***IMPORTANT***
Only attempt the questions listed on the next page
The National Parent Forum of Scotland National 5 Revision in a Nutshell
when looking at the past papers.
These are the questions that are relevant to National 5, all
other questions should be ignored.
Always check the question listed against the level of past
paper (Standard Grade or Int2) and the year of the paper
***IMPORTANT***
The National Parent Forum of Scotland National 5 Revision in a Nutshell
revision
Chemistry
3
UNITS
5
National
Chemical Changes and Structure
Nature’s Chemistry
Chemistry in Society
The Scottish Qualifications Authority National 5 Chemistry subject webpage can be found here.
The Revision in a Nutshell series is designed to complement learning and revision that you have undertaken in class. Please check
with your teachers that these resources are relevant to you. You can find the series at www.parentforumscotland.org
Specimen Paper and Past Papers
The SQA Specimen Paper and marking instructions for National 5 Chemistry can be found here.
After completing the SQA Specimen Question Paper (exam) or any past paper questions, ensure that you look at the marking
instructions as these often contain course content and they will help you to improve your exam technique. National 5 Question Papers
differ from past papers. Ensure that you familiarise yourself with the Specimen Paper: this is what your exam will look like.
Past Papers
Useful SQA past paper questions are listed and organised by topic with guidance here. For direct links to past papers, click on the year
(ie click on '2013') in the table below where you will find questions relevant to the different topics within National 5 Chemistry. Some
topics are new for National 5 and therefore do not have past questions; be sure to revise all of the topics. Marking instructions for past
papers can be accessed in the column 'Answers'. Other past paper questions, which require some wording to be changed to make
them appropriate for National 5, can be found here.
Paper Name and Year
Unit/Paper Number & Title
Question Numbers
Answers
2013
N/A
10, 11a i, 14, 15c, 15d, 16b i, ii, 17a, 17b, 17c, 18b i,
(18b ii Chemical analysis questions related to
Unit 1)
Marking instructions
2012
N/A
12b, 12c, 13a, 13b i, 15a, 15b, 15c, 15d, 16, 17a i, ii,
17b, 18, 19, 20a, 20b, 20c, 21c i, ii
Marking instructions
2011
N/A
12b i, ii, 13a, 14a, 16a, 16b ii, 17b, 18a, 18b, 18c,
19a, 19b i, ii, 20a i, 20b, 20c i, ii, 20d, 21, 22
Marking instructions
Section A
2, 8, 9, 10, 12, 15, 18, 20, 21, 22, 26, 27, 29
Section B
1b, 4, 6c, 8c, 9a, 9b i, 10b i, ii, 13a i, ii, 15b
Section A
4, 5, 7, 9, 16, 22
Section B
2a i, 2b, 5b i, ii, 7a, 7c, 11c, 13b i, ii, 15a i, ii
Section A
7, 8, 12, 13, 14, 22, 25
Section B
1, 2, 3a, 3d, 4a ii, 8a, 9c, 9d, 10a,
(11c ii and iii Chemical Analysis questions related
to Unit 2), 12a, 13, 14a, 14b, 14c, 15a, 15b
Standard Grade Credit
Intermediate 2
2013
2012
2011
Higher past papers overleaf
Marking instructions
Marking instructions
Marking instructions
The National Parent Forum of Scotland National 5 Revision in a Nutshell
Paper Name and Year
Unit/Paper Number & Title
Question Numbers
Answers
Section B
2b i, 4a, 4b i, 4c
Marking instructions
Section A
40
Section B
1b i, 12b, 12c i
Higher
2012
2011
Marking instructions
Useful Websites
BBC Bitesize
Schools
Braidhurst High School
Revision summaries
Carluke High School
National 5 tests and marking schemes
Others
Mrs Smith - Prezi
Unit 1: Chemical Changes and Structure
Milngavie Tutors
Links to a range of websites and a lovely period table for printing out or looking at
www.parentforumscotland.org
enquiries@parentforumscotland.org
parentforumscotland
parentforumscot
The National Parent Forum of Scotland is grateful for the support of the Scottish Government, the Scottish Qualifications Authority,
Education Scotland and the Association of Directors of Education in Scotland in the preparation of this series.
FOR OFFICIAL USE
C
KU
PS
Total
Marks
0500/31/01
NATIONAL
QUALIFICATIONS
2013
CHEMISTRY
WEDNESDAY, 1 MAY
10.50 AM – 12.20 PM
STANDARD GRADE
Credit Level
Fill in these boxes and read what is printed below.
Full name of centre
Town
Forename(s)
Surname
Date of birth
Day
Month
Year
Scottish candidate number
Number of seat
1 All questions should be attempted.
2 Necessary data will be found in the Data Booklet provided for Chemistry at Standard
Grade and Intermediate 2.
3 The questions may be answered in any order but all answers are to be written in this
answer book, and must be written clearly and legibly in ink.
4 Rough work, if any should be necessary, as well as the fair copy, is to be written in this
book.
Rough work should be scored through when the fair copy has been written.
5 Additional space for answers and rough work will be found at the end of the book.
6 The size of the space provided for an answer should not be taken as an indication of how
much to write. It is not necessary to use all the space.
7 Before leaving the examination room you must give this book to the Invigilator. If you do
not, you may lose all the marks for this paper.
SA 0500/31/01 6/23710
*0500/31/01*
©
PART 1
In Questions 1 to 8 of this part of the paper, an answer is given by circling the
appropriate letter (or letters) in the answer grid provided.
In some questions, two letters are required for full marks.
If more than the correct number of answers is given, marks will be deducted.
A total of 20 marks is available in this part of the paper.
SAMPLE QUESTION
A
D
CH4
CO
B
E
C
H2
C2H5OH
F
CO2
C
(a) Identify the hydrocarbon.
A
B
C
D
E
F
The one correct answer to part (a) is A. This should be circled.
(b) Identify the two elements.
A
B
C
D
E
F
As indicated in this question, there are two correct answers to part (b). These are B and F.
Both answers are circled.
If, after you have recorded your answer, you decide that you have made an error and wish
to make a change, you should cancel the original answer and circle the answer you now
consider to be correct. Thus, in part (a), if you want to change an answer A to an answer D,
your answer sheet would look like this:
A
B
C
D
E
F
If you want to change back to an answer which has already been scored out, you should
enter a tick (3) in the box of the answer of your choice, thus:
[0500/31/01]
3A
B
C
D
E
F
Page two
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WRITE
IN THIS
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Marks KU PS
1. The grid shows the names of some elements.
A
B
C
hydrogen
D
copper
oxygen
E
iron
F
magnesium
iodine
(a) Identify the element which melts at 1083 °C.
You may wish to use the data booklet to help you.
A
B
C
D
E
F
1
(b) Identify the element produced in a blast furnace.
A
B
C
D
E
F
1
(c) Identify the element which burns with a pop.
A
B
C
D
E
F
1
(3)
[Turn over
[0500/31/01]
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Marks KU PS
2. The grid shows some ions.
A
B
C
Al3+
D
Cl–
Li+
E
F
H+
Br–
OH–
(a) Identify the ion with the same electron arrangement as a helium atom.
You may wish to use the data booklet to help you.
A
B
C
D
E
F
1
(b) Identify the two ions which combine to form an insoluble compound.
You may wish to use the data booklet to help you.
A
B
C
D
E
F
1
(c) Identify the ion present in all alkaline solutions.
A
B
C
D
E
F
1
(3)
[0500/31/01]
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Marks KU PS
3. Electricity can be produced using electrochemical cells.
A
lead
voltmeter
V
zinc
potassium nitrate solution
voltmeter
D
lead
V
voltmeter
B
tin
potassium nitrate solution
V
gold
tin
potassium nitrate solution
voltmeter
E
V
gold
voltmeter
C
magnesium
potassium nitrate solution
V
tin
tin
potassium nitrate solution
voltmeter
F
V
iron
zinc
potassium nitrate solution
(a) Identify the arrangement which would not produce electricity.
A
B
C
D
E
F
1
(b) Identify the two cells which could be used to compare the reactivity of
gold and lead.
A
B
C
D
E
F
1
(2)
[Turn over
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4. The grid shows the names of some carbohydrates.
A
fructose
B
glucose
C
maltose
D
starch
E
sucrose
Marks KU PS
(a) Identify the condensation polymer.
A
B
C
D
E
1
(b) Identify the two disaccharides.
A
B
C
D
E
1
(c) Identify the two carbohydrates which cannot be hydrolysed.
A
B
C
D
E
1
(3)
[0500/31/01]
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5. A student made some statements about the effect of adding water to an
acidic solution.
A
The pH of the solution will stay the same.
B
The acidity of the solution will decrease.
C
The pH of the solution will fall.
D
The acidity of the solution will increase.
E
The solution will become less concentrated.
Marks KU PS
Identify the two correct statements.
A
B
C
D
E
(1)
[Turn over
[0500/31/01]
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Marks KU PS
6. The grid shows the structural formulae of some monomers.
A
B
C
CN
H
Cl
H
CH3
H
C
C
C
C
C
C
H
H
H
Cl
H
CH3
D
E
F
Cl
H
H
H
CH3
H
C
C
C
C
C
C
Cl
H
H
H
H
H
(a) Identify the monomer which would form poly(propene).
A
B
C
D
E
F
1
(b) Identify the monomer which reacts with hydrogen to form ethane.
A
B
C
D
E
F
A
B
C
D
E
F
1
(c) Identify the two isomers.
[0500/31/01]
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Marks KU PS
6. (continued)
(d) When two different monomers polymerise a copolymer is formed as
shown.
H
H
C
C
H
CH3
+
Cl
H
H
H
Cl
H
C
C
C
C
C
C
H
H
H
CH3
H
H
Identify the two monomers which would polymerise to give the
copolymer below.
CH 3
H
CN
H
C
C
C
C
H
CH3
H
H
A
B
C
D
E
F
1
(4)
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7. A student made some statements about particles found in atoms.
A
Relative mass is almost zero
B
Charge = 1+
C
Charge = 0
D
Found inside the nucleus
E
Relative mass = 1
Marks KU PS
Identify the two statements which apply to both a proton and a neutron.
A
B
C
D
E
[0500/31/01]
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8. Several conductivity experiments were carried out using the apparatus
below.
Marks KU PS
Low voltage
power supply
+
bulb
substance X
substance Y
Experiment
Substance X
Substance Y
A
glucose solution
sodium chloride solution
B
copper nitrate solution
solid potassium nitrate
C
molten tin
liquid mercury
D
potassium sulphate solution
liquid hexane
E
lithium chloride solution
molten nickel bromide
Identify the two experiments in which the bulb would light.
A
B
C
D
E
(2)
[Turn over for Part 2 on Page twelve
[0500/31/01]
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PART 2
Marks KU PS
A total of 40 marks is available in this part of the paper.
9. A student carried out an experiment to investigate the rusting of iron.
A
magnesium
ribbon
iron
nail
B
no blue
colour
copper
ribbon
blue
colour
gel containing
ferroxyl indicator
(a) Write the formula for the ion which turns ferroxyl indicator blue.
1
(b) Name the ion formed from water and oxygen, when they accept
electrons during rusting.
1
(c) Explain why magnesium prevents iron from rusting.
1
(d) Salt, which is spread on roads in winter, speeds up rusting.
Ethylene glycol is used instead of salt on the roadways of iron bridges
because it does not speed up rusting.
Suggest the type of bonding present in ethylene glycol.
1
(4)
[0500/31/01]
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10. The nuclide notation for an isotope of hydrogen is
Marks KU PS
1
1H.
(a) An isotope of copper has atomic number 29 and mass number 63.
(i) Write the nuclide notation for this isotope of copper.
1
(ii) How many neutrons are present in this isotope of copper?
1
(b) A sample of copper was found to contain equal amounts of two
isotopes. One has mass number 63 and the other has mass number 65.
What is the relative atomic mass of this sample of copper?
1
(3)
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11. The table shows information about some useful compounds.
(a)
Compound
Formula
Y
Na3PO4
ammonia
NH3
ammonium nitrate
NH4NO3
Marks KU PS
(i) Name compound Y.
1
(ii) Compound Y can be used as a fertiliser.
Why are fertilisers added to soil?
1
(b) Name the catalyst used in the industrial manufacture of ammonia.
1
(c) What is present in the root nodules of some plants which convert
nitrogen from the atmosphere into nitrogen compounds?
1
(4)
[0500/31/01]
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Marks KU PS
12. Crude oil can be separated into fractions.
(a) One of the fractions contains alkane molecules with chain lengths from
five to eight carbons.
Using information in the data booklet, state the boiling point range for
this fraction.
°C
to
°C
1
(b) The table gives information about some alkanes.
Name
Density g/cm3
pentane
0·626
hexane
0·659
heptane
0·684
octane
0·703
Predict the density of the alkane with nine carbon atoms.
g/cm3
1
(c) A student investigated the reaction of some fuels with oxygen.
The results are shown.
Fuel
Products
A
carbon dioxide
B
water
C
nitrogen, water
D
carbon dioxide, water
(i) Name the elements which must be present in fuel D.
1
(ii) Suggest a name for fuel B.
1
(4)
[0500/31/01]
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13. Dilute hydrochloric acid reacts with sodium thiosulphate, Na2S2O3, as
shown in the equation below.
2HCl(aq) + Na2S2O3(aq)
Marks KU PS
2NaCl(aq) + S(s) + SO2(g) + H2O()
(a) Suggest a name for the type of chemical reaction taking place.
1
(b) A student investigated the effect of temperature on the rate of the
reaction.
The student measured the time taken for enough sulphur to form to
make the cross disappear.
hydrochloric acid
cross marked on
sheet of paper
cloudy
sodium
thiosulphate
solution
at the start
later
cross visible
cross not visible
The results are shown.
Temperature/°C
Time/s
25
89
30
64
35
44
40
33
45
27
Write a general statement describing the effect of temperature on the
rate of the reaction.
1
(2)
[0500/31/01]
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Marks KU PS
14. Zinc displaces copper from copper(II) sulphate solution.
The equation for the reaction is:
Zn(s) + Cu2+(aq) + SO42–(aq)
Zn2+(aq) + SO42–(aq) + Cu(s)
1
(a) Circle the spectator ion in the above equation.
(b) Write the ion-electron equation for the oxidation step in this reaction.
You may wish to use the data booklet to help you.
1
(c) The reaction can also be carried out in a cell.
e
A
e
ion bridge
copper(II) sulphate
solution
(i) Complete the three labels on the diagram.
(An additional diagram, if required, can be found on page 24.)
1
(ii) What is the purpose of the ion bridge?
1
(4)
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15. An antibacterial hand gel contains two alkanols, ethanol and propan-2-ol.
H
H
H
C
C
H
H
O
H
H
H
H
H
C
C
C
H
O
H
Marks KU PS
H
H
ethanol
propan-2-ol
(a) Alkanols are a homologous series containing carbon, hydrogen and
oxygen.
Suggest a general formula for alkanols.
1
(b) Ethanol can be produced by the fermentation of glucose.
(i) Name the gas produced during the fermentation of glucose.
1
(ii) Name the process used to increase the ethanol concentration of
fermentation products.
1
[0500/31/01]
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15. (continued)
(c) When alkanols are oxidised alkanoic acids are produced.
H
H
H
C
C
H
H
O
H
H
H
O
C
C
O
H
H
ethanol
ethanoic acid
Draw the full structural formula for the alkanoic acid produced when
butanol is oxidised.
H
H
H
H
H
C
C
C
C
H
H
H
H
O
H
butanol
butanoic acid
1
(d) Esters are produced when alkanols react with alkanoic acids.
The table gives information on esters.
Alkanol
Alkanoic acid
Ester
methanol
ethanoic acid
methyl ethanoate
ethanol
propanoic acid
ethyl propanoate
propanol
methanoic acid
propyl methanoate
butanol
ethanoic acid
butyl ethanoate
pentanol
butanoic acid
X
Suggest a name for X.
1
(5)
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Marks KU PS
16. Metals can be extracted from their ores by different methods.
(a) Place the following methods in the correct space in the table.
You may wish to use the data booklet to help you.
reacting with carbon
electrolysis
heat alone
Metal
Method
mercury
iron
magnesium
1
(b) Mercury can be extracted from the ore cinnabar, HgS.
(i) Calculate the percentage by mass of mercury in cinnabar.
%
2
(ii) Write the formula for the mercury ion in cinnabar.
1
(4)
[0500/31/01]
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Marks KU PS
17. Nitrogen trifluoride, NF3, is used in the manufacture of plasma screens.
(a) Draw a diagram showing all outer electrons to represent a molecule of
nitrogen trifluoride.
1
(b) The atoms in nitrogen trifluoride are held together by covalent bonds.
Circle the correct words to complete the sentence.
nuclei are held together
{
protons
by their common attraction for a shared pair of neutrons
electrons
{
{
positive
negative
neutral
{
A covalent bond forms when two
.
1
(c) The equation for the formation of nitrogen trifluoride, NF3 , is:
N2 + 3F2
2NF3
Calculate the mass of nitrogen trifluoride produced from 7 g of nitrogen.
Show your working clearly.
g
2
(4)
[Turn over for Question 18 on Page twenty-two
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18. A student investigated the reaction between dilute sulphuric acid and
sodium carbonate.
Marks KU PS
(a) One experiment involved measuring the volume of carbon dioxide
produced when solid sodium carbonate was used.
Time/s
0
10
30
40
50
60
70
Volume of
carbon dioxide/cm3
0
12
29
34
36
37
37
(i) Draw a line graph of these results.
Use appropriate scales to fill most of the graph paper.
(Additional graph paper, if required, will be found on page 24.)
2
(ii) The experiment was repeated at a higher temperature.
The volume and concentration of sulphuric acid and the mass of
sodium carbonate were kept the same.
Predict the final volume of carbon dioxide produced at this
temperature.
cm3
[0500/31/01]
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Marks KU PS
18. (continued)
(b) Another experiment involved determining the concentration of sodium
carbonate solution by titration.
0·05 mol/l sulphuric acid
25·0 cm3 sodium carbonate solution
The results showed that 20 cm3 of sulphuric acid was required to
neutralise the sodium carbonate solution.
(i) Calculate the number of moles of sulphuric acid in this volume.
mol
1
(ii) One mole of sulphuric acid reacts with one mole of sodium
carbonate.
Using your answer from part (b)(i), calculate the concentration, in
mol/l, of the sodium carbonate solution.
mol/l
1
(c) Name the salt produced when dilute sulphuric acid reacts with sodium
carbonate.
1
(6)
[END OF QUESTION PAPER]
[0500/31/01]
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ADDITIONAL SPACE FOR ANSWERS
ADDITIONAL DIAGRAM FOR QUESTION 14(c)
e
A
e
ion bridge
copper(II) sulphate
solution
ADDITIONAL GRAPH PAPER FOR QUESTION 18(a)(i)
[0500/31/01]
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ADDITIONAL SPACE FOR ANSWERS
[0500/31/01]
Page twenty-five
KU PS
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IN THIS
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ADDITIONAL SPACE FOR ANSWERS
[0500/31/01]
Page twenty-six
KU PS
[BLANK PAGE]
[BLANK PAGE]
FOR OFFICIAL USE
C
KU
PS
Total
Marks
0500/31/01
NATIONAL
QUALIFICATIONS
2012
CHEMISTRY
MONDAY, 14 MAY
10.50 AM – 12.20 AM
STANDARD GRADE
Credit Level
Fill in these boxes and read what is printed below.
Full name of centre
Town
Forename(s)
Surname
Date of birth
Day
Month
Year
Scottish candidate number
Number of seat
1 All questions should be attempted.
2 Necessary data will be found in the Data Booklet provided for Chemistry at Standard
Grade and Intermediate 2.
3 The questions may be answered in any order but all answers are to be written in this
answer book, and must be written clearly and legibly in ink.
4 Rough work, if any should be necessary, as well as the fair copy, is to be written in this
book.
Rough work should be scored through when the fair copy has been written.
5 Additional space for answers and rough work will be found at the end of the book.
6 The size of the space provided for an answer should not be taken as an indication of how
much to write. It is not necessary to use all the space.
7 Before leaving the examination room you must give this book to the Invigilator. If you do
not, you may lose all the marks for this paper.
SA 0500/31/01 6/23710
*0500/31/01*
©
PART 1
In Questions 1 to 9 of this part of the paper, an answer is given by circling the
appropriate letter (or letters) in the answer grid provided.
In some questions, two letters are required for full marks.
If more than the correct number of answers is given, marks will be deducted.
A total of 20 marks is available in this part of the paper.
SAMPLE QUESTION
A
D
CH4
CO
B
E
C
H2
C2H5OH
F
CO2
C
(a) Identify the hydrocarbon.
A
B
C
D
E
F
The one correct answer to part (a) is A. This should be circled.
(b) Identify the two elements.
A
B
C
D
E
F
As indicated in this question, there are two correct answers to part (b). These are B and F.
Both answers are circled.
If, after you have recorded your answer, you decide that you have made an error and wish
to make a change, you should cancel the original answer and circle the answer you now
consider to be correct. Thus, in part (a), if you want to change an answer A to an answer D,
your answer sheet would look like this:
A
B
C
D
E
F
If you want to change back to an answer which has already been scored out, you should
enter a tick (3) in the box of the answer of your choice, thus:
[0500/31/01]
3A
B
C
D
E
F
Page two
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MARGIN
Marks KU PS
1. The grid shows the formulae of some gases.
A
B
C
CO
D
NO2
CO2
E
F
H2
HCl
O2
(a) Identify the two toxic gases produced during the burning of
polyvinylchloride (PVC).
A
B
C
D
E
F
1
(b) Identify the gas which burns with a pop.
A
B
C
D
E
F
1
(2)
[Turn over
[0500/31/01]
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IN THIS
MARGIN
Marks KU PS
2. The table shows some fractions from crude oil.
Crude
oil
Fraction
Boiling
range/°C
Name of
fraction
A
–160 to 20 °C
Refinery
Gas
B
20 to 120 °C
Naphtha
C
120 to 240 °C
Kerosene
D
240 to 350 °C
Gas Oils
E
Over 350 °C
Residue
(a) Identify the fraction with the longest chain length.
A
B
C
D
E
1
(b) Identify the fraction which is used as fuel for aeroplanes.
A
B
C
D
E
1
(2)
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3. Lead(II) nitrate solution reacts with potassium iodide solution to give a
yellow solid.
Pb2+(aq) + 2NO3–(aq) + 2K+(aq) + 2I–(aq)
Marks KU PS
Pb2+(I–)2(s) + 2K+(aq) + 2NO3–(aq)
Identify the two spectator ions in the reaction.
A
Pb2+
B
NO3–
C
K+
D
I–
A
B
C
D
(1)
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Marks KU PS
4. The grid shows information about some particles.
Particle
A
B
C
D
E
Number of
neutrons
12
10
13
20
10
protons
11
9
11
19
9
electrons
11
9
11
18
10
(a) Identify the particle which is a negative ion.
A
B
C
D
E
1
(b) Identify the particle which would give a lilac flame colour.
You may wish to use the data booklet to help you.
A
B
C
D
E
1
(c) Identify the two particles which are isotopes.
A
B
C
D
E
1
(3)
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5. The grid shows the structural formulae of some hydrocarbons.
A
B
H
H
H
H
C
C
C
H
H
H
H
D
H
C
H
H
H
H
C
C
C
C
H
H
H
H
E
H
H
H C H
H
H
C C C H
H
C
C H
H H
H
C
C H
H
H
H
H
H
C
H
H
C
C
H
H
H
F
H H
H
C C C
H
C
H
H H H
(a) Identify the hydrocarbon which reacts with hydrogen to form butane.
A
B
C
D
E
F
A
B
C
D
E
F
1
(b) Identify the two isomers.
1
(c) Identify the structural formula which represents propene.
A
B
C
D
E
F
1
(3)
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6. Equations are used to represent chemical reactions.
A
Zn(s)
B
C2H5OH() + 3O2(g)
C
SO2(g) + H2O()
D
H+(aq) + OH– (aq)
E
SO42–(aq) + 2H+(aq) + 2e–
Marks KU PS
Zn2+(aq) + 2e–
2CO2(g) + 3H2O()
2H+(aq) + SO32–(aq)
H2O()
SO32–(aq) + H2O()
(a) Identify the equation which represents the formation of acid rain.
A
B
C
D
E
1
(b) Identify the equation which represents combustion.
A
B
C
D
E
1
(2)
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Marks KU PS
7. The grid shows the names of some soluble compounds.
A
B
sodium iodide
D
C
potassium chloride
E
barium bromide
lithium chloride
F
sodium hydroxide
potassium sulphate
(a) Identify the base.
A
B
C
D
E
F
1
(b) Identify the two compounds whose solutions would form a precipitate
when mixed.
You may wish to use the data booklet to help you.
A
B
C
D
E
F
1
(c) Identify the compound with a formula of the type XY2, where X is a
metal.
A
B
C
D
E
F
1
(3)
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8. The grid shows the names of some processes.
A
distillation
B
precipitation
C
filtering
D
electrolysis
E
dissolving
Marks KU PS
(a) Identify the process which is used to increase the alcohol concentration
of fermentation products.
A
B
C
D
E
1
(b) Identify the two processes which should be used to separate magnesium
carbonate from a mixture of solid magnesium carbonate and solid
magnesium chloride.
You may wish to use the data booklet to help you.
A
B
C
D
E
1
(2)
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9. A student made some statements about the particles in an atom.
A
It has a negative charge.
B
It is found inside the nucleus.
C
It has zero charge.
D
It is found outside the nucleus.
E
It has a relative mass of almost zero.
F
It has a relative mass of 1.
Marks KU PS
Identify the two statements which apply to a proton.
A
B
C
D
E
F
(2)
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Marks KU PS
PART 2
A total of 40 marks is available in this part of the paper.
10. Iron can be coated with a physical barrier to prevent rusting.
(a) How does coating iron prevent rusting?
1
(b) A student investigated the rusting of iron. The coatings on four strips
of iron were scratched to expose the iron. The strips were then placed
in salt water.
salt water
zinc
coated
iron strip
plastic
coated
iron strip
tin
coated
iron strip
silver
coated
iron strip
A
B
C
D
(i) Which iron strip has been galvanised, A, B, C or D?
1
(ii) Which iron strip would have rusted most quickly, A, B, C or D?
1
(3)
[0500/31/01]
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11. A student carried out some experiments between zinc and excess 1 mol/l
hydrochloric acid.
Marks KU PS
The graph shows the results of each experiment.
1
Volume of
hydrogen/cm3
2
3
Time/minutes
(a) In which experiment did the reaction take longest to finish, 1, 2 or 3?
1
(b) In all three experiments she kept the temperature the same and used the
same volume of 1 mol/l hydrochloric acid.
(i) Suggest one factor that could have been changed from experiment 1
to produce the results in experiment 2.
1
(ii) 1 g of zinc was used in experiment 1.
What mass of zinc was used in experiment 3?
g
1
(3)
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Marks KU PS
12. Ammonia is produced in the Haber process.
The percentage yield of ammonia, obtained at different pressures, is shown
in the table.
Pressure/
atmospheres
Percentage yield
of ammonia
50
6
100
10
150
14
200
19
250
22
350
29
400
32
(a) Draw a line graph of the results.
Use appropriate scales to fill most of the graph paper.
(Additional graph paper, if required, can be found on page 26.)
2
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Marks KU PS
12. (continued)
(b) Using your graph, estimate the yield of ammonia at 300 atmospheres.
%
1
(c) Temperature is another factor which affects the percentage yield of
ammonia.
Temperature/°C
Percentage yield
of ammonia
200
88
300
67
400
49
500
18
Suggest a reason why 500 °C is the temperature chosen to operate an
industrial ammonia plant rather than 200 °C.
1
(4)
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13. Hydrogen gas is made up of diatomic molecules.
Marks KU PS
(a) Draw a diagram to show how the electrons are arranged in a molecule of
hydrogen, H2.
1
(b) Hydrogen gas is produced when magnesium reacts with dilute sulphuric
acid.
gas syringe
magnesium ribbon
dilute sulphuric acid
The equation for the reaction is:
Mg(s) + H2SO4(aq)
(i)
[0500/31/01]
MgSO4(aq) + H2(g)
Circle the formula for the salt in the above equation.
Page sixteen
1
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Marks KU PS
13. (b) (continued)
(ii) The table shows the volume of hydrogen gas produced over fifty
seconds.
Time/s
Volume of gas/cm3
0
0
10
20
20
40
30
55
40
65
50
72
The average rate at which gas is produced can be calculated as shown.
average rate between
10 and 20 seconds
=
change in volume of gas during time period
length of time peeriod
=
40 − 20 = 20
20 − 10
10
=
2 cm3/s
Calculate the average rate at which gas is produced between
20 seconds and 30 seconds.
cm3/s
1
(3)
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14. Saliva contains an enzyme which breaks down starch.
Marks KU PS
(a) Name the type of chemical reaction taking place when starch breaks
down.
1
(b) A student carried out an experiment to break down starch.
starch solution
and saliva
water bath at
37 °C
He repeated the experiment using water at 100 °C.
What effect would this have on the activity of the enzyme?
1
(c) The monosaccharide glucose is produced when starch is broken down.
Name another monosaccharide.
1
(3)
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15. Potassium hydroxide reacts with sulphuric acid to form potassium sulphate,
which can be used as a fertiliser.
KOH(aq)
+
H2SO4(aq)
K2SO4(aq)
+
Marks KU PS
H2O()
1
(a) Balance the above equation.
(b) Name the type of chemical reaction taking place.
1
(c) Calculate the percentage, by mass, of potassium in potassium sulphate,
K2SO4.
Show your working clearly.
%
2
(d) Ammonium phosphate is also used as a fertiliser.
Write the ionic formula for ammonium phosphate.
1
(5)
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16. Titanium is an important metal used in aircraft manufacture.
Marks KU PS
(a) Titanium can be produced from titanium chloride as shown.
2Mg(s) + TiCl4()
2MgCl2(s) + Ti(s)
Name the type of chemical reaction represented by the equation.
1
(b) The magnesium chloride produced can be electrolysed as shown.
power
supply
electrode B
electrode A
molten magnesium
chloride
heat
(i) At which electrode would magnesium be produced, A or B?
1
(ii) Write the ion-electron equation for the formation of chlorine.
You may wish to use the data booklet to help you.
1
(3)
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Marks KU PS
17. A solution of 0·1 mol/l hydrochloric acid has a pH of 1.
(a)
(i) What colour would universal indicator turn when added to a
solution of hydrochloric acid?
1
(ii) Starting at pH 1, draw a line to show how the pH of this acid
changes when diluted with water.
13
11
9
pH
7
5
3
1
Increasing dilution
1
(b) Calculate the number of moles of hydrochloric acid in 50 cm3 of
0·1 mol/l hydrochloric acid solution.
mol
1
(3)
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18. A student investigated how the concentration of sodium chloride in water
affected the freezing point.
Marks KU PS
(a) What type of bond is broken in sodium chloride when it dissolves in
water?
1
(b) The table shows information about the freezing point of different
sodium chloride solutions.
Concentration of
sodium chloride
solution (mol/l)
0
0·09
0·18
0·27
0·37
0·46
Freezing point (°C)
0
– 0·2
– 0·5
– 0·8
– 1·1
– 1·5
Describe the relationship between the concentration and freezing point.
1
(c) Predict the freezing point of a 0·55 mol/l sodium chloride solution.
°C
1
(3)
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19. In Australia flow cells are used to store the energy from solar cells.
Marks KU PS
A
electrolyte flow
electrolyte flow
electrode A
electrode B
membrane
(a) The reaction taking place at electrode A when the cell is providing
electricity is:
Zn
Zn2+ + 2e–
Name the type of chemical reaction taking place at electrode A.
1
(b) On the diagram, clearly mark the path and direction of electron flow.
1
(c) Name the non-metal, that conducts electricity, which could be used as
an electrode.
1
(3)
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20. The monomer in superglue has the following structure.
Marks KU PS
H COOCH3
C
C
H CN
(a) Draw a section of the polymer, showing three monomer units joined
together.
1
(b) The polymer does not change shape on heating.
What term is used to describe this type of polymer?
1
(c) Bromine reacts with the monomer to produce a saturated compound.
Draw the structural formula for this compound.
H COOCH3
C
C
+ Br Br
H CN
1
(3)
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Marks KU PS
21. Aluminium is extracted from the ore bauxite.
(a) Circle the correct phrase to complete the sentence.
{
{
Aluminium is extracted from its ore
by heating with carbon
by heating alone
by electrolysis
.
1
(b) Aluminium can be mixed with other metals to make a magnet.
What term is used to describe a mixture of metals?
1
(c) The composition of a 250 g magnet is shown.
Metal
% by mass
aluminium
nickel
cobalt
copper
titanium
iron
10
25
20
4
1
40
(i) Calculate the mass, in grams, of aluminium in the magnet.
Show your working clearly.
g
1
(ii) Using your answer to (c)(i), calculate the number of moles of
aluminium in the magnet.
Show your working clearly.
mol
1
(4)
[END OF QUESTION PAPER]
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ADDITIONAL SPACE FOR ANSWERS
ADDITIONAL GRAPH PAPER FOR QUESTION 12(a)
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ADDITIONAL SPACE FOR ANSWERS
[0500/31/01]
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KU PS
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ADDITIONAL SPACE FOR ANSWERS
[0500/31/01]
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KU PS
FOR OFFICIAL USE
C
KU
PS
Total
Marks
0500/402
NATIONAL
QUALIFICATIONS
2011
CHEMISTRY
THURSDAY, 26 MAY
10.50 AM – 12.20 PM
STANDARD GRADE
Credit Level
Fill in these boxes and read what is printed below.
Full name of centre
Town
Forename(s)
Surname
Date of birth
Day
Month
Year
Scottish candidate number
Number of seat
1 All questions should be attempted.
2 Necessary data will be found in the Data Booklet provided for Chemistry at Standard
Grade and Intermediate 2.
3 The questions may be answered in any order but all answers are to be written in this
answer book, and must be written clearly and legibly in ink.
4 Rough work, if any should be necessary, as well as the fair copy, is to be written in this
book.
Rough work should be scored through when the fair copy has been written.
5 Additional space for answers and rough work will be found at the end of the book.
6 The size of the space provided for an answer should not be taken as an indication of how
much to write. It is not necessary to use all the space.
7 Before leaving the examination room you must give this book to the Invigilator. If you do
not, you may lose all the marks for this paper.
SA 0500/402 6/23910
*0500/402*
©
PART 1
In Questions 1 to 10 of this part of the paper, an answer is given by circling the
appropriate letter (or letters) in the answer grid provided.
In some questions, two letters are required for full marks.
If more than the correct number of answers is given, marks will be deducted.
A total of 20 marks is available in this part of the paper.
SAMPLE QUESTION
A
D
CH4
CO
B
E
C
H2
CO2
F
C2H5OH
C
(a) Identify the hydrocarbon.
A
B
C
D
E
F
The one correct answer to part (a) is A. This should be circled.
(b) Identify the two elements.
A
B
C
D
E
F
As indicated in this question, there are two correct answers to part (b). These are B and F.
Both answers are circled.
If, after you have recorded your answer, you decide that you have made an error and wish
to make a change, you should cancel the original answer and circle the answer you now
consider to be correct. Thus, in part (a), if you want to change an answer A to an answer D,
your answer sheet would look like this:
A
B
C
D
E
F
If you want to change back to an answer which has already been scored out, you should
enter a tick (✓) in the box of the answer of your choice, thus:
✓
[0500/402]
A
B
C
D
E
F
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Marks KU PS
1.
Limewater can be made by dissolving calcium hydroxide in water.
Identify the term used to describe the water.
A
solute
B
solvent
C
solution
D
insoluble
A
B
C
D
(1)
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2.
Marks KU PS
Distillation of crude oil produces several fractions.
crude oil
Fraction
Number of carbon
atoms per molecule
A
1– 4
B
4 –10
C
10 –16
D
16 –20
E
20+
(a) Identify the fraction which is used to tar roads.
A
B
C
D
E
1
(b) Identify the fraction which is most flammable.
A
B
C
D
E
[0500/402]
1
(2)
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3.
Marks KU PS
The grid shows the symbols of some elements.
A
B
C
O
K
D
E
P
F
F
Li
Al
(a) Identify the element with the lowest density.
You may wish to use the data booklet to help you.
A
B
C
D
E
F
1
(b) Identify the two elements which can form ions with the same electron
arrangement as argon.
You may wish to use the data booklet to help you.
A
B
C
D
E
F
1
(c) Identify the two elements which would react together to form a
molecule with the same shape as an ammonia molecule.
A
B
C
D
E
F
1
(3)
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4.
Marks KU PS
The table contains information about some substances.
Substance
Melting
point/°C
Boiling
point/°C
Conducts as Conducts as
a solid
a liquid
A
–7
59
no
no
B
1492
2897
yes
yes
C
1407
2357
no
no
D
606
1305
no
yes
E
–39
357
yes
yes
F
–78
–33
no
no
(a) Identify the substance which is a gas at 0 °C.
A
B
C
D
E
F
1
(b) Identify the two substances which exist as molecules.
A
B
C
D
E
F
[0500/402]
1
(2)
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5.
Marks KU PS
The grid shows the formulae of some oxides.
A
B
ZnO
C
NO2
D
E
CuO
K2O
F
Fe2O3
CO
(a) Identify the two oxides which are covalent.
A
B
C
D
E
F
1
(b) Identify the oxide which dissolves in water to give an alkaline solution.
You may wish to use the data booklet to help you.
A
B
C
D
E
F
1
(c) Identify the oxide which is reduced in a blast furnace.
A
B
C
D
E
F
1
(3)
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6.
Equations are used to represent chemical reactions.
Marks KU PS
2H2O(  )
A
2H2(g) + O2(g)
B
2H2O( ) + O2(g) + 4e–
C
CH4(g) + 2O2(g)
D
H+(aq) + OH–(aq)
H2O( )
E
Zn(s) + FeSO4(aq)
Fe(s) + ZnSO4(aq)
4OH–(aq)
CO2(g) + 2H2O( )
(a) Identify the equation which represents neutralisation.
A
B
C
D
E
1
(b) Identify the equation involved in the rusting of iron.
A
B
C
D
E
[0500/402]
1
(2)
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7.
A student made the following statements about the particles found in an
atom.
A
Relative mass = 1
B
Charge = zero
C
Found outside the nucleus
D
Charge = 1+
E
Charge = 1–
Marks KU PS
Identify the two statements which apply to an electron.
A
B
C
D
E
(1)
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8.
Identify the two statements which apply to zinc.
Marks KU PS
You may wish to use the data booklet to help you.
A
It displaces calcium from a solution of calcium nitrate.
B
It reacts with cold water.
C
It can be obtained by heating its oxide.
D
It reacts with dilute hydrochloric acid.
E
It is displaced from a solution of its chloride by magnesium.
A
B
C
D
E
[0500/402]
(2)
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9.
Marks KU PS
The diagram shows how an object can be coated with silver.
power
supply
object being
coated with
silver
silver electrode
solution containing Ag+(aq)
The following reactions take place at the electrodes.
Negative electrode:
Ag+(aq) + e–
Ag(s)
Positive electrode:
Ag(s)
Ag+(aq) + e–
Identify the two correct statements.
A
Ions flow through the solution.
B
Silver ions move towards the silver electrode.
C
The process is an example of galvanising.
D
The mass of the silver electrode decreases.
E
Reduction occurs at the silver electrode.
A
B
C
D
E
(2)
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10.
A student made the following statements about the rusting of iron.
A
During rusting Fe3+ ions are changed to Fe2+ ions.
B
Rusting is an example of oxidation.
C
Iron rusts when connected to the negative terminal of a battery.
D
Tin gives sacrificial protection to iron.
E
Electroplating provides a surface barrier to air and water.
Marks KU PS
Identify the two correct statements.
A
B
C
D
E
[0500/402]
(2)
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Marks KU PS
PART 2
A total of 40 marks is available in this part of the paper.
11.
(a) The table shows information about two of the gases found in air.
Gas
Boiling point/°C
oxygen
–183
nitrogen
–196
At very low temperatures air is a mixture of liquids.
Name the process which can be used to separate this mixture.
1
(b) In a sample of oxygen there are two different types of oxygen atom:
18
8O
and
16
8O
(i) What term is used to describe these different types of oxygen
atom?
1
(ii) Complete the table for each type of oxygen atom.
Type of atom
Number of
protons
Number of
neutrons
18
8O
16
8O
1
(3)
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12.
Marks KU PS
(a) Ethanol, for alcoholic drinks, can be made from glucose.
Name this process.
1
(b) The table below shows the relationship between the percentage of
ethanol and the density of alcoholic drinks.
Percentage
of ethanol
(%)
Density of
alcoholic
drink
(g/cm3)
40
50
60
70
80
0·928
0·907
0·886
0·865
0·844
(i) Write a general statement describing how the percentage of ethanol
affects the density of the alcoholic drink.
1
(ii) The density of a particular brand of alcoholic drink is 0·970 g/cm3.
Predict the percentage of ethanol in this alcoholic drink.
%
1
(3)
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13.
Polyvinyldichloride (PVDC) is a plastic used in food packaging.
Marks KU PS
The structure of part of a PVDC molecule is shown.
Cl H Cl H Cl H
C C C C C C
Cl H Cl H Cl H
(a) Draw the full structural formula for the monomer used to make PVDC.
1
(b) Name a toxic gas produced when PVDC burns.
1
(2)
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14.
(a) When sulphur dioxide dissolves in water in the atmosphere “acid rain”
is produced.
Marks KU PS
Circle the correct phrase to complete the sentence.
Compared with pure water, acid rain contains
{
{
a higher
concentration of hydrogen ions.
a lower
the same
1
(b) The table shows information about the solubility of sulphur dioxide.
Temperature
/°C
0
20
30
40
50
60
Solubility in
g/100 cm3
22·0
10·0
6·0
3·0
2·0
1·5
Draw a line graph of solubility against temperature.
Use appropriate scales to fill most of the graph paper.
(Additional graph paper, if required, will be found on page 28.)
2
(3)
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15.
Scientists have developed a “bio-battery” which produces electricity from
sucrose.
Marks KU PS
(a) Write the molecular formula for sucrose.
1
(b) Name an isomer of sucrose.
1
(c) The sucrose is broken down using an enzyme.
(i) What is meant by the term “enzyme”?
1
(ii) The graph shows how temperature affects the activity of an
enzyme.
Increasing
enzyme
activity
0
10 20 30 40 50 60
Temperature °C
State one other factor which has a similar effect on enzyme
activity.
1
(4)
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16.
Marks KU PS
Heptane can be cracked as shown.
aluminium oxide
gas
mineral wool
soaked in
heptane
heat
water
One of the reactions which takes place is:
C7H16
C4H10 + C3H6
(a) The product C3H6 decolourises bromine solution quickly.
Draw a structural formula for an isomer of C3H6 , which would not
decolourise bromine solution quickly.
1
(b) Aluminium oxide is used as a catalyst to speed up the reaction.
(i) Suggest another reason for using a catalyst.
1
(ii) Write the formula for aluminium oxide.
1
(3)
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17.
Urea reacts with water, breaking down to form carbon dioxide and ammonia.
H2NCONH2
urea
+
H2O
CO2
+
Marks KU PS
2NH3
(a) Suggest a name for the type of chemical reaction taking place.
1
(b) Calculate the mass of ammonia produced, in grams, when 90 g of urea
breaks down.
g
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(3)
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18.
A student set up the following experiment to electrolyse cobalt chloride
solution.
Marks KU PS
power supply
electrodes
+
–
cobalt chloride
solution
(a) What type of power supply must be used to electrolyse cobalt chloride
solution?
1
(b) Describe what would be seen at the positive electrode.
You may wish to use the data booklet to help you.
1
(c) The formula for cobalt chloride is CoCl2.
What is the charge on the cobalt ion in CoCl2?
1
(3)
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19.
Catalysts can be used in different processes.
Marks KU PS
(a) The flow diagram shows the steps involved in the Haber process.
nitrogen gas
and
hydrogen gas
catalyst
mixture
unreacted gases
separator
ammonia
On the flow diagram above draw an arrow to show how the process is
made more economical.
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1
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19.
Marks KU PS
(continued)
(b) Ammonia can be used to produce nitrogen dioxide as shown.
ammonia
oxygen
catalyst Y
water
nitrogen
dioxide
(i)
Name catalyst Y.
1
(ii)
Why is it not necessary to continue to supply heat once the
reaction has started?
1
(c) Catalysts are also used in catalytic converters.
What is the purpose of a catalytic converter in a car exhaust system?
1
(4)
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20.
Marks KU PS
Metal salts can be produced by different methods.
(a) Lead(II) iodide can be produced by reacting lead(II) nitrate solution
with sodium iodide solution.
The equation for this reaction is:
Pb(NO3)2(aq)
+
NaI(aq)
PbI2(s)
+
NaNO3(aq)
1
(i)
Balance the above equation.
(ii)
What technique could be used to remove lead(II) iodide from the
mixture?
1
(b) The salt copper(II) nitrate can be produced as shown.
X
+
2HNO3
Cu(NO3)2
+
CO2
+
H2O
Name substance X.
1
(c) Potassium sulphate can be produced by titrating potassium hydroxide
solution with dilute sulphuric acid.
burette containing
0·1 mol/l sulphuric acid
conical flask
10 cm3 potassium hydroxide
solution
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20.
Marks KU PS
(c) (continued)
(i) What must be added to the conical flask to show the end-point of
the titration?
1
(ii)
The average volume of sulphuric acid used in the titration is
20 cm3.
Calculate the number of moles of sulphuric acid used.
mol
1
(d) The equation for the reaction is:
H2SO4
+
2KOH
K2SO4
+
2H2O
Using your answer from part (c)(ii), calculate the number of moles of
potassium hydroxide in the 10 cm3 sample of potassium hydroxide
solution.
mol
1
(6)
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21.
Marks KU PS
A technician set up the following cell.
V
electrode A
electrode B
solution containing
gold ions, Au+(aq)
solution containing
bromide ions, Br–(aq)
X
The reaction taking place at electrode B is:
2Br–(aq)
Br2(  )
+
2e–
(a) On the diagram, clearly mark the path and direction of electron flow.
1
(b) Write the ion-electron equation for the reaction taking place at
electrode A.
You may wish to use the data booklet to help you.
1
(c) Name the piece of apparatus labelled X.
1
(3)
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22.
Ethylthioethane belongs to a homologous series of compounds called
thioethers.
Marks KU PS
(a) What is meant by a homologous series?
1
(b) Ethylthioethane is formed when ethylthiol reacts with bromoethane as
shown.
H H
H C C
H H
H H
S H + Br C C H
H H
H H
ethylthiol
H C C
H H
S C C H + HBr
H H
bromoethane
H H
ethylthioethane
hydrogen
bromide
Draw the full structural formula for the thioether produced in the
following reaction.
H
H C
H H H
S H + Br C C C H
H
+ HBr
H H H
1
(c) Ethylthioethane can also be formed by the reaction of ethylthiol with
ethene.
H
H H
H C C
S H +
H H
ethylthiol
H
C
C
H
H H
H C C
H
ethene
H H
H H
S C C H
H H
ethylthioethane
Suggest a name for the type of chemical reaction taking place.
1
(3)
[END OF QUESTION PAPER]
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ADDITIONAL SPACE FOR ANSWERS
ADDITIONAL GRAPH PAPER FOR QUESTION 14(b)
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PS
ADDITIONAL SPACE FOR ANSWERS
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KU
PS
ADDITIONAL SPACE FOR ANSWERS
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KU
PS
[BLANK PAGE]
[BLANK PAGE]
FOR OFFICIAL USE
Section B
Total
Marks
X012/11/02
NATIONAL
QUALIFICATIONS
2013
FRIDAY, 31 MAY
1.00 PM – 3.00 PM
CHEMISTRY
INTERMEDIATE 2
Fill in these boxes and read what is printed below.
Full name of centre
Town
Forename(s)
Surname
Date of birth
Day
Month
Year
Scottish candidate number
Number of seat
Necessary data will be found in the Chemistry Data Booklet for Standard Grade and
Intermediate 2.
Section A – Questions 1–30 (30 marks)
Instructions for completion of Section A are given on page two.
For this section of the examination you must use an HB pencil.
Section B (50 marks)
All questions should be attempted.
The questions may be answered in any order but all answers are to be written in the spaces
provided in this answer book, and must be written clearly and legibly in ink.
Rough work, if any should be necessary, should be written in this book, and then scored
through when the fair copy has been written. If further space is required, a supplementary
sheet for rough work may be obtained from the Invigilator.
Additional space for answers will be found at the end of the book. If further space is required,
supplementary sheets may be obtained from the Invigilator and should be inserted inside the
front cover of this booklet.
Before leaving the examination room you must give this book to the Invigilator. If you do not,
you may lose all the marks for this paper.
SA X012/11/02 6/10710
*X012/11/02*
©
Read carefully
1
Check that the answer sheet provided is for Chemistry Intermediate 2 (Section A).
2
For this section of the examination you must use an HB pencil and, where necessary, an eraser.
3
Check that the answer sheet you have been given has your name, date of birth, SCN (Scottish
Candidate Number) and Centre Name printed on it.
Do not change any of these details.
4
If any of this information is wrong, tell the Invigilator immediately.
5
If this information is correct, print your name and seat number in the boxes provided.
6
The answer to each question is either A, B, C or D. Decide what your answer is, then, using your
pencil, put a horizontal line in the space provided (see sample question below).
7
There is only one correct answer to each question.
8
Any rough working should be done on the question paper or the rough working sheet, not on your
answer sheet.
9
At the end of the examination, put the answer sheet for Section A inside the front cover of
this answer book.
Sample Question
To show that the ink in a ball-pen consists of a mixture of dyes, the method of separation would be
A
chromatography
B
fractional distillation
C
fractional crystallisation
D
filtration.
The correct answer is A—chromatography. The answer A has been clearly marked in pencil with a
horizontal line (see below).
A
B
C
D
Changing an answer
If you decide to change your answer, carefully erase your first answer and using your pencil, fill in the
answer you want. The answer below has been changed to D.
A
[X012/11/02]
B
C
D
Page two
SECTION A
1. In an exothermic reaction
5. Which line in the table correctly describes a
proton?
A
there is no energy change
B
energy is released to the surroundings
C
energy is absorbed from the surroundings
D
the energy of the products is greater than
the energy of the reactants.
2.
When hydrogen chloride gas is dissolved in
water a solution containing hydrogen ions and
chloride ions is formed.
Which equation correctly shows the state
symbols for this change?
A
HCl(g) + H2O(l)
H+(aq) + Cl–(aq)
B
HCl(l) + H2O(aq)
H+(l) + Cl–(l)
C
HCl(aq) + H2O(l)
H+(aq) + Cl–(aq)
D
HCl(g) + H2O(l)
H+(l) + Cl–(l)
Mass
Charge
Location
A
negligible
0
outside nucleus
B
negligible
–1
outside nucleus
C
1
+1
in nucleus
D
1
0
in nucleus
6. In a hydrogen fluoride molecule, the atoms
share electrons in order to achieve the same
electron arrangements as atoms in group
A
0
B
1
C
2
D
7.
3. A bottle of whisky contains 40% ethanol by
volume.
Which line in the table is the correct
description of the mixture?
Solute
Solvent
Solution
A
ethanol
whisky
water
B
ethanol
water
whisky
C
water
ethanol
whisky
D
whisky
water
ethanol
B
Hydrolysis of starch
C
Cracking of hydrocarbons
D
Formation of alkenes from alkanes
[X012/11/02]
Vanadium(V) oxide
B
Vanadium(IV) oxide
C
Vanadium(III) oxide
D
Vanadium(II) oxide
The equation will be balanced when
Identify the process in which the catalyst
could be an enzyme.
Hydration of ethene
A
8. 4NH3 + xO2 → 4NO + yH2O
4. Many chemical processes involve catalysts.
A
7. What is the name of the compound with the
formula VO2?
A
x = 5, y = 6
B
x = 5, y = 10
C
x = 3, y = 6
D
x = 3, y = 10 .
9. Which of the following substances has the
smallest gram formula mass?
A
CO
B
CO2
C
N2
D
CH4
Page three
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10.
11. When a compound is burned completely, the
products are carbon dioxide and water.
H
H C H
H
H
H
C
C
From this information, it can be concluded
that the compound must contain
C
H
H
H
H C H
H
H H H H H
Which of the following compounds is an
H C
H C
H C
H C
H
C
isomerHof the
one shown
above? H
H
H H H H H
C C
H H
H C C C
H
C
H
C
C
C
C
A
H H H H H H
H
C
H
H
C
H
C
H
H
H C
H
H
H
H
C
H
C
H
C
H
H C H
H C H
H
H
C
H
H H
H H
H
C
H
C
H
H
C
H
H
H
C
H
H
H
hydrogen only
C
carbon and hydrogen
D
carbon, hydrogen and oxygen.
12. Which of the following hydrocarbons could be
cyclohexane?
H
H
H C H H C H
C
B
Hydrocarbon
C H
C H
H
H C
C H
C CC H
H
H CC
H
H CC
H
C
C
H
H H
H
H H C H H C H H
H
H
carbon only
H
H
H
B
H
C
C
A
H
C
H
C
C
C
H
C
H
C
C
H
H
C
H
H
H
C
H
C
H
HC
H
H
H
C
H
H
H
H
A
C6H14
no colour change
B
C6H12
rapid decolourisation
C
C6H12
no colour change
D
C6H10
rapid decolourisation
13. Ethanol can be produced from sugar cane by
A
oxidation
B
fermentation
C
polymerisation
D
catalytic hydration.
H
H
14. Propan-1-ol can be dehydrated.
H
H
H
H
D
H
H
H
C
H
C
H
C
H
H
H
C
H
H
H
H
H
H
H
CH
H
C
H
H
H
C
H
H
H
C
H
H
H
H H
C
H HH
C
H
C
C
H HC
C H
C
C HH
C HC
C
H
C
H
H H
C
C
C
H H
H
H H
C
H
H
H
H
C
C
C
H
H
OH
H
Which of the following compounds is a product
of the reaction?
H
A
Propanoic acid
H
B
Propyl propanoate
H
C
Propene
D
Propane
H
[X012/11/02]
Molecular Observations on adding
bromine solution
formula
Page four
15. The first four members of the amine homologous series are:
H
H
C
H
H
H
N
H
H
H
C
C
H
H
H
N
H
H
H
H
H
C
C
C
H
H
H
H
N
H
H
H
H
H
H
C
C
C
C
H
H
H
H
H
N
What is the general formula for this homologous series?
A
Cn Hn+4 N
B
Cn H2n+3 N
C
Cn H3n+2 N
D
Cn H4n+1 N
16. Biopol is a polymer which is
A
natural and biodegradeable
B
synthetic and biodegradeable
C
natural and non-biodegradeable
D
synthetic and non-biodegradeable.
19. In which of the following experiments would
both carbohydrates give an orange precipitate
when heated with Benedict’s solution?
A
17. Which of the following fatty acids contains the
most double bonds per molecule?
A
C17H35COOH
B
B
C17H33COOH
C
C17H31COOH
D
C17H29COOH
maltose
sucrose
glucose
starch
maltose
maltose
glucose
C
18. An alkaline solution contains
A
hydroxide ions but no hydrogen ions
B
equal numbers of hydrogen and hydroxide
ions
C
more hydroxide ions than hydrogen ions
D
more hydrogen ions than hydroxide ions.
[X012/11/02]
sucrose
D
Page five
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H
20. When hydrochloric acid with a pH of 3 is
diluted with water to give a solution with a pH
of 6, the concentration of
A
H+(aq) ions decreases
B
OH–(aq) ions decreases
C
D
25. When nickel(II) chloride solution is added to
sodium carbonate solution an insoluble solid is
formed.
A sample of the solid can be separated from
the mixture by
+
H (aq) ions and the concentration of
OH–(aq) ions become equal
+
H (aq) ions and the concentration of
OH–(aq) ions remain unchanged.
21. 0·25 mol of potassium hydroxide was dissolved
in water and the solution made up to 500 cm3.
A
condensation
B
distillation
C
evaporation
D
filtration.
26.
tin
copper
V
What was the concentration, in mol l–1, of the
solution which was formed?
A
0·0005
B
0·125
C
0·5
D
2·0
ion
bridge
tin chloride
solution
copper chloride
solution
In the cell shown electrons flow through
22. Which of the following compounds is a base?
A
the solution from copper to tin
A
Sodium carbonate
B
the solution from tin to copper
B
Sodium chloride
C
the wires from copper to tin
C
Sodium nitrate
D
the wires from tin to copper.
D
Sodium sulphate
27.
metal
23. Which of the following gases reacts with an
alkaline solution?
A
Argon
B
Oxygen
C
Ammonia
D
Nitrogen dioxide
24. Which of the following compounds is a salt?
A
Ammonium chloride
B
Calcium oxide
C
Hydrogen chloride
D
Sodium hydroxide
[X012/11/02]
V
zinc
sodium chloride solution
Which of the following metals, when linked to
zinc, would give the highest cell voltage?
(You may wish to use the data booklet to help you.)
A
Copper
B
Iron
C
Magnesium
D
Tin
Page six
28. In which test tube will the iron nail corrode fastest?
copper
copper
iron
nail
zinc
iron
nail
zinc
iron
nail
iron
nail
salt water
tap water
salt water
tap water
A
B
C
D
29. When a metal element reacts to form a compound
the metal is
30. Which of the following metals can be obtained
from its ore by heating with carbon monoxide?
(You may wish to use the data booklet to help you.)
A
displaced
B
oxidised
A
Aluminium
C
precipitated
B
Calcium
D
reduced.
C
Magnesium
D
Nickel
Candidates are reminded that the answer sheet for Section A MUST be
placed INSIDE the front cover of this answer book.
[Turn over
[X012/11/02]
Page seven
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[X012/11/02]
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Marks
SECTION B
50 marks are available in this section of the paper.
All answers must be written clearly and legibly in ink.
1. (a) Strontium compounds have many uses.
(i) Strontium nitrate is used in warning flares.
What colour of flame will strontium nitrate give?
(You may wish to use the data booklet to help you.)
1
(ii) Strontium chloride hexahydrate can be used in toothpaste for
sensitive teeth as it plugs the holes in the tooth enamel.
This is possible because strontium has similar chemical properties
to calcium.
Why does strontium have similar chemical properties to calcium?
1
(b)
Strontium can be extracted from the compound strontium chloride
using electrolysis.
Label the diagram to show the charge on each electrode.
power
pack
electrode
electrode
strontium
chlorine
molten strontium chloride
1
(3)
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[X012/11/02]
Page nine
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Marks
2. In the PPA, “Effect of temperature on reaction rate”, the reaction between
sodium thiosulphate solution and dilute hydrochloric acid is investigated.
sodium thiosulphate
solution and dilute
hydrochloric acid
(a) How is the rate of the reaction determined?
1
(b) State a factor which should be kept constant.
1
(c) Apart from wearing safety glasses, state another safety precaution which
must be taken when carrying out this experiment.
1
(d) The equation for the reaction taking place is
2Na+(aq) + S2O32–(aq) + 2H+(aq) + 2Cl–(aq)
2Na+(aq) + 2Cl–(aq) + SO2(g) + S(s) + H2O(l)
Circle a spectator ion in the equation.
1
(4)
[X012/11/02]
Page ten
[Turn over for Question 3 on Page twelve
[X012/11/02]
Page eleven
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Marks
3. Magnesium reacts with dilute sulphuric acid to produce a gas.
gas syringe
100 cm3 of 1 mol l–1
sulphuric acid
magnesium ribbon
(a)Name the gas produced in this reaction.
1
(b) A student carried out the experiment. A graph of the results was plotted.
80
70
60
Volume 50
of
gas
(cm3) 40
30
20
10
0
10
20
30
40
50
60
70
Time (s)
Calculate the average rate of the reaction, in cm3 s–1, for the first 40 seconds.
cm3 s–1
[X012/11/02]
Page twelve
1
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Marks
3. (continued)
(c)Predict the total volume of gas produced if the experiment was repeated
using silver.
cm3.
1
(d)The student repeated the experiment using 100 cm3 of 1 mol l–1 ethanoic
acid solution and the same mass of magnesium ribbon.
How would this affect the rate of the reaction?
1
(4)
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[X012/11/02]
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Marks
4. Tritium is a naturally occurring isotope of hydrogen. It can be represented as
3
H
1
Complete the table to show the number of particles in an atom of
(a)
tritium.
Type of particle
Number of particles
proton
neutron
electron
1
(b)Hydrogen has three isotopes.
Isotope of hydrogen
Mass number
protium
1
deuterium
2
tritium
3
The relative atomic mass of hydrogen is 1.
Which isotope of hydrogen is the most abundant?
1
(2)
[X012/11/02]
Page fourteen
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Marks
5. Electronegativity is a measure of the attraction that an atom has for the
bonded electrons.
(a) What type of bond is formed when the attraction of the atoms for the
bonded electrons is different?
1
(b) The chart shows the electronegativity values for some elements in the
Periodic Table.
4
Electronegativity
3·5
3
2·5
2
1·5
1
0·5
0
1
2
3
4
5
6
7
8
9 10 11 12 13 14 15 16 17 18 19 20
Atomic number
(i) Describe what happens to the electronegativity values going across
a period in the Periodic Table.
1
(ii) Draw a bar on the chart to show the electronegativity value for the
element calcium, atomic number 20.
1
(3)
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6. Dishwasher tablets contain many different types of chemicals.
(a) A dishwasher tablet was found to contain 1·57 g of the bleaching agent,
sodium percarbonate.
How many moles are there in 1·57g of sodium percarbonate?
(Formula mass of sodium percarbonate = 157.)
moles
1
(b) Many dishwasher tablets contain sand which can help to remove food
deposits. Sand contains the covalent compound silicon dioxide.
What type of structure does silicon dioxide have?
(You may wish to use page 6 of the data booklet to help you.)
1
(c) Phosphate ions, present in some types of dishwasher tablets, react with
calcium ions in water forming calcium phosphate.
Write the formula for calcium phosphate.
1
(3)
[X012/11/02]
Page sixteen
7. The car industry and the Government have taken a number of steps to
reduce the emissions of pollutant gases from cars.
Marks
(a) Catalytic converters reduce the emission of carbon monoxide by
converting it to a harmless gas.
Name this harmless gas.
1
(b) Car tax is based on the mass of carbon dioxide gas produced per
kilometre travelled by a car.
(i) The volume of carbon dioxide produced by a car is measured and
then converted into mass using the following equation.
Mass of carbon dioxide gas (g) =
100 × volume of carbon dioxide gas (l)
56·3
Calculate the mass of carbon dioxide gas which is produced by a
car emitting 70·4 l of carbon dioxide gas.
g
1
(ii) Information about car tax bands is shown in the tables.
Car tax
band
Mass of carbon dioxide gas
emitted per kilometre (g)
Car tax
band
A
Up to 100
A
0·00
B
101–110
B
20·00
C
111–120
C
30·00
D
121–130
D
95·00
E
131–140
E
115·00
F
141–150
F
130·00
G
151–165
G
165·00
12 month rate
(£)
What would it cost to tax a car, for 12 months, which emits 146 g
of carbon dioxide per kilometre travelled?
1
£
(3)
[X012/11/02]
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8. Crude oil is a mixture of hydrocarbons which can be separated into fractions
by fractional distillation.
Fraction
Refinery gas
Crude oil
Number of
Carbon atoms
1–5
Petrol
5 –10
Paraffin
10 –16
Diesel
14 –20
Lubricating oil
20 –50
Bitumen
50 or more
(a) What property of hydrocarbons is used to separate crude oil into
fractions?
1
(b) The viscosity of four fractions was compared by measuring the rate of
fall of a ball bearing. The diagram shows the position of the ball
bearings 10 seconds after being dropped.
petrol
paraffin
diesel
lubricating oil
What effect does the number of carbon atoms have on the viscosity of a
fraction?
1
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8. (continued)
(c) Petrol contains the following molecule.
H
H
H
H
H C H H C H
H
C
C
C
C
H
H
H
H
H
Name this molecule.
1
(3)
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9. Alkenes can undergo different reactions.
(a)In ozonolysis an alkene reacts with ozone forming two molecules. The
ozonolysis of hex-3-ene is shown.
H
H
H
C
C
H
H
H
H
C
C
C
C
H
H
H
H
hex-3-ene
H
H
H
H
C
C
C
H
H
H
O + O
H
H
C
C
C
H
H
H
H
Draw the products formed by the ozonolysis of hex-2-ene.
H
H
H
H
H
C
C
C
C
C
C
H
H
H
H
H
H
H
1
(b) Potassium permanganate can be used to convert alkenes into two molecules.
The conversion of pent-1-ene is shown.
H
H
H
H
C
C
C
C
C
H
H
H
H
H
H
H
H
H
H
C
C
C
H
H
H
O
+ CO2
C
OH
molecule X
(i) Name molecule X.
1
(ii) State the test for carbon dioxide.
1
(3)
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10. Some waterproof clothing contains a thin layer of the plastic PTFE.
(a) PTFE is heated and reshaped to make thin layers.
What term is used to describe a plastic which can be heated and
reshaped?
1
(b)
(i) PTFE is a polymer made from the monomer shown.
F
F
C
C
F
F
Draw a section of the PTFE polymer, showing three monomer
units joined together.
1
(ii) Name this type of polymerisation reaction.
1
(c) Name a toxic gas produced when PTFE is burned.
1
(4)
[X012/11/02]
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11.
Migraine, a type of headache, is caused
when calcium ions promote the release of a
chemical called CGRP in the nervous
tissues. Scientists are using cone snails to
develop a treatment for migraine. Cone
snails produce a chemical which can be
used to prevent the release of CGRP.
(a)What is the electron arrangement for a calcium ion, Ca2+?
1
(b) CGRP is formed from different amino acids.
A short sequence of CGRP is shown.
COOH
SH
CH3
H
CH2
O
H
CH2 O
H
HCOH O
N
C
C
N
C
N
C
H
C
H
C
H
(i) Circle a peptide link in the above section.
1
(ii) Draw one of the amino acids used to form the above section.
1
(3)
[X012/11/02]
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12. Fats and oils are examples of esters.
tristearate is shown below.
The structure of the fat glyceryl
O
H
H
C
O
C
O
C17 H35
H
C
O
C
O
C17 H35
H
C
O
C
C17 H35
H
(a)Draw an ester group.
1
(b) Fats and oils can be broken down to form glycerol and fatty acids.
Name this type of chemical reaction.
1
(c)The equation below shows the breakdown of glyceryl tristearate to form
glycerol and stearic acid.
C57H110O6
glyceryl tristearate
+
3H2O
C3H8O3
water
glycerol
+
3C18H36O2
stearic acid
GFM = 890 g
Calculate the mass of stearic acid produced from 8·9 g of glyceryl
tristearate.
g
2
(4)
[X012/11/02]
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13.
When a hippopotamus is seen out of
water it looks as though it is bleeding.
This is due to a red coloured secretion
which protects the hippopotamus
against sunburn caused by UVB
radiation. Scientists have found that
one of the active ingredients in this
natural sunscreen is a chemical called
hipposudoric acid.
O
C
H
O
HO
C
C
C
C
H
H
OH
C
O
C
C
C
C
O
C
C
C
OH
O
C
C
H
C
H
hipposudoric acid
(a)
(i) Suggest a pH value for hipposudoric acid.
1
(ii) Hipposudoric acid contains a hydroxyl group.
Circle the hydroxyl group in the structure of hipposudoric acid.
[X012/11/02]
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13. (continued)
(b) Bottles of sun cream display a sun protection factor which gives an
indication of how well the sun cream protects against UVB radiation.
The table gives information about sun protection factors.
Sun protection factor
0
2
4
8
15
30
50
UVB radiation screened (%)
0
50
70
88
94
97
98
Draw a line graph to show the percentage of UVB radiation screened by
different sun protection factors.
(Additional graph paper, if required, can be found on Page twenty-eight.)
2
(4)
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14. A student’s report is shown for the PPA “Reaction of metals with oxygen”.
Title
Reactions of Metals with Oxygen
Date 15/11/12
Aim
Procedure
The apparatus required to carry out the experiment was collected and assembled as shown.
mineral wool
potassium
permanganate
magnesium ribbon
heat
Results
Metal
Observations
zinc
moderately fast reaction
magnesium
copper
(a) State the aim of the experiment.
1
(b) Why is potassium permanganate used in this experiment?
1
(c) Complete the table to show the observations for magnesium and copper.
1
(d) For safety reasons this experiment would not be carried out with
potassium metal.
Suggest a reason for this.
1
[X012/11/02]
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15. Titanium metal is used to make dental braces.
Titanium is extracted from its ore in the Kroll process. One step in this
process involves the displacement of titanium chloride by sodium metal.
The equation is shown.
4Na
+
TiCl4
4NaCl
+
Ti
(a) What does this method of extraction tell you about the reactivity of
titanium metal compared to sodium metal?
1
(b) During the displacement, sodium atoms, Na, form sodium ions, Na+.
Write the ion-electron equation for this change.
1
(c) The displacement reaction is carried out in an atmosphere of the noble
gas, argon.
Suggest why an argon atmosphere is used.
1
(3)
[END OF QUESTION PAPER]
[X012/11/02]
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ADDITIONAL SPACE FOR ANSWERS
ADDITIONAL PAPER FOR QUESTION 13(b)
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FOR OFFICIAL USE
Section B
Total
Marks
X012/11/02
NATIONAL
QUALIFICATIONS
2012
MONDAY, 14 MAY
1.00 PM – 3.00 PM
CHEMISTRY
INTERMEDIATE 2
Fill in these boxes and read what is printed below.
Full name of centre
Town
Forename(s)
Surname
Date of birth
Day
Month
Year
Scottish candidate number
Number of seat
Necessary data will be found in the Chemistry Data Booklet for Standard Grade and
Intermediate 2.
Section A – Questions 1–30 (30 marks)
Instructions for completion of Section A are given on page two.
For this section of the examination you must use an HB pencil.
Section B (50 marks)
All questions should be attempted.
The questions may be answered in any order but all answers are to be written in the spaces
provided in this answer book, and must be written clearly and legibly in ink.
Rough work, if any should be necessary, should be written in this book, and then scored
through when the fair copy has been written. If further space is required, a supplementary
sheet for rough work may be obtained from the Invigilator.
Additional space for answers will be found at the end of the book. If further space is required,
supplementary sheets may be obtained from the Invigilator and should be inserted inside the
front cover of this booklet.
Before leaving the examination room you must give this book to the Invigilator. If you do not,
you may lose all the marks for this paper.
SA X012/11/02 6/10410
*X012/11/02*
©
Read carefully
1
Check that the answer sheet provided is for Chemistry Intermediate 2 (Section A).
2
For this section of the examination you must use an HB pencil and, where necessary, an eraser.
3
Check that the answer sheet you have been given has your name, date of birth, SCN (Scottish
Candidate Number) and Centre Name printed on it.
Do not change any of these details.
4
If any of this information is wrong, tell the Invigilator immediately.
5
If this information is correct, print your name and seat number in the boxes provided.
6
The answer to each question is either A, B, C or D. Decide what your answer is, then, using your
pencil, put a horizontal line in the space provided (see sample question below).
7
There is only one correct answer to each question.
8
Any rough working should be done on the question paper or the rough working sheet, not on your
answer sheet.
9
At the end of the examination, put the answer sheet for Section A inside the front cover of
this answer book.
Sample Question
To show that the ink in a ball-pen consists of a mixture of dyes, the method of separation would be
A
chromatography
B
fractional distillation
C
fractional crystallisation
D
filtration.
The correct answer is A—chromatography. The answer A has been clearly marked in pencil with a
horizontal line (see below).
A
B
C
D
Changing an answer
If you decide to change your answer, carefully erase your first answer and using your pencil, fill in the
answer you want. The answer below has been changed to D.
A
[X012/11/02]
B
C
D
Page two
SECTION A
1. An element, X, has the following properties.
•
It is a gas.
•
It is not made up of molecules.
•
It does not react with other elements.
Element, X, is likely to be in group
A
0
B
1
C
2
D
7.
4. Which of the following numbers is the same
for lithium and oxygen atoms?
A
Mass number
B
Atomic number
C
Number of outer electrons
D
Number of occupied energy levels
5. Atoms of an element form ions with a single
positive charge and an electron arrangement of
2, 8.
The element is
A
fluorine
B
lithium
AMagnesium ribbon
C
sodium
B
Magnesium powder
D
neon.
C
Zinc ribbon
D
Zinc powder
2.
Which of the following would react fastest
–1
with 2 mol l hydrochloric acid?
6. Which of the following substances is made up
of molecules containing polar covalent bonds?
3. The diagram shows the energy changes during
a reaction.
Products
A
Calcium oxide
B
Chlorine
C
Sodium bromide
D
Water
7. Which of the following pairs of elements
combine to form an ionic compound?
Energy
Reactants
Reaction pathway
A
Lead and fluorine
B
Sulphur and oxygen
C
Carbon and nitrogen
D
Phosphorus and chlorine
Which of the following statements is true?
8. Which of the following compounds exists as
diatomic molecules?
A
The reaction is endothermic.
B
Energy is given out to the surroundings.
CThe reaction is exothermic.
DThe products have less energy than the
reactants.
A
Carbon monoxide
B
Sulphur dioxide
C
Nitrogen trihydride
D
Carbon tetrachloride
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9. The shapes and names of some molecules are
shown below.
13. The following structure represents an amine
called ethylmethylamine:
CH3
H
N
C2 H5
tetrahedral
pyramidal
bent
Another amine has the following structure:
linear
CH3
Phosphine is a compound of phosphorus
and hydrogen. The shape of a molecule of
phosphine is likely to be
H
N
C3H7
A
tetrahedral
B
pyramidal
C
bent
A
methylamine
D
linear.
B
butylamine
C
propylamine
D
methylpropylamine.
This amine is called
10. Solid ionic compounds do not conduct
electricity because
14. The structure of citric acid is
A
the ions are not free to move
B
the electrons are not free to move
C
solid substances never conduct electricity
D
there are no charged particles in ionic
compounds.
H
11. Which of the following alkanes will produce
3 moles of carbon dioxide when 1 mole of it is
completely burned?
A
Ethane
B
Propane
C
Butane
D
Pentane
B
Low viscosity and low flammability
C
High viscosity and high flammability
D
Low viscosity and high flammability
[X012/11/02]
COOH
HO
C
COOH
H
C
COOH
H
A
1
B
2
C
3
D
4
Which of the following properties apply
to a fraction containing large hydrocarbon
molecules?
High viscosity and low flammability
C
How many moles of sodium hydroxide would
be required to exactly neutralise one mole of
citric acid?
12. Fractional distillation of crude oil produces a
number of different fractions.
A
H
Page four
Process X
Ethene + Compound Y
15. C8H18
18. Which of the following plastics could be used to
make a soluble coating for a dishwasher tablet?
Which line in the table correctly identifies
Process X and Compound Y?
A
PVC
B
Biopol
C
Polystyrene
D
Poly(ethenol)
Process X
Compound Y
A
cracking
hexane
B
cracking
hexene
C
distillation
hexane
D
distillation
hexene
19. Which compound could be obtained by the
hydrolysis of a fat?
16. Polyethene terephthalate (PET) is used to
make plastic bottles which can easily be
recycled by heating and reshaping.
O
C
C
O
CH2
CH2
O
Ethanol
B
Glucose
C
Glycerol
D
Propanol
20. To which class of compounds does the hormone
insulin belong?
A section of the PET structure is shown.
O
A
O
O
A
Carbohydrates
C
C
B
Fats
C
Proteins
D
Hydrocarbons
Which line in the table best describes PET?
Type of polymer
Property
21. What is the most likely pH value that would be
obtained when zinc oxide is added to water?
A
addition
thermoplastic
B
condensation
thermosetting
(You may wish to use page 5 of the data booklet
to help you.)
A
5
C
addition
thermosetting
B
7
D
condensation
thermoplastic
C
9
D 11
17. Part of a polymer structure is shown.
CH3 H
C
C
CH3 H
CH3 H
C
C
C
22. Reactions can be represented using ionic
equations.
Which ionic equation shows a
neutralisation reaction?
C
A
H
CN H
CN H
CN
B
2H2O(l) + O2(g) + 4e–
4OH–(aq)
H+(aq) + OH–(aq)
H2O(l)
Which of the following gases could not be
produced when this polymer is burned?
C
SO2(g) + H2O(l)
2H+(aq) + SO32–(aq)
D
NH4+(s) + OH–(s)
NH3(g) + H2O(l)
A
CO
B
CO2
C
HCl
D
HCN
[X012/11/02]
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23. Four cells were made by joining copper, iron, magnesium and zinc to silver. The four cells produced the
following voltages 0·5 V, 0·9 V, 2·7 V and 1·1 V.
V
silver
V
copper
silver
iron
sodium nitrate
solution
V
silver
V
magnesium
silver
zinc
sodium nitrate
solution
Which of the following will be the voltage of the cell containing silver joined to copper?
(You may wish to use page 7 of the data booklet to help you.)
A
0·5 V
B
0·9 V
C
1·1 V
D
2·7 V
24. Which acidic gas is produced by the sparking
of air?
26. Which of the following substances is not a
salt?
A
Carbon dioxide
A
Copper sulphate
B
Sulphur dioxide
B
Sodium oxide
C
Nitrogen dioxide
C
Magnesium chloride
D
Hydrogen chloride
D
Calcium nitrate
25. A student adds a powder to dilute
hydrochloric acid. A gas which burns with a
pop is produced.
The powder could be
A
carbon
B
calcium oxide
C
sodium carbonate
D
zinc.
[X012/11/02]
Page six
27. In which of the following test tubes will a
reaction occur?
29. A metal can be extracted from its ore by
heating the ore with carbon but not by heating
the ore on its own.
The position of the metal in the reactivity
series is most likely to be between
A
(You may wish to use page 7 of the data
booklet to help you.)
magnesium
sulphate
solution
iron
B
sodium
carbonate
solution
A
zinc and magnesium
B
magnesium and potassium
C
zinc and copper
D
copper and gold.
iron
30. In which of the following experiments would
the iron nail not rust?
C
silver
nitrate
solution
A
iron
copper
iron nail
D
sodium chloride
solution
iron(II)
chloride
solution
28.
iron
B
tin
V
zinc
iron nail
copper
sodium chloride
solution
C
zinc
sulphate
solution
ion bridge
copper sulphate
solution
– +
power supply
iron rod
iron nail
Which line in the table is correct for the above
cell?
Zinc
electrode
Copper
electrode
A
mass increases
mass increases
B
mass increases
mass decreases
C
mass decreases
mass decreases
D
mass decreases
mass increases
sodium chloride
solution
D
iron rod
+ –
power supply
iron nail
sodium chloride
solution
Candidates are reminded that the answer sheet for Section A MUST be
placed INSIDE the front cover of this answer book.
[X012/11/02]
Page seven
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SECTION B
Marks
50 marks are available in this section of the paper.
All answers must be written clearly and legibly in ink.
1. Glass is made from the chemical silica, SiO2, which is covalently bonded and
has a melting point of 1700 °C.
(a) What does the melting point of silica suggest about its structure?
1
(b)
Antimony(III) oxide is added to reduce any bubbles that may appear
during the manufacturing process.
Write the chemical formula for antimony(III) oxide.
1
(c)In the manufacture of glass, other chemicals can be added to alter the
properties of the glass. The element boron can be added to glass to
make oven proof dishes.
(i) Information about an atom of boron is given in the table below.
Particle
Number
proton
5
electron
5
neutron
6
Use this information to complete the nuclide notation for this atom
of boron.
B
1
(ii)
Atoms of boron exist which have the same number of protons
but a different number of neutrons from that shown in the table.
What name can be used to describe the different atoms of boron?
1
(4)
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2. Rapid inflation of airbags in cars is caused by the production of nitrogen gas.
The graph gives information on the volume of gas produced over
30 microseconds.
Volume of nitrogen gas produced (litres)
50
40
30
20
10
0
0
5
10
15
20
25
30
Time (microseconds)
(a)
(i)Calculate the average rate of reaction between 2 and 10 microseconds.
litres per microsecond
1
(ii)At what time has half of the final volume of nitrogen gas been
produced?
microseconds
[X012/11/02]
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2. (continued)
(b)In some types of airbag, electrical energy causes sodium azide, NaN3, to
decompose producing sodium metal and nitrogen gas.
Write a formula equation for this reaction.
1
(c)Potassium nitrate is also present in the airbag to remove the sodium
metal by converting it into sodium oxide.
Why is it necessary to remove the sodium metal?
1
(4)
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3. In the PPA, “Effect of Concentration on Reaction Rate”, the reaction
between sodium persulphate and potassium iodide was investigated.
10 cm3 potassium
iodide solution
10 cm3 sodium
persulphate solution
+
1 cm3 starch solution
The results obtained during this PPA are shown in the table.
Experiment
Volume of sodium
persulphate (cm3)
Volume of
water (cm3)
Reaction time
(s)
1
10
0
126
2
8
162
3
6
210
4
4
336
(a)
Complete the results table to show the volumes of water used in
experiments 2, 3 and 4.
1
(b) How was the rate of reaction determined?
1
(c)Apart from using a timer, what allowed the accurate measurement of
reaction times?
1
(3)
[X012/11/02]
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4. Rhubarb contains oxalic acid, C2H2O4.
Oxalic acid reacts with acidified potassium permanganate solution and
decolourises it.
The equation for the reaction is:
2MnO4–(aq) + 5C2H2O4(aq) + 6H+(aq)
2Mn2+(aq) + 10CO2(g) + 8H2O(l)
(a)The reaction is catalysed by the Mn2+(aq) ions produced in the reaction.
Using information from the equation, what type of catalyst is Mn2+(aq)?
1
(b)A student investigated the effect of surface area on the rate of reaction
with acidified potassium permanganate solution.
acidified
potassium
permanganate
solution
acidified
potassium
permanganate
solution
6 cm strip
of rhubarb
6 cm strip of
rhubarb cut into
three sections
It was found that when the rhubarb was cut into three sections the
reaction was faster. Using collision theory, explain why cutting the
rhubarb into three sections increases the rate of reaction.
1
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4. (continued)
(c) A strip of rhubarb was found to contain 1·8 g of oxalic acid.
How many moles of oxalic acid, C2H2O4, are contained in 1·8 g.
(Formula mass of oxalic acid = 90)
moles
1
(3)
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5. The alkanals are a homologous series of compounds that all contain the
elements carbon, hydrogen and oxygen.
(a) What is meant by the term homologous series?
1
(b) The combustion of alkanals releases heat energy.
Name of alkanal
Heat energy released
when one mole burns (kJ)
methanal
510
ethanal
1056
propanal
1624
butanal
2304
(i)
Make a general statement linking the amount of heat energy
released and the number of carbon atoms in the alkanal molecules.
1
(ii)
Predict the amount of heat energy released, when 1 mole of
pentanal burns.
kJ
1
(3)
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6. Kevlar is a polymer which is used in the manufacture of body armour.
(a) What property of Kevlar makes it suitable for use in body armour?
1
(b) Kevlar is made from the following monomers.
H
H
N
H
O
O
C
N
H
Cl
C
Cl
(i)Draw the structure of the repeating unit formed from these two
monomers.
1
(ii) Name the type of link formed.
1
(3)
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7. Ethanol is a member of the alkanol family of compounds.
(a)Ethanol can be manufactured from ethene as shown in the following
addition reaction.
H H
C
H H
catalyst
C + H2O
H
C
H H
C
H
H OH
What other name can be given to this type of addition reaction?
1
(b)Ethanol can be used to make esters which can be used as flavourings for
food. The following ester is used to give ice cream a rum flavour.
H
H H
O
H
H
C
O C
C
C H
H
H
C
H H
Name this ester.
1
(c) Butan-2-ol is another member of the alkanol family.
H
H
H
H H
C
C
C
H
OH H H
C
H
Draw the full structural formula for an isomer of butan-2-ol.
1
(3)
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8. A student completed the PPA “Testing for Unsaturation”. Results from
the experiment are shown in the table.
Hydrocarbon
Molecular
Formula
Observation with
bromine solution
Saturated or
unsaturated
A
C6H14
no change
B
C6H12
unsaturated
C
C6H12
saturated
D
C6H10
bromine
decolourises
2
(a) Complete the table.
(b)
Care had to be taken when using bromine solution. Give a safety
precaution, other than eye protection, which should be taken when
completing this PPA.
1
(c) Suggest a possible name for hydrocarbon C.
1
(4)
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9. During digestion, molecules are broken down enabling them to pass through
the gut wall. Visking tubing can be used to model the gut wall.
water
visking tubing
starch in water
(a)
Describe how you could use iodine solution to show that starch
molecules are too large to pass through the visking tubing.
1
(b) Starch is hydrolysed by the enzyme amylase during digestion.
(i) What is produced when starch is hydrolysed?
1
(ii) Name another substance which can be used to hydrolyse starch.
1
(3)
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10.
The Dead Zone
In the summer of 2006, a 1000 square mile area of water at the bottom of
the Pacific Ocean was found to be covered in dead crabs.
Scientists investigating this found an increased level of chlorophyll at
the surface of the ocean and a zero level of oxygen at the bottom of the
ocean. The increase in chlorophyll was due to increased numbers of
plant plankton.
Scientists think that when plant plankton died they sank to the bottom of
the ocean where they were broken down by bacteria during respiration.
This used up all the oxygen from the water which resulted in the death of
the crabs.
As respiration also produces carbon dioxide, scientists are monitoring the
pH of the ocean water.
(a) What is the function of chlorophyll in plant plankton?
1
(b) Why is respiration essential to all living organisms?
1
(c) The pH of ocean water is normally around 8·2.
What effect will the carbon dioxide gas produced during respiration
have on the pH of the ocean water?
1
(3)
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11. Egg shells are made up mainly of calcium carbonate. A pupil carried out
an experiment to react egg shells with dilute hydrochloric acid. A gas was
produced.
(a)Complete the diagram to show the apparatus which could have been
used to measure the volume of gas produced.
(Additional paper, if required, can be found on Page twenty-eight.)
dilute
hydrochloric
acid
egg shells
1
(b) Name the salt produced in this reaction.
1
(c) The volume of gas produced during the reaction was measured.
Time (min)
Volume of gas (cm3)
0
0
2
47
4
92
6
114
8
118
10
118
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11. (c) (continued)
Plot these results as a line graph.
(Additional graph paper, if required, can be found on Page twenty-nine.)
2
(4)
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12. Three experiments were carried out to compare the pH and conductivity of
Marks
weak and strong acids.
0·01 mol l–1
hydrochloric acid
0·01 mol l–1
sulphuric acid
0·01 mol l–1
ethanoic acid
A
A
A
power
– supply +
power
– supply +
power
– supply +
(a)
The same gas was produced at the negative electrode in each
experiment.
Name the gas that was produced.
1
(b) Ethanoic acid is a weak acid.
What is meant by a weak acid?
1
(c)Circle the correct words in the table to show how the properties of the
sulphuric acid solution compare with the hydrochloric acid solution.
0·01 mol l–1
hydrochloric acid
solution
0·01 mol l–1
sulphuric acid solution
pH
2
lower
the same
higher
Current in a
conductivity cell
(microamps)
45
lower
the same
higher
1
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13. A student carried out the following experiment.
+
barium chloride
solution
sodium
chloride
solution
sodium sulphate
solution
barium sulphate
solid
(a) During the reaction a solid was formed.
Name the type of chemical reaction taking place.
1
(b) The equation for the reaction is
Ba2+(aq) + 2Cl–(aq) + 2Na+(aq) + SO42–(aq)
Ba2+ SO42–(s) + 2Cl–(aq) + 2Na+(aq)
(i) Rewrite the equation showing only the ions which react.
1
(ii) What term is used to describe the ions which do not react?
1
(3)
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14. Cutlery can be coated with silver to prevent corrosion and to make it look
attractive.
(a) What happens to atoms of a metal during corrosion?
1
(b) Electroplating is a process used to coat the cutlery with silver.
This diagram shows how this can be carried out.
+
power
supply
–
spoon
silver
silver(I)
nitrate
solution
(i)Write the ion-electron equation for the reaction taking place at the
positive electrode.
(You may wish to use page 7 of the data booklet to help you.)
1
(ii)Why must the cutlery be attached to the negative terminal of the
power supply?
1
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Page twenty-six
15. Rust, iron(III) oxide, that forms on cars can be treated using rust remover
Marks
which contains phosphoric acid.
When painted on, rust remover changes iron(III) oxide into iron(III) phosphate.
Fe2O3
+
2H3PO4
2FePO4
+
3H2O
(a) The rust remover contains 250 cm3 of 2 mol l–1 phosphoric acid.
(i)
Calculate the number of moles of phosphoric acid in the rust
remover.
mol
1
(ii)Using your answer in part (i), calculate the mass of iron(III) oxide
that will be removed by 250 cm3 of 2 mol l–1 phosphoric acid.
grams
2
(b)The iron(III) phosphate forms an insoluble coating which can be left on
to protect the metal from further corrosion.
How does the iron(III) phosphate protect the iron from further
corrosion?
[END OF QUESTION PAPER]
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ADDITIONAL SPACE FOR ANSWERS
ADDITIONAL PAPER FOR QUESTION 11(a)
dilute
hydrochloric
acid
egg shells
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ADDITIONAL SPACE FOR ANSWERS
ADDITIONAL GRAPH PAPER FOR QUESTION 11(c)
[X012/11/02]
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ADDITIONAL SPACE FOR ANSWERS
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FOR OFFICIAL USE
Section B
Total
Marks
X012/201
NATIONAL
QUALIFICATIONS
2011
THURSDAY, 26 MAY
1.00 PM – 3.00 PM
CHEMISTRY
INTERMEDIATE 2
Fill in these boxes and read what is printed below.
Full name of centre
Town
Forename(s)
Surname
Date of birth
Day
Month
Year
Scottish candidate number
Number of seat
Necessary data will be found in the Chemistry Data Booklet for Standard Grade and
Intermediate 2.
Section A – Questions 1–30 (30 marks)
Instructions for completion of Section A are given on page two.
For this section of the examination you must use an HB pencil.
Section B (50 marks)
All questions should be attempted.
The questions may be answered in any order but all answers are to be written in the spaces
provided in this answer book, and must be written clearly and legibly in ink.
Rough work, if any should be necessary, should be written in this book, and then scored
through when the fair copy has been written. If further space is required, a supplementary
sheet for rough work may be obtained from the Invigilator.
Additional space for answers will be found at the end of the book. If further space is required,
supplementary sheets may be obtained from the Invigilator and should be inserted inside the
front cover of this booklet.
Before leaving the examination room you must give this book to the Invigilator. If you do not,
you may lose all the marks for this paper.
S A X012/201 6 / 1 0 2 1 0
*X012/201*
©
Read carefully
1 Check that the answer sheet provided is for Chemistry Intermediate 2 (Section A).
2 For this section of the examination you must use an HB pencil and, where necessary, an eraser.
3 Check that the answer sheet you have been given has your name, date of birth, SCN (Scottish
Candidate Number) and Centre Name printed on it.
Do not change any of these details.
4 If any of this information is wrong, tell the Invigilator immediately.
5 If this information is correct, print your name and seat number in the boxes provided.
6 The answer to each question is either A, B, C or D. Decide what your answer is, then, using
your pencil, put a horizontal line in the space provided (see sample question below).
7 There is only one correct answer to each question.
8 Any rough working should be done on the question paper or the rough working sheet, not on
your answer sheet.
9 At the end of the examination, put the answer sheet for Section A inside the front cover of
this answer book.
Sample Question
To show that the ink in a ball-pen consists of a mixture of dyes, the method of separation would be
A chromatography
B fractional distillation
C fractional crystallisation
D filtration.
The correct answer is A—chromatography. The answer A has been clearly marked in pencil with a
horizontal line (see below).
A
B
C
D
Changing an answer
If you decide to change your answer, carefully erase your first answer and using your pencil, fill in the
answer you want. The answer below has been changed to D.
A
[ X012/201]
B
C
D
Page two
SECTION A
1. Which of the following compounds contains
both a transition metal ion and a halide ion?
A
Aluminium bromide
B
Cobalt chloride
C
Iron oxide
D
Sodium fluoride
4. Which line in the table describes a neutron?
2. Which of the following compounds contains
only two elements?
A
Magnesium hydroxide
B
Magnesium phosphate
C
Magnesium sulphite
D
Magnesium nitride
Mass
Charge
A
1
–1
B
negligible
0
C
1
+1
D
1
0
5. An atom has 26 protons, 26 electrons and
30 neutrons. The atom has
3. A student investigated the reaction between
marble chips and excess dilute hydrochloric
acid.
A
atomic number 26, mass number 56
B
atomic number 56, mass number 30
C
atomic number 30, mass number 26
D
atomic number 52, mass number 56.
6. Excess magnesium is burned in an enclosed
volume of air.
.
Which line in the table best describes the gas
after burning is complete?
Oxygen
excess dilute
hydrochloric acid
marble chips
Nitrogen Carbon dioxide
A
1%
98%
0·03%
B
1%
79%
19%
C
16%
79%
4%
D
20%
79%
0·03%
Which of the following would not affect the
rate of the reaction?
A
Increasing the volume of the acid
B
Decreasing the size of the marble chips
C
Decreasing the concentration of the acid
D
Increasing the temperature of the acid
7. Copper is a good conductor of electricity
because
A
the atoms are free to vibrate
B
the atoms are in close contact
C
the atoms have the electron arrangement
2, 8, 18, 1
D
electrons can move readily from one
atom to the next.
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8. What is the charge on the chromium ion in
CrCl3?
A
1+
B
1–
C
3+
D
3–
12. Which of the following compounds belongs to
the same homologous series as the compound
with the molecular formula C3H8?
A
H
H
H
C
C
H
H
C
C
H
H
H
9. What name is given to the reaction shown by
the following equation?
C6H12O6 + 6O2 → 6CO2 + 6H2O
A
Combustion
B
Condensation
C
Dehydration
D
Hydrolysis
B
H
H
H
C
C
C
C
H
H
H
H
H
C
H
10. The fractional distillation of crude oil
depends on the fact that different
hydrocarbons have different
A
densities
B
solubilities
C
boiling points
D
ignition temperatures.
H
CH4
B
C3H8
C
C8H18
D
C14H30
H
H
C
C
C
C
H
H
H
H
H
H
H
H
A
C
H
D
11. Which of the following molecules would most
likely be present in petrol?
H
H
H
H
C
C
H
H
13.
H
C
H
C
C
H
H
H
H
H
C
C
C
C
C
H
H
H
H
H
The name of the above compound is
[ X012/201]
Page four
A
but-2-ene
B
pent-2-ene
C
but-3-ene
D
pent-3-ene.
H
14. When propene undergoes an addition reaction with hydrogen bromide, two products are formed.
H
H
H
C
C
C
H
H
H
H + H
H
H
Br
C
C
C
H
H
H
H
Br
H
C
C
C
H
H
H
H
Br
H
H
Which of the following alkenes will also produce two products when it undergoes an addition reaction
with hydrogen bromide?
A
Ethene
B
But-1-ene
C
But-2-ene
D
Hex-3-ene
15. The table shows the result of heating two compounds with acidified potassium dichromate solution.
Acidified potassium
dichromate solution
Compound
H
H
H
H
O
H
C
C
C
C
H
H
H
H
H
O
C
C
C
C
H
H
H
H
stays orange
H
turns green
H
Which of the following compounds will not turn acidified potassium dichromate solution green?
A
H
H
O
H
C
C
C
H
B
H
C
H
H
H
H
H
O
C
C
C
H
H
H
O
C
C
H
H
H
D
O
H
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C
H
Page five
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16.
C6H12O6
20. When one molecule of fat is completely
hydrolysed, the number of ester links broken
is
C12H22O11
The above compounds are
A
isomers
B
hydrocarbons
C
alkanols
D
carbohydrates.
17. What functional group is always found in a
protein molecule?
N
H
B
C
C
D
1
B
2
C
3
D
4.
21. Which of the following oxides dissolves in
water to produce a solution with a pH greater
than 7?
H
A
A
A
Na2O
B
Al2O3
C
SO2
D
Ag2O
C
O
H
C
N
22. Which line in the table describes what
happens to a dilute solution of hydrochloric
acid when water is added to it?
pH
H+(aq)
concentration
A
increases
increases
B
increases
decreases
C
decreases
increases
D
decreases
decreases
O
C
O
C
18. Which of the following are polymers?
A
Plant sugars
B
Animal fats
C
Marine oils
D
Vegetable proteins
23. Which of the following solutions has the
highest pH?
19. Fats and oils are essential in the diet.
Which line in the table best describes an oil?
Degree of
unsaturation
Melting point
A
high
relatively high
B
high
relatively low
C
low
relatively high
D
low
relatively low
[ X012/201]
A
0·1 mol l–1 ammonia
B
–1
0·1 mol l hydrochloric acid
C
–1
0·1 mol l sodium chloride
D
–1
0·1 mol l sodium hydroxide
24. Which of the following pairs of chemicals
react to produce a gas that turns lime water
milky?
Page six
A
Calcium carbonate and dilute
hydrochloric acid
B
Copper oxide and dilute sulphuric acid
C
Copper and dilute hydrochloric acid
D
Magnesium and dilute sulphuric acid
25. H+(aq) + NO3–(aq) + K+(aq) + OH–(aq)
–
K+(aq) + NO3 (aq) + H2O
The spectator ions in the reaction are
A
+
+
H (aq) and K (aq)
B
–
NO3 (aq) and OH (aq)
C
+
–
H (aq) and OH (aq)
D
+
K (aq) and NO3 (aq).
–
–
26. Which of the following metals would react
with zinc chloride solution?
28. Some metals can be obtained from their metal
oxides by heat alone.
(You may wish to use page 7 of the data booklet
to help you.)
Which of the following oxides would produce
a metal when heated?
A
Copper
A
Calcium oxide
B
Gold
B
Copper oxide
C
Iron
C
Zinc oxide
D
Magnesium
D
Silver oxide
27.
29. For iron to rust
Reaction with
Metal
Dilute acid
Water
X
reacts
no reaction
Y
no reaction
no reaction
Z
reacts
reacts
A
only water must be present
B
only oxygen must be present
C
both water and oxygen must be present
D
oxygen, water and salt must be present.
30. The coatings on four strips of iron were
scratched to expose the iron. The strips were
placed in salt solution.
Which of the following shows the metals in
order of increasing reactivity?
A
XYZ
B
YXZ
C
ZXY
D
ZYX
plastic
coated
iron strip
zinc
coated
iron strip
tin coated
iron strip
painted
iron strip
Which iron strip would have rusted most
quickly?
A
Plastic coated
B
Zinc coated
C
Tin coated
D
Painted
Candidates are reminded that the answer sheet for Section A MUST be
placed INSIDE the front cover of this answer book.
[ X012/201]
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Marks
SECTION B
50 marks are available in this section of the paper.
All answers must be written clearly and legibly in ink.
1.
The properties of a substance depend on its type of bonding and structure.
There are four types of bonding and structure.
Discrete covalent
molecular
Covalent
network
Ionic
lattice
Metallic
lattice
(a) Complete the table to match up each type of bonding and structure
with its properties.
Bonding and structure type
Properties
do not conduct electricity and have
high melting points
have high melting points and
conduct electricity when liquid but
not when solid
conduct electricity when solid and
have a wide range of melting points
do not conduct electricity and have
low melting points
2
(b) A section of a covalent network compound is shown below.
= silicon
= oxygen
Write the formula for this covalent network compound.
1
(3)
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2.
Information on some two-element molecules is shown in the table.
Name
Formula
hydrogen fluoride
HF
water
H2O
ammonia
NH3
Shape of molecule
(a) Complete the table to show the shape of a molecule of ammonia.
1
(b) The hydrogen fluoride molecule can be represented as:
H
F
Showing all outer electrons, draw a similar diagram to represent a
molecule of water, H2O.
1
(2)
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3.
Hydrogen peroxide is a useful bleaching agent and is contained in many
hair dyes. Over time, the hair dye becomes less effective as the hydrogen
peroxide decomposes forming water and oxygen.
The equation for the decomposition of hydrogen peroxide is:
H2O2(aq)
O2(g) +
H2O()
1
(a) Balance this equation.
(b) The above reaction is often used to make oxygen in the laboratory.
To speed up the reaction, the catalyst manganese dioxide is added.
Complete the diagram to show how the oxygen can be collected.
hydrogen
peroxide
manganese
dioxide
1
(c) State the test for oxygen gas.
1
(d) When 34 g of hydrogen peroxide decomposes, 12 litres of oxygen is
produced.
Calculate the volume of oxygen produced when 1·7 g of hydrogen
peroxide decomposes.
litres
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4.
Research is being carried out into making chemicals that can be used to
help relieve the side effects of chemotherapy.
Part of the process is shown.
catalyst
chemical A + hydrogen
(a)
chemical B
(i) This reaction is catalysed using the homogeneous catalyst,
ruthenium(II) chloride.
What is meant by a homogeneous catalyst?
1
(ii) Write the formula for ruthenium(II) chloride.
1
(b) As the reaction proceeds the hydrogen is used up and the pressure
decreases.
Time
(min)
0
5
10
15
20
30
35
45
Decrease in
pressure
(bar)
0
0·6
1·2
1·7
2·2
2·9
3·1
3·1
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4.
(b) (continued)
(i) Draw a line graph showing the decrease in pressure as time
proceeds.
(Additional graph paper, if
Page twenty-six.)
required, will be found on
2
(ii) Using your graph, at what time did the reaction finish?
min
1
(iii) Calculate the average rate of the reaction, in bar min−1, between
10 and 20 minutes.
bar min−1
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5.
Ammonium sulphate is a commonly used fertiliser. It can be produced by
the reaction between ammonium carbonate and calcium sulphate.
(NH4)2CO3(aq) + CaSO4(aq)
(NH4)2SO4(aq) + CaCO3(s)
(a) Name this type of chemical reaction.
1
(b) What mass of ammonium carbonate, (NH4)2CO3, would be needed to
make 13·2 kg of ammonium sulphate, (NH4)2SO4?
kg
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2
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6.
In the PPA “Hydrolysis of starch”, dilute hydrochloric acid can be used
to break down starch.
A section of a student’s workcard is shown.
1.
Set up the experiment as shown in the diagram.
water
10 cm3 starch solution
+ 1 cm3 dilute
hydrochloric acid
2.
Boil the water in the beaker for 5 minutes and then turn
off the Bunsen burner.
3.
Add a small amount of solid sodium hydrogencarbonate to
the test tube.
4.
Add 5 cm3 of Benedict’s solution to the test tube and
warm gently.
5.
Observe and record your results.
(a) After heating with dilute hydrochloric acid,
hydrogencarbonate is added to the reaction mixture.
solid
sodium
Why is sodium hydrogencarbonate needed?
1
(b) A control experiment is used in this PPA.
Label the diagram to show this control experiment.
1
(2)
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7.
When marking a student’s report on plastics, the teacher circled three
errors.
The marked report is shown.
Most plastics are made from chemicals which come from
1
coal.
Plastics are made when monomers polymerise to form
polymers.
Some common plastics are polystyrene, poly(ethene) and
Biopol:
• Polystyrene is made from the monomer 2propene
• Poly(ethene) is a thermoplastic
•
3
Biopol is a plastic which is soluble in water.
Correct the circled errors.
1
2
(3)
3
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8.
Many different gases are found in car exhaust fumes. Some of these gases
are produced by the combustion of petrol in car engines.
The pie chart shows the gases present in the exhaust fumes of a car.
oxygen
4 % nitrogen oxides
carbon dioxide
3%
8%
water vapour
9%
carbon
monoxide
5%
nitrogen
71 %
(a) What evidence in the pie chart shows that incomplete combustion of
petrol has taken place?
1
(b) The car’s exhaust fumes were found to contain 3 % nitrogen oxides.
Predict the percentage of nitrogen oxides that could be found in the
exhaust fumes if the car was fitted with a catalytic convertor.
%
1
(c) The burning of some fuels releases sulphur dioxide into the
atmosphere.
Why is this a problem?
1
(3)
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9.
The little pen-tailed tree shrew, found in
the jungles of West Malaysia, feeds on
nectar from the Bertam palm tree. This
nectar contains glucose which ferments,
producing solutions of up to 3·8 % alcohol.
Therefore, the tree shrew regularly drinks
a solution which is equivalent to a man
drinking 9 units of alcohol per day. It
seems that the tree shrew never gets drunk
because it is able to breakdown the alcohol
much quicker than humans can.
(a) Name the process by which plants make glucose from carbon dioxide
and water.
1
(b) What type of substance must be present in the nectar to allow the
fermentation of glucose to take place?
1
(c) The alcohol produced is ethanol.
Draw the shortened structural formula for ethanol.
1
(d) Using information in the passage above, calculate the volume of
alcohol solution the tree shrew drinks each day.
Volume of alcohol solution =
units of alcohol × 1·25
% of alcohol
cm3
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10.
Marks
Synthetic nappies contain hydrogel polymers which attract and absorb
water molecules.
(a) The following is part of the structure of a hydrogel polymer.
H
COOH H
COOH H
COOH
C
C
C
C
C
C
H
H
H
H
H
H
(i) Draw the monomer from which this polymer is made.
1
(ii) The diagram below shows how water molecules are attracted to
the hydrogel.
H
H
O
H
H
O
C
H
O
H
H
O
H
O
O
C
H
O
O
C
O
hydrogel
backbone
What type of bonding must be present in the water molecules,
which allows them to be attracted to the hydrogel?
1
(b) Many hydrogels are polymers of carboxylic acids. Carboxylic acids are
weak acids.
What is meant by a weak acid?
1
(3)
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11.
Many different molecules give us different smells and tastes.
(a) The following molecule gives a “fishy” smell.
H
H
H
H
H
C
C
C
C
H
N
H
H
H
H
H
Name the functional group circled in this molecule.
1
(b) Artificial flavourings added to foods are often esters.
The following ester gives an orange flavour.
H
H
O
C
C
O
H
H
H
H
H
H
H
H
H
C
C
C
C
C
C
C
C
H
H
H
H
H
H
H
H
H
Name this ester.
1
(c) Some household cleaners contain the chemical limonene which gives
them a lemon smell. The structure of limonene is shown below.
CH3
C
H2C
CH
H2C
CH2
C
H
C
CH3
CH2
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11.
Marks
(c) (continued)
Using bromine solution, a student carried out titrations to determine
the concentration of limonene in a household cleaner.
0·50 mol l–1 bromine solution
(orange/red)
Flask
20·0 cm3 household cleaner
(colourless)
Titration
Initial burette
reading (cm3)
Final burette
reading (cm3)
Titre (cm3)
1
2
3
0·5
0·2
0·1
17·1
16·3
16·0
16·6
16·1
15·9
(i) What colour change would be seen in the flask that indicates the
end point of the titrations?
1
to
(ii) What average volume should be used in calculating the
concentration of limonene?
cm3
1
(iii) The equation for the reaction between limonene and bromine
solution is shown.
C10H16(aq) + 2Br2(aq)
C10H16Br4(aq)
Calculate the concentration of limonene in the household cleaner.
mol l–1
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12.
Metals can be extracted from metal compounds by heat alone, heating with
carbon or by electrolysis.
(a) Name the type of chemical reaction which takes place when a metal is
extracted from its compound.
1
(b) In a PPA, a solution of copper(II) chloride was electrolysed.
d.c. supply
carbon
electrode
carbon
electrode
brown
solid
bubbles of gas
copper(II) chloride solution
(i) Complete the table by adding the charge for each electrode.
Observation at
electrode
bubbles of gas
Observation at
electrode
brown solid formed
1
(ii) How could the gas be identified?
1
(3)
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13.
Some indicators can have different colours when in solutions of different
pH values.
The tables give information about two indicators, bromothymol blue and
methyl orange.
Methyl orange
Bromothymol blue
Colour
pH
Colour
pH
yellow
below 6·0
red
below 3·1
blue
above 7·6
yellow
above 4·4
The pH of three solutions was investigated using both indicators.
The results are shown below.
Substance
Colour with
bromothymol blue
Colour with
methyl orange
A
yellow
red
B
yellow
yellow
C
blue
yellow
(a) Which solution is alkaline?
Solution
1
(b) Suggest a pH value for solution B.
pH
1
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14.
The voltage obtained when different pairs of metal strips are connected in a
cell varies and this leads to the electrochemical series.
Using the apparatus below, a student investigated the electrochemical
series. Copper and four other metal strips were used in this investigation.
metal strip
voltmeter
filter paper
soaked in
electrolyte
V
copper strip
The results are shown.
Direction of
electron flow
Metal strip
Voltage (V)
1
0·6
metal 1 to copper
2
0·2
copper to metal 2
3
0·9
metal 3 to copper
4
0·1
copper to metal 4
(a) Which of the metals used is highest in the electrochemical series?
metal
1
(b) Which two of the metals used would produce the highest voltage when
connected in a cell?
metal
and metal
1
(c) What would be the reading on the voltmeter if both strips of metal
were copper?
V
1
(d) Why can glucose solution not be used as the electrolyte?
1
(4)
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15.
Fizzy drinks contain acids.
These acids can attack the compound calcium hydroxyapatite which is
found in tooth enamel.
The equation for the reaction is:
Ca10(PO4)6(OH)2(s) + 8H+(aq)
calcium hydroxyapatite
6CaHPO4(s) + 4Ca2+(aq) + 2 H2O()
(a) What will happen to the pH as the tooth enamel is attacked by the
acids?
1
(b) Fluoride prevents tooth decay by replacing the hydroxide ions of
calcium hydroxyapatite with fluoride ions to form hard wearing
calcium fluoroapatite.
calcium hydroxyapatite
Ca10(PO4)6(OH)2
fluoride ions
calcium fluoroapatite
Write the formula for calcium fluoroapatite.
1
(2)
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