Deck 14: Chemical Equilibrium

Question 1

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.

Answer 1

The forward reaction is favoured.

Question 2

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 =

Answer 2

K_P =

Question 3

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

Answer 3

2.13

Question 4

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 5

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 6

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 7

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

Question 8

Which of the following statements is TRUE about the implication of K ≈ 1?

A) At equilibrium, the amount of products is favoured over the amount of reactants.
B) At equilibrium, the amount of reactants is favoured over the amount of products.
C) The rate of the reaction is fast.
D) The reverse reaction is favoured.
E) Neither the forward nor reverse reaction is strongly favoured; the forward reaction proceeds about halfway.

Question 9

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

Question 10

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 11

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 exists 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 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

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

Question 14

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 15

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 16

Which of the following statements is TRUE about the implication of K << 1?

A) At equilibrium, the amount of products is favoured over the amount of reactants.
B) At equilibrium, the amount of reactants is favoured over the amount of products.
C) The rate of the reaction is fast.
D) The reverse reaction is favoured.
E) Neither the forward nor reverse reaction is strongly favoured; the forward reaction proceeds about halfway.

Question 17

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 18

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 19

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 20

Which of the following statements is TRUE about the implication of K >> 1?

A) At equilibrium, the amount of products is favoured over the amount of reactants.
B) At equilibrium, the amount of reactants is favoured over the amount of products.
C) The rate of the reaction is favoured.
D) The reverse reaction is favoured.
E) Neither the forward nor reverse reaction is strongly favoured; the forward reaction proceeds about halfway.

Question 21

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 22

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 23

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 24

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 25

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 26

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 27

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 28

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 29

For which of the following reactions will ∆n = -2?

A) H₂(g) + I₂(g) ⇌ 2HI(g)
B) CH₄(g) + H₂O(g) ⇌ CO(g) + 3H₂(g)
C) N₂O₄(g) ⇌ 2NO₂(g)
D) 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)
E) N₂(g) + 3H₂(g) ⇌ 2NH₃(g)

Question 30

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 31

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 32

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 33

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 34

For which of the following reactions will ∆n = 2?

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 35

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 36

For which of the following reactions will ∆n = 1?

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 37

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 38

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 39

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 40

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 41

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 42

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 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

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 45

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 46

Which of the following statements is FALSE?

A) Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction.
B) Q < K means the reaction goes to the left (toward reactants).
C) Q < K means the reaction goes to the right (toward products).
D) Q > K means the reaction goes to the left (toward reactant).
E) Q = K means the reaction is at equilibrium.

Question 47

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

A) -1
B) 1
C) ∞
D) 0
E) Q = K

Question 48

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 49

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 50

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 51

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 52

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 53

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 54

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 55

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 56

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 57

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 58

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 59

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

A) -1
B) 1
C) ∞
D) 0
E) Q = K

Question 60

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 61

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 62

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 63

Consider the following reaction and its equilibrium constant: I₂(g) ⇌ 2I(g) K_p = 0.209 atm
A reaction mixture contains 4.0 atm I₂ and 0.5 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 64

Consider the following reaction and its equilibrium constant: I₂(g) + Br₂(g) ⇌ 2IBr(g) K_c = 1.1 × 10²
A reaction mixture contains 0.025 mol L^-1 I₂, 0.01 mol L^-1 Br₂, and 1.0 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 65

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 66

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 67

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 68

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 69

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 2.0 mol L^-1 CH₄, 0.25 mol L^-1 CO₂, and 0.5 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 70

Consider the following reaction and its equilibrium constant: SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g) K_c = 0.33
A reaction mixture contains 1.0 mol L^-1 SO₂, 0.50 mol L^-1 NO₂ , 0.50 mol L^-1 SO₃, and 1.0 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 71

Consider the following reaction and its equilibrium constant: SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g) K_c = 0.33
A reaction mixture contains 0.50 mol L^-1 SO₂, 0.25 mol L^-1 NO₂ , 0.50 mol L^-1 SO₃, and 1.0 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 72

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 73

Consider the following reaction and its equilibrium constant: SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g) K_c = 0.33
A reaction mixture contains 1.0 mol L^-1 SO₂, 2.0 mol L^-1 NO₂ , 0.66 mol L^-1 SO₃, and 1.0 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 74

What is the implication of Q > K?

A) It means the reverse reaction will proceed to form more reactants.
B) It means the forward reaction will proceed to form more products.
C) It means the reaction is at equilibrium.
D) It means the reaction is shifted to the right.

Question 75

What is the implication of Q = K?

A) It means the reverse reaction will proceed to form more reactants.
B) It means the forward reaction will proceed to form more products.
C) It means the reaction is at equilibrium.
D) It means the reaction is shifted to the right.

Question 76

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 77

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 78

What is the implication of Q < K?

A) It means the reverse reaction will proceed to form more reactants.
B) It means the forward reaction will proceed to form more products.
C) It means the reaction is at equilibrium.
D) It means the reaction is shifted to the right.

Question 79

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 = 0.068 mol L^-1

A) 1.9 mol L^-1
B) 0.12 mol L^-1
C) 0.60 mol L^-1
D) 0.028 mol L^-1
E) 0.036 mol L^-1

Question 80

Consider the following reaction and its equilibrium constant: I₂(g) + Br₂(g) ⇌ 2IBr(g) K_c = 1.1 × 10²
A reaction mixture contains 0.5 mol L^-1 I₂, 1.0 mol L^-1 Br₂, and 2.0 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.