1. Which of the following is equal for the forward and reverse ...

1. Which of the following is equal for the forward and reverse reactions at equilibrium
A) concentration
B) rates
C) rate constants
2. All chemical equilibria are _____ in nature.
A) dynamic
B) equal
C) static
D) kinetic
3. An example of a physical equilibrium is _____.
A)
B)
C)
D)
4. Which of the following is not a physical equilibrium
A) melting
B) allotropic transformation
C) vaporization
D) rusting
5. An example of heterogeneous equilibrium is _____.
A)
B)
C) Enzyme-catalyzed reactions
6. Which of the following statements is always correct
A) chemical equilibria are homogeneous
B) physical equilibria are homogeneous
C) physical equilibria are heterogeneous
D) chemical equilibria are heterogeneous
Page 1

7. The expression for K p for the reaction
is _____.
A) P CO2
B) P
HO 2
C)
D)
P CO2
P CO2
HO
/ P 2
HO
ท P 2
8. The expression for K p for the reaction
is _____.
A) 2P
SO 2 O
+ P 2
B) P
2 SO 2 O
ท P 2
C) P
SO 2 O
+ P 2
D) 2P
SO 2 O
/ P 2
9. The equilibrium constant K p is not applicable for the reaction _____.
A)
B)
C)
D)
10. The equilibrium constant K c for the reaction
A)
is given by _____.
B)
C)
D)
Page 2

11. The equation relating K p and K c is _____.
A) K p = K c (RT) ∆n
B) K p = K c RT ∆n
C) K c = K p RT ∆n
D) K c = K p (RT) ∆n
12. K p will be equal to K c if _____.
A) ∆n = 1
B) ∆n = 0
C) RT = 0
D) ∆n = ∞
13. K p will be less than K p if _____.
A) ∆H = negative
B) ∆n = positive
C) ∆n = negative
D) ∆n = 0
14. The equilibrium constants for the reactions
and
are x and y, respectively. The equilibrium constant for the reaction
A)
B) x + y
C) x – y
D) xy
is _____.
Use the following to answer questions 15-16:
The equilibrium constant for the reaction
is x.
Page 3

15. The equilibrium constant for the reaction
A) –x
B) x
C) 1/x
D) 2x
is _____.
16. The equilibrium constant for the reaction is _____.
A) 2x
B) x
C) x/2
D) x 2
17. The equilibrium constant for the reaction
is 4.17 ×
31
A) –4.17 × 10 −
B) 4.17 × 10 31
C) 2.40 × 10 30
D) 2.40× 10 -33
31
10 − . The equilibrium constant for the reaction
is
18. The number of moles of H 2 , S 2 , and H 2 S present at the equilibrium for the reaction
are 2.50, 1.35 × 10 -5 and 8.70 moles respectively in a 12 L flask. The equilibrium
constant, K c for the reaction is _____.
A) 1.08 × 10 7
B) 1.08 × 10 -7
C) 5.6 × 10 3
D) 7.2 × 10 -5
Page 4

19. Kc for the reaction
is 2.24 × 10 22 at 1273 บC. K p for the reaction at the same temperature is _____.
A) 7.16 × 10 -18
B) 1.76 × 10 20
C) 5.12 × 10 -15
D) 3.12 × 10 19
20. The equilibrium partial pressures of N 2 , O 2 and NO in the reaction
are 0.15, 0.33 and 0.050 atm, respectively at 2200ฐC. The value of K p for the reaction is
_____.
A) 5.1
B) 0.51
C) 51
D) 0.051
21. The equilibrium concentrations of NH 3 , N 2 and H 2 are 0.25 M, 0.11 M and 1.91 M,
respectively. The equilibrium constant K c for the reaction
A) 0.082
B) 8.2 × 10 -3
C) 8.2
D) 0.82
is _____.
22. The equilibrium constant, K c , for the reaction
is 0.082. What is K a for
A) 0.164
B) 0.041
C) 0.29
D) 1.64
Page 5

23. The equilibrium constant, K c , for the reaction
is 3.8 × 10 -5 at 727ฐC. The value of K p for the equilibrium
A) 648
B) 320
C) 32.0
D) 6.48
at the same temperature is _____.
24. The equilibrium pressure for the reaction
_____.
A) 0.105
B) 0.210
C) 1.05
D) 10.5
is 0.105 atm at 350ฐC. K p for the reaction is
25. K p for the reaction
same temperature is _____.
A) 4.21 × 10 3
B) 0.105
C) 3.05 × 10 -4
D) 2.05 × 10 -3
at 350 o C is 0.105. K c for the reaction at the
26. The equilibrium constant, K p, for the reaction
is 1.05 at 250ฐC. The reaction is started with PCl 5 , PCl 3 and Cl 2 at 0.177, 0.223 and
0.111 atm at 250ฐC. When the reaction comes to equilibrium, the pressure of _____.
A) PCl 3 must have decreased
B) Cl 2 must have decreased
C) PCl 5 must have decreased
D) PCl 5 must have increased
Page 6

27. Starting with only the solid, the total pressure of NH 3 and CO 2 was found to 0.363 atm
for the equilibrium
equilibrium constant, K p is
A) 7.1 × 10 -3
B) 2.5 × 10 -2
C) 5.3 × 10 -4
D) 3.6 × 10 -6
at 40ฐC. The
28. 1.05 moles of Br 2 in a 0.980 L container undergo 1.2% dissociation. The equilibrium
constant, K c for the reaction
A) 2.5 × 10 -5
B) 1.8 × 10 -3
C) 6.2 × 10 -4
D) 5.9 × 10 -6
is _____.
29. K p = K c for the reaction _____.
A)
B)
C)
D)
30. 3.00 × 10 -2 mol of phosgene gas, COCl 2 , was heated in a 1.50 L container at 800 K. At
equilibrium the pressure of CO was found to be 0.497 atm. The equilibrium constant, K p
for the reaction
A) 3.30
B) 9.80
C) 2.75
D) 5.61
is _____.
31. The equilibrium constant, K p for the reaction
at 2200ฐC is 0.051. The equilibrium constant, K c for the same reaction is _____.
A) 0.102
B) 0.051
C) 2.5 × 10 -3
D) 1.02 × 10 4
Page 7

Use the following to answer questions 32-33:
At equilibrium, nitrosyl bromide in the reaction
is 34% dissociated at 25ฐC and the total pressure is 0.25 atm.
32. The value of K p for the reaction is _____.
A) 9.6 × 10 -3
B) 1.39 × 10 -5
C) 3.8 × 10 -4
D) 6.7 × 10 -6
33. The value of K c for the above reaction is _____.
A) 1.6 × 10 -6
B) 2.7 × 10 -5
C) 3.9 × 10 -4
D) 4.5 × 10 -7
34. 2.50 mole of NOCl was heated in a 1.50 L vessel at 400ฐC.At equilibrium it was found
that 28.0% of the NOCl had dissociated. The equilibrium constant, K c of the reaction
A) 0.0353
B) 3.53 × 10 2
C) 3.53 × 10 -4
D) 3.53
is _____.
35. The ionization constants K c' and K c” for
were found to be 9.5 × 10 -8 and 1.0 × 10 -19 respectively. The equilibrium constant for
the reaction
A) 9.5 × 10 -8
B) 1.0 × 10 -19
C) 9.5 × 10 -27
D) 1.05 × 10 -12
is _____.
Page 8

36. The equilibrium constant, K c = 4.0 ื 10 -6 for the reaction
.
If the equilibrium constant, K c = 6.5 × 10 -2 for the reaction
the equilibrium constant for
A) 4.0× 10 -6
B) 6.1 × 10 -5
C) 1.6 × 10 4
D) 6.5 × 10 -2
,
is _____.
Use the following to answer questions 37-38:
The following equilibrium constants were measured for the reactions:
37. The equilibrium constant for the reaction
A) xy
B) x + y
C) xy 2
D) x + y 2
is _____.
38. The equilibrium constants K 1 and K 2 for the reactions above are
1.3 × 10 14 and 6.0 × 10 -3 , respectively. The equilibrium constant for the reaction
A) 4.7 × 10 9
B) 1.0 × 10 14
C) 1.0 × 10 26
D) 3.6 × 10 18
is _____.
Page 9

39. The equilibrium constants K 1 K 2 and K 3 for the reactions below are
K 1 = 4.2 × 10 52
K 2 = x
The value of K 2 is _____.
A) 9.8 × 10 28
B) 9.8 × 10 128
C) 6.7 × 10 12
D) 2.6 × 10 75
K 3 = 5.6 × 10 23 .
40. The equilibrium constant in terms of rate constants for the forward reaction, k f , and the
reverse reaction, k r , is given as _____.
A) kr
K = k
B) K = k f + k r
C) k
f
K = k
r
D) K = k f k r
f
41. The concentration of H + in pure water at 25ฐC is _____.
A) 10 -14 M
B) 10 -7 M
C) 10 -10 M
D) 10 -8 M
42. The equilibrium constant of a reaction is 12.6. If the rate constant of the reverse
reaction is 5.1 × 10 -2 , the rate constant for the forward reaction is _____.
A) 0.32
B) 0.16
C) 0.64
D) 0.08
43. Which of the following statements can be correct with respect to reaction quotient, Q
and equilibrium constant, K
A) Q < K
B) Q = K
C) Q > K
D) all the above
Page 10

44. The value of K c for the equilibrium
is 5.6 × 10 4 350ฐC. The initial pressures of SO 2 and O 2 in a mixture are 0.350 atm and
0.762 atm. The total pressure at equilibrium will be _____ atm.
A) less than 0.350
B) less than 0.741
C) less than 1.112
D) equal to 1.112
45. The value of Kc for the reaction is 1.2 . The
reaction is started with [H 2 ] 0 = 0.76 M, [N 2 ] 0 = 0.60 M and [NH 3 ] 0 = 0.48 M. Which of
the following is correct as the reaction comes to equilibrium
A) The concentration of N 2 will increase
B) The concentration of H 2 will decrease
C) The concentration of NH 3 will decrease
D) The concentration of both N 2 and H 2 will increase
Use the following to answer questions 46-48:
For the reaction
K c = 0.534 at 700ฐC
46. Calculate the number of moles of H 2 present at equilibrium if a mixture of 0.300 moles
of CO and 0.300 moles of H 2 O is heated to 700ฐC in a 10.0 L container.
A) 0.432 mol
B) 0.273 mol
C) 0.577 mol
D) 0.173 mol
47. Which statement is correct with respect to the above equilibrium when 0.30 moles of
CO and 0.30 moles of H 2 O are heated to 700ฐC and allowed to reach equilibrium.
A) [H 2 O] = [CO 2 ]
B) [CO 2 ] = [CO]
C) [H 2 O] = [CO]
D) [H 2 O] = [H 2 ]
Page 11

48. Which of the following statements is correct
A) All concentrations are equal
B) K p = K c
C) K p < K c
D) K p > K c
49. K p is 158 for the equilibrium
Starting with NO 2 (g) only, the partial pressure of O 2 at equilibrium is 0.25 atm.
Calculate the partial pressure of NO 2 at equilibrium.
A) 0.020 atm
B) 0.20 atm
C) 3.1 atm
D) 0.035atm
50. The partial pressure of NO in the above equilibrium is _____ atm.
A) 0.125
B) 0.50
C) 0.25
D) 0.02
51. The equilibrium constant Kc for the reaction is
2.18 × 10 6 . Starting with 3.20 moles of HBr in a 12.0L container, the concentration of
HBr at equilibrium is _____.
A) 0.167 M
B) 0.0267 M
C) 1.6 M
D) 0.267 M
52.
Kc is 3.8 × 10 -5 at 1000K for the equilibrium
Starting with 0.0456 moles of I 2 in a 2.30 L flask, at 1000 K, the equilibrium
concentration of I 2 at is:
A) 1.94 M
B) 0.0194 M
C) 0.12 M
D) 0.012 M
Page 12

Use the following to answer questions 53-54:
K c for the reaction is 4.63 × 10 -3 at 527ฐC .
53. Starting with pure phosgene, COCl 2 , at 0.760 atm, the equilibrium partial pressure of
CO is _____.
A) 0.352 atm
B) 0.0416 atm
C) 0.0352 atm
D) 0.416 atm
54. Starting with pure phosgene, COCl 2 , at 0.760 atm, the equilibrium partial pressure of
COCl 2 is _____.
A) 0.173 atm
B) 0.204 atm
C) 0.302 atm
D) 0.408 atm
55. What is the value of K c for the reaction
when the equilibrium concentrations of
CO, H 2 , CO 2 and H 2 O are 0.050 M, 0.045 M, 0.086 M and 0.040 M respectively
A) 0.074
B) 0.52
C) 0.063
D) 0.24
Use the following to answer questions 56-57:
The equilibrium constant K p for the reaction
total pressure at equilibrium is 4.50 atm.
is 1.52 and the
56. The equilibrium partial pressure of CO is _____ atm.
A) 0.86
B) 1.62
C) 1.96
D) 1.31
Page 13

57. The equilibrium partial pressure of CO 2 is _____ atm.
A) 2.54 atm
B) 0.98 atm
C) 1.27 atm
D) 0.72 atm
Use the following to answer questions 58-60:
The equilibrium constant, K c for the reaction
4.2. Initially 0.80 mole of H 2 and 0.80 mole CO 2 are placed in a 5.0 L flask.
is
58. The concentration of H 2 at equilibrium is _____.
A) 0.054 M
B) 0.025 M
C) 0.15 M
D) 0.029 M
59. At equilibrium, the concentration of H 2 is equal to the concentration of _____.
A) H 2 O
B) CO
C) CO 2
D) H 2 O + CO 2
60. The concentration of CO at equilibrium is _____.
A) 0.22M
B) 0.056M
C) 0.021M
D) 0.11M
61. Le Chโtelier's principle can help to predict how to maximize _____.
A) Reaction yield
B) Equilibrium constant
C) Temperature
D) Rate constant
Page 14

62. Which can alter the value of the equilibrium constant
A) Catalyst
B) Concentration
C) Pressure
D) Temperature
63. The equilibrium position of the reaction
by _____.
A) Removing SO 2
B) Adding Cl 2
C) Removing Cl 2
D) Removing SO 2 and Cl 2
can be shifted in the forward direction
Use the following to answer questions 64-65:
The equilibrium constant K c for the equilibrium
is x.
64. The equilibrium constant for the reaction
A) x/2
B) x 1/2
C) x 2
D) 2x
is _____.
65. The equilibrium constant for the reaction is _____.
A) x 2
B)
C) x –2
D) –2x
Page 15

66. Which of the following equilibria is not affected by pressure
A)
B)
C)
D)
67. The equilibrium
formation by _____. ∆H = 92.5 kJ.
A) Increasing temperature
B) Increasing pressure
C) Decreasing temperature
D) Increasing the concentration PCl 3
, can be shifted toward more product
68. The equilibrium
can shifted to the reactant side by _____. ∆H = –
198.2 kJ
A) Decreasing temperature
B) Decreasing volume
C) Decreasing pressure
D) Increasing the concentration of SO 2
69. The equilibrium pressure of NO2 in the equilibrium is 1.56
atm. Its pressure on the addition of a catalyst will be _____.
A) 1.06 atm
B) 0.75 atm
C) 1.56 atm
D) 2.71 atm
70. The position of the equilibrium can be shifted
to the left by the addition of _____ at constant pressure.
A) CO
B) He
C) O 2
D) KCl
Page 16

71. The addition of He to the equilibrium at
constant volume _____.
A) Shifts the equilibrium to the left
B) Increases K c
C) Shifts the equilibrium to the right
D) Has no effect
72. Which of the following will shift the equilibrium
A) Decrease of temperature
B) Addition of KCl
C) Addition of CO 2
D) Addition of NaOH solution
to the right
73.
The equilibrium
by _____.
A) increasing temperature
B) decreasing pressure
C) removing some CO 2
D) all of the above
can be shifted to the right
Use the following to answer questions 74-76:
Pure NOCl gas was heated to 240 ฐC in a 1.00-L container. At equilibrium the total pressure was
1.00 atm and the NOCl pressure was 0.64 atm.
74. The partial pressure of NO at equilibrium in the reaction
A) 0.24
B) 0.12
C) 0.34
D) 0.17
is _____ atm.
Page 17

75. The partial pressure of Cl 2 in the equilibrium
A) 0.36
B) 0.09
C) 0.12
D) 0.18
is _____ atm.
76. K p for the equilibrium
A) 1.7
B) 0.12
C) 0.17
D) 0.017
is _____.
Use the following to answer questions 77-78:
K p is 2.9 × 10 -11 at 530ฐC for the reaction
.
77. What is the partial pressure of NO at equilibrium when the equilibrium partial pressures
of N 2 and O 2 are 3.0 atm and 0.012 atm, respectively
A) 1.0 × 10 –6 atm
B) 1.6 × 10 –3 atm
C) 1.6 × 10 –2 atm
D) 0.16 atm
78. What is the partial pressure of NO at equilibrium under atmospheric conditions where
the partial pressures of N 2 and O 2 are 0.78 atm and 0.21 atm at 25ฐC K p for the reaction
is 4.0× 10 -31 at 25 ฐC.
A) 1.12 × 10 -12 atm
B) 2.6 × 10 -16 atm
C) 1.3 × 10 -8 atm
D) 1.45 × 10 -4 atm
Page 18

79. The thermal decomposition of NaHCO 3 (s) is favored by _____.
A) decreasing temperature
B) increasing temperature
C) increasing pressure
D) adding CO 2
80. K p < K c at 25 ฐC for which of the reactions below
A)
B)
C)
D)
81. The condition for maximum yield of NOCl 2 in the reaction
0
is _______. (
∆H f
0
∆H f
of NO = 90.4kJ/mol.)
A) high pressure, high temperature
B) low pressure, low temperature
C) low pressure, high temperature
D) high pressure, low temperature
of NOCl = 51.7 kJ/mol,
82. For the reaction
P A = 0.60 atm and P B = 0.60 atm at equilibrium at some temperature. K p for the reaction
is _____.
A) 1
B) 0.5
C) 1.7
D) 0.6
83. For the reaction
at equilibrium, the P A =0.60 atm and P B =0.60 atm and the total pressure is 1.2 atm. What
is the P A when the total pressure is increased to 1.5 atm
A) 0.69 atm
B) 0.81 atm
C) 0.75 atm
D) 0.91 atm
Page 19

84. The equilibrium mixture in the reaction
consists of 0.020 mole O 2 , 0.040 mole NO and 0.96 mole NO 2 . What is K p for the
reaction at 430ฐC and at a total pressure of 0.20 atm
A) 1.5 × 10 5
B) 7.2 × 10 4
C) 8.1 × 10 –3
D) 5.6 × 10 –6
85. Ammonium carbamate decomposes at a certain temperature .The equilibrium pressure
of the reaction
is 0.318 atm. K p for the reaction is _____.
A) 5.92 × 10 -5
B) 1.26 × 10 -4
C) 3.12 × 10 -6
D) 4.76 × 10 -3
Use the following to answer questions 86-88:
A mixture of 0.47 moles of H 2 and 3.59 moles of HCl is heated to 2800ฐC and allowed to reach
equilibrium. The total pressure at equilibrium is 2.00 atm.
K p = 193 at 2800ฐC.
86. The equilibrium pressure of H 2 is _____ atm.
A) 0.56 atm
B) 0.28 atm
C) 0.049 atm
D) 1.67 atm
87. The partial pressure of Cl 2 in the above equilibrium is _____ atm.
A) 0.28 atm
B) 0.049 atm
C) 0.56 atm
D) 0.49 atm
Page 20

88. The partial pressure of HCl in the above equilibrium is _____ atm.
A) 1.28 atm
B) 1.01 atm
C) 2.06 atm
D) 1.67 atm
89. Initially 1 mole of N 2 O 4 is placed in a vessel and allowed to reach equilibrium. The
relation between the degree of dissociation α, total pressure P and K p for the reaction
A)
2
4α
Kp = ⋅P
2
1−
α
B)
2
4α
Kp = ⋅P
2
(1 − α)
C)
2
α
Kp = ⋅P
2
1−
α
D)
2
2α
Kp = ⋅P
2
1−α
( )
is _____.
90. One mole of N 2 and three moles of H 2 are placed in a flask and allowed to reach
equilibrium. T = 375 บC. The mole fraction of NH 3 at equilibrium is found to be 0.21.
What is the total pressure of the system at equilibrium
A) 50 atm
B) 5 atm
C) 500 atm
D) 0.5 atm
91. What is [S 2 ] at equilibrium in the following reaction if [H 2 S] = 4.84 × 10 -3 M and [H 2 ] =
1.50 × 10 -3 M at equilibrium
A) 2.34 × 10 -2
B) 0.234 M
C) 2.34 × 10 -3 M
D) 2.34 × 10 -4 M
K c = 2.25 × 10 -4
Page 21

92. 6.75 g of SO 2 Cl 2 was placed in a 2.00L flask. At 648 K 0.0345 moles of SO 2 was
present. K c for the reaction
A) 3.83 × 10 -2
B) 4.71 × 10 -3
C) 1.12 × 10 -2
D) 6.12 × 10 -4
is _____.
Use the following to answer questions 93-95:
K p for the reaction
at 375ฐC is 4.31 × 10 -4 . The reaction
is started with 0.373 atm of H 2 and 0.862 atm of N 2 in a constant volume vessel.
93. The partial pressure of N 2 at equilibrium is _____ atm.
A) 0.260
B) 0.760
C) 0.860
D) 0.960
94. The partial pressure of H 2 at equilibrium is _____ atm.
A) 0.366
B) 0.166
C) 0.266
D) 0.566
95. The partial pressure of NH 3 at equilibrium is _____ atm.
A) 4.40 × 10 -3
B) 1.12 × 10 -2
C) 7.20 × 10 -4
D) 2.70 × 10 -5
Use the following to answer questions 96-97:
A 0.244 M fructose solution was prepared and it was found that at equilibrium the fructose
concentration had decreased to 0.113 M.
Page 22

96. The equilibrium constant for the reaction is _____.
A) 2.06
B) 5.16
C) 4.27
D) 1.16
97. The percentage of fructose converted into glucose in the equilibria
A) 53.7%
B) 83.1%
C) 21.7%
D) 63.2%
is _____.
Use the following to answer questions 98-99:
The equilibrium pressure of oxygen for the reaction
0.49 atm .
is
98. K p for the reaction is _____.
A) 0.49
B) 2.5 × 10 -3
C) 0.98
D) 4.9
99. The fraction of CuO that will decompose if 0.16 mole of CuO is placed in a 2.0 L vessel
at 1024ฐC is _____.
A) 0.15
B) 0.71
C) 0.23
D) 0.47
100. 3.9 moles of NO and 0.88 moles of CO 2 are allowed to react as
At equilibrium 0.11 moles of CO 2 was present. K c for the reaction is _____.
A) 0.27
B) 1.7
C) 3.14
D) 6.03
Page 23

Use the following to answer questions 101-102:
For the reaction at 430ฐC, K c = 54.3.
Initially 0.714 moles of H 2 and 0.984 moles of I 2 and 0.886 moles of HI are placed in a 2.40 L
vessel.
101. The equilibrium concentration of H 2 is _____.
A) 0.070 M
B) 0.182 M
C) 0.152 M
D) 0.012 M
102. The equilibrium concentration of I 2 is _____.
A) 0.112
B) 0.082
C) 0.182
D) 0.116
103.
A gaseous compound, A, dissociates as follows:
. A was
heated until equilibrium was reached. The pressure of A at equilibrium was 0.14P,where
P is the total pressure. K p for the reaction is _____.
A) 0.13P
B) 1.3P
C) 0.013P
D) 13P
Use the following to answer questions 104-106:
For the reaction
K c = 1.2 at 375ฐC.
104. K p for the reaction is _____.
A) 4.2 × 10 -2
B) 1.2× 10 2
C) 3.1 × 10 -3
D) 4.2 × 10 -4
Page 24

105. Kc for the reaction is _____.
A) –1.2
B) 0.83
C) 0.38
D) 0.012
106. K c for the formation of one mole of NH 3 from H 2 and N 2 is _____.
A) 0.6
B) 1.1
C) 1.2
D) 2.2
Use the following to answer questions 107-108:
The vapor pressure of water at 20ฐC is 0.0231 atm.
107.
Kp for the process is _____.
A) 0.0231
B) 2.31 × 10 -6
C) 2.31
D) 100
108. K c for vaporization of water is_____.
A) 1.8 × 10 -2
B) 2.3 × 10 -5
C) 9.6 × 10 -4
D) 3.6 × 10 -3
Use the following to answer questions 109-110:
The density of a mixture of the gases, NO 2 and N 2 O 4 , is 2.3 g/L at 74ฐC and 1.3 atm.
109. The partial pressure of NO 2 in the mixture is _____ atm.
A) 1.2
B) 0.12
C) 0.012
D) 0.24
Page 25

110. The partial pressure of N 2 O 4 the mixture is _____ atm.
A) 0.62
B) 0.12
C) 0.062
D) 0.63
111. What is Kp for the reaction when the total pressure at
equilibrium is 2.2 atm
A) 1.1
B) 1.2
C) 2.2
D) 2.1
Use the following to answer questions 112-114:
For the equilibrium , the equilibrium partial pressures of NO 2 and N 2 O 4
are 0.15 and 0.20 atm at 25ฐC.
112. What is the equilibrium partial pressure of NO 2 when the volume is doubled
A) 1.0atm
B) 0.10atm
C) 10atm
D) 0.01atm
113. The equilibrium partial pressure of N 2 O 4 when the volume is doubled will be _____
atm.
A) 0.88
B) 0.44
C) 0.044
D) 0.088
114. Kp for the equilibrium at 25ฐC is _____.
A) 1.13
B) 0.113
C) 11.3
D) 1.13 × 10 4
Page 26

115. The vapor pressure of mercury is 0.0020 mmHg at 26ฐC. K c for the process
A) 1.1 × 10 -7
B) 2.2 × 10 4
C) 1.1 × 10 -3
D) 4.4 × 10 -2
, is _____.
Page 27

Answer Key
1. B
2. A
3. C
4. D
5. A
6. C
7. D
8. B
9. B
10. C
11. A
12. B
13. C
14. D
15. C
16. D
17. C
18. A
19. B
20. D
21. A
22. C
23. B
24. A
25. D
26. C
27. A
28. C
29. D
30. A
31. B
32. A
33. C
34. A
35. C
36. B
37. C
38. A
39. B
40. C
41. B
42. C
43. D
44. C
Page 28

45. B
46. D
47. C
48. B
49. A
50. B
51. D
52. B
53. A
54. D
55. B
56. C
57. A
58. A
59. C
60. D
61. A
62. D
63. B
64. B
65. C
66. A
67. A
68. C
69. C
70. B
71. D
72. D
73. D
74. A
75. C
76. D
77. A
78. B
79. B
80. A
81. D
82. C
83. A
84. A
85. D
86. B
87. B
88. D
89. A
90. A
Page 29

91. C
92. A
93. C
94. A
95. A
96. D
97. A
98. A
99. C
100. B
101. A
102. C
103. B
104. D
105. B
106. B
107. A
108. C
109. A
110. B
111. B
112. B
113. D
114. B
115. A
Page 30