2. 1) In which of the following systems would the number of moles of the substances present at equilibrium NOT be shifted by a change in the volume of the system at constant temperature?
a) CO(g) + NO(g)  CO2(g) + ½ N2(g)
b) N2(g) + 3H2(g)  2NH3(g)
c) N2(g) + 2O2(g)  2NO2(g)
d) N2O4  2NO2
e) NO(g) + O3(g)  NO2(g) + O2(g)

3. E

4. 2) Which of the following is the correct equilibrium expression for the hydrolysis of CO32-?
(a) K = [HCO3-]
[CO32-][H3O+]
(b) K = [HCO3-][OH-]
[CO32-]
(c) K = [CO32-][OH-]
[HCO3-]
(d) K = [CO32-]
[CO2][OH-]2
(e) K = [CO32-][H3O+]

5. B

6. 3) For the reaction whose rate law is second order, a plot of which of the following is a straight line?
a) [X] versus time
b) Log [X] versus time
c) 1/[X] versus time
d) [X] versus 1/time
e) Log [X] versus 1/time

7. C

8. 4) (CH3)3CCl(aq) + OH-  (CH3)3COH(aq) + Cl-
For the reaction represented above, the experimental rate law is given as follows.
Rate = k[(CH3)3CCl]
If some solid sodium hydroxide is added to a solution that is molar in (CH3)3CCl and 0.10-molar in NaOH, which of the following is true? (Assume temp and vol remain constant)
a) Both the reaction rate and k increase
b) Both the reaction rate and k decrease
c) Both the reaction rate and k remain the same.
d) The reaction rate increases but k remains the same
e) The reaction rate decreases but k remains the same

9. C

10. 5) Relatively slow rates of chemical reaction are associated with which of the following?
a) The presence of a catalyst
b) High Temperature
c) High Concentration of reactants
d) Strong Bonds in reactant molecules
e) Low Activation energy

11. D

12. 6) H2C2O H2O  2H3O+ + C2O42-
Oxalic Acid, H2C2O4, is a diprotic acid with K1 = 5.36 x 10-2 and K2 = 5.3 x For the reaction above, what is the equilibrium constant?
(a) x 10-2
(b) 5.3 x 10-5
(c) 2.8 x 10-6
(d) 1.9 x 10-10
(e) 1.9 x 10-13

13. C

14. PCl3(g) + Cl2(g)  PCl5(g) + energy
Some PCl3 and Cl2 are mixed in a container at 200oC and the system reaches equilibrium according to the equation above. Which of the following causes an increase in the number of moles of PCl5 present at equilibrium?
I) Decrease the volume of the container
II) Raising the temperature
III) Adding a mole of He Gas at constant volume
a) I Only
b) II Only
c) III Only
d) II and III only
e) I, II, and III

15. A

16. 8) 4 HCl (g) + O2 (g)  2Cl2 (g) + 2H­2O(g)
Equal numbers of moles of HCl and O2 in a closed system are allowed to reach equilibrium as represented by the equation above. Which of the following must be true at equilibrium?
I. [HCl] must be less than [Cl2]
II. [O2] must be greater than [HCl]
III. [Cl2] must equal [H2O]
a) I only
b) II only
c) I and III only
d) II and III only
e) I, II, and III

17. D

18. 9) 2SO2 (g) + O2 (g)  2 SO3 (g)
When 0.40 mole of SO2 and 0.60 mole of O2 are placed in an evacuated 1.00L flask, the reaction represented above occurs. After the reactants and the products reach equilibrium and the initial temperature is restored, the flask is found to contain 0.30 mole of SO3. Based on the results, the equilibrium constant Kc, for the reaction is
a) 20
b) 10
c) 6.7
d) 2.0
e) 1.2

19. A

20. 10) Which of the following best describes the role of the spark from the spark plug in an automobile engine?
a) The spark decreases the energy of activation for the slow step.
b) The spark increases the concentration of the volatile reactant.
c) The spark supplies some of the energy of activation for the combustion reaction.
d) The spark provides a more favorable activated complex for the combustion reaction.
e) The spark provides the heat of vaporization for the volatile hydrocarbon.

21. C

22. 11. 2SO3 (g)  2SO2 (g) + O2 (g)
After the equilibrium represented above is established, some pure O2 (g) is injected into the reaction vessel at constant temperature. After equilibrium is reestablished, which of the following has a lower value compared to its value at the original equilibrium?
a) Keq for the reaction
b) The total pressure in the reaction vessel
c) The amount of SO3 (g) in the reaction vessel
d) The amount of O2(g) in the reaction vessel
e) The amount of SO2 (g) in the reaction vessel

23. E

24. 12. 2 NO(g) + O2 (g)  2 NO2 (g) Delta H <0
Which of the following changes alone would cause a decrease in the value of Keq for the reaction represented above?
a) Decreasing the Temperature
b) Increasing the temperature
c) Decreasing the volume of the reaction vessel
d) Increasing the volume of the reaction vessel
e) Adding a catalyst

25. B

26. 13. H3AsO4 + 3 I– + 2 H3O+ --> H3AsO3 + I3– + H2O
The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the stoichiometry shown above. The experimental rate law of the reaction is:
Rate = k[H3AsO4] [I–] [H3O+]
What is the order of the reaction with respect to I-?
(A) 1 (C) 3 (E) 6
(B) 2 (D) 5

27. A

28. H3AsO4 + 3 I– + 2 H3O+ --> H3AsO3 + I3– + H2O
Rate = k[H3AsO4] [I–] [H3O+]
14. According to the rate law for the reaction, an increase in the concentration of hydronium ion has what effect on this reaction?
(A) The rate of reaction increases.
(B) The rate of reaction decreases.
(C) The value of the equilibrium constant increases.
(D) The value of the equilibrium constant decreases.
(E) Neither the rate nor the value of the equilibrium constant is changed.

29. A

30. A(g) + B(g)  2 C(g)
When the concentration of substance B in the reaction above is doubled, all other factors being held constant, it is found that the rate of the reaction remains unchanged. The most probable explanation for this observation is that
(A) the order of the reaction with respect to substance B is 1
(B) substance B is not involved in any of the steps in the mechanism of the reaction
(C) substance B is not involved in the rate–determined step of the mechanism, but is involved in subsequent steps
(D) substance B is probably a catalyst, and as such, its effect on the rate of the reaction does not depend on its concentration
(E) the reactant with the smallest coefficient in the balanced equation generally has little or no effect on the rate of the reaction

31. C

32. 16. For the reaction A(g)  B(g) + C(g), the equilibrium constant, Kp, is 2 x10–4 at 25oC. A mixture of the three gases at 25oC is placed in a reaction flask and the initial pressures are PA = 21 atmosphere, PB = 0.5 atmosphere, and PC = 1 atmosphere. At the instant of mixing, which of the following is true for the reaction as written?
(A) DG < 0 (C) DS = 0 (E) DGo < 0
(B) DG > 0 (D) DGo= 0

33. B

34. 17. HgO(s) + H2O  HgI42– + 2 OH–
Consider the equilibrium above. Which of the following changes will increase the concentration of HgI42– ?
(A) Increasing the concentration of OH–
(B) Adding 6 M HNO3
(C) Increasing the mass of HgO present
(D) Increasing the temperature
(E) Adding a catalyst

35. B

36. 18. Step 1. N2H2O2  N2HO2– + H+ (fast equilibrium)
Step 2. N2HO2– --> N2O + OH– (slow)
Step 3. H+ + OH– --> H2O (fast)
Nitramide, N2H2O2, decomposes slowly in aqueous solution. This decomposition is believed to occur according to the reaction mechanism above. The rate law for the decomposition of nitramide that is consistent with this mechanism is given by which of the following?
(A) Rate = k [N2H2O2]
(B) Rate = k [N2H2O2] [H+]
(C) (D) (E) Rate = k [N2H2O2] [OH–]

37. C