Deck 14: Chemical Equilibrium

Question 1

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. N₂O₄(g)⇌ 2NO₂(g)K = 1.46
3N₂O₄(g)⇌ 6NO₂(g)K = ?

A)2.13
B)0.685
C)3.11
D)1.46
E)1.13

Answer 1

3.11

Question 2

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. H₂(g)+ Br₂(g)⇌ 2HBr(g)K = 3.8 × 10⁴
2HBr(g)⇌ H₂(g)+ Br₂(g)K = ?

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

Answer 2

2.6 × 10^-5

Question 3

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. H₂(g)+ Br₂(g)⇌ 2HBr(g)K = 3.8 × 10⁴
4HBr(g)⇌ 2H₂(g)+ 2Br₂(g)K = ?

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

Answer 3

6.9 × 10^-10

Question 4

For the following reaction, what is Δn required in the conversion of K_c to K_p? N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

A)4
B)-4
C)-2
D)2
E)1

Question 5

Express the equilibrium constant for the following reaction: CH₃Cl(g)+ 1/2 Cl₂(g)⇔ CH₂Cl₂(g)+ 1/2 H₂(g)

A)K_P =
B)K_P =
C)K_P =
D)K_P =
E)K_P =

Question 6

Which of the following statements is correct?

A)When K >> 1, the reverse reaction is favoured and essentially goes to completion.
B)When K << 1, the forward reaction is favoured and the reverse reaction does not proceed to a great extent.
C)When K ≈ 1, neither the forward nor reverse reaction is strongly favoured, 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)When K = 0 the reaction is in equilibrium.

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) K_c = 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: 2NH₃(g)⇔ N₂(g)+ 3H₂(g)

A)K_P =
B)K_P =
C)K_P =
D)K_P =
E)K_P =

Question 9

Express the equilibrium constant for the following reaction: N₂(g)+ 3H₂(g)⇔ 2NH₃(g)

A)K_P =
B)K_P =
C)K_P =
D)K_P=
E)K_P =

Question 10

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. N₂O₄(g)⇌ 2NO₂(g)K = 1.46
2N₂O₄(g)⇌ 4NO₂(g)K = ?

A)2.13
B)0.685
C)3.11
D)1.46
E)1.13

Question 11

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) K = 0.24
AB(g)+ A(g)⇌ A₂B(g)K = 3.8
2A(g)+ B(g)⇌ A₂B(g)K = ?

A)4.0
B)0.91
C)3.6
D)16
E)0.63

Question 12

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. 2SO₂(g)+ O₂(g)⇌ 2SO₃(g)K = 1.7 × 10⁶
SO₃(g)⇌ 1/2 O₂(g)+ SO₂(g)K = ?

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

Question 13

Express the equilibrium constant for the following reaction: 2P(g)+ 3Cl₂(g)⇌ 2PCl₃(g)

A)K_P =
B)K_P =
C)K_P =
D)K_P =
E)K_P =

Question 14

Express the equilibrium constant for the following reaction: H₂(g)+ Br₂(g)⇌ 2HBr(g)

A)K_P =
B)K_P =
C)K_P =
D)K_P =
E)K_P =

Question 15

Express the equilibrium constant for the following reaction: P(g)+ 3/2 Cl₂(g)⇌ PCl₃(g)

A)K_P =
B)K_P =
C)K_P =
D)K_P =
E)Kp =

Question 16

Express the equilibrium constant for the following reaction: PCl₅(g)⇌ PCl₃(g)+ Cl₂(g)

A)K_P =
B)K_P =
C)K_P =
D)K_P =
E)K_P =

Question 17

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

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

Question 18

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

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

Question 19

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. 2HD(g)⇌ H₂(g)+ D₂(g) K = 0.28
2H₂(g)+ 2D₂(g)⇌ 4HD(g)K = ?

A)7.8 × 10^-2
B)3.6
C)0.53
D)13
E)1.9

Question 20

Express the equilibrium constant for the following reaction: 2 CH₃Cl(g)+ Cl₂(g)⇔ 2 CH₂Cl₂(g)+ H₂(g)

A)Kp =
B)K_P =
C)K_P =
D)K_P =
E)K_P =

Question 21

For which reaction will K_p = K_c?

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

Question 22

For the following reaction, what is Δn required in the conversion of K_c to K_p? 2SO₂(g)+ O₂(g)⇌ 2SO₃(g)

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

Question 23

For the following reaction, what is Δn required in the conversion of K_c to K_p? N₂O₄(g)⇌ 2NO₂(g)

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

Question 24

Express the equilibrium constant for the following reaction: B(OH)₃(aq) + 2H₂O(l)⇌ B(OH)₃(OH)^-(aq)+ H₃O⁺(aq)

A)K_c =
B)K_c =
C)K_c =
D)K_c =
E)K_c =

Question 25

For which of the following reactions will K_c = K_p?

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

Question 26

Express the equilibrium constant for the following reaction: KClO₃(s)⇌ KClO(s)+ O₂(g)

A)K_c =
B)K_c = [O₂]^-1
C)K_c =
D)K_c =
E)K_c = [O₂]

Question 27

For which of the following reactions will K_c = K_p?

A)4NH₃(g)+ 3O₂(g)⇌ 2N₂(g)+ 6H₂O(g)
B)SO₃(g)+ NO(g)⇌ SO₂(g)+ NO₂(g)
C)2N₂(g)+ O₂(g)⇌ 2N₂O(g)
D)2SO₂(g)+ O₂(g)⇌ 2SO₃(g)
E)PCl_3(g) + 1/2 O_2(g) ⇌ PCl₃O_(g)

Question 28

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

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

Question 29

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

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

Question 30

For the following reaction, what is △n required in the conversion of K_c to K_p? KClO₃(s)⇌ KClO(s)+ O₂(g)

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

Question 31

Express the equilibrium constant for the following reaction: SO_2(g) + H₂O(l)⇌ H₂SO₃(aq)

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

Question 32

For the following reaction, what is Δn required in the conversion of K_c to K_p? CH₄(g)+ H₂O(g)⇌ CO(g)+ 3H₂(g)

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

Question 33

For the following reaction, what is △n required in the conversion of K_c to K_p? 2Na(s)+ 2H₂O(l)⇌ 2NaOH(aq)+ H₂(g)

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

Question 34

Express the equilibrium constant for the following reaction: + 6CN^-(aq)⇌ + 6H₂O(l)

A)K_c =
B)K_c =
C)K_c =
D)K_c =
E)K_c =

Question 35

For the following reaction, what is △n required in the conversion of K_c to K_p? P₄(s)+ 5O₂(g)⇌ P₄O₁₀(s)

A)3
B)4
C)-4
D)5
E)-5

Question 36

Express the equilibrium constant for the following reaction: 2Na(s)+ 2H₂O(l)⇌ 2NaOH(aq)+ H₂(g)

A)K_c =
B)K_c = [H₂][NaOH]^-2
C)K_c =
D)K_c = [H₂][NaOH]²
E)K_c =

Question 37

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [N₂]_eq = 3.6 mol L^-1, [O₂]_eq = 4.1 mol L^-1, [N₂O]_eq = 3.3 × 10^-18 mol L^-1. 2N₂(g)+ O₂(g)⇌ 2N₂O(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 38

The reaction below has a K_c value of 1.0 × 10¹² M^-1. What is the value of K_p for this reaction at 500 K? 2SO₂(g)+ O₂(g)⇌ 2SO₃(g)

A)4.2 × 10^-11 bar^-1
B)1.0 × 10¹² bar^-1
C)2.4 × 10^-12 bar^-1
D)4.1 × 10¹³ bar^-1
E)2.4 × 10¹⁰ bar^-1

Question 39

The reaction below has a K_c value of 61 M^-2. What is the value of K_p for this reaction at 500 K? N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

A)15 bar^-2
B)61 bar^-2
C)28 bar^-2
D)3.6 × 10^-2 bar^-2
E)1.9 × 10^-2 bar^-2

Question 40

The reaction below has a K_p value of 41 bar^-2. What is the value of K_c for this reaction at 400 K? N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

A)2.4 × 10^-2 M^-2
B)4.4 × 10⁴ M^-2
C)41 M^-2
D)2.3 × 10^-5 M^-2
E)1.9 × 10⁴ M^-2

Question 41

Consider the following reaction and its equilibrium constant: I₂(g)+ Br₂(g)⇌ 2IBr(g)K_c = 1.1 × 10²
A reaction mixture contains 0.41 mol L^-1 I₂, 0.27 mol L^-1 Br₂ and 3.5 mol L^-1 IBr. Which of the following statements is TRUE concerning this system?

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

Question 42

Consider the following reaction and its equilibrium constant: 4CuO(s)+ CH₄(g)⇌ CO₂(g)+ 4Cu(s)+ 2H₂O(g)K_c = 1.10
A reaction mixture contains 0.22 mol L^-1 CH₄, 0.67 mol L^-1 CO₂ and 1.3 mol L^-1 H₂O. Which of the following statements is TRUE concerning this system?

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

Question 43

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 mol L^-1, [I₂]_eq = 0.39 mol L^-1, [HI]_eq = 1.6 mol L^-1. H₂(g)+ I₂(g)⇌ 2HI(g)

A)2.1 × 10^-2
B)29
C)47
D)3.4 × 10^-2
E)8.7 × 10^-2

Question 44

Consider the following reaction and its equilibrium constant: I₂(g)⇌ 2I(g)K_p = 0.209 atm
A reaction mixture contains 0.89 atm I₂ and 1.77 atm I. Which of the following statements is TRUE concerning this system?

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

Question 45

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)If Q << K, it means the reaction is shifted to the left.
E)If Q >> K, it means the reaction is shifted to the right.

Question 46

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

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

Question 47

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

A)-1
B)1
C)∞
D)0
E)Q = K

Question 48

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [HCl]_eq = 0.13 mol L^-1, [HI]_eq = 5.6 × 10^-16 mol L^-1, [Cl₂]_eq = 0.0019 mol L^-1. 2HCl(g)+ I₂(s)⇌ 2HI(g)+ Cl₂(g)

A)8.2 × 10^-18 M
B)2.9 × 10³¹ M
C)1.2 × 10¹⁷ M
D)1.4 × 10^-19 M
E)3.5 × 10^-32 M

Question 49

Determine the value of K_p 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. 2NOCl(g)⇌ 2NO(g)+ Cl₂(g)

A)3.7 × 10^-2 atm
B)60 atm
C)27 atm
D)1.7 × 10^-2 atm
E)1.8 × 10^-3 atm

Question 50

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO₃(g). 2SO₂(g)+ O₂(g)⇌ 2SO₃(g) K_c = 1.7 × 10⁸ M^-1
[SO₂]_eq = 0.0034 mol L^-1 [O₂]_eq = 0.0018 mol L^-1

A)1.9 mol L^-1
B)1.0 × 10³ mol L^-1
C)0.53 mol L^-1
D)9.6 × 10^-4 mol L^-1
E)0.73 mol L^-1

Question 51

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)Because the equilibrium is always dynamic, Q can never be equal to K.
E)If Q < K, the reaction proceeding to the left is much faster than the reaction proceeding to the right.

Question 52

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [N₂]_eq = 1.5 mol L^-1, [H₂]_eq = 1.1 mol L^-1, [NH₃]_eq = 0.47 mol L^-1. N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

A)3.5 M^-2
B)0.28 M^-2
C)9.1 M^-2
D)0.11 M^-2
E)0.78 M^-2

Question 53

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

A)-1
B)1
C)∞
D)0
E)Q = K

Question 54

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

A)-1
B)1
C)∞
D)0
E)Q = K

Question 55

Consider the following reaction and its equilibrium constant: SO₂(g)+ NO₂(g)⇌ SO₃(g)+ NO(g)K_c = 0.33
A reaction mixture contains 0.39 mol L^-1 SO₂, 0.14 mol L^-1 NO₂ , 0.11 mol L^-1 SO₃ and 0.14 mol L^-1 NO. Which of the following statements is TRUE concerning this system?

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

Question 56

Calculate the value of [N₂]_eq if [H₂]_eq = 2.0 mol L^-1, [NH₃]_eq = 0.50 mol L^-1, and K_c = 2.0. N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

A)0.016 mol L^-1
B)0.031 mol L^-1
C)0.062 mol L^-1
D)0.40 mol L^-1
E)62.5 mol L^-1

Question 57

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [PCl₅]_eq = 0.56 mol L^-1, [PCl₃]_eq = 0.23 mol L^-1, [Cl₂]_eq = 4.4 mol L^-1. PCl₅(g)⇌ PCl₃(g)+ Cl₂(g)

A)1.8 M
B)0.93 M
C)0.55 M
D)1.1 M
E)0.76 M

Question 58

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 favour the production of more products.
D)Dynamic equilibrium indicates that the amount of reactants and products are equal.
E)Dynamic equilibrium is established when K = 0.

Question 59

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 atm^-1
B)2.8 × 10²⁰ atm^-1
C)4.6 × 10¹¹ atm^-1
D)2.2 × 10^-12 atm^-1
E)3.6 × 10^-15 atm^-1

Question 60

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 M^-1
[C₂H₄]_eq = 0.015 mol L^-1 [C₂H₅OH]_eq = 1.69 mol L^-1

A)9.9 × 10^-7 mol L^-1
B)80. mol L^-1
C)1.0 mol L^-1
D)1.68 mol L^-1
E)0.013 mol L^-1

Question 61

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

A)raising the temperature
B)removing SO₃
C)adding O₂
D)increasing the pressure
E)adding SO₂

Question 62

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 NO₂ is not included in the equilibrium expression.
D)The reaction will shift in the direction of reactants.
E)The equilibrium constant will decrease.

Question 63

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO₂(g). N₂O₄(g)⇌ 2NO₂(g) K_c = 0.21 M
[N₂O₄]_eq = 0.039 mol L^-1

A)1.22 mol L^-1
B)9.0 × 10^-2 mol L^-1
C)7.8 × 10^-2 mol L^-1
D)8.2 × 10^-3 mol L^-1
E)11 mol L^-1

Question 64

Consider the following reaction at equilibrium. What effect will adding more H₂S have on the system? 2H₂S(g)+ 3O₂(g)⇌ 2H₂O(g)+ 2SO₂(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 65

Consider the following reaction: CH₄(g)+ 2H₂S(g)⇌ CS₂(g)+ 4H₂(g)
A reaction mixture initially contains 0.50 mol L^-1 CH₄ and 0.75 mol L^-1 H₂S. If the equilibrium concentration of H₂ is 0.44 mol L^-1, find the equilibrium constant (mol L^-1)for the reaction.

A)0.23 mol² L^-2
B)0.038 mol² L^-2
C)2.9 mol² L^-2
D)10. mol² L^-2
E)0.34 mol² L^-2

Question 66

Identify the change that will always shift the equilibrium to the right.

A)remove reactant
B)increase product
C)remove product
D)increase pressure
E)increase volume

Question 67

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of CO₂(g). NH₂COONH₄(s)⇌ 2NH₃(g)+ CO₂(g)K_c = 1.58 × 10^-8 M³
[NH₃]_eq = 2.9 × 10^-3 mol L^-1

A)0.053 mol L^-1
B)4.6 × 10^-11 mol L^-1
C)1.9 × 10^-3 mol L^-1
D)5.4 × 10^-6 mol L^-1
E)0.022 mol L^-1

Question 68

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO₂(g). 2SO₂(g)+ O₂(g)⇌ 2SO₃(g) K_c = 1.7 × 10⁸ M^-1
[SO₃]_eq = 0.0034 mol L^-1 [O₂]_eq = 0.0018 mol L^-1

A) 2.8 × 10¹³ mol L^-1
B) 1.88 mol L^-1
C)6.1 × 10^-6 mol L^-1
D)1.0 × 10³ mol L^-1
E)1.4 mol L^-1

Question 69

Consider the following reaction at equilibrium. What effect will removing H₂O have on the system? 2H₂S(g)+ 3O₂(g)⇌ 2H₂O(g)+ 2SO₂(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 70

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium pressure of H₂. D₂(g)+ H₂(g)⇌ 2HD(g)K_p = 1.80
P(D₂)_eq = 1.1 × 10^-3 bar P(HD)_eq = 2.7 × 10^-3 bar

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

Question 71

Consider the following reaction: CO₂(g)+ C(graphite)⇌ 2CO(g)
A reaction mixture initially contains 0.56 bar CO₂ and 0.32 bar CO. Determine the equilibrium pressure of CO if K_p for the reaction at this temperature is 2.25 bar.

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

Question 72

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 73

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

A)raising the temperature
B)adding a solid
C)adding argon
D)all of the above
E)none of the above

Question 74

Consider the following reaction: Xe(g)+ 2F₂(g)⇌ XeF₄(g)
A reaction mixture initially contains 2.24 bar Xe and 4.27 bar F₂. If the equilibrium pressure of Xe is 0.34 bar, find the equilibrium constant (K_p)for the reaction.

A)25 bar^-2
B)0.12 bar^-2
C)0.99 bar^-2
D)8.3 bar^-2
E)0.040 bar^-2

Question 75

Consider the following reaction: 2H₂O(g)+ 2SO₂(g)⇌ 2H₂S(g)+ 3O₂(g)
A reaction mixture initially contains 2.8 mol L^-1 H₂O and 2.6 mol L^-1 SO₂. Determine the equilibrium concentration of H₂S if K_c for the reaction at this temperature is 1.3 × 10^-6 mol L^-1.

A)0.045 mol L^-1
B)0.058 mol L^-1
C)0.028 mol L^-1
D)3.1 × 10^-3 mol L^-1
E)0.12 mol L^-1

Question 76

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium pressure of CO. CO(g)+ 2H₂(g)⇌ CH₃OH(l)K_p = 2.25 × 10⁴ bar^-3
P(H₂)_eq = 0.52 bar

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

Question 77

Consider the following reaction: COCl₂(g)⇌ CO(g)+ Cl₂(g)
A reaction mixture initially contains 1.6 mol L^-1 COCl₂. Determine the equilibrium concentration of CO if K_c for the reaction at this temperature is 8.33 × 10^-4 M. Calculate this based on the assumption that the answer is negligible compared to 1.6.

A)4.2 × 10^-4 mol L^-1
B)1.5 × 10^-3 mol L^-1
C)3.7 × 10^-2 mol L^-1
D)2.1 × 10^-2 mol L^-1
E)1.3 × 10^-3 mol L^-1

Question 78

Consider the following reaction: CuS(s)+ O₂(g)⇌ Cu(s)+ SO₂(g)
A reaction mixture initially contains 2.9 mol L^-1 O₂. Determine the equilibrium concentration of O₂ if K_c for the reaction at this temperature is 1.5.

A)1.9 mol L^-1
B)1.7 mol L^-1
C)2.2 mol L^-1
D)1.2 mol L^-1
E)0.59 mol L^-1

Question 79

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

A)raising the temperature
B)decreasing the pressure
C)increasing the volume
D)all of the above
E)none of the above

Question 80

Consider the following reaction: NO(g)+ SO₃(g)⇌ NO₂(g)+ SO₂(g)
A reaction mixture initially contains 0.86 bar NO and 0.86 bar SO₃. Determine the equilibrium pressure of NO₂ if K_p for the reaction at this temperature is 0.0118.

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