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Question
Mark
1
AQA Level 1/2 Certificate
June 2015
2
3
Chemistry
8402/2
4
5
Paper 2
6
Tuesday 9 June 2015
1.30 pm to 3.00 pm
TOTAL
For this paper you must have:
 a ruler
 a calculator
 the periodic table (enclosed).
Time allowed
 1 hour 30 minutes
A
Instructions
 Use black ink or black ball-point pen.
 Fill in the boxes at the top of this page.
 Answer all questions.
 You must answer the questions in the spaces provided. Do not write
outside the box around each page or on blank pages.
 Do all rough work in this book. Cross through any work you do not want
to be marked.
Information
 The marks for questions are shown in brackets.
 The maximum mark for this paper is 90.
 You are expected to use a calculator where appropriate.
 You are reminded of the need for good English and clear presentation in
your answers.
 Question 5(c) should be answered in continuous prose.
In this question you will be marked on your ability to:
– use good English
– organise information clearly
– use specialist vocabulary where appropriate.
Advice
 In all calculations, show clearly how you work out your answer.
(Jun158402201)
G/KL/106784/Jun15/E4
8402/2
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Answer all questions in the spaces provided.
1
This question is about atoms.
Atoms contain electrons, neutrons and protons.
1 (a) (i)
Which of these particles has a positive charge?
Tick () one box.
[1 mark]
Electron
Neutron
Proton
1 (a) (ii) Which of these particles does not have an electrical charge?
Tick () one box.
[1 mark]
Electron
Neutron
Proton
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1 (b)
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How are the elements in the periodic table arranged?
Tick () one box.
[1 mark]
In order of increasing atomic number
In order of increasing mass number
In order of increasing reactivity
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1 (c)
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Figure 1 shows the arrangement of the electrons in an atom of fluorine.
Figure 1
1 (c) (i)
How many protons are in an atom of fluorine?
Tick () one box.
[1 mark]
2
7
9
1 (c) (ii) The boiling point of fluorine is –188 °C.
What is the state of fluorine at room temperature?
Tick () one box.
[1 mark]
Solid
Liquid
Gas
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1 (d)
Fluorine reacts with copper to form an ionic compound.
1 (d) (i)
Explain, in terms of electrons and electronic structure, what happens to a fluorine atom
when it reacts with copper.
Use Figure 1 to help you to answer this question.
[2 marks]
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1 (d) (ii) Describe a chemical test which would show that a solution contains copper(II) ions.
[2 marks]
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2
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A student investigated the viscosity of liquid hydrocarbons.
A viscous liquid is a liquid that flows slowly.
The student used this method.

Measure 50 cm3 of the liquid hydrocarbon.

Pour the liquid hydrocarbon into the funnel, as shown in Figure 2.
Figure 2
Funnel
Liquid hydrocarbon
A
2 (a) (i)

Time how long it takes for all of the liquid hydrocarbon to run out of the funnel.

Repeat the experiment for other liquid hydrocarbons.
Give the name of apparatus A in Figure 2.
[1 mark]
............................................................................................................................................
2 (a) (ii) Name the apparatus that could be used to measure 50 cm3 of liquid hydrocarbon.
[1 mark]
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2 (b)
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The student’s results for six liquid hydrocarbons are shown in Table 1.
Table 1
Formula
of liquid
hydrocarbon
Time for liquid hydrocarbon to run out of the
funnel in seconds
Mean time in
seconds
Experiment 1
Experiment 2
Experiment 3
C5H12
12
11
13
12
C6H14
14
15
15
15
C7H16
19
20
18
C8H18
27
26
28
27
C10H22
46
48
24
47
C12H26
65
67
69
67
2 (b) (i)
The student did the experiment three times with each liquid hydrocarbon.
Give two reasons why.
[2 marks]
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2 (b) (ii) Use the data in Table 1 to calculate the mean time, in seconds, for C7H16
[1 mark]
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Mean time = ................................... seconds
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2 (b) (iii) Complete the sentence.
[1 mark]
As the number of carbon atoms in a molecule of liquid hydrocarbon increases, the time
taken for the liquid hydrocarbon to run out of the funnel ................................................ .
2 (b) (iv) A ring has been drawn around one result in Table 1.
This result has not been used to calculate the mean time for C10H22
Suggest why this result was not used.
[1 mark]
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2 (b) (v) Suggest one error the student may have made to get the ringed result.
[1 mark]
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2 (c)
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The student investigated the effect of temperature on the viscosity of one of the liquid
hydrocarbons.
The liquid hydrocarbon he was using had the hazard symbols shown in Figure 3.
Figure 3
2 (c) (i)
Suggest why the student warmed the liquid hydrocarbon using warm water and
not a Bunsen flame.
[1 mark]
............................................................................................................................................
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2 (c) (ii) The student wore safety glasses.
Give one other safety precaution the student should take, and give a reason for this
safety precaution.
[2 marks]
Safety precaution ...............................................................................................................
Reason ..............................................................................................................................
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2 (d)
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This is the method the student used to investigate the effect of temperature on the
viscosity of one of the liquid hydrocarbons.

Measure 50 cm3 of the liquid hydrocarbon and pour it into a beaker.

Stand the beaker of liquid hydrocarbon in a heated water bath.

Leave for a few minutes.

Measure the temperature of the liquid hydrocarbon.

Pour the liquid hydrocarbon into the funnel, as shown in Figure 4.
Figure 4
Funnel
Liquid hydrocarbon

Time how long it takes for all of the liquid hydrocarbon to run out of the funnel.

Repeat the experiment at different temperatures.
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2 (d) (i)
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The student’s results are shown in Table 2.
Table 2
Temperature of liquid
hydrocarbon in °C
Time to run out of the
funnel in seconds
23
27
30
21
37
17
46
16
55
11
65
9
Plot the results shown in Table 2 on the graph in Figure 5.
Draw a curve of best fit.
[3 marks]
Figure 5
30
25
Time to
20
run out of
the funnel 15
in seconds
10
5
20
25
30 35 40 45 50 55 60 65
Temperature of liquid hydrocarbon in °C
70
2 (d) (ii) One of the points is anomalous.
Draw a ring around the anomalous point on your graph.
[1 mark]
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2 (d) (iii) Predict how long it will take the liquid hydrocarbon to run through the funnel at 70 °C.
Show your working on your graph.
[2 marks]
Time = ........................................ seconds
2 (d) (iv) Describe the relationship between the temperature of the liquid hydrocarbon and the
viscosity of the liquid hydrocarbon.
[3 marks]
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2 (d) (v) The apparatus the student used in Figure 4 could lead to a systematic error in the
results.
Identify one source of systematic error, and describe how the student could avoid or
reduce the error.
[2 marks]
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3
Insoluble salts can be made by mixing solutions of two soluble salts.
3 (a)
A student mixed sodium carbonate solution and copper sulfate solution.
This produced a precipitate of copper carbonate and a solution of sodium sulfate.
3 (a) (i)
Write the correct state symbols from the box in the spaces in the chemical equation.
[2 marks]
aq
Na2CO3(aq) + CuSO4(aq)
g
l
s
CuCO3 (..........) + Na2SO4 (..........)
3 (a) (ii) What process could the student use to separate the precipitate of copper carbonate
from the mixture?
Tick () one box.
[1 mark]
Chromatography
Distillation
Filtration
3 (a) (iii) The student washed the copper carbonate he obtained with water.
Name one substance removed from the copper carbonate by washing it with water.
[1 mark]
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3 (b)
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A student mixed some salt solutions.
His observations are shown in Table 3.
Table 3
Mixture
Salt solution 1
Salt solution 2
Observations
A
Sodium carbonate
Cobalt sulfate
Pink precipitate
Colourless solution
B
Copper sulfate
Lead nitrate
White precipitate
Blue solution
C
Sodium sulfate
Manganese nitrate
No precipitate
Very pale pink solution
3 (b) (i)

All sodium salts are soluble.

All nitrate salts are soluble.
Name the insoluble salt made in mixture B.
[1 mark]
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3 (b) (ii) Name one soluble salt made by the student.
[1 mark]
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3 (b) (iii) What colour is cobalt carbonate?
[1 mark]
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3 (c)
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Barium sulfate is an insoluble salt.
Barium sulfate can be made by adding barium hydroxide solution to dilute sulfuric acid.
The balanced chemical equation for the reaction is:
H2SO4(aq) + Ba(OH)2(aq)
BaSO4(s) + 2 H2O(l)
A student investigated how the electrical conductivity of dilute sulfuric acid changed as
barium hydroxide solution was added.
This is the method she used.
Step
Step
Step
Step
1
2
3
4
Step 5
Place 25.0 cm3 of dilute sulfuric acid in a conical flask.
Add 5.0 cm3 of barium hydroxide solution.
Stir the mixture.
Use a conductivity meter to measure the electrical conductivity of the
mixture.
Repeat Step 2, Step 3 and Step 4 until 50 cm3 of barium hydroxide solution
have been added.
The student’s results are shown on the graph in Figure 6.
Figure 6
700
600
500
Relative
electrical
conductivity
400
300
200
100
0
0
10
20
30
40
50
Volume of barium hydroxide solution added in cm3
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3 (c) (i)
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The ringed point on the graph is anomalous.
What could have happened to cause the anomalous point?
Tick () one box.
[1 mark]
No more barium hydroxide solution was added.
Too much barium hydroxide solution was added.
Too much dilute sulfuric acid was used.
3 (c) (ii) Use the graph in Figure 6 to estimate the relative electrical conductivity of the dilute
sulfuric acid before any barium hydroxide solution was added.
Show your working on the graph.
[2 marks]
Relative electrical conductivity = ........................................
3 (c) (iii) Explain why dilute sulfuric acid conducts electricity.
[2 marks]
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3 (d)
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Figure 6 has been reprinted here to help you to answer the questions.
700
600
500
Relative
electrical
conductivity
400
300
200
100
0
0
10
20
30
40
50
Volume of barium hydroxide solution added in cm3
3 (d) (i)
What was the volume of barium hydroxide solution added when the relative electrical
conductivity of the mixture was zero?
[1 mark]
Volume of barium hydroxide solution = .................... cm3
3 (d) (ii) Suggest why the relative electrical conductivity became zero.
[1 mark]
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3 (e)
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The student did another experiment using the same solutions as she used before.
She used the same volume (25.0 cm3) of dilute sulfuric acid in the conical flask.
She then added an unknown volume of barium hydroxide solution.
She found that the relative electrical conductivity of the mixture was 260.
This is the student’s conclusion:
13 cm3 of barium hydroxide solution must have been added.
3 (e) (i)
Why may the student’s conclusion not be correct?
[1 mark]
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3 (e) (ii) The student said that she could check whether she was correct by adding something to
the mixture.
What could she add to the mixture? How would this tell her whether she was correct?
[3 marks]
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4
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box
Dilute nitric acid reacts with potassium hydroxide solution.
The equation for the reaction is:
HNO3 + KOH
KNO3 + H2O
A student investigated the temperature change in this reaction.
This is the method the student used.
Step 1
Step 2
Step 3
Step 4
Step 5
Put 25 cm3 of dilute nitric acid in a polystyrene cup.
Use a thermometer to measure the temperature of the dilute nitric acid.
Use a burette to add 4 cm3 of potassium hydroxide solution to the
dilute nitric acid and stir the mixture.
Use a thermometer to measure the highest temperature of the mixture.
Repeat steps 3 and 4 until 40 cm3 of potassium hydroxide solution have
been added.
The dilute nitric acid and the potassium hydroxide solution were both at room
temperature.
4 (a)
Figure 7 shows part of the thermometer after some potassium hydroxide solution had
been added to the dilute nitric acid.
Figure 7
°C
35
30
25
20
15
What is the temperature shown on the thermometer?
[1 mark]
The temperature shown is .................... °C
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4 (b)
Errors are possible in this experiment.
4 (b) (i)
Suggest two causes of random error in the experiment.
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[2 marks]
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4 (b) (ii) Another student used a glass beaker instead of a polystyrene cup.
This caused a systematic error.
Why does using a glass beaker instead of a polystyrene cup cause a systematic error?
[1 mark]
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4 (c)
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The results of the student using the polystyrene cup are shown in Figure 8.
Figure 8
34
32
30
Temperature
28
in °C
26
24
22
4 (c) (i)
0
5
10 15 20 25 30 35 40
Volume of potassium hydroxide added in cm3
How do the results in Figure 8 show that the reaction between dilute nitric acid and
potassium hydroxide solution is exothermic?
[1 mark]
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4 (c) (ii) Explain why the temperature readings decrease between 28 cm3 and 40 cm3 of
potassium hydroxide solution added.
[2 marks]
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4 (c) (iii) It is difficult to use the data in Figure 8 to find the exact volume of potassium hydroxide
solution that would give the maximum temperature.
Suggest further experimental work that the student should do to make it easier to
find the exact volume of potassium hydroxide solution that would give the maximum
temperature.
[2 marks]
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4 (d)
The student did further experimental work and found that 31.0 cm3 of potassium
hydroxide solution neutralised 25.0 cm3 of dilute nitric acid.
The concentration of the dilute nitric acid was 2.0 moles per dm3.
HNO3 + KOH
KNO3 + H2O
Calculate the concentration of the potassium hydroxide solution in moles per dm3.
[3 marks]
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Concentration = ............................ moles per dm3
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4 (e)
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The student repeated the original experiment using 25 cm3 of dilute nitric acid in
a polystyrene cup and potassium hydroxide solution that was twice the original
concentration.
She found that:


a smaller volume of potassium hydroxide solution was required to reach the
maximum temperature
the maximum temperature recorded was higher.
Explain why the maximum temperature recorded was higher.
[2 marks]
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5
This question is about ethanol.
5 (a)
Ethanol can be made by fermentation of sugars from plants.
5 (a) (i)
What is a suitable temperature for fermentation?
Draw a ring around the correct answer.
[1 mark]
0 °C
25 °C
450 °C
5 (a) (ii) Fermentation produces a dilute solution of ethanol in water.
Name the process used to obtain ethanol from this dilute solution.
[1 mark]
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5 (b)
Ethanol made by fermentation can be used as a biofuel.
5 (b) (i)
Explain why increasing the use of biofuels may cause food shortages.
[2 marks]
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5 (b) (ii) Explain why burning biofuels contributes less to climate change than burning fossil
fuels.
[2 marks]
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5 (c)
Do not write
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In this question you will be assessed on using good English, organising
information clearly and using specialist terms where appropriate.
Ethanol can also be made by reacting ethene with steam in the presence of a catalyst.
C2H4(g) + H2O(g)
C2H5OH(g)
Figure 9 shows how the percentage yield of ethanol changes as the pressure is
changed at three different temperatures.
Figure 9
100
300 °C
90
80
70
400 °C
60
Percentage
50
yield of
ethanol
40
500 °C
30
20
10
0
0
50
100
150
200
250
Pressure in atmospheres
300
Figure 10 shows how the rate of reaction changes as the temperature changes at three
different pressures.
Figure 10
7
80 atmospheres
6
5
Relative 4
rate of
reaction 3
2
40 atmospheres
1
0
100
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20 atmospheres
150
200
250
300
Temperature in °C
350
400
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In one process for the reaction of ethene with steam the conditions are:

300 °C

65 atmospheres

a catalyst.
Use the information in Figure 9 and Figure 10, and your own knowledge, to justify this
choice of conditions.
[6 marks]
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Extra space ........................................................................................................................
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6
Methane (CH4) is used as a fuel.
6 (a)
The displayed structure of methane is:
Do not write
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box
H
H
C
H
H
Draw a ring around a part of the displayed structure that represents a covalent bond.
[1 mark]
6 (b)
Why is methane a compound?
Tick () one box.
[1 mark]
Methane contains atoms of two elements, combined chemically.
Methane is not in the periodic table.
Methane is a mixture of two different elements.
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6 (c)
Methane burns in oxygen.
6 (c) (i)
Figure 11 shows the energy level diagram for the complete combustion of methane.
Draw and label arrows on the diagram to show:

the activation energy

the enthalpy change, ∆H.
[2 marks]
Figure 11
Energy
Methane and oxygen
Carbon dioxide and water
6 (c) (ii) Complete and balance the symbol equation for the complete combustion of methane.
[2 marks]
CH4
+ ..........
CO2
+
..........
6 (c) (iii) Explain why the incomplete combustion of methane is dangerous.
[2 marks]
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6 (c) (iv) Explain why, in terms of the energy involved in bond breaking and bond making, the
combustion of methane is exothermic.
[3 marks]
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6 (d)
Methane reacts with chlorine in the presence of sunlight.
The equation for this reaction is:
H
H
C
H
H
+
Cl
Cl
H
H
C
Cl
+
H
Cl
H
Some bond dissociation energies are given in Table 4.
Table 4
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Bond
Bond dissociation
energy
in kJ per mole
C―H
413
C―Cl
327
Cl―Cl
243
H―Cl
432
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6 (d) (i)
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Show that the enthalpy change, ∆H, for this reaction is –103 kJ per mole.
[3 marks]
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6 (d) (ii) Methane also reacts with bromine in the presence of sunlight.
H
H
C
H
H
+
Br
Br
H
H
C
Br +
H
Br
H
This reaction is less exothermic than the reaction between methane and chlorine.
The enthalpy change, ∆H, is –45 kJ per mole.
What is a possible reason for this?
Tick () one box.
[1 mark]
CH3Br has a lower boiling point than CH3Cl
The C―Br bond is weaker than the C―Cl bond.
The H―Cl bond is weaker than the H―Br bond.
Chlorine is more reactive than bromine.
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