1. © 2015 Pearson Education, Inc. Clicker Questions Chapter 15 Barbara Mowery York College

2. © 2015 Pearson Education, Inc. At equilibrium, the rate of the forward reaction is _______ the rate of the reverse reaction. a.equal to b.slower than c.faster than d.the reverse of

3. © 2015 Pearson Education, Inc. At equilibrium, the rate of the forward reaction is _______ the rate of the reverse reaction. a.equal to b.slower than c.faster than d.the reverse of

4. © 2015 Pearson Education, Inc. The reaction quotient Q is usually represented by a.[reactants] / [products]. b.[products] / [reactants]. c.[reactants]  [products]. d.[reactants] + [products].

5. © 2015 Pearson Education, Inc. The reaction quotient Q is usually represented by a.[reactants] / [products]. b.[products] / [reactants]. c.[reactants]  [products]. d.[reactants] + [products].

6. © 2015 Pearson Education, Inc. Select the statement that best describes a system at equilibrium. a.The reaction is complete because all reactants have become products. b.The reaction has stopped because all of the catalyst has been used. c.As soon as product molecules form, other molecules of product become reactants. d.The reaction stops when the amounts of reactants and products reach equilibrium amounts.

7. © 2015 Pearson Education, Inc. Select the statement that best describes a system at equilibrium. a.The reaction is complete because all reactants have become products. b.The reaction has stopped because all of the catalyst has been used. c.As soon as product molecules form, other molecules of product become reactants. d.The reaction stops when the amounts of reactants and products reach equilibrium amounts.

8. © 2015 Pearson Education, Inc. Which reaction quotient represents the reaction shown? Co(s) + 2 H + (aq)  Co 2+ (aq) + H 2 (g) a. b. c. d.

9. © 2015 Pearson Education, Inc. Which reaction quotient represents the reaction shown? Co(s) + 2 H + (aq)  Co 2+ (aq) + H 2 (g) a. b. c. d.

10. © 2015 Pearson Education, Inc. If the value of the equilibrium constant is large, then at equilibrium mostly _______ will be present. a.reactants b.products c.catalysts d.water

11. © 2015 Pearson Education, Inc. If the value of the equilibrium constant is large, then at equilibrium mostly _______ will be present. a.reactants b.products c.catalysts d.water

12. © 2015 Pearson Education, Inc. If the value of the equilibrium constant is small, then at equilibrium mostly _______ will be present. a.reactants b.products c.catalysts d.water

13. © 2015 Pearson Education, Inc. If the value of the equilibrium constant is small, then at equilibrium mostly _______ will be present. a.reactants b.products c.catalysts d.water

14. © 2015 Pearson Education, Inc. Q = the reaction quotient K = the equilibrium constant At equilibrium, which is true? a.Q > K b.Q < K c.Q = K d.Q 2 = K

15. © 2015 Pearson Education, Inc. Q = the reaction quotient K = the equilibrium constant At equilibrium, which is true? a.Q > K b.Q < K c.Q = K d.Q 2 = K

16. © 2015 Pearson Education, Inc. K = 2.39 for the gaseous reaction SO 2 Cl 2  SO 2 + Cl 2. For a mixture where Q = 5.21 to reach equilibrium, the concentration of SO 2 Cl 2 must _____. a.increase b.decrease c. remain the same d. change in a way that cannot be predicted

17. © 2015 Pearson Education, Inc. K = 2.39 for the gaseous reaction SO 2 Cl 2  SO 2 + Cl 2. For a mixture where Q = 5.21 to reach equilibrium, the concentration of SO 2 Cl 2 must _____. a.increase b.decrease c. remain the same d. change in a way that cannot be predicted

18. © 2015 Pearson Education, Inc. Equilibrium constants typically have units of a.M. b.M 2. c.M 1−. d.None of the above

19. © 2015 Pearson Education, Inc. Equilibrium constants typically have units of a.M. b.M 2. c.M 1−. d.None of the above

20. © 2015 Pearson Education, Inc. Reaction quotients for heterogeneous equilibria do not include concentrations of a.pure liquids. b.pure solids. c.Both of the above d.Neither of the above

21. © 2015 Pearson Education, Inc. Reaction quotients for heterogeneous equilibria do not include concentrations of a.pure liquids. b.pure solids. c.Both of the above d.Neither of the above

22. © 2015 Pearson Education, Inc. HA  H + + A − [HA] = 1.65  10 –2 M and [H + ] = [A – ] = 5.44  10 –4 M at equilibrium. K c = _______. a.1.79  10 −2 b.1.79  10 −3 c.1.79  10 −4 d.1.79  10 −5

23. © 2015 Pearson Education, Inc. HA  H + + A − [HA] = 1.65  10 –2 M and [H + ] = [A – ] = 5.44  10 –4 M at equilibrium. K c = _______. a.1.79  10 −2 b.1.79  10 −3 c.1.79  10 −4 d.1.79  10 −5

24. © 2015 Pearson Education, Inc. K P = K C when a.the reaction is at equilibrium. b.the reaction is exothermic. c.all of the gases present are at the same pressure. d.the number of moles of gas on both sides of the balanced equation is the same.

25. © 2015 Pearson Education, Inc. K P = K C when a.the reaction is at equilibrium. b.the reaction is exothermic. c.all of the gases present are at the same pressure. d.the number of moles of gas on both sides of the balanced equation is the same.

26. © 2015 Pearson Education, Inc. CO 2 + H 2  CO + H 2 O If all species are gases and H 2 is added, the concentration of CO at equilibrium will a.increase. b.decrease. c.remain unchanged. d.disappear.

27. © 2015 Pearson Education, Inc. CO 2 + H 2  CO + H 2 O If all species are gases and H 2 is added, the concentration of CO at equilibrium will a.increase. b.decrease. c.remain unchanged. d.disappear.

28. © 2015 Pearson Education, Inc. CO 2 + H 2  CO + H 2 O If all species are gases and H 2 O is added, the equilibrium concentration of CO a.will increase. b.will decrease. c.will remain unchanged. d.will disappear.

29. © 2015 Pearson Education, Inc. CO 2 + H 2  CO + H 2 O If all species are gases and H 2 O is added, the equilibrium concentration of CO a.will increase. b.will decrease. c.will remain unchanged. d.will disappear.

30. © 2015 Pearson Education, Inc. CO 2 + H 2  CO + H 2 O If all species are gases and CO 2 is removed, the [CO] at equilibrium will a.increase. b.decrease. c.remain unchanged. d.disappear.

31. © 2015 Pearson Education, Inc. CO 2 + H 2  CO + H 2 O If all species are gases and CO 2 is removed, the [CO] at equilibrium will a.increase. b.decrease. c.remain unchanged. d.disappear.

32. © 2015 Pearson Education, Inc. CO 2 + H 2  CO + H 2 O Increasing the temperature of this endothermic reaction will _______ [CO] at equilibrium. a.increase b.decrease c.not change d.eradicate

33. © 2015 Pearson Education, Inc. CO 2 + H 2  CO + H 2 O Increasing the temperature of this endothermic reaction will _______ [CO] at equilibrium. a.increase b.decrease c.not change d.eradicate

34. © 2015 Pearson Education, Inc. CO 2 + H 2  CO + H 2 O Increasing the temperature of this endothermic reaction will _______ the value of K. a.decrease b.increase c.not change d.change unpredictably

35. © 2015 Pearson Education, Inc. CO 2 + H 2  CO + H 2 O Increasing the temperature of this endothermic reaction will _______ the value of K. a.decrease b.increase c.not change d.change unpredictably

36. © 2015 Pearson Education, Inc. CO 2 + H 2  CO + H 2 O If all species are gases and the container is compressed, the amount of CO will a.increase. b.decrease. c.remain unchanged. d.vanish.

37. © 2015 Pearson Education, Inc. CO 2 + H 2  CO + H 2 O If all species are gases and the container is compressed, the amount of CO will a.increase. b.decrease. c.remain unchanged. d.vanish.

38. © 2015 Pearson Education, Inc. CO 2 + H 2  CO + H 2 O Adding a catalyst to this reaction will cause the [CO] at equilibrium to a.increase. b.decrease. c.remain unchanged. d.cease to exist.

39. © 2015 Pearson Education, Inc. CO 2 + H 2  CO + H 2 O Adding a catalyst to this reaction will cause the [CO] at equilibrium to a.increase. b.decrease. c.remain unchanged. d.cease to exist.

40. © 2015 Pearson Education, Inc. Ni(CO) 4 (g)  Ni(s) + 4 CO(g) Adding nickel to this reaction will cause the equilibrium to a.shift toward products. b.shift toward reactants. c.remain unchanged. d.change based on the amount added.

41. © 2015 Pearson Education, Inc. Ni(CO) 4 (g)  Ni(s) + 4 CO(g) Adding nickel to this reaction will cause the equilibrium to a.shift toward products. b.shift toward reactants. c.remain unchanged. d.change based on the amount added.