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1
AQA Level 1/2 Certificate
June 2015
2
3
Chemistry
8402/1
4
5
Paper 1
6
Thursday 14 May 2015
9.00 am to 10.30 am
7
For this paper you must have:
 a ruler
 a calculator
 the periodic table (enclosed).
8
9
TOTAL
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 4(b)(ii) 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.
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Answer all questions in the spaces provided.
1
The structures of four substances, A, B, C and D, are represented in Figure 1.
Figure 1
A
B
C
1 (a)
Use the correct letter, A, B, C or D, to answer each question.
1 (a) (i)
Which substance is a gas?
D
[1 mark]
1 (a) (ii) Which substance is a liquid?
[1 mark]
1 (a) (iii) Which substance is an element?
[1 mark]
1 (a) (iv) Which substance is made of ions?
[1 mark]
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1 (b)
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Figure 2 shows the bonding in substance C.
Figure 2
O
1 (b) (i)
S
O
What is the formula of substance C?
Draw a ring around the correct answer.
[1 mark]
SO2
SO2
S2O
1 (b) (ii) Use the correct answer from the box to complete the sentence.
[1 mark]
delocalised
shared
transferred
When a sulfur atom and an oxygen atom bond to produce substance C,
electrons are .................................................................. .
1 (b) (iii) What is the type of bonding in substance C?
Draw a ring around the correct answer.
[1 mark]
covalent
ionic
metallic
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There are no questions printed on this page
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ANSWER IN THE SPACES PROVIDED
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5
2
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Five elements, V, W, X, Y and Z, are shown in the periodic table in Figure 3.
The letters are not the chemical symbols of the five elements.
Figure 3
V
Z
W
X
Y
Use the correct letter, V, W, X, Y or Z, to answer each question.
2 (a)
Which element is a transition metal?
[1 mark]
2 (b)
Which element is in Group 2?
[1 mark]
2 (c)
Which element is a noble gas?
[1 mark]
2 (d)
Which element has an atomic (proton) number of 4?
[1 mark]
2 (e)
Which element forms only 1+ ions?
[1 mark]
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3
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This question is about water.
River water needs to be treated before it is safe to drink.
3 (a)
Figure 4 shows two stages of the treatment of river water.
Figure 4
River water
3 (a) (i)
Stage 1
Stage 2
Solid
particles
removed
Water
sterilised
What is the name of the process used to remove solid particles in Stage 1?
Tick () one box.
[1 mark]
Crystallisation
Fermentation
Filtration
3 (a) (ii) What is added in Stage 2 to sterilise the water?
Tick () one box.
[1 mark]
Chlorine
Fluoride
Potassium
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3 (b)
Toxic substances in river water are removed by adding very small amounts of
iron oxide nanoparticles.
3 (b) (i)
How is the size of nanoparticles different from normal-sized particles?
[1 mark]
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3 (b) (ii) Nanoparticles are needed in only very small amounts.
Suggest why.
[1 mark]
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3 (c)
In certain areas of the UK, tap water contains aluminium ions.
What would you see when sodium hydroxide solution is added drop by drop to tap
water containing aluminium ions?
[2 marks]
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4
This question is about magnesium.
4 (a) (i)
The electronic structure of a magnesium atom is shown in Figure 5.
Figure 5
Nucleus
Use the correct answer from the box to complete each sentence.
[3 marks]
electrons
neutrons
protons
shells
The nucleus contains protons and .................................................................................. .
The particles with the smallest relative mass that move around the nucleus
are called ..................................................................................... .
Atoms of magnesium are neutral because they contain the same number of
electrons and ..................................................................................... .
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4 (a) (ii) A magnesium atom reacts to produce a magnesium ion.
Which diagram shows a magnesium ion?
Tick () one box.
[1 mark]
2+
4 (b)
+
Magnesium and dilute hydrochloric acid react to produce magnesium chloride solution
and hydrogen.
Mg(s) + 2 HCl(aq)
4 (b) (i)
2–
MgCl2(aq) + H2(g)
State two observations that could be made during the reaction.
[2 marks]
1 .........................................................................................................................................
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2 .........................................................................................................................................
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4 (b) (ii) In this question you will be assessed on using good English, organising
information clearly and using specialist terms where appropriate.
Describe a method for making pure crystals of magnesium chloride from magnesium
and dilute hydrochloric acid.
In your method you should name the apparatus you will use.
You do not need to mention safety.
[6 marks]
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5
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A student investigated the rate of reaction between sodium thiosulfate solution and
dilute hydrochloric acid, as shown in Figure 6.
Figure 6
Sodium thiosulfate solution
and dilute hydrochloric acid
White paper marked
with a cross
The reaction produced a precipitate, which made the mixture turn cloudy.
The student timed how long it took until she could no longer see the cross.
She calculated the rate of the reaction.
5 (a)
The equation for the reaction is:
Na2S2O3(aq) + 2 HCl(aq)
2 NaCl(aq) + S(s) + SO2(g) + H2O(l)
Name the product that made the mixture go cloudy.
[1 mark]
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5 (b)
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The student investigated the effect of changing the temperature of the
sodium thiosulfate solution on the rate of reaction.
She plotted her results on a graph, as shown in Figure 7.
Figure 7
140
120
100
Relative
rate of
reaction
80
60
40
20
0
20
30
40
50
60
Temperature in °C
70
80
Describe the trends shown in the student’s results.
[2 marks]
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5 (c)
The student then investigated the effect of changing the concentration of
sodium thiosulfate solution on the rate of the reaction.
5 (c) (i)
Suggest two variables the student would need to control to make sure that her results
were valid.
[2 marks]
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5 (c) (ii) From this investigation the student correctly concluded:
‘As the concentration of sodium thiosulfate solution doubles, the rate of reaction
doubles.’
Explain the student’s conclusion in terms of particles.
[3 marks]
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6
This question is about polymers.
6 (a)
The polymer polyvinyl chloride (PVC) is non-biodegradable.
Give one problem caused by non-biodegradable polymers.
[1 mark]
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6 (b)
Figure 8 shows a short section of a PVC molecule.
Figure 8
H
Cl
H
Cl
H
Cl
C
C
C
C
C
C
H
H
H
H
H
H
PVC is produced from a monomer that contains two carbon atoms.
Complete the structure of the monomer.
[2 marks]
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6 (c)
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Figure 9 represents a few short chains of PVC molecules.
Figure 9
Explain why PVC softens and melts when heated.
Use Figure 9 and your knowledge of structure and bonding to help you to answer the
question.
[3 marks]
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6 (d)
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Monomer A and monomer B react to form polymer C.
The displayed structures of monomer A, monomer B and a short section of polymer C
are shown in Figure 10. The functional group of each structure is shown in a box.
Figure 10
Monomer A
Monomer B
O
C
C
O
H
O
O
H
H
O
H
H
C
C
H
H
Polymer C
O
H
O
O
C
C
O
H
H
C
C
H
H
O
Complete Table 1 by writing the names of the functional groups for monomer A and
polymer C.
[2 marks]
Table 1
Name of functional group
Monomer A
Monomer B
Polymer C
...........................................................................
alcohol
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7
This question is about copper.
7 (a)
Copper can be extracted by smelting copper-rich ores in a furnace.
The equation for one of the reactions in the smelting process is:
Cu2S(s) + O2(g)
2 Cu(s) + SO2(g)
Explain why there would be an environmental problem if sulfur dioxide gas escaped into
the atmosphere.
[2 marks]
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7 (b)
The impure copper produced by smelting is purified by electrolysis, as shown in
Figure 11.
Figure 11
d.c. power supply
Negative electrode
(cathode)
pure copper
Positive electrode
(anode)
impure copper
Electrolyte
Copper atoms are oxidised at the positive electrode to Cu2+ ions, as shown in the
half equation.
Cu(s)
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Cu2+(aq) + 2e–
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7 (b) (i)
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How does the half equation show that copper atoms are oxidised?
[1 mark]
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7 (b) (ii) The Cu2+ ions are attracted to the negative electrode, where they are reduced to
produce copper atoms.
Write a balanced half equation for the reaction at the negative electrode.
[1 mark]
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7 (b) (iii) Suggest a suitable electrolyte for the electrolysis.
[1 mark]
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7 (c)
Copper metal is used in electrical appliances.
Describe the bonding in a metal, and explain why metals conduct electricity.
[4 marks]
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7 (d)
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Soil near copper mines is often contaminated with low percentages of copper
compounds.
Phytomining is a new way to extract copper compounds from soil.
Describe how copper compounds are extracted by phytomining.
[3 marks]
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7 (e)
A compound in a copper ore has the following percentage composition by mass:
55.6% copper, 16.4% iron, 28.0% sulfur.
Calculate the empirical formula of the compound.
Relative atomic masses (Ar): S = 32; Fe = 56; Cu = 63.5
You must show all of your working.
[4 marks]
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Empirical formula = ............................................................
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8
This question is about iron and aluminium.
8 (a)
Iron is extracted in a blast furnace. Figure 12 is a diagram of a blast furnace.
Figure 12
Coke (carbon)
Limestone (calcium carbonate)
Haematite (iron(III) oxide)
Waste gases
Hot air
8 (a) (i)
Hot air
Molten iron
Calcium carbonate decomposes at high temperatures.
Complete the word equation for the decomposition of calcium carbonate.
[2 marks]
calcium carbonate
............................................... + ...............................................
8 (a) (ii) Carbon burns to produce carbon dioxide.
The carbon dioxide produced reacts with more carbon to produce carbon monoxide.
Balance the equation.
[1 mark]
C(s)
+
CO2(g)
.......... CO(g)
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8 (a) (iii) Carbon monoxide reduces iron(III) oxide:
Fe2O3(s) + 3 CO(g)
2 Fe(s) + 3 CO2(g)
Calculate the maximum mass of iron that can be produced from 300 tonnes of
iron(III) oxide.
Relative atomic masses (Ar): O = 16; Fe = 56
[3 marks]
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Maximum mass = .............................. tonnes
8 (b)
Aluminium is extracted by electrolysis, as shown in Figure 13.
Figure 13
Positive
electrodes
(anodes)
Negative
electrode
(cathode)
Aluminium oxide
dissolved in
molten cryolite
Molten aluminium
8 (b) (i)
Why can aluminium not be extracted by heating aluminium oxide with carbon?
[1 mark]
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8 (b) (ii) Explain why aluminium forms at the negative electrode during electrolysis.
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8 (b) (iii) Explain how carbon dioxide forms at the positive electrodes during electrolysis.
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9
This question is about ethanol.
9 (a)
Ethanol is produced by the reaction of ethene and steam:
C2H4 + H2O
9 (a) (i)
C2H5OH
Figure 14 shows the energy level diagram for the reaction.
Figure 14
C2H4 + H2O
Energy
C2H5OH
How does the energy level diagram show that the reaction is exothermic?
[1 mark]
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9 (a) (ii) A catalyst is used for the reaction.
Explain how a catalyst increases the rate of the reaction.
[2 marks]
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9 (b)
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Figure 15 shows the displayed structure of ethanol.
Figure 15
H
H
H
C
C
H
H
O
H
Complete the dot and cross diagram in Figure 16 to show the bonding in ethanol.
Show the outer shell electrons only.
[2 marks]
Figure 16
H
H
H
C
C
H
H
O
H
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9 (c)
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A student burned some ethanol.
Figure 17 shows the apparatus the student used.
Figure 17
Thermometer
Glass beaker
50 g of water
Spirit burner
containing ethanol
9 (c) (i)
The student recorded the temperature of the water before and after heating.
His results are shown in Table 2.
Table 2
Temperature before heating
20.7 °C
Temperature after heating
35.1 °C
Calculate the energy used to heat the water.
Use the equation Q = m  c  ∆T
The specific heat capacity of water = 4.2 J/g/°C
[3 marks]
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Energy used = ........................................ J
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9 (c) (ii) Table 3 shows the mass of the spirit burner before the ethanol was burned and after
the ethanol was burned.
Table 3
Mass of spirit burner before ethanol was burned
72.80 g
Mass of spirit burner after ethanol was burned
72.10 g
Calculate the number of moles of ethanol (C2H5OH) that were burned.
Relative atomic masses (Ar): H = 1; C = 12; O = 16
[3 marks]
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Number of moles burned = ........................................
9 (c) (iii) Calculate the energy released in joules per mole.
You should assume that all the energy from the ethanol burning was used to heat the
water.
[1 mark]
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Energy = ........................................ J/mole
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9 (d)
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The names, structures and boiling points of ethanol and two other alcohols are shown
in Table 4.
Table 4
Name
Methanol
Structure
Ethanol
H
H
C
O
H
H
H
Boiling
point in °C
65
H
H
C
C
H
H
Propanol
O
H
78
H
H
H
H
C
C
C
H
H
H
O
H
97
Use your knowledge of structure and bonding to suggest why the boiling points
increase as the number of carbon atoms increases.
[3 marks]
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