STUDENT NUMBER: ____________________

2014 TRIAL HSC EXAMINATION Chemistry

General Instructions Reading time - 5 minutes Working time - 3 hours Write using black or blue pen Draw diagrams using pencil Board-approved calculators may be

used A data sheet and Periodic Table are

provided Write your Student Number at the top

of this page and other pages where indicated.

Total marks – 100

Section I Pages 2-17

75 marksThis section has two parts, Part A and Part B

Part A – 20 marks Attempt Questions 1-20 Allow about 35 minutes for this part

Part B – 55 marks Attempt Questions 21 – 32 Allow about 1 hour and 40 minutes for

this part

Section II Pages – 19-20

25 marks Attempt ALL sections of Question 33 Allow about 45 minutes for this section

2014 Year 12 Chemistry Trial Examination

SECTION I 75 marks

Part A - 20 marksAttempt Questions 1-20Allow about 35 minutes for this part

Use the multiple–choice sheet for Questions 1-20.________________________________________________________________________________

1. Which of the following is formed when bromine water reacts with 2-pentene in the absence of UV light?

A. 2-bromopentane

B. 2-bromopentene

C. 2, 3-dibromopentane

D. 1, 2-dibromopentane

2. Which of the following lists the best conditions for the yeast-catalysed fermentation of glucose to form ethanol?

A. A solution of glucose, a temperature between 30°C and 40°C, a low oxygen concentration

B. A solution of glucose, a temperature between 30°C and 40°C, a high oxygen concentration

C. A solution of glucose, a temperature between 40°C and 50°C, a low oxygen concentration

D. A solution of glucose, a temperature between 40°C and 50°C, a high oxygen concentration

3. Which list contains only transuranic elements?

A. Curium, Californium, Americium

B. Bismuth, Radon, Francium

C. Palladium, Radon, Lawrencium

D. Lead, Uranium, Americium

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4. What is the systematic name for the monomer used in the production of PVC?

A. Polyvinyl chloride

B. Vinyl chloride

C. Polychloroethene

D. Chloroethene

5. An iron nail was placed in a solution of copper sulfate. After some time the nail was covered with a reddish brown coating, and the blue colour of the solution had become lighter. Which of the following best explains these observations?

A. Copper ions gain electrons from the iron nail

B. Iron ions gain electrons from the copper in solution

C. Copper ions lose electrons to the iron nail

D. Iron ions lose electrons to the copper in solution

6. Which fuel produces the lowest amount of carbon dioxide per mole of reactant?

A. Ethanol

B. Methane

C. Ethylene

D. Propane

7. Some radioisotopes used for medical purposes are produced on-site at the hospital by the decay of other unstable isotopes sourced from a nuclear reactor. What is the main reason for producing the required isotope at the hospital?

A. Nuclear reactors cannot produce a variety of different isotopes at the same time, so some

need to be produced elsewhere

B. Transport of some isotopes is too dangerous

C. Alpha ray emitters cannot be transported with other radioisotopes because they may cause

the other isotopes to decay faster

D. The short half-lives of these isotopes means it will decay before it can be transported to the

hospital

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8. Consider the following reaction:

Zn (s) + 2H+ (aq) + 2 MnO2 (s) Zn2+ (aq) + Mn2O3 (s) + H2O (l)

What is the oxidant in this reaction?

A. H+

B. MnO2 (s)

C. Zn(s)

D. Mn2O3 (s)

9. In aqueous solution aluminium ions (Al3+) react with water producing insoluble aluminium hydroxide in the following equilibrium:

Al3+ (aq) + 3H2O(l) ↔ Al(OH)3 (s) + 3H+

(aq)

Under which conditions would the concentration of aluminium ions decrease in aqueous solution?

A. The concentration would be unaffected by pH

B. pH = 7

C. pH < 7

D. pH > 7

10. The pH of sulfuric acid solution is measured at 2.0 by a pH meter. Which of the following alternatives shows the correct concentrations of hydrogen and sulfate ions in this solution? (Assume sulfuric acid is a strong acid)

Concentration of hydrogen ions in solution (mol/L)

Concentration of sulfate ions in solution (mol/L)

A. 1.0 x 10-2 5.0 x 10-3

B. 1.0x 10-2 1.0 x 10-2

C. 1.0 x 10-1 2.0 x 10-2

D. 1.0 x 10-1 5.0 x 10-1

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11. 50 mL of 0.200 mol L-1 hydrochloric acid was diluted to 2000 mL with distilled water. What is the pH of the diluted hydrochloric acid solution?

A. 1.0

B. 1.7

C. 2.0

D. 2.3

12. Which of the following 4 carbon atom molecules has the highest boiling point?

A. Butane

B. 2-Butanol

C. Ethyl ethanoate

D. Butanoic acid

13. Which substance is amphoteric in dilute solutions?

A. Calcium carbonate

B. Sodium hydrogen sulfate

C. Ethanol

D. Ammonium nitrate

14. 0.10 mL of 0.10 mol L-1 HCl is added to a small beaker of each of the following liquids. In which case would the pH remain the same?

A. A solution of ethanol and glucose, at equal concentrations

B. A solution of ammonia and ammonium chloride, at equal concentrations

C. Distilled water

D. A solution of ethanol and ethanoic acid, at equal concentrations

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15. Which of the following is NOT an acid/base conjugate pair?

A. HCl / Cl-

B. H2O / OH-

C. H2SO4 / SO42-

D. NH4+

/ NH3

16. Why is the density of ozone different to that of oxygen?

A. The ozone molecule is larger so it takes up more space compared to an oxygen

molecule so its density is lower.

B. Their densities are different because one mole of ozone occupies a bigger volume than

one mole of oxygen if measured at the same temperature and pressure

C. The dipole-dipole attractions between ozone molecules pulls them closer together to

give ozone a higher density

D. The mass of a single molecule of ozone is 1 ½ times that of a molecule of oxygen

17. A student tested a substance with a number of indicators. Her results are shown below.

Indicator Colour change pH range Student’s results

Phenolphthalein Colourless – red 8.3 – 10.0 Colourless

Methyl orange Red – yellow 3.1 – 4.4 Yellow

Methyl red Pink – yellow 4.4 – 6.0 Yellow

Phenol red Yellow – red 6.8 – 8.4 Yellow

What is the substance most likely to be?

A. Carbonated soft drink

B. Pure water

C. Milk

D. Ammonia

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18. The formula for CFC-112 is CCl3CClF2. What is the correct systematic name for this molecule?

A. 1,1,1,2-tetrachloro-2,2-difluoroethane

B. 1,2,2,2-tetrachloro-1,1-difluoroethane

C. 1,1-difluoro-1,2,2,2-tetrachloroethane

D. 2,2-difluoro-1,1,1,2-tetrachloroethane

19. Which of the following gases can cause major depletion of the ozone layer?

A. O2

B. NO

C. CO2

D. CCl2F2

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20. Which of the following graphs best illustrates the layered structure of the atmosphere?

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STUDENT NUMBER: ____________________Section I (continued)

Part B -55 marksAttempt Questions 21 - 32Allow about 1 hour and 40 minutes for this part.

Answer the questions in the spaces provided. These spaces provide guidelines for the expected length of response.

Show all relevant working in questions involving calculations.________________________________________________________________________________

MarksQuestion 21 (3 marks)Compare addition polymerisation and condensation polymerisation, using named examples and equations. 3

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Question 22 (5 marks) MarksThe following image was found during an investigation about biopolymers.

Assess the validity of the claims made by this source by referring to both a petroleum-based polymer and a recently developed polymer. 5

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Question 23 (6 marks) MarksThe following galvanic cell was constructed:

a) On the diagram, clearly label the anode, cathode and the direction of electron flow. 1

b) Write a balanced net ionic equation for the overall cell reaction. 1

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c) Calculate the standard cell potential (E°). 1

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d) The cell voltage measured was less than the calculated E° value. Propose a possible reason

for this difference. 1

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e) Propose TWO reasons why this particular galvanic process is unsuitable as the basis for

development of a commercial cell. 2

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Question 24 (5 marks) MarksA radioactive decay series is shown in the diagram below:

a) Identify an instrument which could be used to detect radiation. 1

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b) Write an equation to show the α-decay of 1

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c) Write an equation to show the β-decay of 1

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d) Explain why the radioactive decay stops when is formed. 2

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Question 25 (4 marks) Marks

A student wanted to compare the molar heat of combustion of 1-pentanol with that of ethanol. To do this, they burned 2.15 g of 1-pentanol to heat 300.0 mL of water from 10.0oC to 38.0oC.

a) Using the student’s data, calculate the molar heat of combustion of 1-pentanol. 2

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b) How would you expect the student's value to compare with the theoretical value for

1-pentanol found in Chemical Data books? Explain your answer. 2

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Question 26 (4 marks)As part of your course work, you prepared an indicator from a natural material.

a) Outline the procedure used to prepare the natural indicator. 2

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b) Outline how you determined whether the indicator you produced was appropriate for

determining the acid/base nature of a substance. 2

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Question 27 (3 marks) MarksA student mixed 1-pentanol and methanoic acid together and heated them under reflux with concentrated sulfuric acid.

a) Draw the structural formula of the products formed. 2

b) Outline TWO reasons why sulfuric acid was added. 1

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Question 28 (5 marks)When 2.50 L of HBr gas and 1.60 L of NH3 gas, measured at 25°C and 100kPa, are mixed, ammonium bromide is formed as a white solid.

a) Demonstrate, using equations, that this is an acid-base reaction, using Bronsted-Lowry definitions. 2

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b) Calculate the mass of ammonium bromide formed in this reaction. 3

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Question 29 (6 marks) MarksSulfur dioxide is an acidic oxide that produces acid rain.

a) Identify an industrial source of sulfur dioxide. 1

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b) Explain, using balanced equations, how sulfur dioxide produces acid rain. 2

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c) Describe the effects of acid rain. 3

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Question 30 (5 marks) MarksA 250mL container of 2.0 mol L-1 sulfuric acid was dropped, breaking and spilling its contents. Sodium hydrogen carbonate powder was sprinkled over this spill to neutralise it.

a) Write the chemical equation for this neutralisation reaction. 1

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b) What minimum mass of sodium hydrogen carbonate should be used to neutralise the acid spill? 2

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c) Would it be practical to use this minimal mass of sodium hydrogen carbonate? Justify your answer. 2

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Question 31 (4 marks)

a) Use chemical equations to demonstrate how ozone is produced in the stratosphere. 2

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b) Explain why there is concern about the loss of ozone and the appearance of a hole in the ozone layer. 2

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Question 32 (5 marks) MarksThe Haber process produces ammonia (NH3) from nitrogen and hydrogen gases.

a) Identify ONE impact of this on World history. 1

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b) Industrially this process is carried out at moderate temperatures. Explain why this condition is necessary. 2

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c) In the industrial process the ammonia and the unreacted nitrogen and hydrogen are cooled. The ammonia liquefies and is collected while the nitrogen and hydrogen gases are recycled back into the reaction vessel. Referring to the structure and bonding of each of the components explain why ammonia liquefies but the nitrogen and hydrogen do not. 2

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Section II

25 marksAllow about 45 minutes for this section.

Answer parts a) and b) of the question in examination writing booklet 1.Answer parts c) and d) of the question in examination writing booklet 2.Answer parts e) of the question in examination writing booklet 3.

Extra writing paper is available.

Show all relevant working in questions involving calculations.

Page

Question 33 Industrial Chemistry……………….…..………………………..….19-20

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Question 33 – Industrial Chemistry (25 marks) Marks

a) Hydrogen sulfide can be removed from natural gas and then converted to elemental sulfur by the Claus process which is described by the equation below.

2 H2S(g) + SO2 (g) 3 S (s) + 2 H2O (g) H = -145 kJ mol-1

i. Write the equilibrium expression for this reaction.

ii. Calculate the equilibrium constant, when 2.00 mol of H2S and 1.50 mol of SO2

react in a 2.00 L vessel at 373 K to give 0.80 mol of water vapour under

equilibrium conditions.

iii. What would be the effect of changing the volume of the vessel to 1.00 L?

iv. At a higher temperature, would the equilibrium constant be higher or lower?

Explain your answer.

b) A first hand investigation was performed to observe the electrolysis of a concentrated solution of sodium chloride. Identify the reactions that occur at the anode and cathode and give equations for these reactions.

c) This is a diagram of a micelle.

i. Identify the type of surfactant shown in the diagram.

ii. Account for the cleaning action of this surfactant.

QUESTION 33 continued on the next page.

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d) This diagram summarises the Solvay process.

i. Identify substance X.

ii. Write an equation to show the reaction which occurs in the carbonating tower.

iii. Describe how you carried out the step in part ii) in the school laboratory, indicating how it would be different form the industrial process.

e) A chemical company is considering building two new industrial plants. One will be used for the production of sodium carbonate and the other for production of sodium hydroxide. The map shows three sites, labelled A, B and C, being considered for the location of the industrial plants. Assess the suitability of the three sites for locating industrial plants to produce each compound.

END OF PAPER

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