.
C
It is resistant to corrosion.
D
It is strong.
P
death and excretion
Q
painted iron
animals
Which row describes processes X, Y and Z?
air
X
water
What happens to the water level in tubes P and Q?
tube P
Which uses do not need water of this quality?
A
water for cooling in industry
2
water for washing clothes
3
water for drinking
1, 2 and 3
B
1 and 2 only
tube Q
A
falls
rises
B
no change
rises
C
rises
falls
D
rises
no change
Z
respiration
combustion
photosynthesis
B
respiration
photosynthesis
combustion
C
photosynthesis
combustion
respiration
D
photosynthesis
respiration
combustion
temperature
/ °C
pressure
/ atm
25
2
B
25
200
iron
C
450
2
vanadium(V) oxide
D
450
200
vanadium(V) oxide
A
N2(g) + 3H2(g)
1 and 3 only
Y
A
33 Which row shows the conditions used in the Contact process?
31 Ammonia is manufactured by the Haber Process.
C
green plants
dead
organic matter
30 The diagram shows an experiment to investigate how paint affects the rusting of iron.
iron
28 Water can be treated by filtration then chlorination.
1
Y
Z
27 Why is aluminium used to make containers for storing food?
A
X
respiration
decomposition
What is the order of reactivity of these four metals starting with the most reactive?
B
D
2 and 3 only
2NH3(g)
catalyst
iron
The forward reaction is exothermic.
Which conditions maximise the yield of ammonia?
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pressure
temperature
A
high
high
B
high
low
C
low
high
D
low
low
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13
14
34 The diagram represents a lime kiln used to heat limestone to a very high temperature.
15
40 The structure of a polymer is shown.
36 Why is ethanol a member of the homologous series of alcohols but propane is not?
waste gases
lime kiln
A
Ethanol has two carbon atoms per molecule but propane has three.
B
Ethanol can be made from ethene but propane is obtained from petroleum.
C
Ethanol is a liquid but propane is a gas.
D
Ethanol contains the same functional group as other alcohols but propane does not.
O
type of polymer
limestone
fuel in
B
calcium hydroxide
C
calcium oxide
D
calcium sulfate
formed by
carbohydrate
addition polymerisation
B
carbohydrate
condensation polymerisation
Which statements are correct?
C
polyester
addition polymerisation
D
polyester
condensation polymerisation
air in
What leaves the kiln at X?
calcium carbonate
O
A
X
A
O
37 Chlorine reacts with methane.
fuel in
air in
O
Which type of polymer is shown and by which process is it formed?
A
1
The reaction takes place in the dark.
2
The reaction of chlorine with methane forms chloromethane.
3
Chloromethane reacts with chlorine to produce dichloromethane.
4
The reaction of chlorine with methane is an addition reaction.
1 and 2
B
1 and 3
C
2 and 3
D
3 and 4
38 Which statements about aqueous ethanoic acid are correct?
1
35 Which fuel could be gasoline?
Is it obtained
from petroleum?
yes
A
Ethanoic acid contains the functional group –COOH.
2
Ethanoic acid reacts with carbonates to produce hydrogen.
3
Ethanoic acid turns Universal Indicator paper blue.
4
Ethanoic acid has a pH lower than pH 7.
1 and 2
B
1 and 3
C
1 and 4
D
2 and 4
39 The structure of an ester is shown.
no
O
Is it used as
fuel for cars?
Is it used as
fuel for cars?
yes
yes
CH3
C
OCH2CH2CH3
no
A
B
no
C
What is the name of the ester?
D
A
ethyl propanoate
B
methyl propanoate
C
propyl ethanoate
D
propyl methanoate
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2019
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0971/21/M/J/19
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0971/21/M/J/19
2
–
231
232
–
B
N
Candidates answer on the Question Paper.
N
No Additional Materials are required.
N
Cu Cu Cu Cu
N
Cu Cu Cu Cu
Cu Cu Cu Cu
N
N
Cu Cu Cu Cu
D
Write your centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
E
(a) A
nswer the following questions about these structures.
Each structure may be used once, more than once or not at all.
(i)Which two of these structures, A, B, C, D or E, are covalently bonded?
Answer all questions.
Electronic calculators may be used.
A copy of the Periodic Table is printed on page 20.
You may lose marks if you do not show your working or if you do not use appropriate units.
.................................................................. and ....................................................................
[2]
(ii)Which one of these structures, A, B, C, D or E, is a diatomic molecule?
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
........................................................................................................................................ [1]
(iii)Which one of these structures, A, B, C, D or E, is a compound?
........................................................................................................................................ [1]
(iv)Which one of these structures, A, B, C, D or E, is very soluble in water?
........................................................................................................................................ [1]
(v)Which one of these structures, A, B, C, D or E, is used in cutting tools?
........................................................................................................................................ [1]
(vi)Which one of these structures, A, B, C, D or E, is used in electrical wiring?
........................................................................................................................................ [1]
This document consists of 18 printed pages and 2 blank pages.
IB19 06_0971_31/FP
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4
3
2
(b) Substance B is an element.
5
(f) The structure of a compound of iron is shown.
This question is about iron and iron compounds.
(a) Name the main ore of iron.
What is meant by the term element ?
.....................................................................................................................................................
............................................................................................................................................... [1]
[Total: 8]
C
N
N
1 hour 15 minutes
The volume of one mole of any gas is 24 dm at room temperature and pressure (r.t.p.).
Lr
lawrencium
–
No
nobelium
–
Md
mendelevium
–
fermium
Fm
Es
einsteinium
–
–
Cf
californium
–
Pa
protactinium
Th
thorium
Ac
Cl – Li+ Cl – Li+
May/June 2019
Paper 3 Theory (Core)
–
Bk
curium
–
–
neptunium
238
–
Cm
Am
americium
Pu
plutonium
berkelium
Li+ Cl – Li+ Cl –
He
A
READ THESE INSTRUCTIONS FIRST
uranium
Np
Cl – Li+ Cl – Li+
0971/31
CHEMISTRY
0971/21/M/J/19
Li+ Cl – Li+ Cl –
He
He
He
3
U
He
He
actinium
actinoids
71
103
175
Lu
lutetium
70
102
173
Yb
ytterbium
101
169
Tm
–
thulium
69
68
Er
167
erbium
100
99
165
Ho
holmium
67
66
163
Dy
dysprosium
98
97
159
Tb
terbium
65
64
96
95
157
Gd
gadolinium
152
94
63
Eu
europium
150
62
Sm
samarium
–
61
93
92
Pm
promethium
144
91
60
Nd
neodymium
141
90
89
59
Pr
praseodymium
140
139
58
Ce
cerium
La
lanthanum
57
–
–
lanthanoids
–
livermorium
Lv
Fl
flerovium
–
–
Cn
copernicium
–
–
–
–
Rg
roentgenium
Ds
darmstadtium
Mt
meitnerium
Hs
hassium
–
bohrium
Bh
Sg
seaborgium
–
–
Db
dubnium
–
Rf
rutherfordium
Ra
radium
Fr
francium
86
Rn
radon
–
85
At
astatine
–
84
116
Po
polonium
209
Bi
bismuth
83
82
lead
114
207
Pb
Tl
204
thallium
81
80
201
Hg
mercury
112
111
gold
197
Au
79
78
Pt
110
109
195
platinum
192
108
77
Ir
iridium
190
76
Os
osmium
107
186
Re
rhenium
75
74
W
106
184
105
104
72
56
55
tungsten
181
178
73
Ta
tantalum
Hf
hafnium
actinoids
88
87
57–71
89–103
137
133
lanthanoids
Ba
barium
Cs
caesium
54
131
127
84
Xe
xenon
I
iodine
128
Te
tellurium
122
Sb
antimony
tin
Sn
119
115
indium
In
Cd
cadmium
112
108
silver
Ag
103
101
106
Pd
palladium
Rh
rhodium
Ru
ruthenium
–
Tc
technetium
96
Mo
93
91
molybdenum
Nb
niobium
Zr
zirconium
Y
89
88
85
yttrium
Sr
strontium
Rb
rubidium
53
36
80
51
52
79
75
50
73
70
49
48
65
64
47
46
45
44
59
59
56
43
55
42
41
40
52
51
48
39
37
45
40
38
39
40
Kr
krypton
Br
bromine
As
Se
selenium
arsenic
Ge
germanium
gallium
Ga
Zn
zinc
copper
Cu
Ni
iron
nickel
Co
cobalt
Fe
Mn
manganese
Cr
chromium
V
vanadium
Ti
titanium
Sc
scandium
Ca
20
19
calcium
24
23
K
27
26
25
24
23
magnesium
sodium
9
12
Be
Mg
beryllium
7
11
Li
Na
lithium
4
21
22
name
relative atomic mass
atomic symbol
atomic number
Key
3
potassium
18
35
34
33
32
28
29
30
31
20
Ar
35.5
32
neon
argon
chlorine
sulfur
31
phosphorus
silicon
28
27
aluminium
Ne
F
17
19
Cl
fluorine
S
16
16
O
oxygen
14
N
P
nitrogen
15
14
C
Si
carbon
12
11
B
13
Al
boron
2
4
6
5
III
1
hydrogen
Group
1
The Periodic Table of Elements
H
II
Cambridge Assessment International Education
Cambridge International General Certificate of Secondary Education (9 –1)
N
© UCLES 2019
The diagrams show part of the structures of five substances, A, B, C, D and E.
N
I
1
*7137439209*
IV
7
V
8
VI
9
10
He
VIII
VII
helium
16
O
C
OC
............................................................................................................................................... [1]
OC
OC
(b) In a blast furnace used for the extraction of iron, carbon reacts with oxygen from the air to form
carbon monoxide.
Complete the chemical equation for this reaction.
3C + Fe2O3
C
O
CO
Fe
CO
CO
C
O
educe the molecular formula of this compound to show the number of iron, carbon and
D
oxygen atoms.
2CO
....C + .....
[2]
(c) In the hotter parts of the furnace, carbon reacts with the iron(III) oxide present in the iron ore.
Fe
............................................................................................................................................... [1]
[Total: 11]
3CO + 2Fe
How does this equation show that carbon is oxidised?
.....................................................................................................................................................
............................................................................................................................................... [1]
(d) Limestone is added to the blast furnace. The limestone is converted into calcium oxide and
carbon dioxide. The reaction is endothermic.
CaCO3
(i)
heat
CaO + CO2
What type of chemical reaction is this?
........................................................................................................................................ [1]
(ii)
hat type of oxide is calcium oxide?
W
Give a reason for your answer.
..............................................................................................................................................
........................................................................................................................................ [2]
(e) Iron is a metal.
Give three physical properties that are characteristic of metals.
1 ..................................................................................................................................................
2 ..................................................................................................................................................
3 ..................................................................................................................................................
[3]
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3
8
7
(a) The table shows the percentage by mass of the elements on Earth and in the Universe.
element
percentage by
mass on Earth
percentage by mass
in the Universe
helium
0.0
21.0
hydrogen
0.1
76.0
iron
35.0
1.0
magnesium
14.0
0.1
oxygen
29.0
0.8
silicon
14.0
0.1
sulfur
2.9
0.1
100.0
100.0
other elements
4
(c) Helium, neon and argon are noble gases.
(i)
(a) U
se the kinetic particle model to describe the separation between the molecules and the type
of motion of the molecules in:
Explain, in terms of the electronic structure, why neon is unreactive.
..............................................................................................................................................
●●
........................................................................................................................................ [1]
........................................................................................................................................ [1]
[Total: 7]
●●
iodine gas. ...........................................................................................................................
.....................................................................................................................................................
[4]
(b) The graph shows how the volume of iodine gas changes with pressure. The temperature is
kept constant.
0.9
total
solid iodine ...........................................................................................................................
.....................................................................................................................................................
(ii)State one use of argon.
This question is about iodine and compounds of iodine.
Answer these questions using only the information in the table.
(i)
Deduce the percentage by mass of other elements present on Earth.
volume of
iodine gas
.............................. % [1]
(ii)
Which non-metallic element is present on Earth in the greatest percentage by mass?
0
0
........................................................................................................................................ [1]
(iii)
ive two major differences in the percentage by mass of the elements on Earth and in the
G
Universe.
pressure
Describe how the volume of iodine gas changes with pressure.
.....................................................................................................................................................
1 ...........................................................................................................................................
............................................................................................................................................... [1]
..............................................................................................................................................
2 ...........................................................................................................................................
(c) (i)
..............................................................................................................................................
[2]
omplete the word equation to show the halogen and halide compound which react to
C
form the products iodine and potassium bromide.
potassium
........................
........................
iodine
+
+
bromide
........................
[2]
(b) Complete the diagram to show the electron arrangement in an oxygen atom.
(ii)
Explain, in terms of the reactivity of the halogens, why aqueous iodine does not react with
aqueous potassium chloride.
..............................................................................................................................................
........................................................................................................................................ [1]
[1]
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5
Balance the chemical equation for this reaction.
11
(i)
carbon dioxide
ethene
(ii)Which one of the following words describes the ethene molecules in this reaction?
Draw a circle around the correct answer.
hydrogen
The energy level diagram for this reaction is shown.
methane
elements
mixtures
monomers
polymers
[1]
nitrogen
(a) (i)Which one of these gases is an alkane?
energy
(iii)
........................................................................................................................................ [1]
products
(ii)
What is the name given to this type of chemical reaction?
........................................................................................................................................ [1]
carbon monoxide
reactants
Poly(ethene) is a non-biodegradable plastic.
What is meant by the term non-biodegradable?
Draw the structure of a molecule of ethene. Show all of the atoms and all of the bonds.
..............................................................................................................................................
........................................................................................................................................ [1]
progress of reaction
(iv)
Explain how this diagram shows that the reaction is exothermic.
........................................................................................................................................ [1]
Describe one pollution problem caused by non-biodegradable plastics.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [1]
[1]
(iii)
(e) Describe a test for iodide ions.
escribe how aqueous bromine can be used to tell the difference between methane and
D
ethene.
test ..............................................................................................................................................
..............................................................................................................................................
observations ...............................................................................................................................
[2]
..............................................................................................................................................
(c) Ethanol can be made from ethene and one other reactant.
●●
Name the other reactant.
.....................................................................................................................................................
●●
........................................................................................................................................ [2]
State the conditions needed to make ethanol from ethene.
.....................................................................................................................................................
(f) Molten sodium iodide is electrolysed.
.....................................................................................................................................................
[3]
Predict the product at the positive electrode.
............................................................................................................................................... [1]
[Total: 11]
[Total: 14]
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6
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(b) Ethene molecules react with each other to form poly(ethene).
oal gas is made by heating coal in the absence of air.
C
The list shows the main gases present in coal gas.
Na2S4O6 + .....NaI
.....Na2S2O3 + I2
[2]
(ii)
© UCLES 2019
10
9
(d) Iodine reacts with aqueous sodium thiosulfate, Na2S2O3.
(i)
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(a) D
escribe how you could prepare a pure sample of crystals of hydrated copper(II) sulfate using
dilute sulfuric acid and an excess of copper(II) oxide.
number of
electrons
.....................................................................................................................................................
.....................................................................................................................................................
5H2O
(i)
What is meant by the symbol
199.8
........................................................................................................................................ [1]
hydrated
copper(II) sulfate
(ii)
?
199.6
Suggest why an alloy of copper is used to make coins instead of using pure copper.
mass of
reaction
mixture
/g
199.4
........................................................................................................................................ [1]
........................................................................................................................................ [1]
(ii)
200.0
What is meant by the term alloy?
..............................................................................................................................................
CuSO4.5H2O
anhydrous
copper(II) sulfate
............................................................................................................................................... [1]
(b) The graph shows how the mass of the reaction mixture changes with time.
(e) Alloys of copper are used to make coins.
(b) Anhydrous copper(II) sulfate is used to test for water.
CaCl 2(aq) + CO2(g) + H2O(l)
(a) Name the salt formed when calcium carbonate reacts with hydrochloric acid.
29
63
2+
29Cu
(i)
A student investigates the rate of reaction of small pieces of calcium carbonate with an excess of
hydrochloric acid of concentration 1 mol / dm3.
CaCO3(s) + 2HCl (aq) number of
protons
[4]
............................................................................................................................................... [3]
+
14
7
34
16S
.....................................................................................................................................................
.....................................................................................................................................................
number of
neutrons
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13
(d) Complete the table to show the number of electrons, protons and neutrons in the sulfur atom
and copper ion shown.
This question is about copper and copper compounds.
CuSO4
© UCLES 2019
[Total: 13]
How can hydrated copper(II) sulfate be changed into anhydrous copper(II) sulfate?
........................................................................................................................................ [1]
199.2
(c) C
omplete the table to calculate the relative formula mass of anhydrous copper(II) sulfate,
CuSO4.
Use your Periodic Table to help you.
type of atom
number
of atoms
relative
atomic mass
copper
1
64
199.0
198.8
1 × 64 = 64
0
20
40
60
80
100
120
140
time / s
sulfur
(i)
oxygen
State why the reaction mixture decreases in mass.
........................................................................................................................................ [1]
relative formula mass = ...............................
[2]
(ii)
Calculate the loss in mass during the first 40 seconds of the experiment.
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.............................. g [1]
0971/31/M/J/19
16
15
(iii)
The experiment is repeated using hydrochloric acid of concentration 2 mol / dm3.
ll other conditions are kept the same.
A
8
Draw a line on the grid for the experiment using hydrochloric acid of concentration
2 mol / dm3.[2]
(iv)
In the experiment, when 2.00 g of calcium carbonate is used, the loss in mass of the
reaction mixture is 0.88 g.
All other conditions are kept the same.
17
(a) Sulfur dioxide is a pollutant in the air.
(c) Excess sulfuric acid reacts with ammonia to make a salt which can be used as a fertiliser.
(i)State one source of sulfur dioxide in the air.
State the name of the salt formed when excess sulfuric acid reacts with ammonia.
........................................................................................................................................ [1]
(ii)
............................................................................................................................................... [1]
ulfur dioxide is oxidised to sulfur trioxide in the air.
S
Oxides of nitrogen act as catalysts for this reaction.
(d) The table shows some observations about the reactivity of four metals with dilute sulfuric acid.
What is meant by the term catalyst ?
Calculate the loss in mass when 0.50 g of calcium carbonate is used.
metal
........................................................................................................................................ [1]
(iii)
loss in mass = .............................. g [1]
(v)
he experiment is repeated using the same mass of different sized pieces of
T
calcium carbonate.
All other conditions are kept the same.
The sizes of the pieces of calcium carbonate are:
●
●
●
nickel
a few bubbles slowly form
tungsten
no bubbles are seen
se the information in the table to put the four metals in order of their reactivity.
U
Put the least reactive metal first.
pH 4
pH 7
pH 9
pH 13
[1]
least reactive
most reactive
(iv)State one adverse effect of acid rain on buildings.
powder
small pieces
large pieces.
........................................................................................................................................ [1]
Complete the table by writing the sizes of the pieces of calcium carbonate in the first
column.
size of pieces of
calcium carbonate
a slow stream of bubbles is seen
a rapid stream of bubbles is seen
Sulfur trioxide dissolves in rainwater to form acid rain.
Which one of the following pH values could be the pH of acid rain?
Draw a circle around the correct answer.
reaction with sulfuric acid
iron
magnesium
..............................................................................................................................................
(b) Sulfur dioxide melts at –73 °C and boils at –10 °C.
[2]
[Total: 9]
hat is the physical state of sulfur dioxide at –20 °C?
W
Explain your answer.
initial rate of loss
in mass in g / s
.....................................................................................................................................................
0.005
............................................................................................................................................... [2]
0.030
0.100
[1]
[Total: 7]
–
Lr
lawrencium
–
No
nobelium
–
Md
mendelevium
–
Fm
fermium
–
Es
einsteinium
–
Cf
californium
–
Bk
berkelium
–
Cm
curium
–
Am
americium
–
Pu
plutonium
–
neptunium
Np
U
238
uranium
231
protactinium
Pa
actinoids
–
232
Th
thorium
Ac
actinium
57
lanthanoids
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
71
103
175
Lu
70
102
173
ytterbium
Yb
69
101
169
thulium
Tm
68
100
167
erbium
Er
67
99
165
holmium
Ho
66
98
163
dysprosium
Dy
65
97
159
terbium
Tb
64
96
157
gadolinium
Gd
63
95
152
europium
Eu
62
94
150
Sm
samarium
–
93
61
promethium
Pm
60
92
144
neodymium
Nd
59
91
141
praseodymium
Pr
58
90
89
140
Ce
cerium
La
lanthanum
139
–
–
–
–
–
–
–
–
–
–
–
lutetium
–
livermorium
flerovium
copernicium
roentgenium
darmstadtium
meitnerium
hassium
bohrium
seaborgium
dubnium
rutherfordium
–
radium
francium
–
Rn
radon
–
At
astatine
–
116
Lv
Po
polonium
209
Bi
bismuth
Fl
lead
114
Pb
207
204
Tl
thallium
112
201
Hg
mercury
Cn
111
gold
197
Au
Rg
110
195
Ds
platinum
Pt
Ir
109
192
iridium
Mt
108
190
Os
osmium
Hs
107
186
Bh
rhenium
Re
W
106
184
Sg
tungsten
181
105
Hf
178
Rf
actinoids
89–103
lanthanoids
137
Ra
87
133
Fr
Ta
104
88
Db
tantalum
hafnium
Ba
barium
Cs
caesium
54
86
85
84
83
82
81
80
79
78
77
76
75
74
73
72
57–71
56
55
Y
84
131
xenon
Xe
I
127
iodine
128
Te
tellurium
122
Sb
antimony
tin
Sn
119
115
In
indium
112
Cd
cadmium
108
Ag
silver
106
Pd
palladium
103
Rh
rhodium
101
Ru
ruthenium
–
Tc
technetium
96
Mo
molybdenum
93
niobium
Nb
Zr
91
85
88
89
yttrium
Sr
strontium
Rb
rubidium
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2
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zirconium
53
52
51
50
49
48
47
46
45
44
43
42
41
40
39
38
36
© UCLES 2019
37
40
krypton
Kr
35
80
Br
bromine
79
34
Se
selenium
75
33
As
arsenic
73
32
Ge
germanium
70
31
gallium
Ga
30
65
zinc
Zn
29
64
copper
Cu
28
59
nickel
Ni
27
59
cobalt
Co
26
56
iron
Fe
25
55
Mn
manganese
52
24
chromium
Cr
V
23
51
vanadium
48
22
Ti
titanium
20
K
Ca
calcium
19
potassium
23
24
magnesium
sodium
9
12
Be
Mg
beryllium
7
11
Li
Na
4
3
lithium
21
0971/31/M/J/19
45
name
relative atomic mass
atomic symbol
Sc
© UCLES 2019
scandium
1
atomic number
Key
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
0971/31/M/J/19
40
18
20
Ar
Group
The Periodic Table of Elements
1
II
I
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
39
35.5
32
31
28
27
neon
argon
chlorine
sulfur
phosphorus
silicon
aluminium
F
17
19
fluorine
Cl
S
16
O
oxygen
16
P
14
N
nitrogen
15
14
12
C
Si
carbon
11
B
13
8
7
6
5
Al
9
VI
V
IV
III
boron
2
VII
Ne
20
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
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4
19
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VIII
18
BLANK PAGE
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10
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He
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helium
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hydrogen
© UCLES 2019
H
3
1
Cambridge Assessment International Education
Cambridge International General Certificate of Secondary Education (9 –1)
This question is about the structures of atoms and ions.
(a) Define the term proton number.
.....................................................................................................................................................
............................................................................................................................................... [2]
(b) (i)Complete the table to show the number of protons, neutrons and electrons present in
24
26
Mg and 12
Mg.
atoms of 12
*3829634688*
number of
protons
0971/41
CHEMISTRY
May/June 2019
Paper 4 Theory (Extended)
number of
neutrons
number of
electrons
24
12Mg
1 hour 15 minutes
26
12Mg
Candidates answer on the Question Paper.
[2]
No Additional Materials are required.
24
26
Mg and 12
Mg?
(ii)What term is used to describe atoms of the same element, such as 12
READ THESE INSTRUCTIONS FIRST
........................................................................................................................................ [1]
Write your centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
24
26
Mg and 12
Mg are the same.
(iii)Explain why the chemical properties of 12
..............................................................................................................................................
Answer all questions.
Electronic calculators may be used.
A copy of the Periodic Table is printed on page 16.
You may lose marks if you do not show your working or if you do not use appropriate units.
........................................................................................................................................ [2]
(c)Complete the table to identify the atoms and ions which have the following numbers of protons,
neutrons and electrons.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
23
+
11Na
number of
protons
number of
neutrons
number of
electrons
11
12
10
4
5
4
17
20
18
[4]
(d)State the electronic structure of the following atom and ion.
Al ................................
S2– ...............................
[2]
This document consists of 13 printed pages and 3 blank pages.
IB19 06_0971_41/FP
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4
(e)The experiment was repeated using a solid sample of impure Z.
220
Suggest the differences, if any, in the melting point and boiling point of the sample of impure Z
compared to the sample of pure Z.
180
melting point ...............................................................................................................................
160
(a)Zinc is obtained from zinc blende in a two-step process.
............................................................................................................................................... [2]
240
200
3Zinc and copper are elements next to each other in the Periodic Table.
.....................................................................................................................................................
The graph shows how the temperature of the sample of pure Z changed during the first 9 minutes.
100
In your answer:
●● give one chemical equation for each step
●● describe how zinc is removed from the blast furnace in step 2.
step 1 .........................................................................................................................................
.....................................................................................................................................................
chemical equation .......................................................................................................................
step 2 .........................................................................................................................................
40
200
.....................................................................................................................................................
180
chemical equation .......................................................................................................................
160
20
removal of zinc in step 2 ............................................................................................................
140
2
3
4
5
6
7
8
9
10
.....................................................................................................................................................
[5]
120
12
11
temperature
/ °C
100
time / minutes
(a)What is the melting point of pure Z?
(b)Name the alloy formed when zinc is mixed with copper.
80
.............................. °C [1]
............................................................................................................................................... [1]
60
(b)The sample of pure Z began to boil at 9 minutes. It was boiled for 2 minutes.
(c)Copper is a transition element. It can have variable oxidation states.
40
Use this information to sketch on the grid how the temperature of the sample of pure Z changed
between 9 minutes and 11 minutes.
[1]
0
.....................................................................................................................................................
State two other chemical properties of transition elements which make them different from
Group I elements.
20
(c)The sample of pure Z was continually heated between 2 minutes and 5 minutes.
Explain, in terms of attractive forces, why there was no increase in the temperature of the
sample of pure Z between 2 minutes and 5 minutes.
In step 2, zinc oxide is converted into zinc in a blast furnace.
Starting from point ×, sketch on the grid how the temperature of the sample of pure Z changed
between 0 minutes and 8 minutes.
60
1
In step 1, zinc blende is converted into zinc oxide.
●●
(f)A sample of pure Z was allowed to cool from 120 °C to 20 °C. The total time taken was 8 minutes.
80
0
●●
Outline how each of these steps are done.
boiling point ................................................................................................................................
[2]
140
temperature
/ °C
120
0
6
5
(d)Describe how the motion of particles of pure Z changed from 0 minutes to 2 minutes.
2
Z is a covalent substance. In an experiment, a sample of pure solid Z was continually heated for
11 minutes.
1 ..................................................................................................................................................
0
1
2
3
4
5
6
7
8
9
10
12
11
time / minutes
2 ..................................................................................................................................................
[2]
[2]
[Total: 10]
.....................................................................................................................................................
............................................................................................................................................... [2]
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8
7
(d)A compound of copper can be used to test for water.
9
4
Ethanoic acid is a weak acid and hydrochloric acid is a strong acid.
Both ethanoic acid and hydrochloric acid dissociate in aqueous solution.
(i)State the full name of this compound of copper.
(a) (i)
........................................................................................................................................ [1]
(ii)
The chemical equation shows the changes which occur when the strong acid,
hydrochloric acid, is added to water.
from .............................................................. to .................................................................
[2]
H+(aq) + Cl –(aq)
HCl (aq)
MgCO3 + 2HCl
Calculate the mass, in g, of magnesium carbonate needed to react exactly with 50.00 cm3 of
2.00 mol / dm3 hydrochloric acid using the following steps.
(b)A student does experiments to show that hydrochloric acid is a strong acid and ethanoic acid is
a weak acid. The student adds an excess of hydrochloric acid and an excess of ethanoic acid
to separate samples of lumps of calcium carbonate.
(ii)Deduce the charge on the copper ion in CuI.
........................................................................................................................................ [1]
Only the identity of the acid is changed between the experiments. All other conditions are kept
the same.
(i)State two observations which would show that hydrochloric acid is a stronger acid than
ethanoic acid.
........................................................................................................................................ [1]
(iv)Identify the reducing agent.
........................................................................................................................................ [1]
[Total: 16]
●●
Calculate the number of moles of HCl present in 50.00 cm3 of 2.00 mol / dm3 HCl.
●●
Determine the number of moles of MgCO3 which would react with 50.00 cm3 of
2.00 mol / dm3 HCl.
●●
Calculate the relative formula mass, Mr, of MgCO3.
●●
Calculate the mass of MgCO3 needed to react exactly with 50.00 cm3 of 2.00 mol / dm3 HCl.
CH3COOH(aq) ............................................................................................................... [2]
CuI
+
I2
+
K2SO4
KI
+
CuSO4
[2]
(iii)In terms of electron transfer, explain why copper is reduced in this reaction.
MgCl 2 + H2O + CO2
A student used 50.00 cm3 of 2.00 mol / dm3 hydrochloric acid in an experiment to produce
magnesium chloride.
Complete the chemical equation to show the changes which occur when the weak acid,
ethanoic acid, is added to water.
(i)Balance the chemical equation for this reaction.
Magnesium carbonate reacts with hydrochloric acid to produce magnesium chloride.
Define the term acid.
........................................................................................................................................ [1]
(ii)State the colour change that occurs when water is added to this compound of copper.
(e)Aqueous potassium iodide reacts with aqueous copper(II) sulfate to produce iodine.
(c)Hydrochloric acid produces salts called chlorides.
.............................. mol
.............................. mol
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
(ii)The student uses the same size container and checks that the pressure is the same for
each experiment.
Mr of MgCO3 = ..............................
State three other conditions which must be kept the same to ensure fair testing.
1 ...........................................................................................................................................
2 ...........................................................................................................................................
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3 ...........................................................................................................................................
[3]
mass = .............................. g
[4]
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excess
5
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10
(d)
A student prepares crystals of magnesium chloride by adding
magnesium carbonate to 50.00 cm3 of 2.00 mol / dm3 hydrochloric acid.
of
The structures of five alkenes, A, B, C, D and E, are shown.
A
The student filters the mixture and rinses the residue.
H
C
........................................................................................................................................ [1]
H
C
H
C
CH3
C
H
H
........................................................................................................................................ [1]
C
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [3]
(e)Silver chloride, AgCl, is insoluble. It can be made by a precipitation reaction between aqueous
barium chloride and a suitable aqueous silver salt.
(i)What is meant by the term precipitate?
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)Name a suitable silver salt to use to prepare silver chloride.
Complete the chemical equation to show the formation of insoluble silver chloride from
aqueous barium chloride and the silver salt you have named.
name of a suitable silver salt ...............................................................................................
..................... + .....................
BaCl 2 + .....................
[3]
[Total: 22]
CH2CH3
C
H
H
CH2CH2CH3
H
H
H
C
H
CH2CH3
C
H
C
H
H
Describe the colour change seen and draw the structure of the product. Show all of the atoms
and all of the bonds.
CH2CH2CH2CH3
C
H
C
E
H
(iii)Describe how the student would obtain pure crystals of magnesium chloride from the
filtrate.
C
H
C
D
(ii)Why does the student rinse the residue?
(e)A student added aqueous bromine to alkene C.
B
H
[Turn over
12
11
an
(i)Why does the student add an excess of magnesium carbonate?
0971/41/M/J/19
C
colour change from ........................................................ to ......................................................
H
structure
(a)What is the general formula of alkenes?
............................................................................................................................................... [1]
(b)What is the molecular formula of alkene D?
[2]
............................................................................................................................................... [1]
(f)Two different alcohols can be produced from alkene B by an addition reaction.
(c)Predict which alkene, A, B, C, D or E, has the highest boiling point.
Explain your answer.
B
H
alkene .............................
CH3
C
H
explanation .................................................................................................................................
.....................................................................................................................................................
[2]
C
H
(i)Draw the structures of the two alcohols. Show all of the atoms and all of the bonds.
(d)Which alkene, A, B, C, D or E, diffuses most quickly?
Explain your answer.
alkene .............................
[2]
explanation .................................................................................................................................
(ii)State the reagent and conditions needed to produce an alcohol from alkene B.
.....................................................................................................................................................
[2]
reagent ................................................................................................................................
conditions ............................................................................................................................
..............................................................................................................................................
[3]
© UCLES 2019
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© UCLES 2019
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14
15
BLANK PAGE
BLANK PAGE
13
(g)Alkene C can be converted into a polymer.
C
H
CH2CH3
C
C
H
H
(i)What type of polymerisation occurs?
........................................................................................................................................ [1]
(ii)Suggest the name of the polymer formed.
........................................................................................................................................ [1]
(iii)Complete the chemical equation to show this polymerisation.
CH2CH3
H
C
n
C
H
H
[3]
(iv)State the empirical formula of the polymer formed.
........................................................................................................................................ [1]
[Total: 19]
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2019
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© UCLES 2019
0971/41/M/J/19
–
Lr
lawrencium
–
No
nobelium
–
Md
mendelevium
–
Fm
fermium
–
Es
einsteinium
–
Cf
californium
curium
–
–
ethanol
nitrogen
methane
oxygen
silicon(IV) oxide
(a)the main constituent of natural gas
............................................................................................................................................... [1]
0971/42
CHEMISTRY
May/June 2019
Paper 4 Theory (Extended)
(b)a reactant in respiration
1 hour 15 minutes
Candidates answer on the Question Paper.
............................................................................................................................................... [1]
No Additional Materials are required.
(c)the main constituent of bauxite
READ THESE INSTRUCTIONS FIRST
–
Bk
berkelium
Cm
Am
americium
–
Pu
plutonium
–
neptunium
Np
U
238
uranium
231
Pa
protactinium
232
Th
thorium
Ac
actinium
actinoids
–
65
lanthanoids
calcium oxide
iron(III) oxide
State which substance is:
............................................................................................................................................... [1]
Write your centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
(d)a product of photosynthesis
............................................................................................................................................... [1]
Answer all questions.
Electronic calculators may be used.
A copy of the Periodic Table is printed on page 16.
You may lose marks if you do not show your working or if you do not use appropriate units.
(e)a greenhouse gas
............................................................................................................................................... [1]
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
(f)a macromolecular solid.
............................................................................................................................................... [1]
[Total: 6]
This document consists of 13 printed pages and 3 blank pages.
IB19 06_0971_42/FP
© UCLES 2019
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0971/41/M/J/19
© UCLES 2019
0971/42/M/J/19
4
3
2
aluminium oxide
Answer the following questions about these substances.
Each substance may be used once, more than once or not at all.
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
71
103
175
Lu
70
102
173
ytterbium
Yb
69
101
169
thulium
Tm
68
100
167
erbium
Er
67
99
165
holmium
Ho
66
98
97
64
157
159
96
63
152
Tb
terbium
Gd
gadolinium
94
62
60
144
–
93
92
59
91
Pr
90
140
Ce
cerium
89
139
57
La
lanthanum
141
58
praseodymium
61
Pm
promethium
Nd
neodymium
150
Sm
samarium
95
Eu
europium
163
dysprosium
Dy
lutetium
–
–
livermorium
–
flerovium
–
copernicium
–
roentgenium
–
–
darmstadtium
meitnerium
–
hassium
–
bohrium
–
seaborgium
–
–
dubnium
rutherfordium
–
radium
francium
–
Rn
radon
–
At
astatine
–
116
Lv
Po
polonium
209
Bi
bismuth
Fl
lead
114
Pb
207
204
Tl
thallium
112
201
Hg
mercury
Cn
111
gold
197
Rg
Au
Pt
110
195
Ds
platinum
Ir
192
109
iridium
Mt
108
190
Os
osmium
Hs
107
186
Re
rhenium
Bh
106
184
Sg
tungsten
181
105
Hf
178
Rf
actinoids
89–103
137
Ra
87
Fr
Ta
104
88
Db
tantalum
hafnium
Ba
barium
Cs
W
Cambridge Assessment International Education
Cambridge International General Certificate of Secondary Education (9 –1)
caesium
133
54
86
85
84
83
82
81
80
79
78
77
76
75
74
73
72
57–71
56
55
Y
lanthanoids
84
131
xenon
36
Xe
I
127
iodine
128
Te
tellurium
122
Sb
antimony
tin
Sn
119
115
indium
In
Cd
112
106
103
101
Ru
ruthenium
–
Tc
technetium
96
Mo
molybdenum
93
Nb
niobium
85
88
89
yttrium
Sr
strontium
Rb
rubidium
91
zirconium
Zr
108
silver
Pd
palladium
Rh
rhodium
Ag
cadmium
53
52
51
50
49
48
47
46
45
43
41
39
38
37
40
25
42
44
64
40
krypton
Kr
35
80
Br
bromine
79
34
Se
selenium
75
33
As
arsenic
73
32
Ge
germanium
70
31
gallium
Ga
30
65
zinc
Zn
28
59
29
Cu
copper
Ni
nickel
27
59
cobalt
Co
26
56
Fe
iron
52
24
55
Mn
manganese
Cr
chromium
V
23
51
vanadium
48
22
Ti
K
Ca
21
Sc
scandium
20
calcium
19
potassium
23
24
magnesium
sodium
9
12
Be
Mg
beryllium
7
11
Li
Na
titanium
name
relative atomic mass
atomic symbol
atomic number
lithium
45
1
4
40
18
20
Ar
hydrogen
Key
3
39
35.5
32
31
28
27
neon
argon
chlorine
sulfur
phosphorus
silicon
aluminium
Ne
F
17
19
fluorine
Cl
S
16
O
oxygen
16
P
14
N
nitrogen
15
14
12
C
Si
carbon
11
B
13
8
7
6
5
Al
9
VI
V
IV
III
Group
1
The Periodic Table of Elements
H
II
I
© UCLES 2019
2
1The names of eight substances are given.
*5339226275*
boron
2
4
10
He
VII
VIII
helium
16
5
3This question is about phosphorus and compounds of phosphorus.
22
23
24
(a)
11Na, 11Na and 11Na are isotopes of sodium.
(i)Describe how these sodium isotopes are the same and how they are different in terms of
the total number of protons, neutrons and electrons in each.
(a)Phosphorus has the formula P4. Some properties of P4 are shown.
melting point / °C
same ....................................................................................................................................
..............................................................................................................................................
different ................................................................................................................................
..............................................................................................................................................
[3]
(ii)Why do all three isotopes have an overall charge of zero?
(d)Phosphine has the formula PH3.
Complete the dot-and-cross diagram to show the electron arrangement in a molecule of
phosphine. Show outer shell electrons only.
45
boiling point / °C
280
electrical conductivity
non-conductor
solubility in water
insoluble
H
(i)Name the type of bonding that exists between the atoms in a P4 molecule.
H
........................................................................................................................................ [1]
P
H
(ii)Explain, in terms of attractive forces between particles, why P4 has a low melting point.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [1]
(iii)Why do all three isotopes have the same chemical properties?
[2]
........................................................................................................................................ [1]
(iii)Explain why phosphorus is a non-conductor of electricity.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(e)Phosphine, PH3, has a similar chemical structure to ammonia, NH3.
Ammonia acts as a base when it reacts with sulfuric acid.
(i)What is meant by the term base?
........................................................................................................................................ [1]
........................................................................................................................................ [1]
(iv)Why do sodium ions have a charge of +1?
..............................................................................................................................................
........................................................................................................................................ [1]
(b)
Phosphorus, P4, reacts with air to produce phosphorus(V) oxide, P4O10.
(i)Write a chemical equation for this reaction.
........................................................................................................................................ [2]
(b)Carbon is an element which exists in different forms.
(ii)Write a chemical equation for the reaction between ammonia and sulfuric acid.
........................................................................................................................................ [2]
[Total: 13]
(ii)What type of chemical reaction is this?
(i)Name two forms of the element carbon that have giant covalent structures.
........................................................................................................................................ [1]
............................................................... and ............................................................... [1]
(c)Phosphorus(V) oxide, P4O10, is an acidic oxide.
(ii)Name the oxide of carbon that is a toxic gas.
........................................................................................................................................ [1]
[Total: 9]
Phosphorus(V) oxide, P4O10, reacts with aqueous sodium hydroxide to form a salt containing
the phosphate ion, PO43–. Water is the only other product.
Write a chemical equation for the reaction between phosphorus(V) oxide and aqueous
sodium hydroxide.
............................................................................................................................................... [2]
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6
CO(g) + 2H2(g)
(iii)What term is used to describe compounds with the same molecular formula but different
structural formulae?
........................................................................................................................................ [1]
CH3OH(g)
The forward reaction is exothermic.
5Copper(II) sulfate crystals, CuSO4.5H2O, are hydrated.
Copper(II) sulfate crystals are made by reacting copper(II) carbonate with dilute sulfuric acid.
The equation for the overall process is shown.
(d)Alcohols react with carboxylic acids to produce esters.
(a)Suggest a source of hydrogen for this industrial process.
O
H
(b)Complete the table using only the words increases, decreases or no change.
effect on the rate
of the reverse reaction
C
O
effect on the equilibrium
yield of CH3OH(g)
adding a catalyst
CuCO3 + H2SO4 + 4H2O
H
H
C
C
H
H
step 2
step 4The solution is allowed to cool and crystallise.
step 5The crystals are removed and dried.
(a)
Calculate the maximum mass of the copper(II) sulfate crystals, CuSO4.5H2O, that can form
using the following steps.
........................................................................................................................................ [1]
increases
(ii)Give the name of the carboxylic acid and the alcohol that react together to produce ester X.
decreasing the pressure
[4]
The excess of copper(II) carbonate is separated from the aqueous copper(II) sulfate.
step 3The aqueous copper(II) sulfate is heated until the solution is saturated.
H
Name ester X.
no change
CuSO4.5H2O + CO2
step 1Powdered solid copper(II) carbonate is added to 50.0 cm3 of 0.05 mol / dm3 sulfuric acid
until the copper(II) carbonate is in excess.
(i)The structure of ester X is shown.
............................................................................................................................................... [1]
increasing the temperature
8
7
4Methanol is made industrially by reacting carbon monoxide with hydrogen. The gases react at a
temperature of 250 °C and a pressure of 75 atmospheres.
●●
Calculate the number of moles of H2SO4 in 50.0 cm3 of 0.05 mol / dm3 H2SO4.
●●
Determine the number of moles of CuSO4.5H2O that can form.
●●
The Mr of CuSO4.5H2O is 250.
carboxylic acid .....................................................................................................................
alcohol .................................................................................................................................
[2]
(c)Methanol is a member of the homologous series of alcohols.
(iii)Ester Y is different from ester X but also has the formula C3H6O2.
(i)State two general characteristics of a homologous series.
1 ...........................................................................................................................................
Draw the structure of ester Y. Show all of the atoms and all of the bonds.
.............................. mol
2 ...........................................................................................................................................
[2]
(ii)Draw the structures of two different alcohols, each containing three carbon atoms. Show
all of the atoms and all of the bonds.
Name these two alcohols.
name ......................................................
..............................................................................................................................................
[2]
name ......................................................
.............................. mol
Calculate the maximum mass of CuSO4.5H2O that can form.
[Total: 17]
.............................. g
[3]
[4]
© UCLES 2019
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10
9
(b)Steps 1–5 were done correctly but the mass of crystals obtained was less than the maximum
mass.
(c)State two observations that would indicate that the copper(II) carbonate is in excess in step 1.
physical state ..............................................................................................................................
colour ..........................................................................................................................................
[2]
1 ..................................................................................................................................................
(b)When chlorine reacts with aqueous potassium bromide a displacement reaction occurs.
2 ..................................................................................................................................................
[2]
(d)When the reaction in step 1 is done using lumps of copper(II) carbonate instead of powder,
the rate of reaction decreases. All other conditions are kept the same.
7
(a)Predict the physical state and colour of astatine at room temperature and pressure.
Explain why.
............................................................................................................................................... [1]
11
6The halogens are the elements in Group VII of the Periodic Table.
Displacement reactions can be used to determine the order of reactivity of metals such as
lead (Pb), nickel (Ni), and silver (Ag).
The ionic equation for a displacement reaction is shown.
Ni(s) + Pb2+(aq)
from .............................................................. to .................................................................
[2]
(ii)Write a chemical equation for this reaction.
.....................................................................................................................................................
........................................................................................................................................ [2]
.....................................................................................................................................................
(c)Reactions occur when some aqueous solutions of halogens are added to aqueous solutions of
halides.
............................................................................................................................................... [2]
Ni(s)
key
= reaction
= no reaction
............................................................................................................................................... [1]
KCl (aq)
halogens
..............................................................................................................................................
(i)Identify the reducing agent in the displacement reaction. Give a reason for your answer.
reducing agent......................................................................................................................
reason...................................................................................................................................
[2]
........................................................................................................................................ [1]
............................................................................................................................................... [1]
(i)Suggest what is meant by the term saturated solution.
Pb(s)
The ionic half-equations show that electrons are donated by nickel atoms and accepted by
lead ions.
(b)The ionic equation for another displacement reaction is shown.
halides
(g)
The solution of aqueous copper(II) sulfate was heated until it was saturated in step 3.
Ni2+(aq) + 2e–
Pb2+(aq) + 2e–
(ii)What is the general term given to the type of reaction in which electrons are transferred
from one species to another?
Use the key to complete the table to show the results of adding halogens to halides.
(f)
Name the process used to separate the aqueous copper(II) sulfate from the excess of
copper(II) carbonate in step 2.
Pb(s) + Ni2+(aq)
The ionic half-equations for this reaction are shown.
(i)Describe the colour change of the solution.
Give a reason for this. Explain your answer in terms of particles.
(e)Name a different substance, other than copper(II) carbonate, that could be added to dilute
sulfuric acid to produce copper(II) sulfate in step 1.
(a)Displacement reactions occur between metals and metal ions.
KBr(aq)
Cl 2(aq)
KI(aq)
Pb(s) + 2Ag+(aq)

2Ag(s) + Pb2+(aq)
Write the two ionic half-equations for this reaction.
Br2(aq)
1 ..................................................................................................................................................
I2(aq)
2 ..................................................................................................................................................
[2]
..............................................................................................................................................
[2]
........................................................................................................................................ [2]
[Total: 8]
(ii)What evidence would show that the solution was saturated in step 3?
(c)Use the information in (a) and (b) to put the three metals lead, nickel and silver in order of
reactivity.
most reactive
........................................................................................................................................ [1]
(iii)Why should the aqueous copper(II) sulfate not be heated to dryness in step 3?
........................................................................................................................................ [1]
least reactive
[Total: 14]
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[1]
© UCLES 2019
12
(d)Nickel is a transition element. Nickel is stronger than sodium.
0971/42/M/J/19
© UCLES 2019
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13
14
BLANK PAGE
BLANK PAGE
Describe two other differences in the physical properties of nickel and sodium.
1 ..................................................................................................................................................
2 ..................................................................................................................................................
[2]
(e)Predict one difference in the appearance of aqueous solutions of nickel compounds compared
to aqueous solutions of sodium compounds.
.....................................................................................................................................................
............................................................................................................................................... [1]
(f) Copper is refined (purified) by electrolysis. Nickel can be refined using a similar method.
(i)
The diagram shows the refining of nickel by electrolysis.
Complete the labels in the boxes.
power
supply
anode made of
+
–
..........................................
cathode made of
..........................................
electrolyte of
..........................................
[3]
(ii)Indicate, by writing N on the diagram, where nickel is produced.
© UCLES 2019
[1]
[Total: 13]
0971/42/M/J/19
© UCLES 2019
0971/42/M/J/19
© UCLES 2019
0971/42/M/J/19
[Turn over
–
Lr
lawrencium
–
–
No
nobelium
Md
mendelevium
–
Fm
fermium
–
Es
einsteinium
–
Cf
californium
curium
1 hour
Candidates answer on the Question Paper.
No Additional Materials are required.
–
–
–
–
Bk
berkelium
Cm
Am
americium
Pu
plutonium
–
neptunium
Np
U
238
uranium
231
protactinium
Pa
actinoids
May/June 2019
Paper 6 Alternative to Practical
READ THESE INSTRUCTIONS FIRST
–
232
Th
thorium
Ac
actinium
65
lanthanoids
0971/61
CHEMISTRY
Write your centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
103
71
69
169
70
102
101
68
100
167
erbium
Er
67
99
165
holmium
Ho
66
98
97
64
157
152
63
62
159
96
95
94
150
–
93
61
promethium
Pm
60
92
144
neodymium
Nd
59
91
Pr
90
140
Ce
cerium
89
139
57
La
lanthanum
141
58
praseodymium
Tb
terbium
Gd
gadolinium
Eu
europium
Sm
samarium
163
dysprosium
Dy
173
Yb
ytterbium
Tm
thulium
175
Lu
lutetium
–
–
livermorium
–
flerovium
–
copernicium
–
roentgenium
–
–
–
darmstadtium
meitnerium
hassium
–
bohrium
–
seaborgium
–
–
dubnium
rutherfordium
–
radium
francium
–
Rn
radon
–
At
astatine
–
116
Lv
Po
polonium
Bi
bismuth
209
Fl
lead
114
Pb
207
204
Tl
thallium
112
201
Hg
mercury
Cn
111
gold
197
Rg
Au
Pt
110
195
Ds
platinum
Ir
109
192
Mt
iridium
190
108
Os
osmium
Hs
107
186
Bh
rhenium
Re
W
106
184
Sg
tungsten
181
105
Hf
178
Rf
actinoids
89–103
137
Ra
87
Fr
Ta
104
88
Db
tantalum
hafnium
Ba
barium
Cs
caesium
133
54
86
85
84
83
82
81
80
79
78
77
76
75
74
73
72
57–71
56
55
Y
lanthanoids
84
131
Xe
I
127
iodine
122
128
Te
tellurium
Sb
antimony
tin
Sn
119
115
In
indium
112
Cd
cadmium
101
103
106
108
silver
Ag
Pd
palladium
Rh
rhodium
Ru
ruthenium
–
Tc
technetium
96
Mo
molybdenum
93
Nb
niobium
88
89
yttrium
Sr
strontium
Rb
rubidium
91
Zr
zirconium
45
44
43
42
41
40
39
38
37
Ca
K
© UCLES 2019
85
36
53
52
51
50
49
48
47
46
64
40
Kr
35
80
Br
bromine
79
75
33
34
Se
selenium
As
arsenic
73
32
Ge
germanium
70
31
gallium
Ga
30
65
zinc
Zn
28
59
29
Cu
copper
Ni
nickel
26
56
27
iron
59
Co
cobalt
Fe
25
55
Mn
manganese
52
24
chromium
Cr
V
23
51
vanadium
48
22
Ti
scandium
20
calcium
19
potassium
23
24
magnesium
sodium
9
12
Be
Mg
beryllium
7
11
Li
Na
lithium
4
3
titanium
name
relative atomic mass
atomic symbol
atomic number
21
0971/42/M/J/19
45
1
Sc
© UCLES 2019
40
18
20
Ar
hydrogen
Key
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
39
35.5
32
31
28
27
neon
argon
chlorine
sulfur
phosphorus
silicon
aluminium
Ne
F
17
19
fluorine
Cl
S
16
16
O
oxygen
15
14
P
N
nitrogen
14
12
C
Si
carbon
11
B
13
Al
6
5
boron
2
4
10
He
9
8
7
VIII
helium
VII
VI
V
IV
III
Group
1
The Periodic Table of Elements
H
II
I
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education
Cambridge International General Certificate of Secondary Education (9 –1)
*8895278627*
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
xenon
16
krypton
15
BLANK PAGE
Answer all questions.
Electronic calculators may be used.
You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
This document consists of 8 printed pages and 4 blank pages.
IB19 06_0971_61/FP
© UCLES 2019
[Turn over
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2
3
4
BLANK PAGE
1The diagram shows the apparatus a student used to prepare a dry sample of chlorine gas. Chlorine
is more dense than air.
2A student investigated the reaction between aqueous sodium carbonate and aqueous barium nitrate.
●●
●●
●●
●●
●●
●●
●●
A burette was filled with aqueous sodium carbonate.
Seven test-tubes were labelled 1, 2, 3, 4, 5, 6 and 7.
A measuring cylinder was used to pour 6 cm3 of aqueous barium nitrate into each of the seven
test‑tubes in a test‑tube rack.
1.0 cm3 of aqueous sodium carbonate was added from the burette to test-tube 1.
2.0 cm3 of aqueous sodium carbonate was added from the burette to test-tube 2.
4.0 cm3 of aqueous sodium carbonate was added from the burette to test-tube 3.
5.0 cm3 of aqueous sodium carbonate was added from the burette to test-tube 4.
6.0 cm3 of aqueous sodium carbonate was added from the burette to test-tube 5.
7.0 cm3 of aqueous sodium carbonate was added from the burette to test-tube 6.
8.0 cm3 of aqueous sodium carbonate was added from the burette to test-tube 7.
A glass rod was used to stir the contents of each of the test‑tubes. The contents of the test‑tubes
were left to stand until the solid formed had settled. A ruler was used to measure the height of the
solid formed in each test‑tube.
..........................................
manganese(IV) oxide
●●
●●
●●
..........................................
concentrated
hydrochloric
acid
(a)Use a ruler to measure the heights of the solid formed in each test‑tube shown in the diagram.
Record the heights of the solid formed in the table and complete the table.
flask 1
concentrated
sulfuric acid
test-tube number
(a)Complete the boxes to name the apparatus.
[2]
1
2
3
4
5
6
7
volume of aqueous
sodium carbonate / cm3
(b)Use the diagram to identify two mistakes the student made.
1 ..................................................................................................................................................
.....................................................................................................................................................
2 ..................................................................................................................................................
.....................................................................................................................................................
[2]
(c)Suggest one reason why the gas produced in flask 1 is passed through concentrated
sulfuric acid.
............................................................................................................................................... [1]
(d)Describe a test for chlorine.
test ..............................................................................................................................................
observations ...............................................................................................................................
[2]
(e)Suggest why this experiment is done in a fume cupboard.
............................................................................................................................................... [1]
© UCLES 2019
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© UCLES 2019
6
7
3Two substances, solution F and solid G, were analysed. Solution F was dilute hydrochloric acid.
Tests were done on solution F and solid G.
80
tests on solution F
.....................................................................................................................................................
Complete the expected observations.
.....................................................................................................................................................
Solution F was divided into four equal portions in four test‑tubes.
............................................................................................................................................... [2]
60
(f)
Suggest one change to the apparatus used which could be made to obtain more accurate
results.
height of
solid / mm
40
............................................................................................................................................... [1]
(g)Suggest a different method to measure the amount of solid formed during the experiment.
20
.....................................................................................................................................................
.....................................................................................................................................................
0
0
1
2
3
4
5
6
7
.....................................................................................................................................................
8
............................................................................................................................................... [3]
[4]
(h)Suggest how the reliability of the results could be checked.
(c)
From your graph, deduce the height of the solid formed when 3.0 cm3 of aqueous
sodium carbonate is added to 6 cm3 of aqueous barium nitrate.
(a)The pH of the first portion of solution F was tested.
pH = .............................. [1]
(b)Magnesium ribbon was added to the second portion of solution F. The gas produced was
tested.
observations ...............................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
(c)Dilute nitric acid and aqueous silver nitrate were added to the third portion of solution F.
observations ......................................................................................................................... [1]
(d)Dilute nitric acid and aqueous barium nitrate were added to the fourth portion of solution F.
.....................................................................................................................................................
Show clearly on the grid how you worked out your answer.
0971/61/M/J/19
(e)Predict what would happen if the experiment were continued using three further test‑tubes
each containing 6 cm3 of aqueous barium nitrate and separately adding 9.0 cm3, 10.0 cm3 and
11.0 cm3 of aqueous sodium carbonate to each one.
Explain your answer.
5
100
[3]
[Total: 8]
© UCLES 2019
(b)Plot the results on the grid. Draw two intersecting lines of best fit. Label the x-axis.
solid
height of solid / mm
observations ......................................................................................................................... [1]
............................................................................................................................................... [1]
.............................. mm [2]
[Total: 18]
(d)Describe the trend in the heights of the solids formed in test‑tubes 1–7.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
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8
observations
The appearance of solid G was studied.
BLANK PAGE
s how that coating steel nails with paint helps to protect the nails from rusting
show that coating steel nails with zinc helps to protect the nails from rusting
determine which coating is more effective at protecting steel nails from rusting.
You are provided with:
white solid
●●
●●
●●
●●
test 1
Dilute hydrochloric acid was added to solid G.
The gas produced was tested.
Steel nails rust in the presence of air and water. Plan an investigation to:
●●
●●
●●
Some of the tests and observations are shown.
tests on solid G
10
9
4
tests on solid G
rapid effervescence
limewater turned milky
ncoated steel nails
u
steel nails coated with paint
steel nails coated with zinc
common laboratory apparatus.
............................................................................................................................................................
The solution formed was divided into two portions
for test 2.
............................................................................................................................................................
............................................................................................................................................................
test 2
............................................................................................................................................................
An excess of aqueous sodium hydroxide was
added to the first portion of the solution from test 1.
white precipitate formed which
was insoluble in excess
............................................................................................................................................................
An excess of aqueous ammonia was added to the
second portion of the solution from test 1.
no precipitate formed
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
(e)Identify solid G.
............................................................................................................................................... [2]
............................................................................................................................................................
[Total: 8]
...................................................................................................................................................... [6]
© UCLES 2019
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12
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© UCLES 2019
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Cambridge Assessment International Education
Cambridge International General Certificate of Secondary Education (9 –1)
*5340169958*
0971/62
CHEMISTRY
May/June 2019
Paper 6 Alternative to Practical
1 hour
Candidates answer on the Question Paper.
No Additional Materials are required.
READ THESE INSTRUCTIONS FIRST
Write your centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
Answer all questions.
Electronic calculators may be used.
You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2019
0971/61/M/J/19
© UCLES 2019
[Turn over
0971/61/M/J/19
2
BLANK PAGE
This document consists of 8 printed pages and 4 blank pages.
IB19 06_0971_62/FP
© UCLES 2019
4
3
1A student did the following steps to make zinc chloride crystals from solid zinc oxide.
step 1Pour 40 cm3 of dilute hydrochloric acid into a beaker. Add a small amount of zinc oxide.
Warm the mixture and stir it.
step 2Continue to add zinc oxide to the beaker until all of the dilute hydrochloric acid has
reacted.
step 3Remove the excess zinc oxide.
step 4Obtain crystals of zinc chloride from the solution.
(a)Name the apparatus used in step 1 to:
(i)add the zinc oxide
........................................................................................................................................ [1]
(ii)warm the mixture.
........................................................................................................................................ [1]
(b)How did the student know that all of the dilute hydrochloric acid had reacted in step 2?
.....................................................................................................................................................
............................................................................................................................................... [1]
2A student investigated the rate of reaction between magnesium ribbon and solutions of dilute
hydrochloric acid of different concentrations, solutions H, I, J and K. The dilute hydrochloric acid
was in excess in all experiments.
Five experiments were done.
Experiment 1
●● A measuring cylinder was used to pour 30 cm3 of solution H into a beaker.
●● A 5.0 cm length of magnesium ribbon was then added to the beaker.
●● A timer was started immediately.
●● The time taken for all of the magnesium ribbon to react and to disappear completely was
measured.
Experiment 2
●● Experiment 1 was repeated but using solution I instead of solution H.
Experiment 3
●● Experiment 1 was repeated but using solution J instead of solution H.
Experiment 4
●● Experiment 1 was repeated but using solution K instead of solution H.
(a)Use the stop-clock diagrams to record the time taken for each experiment in the table.
experiment
solution
concentration of
hydrochloric acid
in mol / dm3
1
H
2.0
time taken for the
magnesium ribbon to
disappear completely / s
stop-clock
diagram
(c) (i)What is meant by the term excess in step 3?
0
........................................................................................................................................ [1]
45 15
(ii)How is the excess zinc oxide removed in step 3?
5
10
15
minutes
........................................................................................................................................ [1]
0
(d)Describe how the crystals are obtained in step 4.
2
I
1.5
45 15
.....................................................................................................................................................
.....................................................................................................................................................
3
J
1.0
45 15
(e)Suggest how the method would differ if zinc carbonate were used instead of zinc oxide.
5
15
5
15
10
............................................................................................................................................... [1]
[Total: 9]
15
0
............................................................................................................................................... [3]
5
10
0
4
K
0.8
45 15
10
[3]
© UCLES 2019
0971/62/M/J/19
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© UCLES 2019
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6
5
Experiment 5
Solution J was added to some magnesium ribbon in a test‑tube. The gas produced was tested. The
observations were recorded in the table.
observations
7
3Two substances, solid L and solid M, were analysed. Solid L was hydrated ammonium sulfate.
Tests were done on solid L and solid M.
(d) (i)Why was the same length of magnesium used in Experiments 1–4?
........................................................................................................................................ [1]
tests on solid L
(ii)Suggest the effect on the results if Experiments 1–4 were repeated using 2.5 cm lengths of
magnesium ribbon instead of 5.0 cm lengths of magnesium ribbon. Explain your answer.
rapid effervescence and the test-tube felt hot
lighted splint ‘popped’
Complete the expected observations.
(a)Describe the appearance of solid L.
..............................................................................................................................................
(b)Plot the results for Experiments 1–4 on the grid. Draw a smooth line graph.
............................................................................................................................................... [1]
........................................................................................................................................ [1]
Solid L was divided into two portions.
(e)Suggest a different method which a student could use to investigate the rate of reaction
between magnesium ribbon and dilute hydrochloric acid. State the apparatus the student
would use and the measurements the student would take.
(b) The first portion of solid L was heated in a hard-glass test-tube. Any gas produced was tested
with cobalt(II) chloride paper.
apparatus ....................................................................................................................................
observations ...............................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
measurements ............................................................................................................................
The second portion of solid L was added to distilled water. The mixture was shaken to dissolve
solid L and form solution L. The solution of L was divided into two equal portions in two test‑tubes.
.....................................................................................................................................................
time taken for the
magnesium ribbon to
disappear completely / s
.....................................................................................................................................................
[3]
(c) A
n excess of aqueous sodium hydroxide was added to the first portion of solution L. The
mixture was heated and the gas produced was tested.
observations ...............................................................................................................................
(f)Use the observations from Experiment 5 to answer these questions.
(i)
What type of chemical reaction occurs when magnesium ribbon reacts with dilute
hydrochloric acid?
............................................................................................................................................... [2]
........................................................................................................................................ [1]
(d)Dilute nitric acid and aqueous barium nitrate were added to the second portion of solution L.
observation ........................................................................................................................... [1]
(ii)Identify the gas produced.
0
0.5
1.0
1.5
2.0
2.5
concentration of hydrochloric acid in mol / dm
........................................................................................................................................ [1]
3.0
3
[3]
[Total: 16]
(c)
From your graph, deduce the time taken for the magnesium ribbon to disappear completely
if a solution of hydrochloric acid of concentration 2.5 mol / dm3 were used.
Show clearly on the grid how you worked out your answer.
............................................................................................................................................... [3]
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8
tests on solid M
Some of the tests and observations are shown.
tests on solid M
© UCLES 2019
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9
10
4Azurite is an ore of copper which contains copper(II) carbonate. Azurite contains no other metal
ions.
BLANK PAGE
Plan an experiment to show how a sample of copper could be obtained from large lumps of azurite.
observations
Your answer should include:
Solid M was dissolved in water. The solution was
divided into three portions.
●●
●●
test 1
escriptions of the reactions involved
d
the expected observations.
You are provided with a large lump of azurite and common laboratory chemicals and apparatus.
An excess of aqueous sodium hydroxide was
added to the first portion of the solution.
red-brown precipitate formed
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
test 2
An excess of aqueous ammonia was added to the
second portion of the solution.
............................................................................................................................................................
red-brown precipitate formed
............................................................................................................................................................
............................................................................................................................................................
test 3
Dilute nitric acid and aqueous silver nitrate were
added to the third portion of the solution.
............................................................................................................................................................
white precipitate formed
............................................................................................................................................................
...................................................................................................................................................... [6]
(e)Identify solid M.
............................................................................................................................................... [2]
© UCLES 2019
[Total: 9]
0971/62/M/J/19
© UCLES 2019
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12
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© UCLES 2019
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Cambridge International Examinations
Cambridge International General Certificate of Secondary Education (9–1)
0971/22
CHEMISTRY
Paper 2 Multiple Choice (Extended)
October/November 2018
45 minutes
Additional Materials:
*3087881514*
Multiple Choice Answer Sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
READ THESE INSTRUCTIONS FIRST
Write in soft pencil.
Do not use staples, paper clips, glue or correction fluid.
Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless
this has been done for you.
DO NOT WRITE IN ANY BARCODES.
There are forty questions on this paper. Answer all questions. For each question there are four possible
answers A, B, C and D.
Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.
Read the instructions on the Answer Sheet very carefully.
Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
Any rough working should be done in this booklet.
A copy of the Periodic Table is printed on page 16.
Electronic calculators may be used.
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2019
0971/62/M/J/19
© UCLES 2019
0971/62/M/J/19
This document consists of 16 printed pages.
IB18 11_0971_22/RP
© UCLES 2018
[Turn over
2
1
3
Oxygen and fluorine are gaseous elements next to each other in the Periodic Table.
4
Under the same conditions of temperature and pressure, oxygen diffuses ......1...... than fluorine
because its ......2...... is less than that of fluorine.
2
Both isotopes react with iron to form rust.
25 g of calcium carbonate is reacted with an excess of dilute nitric acid.
B
Neither isotope reacts with iron to form rust.
1
2
C
Only 16O reacts with iron to form rust.
molecular mass
D
Only 17O reacts with iron to form rust.
faster
reactivity
C
slower
molecular mass
D
slower
reactivity
5
6
The diagrams show four pieces of laboratory equipment.
balance
pipette
stop-clock
Which mass of calcium nitrate and which volume of carbon dioxide is produced at room
temperature and pressure?
mass of
calcium nitrate / g
A
29
6
A
B
29
12
C
41
6
D
41
12
5
B
6
C
8
D
10
Potassium bromide and methanol are both compounds.
Their melting points are different.
thermometer
9
substance with the
higher melting point
B
methanol
the attractive forces between molecules is greater
than the attractive forces between oppositely charged ions
C
potassium bromide
the attractive forces between oppositely charged ions
is greater than the attractive forces between molecules
D
potassium bromide
the attractive forces between molecules is greater
than the attractive forces between oppositely charged ions
Which equipment is essential to find out if dissolving a salt in water is an exothermic process?
balance
pipette
stop-clock
thermometer
B
C
A
D
B
16 g of oxygen
C
28 g of carbon monoxide
D
28 g of nitrogen
7
How many neutrons are present in the atom 45
21 X ?
21
B
24
C
© UCLES 2018
45
D
PO43–
SO42–
Mg2+
NO3–
K+
Cl –
Which formula is not correct?
Al 3(SO4)2
A
B
K3PO4
C
Mg(NO3)2
D
TiCl 4
Which gas sample contains the smallest number of molecules?
4 g of helium
© UCLES 2018
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5
© UCLES 2018
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6
10 Concentrated aqueous copper(II) chloride is electrolysed using copper electrodes as shown.
7
13 The equation for the formation of ammonia is shown.
11 The diagram shows a circuit used to electrolyse aqueous copper(II) sulfate.
N2 + 3H2 → 2NH3
power supply
+
–
power supply
3
+
negative ion
Ti4+
Al 3+
66
0971/22/O/N/18
copper electrodes
positive ion
the attractive forces between oppositely charged ions
is greater than the attractive forces between molecules
A
The formulae of some ions are shown.
reason why the melting points are different
methanol
A
A
volume of
carbon dioxide / dm3
How many electrons are used to form covalent bonds in a molecule of methanol, CH3OH?
Which row is correct?
3
The equation for the reaction between calcium carbonate and dilute nitric acid is shown.
CaCO3(s) + 2HNO3(aq) → Ca(NO3)2(aq) + CO2(g) + H2O(l)
A
faster
B
8
Which statement is correct?
Which words correctly complete gaps 1 and 2?
A
4
Two naturally occurring isotopes of oxygen are 16O and 17O.
4
–
+
copper electrodes
activation
energy
= +250 kJ / mol
–
aqueous copper(II) chloride
2
total energy
released
= –342 kJ / mol
N2 + 3H2
energy
1
What happens to the mass of each electrode during this process?
The energy level diagram for the reaction is shown.
aqueous
copper(II) sulfate
energy
change
2NH3
Which arrows indicate the movement of the copper ions in the electrolyte and of the electrons in
the external circuit?
positive electrode
negative electrode
A
decreases
decreases
copper ions
electrons
B
decreases
increases
A
1
3
C
increases
decreases
B
1
4
A
–592 kJ / mol
D
increases
increases
C
2
3
B
–92 kJ / mol
D
2
4
C
+92 kJ / mol
D
+592 kJ / mol
progress of reaction
What is the energy change for the reaction?
12 Hydrogen peroxide, H–O–O–H, decomposes to form water and oxygen.
14 The rate of reaction between magnesium ribbon and 2 mol / dm3 hydrochloric acid at 25 °C to
produce hydrogen gas is measured.
2H2O2(g) → 2H2O(g) + O2(g)
The bond energies are shown in the table. The reaction is exothermic.
bond
bond energy
in kJ / mol
In another experiment, either the concentration of the hydrochloric acid or the temperature is
changed. All other conditions are kept the same.
Which conditions increase the rate of reaction?
O–H
+460
A
1 mol / dm3 hydrochloric acid at 25 °C
O–O
+150
B
2 mol / dm3 hydrochloric acid at 10 °C
O=O
+496
C
2 mol / dm3 hydrochloric acid at 20 °C
D
3 mol / dm3 hydrochloric acid at 25 °C
What is the energy change for the reaction?
A
© UCLES 2018
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0971/22/O/N/18
–346 kJ / mol
B
–196 kJ / mol
© UCLES 2018
C
+196 kJ / mol
D
+346 kJ / mol
© UCLES 2018
0971/22/O/N/18
8
9
15 Methanol is prepared by the reversible reaction shown.
CO(g) + 2H2(g)
10
18 When dilute sulfuric acid is added to solid X, a colourless solution is formed and a gas is
produced.
CH3OH(g)
Which conditions produce the highest equilibrium yield of methanol?
21 Elements in Group I of the Periodic Table react with water.
Which row describes the products made in the reaction and the trend in reactivity of the
elements?
What is X?
The forward reaction is exothermic.
A
copper(II) oxide
B
sodium oxide
temperature
pressure
C
copper(II) carbonate
A
high
high
D
sodium carbonate
B
high
low
C
low
high
D
low
low
19 A few drops of methyl orange are added to a reaction mixture.
During the reaction, a gas is produced and the methyl orange turns from red to orange.
products
trend in reactivity
A
metal hydroxide and hydrogen
less reactive down the group
B
metal hydroxide and hydrogen
more reactive down the group
C
metal oxide and hydrogen
less reactive down the group
D
metal oxide and hydrogen
more reactive down the group
22 The equation shows the reaction between a halogen and aqueous bromide ions.
What are the reactants?
16 The thermite reaction can be used to produce iron from iron(III) oxide.
The equation for the reaction is shown.
2Al + Fe2O3 → 2Fe + Al 2O3
Which statements about this reaction are correct?
A
1
Aluminium is the oxidising agent.
2
Aluminium is less reactive than iron.
3
Electrons are transferred from aluminium to iron.
4
The iron in the iron(III) oxide is reduced.
1 and 3
B
1 and 4
C
2 and 3
D
C
D
© UCLES 2018
aqueous sodium hydroxide and calcium carbonate
C
dilute hydrochloric acid and magnesium
D
dilute hydrochloric acid and aqueous sodium hydroxide
3 and 4
basic
B
B
A
●
Chlorides are soluble (except lead(II) chloride and silver chloride).
●
Nitrates are soluble.
●
Sulfates are soluble (except barium sulfate, calcium sulfate and lead(II) sulfate).
calcium chloride and ammonium nitrate
magnesium oxide, sulfur dioxide
carbon dioxide, calcium oxide
C
silver nitrate and zinc chloride
sulfur dioxide, carbon dioxide
calcium oxide, magnesium oxide
D
sodium carbonate and potassium sulfate
calcium oxide, carbon dioxide
0971/22/O/N/18
[Turn over
1
2
3
chlorine
brown
colourless
B
chlorine
colourless
brown
C
iodine
brown
colourless
D
iodine
colourless
brown
Which descriptions of R are correct?
number of outer shell
electrons in atoms of R
structure of gas R
A
2
diatomic molecules
B
2
single atoms
C
8
diatomic molecules
D
8
single atoms
© UCLES 2018
+
Br2
......3......
A
barium chloride and magnesium nitrate
© UCLES 2018
2X–
23 An inert gas R is used to fill weather balloons.
B
0971/22/O/N/18
→
......2......
Which words complete gaps 1, 2 and 3?
Carbonates are insoluble (except ammonium carbonate, potassium carbonate and
sodium carbonate).
sulfur dioxide, carbon dioxide
sulfur dioxide, magnesium oxide
2Br–
+
......1......
Which substances produce an insoluble salt when aqueous solutions of them are mixed?
acidic
magnesium oxide, calcium oxide
aqueous sodium hydroxide and ammonium chloride
20 Some general rules for the solubility of salts in water are listed.
17 In which row are the oxides correctly identified?
A
X2
A
●
[Turn over
0971/22/O/N/18
0971/22/O/N/18
11
12
13
27 Bauxite contains aluminium oxide.
31 The diagrams show experiments involving the rusting of iron.
Heating the copper(II) oxide formed with carbon produces copper.
Aluminium is extracted from aluminium oxide by electrolysis.
Which processes are involved in this conversion of copper(II) carbonate to copper?
Why is cryolite added to the electrolytic cell used to extract aluminium?
A
sublimation followed by oxidation
A
Cryolite prevents the carbon anodes being burned away.
B
sublimation followed by reduction
B
Cryolite removes impurities from the bauxite.
C
thermal decomposition followed by oxidation
C
Cryolite increases the rate at which aluminium ions are discharged.
D
thermal decomposition followed by reduction
D
Molten cryolite dissolves the aluminium oxide.
tube P
tube Q
tube R
oil
iron nails
water
29 Which statements about sulfur dioxide pollution are correct?
What is the approximate percentage of argon in air?
79%
D
99%
respiration and photosynthesis
33 Which statement about sulfur or one of its compounds is correct?
26 Which statement about the uses of metals is not correct?
A
Sulfur occurs naturally as the element sulfur.
A
Aluminium is used in aircraft because of its strength and good electrical conductivity.
B
Sulfur dioxide is used to kill bacteria in drinking water.
B
Copper is used in electrical wiring because of its good electrical conductivity.
C
Sulfuric acid is a weak acid.
C
Stainless steel resists corrosion and is used to make cutlery.
D
Dilute sulfuric acid is a dehydrating agent.
D
Transition elements are often used as catalysts.
© UCLES 2018
0971/22/O/N/18
0971/22/O/N/18
© UCLES 2018
0971/22/O/N/18
© UCLES 2018
gaseous X
boiling or
evaporation
*0969174347*
solid X
October/November 2018
Give the scientific name for each of the numbered physical changes.
Candidates answer on the Question Paper.
2 ...........................................................................................................................................
No Additional Materials are required.
3 ...........................................................................................................................................
READ THESE INSTRUCTIONS FIRST
4 ...........................................................................................................................................
[4]
Write your Centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
(ii)Explain why the changes shown are physical changes.
..............................................................................................................................................
........................................................................................................................................ [1]
Answer all questions.
Electronic calculators may be used.
A copy of the Periodic Table is printed on page 16.
You may lose marks if you do not show your working or if you do not use appropriate units.
(iii)
One difference between boiling and evaporation is the rate at which the processes occur.
State one other difference between boiling and evaporation.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
2
–
lawrencium
Lr
No
nobelium
–
–
mendelevium
Md
Fm
fermium
–
–
Es
einsteinium
–
Cf
californium
–
Bk
berkelium
curium
Cm
–
–
americium
Am
Pu
plutonium
–
–
neptunium
Np
U
uranium
238
231
Pa
232
–
protactinium
Th
thorium
Ac
actinium
actinoids
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
103
175
Lu
71
70
173
Yb
ytterbium
102
101
169
Tm
thulium
69
68
Er
167
erbium
100
99
165
Ho
holmium
67
66
163
Dy
dysprosium
98
97
159
Tb
terbium
65
64
157
Gd
gadolinium
96
95
152
Eu
europium
63
62
94
Sm
samarium
150
–
93
Pm
promethium
61
60
144
Nd
neodymium
92
91
Pr
90
141
140
praseodymium
58
Ce
cerium
89
59
3
4
(b) Describe how the arrangement of electrons in a strontium atom is:
(i)similar to the arrangement of electrons in a calcium atom
..............................................................................................................................................
1 ...........................................................................................................................................
1 hour 15 minutes
1
number of electrons
[1]
3
Paper 4 Theory (Extended)
57
(a) Complete the table to show the arrangement of electrons in a calcium atom.
shell number
1
(a) (i)
139
Magnesium, calcium and strontium are Group II elements.
4
liquid X
0971/42
La
3
2
2
CHEMISTRY
lanthanum
0971/22/O/N/18
2
1Element X can undergo the following physical changes.
Cambridge International Examinations
Cambridge International General Certificate of Secondary Education (9 –1)
lanthanoids
Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local
Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2018
lutetium
–
Lv
livermorium
–
–
Fl
flerovium
actinoids
Ra
radium
Fr
francium
–
Cn
86
radon
Rn
At
astatine
–
–
polonium
Po
Bi
209
bismuth
lead
207
Pb
Tl
thallium
204
201
Hg
mercury
gold
197
Au
Pt
platinum
195
192
iridium
Ir
Os
osmium
190
186
rhenium
Re
W
tungsten
184
181
88
87
Ta
tantalum
54
Hf
137
133
178
89–103
Ba
barium
Cs
caesium
hafnium
85
84
83
82
81
80
79
78
77
76
75
74
73
72
57–71
lanthanoids
56
55
41
84
131
Xe
I
53
iodine
127
128
Te
tellurium
52
51
122
Sb
antimony
tin
50
119
Sn
49
In
indium
115
112
Cd
cadmium
48
47
silver
Ag
108
106
Pd
palladium
46
45
Rh
rhodium
103
101
Ru
ruthenium
44
43
Tc
technetium
–
96
42
molybdenum
Mo
Nb
niobium
93
91
40
39
19
Zr
88
Sc
24
20
23
zirconium
89
38
Sr
strontium
37
36
40
Kr
Br
bromine
80
79
selenium
Se
As
arsenic
75
73
germanium
Ge
Ga
gallium
70
65
zinc
Zn
Cu
copper
64
59
nickel
Ni
Co
cobalt
59
56
iron
Fe
Mn
55
18
20
Ar
21
magnesium
sodium
9
12
Mg
7
11
22
23
atomic symbol
Be
beryllium
Li
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
International Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at
www.cie.org.uk after the live examination series.
Na
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
manganese
35.5
35
34
32
31
33
32
28
OH
85
H
Rb
H
rubidium
HO
C
24
H
H
C
C
lithium
H
C
H
atomic number
C
4
D
C
3
C
H
Key
B
H
H
II
2
C
H
I
1
H
D
OH
52
Which of these processes use a catalyst?
C
H
Cr
OH OH
chromium
B
OH
V
A
reaction between steam and ethene.
51
fermentation
2
25
1
vanadium
H
Which monomer is used to make this polymer?
37 Ethanol can be formed by:
48
H
Ti
H
titanium
H
45
H
40
C
H
Ca
C
calcium
C
K
OH
C
39
OH H
C
potassium
OH H
C
ethene and ethanol
28
H
ethene and ethanoic acid
D
27
ethane and ethanol
C
26
B
Group
ethane and ethanoic acid
The Periodic Table of Elements
40 The structure of an addition polymer is shown.
A
29
36 Which two compounds are molecules which both contain a double bond?
A
31
30
27
argon
chlorine
sulfur
phosphorus
neon
14
silicon
12
C
Si
carbon
11
B
13
Al
boron
reduction of ethene
name
reduction of ethanol
D
relative atomic mass
oxidation of ethene
C
6
oxidation of ethanol
B
5
A
CH4 + Cl 2 → CH2Cl 2 + H2
2CH4 + 2Cl 2 → 2CH3Cl + Cl 2 + H2
III
CH4 + Cl 2 → CH4Cl 2
C
D
IV
39 Which reaction can be used to make ethanoic acid?
aluminium
Ne
F
19
Cl
fluorine
17
16
16
O
oxygen
S
P
15
14
N
7
nitrogen
9
8
VI
V
CH4 + Cl 2 → CH3Cl + HCl
B
2
It uses non-renewable materials.
35 Which equation representing a reaction of methane is correct?
A
4
It needs high temperature and pressure.
D
10
C
He
VIII
It has high labour costs.
It is used to treat acidic soil.
helium
It is a continuous process.
B
D
VII
A
It is used to neutralise acidic industrial waste.
1
What is an advantage of this process?
It is used to desulfurise flue gases.
C
hydrogen
It is used as a bleach in the manufacture of wood pulp.
B
1
A
xenon
16
krypton
15
38 Ethanol is manufactured from ethene.
scandium
14
34 What is not a use of lime?
[Turn over
0971/22/O/N/18
Y
© UCLES 2018
yttrium
[Turn over
0971/22/O/N/18
H
© UCLES 2018
copernicium
C
–
20%
Rg
B
roentgenium
1%
–
A
combustion and respiration
Ds
X
D
darmstadtium
W
combustion and photosynthesis
C
–
Z
combustion and carbonate formation
B
Mt
Y
30 Argon is a noble gas used to fill light bulbs.
A
meitnerium
D
2 and 3
–
X
D
Hs
Z
1 and 3
hassium
W
C
–
Y
2 only
Bh
C
B
2 and 3 only
bohrium
Y
D
–
W
1 and 3 only
Sg
Z
C
seaborgium
X
It causes respiratory problems.
1 only
1 and 2 only
–
B
A
B
Db
Y
1, 2 and 3
dubnium
Z
A
32 In the carbon cycle, which two processes add carbon dioxide to the atmosphere?
–
W
It damages limestone buildings.
3
most reactive
X
It increases the pH of rivers.
2
In tube R, the iron nails do not rust.
Rf
least reactive
A
1
In tube Q, the iron nails do not rust.
3
Which predictions are correct?
fizzes
What is the order of reactivity of the four metals starting with the least reactive?
In tube P, the iron nails rust.
2
rutherfordium
fizzes
violently
1
–
no reaction
The reaction takes place at room temperature and pressure.
–
fizzes
D
116
no reaction
A student predicted the following results.
114
fizzes
vigorously
Nitrogen reacts with hydrogen to make ammonia.
112
no reaction
The nitrogen used is obtained from nitrates in the soil.
C
111
fizzes
B
110
Z
anhydrous
calcium chloride
to dry the air
109
reaction with dilute
hydrochloric acid
Y
The hydrogen used is obtained from the air.
108
reaction with water
X
A
107
metal
W
water boiled to
remove the air
28 Which statement about the Haber process is correct?
106
The results are shown.
105
25 Four metals, W, X, Y and Z, are separately reacted with water and dilute hydrochloric acid.
104
24 Heating copper(II) carbonate produces copper(II) oxide and carbon dioxide.
..............................................................................................................................................
(ii)different from the arrangement of electrons in a calcium atom.
..............................................................................................................................................
..............................................................................................................................................
[2]
(c)Calcium reacts with cold water to form two products:
●●
●●
........................................................................................................................................ [1]
..............................................................................................................................................
........................................................................................................................................ [1]
colourless gas, P, which ‘pops’ with a lighted splint
a
a weakly alkaline solution, Q, which turns milky when carbon dioxide is bubbled through it.
(i)Name gas P.
(ii)
Identify the ion responsible for making solution Q alkaline.
........................................................................................................................................ [1]
(b) Describe the separation, arrangement and motion of particles of element X in the solid state.
separation ...................................................................................................................................
arrangement ...............................................................................................................................
motion .........................................................................................................................................
[3]
(iii)Suggest the pH of solution Q.
........................................................................................................................................ [1]
(iv)Write a chemical equation for the reaction of calcium with cold water.
........................................................................................................................................ [2]
(c)Element X is a Group I metal. It burns in air to form an oxide X2O.
Write a chemical equation for this reaction.
This document consists of 13 printed pages and 3 blank pages.
IB18 11_0971_42/FP
© UCLES 2018
............................................................................................................................................... [2]
[Turn over
[Total: 11]
© UCLES 2018
0971/42/O/N/18
© UCLES 2018
0971/42/O/N/18
[Turn over
4
6
5
(d) Magnesium reacts with chlorine to form magnesium chloride, MgCl 2. Magnesium chloride is
an ionic compound.
3Sulfur is an important element.
(c)Dilute sulfuric acid is used to make salts known as sulfates.
(a) Explain how burning fossil fuels containing sulfur leads to the formation of acid rain.
(i)Complete the diagrams to show the electronic structures of the ions in magnesium chloride.
Show the charges on the ions.
A method consisting of three steps is used to make zinc sulfate from zinc carbonate.
.....................................................................................................................................................
step 1
.....................................................................................................................................................
......
Cl
......
......
Mg
............................................................................................................................................... [2]
Cl
(i)
(i)
(ii)
1 ...........................................................................................................................................
State the conditions and name the catalyst used in this reversible reaction.
2 ...........................................................................................................................................
temperature .........................................................................................................................
3 ...........................................................................................................................................
[3]
pressure ...............................................................................................................................
(ii)State two observations which would show that the reaction is complete in step 1.
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
(iii)
(e)Aqueous magnesium chloride is added to aqueous silver nitrate. A white precipitate forms.
(iii)
(iv)
Describe how the sulfur trioxide formed is converted into sulfuric acid in the next steps of
the Contact process.
............................................................................................................................................... [2]
..............................................................................................................................................
[Total: 16]
..............................................................................................................................................
Why is it important to add an excess of zinc carbonate in step 1?
........................................................................................................................................ [1]
catalyst ................................................................................................................................
[3]
Write an ionic equation for this reaction. Include state symbols.
Heat the filtrate until a saturated solution forms and then allow it to crystallise.
Name a suitable piece of apparatus for measuring 20 cm3 of dilute sulfuric acid in step 1.
........................................................................................................................................ [1]
Write a chemical equation for this reversible reaction. Include the correct symbol to show
that the reaction is reversible.
........................................................................................................................................ [2]
(ii)Give three physical properties that are typical of ionic compounds such as MgCl 2.
step 3
(b) Sulfuric acid is manufactured by the Contact process. One step in the Contact process involves
a reversible reaction in which sulfur trioxide, SO3, is formed.
[3]
Add an excess of zinc carbonate to 20 cm3 of 0.4 mol / dm3 dilute sulfuric acid until
the reaction is complete.
step 2Filter the mixture.
What is meant by the term saturated solution in step 3?
..............................................................................................................................................
........................................................................................................................................ [2]
(v)The equation for the reaction is shown.
ZnCO3(s) + H2SO4(aq)
........................................................................................................................................ [2]
ZnSO4(......) + H2O(l) + CO2(g)
Complete the equation by inserting the state symbol for zinc sulfate.
(vi)
[1]
ame another zinc compound which could be used to make zinc sulfate from dilute
N
sulfuric acid using this method.
........................................................................................................................................ [1]
(vii)Suggest why this method would not work to make barium sulfate from barium carbonate
and dilute sulfuric acid.
........................................................................................................................................ [1]
© UCLES 2018
0971/42/O/N/18
© UCLES 2018
© UCLES 2018
9
(e)Iron(II) sulfate decomposes when heated strongly.
2FeSO4(s)
4
Fe2O3(s) + SO2(g) + SO3(g)
A student investigated the progress of the reaction between dilute hydrochloric acid, HCl, and an
excess of large pieces of marble, CaCO3, using the apparatus shown.
15.20 g of FeSO4(s) was heated and formed 4.80 g of Fe2O3(s).
Na2SO4 + 2H2O
gas syringe
[Mr, FeSO4 = 152; Mr, Fe2O3 = 160]
(i)What was the colour of the methyl orange in the aqueous sodium hydroxide?
Calculate the percentage yield for this reaction.
dilute
hydrochloric acid
........................................................................................................................................ [1]
(ii)
Determine the concentration of the dilute sulfuric acid in g / dm3.
●
an excess of large
pieces of marble
(a)A graph of the volume of gas produced against time is shown.
alculate the number of moles of aqueous sodium hydroxide added to the conical
C
flask.
150
.............................. % [3]
[Total: 26]
100
volume of gas
produced / cm3
.............................. mol
●
0971/42/O/N/18
8
7
(d) In a titration, a student added 25.0 cm3 of 0.200 mol / dm3 aqueous sodium hydroxide to a
conical flask. The student then added a few drops of methyl orange to the solution in the
conical flask.
Dilute sulfuric acid was then added from a burette to the conical flask. The volume of dilute
sulfuric acid needed to neutralise the aqueous sodium hydroxide was 20.0 cm3.
2NaOH + H2SO4
[Turn over
0971/42/O/N/18
50
Calculate the number of moles of dilute sulfuric acid added from the burette.
0
.............................. mol
●
0
30
60
90
120 150 180 210 240
time / s
Calculate the concentration of the dilute sulfuric acid in mol / dm .
3
(i)How does the shape of the graph show that the rate of reaction decreased as the reaction
progressed?
..............................................................................................................................................
........................................................................................................................................ [1]
.............................. mol / dm3
●
(ii)Why did the rate of reaction decrease as the reaction progressed?
Calculate the concentration of the dilute sulfuric acid in g / dm3.
........................................................................................................................................ [1]
(iii)
After how many seconds did the reaction finish?
.............................. g / dm3
[4]
© UCLES 2018
0971/42/O/N/18
[Turn over
.............................. s [1]
(b) The experiment was repeated using the same mass of smaller pieces of marble. All other
conditions were kept the same.
Draw a graph on the grid to show the progress of the reaction using the smaller pieces of
marble.
[2]
© UCLES 2018
0971/42/O/N/18
10
© UCLES 2018
escribe and explain, in terms of collisions between particles, the effect of using a higher
D
temperature on the time taken for the reaction to finish.
5
C 2H 2
C 3H 4
.....................................................................................................................................................
structure
H–C≡C–H
H–C≡C–CH3
.....................................................................................................................................................
name
ethyne
.....................................................................................................................................................
Name an oxidising agent which can be used to oxidise ethanol to ethanoic acid.
........................................................................................................................................ [2]
(a) Complete the table showing information about the first three alkynes.
formula
.....................................................................................................................................................
(e) (i)
Alkynes are a homologous series of unsaturated hydrocarbons.
ll members contain a C≡C triple bond.
A
.....................................................................................................................................................
.....................................................................................................................................................
[Turn over
12
11
(c)The original experiment was repeated at a higher temperature. All other conditions were kept
the same.
(ii)
H–C≡C–CH2–CH3
Draw the structure of ethanoic acid. Show all of the atoms and all of the bonds.
[1]
butyne
[2]
(f) Carboxylic acids can be converted into esters.
(i)
(b) Complete the dot-and-cross diagram to show the electron arrangement in a molecule of ethyne,
H–C≡C–H. Show outer shell electrons only.
The ester formed by reacting propanoic acid and methanol has the molecular formula
C4H8O2.
Name this ester and draw its structure. Show all of the atoms and all of the bonds.
.....................................................................................................................................................
name of the ester .................................................................................................................
.....................................................................................................................................................
H
............................................................................................................................................... [5]
0971/42/O/N/18
C
C
structure of the ester
H
[Total: 10]
[2]
[2]
(c)Compounds in the same homologous series have the same general formula.
(ii)Name another ester with the molecular formula C4H8O2.
(i)Give two other characteristics of members of a homologous series.
........................................................................................................................................ [1]
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
(ii)
(g)Polyesters are polymers.
(i)What type of polymerisation is used in the manufacture of polyesters?
Use the information in the table in (a) to deduce the general formula of alkynes.
........................................................................................................................................ [1]
........................................................................................................................................ [1]
(ii)Name a polyester.
(d) Alkynes are unsaturated.
........................................................................................................................................ [1]
Describe a test for unsaturation.
[Total: 17]
test ..............................................................................................................................................
result ...........................................................................................................................................
[2]
© UCLES 2018
0971/42/O/N/18
© UCLES 2018
0971/42/O/N/18
[Turn over
© UCLES 2018
0971/42/O/N/18
13
14
15
BLANK PAGE
BLANK PAGE
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable
effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will
be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International
Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after
the live examination series.
Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local
Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2018
0971/42/O/N/18
© UCLES 2018
0971/42/O/N/18
© UCLES 2018
0971/42/O/N/18
–
Lr
lawrencium
–
No
nobelium
Md
mendelevium
–
–
Fm
fermium
–
Es
einsteinium
–
Cf
californium
–
Bk
magnesium
burning
0971/62
CHEMISTRY
October/November 2018
Paper 6 Alternative to Practical
1 hour
............................................................................................................................................... [1]
No Additional Materials are required.
(c) Name the product formed when the magnesium ribbon was burned in air.
Write your Centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
............................................................................................................................................... [1]
The product from burning the magnesium ribbon in air was added to water and heated. The solution
formed was tested with Universal Indicator solution.
Answer all questions.
Electronic calculators may be used.
You may lose marks if you do not show your working or if you do not use appropriate units.
(d)Suggest why the product was heated after it had been added to water. Explain your answer.
.....................................................................................................................................................
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
............................................................................................................................................... [2]
(e)Suggest the pH value shown when Universal Indicator was added to the mixture.
............................................................................................................................................... [1]
(f)State one safety precaution that should be taken when magnesium is burned in air.
............................................................................................................................................... [1]
[Turn over
© UCLES 2018
3
4
(a)Use the stop-clock diagrams to record the time taken for each experiment in the table.
experiment
number
volume of
solution L / cm3
volume of
distilled
water / cm3
●●
10
0
45 15
●●
●●
●●
●●
●●
8
2
45 15
5
15
5
15
5
15
80
time taken for
the mixture to
turn blue-black / s
60
30
0
40
0
3
6
4
45 15
Experiment 2 was repeated but 6 cm3 of solution L and 4 cm3 of distilled water were added to
the conical flask before adding the other reagents.
20
10
30
0
Experiment 2 was repeated but 5 cm3 of solution L and 5 cm3 of distilled water were added to
the conical flask before adding the other reagents.
0
0
4
5
5
45 15
Experiment 5
●●
100
10
Experiment 4
●●
15
0
2
120
minutes
30
0
measuring cylinder was used to add 8 cm3 of solution L and 2 cm3 of distilled water to the
A
conical flask.
10 cm3 of dilute hydrochloric acid, 10 cm3 of sodium thiosulfate solution and 1 cm3 of
starch solution were then added to the conical flask.
The reaction was started by using a measuring cylinder to add 10 cm3 of solution M to the
conical flask. The timer was started immediately and the mixture was swirled.
The time taken for the mixture to turn blue-black was measured.
The conical flask was emptied and rinsed with distilled water.
Experiment 3
●●
5
10
Experiment 2
140
seconds
0
1
(b)Plot the results for Experiments 1–5 on the grid. Draw a smooth line graph.
time taken for
the mixture to
turn blue-black / s
stop-clock
diagram
0
A measuring cylinder was used to add 10 cm3 of solution L to a conical flask.
10 cm3 of dilute hydrochloric acid, 10 cm3 of sodium thiosulfate solution and 1 cm3 of
starch solution were then added to the conical flask.
The reaction was started by using a measuring cylinder to add 10 cm3 of solution M to the
conical flask. A timer was started immediately and the mixture was swirled.
The time taken for the mixture to turn blue-black was measured.
The conical flask was emptied and rinsed with distilled water.
0971/62/O/N/18
5
Experiment 1
●●
●●
[Total: 7]
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IB18 11_0971_62/FP
© UCLES 2018
0971/42/O/N/18
Five experiments were done.
[1]
(b)Suggest the appearance of the product formed when the magnesium ribbon was burned in air.
Candidates answer on the Question Paper.
2A student investigated the rate of reaction between solution L, solution M and hydrochloric acid.
When these chemicals react they form iodine. Sodium thiosulfate solution and starch solution were
used to show how fast the reaction proceeded.
●●
●●
(a)Complete the box to name the apparatus.
READ THESE INSTRUCTIONS FIRST
berkelium
curium
U
232
231
238
uranium
Pa
protactinium
Th
–
actinium
Ac
thorium
–
–
–
–
Cm
Am
americium
Pu
plutonium
Np
neptunium
96
actinoids
lanthanoids
.........................................
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
103
71
69
169
70
102
101
68
167
erbium
Er
66
67
99
98
65
97
163
152
63
62
150
–
64
95
94
93
141
59
58
140
60
92
91
90
57
89
139
lanthanum
La
144
Nd
neodymium
Pr
praseodymium
Ce
cerium
61
157
Gd
gadolinium
Eu
europium
Sm
samarium
Pm
promethium
159
terbium
Tb
165
Ho
holmium
Dy
dysprosium
100
173
Yb
ytterbium
Tm
thulium
175
Lu
lutetium
–
–
livermorium
–
flerovium
–
copernicium
–
roentgenium
–
–
–
radium
francium
–
181
–
seaborgium
dubnium
rutherfordium
–
–
–
–
darmstadtium
meitnerium
hassium
bohrium
Rn
radon
–
At
astatine
–
116
Lv
Po
polonium
Bi
bismuth
209
Fl
lead
114
207
Pb
Tl
204
thallium
112
201
Hg
mercury
Cn
111
gold
197
Rg
Au
Pt
110
195
Ds
platinum
Ir
109
192
Mt
iridium
108
190
Hs
Os
osmium
107
W
105
Rf
106
Sg
Db
104
178
89–103
88
137
Ba
Ra
87
barium
Fr
Cs
actinoids
184
tungsten
Ta
tantalum
Hf
hafnium
186
Bh
Re
rhenium
78
caesium
133
54
86
85
84
83
82
81
80
79
77
76
75
74
73
72
57–71
56
55
Y
lanthanoids
84
131
Xe
I
xenon
122
128
Te
tellurium
Sb
tin
119
115
In
indium
112
Cd
cadmium
91
93
96
Mo
molybdenum
Nb
niobium
Zr
88
89
yttrium
Sr
strontium
Rb
rubidium
39
38
37
85
36
42
41
40
zirconium
–
101
103
106
Pd
palladium
Rh
rhodium
Ru
ruthenium
Tc
technetium
108
Ag
silver
Sn
antimony
127
iodine
53
52
51
50
49
48
47
45
44
43
46
40
krypton
Kr
35
80
Br
bromine
79
75
33
34
Se
selenium
As
arsenic
73
32
germanium
Ge
30
65
70
zinc
31
Ga
gallium
Zn
64
29
copper
Cu
28
59
nickel
Ni
26
56
27
iron
55
25
59
Co
cobalt
Fe
Mn
manganese
52
24
51
V
22
Ti
K
Ca
21
Sc
scandium
20
calcium
19
potassium
23
24
magnesium
sodium
9
12
Be
Mg
beryllium
7
11
Li
Na
48
Cr
chromium
23
vanadium
titanium
name
relative atomic mass
atomic symbol
atomic number
lithium
45
1
4
40
18
20
Ar
hydrogen
Key
3
39
35.5
32
31
28
27
neon
argon
chlorine
sulfur
phosphorus
silicon
aluminium
Ne
F
17
19
fluorine
Cl
S
16
16
O
oxygen
15
14
P
N
nitrogen
14
12
C
Si
carbon
11
B
13
6
5
Al
IV
III
Group
1
The Periodic Table of Elements
H
II
I
© UCLES 2018
2
1Magnesium ribbon was burned in air.
Cambridge International Examinations
Cambridge International General Certificate of Secondary Education (9 –1)
*4951915096*
boron
2
4
9
8
7
10
He
VII
VI
V
VIII
helium
16
0
2
4
6
8
10
volume of solution L / cm3
[4]
10
Experiment 2 was repeated but 3 cm3 of solution L and 7 cm3 of distilled water were added to
the conical flask before adding the other reagents.
(c)
From your graph, deduce the time taken for the mixture to turn blue-black if Experiment 2
were repeated using 4 cm3 of solution L and 6 cm3 of distilled water.
30
0
0
5
3
7
45 15
Show clearly on the grid how you worked out your answer.
5
15
............................................................................................................................................... [3]
10
30
[4]
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6
tests on solid O
3Solid N and solid O were analysed. Solid N was ammonium sulfate. Tests were done on each solid.
Some of the tests and observations are shown.
tests on solid N
........................................................................................................................................ [1]
(ii)Explain, in terms of particles, why the rate of reaction was greatest in this experiment.
Complete the expected observations.
tests on solid O
(a)Describe the appearance of solid N.
..............................................................................................................................................
..............................................................................................................................................
observations
The appearance of solid O was studied.
white crystals
............................................................................................................................................... [1]
........................................................................................................................................ [2]
Distilled water was added to some of solid O to
form solution O.
Solid N was dissolved in distilled water to form solution N. Solution N was divided into two portions
in two test‑tubes.
(e) (i)Suggest an advantage of using a graduated pipette instead of a measuring cylinder to
measure solution L.
Solution O was divided into two equal portions in
two test‑tubes.
(b) Dilute nitric acid and aqueous barium nitrate were added to the first portion of solution N.
........................................................................................................................................ [1]
test 1
observations ......................................................................................................................... [2]
(ii)Suggest and explain a disadvantage of using a graduated pipette instead of a measuring
cylinder to measure solution M.
An excess of aqueous sodium hydroxide was
added to the first portion of solution O.
(c)Aqueous sodium hydroxide was added to the second portion of solution N. The mixture was
heated and the gas produced was tested.
..............................................................................................................................................
........................................................................................................................................ [2]
(f)Suggest one way to improve the reliability of the results of these experiments.
observations ...............................................................................................................................
test 2
............................................................................................................................................... [2]
Dilute nitric acid and aqueous silver nitrate were
added to the second portion of solution O.
no reaction
white precipitate
(d)Name the gas produced in (c).
............................................................................................................................................... [1]
8
7
(d) (i)In which experiment, 1, 2, 3, 4 or 5, was the rate of reaction greatest?
test 3
............................................................................................................................................... [1]
[Total: 18]
A flame test was done on the rest of solid O.
lilac colour
(e)What conclusion can you draw about the identity of solid O from test 1?
............................................................................................................................................... [1]
(f)Identify solid O.
............................................................................................................................................... [2]
© UCLES 2018
0971/62/O/N/18
© UCLES 2018
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© UCLES 2018
[Total: 9]
0971/62/O/N/18
9
10
11
4When solid C and solid D separately react with dilute hydrochloric acid, one reaction is exothermic
and one reaction is endothermic.
BLANK PAGE
BLANK PAGE
Plan an investigation to determine:
●●
●●
hich reaction is exothermic and which reaction is endothermic
w
which energy change is greater.
You are provided with solid C and solid D, dilute hydrochloric acid and common laboratory apparatus.
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
...................................................................................................................................................... [6]
© UCLES 2018
[Total: 6]
0971/62/O/N/18
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Cambridge Assessment International Education
Cambridge International General Certificate of Secondary Education (9 –1)
*4798355395*
0971/62
CHEMISTRY
Paper 6 Alternative to Practical
October/November 2019
1 hour
Candidates answer on the Question Paper.
No Additional Materials are required.
READ THESE INSTRUCTIONS FIRST
Write your centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
Answer all questions.
Electronic calculators may be used.
You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable
effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will
be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International
Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after
the live examination series.
Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local
Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2018
0971/62/O/N/18
This document consists of 8 printed pages and 4 blank pages.
IB19 11_0971_62/FP
© UCLES 2019
[Turn over
© UCLES 2019
0971/62/O/N/19
4
3
1
A student did a single titration to find the concentration of a solution of dilute sulfuric acid.
2
The student added 25.0 cm3 of aqueous sodium hydroxide to a conical flask, followed by a few
drops of indicator. Dilute sulfuric acid was then added to the aqueous sodium hydroxide until the
solution was neutral.
Experiment 1
The apparatus used is shown in the diagram.
5
(c) P
lot the results for Experiments 1 and 2 on the grid. Draw two smooth line graphs.
Clearly label your graphs.
student investigated the temperature changes when two different solids, N and O, dissolve in
A
water.
Two experiments were done.
●●
●●
●●
●●
30
sing a measuring cylinder, 30 cm3 of distilled water was poured into a polystyrene cup.
U
The initial temperature of the distilled water was measured.
Solid N was added to the distilled water, a timer started and the mixture was stirred with a
stirring thermometer.
The temperature of the mixture was measured every 30 seconds for three minutes (180 seconds).
20
(a) Use the thermometer diagrams to record the temperatures in the table.
time / s
dilute
sulfuric acid
0
thermometer
diagram
aqueous
sodium hydroxide
60
90
120
150
180
25
25
25
30
30
30
30
20
20
20
25
25
25
25
15
15
15
20
20
20
20
temperature
of mixture
/ °C
10
temperature of
mixture / °C
(a)
Complete the boxes to name the apparatus.
[2]
[2]
Experiment 2
(b) Name a suitable indicator to use in the titration and give the colour change.
time / s
(c)
What readings should the student take when doing this single titration?
thermometer
diagram
.............................................................................................................................................. [2]
(d) After the titration, the student discarded the contents of the conical flask and rinsed the
conical flask with distilled water.
0
30
60
90
0
30
60
90
120
180
150
210
240
time / s
(b) Use the thermometer diagrams to record the temperatures in the table.
colour change from ........................................................ to . ......................................................
[2]
uggest and explain what would be the effect, if any, on the titration values if the conical flask
S
was not dried before repeating the titration.
0
Experiment 1 was repeated using a new polystyrene cup and solid O instead of solid N.
indicator ......................................................................................................................................
30
120
150
180
30
20
20
20
10
10
20
25
15
15
15
5
5
15
20
10
10
10
0
0
10
[3]
(d) (i)
From your graph, deduce the time taken for the initial temperature of the solution in
Experiment 2 to change by 3 °C.
Show clearly on the grid how you worked out your answer.
temperature of
mixture / °C
[2]
....................................................................................................................................................
.............................. s [3]
(ii)
xtend your graph for Experiment 1 to give the expected temperature of the mixture after
E
240 seconds.
.............................. °C [2]
....................................................................................................................................................
(e) Is the energy change in Experiment 2 exothermic or endothermic? Explain your answer.
.............................................................................................................................................. [2]
....................................................................................................................................................
[Total: 8]
.............................................................................................................................................. [1]
© UCLES 2019
[Turn over
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© UCLES 2019
0971/62/O/N/19
6
© UCLES 2019
8
7
(f)State two possible sources of error in these experiments. Suggest two improvements to
reduce each of these sources of error.
source of error 1 .........................................................................................................................
3
Two substances, solid P and solid Q, were analysed. Solid P was copper(II) nitrate.
ests were done on solid P and solid Q.
T
tests on solid Q
Some of the tests and observations are shown.
tests on solid P
improvement 1 . ..........................................................................................................................
Complete the expected observations.
source of error 2 .........................................................................................................................
(a) A flame test was done on solid P.
tests on solid Q
improvement 2 . ..........................................................................................................................
[4]
observations ������������������������������������������������������������������������������������������������������������������������ [1]
[Total: 17]
Solid P was added to distilled water and the mixture shaken to dissolve solid P and form solution P.
Solution P was divided into three equal portions in two test‑tubes and one boiling tube.
A flame test was done on solid Q.
Solid Q was dissolved in water.
Dilute nitric acid and aqueous silver nitrate were
added to the solution.
observations ������������������������������������������������������������������������������������������������������������������������ [1]
.............................................................................................................................................. [2]
[Total: 9]
An excess of aqueous ammonia was then added to this mixture.
observations ����������������������������������������������������������������������������������������������������������������� [2]
(d) Aluminium foil and aqueous sodium hydroxide were added to the third portion of solution P in
a boiling tube. The mixture was heated and the gas produced tested.
observations ...............................................................................................................................
.............................................................................................................................................. [2]
© UCLES 2019
0971/62/O/N/19
© UCLES 2019
9
4
The table gives some information about the properties of three substances found in a hand cream.
substance
0971/62/O/N/19
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© UCLES 2019
0971/62/O/N/19
10
11
BLANK PAGE
BLANK PAGE
reaction with dilute nitric acid
polystyrene beads
no reaction
calcium carbonate
reacts and dissolves
sodium fluoride
dissolves
se the information in the table to plan an experiment to obtain a pure, dry sample of
U
polystyrene beads from this mixture of substances.
You are provided with a mixture of the three substances and common laboratory apparatus.
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
..................................................................................................................................................... [6]
© UCLES 2019
0971/62/O/N/19
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© UCLES 2019
0971/62/O/N/19
cream precipitate formed
(e)
Identify solid Q.
few drops of aqueous ammonia were added to the second portion of solution P in a
A
test‑tube.
observations ����������������������������������������������������������������������������������������������������������������� [1]
lilac colour
test 2
(b)
An excess of aqueous sodium hydroxide was added to the first portion of solution P in a
test‑tube.
(ii)
observations
test 1
(c) (i)
[Turn over
0971/62/O/N/19
© UCLES 2019
0971/62/O/N/19
12
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2019
0971/62/O/N/19