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Chemistry A Molecular Approach 2^nd Edition Tro Test Bank

ISBN-13: 978-0321651785

ISBN-10: 0321651782

 

 

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Principles of Chemistry: A Molecular Approach 2e (Tro)

Chapter 14   Chemical Equilibrium

 

1) Which of the following statements is FALSE?

1. A) When K >> 1, the forward reaction is favored and essentially goes to completion.
2. B) When K << 1, the reverse reaction is favored and the forward reaction does not proceed to a great extent.
3. C) When K ≈ 1, neither the forward or reverse reaction is strongly favored, and about the same amount of reactants and products exist at equilibrium.
4. D) K >> 1 implies that the reaction is very fast at producing products.
5. E) None of the above.

Answer:  D

Diff: 1    Page Ref: 14.3

Global:  G2

 

2) Give the direction of the reaction, if K >> 1.

1. A) The forward reaction is favored.
2. B) The reverse reaction is favored.
3. C) Neither direction is favored.
4. D) If the temperature is raised, then the forward reaction is favored.
5. E) If the temperature is raised, then the reverse reaction is favored.

Answer:  A

Diff: 1    Page Ref: 14.3

Global:  G2

 

3) Give the direction of the reaction, if K << 1.

1. A) The forward reaction is favored.
2. B) The reverse reaction is favored.
3. C) Neither direction is favored.
4. D) If the temperature is raised, then the forward reaction is favored.
5. E) If the temperature is raised, then the reverse reaction is favored.

Answer:  B

Diff: 1    Page Ref: 14.3

Global:  G2

 

4) Express the equilibrium constant for the following reaction.

 

2 CH3Cl(g) + Cl2(g) ⇔  2 CH2Cl2(g) + H2(g)

 

1. A) K =
2. B) K =
3. C) K =
4. D) K =
5. E) K =

Answer:  B

Diff: 2    Page Ref: 14.3

Global:  G2

LO:  14.3a

 

5) Express the equilibrium constant for the following reaction.

 

N2(g) + 3 H2(g) ⇔  2 NH3(g)

 

1. A) K =
2. B) K =
3. C) K =
4. D) K =
5. E) K =

Answer:  C

Diff: 2    Page Ref: 14.3

Global:  G2

LO:  14.3a

6) Express the equilibrium constant for the following reaction.

 

PCl5(g) ⇌ PCl3(g) + Cl2(g)

 

1. A) K =
2. B) K =
3. C) K =
4. D) K =
5. E) K =

Answer:  D

Diff: 2    Page Ref: 14.3

Global:  G2

LO:  14.3a

 

7) Express the equilibrium constant for the following reaction.

 

H2(g) + Br2(g)  ⇌  2 HBr(g)

 

1. A) K =
2. B) K =
3. C) K =
4. D) K =
5. E) K =

Answer:  E

Diff: 2    Page Ref: 14.3

Global:  G2

LO:  14.3a

8) Express the equilibrium constant for the following reaction.

 

2 P(g) + 3 Cl2(g)  ⇌  2 PCl3(g)

 

1. A) K =
2. B) K =
3. C) K =
4. D) K =
5. E) K =

Answer:  A

Diff: 2    Page Ref: 14.3

Global:  G2

LO:  14.3a

 

9) The equilibrium constant is given for one of the reactions below.  Determine the value of the missing equilibrium constant.

 

H2(g) + Br2(g)  ⇌  2 HBr(g)  Kc = 3.8 × 104

2 HBr(g)  ⇌  H2(g) + Br2(g)  Kc =  ?

 

1. A) 1.9 × 104
2. B) 5.3 × 10-5
3. C) 2.6 × 10-5
4. D) 6.4 × 10-4
5. E) 1.6 × 103

Answer:  C

Diff: 2    Page Ref: 14.3

Global:  G4

LO:  14.3b

 

10) The equilibrium constant is given for one of the reactions below.  Determine the value of the missing equilibrium constant.

 

2 HD(g)  ⇌  H2(g) + D2(g)    Kc = 0.28

2 H2(g) + 2 D2(g)  ⇌  4 HD(g)          Kc = ?

 

7. A) 7.8 × 10-2
8. B) 3.6
9. C) 0.53
10. D) 13
11. E) 1.9

Answer:  D

Diff: 2    Page Ref: 14.3

Global:  G4

LO:  14.3b

 

11) The equilibrium constant is given for one of the reactions below.  Determine the value of the missing equilibrium constant.

 

2 SO2(g) + O2(g)  ⇌  2 SO3(g)         Kc = 1.7 × 106

SO3(g)  ⇌  1/2 O2(g) + SO2(g)         Kc =  ?

 

3. A) 3.4 × 102
4. B) 8.5
5. C) 1.3 × 103
6. D) 1.2 × 10-6
7. E) 7.7 × 10-4

Answer:  E

Diff: 2    Page Ref: 14.3

Global:  G4

LO:  14.3b

12) The equilibrium constant is given for one of the reactions below.  Determine the value of the missing equilibrium constant.

 

N2O4(g)  ⇌  2 NO2(g)           Kc = 1.46

3 N2O4(g)  ⇌  6 NO2(g)        Kc = ?

 

2. A) 2.13
3. B) 0.685
4. C) 3.11
5. D) 1.46
6. E) 1.13

Answer:  C

Diff: 2    Page Ref: 14.3

Global:  G4

LO:  14.3b

 

13) The equilibrium constant is given for two of the reactions below.  Determine the value of the missing equilibrium constant.

 

A(g) + B(g)  ⇌  AB(g)           Kc = 0.24

AB(g) + A(g) ⇌  A2B(g)        Kc = 3.8

2 A(g) + B(g)  ⇌  A2B(g)      Kc = ?

 

4. A) 4.0
5. B) 0.91
6. C) 3.6
7. D) 16
8. E) 0.63

Answer:  B

Diff: 2    Page Ref: 14.3

Global:  G4

LO:  14.3b

14) The equilibrium constant is given for two of the reactions below.  Determine the value of the missing equilibrium constant.

 

A(g) + 2B(g)  ⇌  AB2(g)       Kc = 59

AB2(g) + B(g) ⇌  AB3(g)      Kc = ?

A(g) + 3B(g)  ⇌  AB3(g)       Kc = 478

 

3. A) 3.5 × 10-5
4. B) 2.8 × 104
5. C) 8.1
6. D) 0.12
7. E) 89

Answer:  C

Diff: 2    Page Ref: 14.3

Global:  G4

LO:  14.3b

 

 

15) What is △n for the following equation in relating Kc to Kp?

 

N2(g) + 3 H2(g)  ⇌  2 NH3(g)

 

1. A) 4
2. B) -4
3. C) -2
4. D) 2
5. E) 1

Answer:  C

Diff: 2    Page Ref: 14.4

Global:  G4

LO:  14.4

 

16) What is △n for the following equation in relating Kc to Kp?

 

2 NH3(g)  ⇌  N2(g) + 3 H2(g)

 

1. A) 4
2. B) -4
3. C) -2
4. D) 2
5. E) 1

Answer:  D

Diff: 2    Page Ref: 14.4

Global:  G4

LO:  14.4

17) What is △n for the following equation in relating Kc to Kp?

 

2 SO2(g) + O2(g)  ⇌  2 SO3(g)

 

1. A) 3
2. B) -1
3. C) -2
4. D) 2
5. E) 1

Answer:  B

Diff: 2    Page Ref: 14.4

Global:  G4

LO:  14.4

 

 

18) What is △n for the following equation in relating Kc to Kp?

 

H2(g) + Br2(g) ⇌ 2 HBr(g)

 

1. A) 0
2. B) -1
3. C) -2
4. D) 2
5. E) 1

Answer:  A

Diff: 2    Page Ref: 14.4

Global:  G4

LO:  14.4

 

19) In which of the following reactions will Kc = Kp?

1. A) H2(g) + I2(g) ⇌ 2 HI(g)
2. B) CH4(g) + H2O(g) ⇌ CO(g) + 3 H2(g)
3. C) N2O4(g) ⇌ 2NO2(g)
4. D) CO(g) + 2 H2(g) ⇌ CH3OH(g)
5. E) N2(g) + 3 H2(g) ⇌ 2 NH3(g)

Answer:  A

Diff: 2    Page Ref: 14.4

Global:  G2

LO:  14.4

20) In which of the following reactions will Kc = Kp?

1. A) 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H2O(g)
2. B) SO3(g) + NO(g) ⇌ SO2(g) + NO2(g)
3. C) 2 N2(g) + O2(g) ⇌ 2 N2O(g)
4. D) 2 SO2(g) + O2(g) ⇌ 2 SO3(g)
5. E) None of the above reactions have Kc= Kp.

Answer:  B

Diff: 2    Page Ref: 14.4

Global:  G2

LO:  14.4

 

 

21) The reaction below has a Kc value of 61.  What is the value of Kp for this reaction at 500 K?

 

N2(g) + 3 H2(g)  ⇌  2 NH3(g)

 

1. A) 15
2. B) 61
3. C) 28
4. D) 3.6 × 10-2
5. E) 1.9 × 10-2

Answer:  D

Diff: 3    Page Ref: 14.4

Global:  G4

LO:  14.4

 

22) The reaction below has a Kp value of 41.  What is the value of Kc for this reaction at 400 K?

 

N2(g) + 3 H2(g)  ⇌  2 NH3(g)

 

2. A) 2.4 × 10-2
3. B) 4.4 × 104
4. C) 41
5. D) 2.3 × 10-5
6. E) 1.9 × 104

Answer:  B

Diff: 3    Page Ref: 14.4

Global:  G4

LO:  14.4

23) The reaction below has a Kc value of 1.0 × 1012.  What is the value of Kp for this reaction at 500 K?

 

2 SO2(g) + O2(g)  ⇌  2 SO3(g)

 

4. A) 4.2 × 10-11
5. B) 1.0 × 1012
6. C) 2.4 × 10-12
7. D) 4.1 × 1013
8. E) 2.4 × 1010

Answer:  E

Diff: 3    Page Ref: 14.4

Global:  G4

LO:  14.4

 

 

24) The reaction below has a Kp value of 3.3 x 10-5.  What is the value of Kc for this reaction at 700 K?

 

2 SO3(g) ⇌  2 SO2(g) + O2(g)

 

5. A) 5.7 × 10-7
6. B) 1.7 × 106
7. C) 3.3 × 10-5
8. D) 3.0 × 104
9. E) 1.9 × 10-3

Answer:  A

Diff: 3    Page Ref: 14.4

Global:  G4

LO:  14.4

25) Express the equilibrium constant for the following reaction.

 

P4(s) + 5 O2(g)  ⇌  P4O10(s)

 

1. A) K =
2. B) K =
3. C) K = [O2]-5
4. D) K = [O2]5
5. E) K =

Answer:  C

Diff: 2    Page Ref: 14.5

Global:  G2

LO:  14.5

 

 

26) Express the equilibrium constant for the following reaction.

 

2 Na(s) + 2 H2O(l)  ⇌  2 NaOH(aq) + H2(g)

 

1. A) K =
2. B) K = [H2][NaOH]-2
3. C) K =
4. D) K = [H2][NaOH]2
5. E) K =

Answer:  D

Diff: 2    Page Ref: 14.5

Global:  G2

LO:  14.5

27) Express the equilibrium constant for the following reaction.

 

KClO3(s)  ⇌  KClO(s) + O2(g)

 

1. A) K =
2. B) K = [O2]-1
3. C) K =
4. D) K =
5. E) K = [O2]

Answer:  E

Diff: 2    Page Ref: 14.5

Global:  G2

LO:  14.5

 

 

28) For which reaction will Kp = Kc?

1. A) S(s) + O2(g) ⇌ SO2(g)
2. B) 2 HgO(s) ⇌ Hg(l) + O2(g)
3. C) CaCO3(s) ⇌ CaO(s) + CO2(g)
4. D) H2CO3(s) ⇌ H2O(l) + CO2(g)
5. E) 2 H2O(l) ⇌ 2 H2(g) + O2(g)

Answer:  A

Diff: 2    Page Ref: 14.5

Global:  G2

LO:  14.5

29) Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 3.6 M, [O2]eq = 4.1 M, [N2O]eq = 3.3 × 10-18 M.

 

2 N2(g) + O2(g) ⇌ 2 N2O(g)

 

2. A) 2.2 × 10-19
3. B) 4.5 × 1018
4. C) 2.0 × 10-37
5. D) 5.0 × 1036
6. E) 4.9 × 10-17

Answer:  C

Diff: 3    Page Ref: 14.6

Global:  G4

LO:  14.6

 

30) Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 1.5 M, [H2]eq = 1.1 M, [NH3]eq = 0.47 M.

 

N2(g) + 3 H2(g) ⇌ 2 NH3(g)

 

3. A) 3.5
4. B) 0.28
5. C) 9.1
6. D) 0.11
7. E) 0.78

Answer:  D

Diff: 3    Page Ref: 14.6

Global:  G4

LO:  14.6

 

31) Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [HCl]eq = 0.13 M, [HI]eq = 5.6 × 10-16 M, [Cl2]eq = 0.0019 M.

 

2 HCl(g) + I2(s) ⇌ 2 HI(g) + Cl2(g)

 

8. A) 8.2 × 10-18
9. B) 2.9 × 1031
10. C) 1.2 × 1017
11. D) 1.4 × 10-19
12. E) 3.5 × 10-32

Answer:  E

Diff: 3    Page Ref: 14.6

Global:  G4

LO:  14.6

 

32) Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [PCl5]eq = 0.56 M, [PCl3]eq = 0.23 M, [Cl2]eq = 4.4 M.

 

PCl5(g) ⇌  PCl3(g) + Cl2(g)

 

1. A) 1.8
2. B) 0.93
3. C) 0.55
4. D) 1.1
5. E) 0.76

Answer:  A

Diff: 3    Page Ref: 14.6

Global:  G4

LO:  14.6

33) Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 M, [I2]eq = 0.39 M, [HI]eq = 1.6 M.

 

H2(g) + I2(g)  ⇌  2 HI(g)

 

2. A) 2.1 × 10-2
3. B) 29
4. C) 47
5. D) 3.4 × 10-2
6. E) 8.7 × 10-2

Answer:  C

Diff: 3    Page Ref: 14.6

Global:  G4

LO:  14.6

 

34) Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(CO)eq = 6.8 × 10-11 atm, P(O2)eq = 1.3 × 10-3 atm, P(CO2)eq = 0.041 atm.

 

2 CO(g) + O2(g) ⇌ 2 CO2(g)

 

3. A) 3.6 × 10-21
4. B) 2.8 × 1020
5. C) 4.6 × 1011
6. D) 2.2 × 10-12
7. E) 3.6 × 10-15

Answer:  B

Diff: 3    Page Ref: 14.6

Global:  G4

LO:  14.6

35) Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(NOCl)eq = 0.22 atm, P(NO)eq = 0.10 atm, P(Cl2)eq = 0.081 atm.

 

2 NOCl(g)  ⇌  2 NO(g) + Cl2(g)

 

3. A) 3.7 × 10-2
4. B) 60.
5. C) 27
6. D) 1.7 × 10-2
7. E) 1.8 × 10-3

Answer:  D

Diff: 3    Page Ref: 14.6

Global:  G4

LO:  14.6

 

36) Calculate the value of [N2]eq if [H2]eq = 2.0 M, [NH3]eq = 0.5 M, and Kc = 2.

 

N2(g) + 3 H2(g) ⇌ 2 NH3(g)

 

1. A) 0.016 M
2. B) 0.031 M
3. C) 0.062 M
4. D) 0.40 M
5. E) 62.5 M

Answer:  A

Diff: 4    Page Ref: 14.6

Global:  G4

LO:  14.6

 

 

37) Calculate P [NO]eq, if  P [NOCl]eq = 0.33 atm, P [Cl2]eq = 0.50 atm, and Kp = 1.9 x 10-2.

 

2 NOCl(g)  ⇌  2 NO(g) + Cl2(g)

 

1. A) 1.7 atm
2. B) 0.0042 atm
3. C) 0.30 atm
4. D) 0.064 atm
5. E) 0.087 atm

Answer:  D

Diff: 4    Page Ref: 14.6

Global:  G4

LO:  14.6

38) Which of the following statements are TRUE?

1. A) Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction.
2. B) The equilibrium constant for the forward reaction is equal to the equilibrium constant for the reverse reaction.
3. C) A reaction quotient (Q) larger than the equilibrium constant (K) means that the reaction will favor the production of more products.
4. D) Dynamic equilibrium indicates that the amount of reactants and products are equal.
5. E) All of the above are true.

Answer:  A

Diff: 1    Page Ref: 14.7

Global:  G2

 

39) In a reaction mixture containing only reactants, what is the value of Q?

1. A) -1
2. B) 1
3. C) ∞
4. D) 0
5. E) It cannot be determined without concentrations.

Answer:  D

Diff: 1    Page Ref: 14.7

Global:  G2

LO:  14.7

 

40) Which of the following statements is TRUE?

1. A) If Q < K, it means the reverse reaction will proceed to form more reactants.
2. B) If Q > K, it means the forward reaction will proceed to form more products.
3. C) If Q = K, it means the reaction is at equilibrium.
4. D) All of the above are true.
5. E) None of the above are true.

Answer:  C

Diff: 1    Page Ref: 14.7

Global:  G2

LO:  14.7

41) Consider the following reaction and its equilibrium constant:

 

SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)      Kc = 0.33

 

A reaction mixture contains  0.39 M SO2,  0.14 M NO2 , 0.11 M SO3 and 0.14 M NO.  Which of the following statements is TRUE concerning this system?

1. A) The reaction will shift in the direction of reactants.
2. B) The equilibrium constant will decrease.
3. C) The reaction will shift in the direction of products.
4. D) The reaction quotient will decrease.
5. E) The system is at equilibrium.

Answer:  C

Diff: 3    Page Ref: 14.7

Global:  G2

LO:  14.7

 

42) Consider the following reaction and its equilibrium constant:

 

4 CuO(s) + CH4(g)  ⇌  CO2(g) + 4 Cu(s) + 2 H2O(g)          Kc = 1.10

 

A reaction mixture contains  0.22 M CH4,  0.67 M  CO2 and 1.3 M H2O.  Which of the following statements is TRUE concerning this system?

1. A) The reaction will shift in the direction of products.
2. B) The equilibrium constant will increase.
3. C) The reaction quotient will increase.
4. D) The reaction will shift in the direction of reactants.
5. E) The system is at equilibrium.

Answer:  D

Diff: 3    Page Ref: 14.7

Global:  G2

LO:  14.7

43) Consider the following reaction and its equilibrium constant:

 

I2(g) + Br2(g) ⇌  2 IBr(g)      Kc = 1.1 × 102

 

A reaction mixture contains  0.41 M I2,  0.27 M Br2 and 3.5 M IBr.  Which of the following statements is TRUE concerning this system?

1. A) The reaction will shift in the direction of products.
2. B) The reaction will shift in the direction of reactants.
3. C) The reaction quotient will decrease.
4. D) The equilibrium constant will increase.
5. E) The system is at equilibrium.

Answer:  E

Diff: 3    Page Ref: 14.7

Global:  G2

LO:  14.7

 

44) Consider the following reaction and its equilibrium constant:

 

I2(g) ⇌ 2I(g)            Kp = 0.209

 

A reaction mixture contains  0.89 atm I2 and 1.77 atm I.  Which of the following statements is TRUE concerning this system?

1. A) The reaction will shift in the direction of reactants.
2. B) The reaction quotient will increase.
3. C) The reaction will shift in the direction of products.
4. D) The equilibrium constant will decrease.
5. E) The system is at equilibrium.

Answer:  A

Diff: 3    Page Ref: 14.7

Global:  G2

LO:  14.7

45) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature.  Determine the equilibrium concentration of H2O(g).

 

C2H4(g) + H2O(g) ⇌  C2H5OH(g) Kc = 9.0 × 103

 

[C2H4]eq = 0.015 M                        [C2H5OH]eq = 1.69 M

 

9. A) 9.9 × 10-7M
10. B) 80. M
11. C) 1.0 M
12. D) 1.68 M
13. E) 0.013 M

Answer:  E

Diff: 3    Page Ref: 14.8

Global:  G4

LO:  14.8a

 

 

46) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature.  Determine the equilibrium concentration of SO3(g).

 

2 SO2(g) + O2(g)  ⇌  2 SO3(g)          Kc = 1.7 × 108

 

[SO2]eq = 0.0034 M                           [O2]eq = 0.0018 M

 

1. A) 1.9 M
2. B) 1.0 × 103M
3. C) 0.53 M
4. D) 9.6 x 10-4M
5. E) 0.73 M

Answer:  A

Diff: 3    Page Ref: 14.8

Global:  G4

LO:  14.8a

47) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature.  Determine the equilibrium concentration of NO2(g).

 

N2O4(g) ⇌ 2 NO2(g)       Kc = 0.21

 

[N2O4]eq = 0.039 M

 

1. A) 1.22 M
2. B) 9.0 × 10-2 M
3. C) 7.8 × 10-2M
4. D) 8.2 × 10-3 M
5. E) 11 M

Answer:  B

Diff: 3    Page Ref: 14.8

Global:  G4

LO:  14.8a

 

 

48) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature.  Determine the equilibrium concentration of CO2(g).

 

NH2COONH4(s) ⇌ 2 NH3(g) + CO2(g)       Kc = 1.58 × 10-8

 

[NH3]eq = 2.9 × 10-3 M

 

1. A) 0.053 M
2. B) 4.6 × 10-11M
3. C) 1.9 × 10-3M
4. D) 5.4 × 10-6M
5. E) 0.022 M

Answer:  C

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LO:  14.8a

49) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature.  Determine the equilibrium pressure of H2.

 

D2(g) + H2(g)  ⇌ 2 HD(g)              Kp = 1.80

 

P(D2)eq = 1.1 × 10-3 atm                P(HD)eq = 2.7 × 10-3 atm

 

2. A) 2.7 atm
3. B) 1.4 atm
4. C) 0.73 atm
5. D) 3.7 × 10-3atm
6. E) 8.1 × 10-4atm

Answer:  D

Diff: 3    Page Ref: 14.8

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LO:  14.8b

 

 

50) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature.  Determine the equilibrium pressure of CO.

 

CO(g) + 2 H2(g) ⇌  CH3OH(l)          Kp = 2.25 × 104

 

P(H2)eq = 0.52 atm

 

8. A) 8.3 x 104atm
9. B) 1.2 x 10-5atm
10. C) 6.25 x 10-3atm
11. D) 8.5 x 10-5atm
12. E) 1.6 x 10-4atm

Answer:  E

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LO:  14.8b

51) Consider the following reaction:

 

Xe(g) + 2 F2(g)  →  XeF4(g)

 

A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F2.  If the equilibrium pressure of Xe is 0.34 atm, find the equilibrium constant (Kp) for the reaction.

1. A) 25
2. B) 0.12
3. C) 0.99
4. D) 8.3
5. E) 0.040

Answer:  A

Diff: 4    Page Ref: 14.8

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LO:  14.8c

 

 

52) Consider the following reaction:

 

CH4(g) + 2 H2S(g) ⇌  CS2(g) + 4 H2(g)

 

A reaction mixture initially contains 0.50 M CH4 and 0.75 M H2S.  If the equilibrium concentration of H2 is 0.44 M, find the equilibrium constant (Kc) for the reaction.

1. A) 0.23
2. B) 0.038
3. C) 2.9
4. D) 10.
5. E) 0.34

Answer:  B

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53) Consider the following reaction:

 

COCl2(g)  ⇌  CO(g) + Cl2(g)

 

A reaction mixture initially contains 1.6 M COCl2.  Determine the equilibrium concentration of CO if Kc for the reaction at this temperature is 8.33 × 10-4.  Calculate this based on the assumption that the answer is negligible compared to 1.6.

4. A) 4.2 × 10-4M
5. B) 1.5 × 10-3M
6. C) 3.7 × 10-2M
7. D) 2.1 × 10-2M
8. E) 1.3 × 10-3M

Answer:  C

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LO:  14.8d

 

 

54) Consider the following reaction:

 

CuS(s) + O2(g)  ⇌  Cu(s) + SO2(g)

 

A reaction mixture initially contains 2.9 M O2.  Determine the equilibrium concentration of O2 if Kc for the reaction at this temperature is 1.5.

1. A) 1.9 M
2. B) 1.7 M
3. C) 2.2 M
4. D) 1.2 M
5. E) 0.59 M

Answer:  D

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55) Consider the following reaction:

 

2 H2O(g) + 2 SO2(g) ⇌  2 H2S(g) + 3 O2(g)

 

A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2.  Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10-6.

1. A) 0.045 M
2. B) 0.058 M
3. C) 0.028 M
4. D) 3.1 × 10-3M
5. E) 0.12 M

Answer:  E

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LO:  14.8c

 

56) Consider the following reaction:

 

CO2(g) + C(graphite)  ⇌  2 CO(g)

 

A reaction mixture initially contains 0.56 atm CO2 and 0.32 atm CO.  Determine the equilibrium pressure of CO if Kp for the reaction at this temperature is 2.25.

1. A) 0.83 atm
2. B) 0.31 atm
3. C) 0.26 atm
4. D) 0.58 atm
5. E) 0.42 atm

Answer:  A

Diff: 5    Page Ref: 14.8

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LO:  14.8b

57) Consider the following reaction:

 

NO(g) + SO3(g)  ⇌  NO2(g) + SO2(g)

 

A reaction mixture initially contains 0.86 atm NO and 0.86 atm SO3.  Determine the equilibrium pressure of NO2 if Kp for the reaction at this temperature is 0.0118.

1. A) 0.78 atm
2. B) 0.084 atm
3. C) 0.012 atm
4. D) 0.85 atm
5. E) 0.048 atm

Answer:  B

Diff: 5    Page Ref: 14.8

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LO:  14.8b

 

58) Consider the following reaction at equilibrium.  What effect will adding more SO3 have on the system?

 

SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)

 

1. A) The reaction will shift in the direction of products.
2. B) The reaction will shift to decrease the pressure.
3. C) No change will occur since SO3is not included in the equilibrium expression.
4. D) The reaction will shift in the direction of reactants.
5. E) The equilibrium constant will decrease.

Answer:  D

Diff: 2    Page Ref: 14.9

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LO:  14.9a

 

59) Consider the following reaction at equilibrium.  What effect will adding more H2S have on the system?

 

2 H2S(g) + 3 O2(g)  ⇌  2 H2O(g) + 2 SO2(g)

 

1. A) The reaction will shift to the left.
2. B) No change will be observed.
3. C) The equilibrium constant will decrease.
4. D) The equilibrium constant will increase.
5. E) The reaction will shift in the direction of products.

Answer:  E

Diff: 2    Page Ref: 14.9

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LO:  14.9a

 

60) Consider the following reaction at equilibrium.  What effect will adding some C have on the system?

 

CO2(g) + C(graphite) ⇌ 2 CO(g)

 

1. A) No effect will be observed since C is not included in the equilibrium expression.
2. B) The equilibrium constant will decrease.
3. C) The reaction will shift to the left in the direction of reactants.
4. D) The equilibrium constant will increase.
5. E) The reaction will shift to the right in the direction of products.

Answer:  A

Diff: 2    Page Ref: 14.9

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LO:  14.9a

 

61) Consider the following reaction at equilibrium.  What effect will reducing the volume of the reaction mixture have on the system?

 

CuS(s) + O2(g)  ⇌  Cu(s) + SO2(g)

 

1. A) The equilibrium constant will decrease.
2. B) No effect will be observed.
3. C) The reaction will shift to the right in the direction of products.
4. D) The equilibrium constant will increase.
5. E) The reaction will shift to the left in the direction of reactants.

Answer:  B

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LO:  14.9c

 

62) Consider the following reaction at equilibrium.  What effect will increasing the volume of the reaction mixture have on the system?

 

2 H2S(g) + 3 O2(g)  ⇌  2 H2O(g) + 2 SO2(g)

 

1. A) The reaction will shift to the right in the direction of products.
2. B) No effect will be observed.
3. C) The reaction will shift to the left in the direction of reactants.
4. D) The equilibrium constant will decrease.
5. E) The equilibrium constant will increase.

Answer:  C

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LO:  14.9c

 

63) Consider the following reaction at equilibrium.  What effect will reducing the volume of the reaction mixture have on the system?

 

Xe(g) + 2 F2(g)  →  XeF4(g)

 

1. A) The reaction will shift to the left in the direction of reactants.
2. B) The equilibrium constant will increase.
3. C) No effect will be observed.
4. D) The reaction will shift to the right in the direction of products.
5. E) The equilibrium constant will decrease.

Answer:  D

Diff: 2    Page Ref: 14.9

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LO:  14.9c

 

64) Consider the following reaction at equilibrium.  What effect will increasing the pressure of the reaction mixture have on the system?

 

2 H2S(g) + 3 O2(g)  ⇌  2 H2O(g) + 2 SO2(g)

 

1. A) The reaction will shift to the right in the direction of products.
2. B) No effect will be observed.
3. C) The reaction will shift to the left in the direction of reactants.
4. D) The equilibrium constant will decrease.
5. E) The equilibrium constant will increase.

Answer:  A

Diff: 2    Page Ref: 14.9

Global:  G2

 

65) Consider the following reaction at equilibrium.  What effect will reducing the pressure of the reaction mixture have on the system?

 

Xe(g) + 2 F2(g)  →  XeF4(g)

 

1. A) The reaction will shift to the left in the direction of reactants.
2. B) The equilibrium constant will increase.
3. C) No effect will be observed.
4. D) The reaction will shift to the right in the direction of products.
5. E) The equilibrium constant will decrease.

Answer:  A

Diff: 2    Page Ref: 14.9

Global:  G2

 

66) Consider the following reaction at equilibrium.  What effect will adding 1 atm of Ar to the reaction mixture have on the system?

 

2 H2S(g) + 3 O2(g)  ⇌  2 H2O(g) + 2 SO2(g)

 

1. A) The reaction will shift to the right in the direction of products.
2. B) No effect will be observed.
3. C) The reaction will shift to the left in the direction of reactants.
4. D) The equilibrium constant will decrease.
5. E) The equilibrium constant will increase.

Answer:  B

Diff: 2    Page Ref: 14.9

Global:  G2

 

67) Consider the following reaction at equilibrium.  What effect will increasing the temperature have on the system?

 

Fe3O4(s) + CO(g) ⇌  3 FeO(s) + CO2(g)      ΔH°= +35.9 kJ

 

1. A) The reaction will shift to the left in the direction of reactants.
2. B) The equilibrium constant will increase.
3. C) The equilibrium constant will decrease.
4. D) No effect will be observed.
5. E) The reaction will shift to the right in the direction of products.

Answer:  E

Diff: 2    Page Ref: 14.9

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LO:  14.9b

 

68) Consider the following reaction at equilibrium.  What effect will decreasing the temperature have on the system?

 

CO2(g) + 2 H2O(l) ⇌ CH4(g) + 2 O2(g)       ΔH° = +890 kJ

 

1. A) The reaction will shift to the left in the direction of reactants.
2. B) The equilibrium constant will decrease.
3. C) The equilibrium constant will increase.
4. D) The reaction will shift to the right in the direction of products.
5. E) No effect will be observed.

Answer:  A

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LO:  14.9b

 

69) Consider the following reaction at equilibrium.  What effect will adding water have on the system?

 

CO2(g) + 2 H2O(l) ⇌ CH4(g) + 2 O2(g)       ΔH° = +890 kJ

 

1. A) The reaction will shift to the left in the direction of reactants.
2. B) The equilibrium constant will decrease.
3. C) The equilibrium constant will increase.
4. D) The reaction will shift to the right in the direction of products.
5. E) No effect will be observed.

Answer:  E

Diff: 2    Page Ref: 14.9

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LO:  14.9a

 

70) Consider the following reaction at equilibrium.  What effect will adding a catalyst have on the system?

 

CO2(g) + 2 H2O(l) ⇌ CH4(g) + 2 O2(g)       ΔH° = +890 kJ

 

1. A) The reaction will shift to the left in the direction of reactants.
2. B) The equilibrium constant will decrease.
3. C) The equilibrium constant will increase.
4. D) The reaction will shift to the right in the direction of products.
5. E) No effect will be observed.

Answer:  E

Diff: 2    Page Ref: 14.9

Global:  G2

 

71) Consider the following reaction at equilibrium.  What effect will increasing the temperature have on the system?

 

C3H8(g) + 5 O2(g)  ⇌ 3 CO2(g) + 4 H2O(l) ΔH° = -2220 kJ

 

1. A) The reaction will shift to the right in the direction of products.
2. B) The reaction will shift to the left in the direction of reactants.
3. C) The equilibrium constant will increase.
4. D) The equilibrium constant will decrease.
5. E) No effect will be observed.

Answer:  B

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LO:  14.9b

 

Match the following.

 

1. A) Reaction will favor formation of reactants.
2. B) Reaction has a larger amount of products than reactants.
3. C) Reaction does not strongly favor reactants or products.
4. D) Reaction is at equilibrium.
5. E) Reaction favors formation of more products.

 

72) Q < K

Diff: 1    Page Ref: 14.7

Global: G2

LO:  14.7

 

73) K << 1

Diff: 1   Page Ref: 14.7

Global:  G2

 

74) Q = K

Diff: 1   Page Ref: 14.7

Global:  G2

LO:  14.7

 

75) K ≈ 1

Diff: 1    Page Ref: 14.7

Global:  G2

 

76) Q  >>  1

Diff: 1    Page Ref: 14.7

Global:  G2

 

Answers: 72) E  73) A  74) D  75) C  76) B

 

 

77) Explain dynamic equilibrium.  Use the generic reaction A(g) ⇌  B(g)  to explain.

Answer:  Dynamic equilibrium means that the ratio of [B]/[A] is constant, but the forward and reverse reactions continue to occur.  The rates of the forward and reverse reactions are equal in order to keep the ratio of [B]/[A] constant.

Diff: 1    Page Ref: 14.2

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78) Why is an equilibrium constant unitless?

Answer:  Each concentration or pressure is a ratio to a reference concentration or pressure.  As ratios have no units, the equilibrium constant is unitless as well.

Diff: 1    Page Ref: 14.4

Global:  G2, G8

 

 

79) Why aren’t solids or liquids included in an equilibrium expression?

Answer:  The equilibrium constant relates different concentrations of reactants and products to one another.  Since the concentrations of liquids and solids are constant, their concentration(s) becomes part of the constant value of the equilibrium constant.

Diff: 1    Page Ref: 14.5

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80) Can the Kp and Kc for a reaction ever have the same value?  Why or why not?

Answer:   Kp and Kc are equal for reactions in which the number of moles of gaseous reactants are equal to the number of moles of gaseous products.

Diff: 2    Page Ref: 14.6

Global:  G2, G8

LO:  14.4

 

81) How is the reaction quotient different from an equilibrium constant for a given reaction?

Answer:  The expression for both is identical.  However, the equilibrium constant (K) in only useful for systems at equilibrium.  In systems not at equilibrium, the reaction quotient (A) can be calculated to determine in which direction the reaction will proceed.

Diff: 1    Page Ref: 14.7

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LO:  14.7

 

82) Define reaction quotient.

Answer:  The concentration of the products raised to their stoichiometric coefficients divided the concentrations of the reactants raised to their stoichiometric coefficients.

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LO:  14.7

 

83) For the reaction: N2(g) + 2 O2(g) ⇌ 2 NO2(g), Kc = 8.3 × 10-10 at 25°C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is five times the concentration of O2 gas?

3. A) 3.3 × 10-11M
4. B) 1.7 × 10-10M
5. C) 6.0 × 109M
6. D) 3.0 × 1010M

Answer:  D

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LO:  14.8a

 

84) The Kp for the reaction below is 1.49 × 108 at 100.0°C:

 

CO(g) + Cl2 (g)  →  COCl2 (g)

 

In an equilibrium mixture of the three gases, PCO = PCl2  = 2.22 × 10-4 atm. The partial pressure of the product, phosgene (COCl2), is ________ atm.

7. A) 7.34
8. B) 3.02 × 1015
9. C) 3.31 × 10-16
10. D) 3.31 × 104
11. E) 6.67 × 1011

Answer:  A

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LO:  14.8b

 

85) At 900.0 K, the equilibrium constant (Kp) for the following reaction is 0.345.

 

2 SO2 + O2 (g)  →  2 SO3 (g)

 

At equilibrium, the partial pressure of SO2 is 35.0 atm and that of O2 is 15.9 atm. The partial pressure of SO3 is ________ atm.

82. A) 82.0
83. B) 4.21 ×
84. C) 192
85. D) 6.20 × 10-4
86. E) 40.2

Answer:  A

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86) The decomposition of ammonia is: 2 NH3(g)  →  N2(g) + 3 H2(g). If Kp is 1.5 × 103 at 400°C, what is the partial pressure of ammonia at equilibrium when N2 is 0.10 atm and H2 is 0.15 atm?

2. A) 2.2 × 10-7atm
3. B) 4.7 × 10-4atm
4. C) 2.1 × 103atm
5. D) 4.4 × 106atm

Answer:  B

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LO:  14.8b

 

 

87) Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction:

 

PCl3 (g) + Cl2 (g)  →  PCl5 (g)

 

An equilibrium mixture at 450 K contains

PPCl3 = 0.124 atm,

PCl2 = 0.157 atm, and

PPCl5 = 1.30 atm. What is the value of Kp at this temperature?

66. A) 66.7
67. B) 1.50 × 10-2
68. C) 2.53 × 10-2
69. D) 1.02
70. E) 4.63

Answer:  A

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88) An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0100 M O2. At this temperature, Kc equals 1.4 × 102 for the reaction:

 

2 CO(g) + O2(g) ⇌ 2 CO2(g).

 

What is the equilibrium concentration of CO?

7. A) 7.1 × 10-7M
8. B) 8.4 × 10-4M
9. C) 1.4 × 10-2M
10. D) 1.2 × 10-1M

Answer:  B

Diff: 4    Page Ref: 14.6

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LO:  14.6

 

 

89) At a certain temperature, Kc equals 1.4 × 102 for the reaction:

 

2 CO(g) + O2(g) ⇌ 2 CO2(g).

 

If a 3.00-L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium, how many moles of CO are also present in the flask?

1. A) 0.555 mol
2. B) 0.185 mol
3. C) 0.107 mol
4. D) 0.0114 mol

Answer:  B

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LO:  14.6

90) At a certain temperature, nitogen and hydrogen react to form ammonia:

 

N2(g) + 3 H2(g) ⇌ 2 NH3(g).

 

When initial amounts of N2, H2, and NH3 are mixed, the concentration of NH3 increases. Which statement below is TRUE?

1. A) Kc< Q
2. B) Kc> Q
3. C) Kc= Q
4. D) More information is needed to make a statement about Kc.

Answer:  B

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LO:  14.7

 

91) For the isomerization reaction:

butane ⇌ isobutane

Kp equals 25 at 500°C. If the initial pressures of butane and isobutane are 20. atm and 0.0 atm, respectively, what are the pressures of the two gases at equilibrium?

1. A) P(butane) = 0.77 atm and P(isobutane) = 19.2 atm
2. B) P(butane) = 0.80 atm and P(isobutane) = 20. atm
3. C) P(butane) = 19.2 atm and P(isobutane) = 0.77 atm
4. D) P(butane) = 20 atm and P(isobutane) = 0.80 atm

Answer:  A

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92) Cyclohexane, C6H12, undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane, CH3C5H9, according to the equation:

 

C6H12 ⇌ CH3C5H9

 

If Kc = 0.143 at 25°C for this reaction, find the equilibrium concentrations of C6H12 and CH3C5H9 if the initial concentrations are 0.200 M and 0.075 M, respectively.

1. A) [C6H12] = 0.041 M, [CH3C5H9] = 0.041 M
2. B) [C6H12] = 0.159 M, [CH3C5H9] = 0.116 M
3. C) [C6H12] = 0.241 M, [CH3C5H9] = 0.034 M
4. D) [C6H12] = 0.253 M, [CH3C5H9] = 0.022 M

Answer:  C

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LO:  14.8c

93) At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction:

 

2 ICl(g) ⇌ I2(g) + Cl2(g).

 

What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0-L flask?

1. A) 0.14 M
2. B) 0.17 M
3. C) 0.27 M
4. D) 0.34 M

Answer:  A

Diff: 5    Page Ref: 14.8

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LO:  14.8c

 

94) The equilibrium constant, Kp, equals 3.40 for the isomerization reaction:

            cis-2-butene ⇌ trans-2-butene.

If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene, what is the equilibrium pressure of each gas?

1. A) P(cis-2-butene) = 0.0426 atm and P(trans-2-butene) = 0.145 atm
2. B) P(cis-2-butene) = 0.0471 atm and P(trans-2-butene) = 0.160 atm
3. C) P(cis-2-butene) = 0.0735 atm and P(trans-2-butene) = 0.250 atm
4. D) P(cis-2-butene) = 0.0898 atm and P(trans-2-butene) = 0.305 atm

Answer:  D

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LO:  14.8c

 

 

95) Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation:

 

PCl5(g) ⇌ PCl3(g) + Cl2(g)

 

At 250° 0.125 M PCl5 is added to the flask. If Kc = 1.80, what are the equilibrium concentrations of each gas?

1. A) [PCl5] = 0.00765 M, [PCl3] = 0.117 M, and [Cl2] = 0.117 M
2. B) [PCl5] = 0.0625 M, [PCl3] = 0.335 M, and [Cl2] = 0.335 M
3. C) [PCl5] = 1.80 M, [PCl3] = 1.80 M, and [Cl2] = 1.80 M
4. D) [PCl5] = 3.96 M, [PCl3] = 3.83 M, and [Cl2] = 3.83 M

Answer:  A

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LO:  14.8c

96) Kc is 1.67 × 1020 at 25°C for the formation of iron(III) oxalate complex ion:

 

Fe3+(aq) + 3 C2O42-(aq) ⇌ [Fe(C2O4)3]3-(aq).

 

If 0.0200 M Fe3+ is initially mixed with 1.00 M oxalate ion, what is the concentration of Fe3+ ion at equilibrium?

1. A) 1.44 × 10-22M
2. B) 0.0100 M
3. C) 8.35 × 1019M
4. D) 6.94 × 1021M

Answer:  A

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LO:  14.8c

 

 

97) Dinitrogen tetroxide partially decomposes according to the following equilibrium:

 

N2O4 (g)  →  2NO2 (g)

 

A 1.000-L flask is charged with 3.00 × 10-2  mol of N2O4. At equilibrium, 2.36 × 10-2  mol of N2O4 remains. Keqfor this reaction is ________.

1. A) 0.723
2. B) 0.391
3. C) 0.212
4. D) 6.94 ×
5. E) 1.92 × 10-4

Answer:  D

Diff: 5    Page Ref: 14.8

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LO:  14.6

98) Cyclohexane (C6H12) undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane (MCP) according to the equation:

 

C6H12 ⇌ MCP

 

If Kc = 0.143 at 25°C for this reaction, predict the direction in which the system will shift if the initial concentrations of C6H12 and MCP are 0.0400 M and 0.0200 M, respectively. The system

1. A) will shift left.
2. B) will shift right.
3. C) is already at equilibrium.
4. D) is not at equilibrium and will remain in an unequilibrated state.

Answer:  A

Diff: 2    Page Ref: 14.9

Global:  G2

LO:  14.9a

 

99) The equilibrium constant is equal to 5.00 at 1300 K for the reaction:

 

2 SO2(g) + O2(g) ⇌ 2 SO3(g).

 

If initial concentrations are [SO2] = 6.00 M, [O2] = 0.45 M, and [SO3] = 9.00 M, the system is

1. A) at equilibrium.
2. B) not at equilibrium and will remain in an unequilibrated state.
3. C) not at equilibrium and will shift to the left to achieve an equilibrium state.
4. D) not at equilibrium and will shift to the right to achieve an equilibrium state.

Answer:  A

Diff: 2    Page Ref: 14.9

Global:  G2

LO:  14.9a

 

100) The equilibrium constant, Kp, equals 3.40 at 25°C for the isomerization reaction:

            cis-2-butene ⇌ trans-2-butene.

If a flask initially contains 5.00 atm of each gas, in what direction will the system shift to reach equilibrium?

1. A) It will shift left.
2. B) It will shift right.
3. C) The system is already at equilibrium.
4. D) The system is not at equilibrium and will remain in an unequilibrated state.

Answer:  B

Diff: 3    Page Ref: 14.9

Global:  G2