UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS
General Certificate of Education Ordinary Level
* 2 3 2 5 3 8 8 8 4 8 *
5070/21
CHEMISTRY
Paper 2 Theory
October/November 2013
1 hour 30 minutes
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 a soft pencil for any diagrams, graphs or rough working.
Do not use staples, paper clips, highlighters, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
Section A
Answer all questions.
Write your answers in the spaces provided in the Question Paper.
Section B
Answer any three questions.
Write your answers in the spaces provided in the Question Paper.
Electronic calculators may be used.
You may lose marks if you do not show your working or if you do not use appropriate units.
A copy of the Periodic Table is printed on page 16.
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 16 printed pages.
DC (SJF/SW) 58088/4
© UCLES 2013
[Turn over
2
Section A
For
Examiner’s
Use
Answer all the questions in this section in the spaces provided.
The total mark for this section is 45.
A1 Choose from the following compounds to answer the questions below.
calcium oxide
carbon dioxide
carbon monoxide
copper(II) sulfate
ethanol
ethene
iron(II) chloride
iron(III) chloride
nitrogen dioxide
silver chloride
silver iodide
sulfur dioxide
Each compound can be used once, more than once or not at all.
Which compound is
(a) a solid, which when dissolved in water, gives a green precipitate with aqueous
ammonia,
...................................................................................................................................... [1]
(b) a colourless gas which is formed when limestone is heated strongly,
...................................................................................................................................... [1]
(c) a gas which is formed in the atmosphere by lightning activity,
...................................................................................................................................... [1]
(d) a basic oxide,
...................................................................................................................................... [1]
(e) formed when ethane undergoes complete combustion,
...................................................................................................................................... [1]
(f)
a white salt which is insoluble in water?
...................................................................................................................................... [1]
[Total: 6]
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A2 Alkenes are a homologous series of unsaturated hydrocarbons.
For
Examiner’s
Use
(a) Give the general formula of alkenes.
...................................................................................................................................... [1]
(b) In addition to having a general formula, state two other characteristics of a homologous
series.
1 .......................................................................................................................................
2 ................................................................................................................................... [2]
(c) Alkenes can be made by cracking alkanes.
(i)
Give one condition required for cracking.
.............................................................................................................................. [1]
(ii)
Tetradecane, C14H30, can be cracked to form an alkene containing eight carbon
atoms and an alkane.
Construct an equation for this reaction.
[1]
(d) Ethene reacts with bromine to form 1,2-dibromoethane, CH2BrCH2Br.
Name this type of reaction.
...................................................................................................................................... [1]
(e) Ethene reacts with hydrogen chloride to form the covalent compound chloroethane,
CH3CH2Cl.
Suggest two physical properties of chloroethane.
1 .......................................................................................................................................
2 ................................................................................................................................... [2]
(f)
Halogenoalkanes such as CCl2F2 are responsible for the depletion of ozone in the
upper atmosphere.
Describe the importance of the ozone layer in the upper atmosphere.
..........................................................................................................................................
..........................................................................................................................................
...................................................................................................................................... [2]
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[Total: 10]
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A3 Calcium, proton number 20, is an element in Group II of the Periodic Table.
For
Examiner’s
Use
(a) Give the electronic configuration for calcium.
...................................................................................................................................... [1]
(b) Calcium has six naturally-occurring isotopes.
(i)
State the meaning of the term isotopes.
..................................................................................................................................
.............................................................................................................................. [1]
(ii)
Complete the following table to show the number of sub-atomic particles in two of
these isotopes.
isotope
number of
protons
number of
electrons
number of
neutrons
42Ca
48Ca
[3]
(c) Calcium chloride can be formed by reacting calcium carbonate with dilute hydrochloric
acid.
(i)
Construct an equation for this reaction.
[1]
(ii)
Write both the formula and the electronic configuration for the ions present in
calcium chloride.
[2]
(d) (i)
Name the products formed at the anode and cathode when molten calcium chloride
is electrolysed.
anode .......................................................................................................................
cathode ................................................................................................................ [1]
(ii)
Predict the product formed at the cathode when a dilute aqueous solution of
calcium chloride is electrolysed.
.............................................................................................................................. [1]
(iii)
Explain why solid calcium chloride does not conduct electricity.
.............................................................................................................................. [1]
[Total: 11]
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A4 Nitrogen and oxygen are present in dry air.
For
Examiner’s
Use
(a) What is the percentage composition by volume of each of these gases in dry air?
nitrogen ............................................................................................................................
oxygen ......................................................................................................................... [2]
(b) What method is used to separate these gases from each other?
...................................................................................................................................... [1]
(c) In a petrol engine, nitrogen and oxygen combine to form oxides of nitrogen such as
nitrogen dioxide, NO2.
State one harmful effect that nitrogen dioxide has on the environment.
...................................................................................................................................... [1]
(d) One of the hydrocarbons in petrol is octane, C8H18.
In a petrol engine, some of the octane reacts to form carbon monoxide and water.
Construct an equation for this reaction.
[2]
(e) Catalytic converters are used to remove carbon monoxide and nitrogen dioxide from the
exhaust gases of petrol engines.
A catalyst containing rhodium and platinum or palladium is present in a catalytic
converter.
What is the function of a catalyst?
...................................................................................................................................... [1]
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(f)
In a catalytic converter, carbon monoxide and nitrogen dioxide undergo redox reactions.
These reactions reduce the amount of carbon monoxide and nitrogen dioxide in car
exhausts.
(i)
What is meant by the term redox reaction?
..................................................................................................................................
.............................................................................................................................. [1]
(ii)
Explain how the redox reactions in the catalytic converter decrease the amounts of
carbon monoxide and nitrogen dioxide in car exhausts.
..................................................................................................................................
..................................................................................................................................
.............................................................................................................................. [2]
[Total: 10]
A5 Hydrogen peroxide, H2O2, is a colourless liquid.
(a) Calculate the percentage by mass of oxygen in hydrogen peroxide.
..............................................% [2]
(b) The enzyme catalase is present in yeast. The enzyme catalyses the decomposition of
aqueous hydrogen peroxide.
2H2O2(aq)
2H2O(l) + O2(g)
The apparatus below is used to monitor this reaction.
water
yeast
+ hydrogen
peroxide solution
water
What measurements should be taken in order to monitor the rate of this reaction?
..........................................................................................................................................
...................................................................................................................................... [2]
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Examiner’s
Use
7
(c) Describe and explain the effect of increasing the concentration of hydrogen peroxide on
the rate of this reaction.
For
Examiner’s
Use
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
...................................................................................................................................... [3]
(d) The graph below shows how the rate of decomposition of hydrogen peroxide, catalysed
by yeast, varies with temperature. All other conditions are kept constant.
rate of
reaction
0
10
20
30
40
50
temperature / °C
60
Suggest why the rate of reaction decreases rapidly from 45 °C to 60 °C.
...................................................................................................................................... [1]
[Total: 8]
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Section B
Answer three questions from this section in the spaces provided.
The total mark for this section is 30.
B6 Iron is extracted from its ore (haematite, Fe2O3) in a blast furnace.
Coke (carbon) and limestone (calcium carbonate) are also added to the furnace.
(a) Describe the essential reactions taking place in the blast furnace.
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
...................................................................................................................................... [4]
(b) Steel is an alloy made by the addition of carbon or metals to iron.
Use the diagrams below to explain why an alloy of iron and manganese is less malleable
than pure iron.
Key
iron atoms
manganese atoms
iron
alloy of iron and manganese
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
...................................................................................................................................... [2]
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Examiner’s
Use
9
(c) Iron reacts with dilute hydrochloric acid to form iron(II) chloride.
Fe(s) + 2HCl (aq)
For
Examiner’s
Use
FeCl2(aq) + H2(g)
A student added 2.1 g of iron to 50 cm3 of 0.10 mol / dm3 hydrochloric acid.
(i)
Calculate the amount, in moles, of iron present.
........................................... mol [1]
(ii)
Calculate the amount, in moles, of hydrochloric acid present.
........................................... mol [1]
(iii)
Calculate the volume of hydrogen formed in this reaction, measured at room
temperature and pressure.
...........................................cm3 [2]
[Total: 10]
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B7 (a) A compound of carbon, hydrogen and chlorine contains 0.48 g of carbon, 0.08 g of
hydrogen and 1.42 g of chlorine.
(i)
Deduce the empirical formula of this compound.
[2]
(ii)
The relative molecular mass of this compound is 99.
Deduce the molecular formula of this compound.
[1]
(b) Chloroethene is another compound containing carbon, hydrogen and chlorine.
The structure of chloroethene is shown below.
H
Cl
C
C
H
H
Draw a section of the polymer formed when chloroethene undergoes polymerisation to
form poly(chloroethene).
[2]
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Examiner’s
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11
(c) Poly(chloroethene) is an addition polymer but nylon is a condensation polymer.
Describe the difference between an addition polymer and a condensation polymer in
terms of how they are formed from their monomers.
For
Examiner’s
Use
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
...................................................................................................................................... [1]
(d) Chloroethene is made by reacting ethene with hydrogen chloride and oxygen in the
presence of a catalyst of copper(II) chloride, CuCl2. The other product of the reaction is
water.
(i)
Construct an equation for this reaction.
[1]
(ii)
Copper(II) chloride is made by heating copper(II) oxide, CuO, with hydrochloric
acid.
Construct an equation for this reaction.
[1]
(iii)
Copper is a transition element.
State two physical properties of copper which are different from those of a typical
Group I element such as sodium.
1 ...............................................................................................................................
2 ........................................................................................................................... [2]
[Total: 10]
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B8 Zinc sulfide is a compound that can be made by heating zinc powder with sulfur powder.
(a) Describe two differences between a mixture of zinc and sulfur and a compound of zinc
and sulfur.
1 .......................................................................................................................................
..........................................................................................................................................
2 .......................................................................................................................................
...................................................................................................................................... [2]
(b) The reaction between zinc and sulfur is exothermic.
Complete the energy profile diagram for this reaction.
On your diagram label
the product,
the enthalpy change for the reaction, ΔH.
energy
zinc + sulfur
progress of reaction
[2]
(c) Part of the structure of zinc sulfide is shown below.
Key
Zn ions
S ions
Deduce the empirical formula of zinc sulfide from this structure.
...................................................................................................................................... [1]
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Examiner’s
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13
(d) Zinc sulfide reacts with hydrochloric acid to form hydrogen sulfide.
An aqueous solution of hydrogen sulfide behaves as a weak acid.
For
Examiner’s
Use
Describe what is meant by the term weak acid.
..........................................................................................................................................
...................................................................................................................................... [1]
(e) Zinc sulfate can be made by reacting zinc with dilute sulfuric acid.
Zn(s) + H2SO4(aq)
(i)
ZnSO4(aq) + H2(g)
Write an ionic equation for this reaction.
[1]
(ii)
Describe how you would prepare crystals of pure, dry zinc sulfate using this
reaction.
..................................................................................................................................
..................................................................................................................................
..................................................................................................................................
..................................................................................................................................
.............................................................................................................................. [3]
[Total: 10]
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B9 Ethanoic acid reacts with sodium hydroxide to form water and a salt.
(a) Give the formula of the salt.
...................................................................................................................................... [1]
(b) The reaction between ethanoic acid and sodium hydroxide is described as a
neutralisation reaction.
Write the simplest ionic equation for this reaction.
...................................................................................................................................... [1]
(c) Ethanoic acid reacts with methanol to form an ester and water.
CH3CO2H + CH3OH
CH3CO2CH3 + H2O
The reaction is endothermic.
(i)
Describe what happens to the position of this equilibrium when the concentration of
methanol is increased. Explain your answer.
..................................................................................................................................
.............................................................................................................................. [1]
(ii)
Describe what happens to the position of this equilibrium when the temperature of
the reaction mixture is decreased. Explain your answer.
..................................................................................................................................
.............................................................................................................................. [1]
(d) The structure of the ester methyl benzoate is shown below.
H
O
O
C
H
C
C
C
C
C
H
H
H
C
H
C
H
H
Deduce the molecular formula for methyl benzoate.
...................................................................................................................................... [1]
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For
Examiner’s
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15
(e) Sodium hydroxide is an alkali.
Give the formula of the ion present in sodium hydroxide which causes it to be alkaline.
For
Examiner’s
Use
...................................................................................................................................... [1]
(f)
A student titrated a metal hydroxide with 0.200 mol/dm3 hydrochloric acid.
It required 12.5 cm3 of hydrochloric acid to neutralise 25.0 cm3 of 0.0500 mol / dm3 metal
hydroxide solution.
(i)
Calculate the amount, in moles, of hydrochloric acid used.
........................................... mol [1]
(ii)
Calculate the amount, in moles, of metal hydroxide present.
........................................... mol [1]
(iii)
Construct an equation for this reaction.
Use the letter M to represent the metal in the metal hydroxide solution.
[1]
(g) Name a metal hydroxide which can be used to treat excess acidity in soils.
...................................................................................................................................... [1]
[Total: 10]
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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.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of
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© UCLES 2013
5070/21/O/N/13
© UCLES 2013
20
Calcium
5070/21/O/N/13
Strontium
Actinium
†
Key
b
X
a
b = atomic (proton) number
X = atomic symbol
a = relative atomic mass
* 58–71 Lanthanoid series
† 90–103 Actinoid series
89
Radium
88
Francium
87
227
Ac
226
Ra
72
Hafnium
*
Lanthanum
57
178
Hf
40
Zirconium
Zr
91
Titanium
139
Yttrium
22
48
Ti
La
39
Y
89
Scandium
21
223
Barium
56
Caesium
45
Sc
Fr
55
137
Ba
133
Cs
38
Rubidium
37
88
Sr
85
Rb
19
Potassium
40
Ca
39
Magnesium
Sodium
12
24
Mg
23
Na
Beryllium
4
Lithium
K
11
3
9
Be
7
II
Li
I
93
Ta
181
Niobium
Nb
90
58
73
52
96
Mo
W
184
55
Tc
186
Re
144
Nd
92
60
Uranium
U
238
Neodymium
75
Rhenium
43
Technetium
25
Manganese
Mn
27
59
28
59
29
64
30
65
5
Ru
101
Iron
190
Pm
147
Osmium
Os
237
Np
93
Neptunium
61
Promethium
76
44
Ruthenium
26
56
Fe
150
Sm
244
Pu
94
Plutonium
62
Eu
152
Platinum
243
Am
95
Americium
63
Europium
78
Pt
Iridium
195
Ir
46
Palladium
Pd
106
Nickel
Ni
192
Samarium
77
45
Rhodium
Rh
103
Cobalt
Co
Gd
157
Gold
Au
197
Silver
96
64
Curium
Cm
247
Gadolinium
79
47
Ag
108
Copper
Cu
201
Bk
247
Terbium
Tb
159
Mercury
Hg
97
Berkelium
65
80
48
Cadmium
Cd
112
Zinc
Zn
11
6
Dy
162
Thallium
Tl
204
Indium
251
Cf
98
Californium
66
Es
252
Holmium
Ho
165
Lead
Pb
207
Tin
99
Einsteinium
67
82
50
119
Sn
115
32
Germanium
Ge
73
Silicon
In
Gallium
Dysprosium
81
49
31
70
Ga
14
28
Si
Carbon
27
Aluminium
13
12
C
Al
Boron
B
7
14
75
Sb
122
Arsenic
As
Bi
209
Fermium
Fm
257
Erbium
Er
167
Bismuth
100
68
83
51
Antimony
33
15
Phosphorus
P
31
Nitrogen
N
8
Se
79
Sulfur
S
32
Oxygen
209
Po
169
Md
258
Thulium
Tm
101
Mendelevium
69
84
Polonium
52
Tellurium
Te
128
Selenium
34
16
16
O
9
Yb
173
Astatine
At
210
Iodine
I
127
Bromine
Br
80
Chlorine
259
No
102
Nobelium
70
Ytterbium
85
53
35
17
Cl
35.5
Fluorine
F
19
Lr
260
Lutetium
Lu
175
Radon
Rn
222
Xenon
Xe
131
Krypton
Kr
84
Argon
Ar
40
Neon
103
Lawrencium
71
86
54
36
18
10
Ne
20
Helium
2
0
Hydrogen
VII
4
VI
He
V
1
IV
H
III
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
91
Protactinium
Thorium
231
Pa
Th
232
Praseodymium
Cerium
59
141
Pr
140
74
Tungsten
42
Molybdenum
24
Chromium
Cr
Ce
Tantalum
41
23
Vanadium
V
51
1
Group
DATA SHEET
The Periodic Table of the Elements
16
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS
General Certificate of Education Ordinary Level
* 4 1 7 8 9 7 1 3 5 7 *
5070/22
CHEMISTRY
Paper 2 Theory
October/November 2013
1 hour 30 minutes
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 a soft pencil for any diagrams, graphs or rough working.
Do not use staples, paper clips, highlighters, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
Section A
Answer all questions.
Write your answers in the spaces provided in the Question Paper.
Section B
Answer any three questions.
Write your answers in the spaces provided in the Question Paper.
Electronic calculators may be used.
You may lose marks if you do not show your working or if you do not use appropriate units.
A copy of the Periodic Table is printed on page 16.
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 16 printed pages.
DC (SJF/SW) 58087/5
© UCLES 2013
[Turn over
2
Section A
For
Examiner’s
Use
Answer all the questions in this section in the spaces provided.
The total mark for this section is 45.
A1 Choose from the following elements to answer the questions below.
chlorine
hydrogen
iron
lithium
nickel
nitrogen
oxygen
potassium
silver
sulfur
vanadium
zinc
Each element can be used once, more than once or not at all.
Which element
(a) is liberated at the anode when an aqueous solution of potassium sulfate is electrolysed,
...................................................................................................................................... [1]
(b) is used as a catalyst in the manufacture of margarine,
...................................................................................................................................... [1]
(c) is a non-metallic solid, an atom of which contains only six valency electrons,
...................................................................................................................................... [1]
(d) is higher than sodium in the reactivity series,
...................................................................................................................................... [1]
(e) is in Period 5 of the Periodic Table,
...................................................................................................................................... [1]
(f)
forms a white oxide which is amphoteric?
...................................................................................................................................... [1]
[Total: 6]
© UCLES 2013
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A2 Carboxylic acids are a homologous series containing the –CO2H group.
The table shows some properties of the first four carboxylic acids in the series.
carboxylic acid
molecular
formula
density
in g / cm3
boiling point
in °C
CH2O2
1.220
101
C2H4O2
1.049
118
propanoic acid
C3H6O2
0.993
141
butanoic acid
C4H8O2
0.958
165
methanoic acid
(a) (i)
For
Examiner’s
Use
Describe how the density of these carboxylic acids varies with the number of
carbon atoms in the molecule.
.............................................................................................................................. [1]
(ii)
Name the carboxylic acid with the molecular formula C2H4O2.
.............................................................................................................................. [1]
(iii)
Draw the structure of propanoic acid, showing all atoms and bonds.
[1]
(b) The next carboxylic acid in this homologous series is pentanoic acid.
Pentanoic acid has five carbon atoms.
(i)
Deduce the molecular formula for pentanoic acid.
.............................................................................................................................. [1]
(ii)
Suggest a value for the boiling point of pentanoic acid.
............................................. °C [1]
(c) Butanoic acid, C3H7CO2H, reacts with sodium to form a salt and a gas.
(i)
Name the gas.
.............................................................................................................................. [1]
(ii)
Give the formula of the salt.
.............................................................................................................................. [1]
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(d) Esters are formed when carboxylic acids react with alcohols.
The reaction is catalysed by hydrogen ions.
(i)
For
Examiner’s
Use
Describe and explain the effect of a catalyst on reaction rate.
..................................................................................................................................
..................................................................................................................................
.............................................................................................................................. [2]
(ii)
State one commercial use of esters.
.............................................................................................................................. [1]
(iii)
The structure of an ester is shown below.
O
H
C
O
H
H
H
C
C
C
H
H
H
H
Name this ester.
.............................................................................................................................. [1]
[Total: 11]
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A3 Silicon is an element in Group IV of the Periodic Table.
For
Examiner’s
Use
(a) Give the electronic configuration for a silicon atom.
...................................................................................................................................... [1]
(b) Silicon has three naturally occurring isotopes.
Complete the following table for two of these isotopes.
isotope
28Si
30Si
number of protons
number of electrons
number of neutrons
[3]
(c) Silicon reacts with chlorine on heating to form silicon(IV) chloride, SiCl4.
Construct an equation for this reaction.
[1]
(d) Silicon(IV) chloride is a simple molecular compound.
(i)
Suggest two physical properties of silicon(IV) chloride other than solubility.
1 ...............................................................................................................................
2 ........................................................................................................................... [2]
(ii) Draw a ‘dot-and-cross’ diagram for silicon(IV) chloride.
You only need to show the outer shell electrons for each atom.
[2]
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(e) Silicon(IV) chloride reacts with water to form silicon(IV) oxide.
Part of the structure of silicon(IV) oxide is shown below.
For
Examiner’s
Use
Key
silicon atom
oxygen atom
Explain, in terms of structure and bonding, why silicon(IV) oxide has a very high melting
point.
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
...................................................................................................................................... [2]
[Total: 11]
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A4 The carbon cycle regulates the amount of carbon dioxide in the atmosphere.
(a) (i)
For
Examiner’s
Use
State two processes which release carbon dioxide into the atmosphere.
1 ...............................................................................................................................
2 ........................................................................................................................... [2]
(ii)
Name one process which removes carbon dioxide from the atmosphere.
.............................................................................................................................. [1]
(b) Carbon dioxide is a greenhouse gas.
(i)
What is the meaning of the term greenhouse gas?
..................................................................................................................................
.............................................................................................................................. [1]
(ii)
Name another greenhouse gas and give a natural source of this gas.
name ........................................................................................................................
source .................................................................................................................. [2]
(c) Carbon dioxide dissolves in water to form a weakly acidic solution.
CO2(g) + H2O(l)
(i)
HCO3–(aq) + H+(aq)
What is the meaning of the term weak acid ?
..................................................................................................................................
.............................................................................................................................. [1]
(ii)
Describe how you could measure the pH of this solution other than by using a pH
meter.
..................................................................................................................................
..................................................................................................................................
.............................................................................................................................. [2]
(d) Sodium hydrogencarbonate, NaHCO3, decomposes on heating to form a carbonate,
water and a gas which turns limewater milky.
Construct an equation for this reaction.
[2]
[Total: 11]
© UCLES 2013
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8
A5 A student reacts magnesium ribbon with excess hydrochloric acid.
She follows the course of the reaction by measuring the volume of gas produced against
time.
(a) Write the equation for the reaction of magnesium with hydrochloric acid.
...................................................................................................................................... [1]
(b) (i)
On the axes below draw a sketch graph to show how the volume of gas produced
during the reaction varies with time and label this line ‘A’.
Label the axes with the appropriate units.
[2]
(ii)
The student then carries out the experiment at a lower temperature. All the other
conditions remain the same.
On the axes above draw another line to show how the volume of gas produced
varies with time and label this line ‘B’.
[1]
(c) Magnesium reacts with carbon to form the compound magnesium carbide.
Calculate the percentage by mass of magnesium in magnesium carbide, MgC2.
[2]
[Total: 6]
© UCLES 2013
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Examiner’s
Use
9
Section B
For
Examiner’s
Use
Answer three questions from this section in the spaces provided.
The total mark for this section is 30.
B6 Aluminium is extracted from purified bauxite by electrolysis.
(a) Describe how this electrolysis is carried out and construct equations for the reactions
occurring at both the anode and cathode.
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
...................................................................................................................................... [4]
(b) What properties of aluminium make it useful for
(i)
making aircraft, .........................................................................................................
(ii)
making electricity cables. ...................................................................................... [2]
(c) Aluminium is high in the reactivity series.
(i)
Explain why aluminium does not react with aqueous copper(II) sulfate.
..................................................................................................................................
.............................................................................................................................. [2]
(ii)
When a few drops of aqueous sodium chloride are added to a mixture of aluminium
and aqueous copper(II) sulfate, a vigorous reaction occurs.
copper(II) sulfate + aluminium
aluminium sulfate + copper
What type of reaction is this?
.............................................................................................................................. [1]
(iii)
State the formula of aluminium sulfate.
.............................................................................................................................. [1]
[Total: 10]
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10
B7 Ethene is an unsaturated hydrocarbon.
For
Examiner’s
Use
(a) What is the meaning of each of these terms?
unsaturated ......................................................................................................................
hydrocarbon ................................................................................................................. [2]
(b) Ethene can be manufactured by cracking.
(i)
State the conditions used for cracking.
..................................................................................................................................
.............................................................................................................................. [2]
(ii)
Construct an equation for the cracking of tetradecane, C14H30, to form ethene and
one other hydrocarbon.
.............................................................................................................................. [1]
(c) Alkenes such as ethene can undergo addition polymerisation.
(i)
State one use of poly(ethene).
.............................................................................................................................. [1]
(ii)
The diagram below shows a section of a polymer chain.
C2H5
CH
C2H5
CH2
CH
C2H5
CH2
CH
CH2
Deduce the structure of the monomer which is used to make this polymer.
[1]
© UCLES 2013
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11
(d) Ethanol can be manufactured by the catalytic addition of steam to ethene.
C2H4 + H2O
For
Examiner’s
Use
C2H5OH
If the reactants are not recycled, only 5% of the ethene is converted to ethanol.
Calculate the mass of ethanol formed from 0.4 tonnes of ethene when only 5% of the
ethene is converted to ethanol.
[1 tonne is 1 000 000 grams]
mass of ethanol ...................................... tonnes [3]
[Total: 10]
© UCLES 2013
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12
B8 When hydrogen iodide, HI, is heated in a closed tube, the following dynamic equilibrium is
established.
2HI(g)
H2(g) + I2(g)
ΔH = + 9.6 kJ / mol
(a) What is meant by the term dynamic equilibrium?
..........................................................................................................................................
..........................................................................................................................................
...................................................................................................................................... [2]
(b) The table shows the concentrations of HI(g), H2(g) and I2(g) in the equilibrium mixture
at 25 °C and 450 °C.
(i)
substance
concentration at 25 °C
/ mol / dm3
concentration at 450 °C
/ mol / dm3
HI(g)
0.94
0.79
H2(g)
0.033
0.11
I2(g)
0.033
0.11
The tube has a volume of 50 cm3.
Calculate the mass of hydrogen iodide in the equilibrium mixture at 25 °C.
[2]
(ii)
Describe and explain the differences in the concentrations of reactant and products
at 25 °C and 450 °C.
..................................................................................................................................
..................................................................................................................................
..................................................................................................................................
.............................................................................................................................. [2]
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Examiner’s
Use
13
(c) Complete the energy profile diagram for the decomposition of hydrogen iodide.
On your diagram label
• the products,
• the enthalpy change of the reaction, ΔH.
energy
For
Examiner’s
Use
reactants
progress of reaction
[2]
(d) An aqueous solution of hydrogen iodide contains iodide ions.
Describe a test for iodide ions.
..........................................................................................................................................
...................................................................................................................................... [2]
[Total: 10]
© UCLES 2013
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14
B9 The compounds ammonium nitrate and ammonium sulfate are both fertilisers.
(a) Explain why farmers add these fertilisers to soils.
..........................................................................................................................................
...................................................................................................................................... [1]
(b) Ammonium sulfate can be prepared by adding sulfuric acid to aqueous ammonia.
Construct the equation for this reaction.
...................................................................................................................................... [1]
(c) Excess acidity in soils can be treated by adding calcium hydroxide.
(i)
Give the formula of the ion present in calcium hydroxide which causes it to be
alkaline.
.............................................................................................................................. [1]
(ii)
Explain why adding calcium hydroxide causes loss of nitrogen from fertilisers such
as ammonium nitrate, which have been previously added to the soil.
..................................................................................................................................
..................................................................................................................................
.............................................................................................................................. [2]
(d) A student titrated 10.0 cm3 of aqueous calcium hydroxide with hydrochloric acid.
Ca(OH)2(aq) + 2HCl(aq)
CaCl2(aq) + 2H2O(l)
It required 4.00 cm3 of 0.0100 mol / dm3 hydrochloric acid to neutralise 10.0 cm3 of
aqueous calcium hydroxide.
Calculate the concentration of the calcium hydroxide.
................................... mol/ dm3 [3]
© UCLES 2013
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For
Examiner’s
Use
15
(e) Describe how to obtain pure dry crystals of calcium chloride from an aqueous solution
of calcium chloride.
For
Examiner’s
Use
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
...................................................................................................................................... [2]
[Total: 10]
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.
University of 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 2013
5070/22/O/N/13
© UCLES 2013
20
Calcium
5070/22/O/N/13
Strontium
Actinium
†
Key
b
X
a
b = atomic (proton) number
X = atomic symbol
a = relative atomic mass
* 58–71 Lanthanoid series
† 90–103 Actinoid series
89
Radium
88
Francium
87
227
Ac
226
Ra
72
Hafnium
*
Lanthanum
57
178
Hf
40
Zirconium
Zr
91
Titanium
139
Yttrium
22
48
Ti
La
39
Y
89
Scandium
21
223
Barium
56
Caesium
45
Sc
Fr
55
137
Ba
133
Cs
38
Rubidium
37
88
Sr
85
Rb
19
Potassium
40
Ca
39
Magnesium
Sodium
12
24
Mg
23
Na
Beryllium
4
Lithium
K
11
3
9
Be
7
II
Li
I
93
Ta
181
Niobium
Nb
90
58
73
52
96
Mo
W
184
55
Tc
186
Re
144
Nd
92
60
Uranium
U
238
Neodymium
75
Rhenium
43
Technetium
25
Manganese
Mn
27
59
28
59
29
64
30
65
5
Ru
101
Iron
190
Pm
147
Osmium
Os
237
Np
93
Neptunium
61
Promethium
76
44
Ruthenium
26
56
Fe
150
Sm
244
Pu
94
Plutonium
62
Eu
152
Platinum
243
Am
95
Americium
63
Europium
78
Pt
Iridium
195
Ir
46
Palladium
Pd
106
Nickel
Ni
192
Samarium
77
45
Rhodium
Rh
103
Cobalt
Co
Gd
157
Gold
Au
197
Silver
96
64
Curium
Cm
247
Gadolinium
79
47
Ag
108
Copper
Cu
201
Bk
247
Terbium
Tb
159
Mercury
Hg
97
Berkelium
65
80
48
Cadmium
Cd
112
Zinc
Zn
11
6
Dy
162
Thallium
Tl
204
Indium
251
Cf
98
Californium
66
Es
252
Holmium
Ho
165
Lead
Pb
207
Tin
99
Einsteinium
67
82
50
119
Sn
115
32
Germanium
Ge
73
Silicon
In
Gallium
Dysprosium
81
49
31
70
Ga
14
28
Si
Carbon
27
Aluminium
13
12
C
Al
Boron
B
7
14
75
Sb
122
Arsenic
As
Bi
209
Fermium
Fm
257
Erbium
Er
167
Bismuth
100
68
83
51
Antimony
33
15
Phosphorus
P
31
Nitrogen
N
8
Se
79
Sulfur
S
32
Oxygen
209
Po
169
Md
258
Thulium
Tm
101
Mendelevium
69
84
Polonium
52
Tellurium
Te
128
Selenium
34
16
16
O
9
Yb
173
Astatine
At
210
Iodine
I
127
Bromine
Br
80
Chlorine
259
No
102
Nobelium
70
Ytterbium
85
53
35
17
Cl
35.5
Fluorine
F
19
Lr
260
Lutetium
Lu
175
Radon
Rn
222
Xenon
Xe
131
Krypton
Kr
84
Argon
Ar
40
Neon
103
Lawrencium
71
86
54
36
18
10
Ne
20
Helium
2
0
Hydrogen
VII
4
VI
He
V
1
IV
H
III
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
91
Protactinium
Thorium
231
Pa
Th
232
Praseodymium
Cerium
59
141
Pr
140
74
Tungsten
42
Molybdenum
24
Chromium
Cr
Ce
Tantalum
41
23
Vanadium
V
51
1
Group
DATA SHEET
The Periodic Table of the Elements
16