1.
When copper carbonate reacts with
excess acid, carbon dioxide is produced.
The curves shown were obtained under
different conditions.
The change from P to Q could be
brought about by
A.
increasing the concentration of
the acid
B.
increasing the mass of copper
carbonate
C.
Adding a catalyst
D.
Decreasing the particle size of the
copper carbonate
2.
When 3.6g of butanal (relative formula
mass = 72) was burned, 134kJ of energy
was released. From this result, what is the
enthalpy of combustion, in kJ mol-1?
A.
-6.7
B.
+6.7
C.
–2680
D.
+2680
3.
Which of the following chlorides is likely
to have the most ionic character?
A.
LiCl
B.
CsCl
C.
BeCl2
D.
CaCl2
4.
Which equation represents the first
ionisation energy of a diatomic element,
X2?
A.
½ X2(s)
X+(g)
B.
½ X2(g)
X-(g)
C.
X(g)
X+(g)
D.
X(s)
X-(g)
5.
Which of the following elements exists as
discrete molecules?
A.
boron
B.
carbon (diamond)
C.
silicon
D.
sulphur
1
6.
Which of the following chlorides is most
likely to be soluble in tetrachloromethane,
CCl4?
A.
barium chloride
B.
caesium chloride
C.
calcium chloride
D.
phosphorus chloride
7.
In which of the following liquids does
hydrogen bonding occur?
A.
ethanoic acid
B.
ethyl ethanoate
C.
hexane
D.
hex-1-ene
8.
A compound boils at –33oC. It also
dissolves in water to give an alkaline
solution. Which type of bonding is present
within the compound?
A.
metallic
B.
covalent (polar)
C.
ionic
D.
covalent (non-polar)
9.
The number of moles of ions in 1 mol of
copper(II)phosphate is
A.
1
B.
2
C.
4
D.
5
10.
The Avogadro Constant is the same as the
number of
A.
atoms in 24 g of carbon
B.
molecules in 16g of oxygen
C.
molecules in 2g of hydrogen
D.
ions in 1 litre of sodium chloride
solution, concentration 1 moll-1.
11.
What volume of oxygen, in litres, is
required for the complete combustion of
1 litre of butane gas? (All volumes are
measured under the same conditions of
temperature and pressure)
A.
1
B.
4
C.
6.5
D.
13
12.
Which of the following is the correct
interpretation of the above energy distribution
diagram for a reaction as the temperature
decreases from T2 to T1?
Activation
Number of
Energy (EA)
successful
collisions
A Remains the
Increases
same
B Decreases
Decreases
C Decreases
Increases
D Remains the
Decreases
same
13.
A metal (melting point 843oC, density
1.54 gcm3) was obtained by electrolysis of
its chloride (melting point 772oC, density
2.15 gcm3). During the electrolysis the
metal would occur as
A.
a solid on the surface of the
electrolyte
B.
a liquid on the surface of the
electrolyte
C.
a solid at the bottom of the
electrolyte
D.
a liquid at the bottom of the
electrolyte.
16.
Which of the following contains the
largest number of molecules?
A.
0.10g of hydrogen gas
B.
0.17g of ammonia gas
C.
0.32g of methane gas
D.
0.35g of chlorine gas
17.
The equation for the complete combustion
of propane is:
C3H8 + 5O2
3CO2 + 4 H2O
50cm3 of propane is mixed with 500cm3
of oxygen and the mixture is ignited.
What is the volume of the resulting gas
mixture? (All volumes measured at the
same temperature and pressure).
A.
150cm3
B.
300cm3
C.
400cm3
D.
700cm3
18.
It is now known that protons and neutrons
are made up of smaller particles called
quarks. Each proton and each neutron
contains 3 quarks. What is the
approximate number of quarks in 1g of
carbon-12?
A.
6 x 1023
B.
9 x 1023
C.
1.8 x 1024
D.
2.16 x 1025
The potential energy diagram for the
reaction
CO(g) + NO2(g) -> CO2(g) + NO(g)
is shown.
H, in kJmol-1, for the forward reaction is
A.
-361
B.
–227
C.
–93
D.
+361
14.
15.
Which type of bond is broken when ice is
melted?
A.
ionic
B.
polar covalent
C.
hydrogen
D.
non-polar covalent
2
19.
Excess marble chips (calcium carbonate)
were added to 25cm3 of hydrochloric acid,
concentration 2 moll-1. Which
measurement, taken at regular intervals
and plotted against time, would give the
graph shown below?
A.
B.
C.
D.
20.
21.
The enthalpy of neutralisation in an
acid/alkali reaction is always the energy
released in
A.
the neutralisation of one mole of
acid
B.
the neutralisation of one mole of
alkali
C.
the formation of one mole of water
D.
the formation of one mole of salt
22.
Which entry in the table shows the trends
in the electronegativity values of the
elements in the Periodic Table?
A
B
C
D
temperature
volume of gas produced
pH of solution
mass of the beaker and contents
3
Down a group
Decrease
Increase
Decrease
Increase
23.
Which type of structure is found in a
fullerene?
A.
ionic lattice
B.
metallic lattice
C.
covalent network
D.
covalent molecular
24.
Which type of bonding can be described
as intermolecular?
A.
covalent bonding
B.
hydrogen bonding
C.
ionic bonding
D.
metallic bonding
25.
An element melts at about room
temperature and forms an oxide which
reacts with water to form a solution with a
pH less than 7. Which statement is most
likely to be true?
A.
the element conducts electricity
B.
the oxide contains covalent bonds
C.
the oxide has a high melting point
D.
the element has a covalent network
structure
26.
Which gas occupies the largest volume?
(Assume all measurements are made at
the same temperature and pressure.)
A.
0.32g of oxygen
B.
0.44g of carbon dioxide
C.
0.20g of hydrogen
D.
0.80g of argon
The following potential energy diagram is
for an uncatalysed reaction.
When a catalyst is used the activation
energy of the forward reaction is reduced
to 35 kJmol-1. What is the activation
energy of the catalysed reverse reaction,
in kJmol-1?
A.
35
B.
65
C.
125
D.
155
Across a period
Decrease
Decrease
Increase
Increase
27.
How many atoms will be present in 11.2
litres of gaseous fluorine (molar volume
22.4 litres mol-1)
A.
1.505 x 1023
B.
3.01 x 1023
C.
6.02 x 1023
D.
1.204 x 1024
28.
The difference between the atomic size of
sodium and chlorine is mainly due to the
difference in the
A.
number of electrons
B.
number of protons
C.
number of neutrons
D.
mass of each atom
29.
In which molecule willl the chlorine atom
carry a partial charge (+)?
A.
Cl – Br
B.
Cl – Cl
C.
Cl – F
D.
Cl – I
30.
Which statement may correctly be applied
to silicon dioxide?
A.
it consists of discrete molecules
B.
it has a covalent network structure
C.
it is similar in structure to carbon
dioxide
D.
Van der Waals’ forces are
important to its structure
31.
32.
A new form of carbon has been
discovered. It consists of a footballshaped molecule consisting of 60 carbon
atoms. Approximately how many such
molecules are present in 12g of this type
of carbon?
A.
1.0 x 1022
B.
1.2 x 1023
C.
6.0 x 1023
D.
3.6 x 1025
33.
Which of the following shows the types of
bonding in decreasing order of strength?
A.
covalent, hydrogen, Van der
Waals’
B.
covalent, Van der Waals’,
hydrogen
C.
hydrogen, Van der Waals’,
covalent
D.
Van der Waals’ hydrogen,
covalent
34.
Silicon carbide can be used as
A.
a lubricant
B.
a tip for cutting/grinding tools
C.
a substitute for pencil “lead”
D.
an electrical conductor
35.
For any chemical, the temperature is a
measure of
A.
the average kinetic energy of the
particles which react
B.
the average kinetic energy of all
the particles
C.
the activation energy
D.
the minimum kinetic energy
required before a reaction occurs
36.
Which element is a solid at room
temperature and consists of discrete
molecules?
A.
carbon
B.
silicon
C.
sulphur
D.
boron
The same reaction was carried out at four
different temperatures. The table shows
the times taken for the reaction to occur.
Temperature /oC
Time / s
20
60
30
30
40
14
50
5
The results show that
A.
a small rise in temperature results
in a large increase in reaction rate
B.
the activation energy increases
with increasing temperature
C.
the rate of the reaction is directly
proportional to the temperature
D.
the reaction is endothermic
4
37.
Which element would require the most
energy to convert one mole of gaseous
atoms into one mole of gaseous ions
carrying two positive changes? (You may
wish to use the data booklet)
A.
scandium
B.
titanium
C.
vanadium
D.
chromium
41.
In which of the substances, in the solid
state, would van der Waals’ attractions be
a significant “intermolecular force”?
A.
sodium chloride
B.
carbon dioxide
C.
magnesium
D.
ice
42.
Tetrachloromethane, CCl4, is considered
to be a non-polar substance because
A.
the C-Cl bonds are non-polar
B.
the polar bonds are arranged
symmetrically
C.
a covalent network structure exists
D.
only linear molecules are polar
43.
The melting points of the Group 7
elements increases on descending the
group because the
A.
covalent bond lengths increase
B.
the size of the nucleus increases
C.
the van der Waals’ forces increase
D.
the nuclear charge increases
44.
Ethanol (C2H5OH) has a different
enthalpy of combustion from diethyl ether
(CH3OCH3) because the compounds have
different
A.
molecular masses
B.
bonds within the molecules
C.
products of combustion
D.
boiling points
45.
Which of the following represents an
exothermic change?
A.
O2(g)
2O(g)
B.
CH4(g)
C(g) + 4H(g)
C.
2N(g)
N2(g)
D.
H2O(g)
2H(g) + O(g)
38.
In area X
A.
molecules always form an
activated complex
B.
no molecules have the energy to
form an activated complex
C.
collisions between molecules are
always successful in forming
products
D.
all molecules have the energy to
form an activated complex
39.
Potassium nitrate decomposes on heating
to give potassium nitrite and oxygen.
KNO3(s)
KNO2(s) + ½ O2(g)
What volume of oxygen would be
obtained by the decomposition of 0.05
mol of potassium nitrate in such a
reaction? (The molar volume of oxygen
under these conditions is 24 litres mol-1)
A.
0.3 litres
B.
0.6 litres
C.
0.9 litres
D.
1.2 litres
40.
The mass of 1 mol of sodium is 23g. What
is the approximate mass of 1 sodium
atom?
A.
6.0 x 1023 g
B.
6.0 x 10-23g
C.
3.8 x 10-23 g
D.
3.8 x 10-24 g
5
46.
Excess zinc was added to 100cm3 of
hydrochloric acid, concentration 1 moll-1
Graph I refers to this reaction.
48.
Graph II could be for
A.
excess zinc reacting with 100cm3
of hydrochloric acid, concentration
2 moll-1
B.
excess zinc reacting with 100cm3
of sulphuric acid, concentration
1 moll-1
C.
excess zinc reacting with 100cm3
of ethanoic acid, concentration 1
moll-1
D.
excess magnesium reacting with
100cm3 of hydrochloric acid,
concentration 1 moll-1
The potential energy diagram below refers
to the reversible reaction involving
reactants R and products P.
What is the enthalpy change, in kJmol-1,
for the reverse reaction P
R?
A.
+30
B.
+10
C.
–10
D.
–40
47.
The enthalpy change for the forward
reaction can be represented by
A.
x
B.
y
C.
x+y
D.
x–y
6
49.
When copper carbonate reacts with excess
acid, carbon dioxide is produced. The
curves shown were obtained under
different conditions.
The change P to Q could be brought about
by
A.
increasing the concentration of the
acid
B.
decreasing the mass of copper
carbonate
C.
decreasing the particle size of the
copper carbonate
D.
adding a catalyst
50.
The above diagram could represent
A.
the fermentation of glucose
B.
neutralisation of an acid by an
alkali
C.
the combustion of sucrose
D.
the reaction of a metal with acid
7
Multiple Choice Past Paper
Questions
Unit 1
Answers
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
B
C
B
C
D
D
A
B
D
C
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
C
D
A
C
A
A
C
C
D
B
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
C
C
D
B
B
C
C
B
C
B
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
A
A
A
B
B
C
D
D
B
C
41.
42.
43.
44.
45.
46.
47.
48.
49.
50.
8
B
B
C
B
C
D
B
C
B
A