Production of Materials HSC Questions
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2001
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2002
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2003
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2004
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2005
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2006
C
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2007
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2008
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2009
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2010
B
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2011
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2006
9.2.1.2.2
2008
1 Which is the main industrial source of ethylene?
(A) Ethanol
(B) Glucose
(C) Petroleum
(D) Polyethylene
Question 16 The process of fractional distillation is used to separate crude oil into different
fractions. One of the compounds obtained from fractional distillation is C10H22
This compound undergoes catalytic cracking as follows:
9.2.1.2.2
(a) Complete the table below to identify the products and the homologous series to which they
belong. (2 marks)
(b) Using examples from your first-hand investigation, explain how you distinguished between
9.2.1.3.2 these two series of compounds. Include a relevant equation in your answer.
(3 marks)
9.1.13.1d
2010
Question 24
In the margarine industry, alkenes are often hydrogenated to convert unsaturated oils into solid
fats that have a greater proportion of saturated molecules.
9.2.1.2.3
(a) Using ethene as an example, write an equation for this reaction and state the type of reaction
this represents. (2 marks)
9.2.1.3.2
(b) Describe a test that could be used to confirm that all the ethene has been converted. (2
marks)
2004
Question 17
The structures of two commercially significant monomers are shown.
9.2.1.2.7
(a) Identify the common name of ONE of the monomers. (1 mark)
9.2.1.2.8
(b) The uses of polymers are dependent on their properties.
Discuss this statement with reference to a polymer made from one of the above monomers. (3
marks)
9.2.1.2.7
2010
(c) Draw the structure of a polymer made from one of the above monomers. (1 mark)
6 The diagram shows a section of a polymer.
9.2.1.2.7
2005
What is the systematic name of the monomer?
(A) Polybenzene
(B) Benzylethene
(C) Ethylbenzene
(D) Ethenylbenzene
Question 23
(b) Write a balanced equation for the incomplete combustion of methane. (1 mark)
9.2.1.3.1
9.2.1.2.1
2005
Question 24
An antacid tablet is known to contain calcium carbonate (CaCO3). To determine the mass of
calcium carbonate in the tablet, the following procedure was used.
• The tablet was crushed and then placed in a beaker.
• A pipette was used to add 25.0 mL of 0.600 mol L–1 hydrochloric acid to the crushed tablet in
the beaker.
• Once the reaction between the calcium carbonate and hydrochloric acid had stopped,
phenolphthalein indicator was added to the reaction mixture.
• A teflon-coated burette was then used to add 0.100 mol L–1 sodium hydroxide to the beaker to
neutralise the excess hydrochloric acid.
• The phenolphthalein changed from colourless to pink after 14.2 mL of the sodium hydroxide
solution had been added.
9.2.1.3.1
9.2.1.2.1
2005
(a) Write a balanced chemical equation for the reaction that occurred between the calcium
carbonate in the tablet and the hydrochloric acid.
(1 mark)
9.2.1.3.2
Question 16
During your practical work you performed a first-hand investigation to distinguish between an
alkene and the corresponding alkane.
(a) Name the alkene used in your investigation.
(1 mark)
9.2.1.3.2
(b) Identify a potential hazard in your investigation, and outline how you addressed this hazard.
(2 marks)
9.2.1.3.2
2009
(c) Outline the procedure you used for your first-hand investigation.
(2 marks)
6 Bromine, Br2, dissolves in unsaturated hydrocarbons and reacts immediately. Which of the
following is the best description of this process?
9.2.1.3.2
2007
9.2.1.3.3
9.2.1.2.8
9.2.1.2.7
9.2.1.2.6
2001
9.2.1
(A) Bromine is polar and reacts by adding bromine atoms across the double bond.
(B) Bromine is polar and reacts by substituting hydrogen atoms with bromine atoms.
(C) Bromine is non-polar and reacts by substituting hydrogen atoms with bromine atoms.
(D) Bromine is non-polar and reacts by adding bromine atoms across the double bond.
Question 26 (4 marks)
Explain how the structure and properties of polyethylene and polystyrene relate to the way each is
used.
1 Ethene may be converted into poly(ethene).
What type of reaction is this?
(A) Condensation
(B) Hydrolysis
(C) Oxidation/reduction
(D) Polymerisation
2001
3 Which equation best represents catalytic cracking of a petroleum fraction?
9.2.1
2003
11 Which polymer is made by the polymerisation of methyl methacrylate?
9.2.1
2002
9.2.1
Question 17 (3 marks)
Explain why alkanes and their corresponding alkenes have similar physical properties, but very
different chemical properties.
2002
9.2.1
9.2.1
9.2.1
2003
Question 16
You have carried out a first-hand investigation to compare the reactivity of an alkene with its
corresponding alkane.
(a) State the name of the alkene.
(1 mark)
(b) Outline a procedure to compare the reactivity of this alkene with its
corresponding alkane.
(2 marks)
(c) Describe the results obtained from this first-hand investigation and include relevant
chemical equations.
(3 marks)
Question 17
The flowchart shows the production of polyethylene.
9.2.1
9.2.1
(b) Describe Process Y.
(3 marks)
9.2.1
(c) A sample of polyethylene was produced by Process Y. The following graph shows the
distribution of molecular weights of polymer molecules in the sample.
Why is a range of molecular weights observed? (1 mark)
2003
Question 23 (4 marks)
25.0 mL of 0.12 mol L-1 standard barium hydroxide solution was titrated with nitric acid. The
results are recorded in the table.
9.2.1
(a) Write a balanced chemical equation for the reaction of barium hydroxide with nitric acid.
(1 mark)
2009
Question 19 (6 marks)
9.2.1
Outline the chemical and physical processes involved in the production of ONE of the following
from a natural raw material:
•
•
•
a polyethylene bottle
a polyvinyl chloride pipe
a polystyrene cup.
Include relevant chemical equations in your answer.
2005
4 Terylene (polyester) is a condensation polymer. Part of the structure of the polymer is shown.
9.2.2.2.3
What are the two monomers that form this polymer?
2006
9.2.2.2.3
9.1.12.4b
2010
9.2.2.2.3
6 Glucose (C6H12O6) is a monomer that can form naturally occurring polymers.
The approximate atomic weights for the elements which make up glucose are shown in
the table.
Using data from the table, what would be the approximate molecular weight of a polymer
made from 5 glucose monomers?
(A) 810
(B) 828
(C) 882
(D) 900
1 Water is released during a polymerisation reaction.
Which monomer is likely to have been involved in the reaction?
(A) Ethene
(B) Glucose
(C) Styrene
(D) Vinyl chloride
2007
2 What type of reaction describes the polymerisation of glucose into cellulose?
9.2.2.2.4
(A) Addition
(B) Hydrolysis
(C) Substitution
2010
9.2.2.2.4
9.2.2.2.3
9.2.2.2.2
9.2.1.2.6
9.2.1.2.5
9.1.14.3d
9.1.14.1f
(D) Condensation
Question 30
(a) Compare the process of polymerisation of ethylene and glucose. Include relevant chemical
equations in your answer. (3 marks)
(b) Explain the relationship between the structures and properties of THREE different polymers
(5 marks)
9.2.2.2.5 from ethylene and glucose, and their uses.
9.2.2.2.4
9.2.1.2.8
9.1.14.3d
2005
9.2.2.2.5
9.2.2.2.4
2005
9.2.2.3.1
9.2.2.2.1
2 Which of the following makes cellulose a potential raw material for the petrochemical
industry?
(A) It is available in many parts of the world.
(B) It is light in weight and easy to transport.
(C) It is an organic polymer based on carbon.
(D) It is a polymer that undergoes combustion.
Question 18 (4 marks)
Assess the impact of the recent development of a named biopolymer on society and
the environment.
2011
9.2.2.3.1
9.2.1.2.8
Question 27 (5 marks)
The following extract was taken from a blog about environmental issues.
… the use of long-lasting polymers for short-lived applications can cause
problems for the preservation of living systems… Plastic debris has a costly
impact on waste management for municipalities.
Assess the uses of polystyrene and a named biopolymer in terms of their properties, with
reference to the statements made in this blog.
2001
9.2.2
2001
9.2.2
2 Which of the following is a major component of biomass?
(A) Cellulose
(B) Ethanol
(C) Natural gas
(D) Oil
4 Cellulose is a linear polymer which is a basic structural component of plant cell walls.
Which is the correct representation of part of a cellulose polymer?
2002
Question 18
(a) Name the type of polymerisation shown in the following reaction: (1 mark)
9.2.2
(b) Assess current developments in the use of biopolymers. (5 marks)
9.2.2
2003
9.2.2
Question 20 (5 marks)
Assess the suitability of biomass as a future source of energy and chemicals for industry.
2009
Question 17 (4 marks)
9.2.3.2.3 Water and ethanol are both used as solvents.
9.1.14.1h Explain the differences and similarities in their solvent behaviour in terms of their molecular
9.1.14.1g structures. Include a diagram in your answer.
9.1.13.1e
2006
9.2.3.2.4
9.2.3.2.2
9.2.1.2.8
9.2.1.2.7
9.2.1.2.6
9.2.1.2.5
9.2.1.2.4
9.2.1.2.3
9.2.1.2.1
Question 20 (7 marks)
Analyse why ethylene is such an important starting material for the chemical industry.
In your answer, include relevant chemical equations, and a description of new materials and
fuels that can be prepared from ethylene.
2007
1 Which of the following is a renewable resource?
9.2.3.2.4
(A) Ethanol
(B) Uranium
(C) Petroleum
(D) Aluminium
2006
4 A student used the apparatus shown to determine the molar heat of combustion of
ethanol.
9.2.3.2.7
9.1.12.4b
The following results were obtained.
What is the molar heat of combustion calculated from this data?
(A) 22.4 kJ mol–1
(B) 25.7 kJ mol–1
(C) 1030 kJ mol–1
(D) 1180 kJ mol–1
2004
11 In gas chromatography, compounds may be separated based on their molecular weight.
The smaller the molecular weight the more quickly the compound is detected. A gas
9.2.3.2.9 chromatographic analysis was performed on a mixture of 1-hexanol, 1-octanol, 1-heptanol and
9.1.12.3c 1-pentanol. The results are shown in the diagram.
Which substance does peak X correspond to?
(A) 1-hexanol
(B) 1-octanol
(C) 1-heptanol
(D) 1-pentanol
2007
4 What is the IUPAC name for the following compound?
9.2.3.2.9
9.1.13.1d
2010
9.2.3.2.9
9.2.3.2.1
(A) Hexan-3-ol
(B) Hexan-4-ol
(C) Heptan-3-ol
(D) Heptan-5-ol
11 An organic liquid, when reacted with concentrated sulfuric acid, produces a compound
that decolourises bromine water.
What is the formula of the organic liquid?
(A) C6H12
(B) C6H14
(C) C6H11OH
(D) C5H11COOH
2011
9.2.3.2.9
9.2.3.2.7
−1
17 The molar heat of combustion of pentan-1-ol is 2800 kJ mol . A quantity of pentan-1-ol was
combusted, generating 108 kJ of heat.
What mass of pentan-1-ol was combusted?
(A) 2.29 g
(B) 2.86 g
(C) 3.32 g
2011
(D) 3.40 g
Question 21 (4 marks)
What features of the molecular structure of ethanol account for its extensive use as a solvent?
9.2.3.2.9
9.2.3.2.3
Include a diagram in your answer.
2011
1 Which of the following industrial processes is used to produce ethanol from ethylene?
9.2.3.3.1
9.2.3.2.2
(A) Hydration
(B) Dehydration
(C) Addition polymerisation
(D) Condensation polymerisation
2006
2 Catalysts are required for the production of both ethanol from ethylene and ethylene from
ethanol.
9.2.3.3.1
9.2.3.2.2
9.2.3.2.1
What are the identities of Catalyst A and Catalyst B?
2008
Question 22 (5 marks)
The following extract was taken from the website of a leading car manufacturer.
9.2.3.3.3
9.2.3.2.8
9.2.3.2.4
Critically evaluate the extract with reference to ethanol being a ‘carbon-neutral’ fuel. Support
your answer with relevant chemical equations.
2009
13 In a fermentation experiment 6.50 g of glucose was completely converted to ethanol and carbon
dioxide.
9.2.3.3.5
9.2.3.2.6 What is the mass of carbon dioxide produced?
9.1.12.4b
(A) 1.59 g
(B) 3.18 g
(C) 9.53 g
(D) 13.0 g
2006
Question 18
A student studying the mass change that occurs during fermentation added glucose, water and
yeast to a flask and stoppered the flask with some cotton wool.
The student measured the mass of the flask daily for seven days. The table shows the data
collected.
9.2.3.3.4 (a) Calculate the moles of CO2 released between days 1 and 7. (1 mark)
9.1.12.4b
9.2.3.3.5
9.2.3.3.4 (b) Calculate the mass of glucose that underwent fermentation between days 1 and 7. Include a
9.2.3.2.6 balanced chemical equation in your answer. (3 marks)
9.1.12.4b
2010
15 What mass of ethanol is obtained when 5.68 g of carbon dioxide is produced during
fermentation, at 25°C and 100 kPa?
9.2.3.3.5
9.2.3.3.4 (A) 2.95 g
9.1.14.1d (B) 5.95 g
2011
9.2.3.3.5
9.2.3.3.4
9.2.3.2.6
9.2.3.2.5
(C) 33.6 g
(D) 147.2 g
2 Which of the following shows two products that result from the fermentation of glucose?
(A) Cellulose and water
(B) Ethanol and oxygen
(C) Carbon dioxide and water
2005
(D) Ethanol and carbon dioxide
3 The heat of combustion of butan-1-ol is 2676 kJ mol-1.
9.2.3.3.6
What is the value of the heat of combustion in kJ g1?
(A) 30.41
(B) 36.10
(C) 44.60
(D) 47.79
2008
Question 24 The table shows four fuels and their various properties.
9.2.3.2.8
9.2.3.2.7
9.1.12.4b
9.1.12.3c
9.2.3.3.3
9.1.12.4b
9.1.12.3c
(a) Which fuel provides the greatest amount of energy per gram? (1 mark)
9.3.2.3.9
9.1.12.4b
9.1.12.3c
(b) A car has an 80 L petrol tank. Calculate the energy released by the complete combustion of
one full tank of petrol. (2 marks)
(c) How many litres of hydrogen gas at 25°C and 100 kPa would be needed to supply the same
amount of energy as 80 L of petrol? (2 marks)
2004
13 A student used the apparatus below to determine the molar heat of combustion of
propanol.
9.2.3.3.6
9.2.3.2.9
The following results were obtained:
Mass of 1-propanol burnt = 0.60 g
Mass of water heated = 200 g
Initial temperature of water = 21.0°C
The molar heat of combustion of 1-propanol is 2021 kJ mol−1. Assuming no heat loss,
what would be the final temperature of the water?
(A) 24.2°C
(B) 29.1°C
(C) 45.2°C
(D) 48.4°C
2005
Question 17
The heat of combustion of ethanol is 1367 kJ mol–1. In a first-hand investigation to determine
the heat of combustion of ethanol, the experimental value determined differed from the
theoretical value.
9.2.3.3.6
9.2.3.2.7
(a) Identify a reason for this difference.
(1 mark)
(b) Calculate the theoretical mass of ethanol required to heat 200 mL of water from 21.0°C to
45.0°C. (2 marks)
9.2.3.3.6
9.2.3.2.7
2007
Question 24 The heats of combustion (–ΔHc) of three alkanols were determined.
The results are shown in the table.
9.2.3.3.6
9.1.13.1g
9.1.13.1f
9.1.12.4b
9.1.12.3c
(a) Plot a graph of the heat of combustion versus the molecular weight for the three alkanols.
(3 marks)
(b) (i) Use the graph to estimate the heat of combustion of propan-1-ol.
9.2.3.3.6
9.1.13.1d
9.1.12.3c
(1 mark)
2008
6 What is the specific heat of a compound?
9.2.3.3.6
(A) The quantity of heat required to boil 1 g of the compound
(B) The quantity of heat required to melt 1 g of the compound
(C) The quantity of heat required to increase the temperature of the compound by 1°C
(D) The quantity of heat required to increase the temperature of 1 g of the compound by 1°C
2008
–1
10 The molar heat of combustion of ethanol is 1367 kJ mol .
9.2.3.3.6
What quantity of ethanol must be combusted to raise the temperature of 1.0 kg water from 50°C to
9.2.3.2.9
boiling point at sea level (assuming no loss of heat to the surroundings)?
9.1.12.4b
(A) 6.5 g
(B) 7.0 g
(C) 209 g
2009
(D) 300 g
5 The apparatus shown is used in a first-hand investigation to determine and compare the heat
of combustion of three different liquid alkanols.
9.2.3.3.6
9.1.11.2a
Which is the independent variable?
(A) Type of alkanol used
(B) Amount of water used
(C) Amount of alkanol used
2009
(D) Temperature change in the water
Question 20
(a) Calculate the mass of ethanol that must be burnt to increase the temperature of 210 g of water by
9.2.3.3.6 65°C, if exactly half of the heat released by this combustion is lost to the surroundings. The heat of
9.2.3.2.7 combustion of ethanol is 1367 kJ mol−1. (3 marks)
9.1.12.4b
9.2.3.3.6
9.1.11.3a (b) What are TWO ways to limit heat loss from the apparatus when performing a first-hand
9.1.11.2e investigation to determine and compare heat of combustion of different liquid alkanols? (1 mark)
9.1.11.2d
9.1.11.2c
2010
Question 23 (3 marks)
(a) Write a balanced chemical equation for the complete combustion of 1-butanol. (1 mark)
9.2.3.3.6
9.2.3.3.6 (b) A student measured the heat of combustion of three different fuels. The results
9.1.12.4b are shown in the table. (2 marks)
The published value for the heat of combustion of 1-butanol is 2676 kJ mol. Which fuel from
the table is likely to be 1-butanol? Justify your answer.
2001
Question 17
Students were asked to perform a first-hand investigation to determine the molar heat of
combustion of ethanol.
The following extract is from the practical report of one student.
Lab data:
Mass of water 250.0 g
Initial mass of burner 221.4 g
Final mass of burner 219.1 g
Initial temperature of water 19.0°C
Final temperature of water 59.0°C
9.2.3
(a) After completing the calculations correctly, the student found that the answer did not agree
with the value found in data books. Suggest ONE reason for this.
(1 mark)
9.2.3
(b) Propose TWO adjustments that could be made to the apparatus or experimental
method to improve the accuracy of the results. (2 marks)
9.2.3
(c) Calculate the molar heat of combustion of ethanol, using the student’s data. (3 marks)
2002
1 Which conditions would be best for the fermentation of sugars by yeast?
9.2.3
(A) Low oxygen concentration and a temperature between 25°C and 35°C
(B) High oxygen concentration and a temperature between 25°C and 35°C
(C) Low oxygen concentration and a temperature between 45°C and 60°C
(D) High oxygen concentration and a temperature between 45°C and 60°C
2 What is the catalyst for the conversion of ethanol to ethene?
2002
9.2.3
2003
(A) NaOH
(B) H2SO4
(C) HNO3
(D) Pt
6 The table gives the heat of combustion in kJ g for a number of different fuels.
9.2.3
9.1
The heat of combustion in kJ mol-1 for one of the fuels was calculated as 2016 kJ mol-1. What
was the fuel?
2003
9.2.3
9.2.1
(A) Methanol
(B) Ethanol
(C) Propanol
(D) Petrol
Question 22
(a) Write a balanced chemical equation for the complete combustion of ethanol.
(1 mark)
2003
9.2.3
9.1
Question 16
You performed a first-hand investigation that monitored mass changes during the fermentation
of glucose to ethanol.
(a) Outline the procedure you used.
(2 marks)
9.2.3
9.1
(b) Write a balanced chemical equation for this reaction.
Question 17
The flowchart shows the production of polyethylene.
(a) Identify Compound X.
2004
(1 mark)
(1 marks)
Question 19 (6 marks)
The following experiment was performed to investigate the relative activity of metals.
The beaker initially contained 250.0 mL of 0.050 mol L-1 copper sulfate solution.
After several hours the dark blue colour of the solution had become lighter and a
red-brown deposit had formed on the piece of zinc metal.
9.2.4.2.1
(a) Account for the changes observed. Provide a balanced oxidation–reduction equation in your
answer. (3 marks)
The red-brown deposit was removed from the piece of zinc metal and dried. It was
found to weigh 0.325 g.
9.2.4.2.1 (b) Calculate the concentration of copper sulfate solution remaining in the beaker. (3 marks)
9.1.13.1d
2009
9 One test used for random breath testing in NSW involved crystals of potassium dichromate
reacting with ethanol. In this reaction the orange dichromate ion, Cr2O72−, changes to the green
chromium ion, Cr3+. Which statement is true for this reaction?
9.2.4.2.3
9.1.12.4b
9.1.12.3c (A) Chromium has lost electrons and reached a lower oxidation state.
(B) Chromium has lost electrons and reached a higher oxidation state.
(C) Chromium has gained electrons and reached a lower oxidation state.
(D) Chromium has gained electrons and reached a higher oxidation state.
2010
12 In which of the following reactions does the metal atom show the greatest change in
oxidation state?
9.2.4.2.3 (A) MnO4 to Mn2
9.1.12.4b (B) MnO2 to Mn(OH)3
(C) PbO2 to PbSO4
(D) VO2to VO2
2008
13 Some reactions of the metals Q, R and S are given below.
9.2.4.2.4
9.2.4.2.2
9.1.12.3c
+
+
+
In a galvanic cell, Q , R and S would represent cations of these metals. Which galvanic cell
will produce the greatest voltage?
2011
Question 24 A galvanic cell was constructed as shown in the diagram.
(b) After a period of time, a solid deposit that had formed on the copper electrode was removed
and dried. The deposit had a mass of 0.395 g.
9.2.4.2.4
9.2.4.2.1
(i) Calculate the final mass of the nickel electrode.
9.2.4.2.4
9.2.4.2.1
(ii) Calculate the final concentration of the nickel(II) nitrate solution.
(3 marks)
(2 marks)
2010
Question 27 (2 marks)
The diagram shows a particular cell with relevant half equations.
9.2.4.2.6
9.2.4.2.4
Zn(s) + 2OH(aq) →ZnO(s) + H2O(l) + 2e

HgO(s) + H2O(l) + 2e→Hg(l) + 2OH(aq)
Identify the anode, cathode and electrolyte for this cell.
2009
Question 26 An electrochemical cell is constructed using two half cells. One half cell consists
2+
9.2.4.2.6
9.2.4.2.5
9.1.13.1e
3+
of an inert platinum electrode and a solution of Fe and Fe . The other half cell consists of a
2+
lead electrode and a solution of Pb .
Current will flow from one electrode to the other electrode when the cell is completed using a
voltmeter and a salt bridge.
(c) Identify the anode, cathode, metals and ions by labelling the following diagram. (3 marks)
2010
13 The diagram shows a galvanic cell.
9.2.4.2.6
9.2.4.2.4
Which of the following metals (M) acting as an anode would produce the lowest
theoretical potential for the cell?
(A) Calcium
(B) Copper
(C) Iron
(D) Manganese
2005
5 An electrochemical cell is set up as shown in the diagram.
9.2.4.3.1
9.2.4.2.5
9.2.4.2.2
9.2.4.2.1
What are two observations for this electrochemical cell?
2004
14 Four metals Pb, x, y and z, were connected in pairs and the voltage was recorded.
9.2.4.3.2
9.2.4.2.2
The results obtained are set out in the table below.
What is the order of increasing ease of oxidation of the metals?
(A) z, y, Pb, x
(B) Pb, x, y, z
(C) x, y, Pb, z
(D) x, Pb, y, z
2007
3 In a galvanic cell, what is the pathway of electron flow?
9.2.4.2.5
2006
Question 19 A student was asked to perform a first-hand investigation to measure the
difference in potential of various combinations of metals in an electrolyte solution. The student
was provided with three metals: aluminium, zinc and silver; and three electrolyte solutions:
aluminium nitrate, zinc nitrate and silver nitrate.
9.2.4.3.4
(a) Identify which combination of the metals supplied should give the highest potential
difference. (1 mark)
9.2.4.3.2
9.2.4.2.5
9.1.13.1e
9.1.11.3a
(b) Sketch and label a diagram of an experimental setup that the student could use with the
combination of metals identified in part (a). (2 marks)
9.2.4.3.4
9.2.1.3.1
9.1.13.1d (c) Write a balanced chemical equation for the overall reaction for the metals identified in part
9.1.12.4b (a), and calculate the expected potential difference. (2 marks)
9.2.4.3.4 (d) The measured potential difference obtained varied from the theoretical value. Outline steps
9.2.4.3.2 the student could have taken to minimise this variation. (2 marks)
9.2.4.3.1
9.1.14.1d
9.1.12.4e
2004
9.2.4.3.3
15 Diagram A shows a dry cell. Diagram B shows a lead-acid cell.
Which of the following shows the correctly labelled parts?
2005
Question 19
You have studied one of the cells shown below.
Choose ONE of the cells and answer parts (a) and (b).
9.2.4.3.3
(a) State ONE environmental impact associated with the cell you have chosen. (1 mark)
9.2.4.3.3
9.2.4.2.6
9.2.4.2.5
9.2.4.2.4
(b) Describe the chemistry of the cell you have chosen. (3 marks)
2007
Question 20 The diagram represents a typical car battery.
As the battery discharges, the following half reactions occur:
Pb(s) +SO42-(aq) → PbSO4(s) +2e–
9.2.4.2.6
PbO2(s) + SO42-(aq) + 4H+(aq) +2e– → PbSO4(s) +2H2O(l)
9.1.13.1d (a)Identify the anode, then write the equation that represents the overall chemical reaction.
(2 marks)
9.2.4.3.3
(b)Explain one benefit of car batteries lasting several years.
2009
(2 marks)
Question 26 (7 marks)
9.2.4.3.3 An electrochemical cell is constructed using two half cells. One half cell consists of an
2+
3+
9.2.4.2.1
inert platinum electrode and a solution of Fe and Fe . The other half cell consists of a
9.1.13.1d
2+
lead electrode and a solution of Pb .
Current will flow from one electrode to the other electrode when the cell is completed
using a voltmeter and a salt bridge.
(a) Write relevant half equations and a balanced net ionic equation for the overall cell reaction.
(2 marks)
2007
5 The diagram represents a cell in which two metals have been placed in a solution containing
their respective metallic ions. The metals are connected to a voltmeter.
9.2.4.3.4
9.2.4.3.2
9.1.12.4b
Which of the following combinations of metals would produce the highest reading on the
voltmeter?
(A) Tin and zinc
(B) Copper and zinc
(C) Copper and silver
(D) Magnesium and lead
2008
Question 25 A galvanic cell under standard conditions is represented below.
9.2.4.2.6
9.2.4.2.5
9.1.12.3c
(a) On the diagram, clearly label the anode, the cathode and the direction of electron flow. (1 mark)
9.2.4.2.3
9.1.13.1d
(b) Write a balanced net ionic equation for the overall cell reaction.
−
9.2.4.2.6
9.2.4.2.5
9.1.12.3c
(c) Calculate the standard cell potential (E °).
(1 mark)
(1 mark)
9.2.4.2.3 (d) Explain any colour changes observed in this cell as the reaction proceeds.
9.2.4.2.1
9.1.14.1d
2009
(2 marks)
Question 26
9.2.4.3.4 An electrochemical cell is constructed using two half cells. One half cell consists of an
2+
3+
9.1.12.4b
inert platinum electrode and a solution of Fe and Fe . The other half cell consists of a
2+
lead electrode and a solution of Pb .
Current will flow from one electrode to the other electrode when the cell is completed
using a voltmeter and a salt bridge.
−
(b) Calculate the standard cell potential (E ° ).
(1 marks)
2011
12 A table of redox couples and their standard reduction potentials is shown.
9.2.4.3.4
9.2.4.2.2
Which of the following ranks the metals in decreasing order of their electrochemical activity?
(A) Ni > Cd > Ag > Pd
(B) Pd > Ag > Cd > Ni
(C) Pd > Ag > Ni > Cd
2011
(D) Cd > Ni > Ag > Pd
Question 24 A galvanic cell was constructed as shown in the diagram.
9.2.4.3.4
9.2.4.2.4
ᶱ
(a) Calculate the standard cell potential (E ). In your answer, include a net ionic equation for
the overall cell reaction.
(2 marks)
2001
Question 18
A galvanic cell was made by connecting two half-cells. One half-cell was made by putting a
copper electrode in a copper (II) nitrate solution. The other half-cell was made by putting a
silver electrode in a silver nitrate solution. The electrodes were connected to a voltmeter as
shown in the diagram.
9.2.4
(a) Complete the above diagram by drawing a salt bridge.
9.2.4
(b) Using the standard potentials table in the data sheet, calculate the theoretical voltage of this
galvanic cell.
(2 marks)
9.2.4
(c) A student removes the voltmeter from the circuit and replaces it with an electrical generator.
The generator causes the copper electrode to increase in mass. Explain, using an equation, why
the copper electrode will increase in mass.
(3 marks)
2001
9.2.4
(1 mark)
Question 19 (7 marks)
Name ONE type of cell, other than the dry cell or lead–acid cell, you have studied. Evaluate it
in comparison with either the dry cell or lead–acid cell, in terms of chemistry and the impact on
society. Include relevant chemical equations in your answer.
2002
3 Which explanation best describes why an understanding of electrolysis has made a significant
impact on the production of materials?
9.2.4
2002
9.2.4
2002
(A) Electrolysis reactions do not require an energy source.
(B) Electrolysis can be used to split water into hydrogen and oxygen.
(C) Electrolysis provides a way to make non-spontaneous reactions occur.
(D) Electrolysis can be used to produce aluminium.
4 Which statement concerning galvanic cells is correct?
(A) Oxidation occurs at the anode.
(B) They are also known as electrolytic cells.
(C) The cathode is assigned a negative charge.
(D) An external power source must be present.
5 What arrangement of an electrolytic cell would electroplate a silver coin with copper?
9.2.4
2003
9.2.4
9.1
2003
9.2.4
9.1
13 A student performed three tests to investigate the relative activity of metals. In each test a
metal strip was placed in a solution containing ions of a different metal. The results are shown
in the diagrams.
What is the order of activity of the metals, based on these results?
(A) X > Z > Y
(B) Y > X > Z
(C) Z > Y > X
(D) Z > X > Y
Question 19
(a) Identify the cathode in this diagram.
(1 mark)
ᶱ
(b) Write the net redox equation for the cell reaction, and calculate the cell potential (E ).
(2 marks)
2005
1 Which of the following conditions would produce a radioactive isotope?
9.2.5.2.1
(A) Too many atoms in the sample provided
(B) Too many protons and neutrons in the atom
(C) Too many electrons in the outer shell of the atom
(D) Too many electrons for the number of neutrons in the atom
3 Which set contains only stable nuclei?
2006
9.2.5.2.1
9.1.14.1a
9.1.13.1d
2009
1 Which of the following is an important factor in predicting the nuclear stability of an isotope?
9.2.5.2.1
(A) Atomic radius
(B) Nuclear radius
(C) The ratio of neutrons to protons
2011
(D) The ratio of electrons to protons
7 Which of the following lists contains ONLY unstable isotopes?
9.2.5.2.1
2010
2 Which of the following is an example of a transuranic element?
9.2.5.2.2
(A) C–14
(B) Co–60
(C) U–238
(D) Cm–249
2011
9.2.5.2.2
9.2.5.2.1
Question 23
(a) Element 112 was first synthesised in 1996 and officially named in 2009 as copernicium, Cn.
Explain why the transuranic isotope 278
(1 mark)
112𝐶𝑛 is unstable.
(b) Describe a method by which transuranic elements can be synthesised.
(2 marks)
9.2.5.2.2
2008
1 Which of the following radiations is measured with a Geiger counter?
9.2.5.2.4
(A) Beta
(B) Infrared
(C) Microwave
(D) Ultraviolet
Question 16 (3 marks)
Describe how technology has enabled the transuranic elements to be produced.
2006
9.2.5.3.1
9.2.5.2.2
2004
9.2.5.3.2
9.2.5.2.6
2007
9.2.5.3.2
9.2.5.2.6
9.2.5.2.5
9.1.14.3b
Question 26 (4 marks)
Discuss the benefits and problems associated with the use of ONE radioactive isotope in
industry.
Question 19 (7 marks)
There are many benefits and problems associated with the use of radioisotopes in industry and
medicine. Evaluate the impact on society of the use of radioisotopes in both industry and
medicine. In your answer, give examples of specific radioisotopes, making reference to their
chemical properties.
2001
9.2.5
2002
Question 16 (3 marks)
Radioisotopes are used in industry, medicine and chemical analysis. For ONE of these fields,
relate the use of a named radioisotope to its properties.
Question 19
(a) Describe the conditions under which a nucleus is unstable.
(2 marks)
9.2.5
9.2.5
(b) The following is a flow diagram showing the sequence of products released during the
decay of uranium.
Use examples from the flow diagram to describe processes by which an unstable isotope
undergoes radioactive decay.
(3 marks)
2003
2 Which of the following is a transuranic element?
9.2.5
9.1
(A) Caesium
(B) Cerium
(C) Chromium
(D) Curium
2003
3 Which instrument is used to detect radiation from radioactive isotopes?
9.2.5
9.1
(A) pH meter
(B) Geiger counter
(C) Ion-selective electrode
(D) Atomic absorption spectrophotometer (AAS)
Question 18 (4 marks)
2003
9.2.5
Describe how commercial radioisotopes are produced, and how transuranic elements are
produced.