Basic Chemistry, 4/e Chapter 13: Reaction Rates & Chemical Equilibrium Karen Timberlake

Chapter 13 – Reaction Rates and Chemical Equilibrium 1. All of the following are factors that affect the rate of a reaction except A. changes in temperature. B. changes in orientation of the reactants. C. changes in concentration of the reactants. D. addition of catalysts. Answer: B

Chapter 13 – Reaction Rates and Chemical Equilibrium 1. All of the following are factors that affect the rate of a reaction except A. changes in temperature. B. changes in orientation of the reactants. C. changes in concentration of the reactants. D. addition of catalysts. Answer: B

Chapter 13 – Reaction Rates and Chemical Equilibrium 2. Which of the following statements about reversible reactions is not true? A. Consist of both a forward and a reverse reaction B. The forward reaction begins as collisions occur between the reactant molecules C. Are always complete D. Begin once there are sufficient product molecules to undergo collisions Answer: C

Chapter 13 – Reaction Rates and Chemical Equilibrium 2. Which of the following statements about reversible reactions is not true? A. Consist of both a forward and a reverse reaction B. The forward reaction begins as collisions occur between the reactant molecules C. Are always complete D. Begin once there are sufficient product molecules to undergo collisions Answer: C

Chapter 13 – Reaction Rates and Chemical Equilibrium 3. Which one of the following is the equilibrium constant expression? A. Kc = reactants/products B. Kc = reactants × products C. Kc = products/reactants D. Kc = [reactants]2 × [products]2 Answer: C

Chapter 13 – Reaction Rates and Chemical Equilibrium 3. Which one of the following is the equilibrium constant expression? A. Kc = reactants/products B. Kc = reactants × products C. Kc = products/reactants D. Kc = [reactants]2 × [products]2 Answer: C

Chapter 13 – Reaction Rates and Chemical Equilibrium 4. A certain reaction has an equilibrium constant of 0.5. Calculate the constant for the reverse reaction. A. 0.25 B. 0.5 C. 1 D. 2 Answer: D

Chapter 13 – Reaction Rates and Chemical Equilibrium 4. A certain reaction has an equilibrium constant of 0.5. Calculate the constant for the reverse reaction. A. 0.25 B. 0.5 C. 1 D. 2 Answer: D

Chapter 13 – Reaction Rates and Chemical Equilibrium What effect would increasing the amount of CO have on the products of the following reaction? CuO + CO  Cu + CO2 A. It would raise the amount of both products. B. It would raise the amount of Cu. C. It would raise the amount of CO2. D. It wouldn’t have any effect on the products. Answer: A

Chapter 13 – Reaction Rates and Chemical Equilibrium What effect would increasing the amount of CO have on the products of the following reaction? CuO + CO  Cu + CO2 A. It would raise the amount of both products. B. It would raise the amount of Cu. C. It would raise the amount of CO2. D. It wouldn’t have any effect on the products. Answer: A

Chapter 13 – Reaction Rates and Chemical Equilibrium 6. Write the equilibrium equation for the following reaction: 2 ZnS + 3 O2  2 ZnO + 2 SO2 A. K = [ZnS]2[O]2 C. K = [ZnS]2[O2]3 [ZnO]2[SO2]2 [ZnO]2[SO2]2 B. K = [ZnO]2[SO2]2 D. K = [ZnO]2[SO2] [ZnS]2[O]2 [ZnS]2[O2]3 Answer: D

Chapter 13 – Reaction Rates and Chemical Equilibrium 6. Write the equilibrium equation for the following reaction: 2 ZnS + 3 O2  2 ZnO + 2 SO2 A. K = [ZnS]2[O]2 C. K = [ZnS]2[O2]3 [ZnO]2[SO2]2 [ZnO]2[SO2]2 B. K = [ZnO]2[SO2]2 D. K = [ZnO]2[SO2] [ZnS]2[O]2 [ZnS]2[O2]3 Answer: D

Chapter 13 – Reaction Rates and Chemical Equilibrium Write the equilibrium equation for the reverse of the following reaction: 2 NOCl  2 NO +Cl2 A. K = [NOCl]2 C. K = [NO]2[Cl]2 [NO]2[Cl]2 [NOCl]2 B. K = [NOCl]2 D. K = [NO]2[Cl2] [NO]2[Cl2] [NOCl]2 Answer: B

Chapter 13 – Reaction Rates and Chemical Equilibrium Write the equilibrium equation for the reverse of the following reaction: 2 NOCl  2 NO +Cl2 A. K = [NOCl]2 C. K = [NO]2[Cl]2 [NO]2[Cl]2 [NOCl]2 B. K = [NOCl]2 D. K = [NO]2[Cl2] [NO]2[Cl2] [NOCl]2 Answer: B

Chapter 13 – Reaction Rates and Chemical Equilibrium 8. What is the type of equilibrium when the reactants and products are in two or more states? A. Equilibrium with a small Kc B. Homogeneous equilibrium C. Equilibrium with a large Kc D. Heterogeneous equilibrium Answer: D

Chapter 13 – Reaction Rates and Chemical Equilibrium 8. What is the type of equilibrium when the reactants and products are in two or more states? A. Equilibrium with a small Kc B. Homogeneous equilibrium C. Equilibrium with a large Kc D. Heterogeneous equilibrium Answer: D

Chapter 13 – Reaction Rates and Chemical Equilibrium 9. Which of the following would not increase the rate of the reaction? 2SO2 + O2  2SO3 A. Adding SO2 B. Raising the temperature C. Adding a catalyst D. Removing some SO2 Answer: D

Chapter 13 – Reaction Rates and Chemical Equilibrium 9. Which of the following would not increase the rate of the reaction? 2SO2 + O2  2SO3 A. Adding SO2 B. Raising the temperature C. Adding a catalyst D. Removing some SO2 Answer: D

Chapter 13 – Reaction Rates and Chemical Equilibrium 10. The tendency for a system to adjust itself to compensate for stresses upon the system is known as A. non-equilibrium. B. Le Châtlier’s Principle. C. heterogeneous equilibrium. D. activation energy. Answer: B

Chapter 13 – Reaction Rates and Chemical Equilibrium 10. The tendency for a system to adjust itself to compensate for stresses upon the system is known as A. non-equilibrium. B. Le Châtlier’s Principle. C. heterogeneous equilibrium. D. activation energy. Answer: B

Chapter 13 – Reaction Rates and Chemical Equilibrium 11. According to Le Châtelier’s Principle, the only condition that has no effect on the reaction to remove stress is A. a catalysts. B. temperature. C. concentration. D. volume. Answer: A

Chapter 13 – Reaction Rates and Chemical Equilibrium 11. According to Le Châtelier’s Principle, the only condition that has no effect on the reaction to remove stress is A. a catalysts. B. temperature. C. concentration. D. volume. Answer: A

Chapter 13 – Reaction Rates and Chemical Equilibrium 12. What effect would increasing the amount of CO have on the products of the following reaction? CuO(s) + CO(g)  Cu(s) + CO2(g) A. It would raise the amount of both products. B. It would raise the amount of Cu. C. It would raise the amount of CO2. D. It wouldn’t have any affect on the products. Answer: A

Chapter 13 – Reaction Rates and Chemical Equilibrium 12. What effect would increasing the amount of CO have on the products of the following reaction? CuO(s) + CO(g)  Cu(s) + CO2(g) A. It would raise the amount of both products. B. It would raise the amount of Cu. C. It would raise the amount of CO2. D. It wouldn’t have any affect on the products. Answer: A

Chapter 13 – Reaction Rates and Chemical Equilibrium 13. What effect does raising temperature have on an endothermic reaction? A. Shifts the reaction toward reactants B. Shifts the reaction toward products C. Has no effect Answer: B

Chapter 13 – Reaction Rates and Chemical Equilibrium 13. What effect does raising temperature have on an endothermic reaction? A. Shifts the reaction toward reactants B. Shifts the reaction toward products C. Has no effect Answer: B

Chapter 13 – Reaction Rates and Chemical Equilibrium What effect would doubling the pressure have on the following reaction? 2 H2(g) + O2(g)  2 H2O(g) A. Shifts the reaction toward reactants B. Shifts the reaction toward products C. Has no effect Answer: B

Chapter 13 – Reaction Rates and Chemical Equilibrium What effect would doubling the pressure have on the following reaction? 2 H2(g) + O2(g)  2 H2O(g) A. Shifts the reaction toward reactants B. Shifts the reaction toward products C. Has no effect Answer: B

Chapter 13 – Reaction Rates and Chemical Equilibrium The following equation is an example of what kind of equilibrium? CO2(g) + C(s)  2 CO2(g) A. Physical equilibrium B. Non-equilibrium C. Homogeneous equilibrium D. Heterogeneous equilibrium Answer: D

Chapter 13 – Reaction Rates and Chemical Equilibrium The following equation is an example of what kind of equilibrium? CO2(g) + C(s)  2 CO2(g) A. Physical equilibrium B. Non-equilibrium C. Homogeneous equilibrium D. Heterogeneous equilibrium Answer: D