Deck 16: Chemical Equilibrium

Question 1

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)K_c = 1.7 × 10⁶
SO₃(g)⇌ 1/2 O₂(g)+ SO₂(g)K_c = ?

A) 3.4 × 10²
B) 8.5
C) 1.3 × 10³
D) 1.2 × 10^-6
E) 7.7 × 10^-4

Answer 1

7.7 × 10^-4

Question 2

In which of the following reactions will K_c = K_p?

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

Answer 2

SO₃(g) + NO(g) ⇌ SO₂(g) + NO₂(g)

Question 3

What is Δn for the following equation in relating K_c to K_p?
N₂O₄(g)⇌ 2NO₂(g)

A) 3
B) -1
C) -2
D) 2
E) 1

Answer 3

1

Question 4

Which of the following statements is FALSE?

A) When K >> 1, the forward reaction is favored and essentially goes to completion.
B) When K << 1, the reverse reaction is favored and the forward reaction does not proceed to a great extent.
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.
D) K >> 1 implies that the reaction is very fast at producing products.
E) None of the above

Question 5

Chemical equilibrium is the result of

A) all of the reactants being converted into products.
B) stoppage of further reaction.
C) formation of products equal in mass to the mass of the reactants.
D) opposing reactions attaining equal rates.
E) a loss of pressure in the system.

Question 6

Equilibrium in which rate of the forward reaction equals the rate of the reverse reaction is

A) dynamic.
B) temperature independent.
C) concentration independent.
D) volume independent.
E) impossible.

Question 7

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)K_c = ?
A(g)+ 3B(g)⇌ AB₃(g)K_c = 478

A) 3.5 × 10^-5
B) 2.8 × 10⁴
C) 8.1
D) 0.12
E) 89

Question 8

Express the equilibrium constant for the following reaction. 16 CH₃Cl(g)+ 8 Cl₂(g)⇔ 16 CH₂Cl₂(g)+ 8 H_2(g)

A) K =
B) K =
C) K =
D) K =
E) K =

Question 9

What is Δn for the following equation in relating K_c to K_p?
SO₃(g)+ NO(g)⇌ SO₂(g)+ NO₂(g)

A) 0
B) -1
C) -2
D) 2
E) 1

Question 10

What is Δn for the following equation in relating K_c to K_p?
2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g)

A) 3
B) -1
C) -2
D) 2
E) 1

Question 11

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)K_c = 3.8 × 10⁴
4 HBr(g)⇌ 2 H₂(g)+ 2 Br₂(g)K_c = ?

A) 1.9 × 10⁴
B) 5.1 × 10^-3
C) 2.6 × 10^-5
D) 6.9 × 10^-10
E) 1.6 × 10³

Question 12

Give the direction of the reaction,if K ≈ 1.

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

Question 13

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

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

Question 14

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

A) 1.9 × 10⁴
B) 5.3 × 10^-5
C) 2.6 × 10^-5
D) 6.4 × 10^-4
E) 1.6 × 10³

Question 15

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

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

Question 16

What is Δn for the following equation in relating K_c to K_p?
4 NH₃(g)+ 3 O₂(g)⇌ 2 N₂(g)+ 6 H₂O(g)

A) 3
B) -1
C) -2
D) 2
E) 1

Question 17

What is Δn for the following equation in relating K_c to K_p?
C₃H₈(g)+ 5 O₂(g)⇌ 3 CO₂(g)+ 4 H₂O(l)

A) 3
B) -1
C) -3
D) 2
E) 1

Question 18

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)K_c = 3.8
2 A(g)+ B(g)⇌ A₂B(g)K_c = ?

A) 4.0
B) 0.91
C) 3.6
D) 16
E) 0.063

Question 19

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. 2A(g)+ B(g)⇌ A₂B(g)Kc = ?
A₂B(g)+ B(g)⇌ A₂B₂(g)K_c = 16.4
2A(g)+ 2B(g)⇌ A₂B₂(g)K_c = 28.2

A) 11.8
B) 0.00216
C) 0.582
D) 462
E) 1.72

Question 20

The reaction below has a K_p value of 3.3 × 10^-5.What is the value of K_c for this reaction at 700 K?
2 SO₃(g)⇌ 2 SO₂(g)+ O₂(g)

A) 5.7 × 10^-7
B) 1.7 × 10⁶
C) 3.3 × 10^-5
D) 3.0 × 10⁴
E) 1.9 × 10^-3

Question 21

Express the equilibrium constant for the following reaction. P₄(s)+ 5 O₂(g)⇌ P₄O₁₀(s)

A) K =
B) K =
C) K = [O₂]^-5
D) K = [O₂]⁵
E) K =

Question 22

The reaction below has a K_c value of 3.64 × 10^-3.What is the value of K_p for this reaction at 25°C?
2 NaN₃(s)⇌ 2 Na(s)+ 3 N₂(g)

A) 131
B) 0.613
C) 8.90 × 10^-2
D) 29.9
E) 53.2

Question 23

Which of the following statements is TRUE?

A) If Q < K, it means the forward reaction will proceed to form more products.
B) If Q > K, it means the forward reaction will proceed to form more products.
C) If Q = K, it means the reaction is not at equilibrium.
D) All of the above are true.
E) None of the above are true.

Question 24

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [P₄O₁₀]_eq = 2.000 moles,[P₄]_eq = 3.000 moles,[O₂]_eq = 4.000 M P₄O₁₀(s)⇌ P₄(s)+ 5 O₂(g)

A) 20.00
B) 4.000
C) 1.320
D) 1536
E) 1024

Question 25

In a reaction mixture containing only products,what is the value of Q?

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

Question 26

In a reaction mixture containing reactants and products,each at a concentration of 1M,what is the value of Q?

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

Question 27

Determine the value of K_c 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)

A) 3.5
B) 0.28
C) 9.1
D) 0.11
E) 0.78

Question 28

Which of the following statements is TRUE?

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

Question 29

Determine the value of K_c 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 HI(g)+ Cl₂(g)⇌ 2 HCl(g)+ I₂(s)

A) 8.2 × 10^-18
B) 2.8 × 10³¹
C) 1.2 × 10¹⁷
D) 1.4 × 10^-19
E) 3.5 × 10^-32

Question 30

Determine the value of K_c 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)

A) 8.2 × 10^-18
B) 2.8 × 10³¹
C) 1.2 × 10¹⁷
D) 1.4 × 10^-19
E) 3.5 × 10^-32

Question 31

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)K_c = 9.0 × 10³
[C₂H₄]_eq = 0.015 M [C₂H₅OH]_eq = 1.69 M

A) 9.9 × 10^-7 M
B) 80. M
C) 1.0 M
D) 1.68 M
E) 0.013 M

Question 32

Calculate the value of [N₂]_eq if [H₂]_eq = 2.0 M,[NH₃]_eq = 0.5 M,and K_c = 2. N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g)

A) 0.016 M
B) 0.031 M
C) 0.062 M
D) 0.40 M
E) 62.5 M

Question 33

Express the equilibrium constant for the following reaction. P₄O₁₀(s)⇌ P₄(s)+ 5 O₂(g)

A) K =
B) K =
C) K = [O₂]^-5
D) K = [O₂]⁵
E) K =

Question 34

Calculate P [NO]eq,if P [NOCl]_eq = 0.33 atm,P [Cl₂]_eq = 0.50 atm,and K_p = 1.9 × 10^-2. 2 NOCl(g)⇌ 2 NO(g)+ Cl₂(g)

A) 1.7 atm
B) 0.0042 atm
C) 0.30 atm
D) 0.064 atm
E) 0.087 atm

Question 35

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 (K_c)for the reaction.

A) 0.23
B) 0.038
C) 2.9
D) 10.
E) 0.34

Question 36

Determine the value of K_c 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)

A) 2.2 × 10^-19
B) 4.5 × 10¹⁸
C) 2.0 × 10^-37
D) 5.0 × 10³⁶
E) 4.9 × 10^-17

Question 37

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

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

Question 38

Determine the value of K_p 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)

A) 3.6 × 10^-21
B) 2.8 × 10²⁰
C) 4.6 × 10¹¹
D) 2.2 × 10^-12
E) 3.6 × 10^-15

Question 39

Which of the following statements is TRUE?

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

Question 40

Which of the following statements is TRUE?

A) If Q < K, it means the reverse reaction will proceed to form more reactants.
B) If Q > K, it means the reverse reaction will proceed to form more reactants.
C) If Q = K, it means the reaction is not at equilibrium.
D) All of the above are true.
E) None of the above are true.

Question 41

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 K_c for the reaction at this temperature is 1.3 × 10^-6.

A) 0.045 M
B) 0.058 M
C) 0.028 M
D) 3.1 × 10^-3 M
E) 0.12 M

Question 42

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)K_p = 2.25 × 10⁴
P(H₂)_eq = 0.52 atm

A) 8.3 × 10⁴ atm
B) 1.2 × 10^-5 atm
C) 6.25 × 10^-3 atm
D) 8.5 × 10^-5 atm
E) 1.6 × 10^-4 atm

Question 43

Consider the following reaction at equilibrium.What effect will raising the pressure of the system from 5 atm to 8 atm?
2 NH₃(g)⇌ N₂(g)+ 3 H₂(g)

A) It will shift to the right
B) It will shift to the left
C) It will have no effect
D) It will speed up the reaction
E) It will slow down the reaction

Question 44

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)

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

Question 45

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 (K_p)for the reaction.

A) 25
B) 0.12
C) 0.99
D) 8.3
E) 0.040

Question 46

The following reaction is exothermic.What set of conditions will always lead to the equilibrium shifting to the left?
2 NO(g)+ Br₂(g)⇌ 2 NOBr(g)

A) decrease the volume, decrease the temperature
B) increase the volume, decrease the temperature
C) increase the volume, increase the temperature
D) decrease the volume, increase the temperature
E) none of the above

Question 47

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 K_c for the reaction at this temperature is 1.5.

A) 1.9 M
B) 1.7 M
C) 2.2 M
D) 1.2 M
E) 0.59 M

Question 48

The following reaction is exothermic.Which change will shift the equilibrium to the left?
2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g)

A) raising the temperature
B) adding SO₃
C) removing O₂
D) all of the above
E) none of the above

Question 49

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 K_c 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.

A) 4.2 × 10^-4 M
B) 1.5 × 10^-3 M
C) 3.7 × 10^-2 M
D) 2.1 × 10^-2 M
E) 1.3 × 10^-3 M

Question 50

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)

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

Question 51

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 K_p for the reaction at this temperature is 2.25.

A) 0.83 atm
B) 0.31 atm
C) 0.26 atm
D) 0.58 atm
E) 0.42 atm

Question 52

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)K_p = 1.80
P(D₂)_eq = 1.1 × 10^-3 atm P(HD)_eq = 2.7 × 10^-3 atm

A) 2.7 atm
B) 1.4 atm
C) 0.73 atm
D) 3.7 × 10^-3 atm
E) 8.1 × 10^-4 atm

Question 53

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 K_p for the reaction at this temperature is 0.0118.

A) 0.78 atm
B) 0.084 atm
C) 0.012 atm
D) 0.85 atm
E) 0.048 atm

Question 54

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)K_c = 1.7 × 10⁸
[SO₂]_eq = 0.0034 M [O₂]_eq = 0.0018 M

A) 1.9 M
B) 1.0 × 10³ M
C) 0.53 M
D) 9.6 × 10^-4 M
E) 0.73 M

Question 55

Consider the following reaction at equilibrium.What effect will adding more SO₃ have on the system?
SO₂(g)+ NO₂(g)⇌ SO₃(g)+ NO(g)

A) The reaction will shift in the direction of products.
B) The reaction will shift to decrease the pressure.
C) No change will occur since SO₃ is not included in the equilibrium expression.
D) The reaction will shift in the direction of reactants.
E) The equilibrium constant will decrease.

Question 56

The following reaction is exothermic.Which change will shift the equilibrium to the left?
2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g)

A) raising the temperature
B) decrease pressure
C) increase volume
D) all of the above
E) none of the above

Question 57

The following reaction is endothermic.What effect will decreasing the temperature have on the system?
I₂(g)+ Cl₂(g)⇌ 2 ICl(g)

A) The equilibrium constant will change and the reaction will proceed in the forward direction
B) The equilibrium constant will change and the reaction will proceed in the reverse direction
C) The equilibrium constant will remain constant and the reaction will proceed in the forward direction
D) The equilibrium constant will remain constant and the reaction will proceed in the reverse direction

Question 58

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)K_c = 1.7 × 10⁸
[SO₃]_eq = 0.0034 M [O₂]_eq = 0.0018 M

A) 2.8 × 10¹³ M
B) 1.88 M
C) 6.1 × 10^-6 M
D) 1.0 × 10³ M
E) 1.4 M

Question 59

Consider the following reaction at equilibrium.What effect will removing NO₂ have on the system?
SO₂(g)+ NO₂(g)⇌ SO₃(g)+ NO(g)

A) The reaction will shift in the direction of products.
B) The reaction will shift to decrease the pressure.
C) No change will occur since SO₃ is not included in the equilibrium expression.
D) The reaction will shift in the direction of reactants.
E) The equilibrium constant will decrease.

Question 60

Consider the following reaction at equilibrium.What effect will removing H₂O have on the system?
2 H₂S(g)+ 3 O₂(g)⇌ 2 H₂O(g)+ 2 SO₂(g)

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

Question 61

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [C₃H₈]= 0.15 M,[O₂] = 0.35 M,[CO₂] = 1.3 M,[H₂O] = 2.8 M C₃H₈(g)+ 5 O₂(g)⇌ 3 CO₂(g)+ 4 H₂O(g)

A) 1.7 × 10⁵
B) 3.2 × 10-6
C) 6.7 × 10³
D) 7.4 × 10²
E) 6.1.9 × 10^-4

Question 62

Consider the following reaction at equilibrium.What effect will adding some C have on the system?
CO₂(g)+ C(graphite)⇌ 2 CO(g)

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

Question 63

Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system?
CuS(s)+ O₂(g)⇌ Cu(s)+ SO₂(g)

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

Question 64

Consider the following reaction at equilibrium.What effect will reducing the volume have on the system?
C₃H₈(g)+ 5 O₂(g)⇌ 3 CO₂(g)+ 4 H₂O(l)ΔH° = -2220 kJ

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

Question 65

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of H₂O(g). 2 H₂(g)+ O₂(g)⇌ 2 H₂O(g)K_c = 5.50 × 10²
[H₂] = 0.480 M [O₂] = 0.310 M

A) 4.23 × 10^-3 M
B) 0.426 M
C) 6.27 M
D) 39.3 M
E) 5.52 × 10⁶ M

Question 66

The following reaction is allowed to come to equilibrium with a measured partial pressure of 0.68 atm for O₂,0.72 atm for N₂,and 2.83 atm for NO.What is K_p for the reaction at this temperature?
N₂(g)+ O₂(g)→ 2 NO(g)

A) 32.7
B) 16.4
C) 5.78
D) 2.29
E) 0.0611

Question 67

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)

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

Question 68

For the following reaction: I₂(g)+ Br₂(g)⇌ 2 IBr(g)
A vessel initially contains 2.50 M I₂ and 2.50 M Br₂.Determine the equilibrium concentration of IBr if K_c for the reaction at this temperature is 3.27.

A) 1.19 M
B) 1.84 M
C) 2.18 M
D) 0.854 M
E) 0.642 M

Question 69

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

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

Question 70

Consider the following reaction at equilibrium.What effect will adding CO₂ have on the system?
CO₂(g)+ C(graphite)⇌ 2 CO(g)

A) No effect will be observed since CO₂ is not included in the equilibrium expression.
B) The equilibrium constant will decrease.
C) The reaction will shift to the left in the direction of reactants.
D) The equilibrium constant will increase.
E) The reaction will shift to the right in the direction of products.

Question 71

Express the equilibrium constant for the following reaction. 2 N₂(g)+ 6 H₂(g)⇔ 4 NH₃(g)

A) K =
B) K =
C) K =
D) K =
E) K =

Question 72

For the following reaction of N₂O₄,the equilibrium constant is 0.593 at a particular temperature. N₂O₄(g)⇌ 2 NO₂(g)
If the initial concentration of N₂O₄ is 0.880M,what are the equilibrium concentrations?

A) [N₂O₄] = 0.705M, [NO₂] = 0.350M
B) [N₂O₄] = 0.678M, [NO₂] = 0.404M
C) [N₂O₄] = 0.332M, [NO₂] = 1.094M
D) [N₂O₄] = 0.586M, [NO₂] = 0.588M
E) [N₂O₄] = 0.000M, [NO₂] = 1.760M

Question 73

Consider the following reaction at equilibrium.What effect will reducing the pressure have on the system?
C₃H₈(g)+ 5 O₂(g)⇌ 3 CO₂(g)+ 4 H₂O(l)ΔH° = -2220 kJ

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

Question 74

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

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

Question 75

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

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

Question 76

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)

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

Question 77

Consider the following reaction at equilibrium.What effect will adding 1 mole of Ar to the reaction mixture have on the system?
2 H₂S(g)+ 3 O₂(g)⇌ 2 H₂O(g)+ 2 SO₂(g)

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

Question 78

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)

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

Question 79

Express the equilibrium constant for the following reaction. 3 CH₃Cl(g)+ 3/2 Cl₂(g)⇔ 3 CH₂Cl₂(g)+ 3/2 H_2(g)

A) K =
B) K =
C) K =
D) K =
E) K =

Question 80

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)

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