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2001 - Q8

 

The burning of sulfur can be described by the following equation:

 

          S (s) + O2 (g) --> SO2 (g)

 

What volume of sulfur dioxide gas will be released at 25'C and 101.3 kPa when 8.00 g of sulfur is burnt?

 

(A) 3.06 L

(B) 6.12 L

(C) 12.24 L

(D) 24.47 L

2001 - Q9

 

An understanding of Le Chatelier's Principle is important in the chemical industry. Which prediction can be made using the principle?

 

(A) The identity of products of a chemical reaction

(B) The effect of changes in temperature on the rates of reactions

(C) The effect of catalysts on the position of equilibrium reactions

(D) The effect of changes in the concentration of chemical substances in equilibrium

2002 - Q21 (7 marks)

 

Evaluate the impact of industrial sources of sulfur dioxide and nitrogen oxides on the environment, making use of appropriate chemical equations.

2002 - Q23 (4 marks)

 

A bottle of soft drink was placed on an electronic balance and weighed. The cap was removed and placed next to the bottle on the balance. The mass of the cap, bottle and its contents was monitored. The results are shown in the graph. The experiment was conducted at 25°C and 101.3 kPa. Assume that no evaporation has occurred.

 

 

 

 

 

 

 

 

 

 

 

 

(a) Identify the gas released (1 mark)

 

(b) Calculate the volume of the gas released (3 marks)

2002 - Q12

 

Oxides of nitrogen are produced by the combustion of coal. The percentage of these compounds remaining in emissions can be reduced using the methods named in the graph.

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Which of the following is the most effective method for removing oxides of nitrogen produced by the combustion of coal?

 

(A) Low nitrogen oxide burners

(B) Reburning technologies

(C) Ammonia-injecting scrubbers

(D) Selective catalytic scrubbers

2003 - Q7

 

The diagram is a representation of the Periodic Table. The positions of six different elements are shown.

2004 - Q9

 

Ozone reacts with nitric oxide according to the equation:                                                          NO(g) + O3(g) → NO2(g) + O2(g)

 

0.66 g NO(g) was mixed with 0.72 g O3(g).

What is the maximum volume of NO2(g) produced at 0°C and 100 kPa?

 

(A) 0.34 L

(B) 0.37 L

(C) 0.45 L

(D) 0.50 L

2004 - Q18 (4 marks)

 

Analyse the relationship between the position of elements in the Periodic Table, and the acid–base behaviour of their oxides.

2006 - Q22 (4 marks)

 

The atmosphere contains acidic oxides of sulfur which have been increasing in concentration since the Industrial Revolution.

 

Discuss the evidence for this statement, and include relevant balanced chemical equations.

2007 - Q22 (7 marks)

 

The following article was sourced from the internet.

 

In 2004, Australia’s Minister for the Environment announced that the allowable amounts of sulfur in unleaded petrol and diesel would be reduced over the next 5 years. Currently sulfur in diesel is 500 parts per million (ppm) but it will be cut to 50 ppm on 1 January 2006 and capped at 10 ppm from January 2009.

 

(a) Calculate the volume of sulfur dioxide produced when a full tank (capacity 60 kg) of diesel is consumed at 25°C and 100 kPa in November 2007. (3 marks)

 

(b) Evaluate the effect of the sulfur reduction policy on the environment. (4 marks)

2008 - Q20 (3 marks)

 

1.22 g of an unknown gas has a volume of 15.0 L at 100 kPa and 25°C.

 

(a) Calculate the molar mass of the gas.

 

(b) Identify the gas.

2009 - Q18 (5 marks)

 

There has been an increase in the concentration of the oxides of nitrogen in the atmosphere as a result of combustion.

 

Assess both the evidence to support this statement and the need to monitor these oxides.

2010 - Q26 (4 marks)

 

A gas is produced when 10.0 g of zinc is placed in 0.50 L of 0.20 mol L−1 nitric acid.

 

Calculate the volume of gas produced at 25°C and 100 kPa. Include a balanced chemical equation in your answer.

2008 - Q2

 

What are the volumes of one mole of argon, Ar, and one mole of fluorine, F2, at 0°C and 100 kPa?

2008 - Q7

 

Which of the following changes will always shift this equilibrium reaction to the right?

 

                                 2HI(g)         H2(g) + I2(g)        Î”H = –52 kJ

 

(A) Adding a catalyst

(B) Increasing the pressure

(C) Increasing the temperature

(D) Adding more of the reactant

2008 - Q9

 

Which of the following lower atmosphere pollutant gases is produced directly by the smelting of mineral ores?

 

(A) Carbon monoxide

(B) Nitrogen dioxide

(C) Ozone

(D) Sulfur dioxide

2009 - Q2

 

Unpolluted rain water in New South Wales is slightly acidic. Which substance is the major contributor to this acidity?

 

(A) Ozone

(B) Sulfur dioxide

(C) Carbon dioxide

(D) Nitrogen dioxide

2010 - Q19

 

Sodium azide is used in automobile airbags to provide a source of nitrogen gas for rapid inflation in an accident.The equation shows the production of nitrogen gas from sodium azide.

 

                                           2NaN3(s) → 2Na(s) + 3N2(g)

 

What mass of sodium azide will produce 40 L of N2 at 100 kPa and 0°C?

 

(A) 70 g

(B) 76 g

(C) 114 g

(D) 172 g

2011 - Q13

 

When chloride ions are added to a solution containing Co(H2O)6 2+ (aq), the following equilibrium is established.

 

              Co(H2O)6 2+ (aq) + 4Cl− (aq)  <----> CoCl4 2− (aq) + 6H2O(l)

                   Pink                                                  Blue

 

Which of the following statements about the colour of the solution is true?

 

(A) Diluting the solution with water will make it turn blue.

(B) If the reaction is exothermic, heating the solution will make it turn blue. (C) If the reaction is endothermic, cooling the solution will make it turn pink.

(D) Adding a large amount of solid potassium chloride to the solution will make it turn pink.

2011 - Q19

 

All of the carbon dioxide in a soft drink with an initial mass of 381.04 g was carefully extracted and collected as a gas. The final mass of the drink was 380.41 g.

 

What volume would the carbon dioxide occupy at 100 kPa and 25°C?

 

(A) 0.33 L

(B) 0.35 L

(C) 0.56 L

(D) 0.63 L

2012 - Q23 (3 marks)

 

Explain the impact of an increase in pressure and an increase in temperature on the solubility of carbon dioxide in water. Include a relevant equation in your answer.

2014 - Q29 (5 marks)

 

An experiment was performed to model the formation of acid rain.

 

A sample of sulfur was burned on a metal spoon. While alight, it was placed in a gas jar with some dry litmus paper.

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

When a fine mist of water was sprayed into the jar, the litmus paper turned red.

 

Assess the suitability of this experiment as a model for the formation of acid rain.

2016 - Q27 (4 marks)

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The volume of gas formed at 25°C and 100 kPa as hydrochloric acid was added to a pure sample of aluminium is shown in the graph.

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Calculate the original mass of the aluminium sample used in the reaction.

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2016 - Q28 (5 marks)

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A mixture of carbon monoxide, chlorine and phosgene (COCl2) gases was placed in a closed container. The concentrations of the gases were monitored over time.

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(a) At what time does the system first reach equilibrium? Justify your answer. (2 marks)

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(b) At four minutes, the temperature of the container was increased.

 

Explain, with reference to the graph, whether the decomposition of COCl2 into CO and Cl2 is exothermic or endothermic. (3 marks)

2012 - Q15

 

In which row of the following table are the listed oxides correctly classified?

2012 - Q16

 

The graph shows the concentrations over time for the system:

2013 - Q5

 

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.

2013 - Q6

 

A representation of the Periodic Table is shown. The positions of six different elements, P, Q, R, S, T and U are given.

2013 - Q14

 

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 

(B) 12.40 L

(C) 22.71 L

(D) 24.79 L

2014 - Q15

 

If exactly one gram of each of the following compounds is treated with excess hydrochloric acid, which would release the greatest volume of CO2(g) at 25°C and 100 kPa?

 

(A) K2CO3

(B) KHCO3

(C) Na2CO3

(D) NaHCO3

2015 - Q5

 

The oxides CaO, CO2, Na2O and N2O4 are placed in water to form four separate solutions.

 

Which row of the table correctly indicates the solutions with pH less than 7 and the solutions with pH greater than 7?

2015 - Q16

 

The equation describes an equilibrium reaction occurring in a closed system.

 

                           X(g) + Y(g) <---> 4Z(g)    H = +58 kJ

 

Under which set of conditions would the highest yield of Z(g) be obtained?

 

             Temperature (°C)               Pressure (kPa)

(A)                  50                                       100

(B)                  50                                       200

(C)                300                                       100

(D)               300                                       200

2016 - Q14

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Consider the following endothermic reaction taking place in a closed vessel.

 

                                             N2O4(g) <----> 2NO2(g)

 

Which of the following actions would cause more N2O4 to be produced?

(A) Adding a catalyst

(B) Decreasing the volume

(C) Decreasing the pressure

(D) Increasing the temperature

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