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R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 01), P. 1 / 68 Chemistry 12 Provincial Workbook Unit 01: Reaction Kinetics Multiple Choice Questions 1. Which of the following describes what happens to the KE and PE as an activated complex forms products? 2. Increasing the concentration of which of the following substances would cause the greatest increase in the reaction rate? A. 2 H B. NO C. 2 NO D. 2 HO

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Page 1: R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 01 ... · R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 01), P. 8 / 68 19. A chemical reaction that gives off energy

R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 01), P. 1 / 68

Chemistry 12 Provincial Workbook

Unit 01: Reaction Kinetics

Multiple Choice Questions 1. Which of the following describes what happens to the KE and PE as an activated

complex forms products?

2. Increasing the concentration of which of the following substances would cause the

greatest increase in the reaction rate?

A. 2H

B. NO

C. 2N O

D. 2H O

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R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 01), P. 2 / 68

3. Which of the following are products in the overall reaction?

I 2N

II 2 2N O

III 2N O

IV 2H O

A. I and II only B. I and IV only C. II and III only D. III and IV only 4. Which factor affects the reaction rate of heterogeneous reactions, but not of

homogeneous reactions? A. catalyst B. temperature C. surface area D. concentration 5. Consider the following reaction...

3 3 3 2 2CH COOH(aq)+NaHCO (s) NaCH COO(aq)+CO (g)+H O(l)

Which of the following properties could best be used to measure the reaction rate?

A. the volume of 2CO

B. the volume of 2H O

C. the mass of 3CH COOH

D. the surface area of 3NaHCO

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6. Consider the following reaction...

2 32Al(s)+3CuCl (aq) 3Cu(s)+2AlCl (aq)

If 0.56 g Cu is produced in 1.0 minute, what mass of Al is used up in 20.0 seconds?

A. 0.053 g B. 0.12 g C. 0.16 g D. 0.37 g 7. The average kinetic energy of colliding particles can be increased by… A. adding a catalyst B. increasing pressure C. increasing temperature D. increasing reactant concentration 8. A substance that increases the rate of a chemical reaction and may be recovered

unchanged at the end of the reaction is a(n)… A. product B. catalyst C. activated complex D. reaction intermediate

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9. Consider the following PE diagram for a reversible reaction…

10. Consider the following reaction…

2 2 2 22H O (l) 2H O(l) O (g)

Which graph shows the relationship between rate of consumption of 2 2H O and time?

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11. Consider the following reaction…

2 2Mg(s) 2HCl(aq) H (g) MgCl (aq)

The rate of this reaction increases when more magnesium is added. This change is caused by the…

A. addition of a catalyst B. increase in surface area C. change in nature of the reactants D. increase in concentration of reactants 12. Consider the following PE diagram…

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13. Which graph shows the relationship between activation energy and temperature?

14. A catalyst changes the rate of a reaction by…

A. changing H B. increasing the temperature C. decreasing the energy of the products D. providing an alternate reaction mechanism 15. At room temperature, which of the following reactions is fastest?

A. 2 2 22H (g) O (g) 2H O(g)

B. 2

2Pb (aq) 2I (aq) PbI (s)

C. 2 2 34Fe(s) 3O (g) 2Fe O (s)

D. 2Cu(s) 2Ag (aq) Cu (aq) 2Ag(s)

16. Consider the following reaction…

4 2 2 2CH (g) 2O (g) CO (g) 2H O(g)

At a certain temperature, 1.0 mol 4CH is consumed in 4.0 minutes. The rate of production of

2H O is…

A. 0.25mol/min

B. 0.50mol/min

C. 2.0mol/min

D. 8.0mol/min

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17. The changes in PE and KE, as reactant molecules approach each other, can be represented by…

18. Consider the following PE diagram…

Which of the following describes this reaction?

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19. A chemical reaction that gives off energy is…

A. exothermic and H is positive

B. exothermic and H is negative

C. endothermic and H is positive

D. endothermic and H is negative 20. Consider the following reaction involving 10. g of powdered zinc…

2 2Zn(s) 2HCl(aq) ZnCl (aq) H (g)

The rates, in order of fastest to slowest, are… A. 1, 2, 3 B. 2, 1, 3 C. 3, 1, 2 D. 3, 2, 1 21. Activation energy can be described as the… A. energy of motion B. energy of the activated complex C. energy difference between the reactants and the products D. energy difference between the reactants and the activated complex

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22. Consider the following potential energy diagram for a reversible reaction…

Which of the following describes the system above?

23. Increasing the temperature of a reaction increases the reaction rate by (1) increasing

frequency of collisions, (2) increasing the kinetic energy of collision, and/or (3) decreasing the potential energy of collision…

A. I only B. I and II only C. II and III only D. I, II and III 24. What effect does a catalyst have on a reaction?

A. It changes the H of a reaction B. It increases the kinetic energy of the reactants C. It decreases the potential energy of the products D. It provides a reaction mechanism with a lower activation energy

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25. Consider the graph for the following reaction…

3 2 2 2CaCO (s) 2HCl(aq) CaCl (aq) CO (g) H O(l)

The average rate of reaction is greatest in the time interval… A. 0 - 1 minute B. 0 - 2 minutes C. 0 - 3 minutes D. 0 - 4 minutes 26. Which of the following changes will increase the average kinetic energy of reactant

molecules? A. adding a catalyst B. increasing the temperature C. increasing the surface area D. increasing the concentration

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27. Consider the following potential energy diagram…

Which of the following represents the heat of reaction, H, for the forward reaction? A. I B. II C. III D. IV 28. When a catalyst is added to a reaction (1) the heat of reaction increases, (2) a new

mechanism is provided, and/or (3) the equilibrium constant increases… A. II only B. I and II only C. II and III only D. I, II and III 29. Consider the following mechanism for a reaction…

Step 01 2HBr O HOOBr

Step 02 HBr HOOBr 2HOBr

Step 03 2 22HBr 2HOBr 2H O 2Br

Which of the following statements is correct?

A. 2Br is a reactant

B. HBr is a product C. HOBr is a catalyst

D. HOOBr is a reaction intermediate

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30. Which of the following reactions will be slowest at 25°C? A. Cu(s) S(s) CuS(s)

B. 2H (aq) OH (aq) H O(l)

C. 2

2Pb (aq) 2Cl (aq) PbCl (s)

D. 22NaOCl(aq) 2NaCl(aq) O (g)

31. Which of the following could be used as the units for rate of a reaction?

I. mL/sec

II. g/min

III. M/min

A. I only B. I and II only C. II and III only D. I, II and III 32. Consider the following reaction…

2 2Zn(s) 2HCl(aq) ZnCl (aq) H (g)

A graph of concentration of HCl vs time could be represented by…

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33. Consider the following experiments, each involving equal masses of zinc and 10.0 mL of acid…

The rate of reaction in order from fastest to slowest is… A. I > II > III B. II > I > III C. III > I > II D. III > II > I 34. What happens to the energy of reactant molecules as they approach one another?

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35. Consider the following reaction mechanism:

Step 01 2ClO H O HClO OH

Step 02 I HClO HIO Cl

Step 03 2HIO OH IO H O

The catalyst is…

A. IO

B. 2H O

C. ClO

D. ClOH

36. Consider the following reaction…

2 2 3N (g) 3H (g) 2NH (g)

If the rate of formation of NH3 is 4.0 x 10-4 mol/s, then the rate of consumption of 2H is…

A. 42.0x10 mol/sec

B. 44.0x10 mol/sec

C. 46.0x10 mol/sec

D. 31.2x10 mol/sec

37. Consider the following reaction…

2 2Zn(s) 2HCl(aq) ZnCl (aq) H (g)

Which of the following instruments could be used to monitor the rate of the reaction in an open system?

I. Balance

II. Pressure gauge

III. pH meter

A. I and II only B. I and III only C. II and III only D. I, II and III

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38. Which of the following changes occur when the temperature of a reaction is increased?

I. H of the reaction increases

II. Frequency of the collisions increases

III. Kinetic energy of the reactants increases

A. I and II only B. I and III only C. II and III only D. I, II and III 39. Which of the following is true for an activated complex? A. stable and has low PE B. stable and has high PE C. unstable and has low PE D. unstable and has high PE 40. As you increase the temperature of a reaction, the… A. rate increases and the time required for the reaction increases B. rate increases and the time required for the reaction decreases C. rate decreases and the time required for the reaction increases D. rate decreases and the time required for the reaction decreases 41. Which of the following potential energy curves represents a catalyzed endothermic

reaction in the forward direction?

A. I B. II C. III D. IV

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42. The statement, the minimum energy needed to achieve a successful collision, defines A. entropy B. activation energy

C. the H of reaction D. the activated complex 43. As an activated complex changes to products… A. potential energy changes to kinetic energy B. kinetic energy changes to potential energy C. kinetic energy changes to activation energy D. potential energy changes to activation energy 44. Consider the following PE diagram for an uncatalyzed and a catalyzed reaction…

Which of the following describes the forward catalyzed reaction?

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45. A substance that increases the rate of a reaction without appearing in the equation for the overall reaction is a(n)…

A. product B. catalyst C. reactant D. intermediate 46. Consider the following reaction:

2 2CaO(s) 2HCl(aq) CaCl (aq) H O(l)

Which of the following could be used to measure the rate of this reaction?

A. change in acidity B. change in volume C. change in pressure D. change in total mass 47. In order for a collision between reactant particles to be successful…

A. H must be positive B. the system must be closed C. there must be sufficient KE D. the change in KE must be less than the change in PE 48. Consider the following PE diagram…

The activation energy for the forward reaction is represented by… A. I B. II C. III D. IV

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49. What is the relationship between the activation energy and the rate of a reaction? A. When the activation energy is high, the rate of reaction is fast B. When the activation energy is low, the rate of reaction is slow C. When the activation energy is high, the rate of reaction is slow D. There is no relationship between activation energy and rate of reaction 50. Consider the following reaction mechanism…

Step 01 2ClO H O HClO OH

Step 02 I HClO HIO Cl

Step 03 2

HIO OH IO H O

Which of the following is correct for the overall reaction?

A. HOI is a product

B. 2H O is a reactant

C. HOCl is a catalyst

D. OH is a reaction intermediate

51. Which of the following reactions is slowest at room temperature?

A. 3 4NH (g) HCl(g) NH Cl(s)

B. 2 2MgCl (s) Ca(s) Mg(s) CaCl (s)

C. 2HCl(aq) NaOH(aq) NaCl(aq) H O(l)

D. 3 2 2 4 4 3Ba(NO ) (aq) Na SO (aq) BaSO (s) 2NaNO (aq)

52. Consider the following reaction:

2 2COCl (g) CO(g) Cl (g)

Which of the following could be used to determine reaction rate in a closed system?

A. a decrease in gas pressure B. an increase in gas pressure C. a decrease in the mass of the system D. an increase in the mass of the system 53. Activation energy is defined as the…

A. H B. average kinetic energy C. energy of a particle’s motion D. minimum energy needed for a successful collision

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54. Which of the following reactions is endothermic?

A. 4 2 2 2CH (g) 2O (g) CO (g) 2H O(l) 890.3kJ

B. 2 2 2 22Na O (s) 2H O(l) 287.0kJ 4NaOH(aq) O (g)

C. 2 2CaO(s) H O(l) Ca(OH) (aq), H 62.5kJ

D. 2CaO(s) 3C(s) CaCl (s) CO(g), H 464.8kJ

55. The following diagram shows reactant molecules approaching one another…

What is happening to the kinetic energy and the potential energy?

56. A proposed mechanism for a reaction is…

Step 1. 3 2H O I HI H O

Step 2. 2 2 2H O HI H O HOI

Step 3. 3 2 2HOI H O I 2H O I

Step 4. 2 3I I I

In the above mechanism, which of the following is true for the overall reaction?

A. HI is a catalyst

B. 3H O is a product

C. 2 2H O is a reactant

D. 2H O is an intermediate

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57. Consider the following reaction…

2 4 2 2 2 2N H (l) 2H O (l) N (g) 4H O(l)

In 5.0seconds, 0.015 mol of 2 2H O is consumed. The rate of production of 2N is…

A. 31.5x10 mol/sec

B. 33.0x10 mol/sec

C. 36.0x10 mol/sec

D. 21.5x10 mol/sec

58. Consider the following reaction…

2 3 3 4 23Fe O (s) CO(g) 2Fe O (s) CO (g) 46kJ

Which of the following would cause the rate of the reaction to increase?

A. removing the 3 4Fe O

B. decreasing the temperature

C. increasing the surface area of 2 3Fe O

D. increasing the volume of the reaction vessel 59. Activation energy is described as A. the energy of the activated complex B. a point on the PE diagram where KE = PE C. the unstable high PE structural arrangement of atoms D. the minimum PE difference between the activated complex and the reactants

60. What happens to the activation energy and H when a catalyst is added to a reaction?

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61. Consider the following potential energy diagram for a reaction…

What is the value of H for this reaction? A. -120 kJ B. -30 kJ C. +30 kJ D. +120 kJ 62. A substance that is produced in one step in a reaction mechanism and consumed in a

subsequent step, without appearing in the overall reaction, is a(n) A. catalyst B. product C. reactant D. intermediate 63. Which of the following has the greatest reaction rate?

A. 2 2C(s) O (g) CO (g)

B. 2 2 2 22H O (l) 2H O(l) O (g)

C. 2 32Al(s) 3CuCl (aq) 2AlCl (aq) 3Cu(s)

D. 3 3NaCl(aq) AgNO (aq) AgCl(s) NaNO (aq)

64. Which factor explains why potassium generally reacts faster than sodium? A. surface area B. temperature C. concentration D. nature of reactants

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65. What happens to the PE and KE of the reactants particles as the activated complex is formed?

PE KE

A. increases decreases

B. increases increases

C. decreases decreases

D. decreases increases

66. Consider the following PE diagram…

What are the values of H and activation energy for the forward reaction?

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67. Consider the following reaction mechanism…

Which of the following is a reactant in the overall reaction? A. Cl

B. HCl

C. 3CCl

D. 3CHCl

68. Consider the following PE diagram for a catalyzed and uncatalyzed reaction…

Which of the following describes the reverse reaction?

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69. Which of the following could be used to describe the rate of a reaction?

A. change in time

change in mass

B. change in mass

change in volume

C. change in volume

change in time

D. change in volume

change in mass

70. Consider the following reaction…

2 2 2 22H O (aq) 2H O(l) O (g)

Which factor explains why the above reaction speeds up in the presence of 2MnO (s)?

A. temperature B. concentration C. nature of reactants D. presence of catalyst 71. What happens to the potential energy and the total energy as an activated complex

changes into products?

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72. Consider the following PE diagram…

Which of the following describes the type of reaction and H for the reverse reaction?

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73. Consider the following diagram for a catalyzed and uncatalyzed reaction:

Which of the following describes the forward reaction?

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74. Consider the following PE diagram:

Which of the following is true for the forward reaction?

75. Consider the following reaction...

2 22NO(g)+O (g) 2NO (g)

Why would this reaction probably involve more than one step?

A. There is insufficient activation energy. B. This reaction has high activation energy. C. Reactions between gases are typically slow. D. A successful collision between more than two molecules is unlikely.

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76. Consider the following reaction mechanism...

Which of the following could represent the activated complex for Step 2? A. O

B. 2O

C. 3O

D. 4O

77. If the rate of production of CO2 is 0.98g min, what is the rate of oxygen consumption?

A. 0.47g/min

B. 0.54g/min

C. 0.71g/min

D. 1.1g/min

78. Which of the following properties could best be monitored in order to determine the

reaction rate of the burning candle?

A. mass of C20H42(s) B. pressure of H2O(g) C. surface area of C20H42(s) D. concentration of C20H42(s)

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79. Which of the following is true of the kinetic and potential energies as reactant molecules approach each other to form an activated complex?

80. Which of the following are necessary for successful collisions between reactant

molecules?

I. high concentration II. sufficient energy III. correct geometry

IV. presence of a catalyst A. I and II only B. II and III only C. III and IV only D. I, II and III only 81. Which of the following graphs most likely represents the slowest forward reaction?

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82. For an exothermic reaction, which of the following is true? A. PE reactants > PE activated complex > PE products B. PE products > PE activated complex > PE reactants C. PE activated complex > PE reactants > PE products D. PE activated complex > PE products > PE reactants 83. Consider the following reaction...

Which of the following describes how the reaction’s catalyzed PE diagram compares to the reaction’s uncatalyzed PE diagram?

84. Consider the following reaction mechanism...

Which of the following substances is the catalyst? A. O

B. 2O

C. NO

D. 2NO

85. Which of the following could represent the units for reaction rate? A. g/mL

B. g / min

C. g / mol

D. mol / L

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86. Consider the following reaction...

2 2Zn(s)+2HCl(aq) ZnCl (aq)+H (g)

Which of the following would increase the reaction rate?

A. an increase in pressure B. an increase in temperature

C. an increase in the concentration of 2H

D. an increase in the concentration of 2ZnCl

87. Consider the following reaction:

2 2H (g)+I (g) 2HI(g)

Which of the following is true of the activated complex relative to the reactants?

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88. Consider the following PE diagram:

Which of the following is true for the forward reaction?

89. Which of the following could describe a catalyst? A. A substance that increases the reaction time. B. A substance that provides an alternate mechanism with a higher activation energy. C. A substance that is formed in one step and used up in a subsequent step in a reaction mechanism. D. A substance that is used up in one step and reformed in a subsequent step in a reaction mechanism. 90. Which of the following reactions is most likely to proceed at the greatest rate under

standard conditions? A. Zn(s) S(s) ZnS(s)

B. 2 2H (g)+I (g) 2HI(g)

C. 2 2Cu(s)+Cl (g) CuCl (s)

D. 2 4 2 2 42KOH(aq)+H SO (aq) 2H O(l)+K SO (aq)

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91. Nitrogen monoxide and hydrogen react according to the following equation...

2 2 22NO(g)+2H (g) N (g)+2H O(g)

If the rate of hydrogen consumption is 0.087 g per minute, what is the rate of nitrogen

production? A. 0.044g/min

B. 0.61g/min

C. 1.2g/min

D. 2.4g/min

92. A student placed 3.0 g of Mg into some HCl in two different experiments. In each

case, it reacted according the following equation...

2 2Mg(s)+2HCl(aq) MgCl (aq)+H (g)

In the first experiment, it took 3.2 minutes for all of the Mg to react. In the second experiment, it took 5.4 minutes for all of the Mg to react. Which of the following could account for the change in rate of the second experiment? A. A catalyst was added. B. The Mg was powdered.

C. The 2H was decreased.

D. The temperature was decreased. 93. Which of the following would change the value of the activation energy for a

heterogeneous reaction? A. adding a catalyst B. changing the surface area C. changing the temperature D. changing the average kinetic energy

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94. Consider the following reaction...

2 2H (g)+I (g) 2HI(g)

As a molecule of 2H approaches a molecule of 2I on a collision course, how do the KE and

PE change?

95. Which of the following reactions is endothermic?

A. 2 2H (g)+S(s) H S(g)+20kJ

B. 2 2 34Fe(s)+3O (g) - 821kJ 2Fe O (s)

C. 2 2CO (g) C(s)+O (g), ΔH=+393kJ

D. 2 2 3N (g)+3H (g) 2NH (g), ΔH=-92kJ

96. A reaction has the following mechanism:

Which of the following substances is a reaction intermediate?

A. 2H

B. NO

C. 2H O

D. 2N O

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97. Which of the following could NOT be units for reaction rate?

A. -1sec

B. g/mL

C. M/min D. °C/hour

98. Which of the following represents the typical mathematical relationship between

reaction rate and time?

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99. Consider the following reaction...

2 2Zn(s)+2HCl(aq) ZnCl (aq)+H (g)

In two different experiments, equal moles of Zn and equal volumes of HCl are reacted. After

2 minutes, the volume of 2H produced is recorded as follows...

Which of the following factors explains why the rate in Experiment 1 is different than the rate

in Experiment 2?

A. HCl

B. temperature C. nature of reactants D. surface area of Zn

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100. Consider the following reaction...

Which of the following could be true of the activated complex?

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Written Questions

1. Consider the following reaction mechanism for the formation of 2NO .

A. Complete Step 2. (2 marks)

B. Define the term reaction intermediate. (2 marks)

C. Identify a reaction intermediate in the above mechanism. (2 marks)

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2. An Alka-Seltzer tablet is added to water to produce carbon dioxide gas. The gas was collected using water displacement.

A. Calculate the average rate of reaction for the formation of 2

CO gas for the times...

0-10s (1 mark)

10-20s (1 mark)

B. Suggest a reason why the rate of reaction from 0 to 10.0 s is slower than the rate from 10.0 to 20.0 s? (1 mark)

C. The rate of reaction is not constant during the entire interval from 10.0 to 40.0 s. Describe the change in rate and explain a reason for the change. (2 marks)

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3. The mass of a burning candle is monitored to determine the rate of combustion of paraffin. An accepted reaction for the combustion of paraffin is...

28 58 2 2 22C H (s) 85O (g) 56CO (g) 58H O(g)

A. Calculate the average rate of consumption of paraffin in g/min for the time interval 12.0 to 24.0 minutes. (2 marks)

B. Calculate the rate of 2CO production in mol/min for the time interval 12.0 to 24.0 minutes.

(2 marks)

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4. Consider the following proposed reaction mechanism…

A. Write the overall reaction. (2 marks)

B. Define the term catalyst and identify a catalyst in the above mechanism. (2 marks)

5. Consider the following reaction…

12 22 11 2C H O (s) H O(g) 12C(s)

The rate of decomposition of 12 22 11C H O is 0.75 mol/min. What mass of C is produced in 10.0

seconds? (3 marks)

6. Define the term activation energy. (2 marks)

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7. Consider the reaction…

2 4 2 2 2C H (g) 3O (g) 2CO (g) 2H O(g)

At certain conditions, 0.15 mol 2

CO is produced in 2.0 minutes. What is the rate of

consumption of 2 4C H in g/s ? (3 marks)

8. Define the term reaction mechanism. (2 marks)

9. Consider the reaction... (3 marks)

3 22 6 2 3Al(s) HCl(aq) AlCl (aq) H

A 10.0 g sample of Al reacts completely in excess HCl in 300.0 s. What is the rate of

production of 2

H in mol/s?

10. Using collision theory, give two reasons why reactions occur more rapidly at a higher

temperature. (2 marks)

11. Consider the reaction... (3 marks)

2 2 22H O(l) 2H (g) O (g)

The rate of production of 2O is 21.2x10 mol/sec . How many seconds will it take to

decompose 100.0 g 2H O?

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12. Define the term catalyst. (2 marks)

13. Using the axes below, sketch a PE diagram for the reacting system where... (3

marks)

a

ΔH 30kJ/mol

E 50kJ/mol

14. Consider the following reaction mechanism…

A. Determine the overall reaction. (2 marks)

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B. Identify a reaction intermediate. (1 mark)

15. Consider the following reaction…

3 3 223Cu(s)+8HNO (aq) 3Cu NO (aq)+2NO(g)+4H O(l)

A piece of copper is added to a nitric acid solution in an open beaker, allowing the NO(g) to

escape. The following data was obtained…

A. Calculate the reaction rate for the time period 2.0 to 6.0min. (2 marks)

B. Calculate the mass of copper consumed in the first 5 minutes. (3 marks)

16. Using collision theory, explain why reactions between two solutions occur more

rapidly than reactions between two solids. (2 marks)

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17. Consider the following reaction in an open flask…

3 2 2 22CaCO (s) HCl(aq) CaCl (aq) H O(l) CO (g)

A 155.0 g sample of 3

CaCO (s) is placed in the flask and HCl(aq) is added. The reaction

consumes HCl(aq) at an average rate of 0.200 mol/min for 10.0 min. What mass of

3CaCO (s) remains? (3 marks)

18.

A. Write the equation for Step 3 in the following reaction mechanism. (1 mark)

B. Identify a reaction intermediate in the above mechanism. (1 mark)

19. Consider the following reaction…

2 2Mg(s)+2HBr(aq) MgBr (aq)+H (g)+energy

In terms of collision theory, describe how each of the factors below would influence the reaction rate.

A. Increasing the concentration of HBr (1 mark)

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B. Decreasing the temperature (1 mark)

C. Increasing the surface area of Mg (1 mark)

20. Consider the following reaction mechanism…

The overall reaction is exothermic. Sketch a PE diagram on the axes below to describe the energy changes that occur as the reaction takes place. (3 marks)

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21. The release of 2O (g) resulting from the decomposition of bleach was measured in

two different experiments. Data was collected and the following graph was drawn...

A. Calculate the average rate of reaction for each experiment. (2 marks)

Experiment 1

Experiment 2

B. Identify a variable from experiment 1 and how it was changed to produce the different reaction rate for experiment 2. Explain using collision theory. (3 marks)

22. When solid sodium is placed in water at room temperature, an immediate, violent

reaction occurs...

2 22Na(s)+2H O(l) 2NaOH(aq)+H (g)+energy

A. Describe two methods that could be used to experimentally determine the rate of the reaction. (2 marks)

Method 1

Method 2

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B. Would you expect the activation energy of this reaction to be high or low? Explain using collision theory. (2 marks)

High or Low?

Explanation

23. Consider the following overall reaction which is exothermic...

2 22NO(g)+O (g) 2NO (g)

A. Complete the proposed two step reaction mechanism... (2 marks)

B. Describe how adding a catalyst would affect the activation energy and the H for the overall reaction... (2 marks)

24. Consider the following reaction mechanism...

A. Identify a reaction intermediate in the reaction mechanism. (1 mark)

B. Write the overall reaction. (2 marks)

C. Explain why increasing the carbon dioxide concentration will increase the reaction rate but increasing the chlorine gas concentration will not. (2 marks)

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25. Consider the reaction...

22Zn(s)+O (g) 2ZnO(s)

State two different methods that would increase the rate of this reaction. Explain each in terms of collision theory.

Method 01 (1 mark)

Explanation (1 mark)

Method 02 (1 mark)

Explanation (1 mark)

26. A catalyzed decomposition of ozone ( 3O ) occurs in a series of steps as illustrated

below...

A. Write the equation for the overall reaction and then identify the catalyst in the spaces above. (2 marks)

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B. On the PE diagram below sketch a curve that could represent the mechanism for the catalyzed decomposition. (2 marks)

27. A student burned a paraffin candle ( 25 52C H ) in an open beaker according to the

following equation...

25 52 2 2 2C H (s)+38O (g) 25CO (g)+26H O(g)

The following data was recorded...

Calculate the rate of paraffin consumption in moles of 25 52C H per minute then calculate how

long it would take to produce 0.70 g of carbon dioxide. (4 marks)

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28. Consider the following reaction mechanism...

A. Write the equation for the overall reaction. (1 mark)

B. Given that the overall reaction is exothermic sketch a PE diagram for the mechanism on the axis provided. (3 marks)

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Multiple Choice Questions Answer Key

1 D 21 D 41 D 61 B 81 A

2 A 22 A 42 B 62 D 82 C

3 B 23 B 43 A 63 D 83 A

4 C 24 D 44 A 64 D 84 C

5 A 25 A 45 B 65 A 85 B

6 A 26 B 46 A 66 A 86 B

7 C 27 D 47 C 67 D 87 D

8 B 28 A 48 B 68 A 88 D

9 D 29 D 49 C 69 C 89 D

10 A 30 A 50 D 70 D 90 D

11 B 31 D 51 B 71 D 91 B

12 C 32 C 52 B 72 B 92 D

13 A 33 C 53 D 73 A 93 A

14 D 34 B 54 D 74 B 94 B

15 B 35 B 55 B 75 D 95 C

16 B 36 C 56 C 76 D 96 D

17 A 37 B 57 A 77 D 97 B

18 D 38 C 58 C 78 A 98 D

19 B 39 D 59 D 79 B 99 A

20 C 40 B 60 C 80 B 100 D

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Written Questions Answer Key 1.

2.

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3.

4.

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5.

6.

7.

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8.

9.

10.

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11.

12.

13.

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14.

15.

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16.

17.

18.

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19.

20.

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21.

22.

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23.

24.

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25.

26.

27.

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28.

End of Unit 01 Provincial Exam Workbook