Chemistry 12 Provincial Workbook Unit 01: Reaction Kinetics. Multiple Choice Questions

Transcription

1 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 1 / 68 Chemistry 1 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?. Increasing the concentration of which of the following substances would cause the greatest increase in the reaction rate? A. H B. NO C. NO D. HO

2 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. / Which of the following are products in the overall reaction? A. I and II only B. I and IV only C. II and III only D. III and IV only I N II NO III NO IV HO 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... CH 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 CO B. the volume of HO C. the mass of CH3 COOH D. the surface area of NaHCO 3

3 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 3 / Consider the following reaction... Al(s)+3CuCl (aq) 3Cu(s)+AlCl (aq) 3 A g B. 0.1 g C g D g If 0.56 g Cu is produced in 1.0 minute, what mass of Al is used up in 0.0 seconds? 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

4 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 4 / Consider the following PE diagram for a reversible reaction 10. Consider the following reaction HO (l) HO(l) O (g) Which graph shows the relationship between rate of consumption of HO and time?

5 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 5 / Consider the following reaction Mg(s) HCl(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 1. Consider the following PE diagram

6 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 6 / 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. H (g) O (g) HO(g) B. Pb (aq) I (aq) PbI (s) C. 4Fe(s) 3O (g) FeO 3(s) Cu(s) Ag (aq) Cu (aq) Ag(s) D. 16. Consider the following reaction CH 4(g) O (g) CO (g) HO(g) At a certain temperature, 1.0 mol CH 4 is consumed in 4.0 minutes. The rate of production of HO is A. 0.5mol/min B. 0.50mol/min C..0mol/min D. 8.0mol/min

7 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 7 / 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?

8 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 8 / 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 0. Consider the following reaction involving 10. g of powdered zinc Zn(s) HCl(aq) ZnCl (aq) H (g) A. 1,, 3 B., 1, 3 C. 3, 1, D. 3,, 1 The rates, in order of fastest to slowest, are 1. 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

9 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 9 / 68. Consider the following potential energy diagram for a reversible reaction Which of the following describes the system above? 3. Increasing the temperature of a reaction increases the reaction rate by (1) increasing frequency of collisions, () 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 4. 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

10 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 10 / Consider the graph for the following reaction CaCO 3(s) HCl(aq) CaCl (aq) CO (g) HO(l) A. 0-1 minute B. 0 - minutes C. 0-3 minutes D. 0-4 minutes The average rate of reaction is greatest in the time interval 6. 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

11 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 11 / Consider the following potential energy diagram A. I B. II C. III D. IV Which of the following represents the heat of reaction, H, for the forward reaction? 8. When a catalyst is added to a reaction (1) the heat of reaction increases, () 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 9. Consider the following mechanism for a reaction A. Br is a reactant B. HBr is a product C. HOBr is a catalyst D. HOOBr is a reaction intermediate Step 01 HBr O HOOBr Step 0 HBr HOOBr HOBr Step 03 HBr HOBr HO Br Which of the following statements is correct?

12 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 1 / Which of the following reactions will be slowest at 5 C? A. Cu(s) S(s) CuS(s) B. H (aq) OH (aq) HO(l) C. Pb (aq) Cl (aq) PbCl (s) D. NaOCl(aq) NaCl(aq) O (g) 31. Which of the following could be used as the units for rate of a reaction? A. I only B. I and II only C. II and III only D. I, II and III 3. Consider the following reaction I. ml/sec II. g/min III. M/min Zn(s) HCl(aq) ZnCl (aq) H (g) A graph of concentration of HCl vs time could be represented by

13 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 13 / Consider the following experiments, each involving equal masses of zinc and 10.0 ml of acid A. I > II > III B. II > I > III C. III > I > II D. III > II > I The rate of reaction in order from fastest to slowest is 34. What happens to the energy of reactant molecules as they approach one another?

14 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 14 / Consider the following reaction mechanism: A. IO B. HO C. ClO D. ClOH 36. Consider the following reaction Step 01 ClO HO HClO OH Step 0 I HClO HIO Cl Step 03 HIO OH IO HO The catalyst is N (g) 3H (g) NH 3(g) If the rate of formation of NH3 is 4.0 x 10-4 mol/s, then the rate of consumption of H is A. B. C. D. 4.0x10 mol/sec 4 4.0x10 mol/sec 4 6.0x10 mol/sec 3 1.x10 mol/sec 37. Consider the following reaction Zn(s) HCl(aq) ZnCl (aq) H (g) Which of the following instruments could be used to monitor the rate of the reaction in an open system? A. I and II only B. I and III only C. II and III only D. I, II and III I. Balance II. Pressure gauge III. ph meter

15 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 15 / 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

16 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 16 / 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?

17 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 17 / 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: CaO(s) HCl(aq) CaCl (aq) HO(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 A. I B. II C. III D. IV The activation energy for the forward reaction is represented by

18 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 18 / 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 A. HOI is a product B. HO is a reactant C. HOCl is a catalyst D. OH is a reaction intermediate Step 01 ClO HO HClO OH Step 0 I HClO HIO Cl Step 03 HIO OH IO HO Which of the following is correct for the overall reaction? 51. Which of the following reactions is slowest at room temperature? A. NH 3(g) HCl(g) NH4Cl(s) B. MgCl (s) Ca(s) Mg(s) CaCl (s) C. HCl(aq) NaOH(aq) NaCl(aq) HO(l) D. Ba(NO 3 ) (aq) NaSO 4(aq) BaSO 4(s) NaNO 3(aq) 5. Consider the following reaction: COCl (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

19 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 19 / Which of the following reactions is endothermic? A. CH 4(g) O (g) CO (g) HO(l) 890.3kJ B. NaO (s) HO(l) 87.0kJ 4NaOH(aq) O (g) C. CaO(s) HO(l) Ca(OH) (aq), H 6.5kJ D. CaO(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. H3O I HI HO Step. HO HI HO HOI Step 3. HOI H3O I HO I Step 4. I I I3 In the above mechanism, which of the following is true for the overall reaction? A. HI is a catalyst B. HO 3 is a product C. HO is a reactant D. HO is an intermediate

20 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 0 / Consider the following reaction NH 4(l) HO (l) N (g) 4HO(l) In 5.0seconds, mol of HO is consumed. The rate of production of N is 3 A. 1.5x10 mol/sec 3 B. 3.0x10 mol/sec 3 C. 6.0x10 mol/sec D. 1.5x10 mol/sec 58. Consider the following reaction 3FeO 3(s) CO(g) Fe3O 4(s) CO (g) 46kJ Which of the following would cause the rate of the reaction to increase? A. removing the Fe3O 4 B. decreasing the temperature C. increasing the surface area of FeO 3 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?

21 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 1 / Consider the following potential energy diagram for a reaction A. -10 kj B. -30 kj C. +30 kj D. +10 kj What is the value of H for this reaction? 6. 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. C(s) O (g) CO (g) B. HO (l) HO(l) O (g) C. Al(s) 3CuCl (aq) AlCl 3(aq) 3Cu(s) D. NaCl(aq) AgNO 3(aq) AgCl(s) NaNO 3(aq) 64. Which factor explains why potassium generally reacts faster than sodium? A. surface area B. temperature C. concentration D. nature of reactants

22 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. / What happens to the PE and KE of the reactants particles as the activated complex is formed? 66. Consider the following PE diagram PE KE A. increases decreases B. increases increases C. decreases decreases D. decreases increases What are the values of H and activation energy for the forward reaction?

23 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 3 / Consider the following reaction mechanism A. Cl B. HCl C. CCl 3 D. CHCl 3 Which of the following is a reactant in the overall reaction? 68. Consider the following PE diagram for a catalyzed and uncatalyzed reaction Which of the following describes the reverse reaction?

24 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 4 / Which of the following could be used to describe the rate of a reaction? A. B. C. D. change in time change in mass change in mass change in volume change in volume change in time change in volume change in mass 70. Consider the following reaction HO (aq) HO(l) O (g) Which factor explains why the above reaction speeds up in the presence of MnO (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?

25 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 5 / Consider the following PE diagram Which of the following describes the type of reaction and H for the reverse reaction?

26 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 6 / Consider the following diagram for a catalyzed and uncatalyzed reaction: Which of the following describes the forward reaction?

27 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 7 / Consider the following PE diagram: Which of the following is true for the forward reaction? 75. Consider the following reaction... NO(g)+O (g) NO (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.

28 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 8 / Consider the following reaction mechanism... A. O B. O C. O 3 D. O 4 Which of the following could represent the activated complex for Step? 77. If the rate of production of CO 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 C0H4(s) B. pressure of HO(g) C. surface area of C0H4(s) D. concentration of C0H4(s)

29 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 9 / 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? A. I and II only B. II and III only C. III and IV only D. I, II and III only I. high concentration II. sufficient energy III. correct geometry IV. presence of a catalyst 81. Which of the following graphs most likely represents the slowest forward reaction?

30 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 30 / 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... A. O B. O C. NO D. NO Which of the following substances is the catalyst? 85. Which of the following could represent the units for reaction rate? A. g/ml B. g / min C. g / mol D. mol / L

31 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 31 / Consider the following reaction... Zn(s)+HCl(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 H D. an increase in the concentration of ZnCl 87. Consider the following reaction: H (g)+i (g) HI(g) Which of the following is true of the activated complex relative to the reactants?

32 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 3 / 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) H (g)+i (g) HI(g) B. Cu(s)+Cl (g) CuCl (s) C. KOH(aq)+H SO (aq) H O(l)+K SO (aq) D. 4 4

33 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 33 / Nitrogen monoxide and hydrogen react according to the following equation... NO(g)+H (g) N (g)+h O(g) If the rate of hydrogen consumption is g per minute, what is the rate of nitrogen production? A g/min B. 0.61g/min C. 1.g/min D..4g/min 9. A student placed 3.0 g of Mg into some HCl in two different experiments. In each case, it reacted according the following equation... Mg(s)+HCl(aq) MgCl (aq)+h (g) In the first experiment, it took 3. 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. H was decreased. C. The 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

34 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 34 / Consider the following reaction... H (g)+i (g) HI(g) As a molecule of H approaches a molecule of I on a collision course, how do the KE and PE change? 95. Which of the following reactions is endothermic? A. H (g)+s(s) HS(g)+0kJ B. 4Fe(s)+3O (g) - 81kJ 3 C. CO (g) D. N (g)+3h (g) 3 Fe O (s) C(s)+O (g), ΔH=+393kJ NH (g), ΔH=-9kJ 96. A reaction has the following mechanism: A. H B. NO C. HO D. NO Which of the following substances is a reaction intermediate?

35 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 35 / Which of the following could NOT be units for reaction rate? -1 A. sec B. g/ml C. M/min D. C/hour 98. Which of the following represents the typical mathematical relationship between reaction rate and time?

36 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 36 / Consider the following reaction... Zn(s)+HCl(aq) ZnCl (aq)+h (g) In two different experiments, equal moles of Zn and equal volumes of HCl are reacted. After minutes, the volume of H produced is recorded as follows... Which of the following factors explains why the rate in Experiment 1 is different than the rate in Experiment? A. HCl B. temperature C. nature of reactants D. surface area of Zn

37 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 37 / Consider the following reaction... Which of the following could be true of the activated complex?

38 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 38 / 68 Written Questions 1. Consider the following reaction mechanism for the formation of NO. A. Complete Step. ( marks) B. Define the term reaction intermediate. ( marks) C. Identify a reaction intermediate in the above mechanism. ( marks)

39 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 39 / 68. 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 CO gas for the times s (1 mark) 10-0s (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 0.0 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. ( marks)

40 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 40 / 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... C8H 58(s) 85O (g) 56CO (g) 58HO(g) A. Calculate the average rate of consumption of paraffin in g/min for the time interval 1.0 to 4.0 minutes. ( marks) B. Calculate the rate of CO production in mol/min for the time interval 1.0 to 4.0 minutes. ( marks)

41 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 41 / Consider the following proposed reaction mechanism A. Write the overall reaction. ( marks) B. Define the term catalyst and identify a catalyst in the above mechanism. ( marks) 5. Consider the following reaction C1H O 11(s) HO(g) 1C(s) The rate of decomposition of C1H O 11 is 0.75 mol/min. What mass of C is produced in 10.0 seconds? (3 marks) 6. Define the term activation energy. ( marks)

42 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 4 / Consider the reaction CH 4(g) 3O (g) CO (g) HO(g) At certain conditions, 0.15 mol CO is produced in.0 minutes. What is the rate of consumption of CH 4 in g/s? (3 marks) 8. Define the term reaction mechanism. ( marks) 9. Consider the reaction... (3 marks) Al(s) 6HCl(aq) AlCl (aq) 3H 3 A 10.0 g sample of Al reacts completely in excess HCl in s. What is the rate of production of H in mol/s? 10. Using collision theory, give two reasons why reactions occur more rapidly at a higher temperature. ( marks) 11. Consider the reaction... (3 marks) HO(l) H (g) O (g) The rate of production of O is decompose g HO? 1.x10 mol/sec. How many seconds will it take to

43 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 43 / Define the term catalyst. ( marks) 13. Using the axes below, sketch a PE diagram for the reacting system where... (3 marks) ΔH 30kJ/mol E a 50kJ/mol 14. Consider the following reaction mechanism A. Determine the overall reaction. ( marks)

44 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 44 / 68 B. Identify a reaction intermediate. (1 mark) 15. Consider the following reaction 3Cu(s)+8HNO (aq) 3Cu NO (aq)+no(g)+4h O(l) 3 3 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.0 to 6.0min. ( 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. ( marks)

45 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 45 / Consider the following reaction in an open flask CaCO (s) HCl(aq) CaCl (aq) H O(l) CO (g) 3 A g sample of CaCO 3(s) is placed in the flask and HCl(aq) is added. The reaction consumes HCl(aq) at an average rate of 0.00 mol/min for 10.0 min. What mass of CaCO 3(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 Mg(s)+HBr(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)

46 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 46 / 68 B. Decreasing the temperature (1 mark) C. Increasing the surface area of Mg (1 mark) 0. 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)

47 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 47 / The release of O (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. ( marks) Experiment 1 Experiment B. Identify a variable from experiment 1 and how it was changed to produce the different reaction rate for experiment. Explain using collision theory. (3 marks). When solid sodium is placed in water at room temperature, an immediate, violent reaction occurs... Na(s)+H O(l) NaOH(aq)+H (g)+energy A. Describe two methods that could be used to experimentally determine the rate of the reaction. ( marks) Method 1 Method

48 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 48 / 68 B. Would you expect the activation energy of this reaction to be high or low? Explain using collision theory. ( marks) High or Low? Explanation 3. Consider the following overall reaction which is exothermic... NO(g)+O (g) NO (g) A. Complete the proposed two step reaction mechanism... ( marks) B. Describe how adding a catalyst would affect the activation energy and the H for the overall reaction... ( marks) 4. Consider the following reaction mechanism... A. Identify a reaction intermediate in the reaction mechanism. (1 mark) B. Write the overall reaction. ( marks) C. Explain why increasing the carbon monoxide concentration will increase the reaction rate but increasing the chlorine gas concentration will not. ( marks)

49 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 49 / Consider the reaction... Zn(s)+O (g) ZnO(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 0 (1 mark) Explanation (1 mark) 6. A catalyzed decomposition of ozone ( O 3 ) 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. ( marks)

50 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 50 / 68 B. On the PE diagram below sketch a curve that could represent the mechanism for the catalyzed decomposition. ( marks) 7. A student burned a paraffin candle ( C5H 5 ) in an open beaker according to the following equation... C H (s)+38o (g) 5CO (g)+6h O(g) 5 5 The following data was recorded... Calculate the rate of paraffin consumption in moles of 5 5 C H per minute then calculate how long it would take to produce 0.70 g of carbon dioxide. (4 marks)

51 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 51 / 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)

52 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 5 / 68 Multiple Choice Questions Answer Key 1 D 1 D 41 D 61 B 81 A A A 4 B 6 D 8 C 3 B 3 B 43 A 63 D 83 A 4 C 4 D 44 A 64 D 84 C 5 A 5 A 45 B 65 A 85 B 6 A 6 B 46 A 66 A 86 B 7 C 7 D 47 C 67 D 87 D 8 B 8 A 48 B 68 A 88 D 9 D 9 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 1 C 3 C 5 B 7 B 9 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 0 C 40 B 60 C 80 B 100 D

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62 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 6 /

63 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 63 /

64 R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 64 / End of Unit 01 Provincial Exam Workbook