(04) WMP/Jan11/CHEM2

Transcription

1 Kinetics

2 4 2 The diagram below shows a Maxwell Boltzmann distribution for a sample of gas at a fixed temperature. E a is the activation energy for the decomposition of this gas. Number of molecules with a given energy E a Energy 2 (a) (i) On this diagram, sketch the distribution for the same sample of gas at a higher temperature. 2 (a) (ii) With reference to the Maxwell Boltzmann distribution, explain why an increase in temperature increases the rate of a chemical reaction. (Extra space)... (04) WMP/Jan11/CHEM2

3 5 2 (b) Dinitrogen oxide (N 2 O) is used as a rocket fuel. The data in the table below show how the activation energy for the decomposition of dinitrogen oxide differs with different catalysts. 2N 2 O(g) 2N 2 (g) + O 2 (g) E a / kj mol 1 Without a catalyst 245 With a gold catalyst With an iron catalyst With a platinum catalyst (b) (i) Use the data in the table to deduce which is the most effective catalyst for this decomposition. 2 (b) (ii) Explain how a catalyst increases the rate of a reaction. (Extra space)... 7 Turn over (05) WMP/Jan11/CHEM2

4 2 Section A Answer all questions in the spaces provided. 1 A student carried out an experiment to determine the rate of decomposition of hydrogen peroxide into water and oxygen gas. The student used 100 cm 3 of a 1.0 mol dm 3 solution of hydrogen peroxide at 298 K and measured the volume of oxygen collected. Curve R, in each of Figures 1, 2 and 3, shows how the total volume of oxygen collected changed with time under these conditions. 1 (a) Draw a curve on Figure 1 to show how the total volume of oxygen collected will change with time if the experiment is repeated at 298 K using 100 cm 3 of a 2.0 mol dm 3 solution of hydrogen peroxide. Figure 1 Volume of oxygen / cm 3 R Time / s 1 (b) Draw a curve on Figure 2 to show how the total volume of oxygen collected will change with time if the experiment is repeated at 298 K using 100 cm 3 of a 0.4 mol dm 3 solution of hydrogen peroxide. Figure 2 Volume of oxygen / cm 3 R Time / s (02) WMP/Jun12/CHEM2

5 3 1 (c) Draw a curve on Figure 3 to show how the total volume of oxygen collected will change with time if the original experiment is repeated at a temperature higher than 298 K. You should assume that the gas is collected at a temperature of 298 K. Figure 3 Volume of oxygen / cm 3 R Time / s 1 (d) Explain why the slope (gradient) of curve R decreases as time increases (Extra space)... Question 1 continues on the next page Turn over (03) WMP/Jun12/CHEM2

6 4 1 (e) The student discovered that hydrogen peroxide decomposes at a faster rate when a few drops of aqueous hydrogen bromide are added to the solution. The student found on the Internet that this decomposition is thought to proceed in two steps as shown by the following equations. Step 1 H 2 O 2 + HBr HBrO + H 2 O Step 2 HBrO + H 2 O 2 H 2 O + O 2 + HBr 1 (e) (i) Write an equation for the overall reaction. 1 (e) (ii) Give one reason, other than the increase in rate of reaction, why the student was able to deduce that hydrogen bromide behaves as a catalyst in this two-step reaction. 10 (04) WMP/Jun12/CHEM2

7 6 3 The diagram shows the Maxwell Boltzmann distribution of molecular energies in a gas at two different temperatures. V W X Y Energy 3 (a) One of the axes is labelled. Complete the diagram by labelling the other axis. 3 (b) State the effect, if any, of a solid catalyst on the shape of either of these distributions. 3 (c) In the, write the letter, V, W, X or Y, that represents the most probable energy of the molecules at the lower temperature. 3 (d) Explain what must happen for a reaction to occur between molecules of two different gases. (06) WMP/Jan12/CHEM2

8 7 3 (e) Explain why a small increase in temperature has a large effect on the initial rate of a reaction. 6 Turn over for the next question Turn over (07) WMP/Jan12/CHEM2

9 9 3 The diagram shows the Maxwell Boltzmann distribution for a sample of gas at a fixed temperature. E a is the activation energy for the decomposition of this gas. Number of molecules Energy E a E mp is the most probable value for the energy of the molecules. 3 (a) On the appropriate axis of this diagram, mark the value of E mp for this distribution. On this diagram, sketch a new distribution for the same sample of gas at a lower temperature. (3 marks) 3 (b) With reference to the Maxwell Boltzmann distribution, explain why a decrease in temperature decreases the rate of decomposition of this gas. 5 Turn over (09) WMP/Jun13/CHEM2

10 2 Section A Answer all questions in the spaces provided. 1 (a) Figure 1 shows the volume of hydrogen gas collected when a sample of magnesium reacted with an excess of dilute hydrochloric acid. The rate of this reaction can be studied by measuring the time it takes for a given volume of hydrogen to be collected. Figure 1 Volume of hydrogen / cm 3 W 1 (a) (i) State the meaning of the term rate of reaction. Time / s 1 (a) (ii) State and explain what has happened to the rate of this reaction at point W in Figure 1. (02) WMP/Jan13/CHEM2

11 3 1 (a) (iii) In terms of collision theory explain why, at a fixed temperature, the rate of this reaction doubles when the concentration of the hydrochloric acid doubles. 1 (b) In a study of the reaction in part (a), a student referred to activation energy. 1 (b) (i) State the meaning of the term activation energy. 1 (b) (ii) Complete Figure 2 by drawing the shape of the reaction profile from reactants to products for an exothermic reaction. Show the position of the products. Show and label the activation energy. Figure 2 Energy Reactants Question 1 continues on the next page Turn over (03) WMP/Jan13/CHEM2

12 4 2 Figure 2 shows the Maxwell Boltzmann distribution of molecular energies in a sample of gas at temperature T. Figure Y Energy 2 (a) One of the axes is labelled. Label the other axis. 2 (b) State why the curve starts at the origin. [1 mark] [1 mark] 2 (c) Which of the following, A, B or C, describes what the value of Y represents in Figure 2? Write the correct letter, A, B or C, in the. [1 mark] A The energy needed for a successful collision B The minimum energy needed for a reaction to occur C The most probable energy (04) WMP/Jun14/CHEM2

13 5 2 (d) On Figure 2, draw a distribution of molecular energies in this sample of gas at a higher temperature. [2 marks] 2 (e) The pressure of the original sample of gas is doubled at temperature T. State the effect, if any, of this change on the value of Y. [1 mark] 6 Turn over for the next question Turn over (05) WMP/Jun14/CHEM2

14 17 7 (c) A student determined a value for the enthalpy change when a sample of propanone was burned. The heat produced was used to warm some water in a copper calorimeter. The student found that the temperature of 150 g of water increased by 8.0 ºC when mol of pure propanone was burned in air. Use the student s results to calculate a value, in kj mol 1, for the enthalpy change when one mole of propanone is burned. (The specific heat capacity of water is 4.18 J K 1 g 1 ) [3 marks] Question 7 continues on the next page Turn over (17) WMP/Jun15/CHEM2

15 12 5 Methanol, for use as a fuel, can be produced by the reaction of carbon monoxide with hydrogen. CO(g) + 2H 2 (g) CH 3 OH(g) ΔH = 90 kj mol 1 The reaction is typically carried out at 300 ºC and Pa, in the presence of a catalyst. 5 (a) Figure 2 shows the Maxwell Boltzmann distribution for a mixture of carbon monoxide and hydrogen at 300 ºC. Figure 2 Number of molecules energy E a 5 (a) (i) Sketch a second curve on Figure 2 to show the distribution of molecular energies in this mixture at a higher temperature. [1 mark] 5 (a) (ii) Explain with reference to both curves in Figure 2 how a small change in temperature leads to a large change in the rate of reaction. [2 marks] (12) WMP/Jun16/CHEM2

16 22 8 (c) The rates of hydrolysis of two chloroalkanes can be investigated by adding aqueous silver nitrate to the chloroalkanes. During the hydrolysis reactions, chloride ions are liberated slowly. Precipitates of silver chloride are formed. Outline a method to compare the rate of hydrolysis of 1-chlorobutane with that of 2-chlorobutane. State how the method would ensure a fair test. [4 marks] 17 (22) WMP/Jun16/CHEM2