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2013H I G H E R S C H O O L C E R T I F I C AT E
E X A M I N AT I O N
Chemistry
General Instructions
• Reading time – 5 minutes
• Working time – 3 hours
• Write using black or blue pen Black pen is preferred
• Draw diagrams using pencil
• Board-approved calculators may be used
• A data sheet and a Periodic Table are provided at the back of this paper
• Write your Centre Number and Student Number at the top of pages 13, 17, 19, 21 and 25
Total marks – 100
Section I Pages 2–28
75 marks
This section has two parts, Part A and Part B
Part A – 20 marks
• Attempt Questions –
• Allow about 35 minutes for this part
Part B – 55 marks
• Attempt Questions
1 20
21–31
• Allow about 1 hour and 40 minutes for this part
Section II Pages 29–44
25 marks
• Attempt ONE question from Questions –
• Allow about 45 minutes for this section
32 36
2060
Section I 75 marks
Part A – 20 marks Attempt Questions 1–20 Allow about 35 minutes for this part
Use the multiple-choice answer sheet for Questions 1–20.
1 Which pair of reactants is used to industrially synthesise ammonia?
(A) H2 and C
(B) H2 and N2
(C) H2O and N2
(D) H2O and NO2
2 What is the purpose of the flame in atomic absorption spectroscopy (AAS)?
(A) To ionise the sample
(B) To produce a spectrum
(C) To atomise the substance
(D) To provide the absorption wavelength
3 What is the main environmental problem associated with chlorofluorocarbon compounds?
(A) Acid rain
(B) Eutrophication
(C) Global warming
(D) Ozone depletion
– 2 –
– 3 –
4 Butan-1-ol burns in oxygen according to the following equation.
C4H9OH(l) + 6O2(g) → 4CO2(g) + 5H2O(l)
How many moles of carbon dioxide would form if two moles of butan-1-ol were burnt in excess oxygen?
(A) 2
(B) 4
(C) 8
(D) 10
5 When placed in the Periodic Table, the recently discovered element 116 would be found in the same group as
(A) element 16.
(B) element 43.
(C) element 87.
(D) element 102.
6 A representation of the Periodic Table is shown. The positions of six different elements, P, Q, R, S, T and U are given.
P Q R S
T U
Which row of the following table shows the correct acid and base reactivities of the oxides of these elements?
(A)
(B)
(C)
(D)
Oxide reacts with acid only
Oxide reacts with base only
Oxide reacts with both acid and base
P, T R, U Q, S
P, R , T U Q, S
Q, R P, S T, U
Q, S R, U P, T
7 Which of the following is the correct equation for an INCOMPLETE combustion of octane?
(A) C8H18(l) + 8O2(g) → 8CO2(g) + 9H (g2 )
(B) C8H l18( ) + 25O2(g) → 8CO2(g) + 9H O(l2 )2
(C) C8H l18( ) + 6O g g2( ) → 3CO( ) + 5C(s) + 9H2O(l)
(D) C (l) + 13O g g s l8H18 2( ) → 4CO( ) + 4C( ) + 9H2O( )
8 Which of the following structural formulae shows citric acid, also known as 2-hydroxypropane-1,2,3-tricarboxylic acid?
(A)
(B)
(C)
(D)
O OH O OH O OH C C C
H C
H
C
OH
C
H
H
C O OH
C O OH
C O OH
H C
OH
C
OH
C
H
OH
C O OH
C O OH
C O OH
HO C
H
C
H
C
H
H
C O OH
C O OH
C O OH
HO C
H
C
H
C
H
OH
– 4 –
O OH O OH C C
CH2 CH CH2 CH n
9 A portion of a resin made from acrylic acid (CH2 =CHCOOH) is shown.
Which type of reaction results in the formation of this polymer?
(A) Addition
(B) Condensation
(C) Dehydration
(D) Esterification
10 The following equilibrium is set up in a sealed reaction vessel.
N2O4(g) 2NO2(g) ΔH = +54.8 kJ mol–1
Which of the following would INCREASE the yield of nitrogen dioxide?
(A) Adding a catalyst to the reaction vessel
(B) Decreasing the volume of the reaction vessel
(C) Raising the temperature of the reaction vessel
(D) Increasing the pressure by adding argon to the reaction vessel
11 The table shows the heat of combustion for four compounds.
Compound Heat of combustion (kJ mol–1)
CO 233
CH4 890
C2H2 1300
C2H6 1560
Which of these compounds would produce the greatest amount of energy if 1.00 g of each is burnt?
(A) CO
(B) CH4
(C) C2H2
(D) C2H6
– 5 –
12 An experiment was set up as shown.
ZnCl2(aq)
Cl2(g)
Zn(s)Pt(s)
V
Which of the following statements is correct?
(A) The chlorine gas is the anode.
(B) The zinc electrode is the anode.
(C) The platinum electrode is the anode.
(D) There is no anode because there is no salt bridge.
– 6 –
13
What is the structure of the polymer most likely to have been used in the manufacture of the cup shown?
(A)
(B)
H H
(C)
C
H H H H H H
C C C C C C
H H H H H H n
H H H H H H
C C C C C C
H
n
H Cl H Cl H Cl
C C C C C
H H H H H H n
(D)
H H
H OH
CH2OH
OH H
OO
CCCC
CC CC
H
CC
HH HH
OO
CH2OH
H OH
H CCCC
CC OO
OH H
CC H H
OO
H OH
CH2OH
OH H
OO
CCCC
CC CC
H
CC
HH
OO
OO
HH CC
n
– 7 –
14 Sodium reacts with water to give hydrogen gas and sodium hydroxide solution.
What volume of gas would be produced from the reaction of 22.99 g of sodium at 25°C and 100 kPa?
(A) 11.36 L
L
L
L
(B) 12.40
(C) 22.71
(D) 24.79
15 A pH 3.0 solution of HCl(aq) is diluted by adding water to produce a pH 5.0 solution.
Which row in the following table correctly identifies an appropriate volume of the original solution and the volume of water added for this dilution?
Volume of original solution (mL) Volume of water added (mL)
(A) 100 900
(B) 100 1000
(C) 10 990
(D) 1 1000
16 Which two species will react to form a product containing a coordinate covalent bond?
(A) Ca(s) and 2H (aq)
(B) H O( +l) and H (aq2 )
(C) Ag+(aq) and Cl–(aq)
(D) NH +4 (aq) and OH–(aq)
+
17 A 25.0 mL sample of a 0.100 mol L–1 hydrochloric acid solution completely reacted with 23.4 mL of sodium hydroxide solution.
What volume of the same sodium hydroxide solution would be required to completely react with 25.0 mL of a 0.100 mol L–1 acetic acid solution?
(A) Less than 23.4 mL
(B) 23.4 mL
(C) More than 23.4 mL
(D) Unable to calculate unless the concentration of the sodium hydroxide solution is also known
– 8 –
18 Consider the following series of reactions.
Catalytic cracking
Dilute sulfuric acid
cid Concentrated sulfuric acid
Petroleum fractions
Compound X
Compound Y
Compound Z
Propanoic a
Which row in the table correctly identifies Compounds X, Y and Z?
Compound X Compound Y Compound Z
(A) Propene Propan-1-ol Ethyl propanoate
(B) Propene Ethanol Propyl ethanoate
(C) Ethanol Ethylene Propyl ethanoate
(D) Ethylene Ethanol Ethyl propanoate
– 9 –
O O O O O
Ozone Oxygen
19 A solution was obtained by boiling flowers in water. After various substances were added to separate samples of the solution, the colour of each was noted.
Substance added Colour observed
0.1 mol L–1 HCl(aq) Bright pink
0.01 mol L–1 HCl(aq) Bright pink
0.001 mol L–1 HCl(aq) Pale yellow
Distilled water Bright yellow
0.001 mol L–1 NaOH(aq) Bright yellow
0.01 mol L–1 NaOH(aq) Bright yellow
For which of the following titrations would it be appropriate to use this solution as an indicator?
(A) HCl(aq) + NH3(aq)
(B) HCl(aq) + NaOH(aq)
(C) CH COOH(aq) + NH aq3 3( )
(D) CH3COOH(aq) + NaOH(aq)
20 The structures of ozone and molecular oxygen are shown.
Ozone is more easily decomposed than molecular oxygen because
(A) it is polar.
(B) it is a bent molecule.
(C) it has a greater molecular mass.
(D) it has a lower average bond energy.
– 10 –
BLANK PAGE
– 11 –
BLANK PAGE
– 12 –
© Board of Studies NSW 2013
2013 HIGHER SCHOOL CERTIFICATE EXAMINATION
Chemistry Centre Number
Student Number
Section I (continued)
Part B – 55 marks Attempt Questions 21–31 Allow about 1 hour and 40 minutes for this part
Answer the questions in the spaces provided. These spaces provide guidance for the expected length of response.
Show all relevant working in questions involving calculations.
Question 21 (6 marks)
Please turn over
2061 – 13 –
Question 21 (6 marks)
An ester and an acid are both listed as additives on a food label.
(a) 2 Why is acid used as a food preservative?
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(b) 4 Explain, on a labelled diagram, why reflux is used to produce an ester.
– 14 –
Question 22 (5 marks)
A solution contains three cations, Ba2+, Cu2+ and Pb2+. The flow chart indicates theplan used to confirm the identity of these cations.
(a) 1Name Precipitate 2.
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(b) 2Write a balanced net ionic equation for the formation of Precipitate 1.
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(c) 2Suggest a test and the expected result that would confirm the identity of themetal cation remaining in Filtrate 2.
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BLANK PAGE
– 16 –
© Board of Studies NSW 2013
2013 HIGHER SCHOOL CERTIFICATE EXAMINATION
Chemistry Centre Number
Student Number
Section I – Part B (continued)
Question 23 (7 marks)
A 20.72 g sample of solid lead was placed into 0.100 L of 1.00 mol L–1 silver nitrate solution.
(a) 5 Complete the table. Show relevant calculations in the space below the table.
Chemical species
Pb2+(aq) Pb(s) Ag+(aq) Ag(s) NO3 −(aq)
Moles in final mixture
Balanced chemical equation
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(b) 2 With reference to only ONE species in the product mixture, explain why care must be taken in disposing of the final mixture.
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2062 – 17 –
Question 24 (4 marks)
Consider this chemical system which is at equilibrium.
X(g) + Y(g) Z(g) + heat
(a) 2 Explain the effect of decreasing the volume of the reaction vessel.
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(b) 2 Explain the effect of adding a catalyst to this equilibrium mixture.
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Question 25 (4 marks)
4 An indicator is placed in water. The resulting solution contains the green ion, Ind , and the red molecule, HInd.
Explain why this solution can be used as an indicator. In your response, include a suitable chemical equation that uses −Ind and HInd.
−
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© Board of Studies NSW 2013
2013 HIGHER SCHOOL CERTIFICATE EXAMINATION
Chemistry Centre Number
Student Number
Section I – Part B (continued)
Question 26 (4 marks)
4 Explain how microscopic membrane filters purify contaminated waters, in terms of their design and composition.
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2063 – 19 –
Tem
pera
ture
of
oily
liqu
id (
°C) 60.0
50.0
40.0
30.0
20.0
10.0
0 Measurements
stopped Heating
completed Heating
commenced
Question 27 (4 marks)
4 A 0.259 g sample of ethanol is burnt to raise the temperature of of an oily liquid, as shown in the graph. There is no loss of heat to the surroundings.
120 g
Time
Using the information shown on the graph, calculate the specific heat capacity of the oily liquid. The heat of combustion of ethanol is 1367 kJ mol–1.
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– 20 –
© Board of Studies NSW 2013
2013 HIGHER SCHOOL CERTIFICATE EXAMINATION
Chemistry Centre Number
Student Number
Section I – Part B (continued)
Question 28 (5 marks)
Please turn over
2064 – 21 –
Question 28 (5 marks)
A student attempted to determine the concentration of a hydrochloric acid solution. The following steps were performed.
Step 1. A conical flask was rinsed with water.
Step 2. A 25.0 mL pipette was rinsed with water.
Step 3. The student filled the pipette with a standard sodium carbonate solution to the level shown in the diagram.
Gradation mark
Sodium carbonate solution
Step 4. The standard sodium carbonate solution in the pipette was transferred to the conical flask. The student ensured that all of the sodium carbonate solution was transferred to the conical flask by blowing through the pipette. Three drops of an appropriate indicator were added to the conical flask.
Step 5. A burette was rinsed with the hydrochloric acid solution and then filled with the acid. The student then carried out a titration to determine the concentration of the hydrochloric acid solution.
In steps 2, 3 and 4 above the student did not follow acceptable procedures.
(a) 2 Identify the mistake the student made in step 4 and propose a change that would improve the validity of the result.
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Question 28 continues on page 23
– 22 –
Question 28 (continued)
(b) 3 Explain the effect of the mistakes made in steps 2 and 3 on the calculation of the concentration of the hydrochloric acid solution.
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End of Question 28
Please turn over
– 23 –
Question 29 (2 marks)
2 Consider this chemical equation.
2Cl–(aq) + Br2(l) → 2Br–(aq) + Cl2(g)
Will the reaction occur spontaneously? Justify your response.
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– 24 –
© Board of Studies NSW 2013
2013 HIGHER SCHOOL CERTIFICATE EXAMINATION
Chemistry Centre Number
Student Number
Section I – Part B (continued)
Question 30 (6 marks)
Please turn over
2065 – 25 –
Question 30 (6 marks)
6 The images below represent the concentration of ozone in the atmosphere above Antarctica near the South Pole for the years 1979, 1994 and 2012, measured at the same time each year.
South Pole
1979 1994 2012
0 100 200 300 400 500
Total ozone (Dobson units)
Account for the changes in ozone concentration above Antarctica between 1979 and 2012. Your response should include relevant equations.
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Question 30 continues on page 27
– 26 –
Question 30 (continued)
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End of Question 30
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Question 31 (8 marks)
(a) 5 Construct separate flow diagrams to show the steps used in the production of polyethylene and those used in the production of a recently developed biopolymer.
Polyethylene Name of biopolymer:
(b) 3 Justify the use of a recently developed biopolymer over a polymer obtained from fossil fuel.
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– 28 –
© Board of Studies NSW 2013
2013 HIGHER SCHOOL CERTIFICATE EXAMINATION
Chemistry
Section II
25 marks Attempt ONE question from Questions 32–36 Allow about 45 minutes for this section
Answer parts (a)–(c) of the question in Section II Answer Booklet 1. Answer parts (d)–(e) of the question in Section II Answer Booklet 2. Extra writing booklets are available.
Show all relevant working in questions involving calculations.
Pages
Question 32 Industrial Chemistry ............................................................. 30–32
Question 33 Shipwrecks, Corrosion and Conservation ............................ 33–34
Question 34 The Biochemistry of Movement .......................................... 35–38
Question 35 The Chemistry of Art ........................................................... 39–40
Question 36 Forensic Chemistry .............................................................. 41–44
2066 – 29 –
Question 32 — Industrial Chemistry (25 marks)
Answer parts (a)–(c) in Section II Answer Booklet 1.
(a) 3 The diagram shows a sequence of steps in the removal of grease from a surface.
Explain the process shown in these steps.
Grease
Surface Step 1 Step 2 Step 3
(b) Hydrogen iodide is a colourless gas that will decompose into colourless hydrogen gas and purple iodine gas according to the following endothermic reaction.
2HI(g) H2(g) + I2(g)
(i) 3 A 1.0 L glass container was filled with 0.60 moles of hydrogen iodide gas. When equilibrium was established, there were 0.25 moles of iodine gas present in the container.
Calculate the equilibrium constant for this reaction.
(ii) 2 The container was then cooled.
Explain the change in the appearance of its contents.
Question 32 continues on page 31
– 30 –
Question 32 (continued)
(c) The diagram shows a region where construction of a Solvay plant is being considered.
Ocean
B
A
Limestone deposit
50 km
Railway line Key
OceanOcean
Port City
(i) 2 Why is limestone important in the Solvay process? Include a relevant chemical equation in your response.
– 31 –
(ii) 3 Justify which of sites A or B would be the preferred location for a Solvay plant.
Question 32 continues on page 32
Question 32 (continued)
Answer parts (d)–(e) in Section II Answer Booklet 2.
(d) A first-hand investigation is conducted on the electrolysis of an aqueous solution of sodium chloride.
(i) 2 Justify the use of a safety precaution, other than wearing safety glasses, when carrying out this investigation.
(ii) 3 Describe how the THREE products of this electrolysis could be identified.
(e) 7 There is often a compromise between maximising yield and minimising the environmental impact of industrial processes.
Justify this statement with reference to the production of sulfuric acid.
End of Question 32
– 32 –
Question 33 — Shipwrecks, Corrosion and Conservation (25 marks)
Answer parts – in Section II Answer Booklet 1.
(a)
Connection to metal mesh cage
Insulating stand for artefact
Electrolyte solution
(a) (c)
3 The treatment of a marine artefact is shown.
Power supply
Explain why this process is used.
(b) (i) 2 Write a balanced chemical equation for the corrosion of tin in shallow water.
(ii) 3 Summarise the role of electron transfer in corrosion reactions. Include relevant equations in your answer.
Question 33 continues on page 34
– 33 –
Question 33 (continued)
(c) The solubility of oxygen in sea water at various temperatures is shown in the graph.
4
5
6
7
8
9
10
11
12
Solu
bilit
y (m
g L
–1 )
0 10 20 30 Temperature (°C)
40 50
(i) 2 Predict the solubility of oxygen at 4°C.
(ii) 3 Analyse the factors that affect the concentration of dissolved oxygen at increasing depths in the ocean.
Answer parts (d)–(e) in Section II Answer Booklet 2.
(d) (i) 3 Design a suitable first-hand investigation that could be carried out in a school laboratory to compare the effectiveness of different ways of preventing the corrosion of iron in a marine environment. Include relevant diagrams in your answer.
(ii) 2 Use the expected results of the investigation to justify the ongoing use of iron in the construction of ocean-going vessels.
(e) 7 From the scientists studied in this option, assess whose work has most changed the nature of scientific thinking about redox reactions.
End of Question 33
– 34 –
N
N
N
C
HC C
C
N
CH
NH2
O
P P PO O O
O O
O –
O –
O –
O –
CH2
OH OH
CH
HC CH
CH
O
X Y Z
Question 34 — The Biochemistry of Movement (25 marks)
Answer parts (a)–(c) in Section II Answer Booklet 1.
(a) 3 The molecule below is adenosine triphosphate (ATP).
Explain which part of the molecule, X, Y or Z, is the most important biologically. Include a relevant equation in your answer.
Question 34 continues on page 36
– 35 –
Question 34 (continued)
(b) The table below gives the abbreviation and structural formulae for two amino acids.
Part of the glycine molecule has been replaced by X.
Name Abbreviation Formula
Glycine Gly COOHX
H
H
C
Tyrosine Tyr HO COOH
NH2
H
H
C
H
C
(i) 2 Write an equation using the correct structural formulae showing the formation of a dipeptide between glycine and tyrosine.
(ii) 3 Explain, in terms of chemical bonding, how the three-dimensional shape of a protein depends upon its primary structure.
Question 34 continues on page 37
– 36 –
Question 34 (continued)
(c) The following energy profile is for the combustion of glucose during cellular respiration.
Ene
rgy
Glucose and oxygen 181 kJ mol–1
2997 kJ mol–1
Carbon dioxide and water
Progress of reaction
(i) 2 The hourly energy requirement of an astronaut is supplied by 36.0 g of glucose.
Using the energy profile above, determine the energy required by the astronaut in one hour.
(ii) 3 Calculate the volume of oxygen consumed by the astronaut in one hour. The conditions are 25° and 100 Include a chemical equation in your answer.
C kPa.
Question 34 continues on page 38
– 37 –
Question 34 (continued)
Answer parts (d)–(e) in Section II Answer Booklet 2.
(d) A first-hand investigation was conducted to demonstrate the effect of temperature on the reaction of an enzyme.
(i) 3 Describe a procedure that could be used to demonstrate the effect of temperature on the reaction of an enzyme.
(ii) 2 A sketch showing a student’s results is provided below.
Rate of reaction
Temperature
Explain the shape of the curve.
(e) 7 ‘Give me a muscle biopsy and I’ll tell you whether you should be a sprinter or a marathon runner.’
Evaluate the scientific accuracy of this statement in terms of muscle fibre structure and function.
End of Question 34
– 38 –
Question 35 — The Chemistry of Art (25 marks)
Answer parts (a)–(c) in Section II Answer Booklet 1.
(a) 3The emission spectrum of a metal salt is observed with a spectroscope.
A B
Blue Red
CN
CN
CNNi
CN
NC
3–
Explain the processes by which emission lines arise. Include an energy leveldiagram for the lines marked A and B in your response.
(b) (i) 2
– 39 –
Identify in which of the s, p, d or f blocks of the Periodic Table theelement Ra is found. Justify your answer.
(ii) 3An atom has FIVE valence electrons in its d orbital. Using an orbitaldiagram of the valence shell of the atom, explain how Hund’s ruledetermines the electronic configuration.
(c) The structure of a nickel cyanide complex is shown.
(i) 2What is the oxidation state of nickel in this complex? Justify youranswer.
(ii) 3Explain the bonding of the complex with the aid of a Lewis structure forthe cyanide ligand.
Question 35 continues on page 40
Question 35 (continued)
Answer parts (d)–(e) in Section II Answer Booklet 2.
(d) A first-hand investigation is conducted to demonstrate the oxidising strength of potassium permanganate.
(i) 2 Describe a procedure that could be used to demonstrate the oxidising strength of potassium permanganate.
(ii) 3 What does this investigation show about the oxidising strength of potassium permanganate? Use half-equations in your answer.
(e) 7 Discuss the principles involved in using infra-red and ultraviolet spectroscopy for the analysis of pigments.
End of Question 35
– 40 –
Question 36 — Forensic Chemistry (25 marks)
Answer parts (a)–(c) in Section II Answer Booklet 1.
(a) 3 A sample was collected from inside a reaction vessel at a suspected illegal drug laboratory. The sample was analysed by high performance liquid chromatography (HPLC). The chromatogram obtained from the collected sample is provided below.
Sample chromatogram from the reaction vessel
Signal intensity
150 5 10 Retention time (minutes)
The chromatogram of a standard mixture containing four compounds commonly produced in illegal drug laboratories is also provided.
Standard chromatogram
C Key A Amphetamine B Methamphetamine C Methcathinone D MDMA
Signal intensity
15
A
B D
0 5 10 Retention time (minutes)
By referring to the chromatograms, explain how this information could be used as evidence to support a guilty verdict in a court case.
Question 36 continues on page 42
– 41 –
Question 36 (continued)
(b) (i) 2 Information about three polysaccharides (cellulose, glycogen and starch) is provided in the table below.
X
Plant polysaccharide
Contains branched and linear chains
Y
Animal polysaccharide
Contains highly branched chains
Z
Plant polysaccharide
Contains linear chains
Identify X, Y and Z.
(ii) 3 Select ONE of cellulose, glycogen or starch and explain its primary function in terms of its composition and structure.
Question 36 continues on page 43
– 42 –
Question 36 (continued)
(c) A pesticide manufacturer is suspected of releasing waste water contaminatedwith heavy metal ions into a local river. Atomic emission spectroscopy is usedto identify the possible pollutants.
(i) 2Use the following emission spectra to identify a metal pollutant in theriver. Justify your answer.
Cadmium
Mercury
Lead
River sample
400 500Wavelength (nm)
600 700
– 43 –
(ii) 3Outline a procedure that could be used in a school laboratory to SAFELYproduce and analyse the emission spectrum of an element.
Question 36 continues on page 44
Question 36 (continued)
Answer parts (d)–(e) in Section II Answer Booklet 2.
(d) Alkanes, alkenes, alkanols and alkanoic acids are four different classes of organic compounds.
(i) 2 Describe a simple test that would confirm that a compound is organic.
(ii) 3 Describe a sequence of tests that could be used to distinguish between any THREE of the classes of organic compounds named above.
(e) 7 A chemist working in a forensic laboratory is asked to analyse a residue of an explosive. They selected chromatography as the preferred analytical technique over electrophoresis. Justify this decision.
End of paper
– 44 –
© Board of Studies NSW 2013
– 45 –
NA .................................................................. 6.022 ¥ 1023 mol 1
100 kPa 0°C (273.15 K) ...................... 22.71 L25°C (298.15 K) .................... 24.79 L
25°C (298.15 K), Kw ................. 1.0 ¥ 10 14
..................................................... 4.18 ¥ 103 J kg–1 K 1
pH = –log10[H+ ] DH = m CDT
2013 HIGHER SCHOOL CERTIFICATE EXAMINATION
Chemistry
2067
DATA SHEET
Avogadro constant, –
Volume of 1 mole ideal gas: at andat at
Ionisation constant for water at –
Specific heat capacity of water –
Some useful formulae –
Some standard potentials
Aylward and Findlay, SI Chemical Data (5th Edition) is the principal source of data forthis examination paper. Some data may have been modified for examination purposes.
– 46 –
112
C
Cop
erni
cium
9 F
Fluo
rine
17 Cl
Chl
orin
e
35 Br
Bro
min
e
53 I
Iodi
ne
85 A
Ast
atin
e
7 N
Nitr
ogen
15 P
Phos
phor
us
33 As
Ars
enic
51 Sb
Ant
imon
y
83 Bi
Bis
mut
h
5 B
Bor
on
13 Al
Alu
min
ium
31 Ga
Gal
lium
49 In
Indi
um
81 Tl
Tha
llium
107
B
Boh
rium
108
H
Has
sium
109
M
Mei
tner
ium
110
D
Dar
mst
adtiu
m
111
R
Roe
ntge
nium
87 F
Fran
cium
88 R
Rad
ium
8910
310
4R
Rut
herf
ordi
um
105
D
Dub
nium
106
S
Seab
orgi
um
1 H
Hyd
roge
n
PE
RIO
DIC
TA
BL
E O
F T
HE
EL
EM
EN
TS
KE
Y
2 He
1.00
84.
003
Hel
ium
3 Li
6.94
1L
ithiu
m
4 Be
9.01
2B
eryl
lium
Ato
mic
Num
ber
Sym
bol
Stan
dard
Ato
mic
Wei
ght
Nam
e
79 Au
197.
0G
old
6 C10
.81
12.0
1C
arbo
n
8 O14
.01
16.0
0O
xyge
n
10 Ne
19.0
020
.18
Neo
n
11 Na
22.9
9So
dium
12 Mg
24.3
1M
agne
sium
14 Si26
.98
28.0
9Si
licon
16 S
Sulf
ur
18 Ar
Arg
on
19 K
Pota
ssiu
m
20 Ca
Cal
cium
21 Sc
Scan
dium
22 Ti
Tita
nium
23 V
Van
adiu
m
24 Cr
Chr
omiu
m
25 Mn
Man
gane
se
26 Fe Iron
27 Co
Cob
alt
28 Ni
Nic
kel
29 Cu
Cop
per
30 Zn
Zin
c
32 Ge
Ger
man
ium
34 Se
Sele
nium
36 Kr
Kry
pton
37 Rb
Rub
idiu
m
38 Sr
Stro
ntiu
m
39 Y
Yttr
ium
40 Zr
Zir
coni
um
41 Nb
Nio
bium
42 Mo
Mol
ybde
num
43 T
Tech
netiu
m
44 Ru
Rut
heni
um
45 Rh
Rho
dium
46 Pd
Palla
dium
47 Ag
Silv
er
48 Cd
Cad
miu
m
50 Sn Tin
52 Te
Tellu
rium
54 Xe
Xen
on
55 Cs
Cae
sium
56 Ba
Bar
ium
5771
72 Hf
Haf
nium
73 Ta
Tant
alum
74 W
Tun
gste
n
75 Re
Rhe
nium
76 Os
Osm
ium
77 Ir
Irid
ium
78 Pt
Plat
inum
79 Au
Gol
d
80 Hg
Mer
cury
82 Pb Lea
d
84 P
Polo
nium
86 R Rad
on
Lan
than
oids
57 La
Lan
than
um
58 Ce
Cer
ium
59 Pr
Pras
eody
miu
m
60 Nd
Neo
dym
ium
61 P
Prom
ethi
um
62 Sm
Sam
ariu
m
63 Eu
Eur
opiu
m
64 Gd
Gad
olin
ium
65 Tb
Terb
ium
66 Dy
Dys
pros
ium
67 Ho
Hol
miu
m
68 Er
Erb
ium
69 Tm
Thu
lium
70 Yb
Ytte
rbiu
m
71 Lu
Lut
etiu
m
Act
inoi
ds
89 A
Act
iniu
m
90 Th
Tho
rium
91 Pa
Prot
actin
ium
92 U
Ura
nium
93 N
Nep
tuni
um
94 P
Plut
oniu
m
95 A
Am
eric
ium
96 C Cur
ium
97 B
Ber
keliu
m
98 C
Cal
ifor
nium
99 E
Ein
stei
nium
100
F
Ferm
ium
101
M
Men
dele
vium
102
N
Nob
eliu
m
103
L
Law
renc
ium
30.9
732
.07
35.4
539
.95
39.1
040
.08
44.9
647
.87
50.9
452
.00
54.9
455
.85
58.9
358
.69
63.5
565
.38
69.7
272
.64
74.9
278
.96
79.9
083
.80
85.4
787
.61
88.9
191
.22
92.9
195
.96
c10
1.1
102.
910
6.4
107.
911
2.4
114.
811
8.7
121.
812
7.6
126.
913
1.3
132.
913
7.3
Lan
than
oids
–
138.
914
0.1
140.
914
4.2
m15
0.4
152.
015
7.3
158.
916
2.5
164.
916
7.3
168.
917
3.1
175.
0
178.
518
0.9
183.
918
6.2
190.
219
2.2
195.
119
7.0
200.
620
4.4
207.
220
9.0
ot
n
ra
Act
inoi
ds
–
c23
2.0
231.
023
8.0
pu
mm
kf
sm
do
r
fb
gh
st
sg
n
Ele
men
ts w
ith a
tom
ic n
umbe
rs 1
13 a
nd a
bove
hav
e be
en r
epor
ted
but n
ot f
ully
aut
hent
icat
ed.
Stan
dard
ato
mic
wei
ghts
are
abr
idge
d to
fou
r si
gnif
ican
t fig
ures
.E
lem
ents
with
no
repo
rted
val
ues
in th
e ta
ble
have
no
stab
le n
uclid
es.
The
Int
erna
tiona
l Uni
on o
f Pu
re a
nd A
pplie
d C
hem
istr
y Pe
riod
ic T
able
of
the
Ele
men
ts (
Febr
uary
201
0 ve
rsio
n) is
the
prin
cipa
l sou
rce
of d
ata.
Som
e da
ta m
ay h
ave
been
mod
ifie
d.
Recommended