Question 1

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

Accepted Answer

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. 
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 2

Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ⇌ 2IBr(g) Kc = 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?

Accepted Answer

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. 
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 3

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

Accepted Answer

A)  Kc =   
B)  Kc =   
C)  Kc =   
D)  Kc =   
E)  Kc =   
A)  Kc =   
B)  Kc =   
C)  Kc =   
D)  Kc =   
E)  Kc =

Question 4

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

Accepted Answer

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 
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 5

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

Accepted Answer

A)  KP =   
B)  KP =   
C)  KP =   
D)  KP =   
E)  KP =   
A)  KP =   
B)  KP =   
C)  KP =   
D)  KP =   
E)  KP =

Question 6

Consider the following reaction and its equilibrium constant: 4CuO(s) + CH4(g) ⇌ CO2(g) + 4Cu(s) + 2H2O(g) Kc = 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?

Accepted Answer

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. 
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 7

Express the equilibrium constant for the following reaction: SO2(g) + H2O(l) ⇌ H2SO3(aq)

Accepted Answer

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

Question 8

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

Accepted Answer

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

Question 9

Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ⇌ 2IBr(g) Kc = 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?

Accepted Answer

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. 
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 10

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. 2NOCl(g) ⇌ 2NO(g) + Cl2(g)

Accepted Answer

A)  3.7 × 10-2 atm 
B)  60 atm 
C)  27 atm 
D)  1.7 × 10-2 atm 
E)  1.8 × 10-3 atm 
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 11

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 Kc for the reaction at this temperature is 1.3 × 10-6 mol L-1.

Accepted Answer

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 
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 12

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO2(g). N2O4(g) ⇌ 2NO2(g) Kc = 0.21 M
[N2O4]eq = 1.34 mol L-1

Accepted Answer

A)  0.25 mol L-1 
B)  0.043 mol L-1 
C)  0.60 mol L-1 
D)  0.028 mol L-1 
E)  0.53 mol L-1 
A)  0.25 mol L-1 
B)  0.043 mol L-1 
C)  0.60 mol L-1 
D)  0.028 mol L-1 
E)  0.53 mol L-1

Question 13

For which of the following reactions will Kc = Kp?

Accepted Answer

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) 
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 14

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.

Accepted Answer

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 
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 15

Dinitrogen tetroxide partially decomposes according to the following equilibrium:     (g) ⇌   (g) A 1.000 L flask is charged with 6.00 × 10-2 mol of     . At equilibrium, 3.21 × 10-2 mol of     remains.   for this reaction is ________.

Accepted Answer

A)  10.3 mol L-1 
B)  1.74 mol L-1 
C)  0.465 mol L-1 
D)  2.42 × 10-2 mol L-1 
E)  9.70 × 10-2 mol L-1 
A)  10.3 mol L-1 
B)  1.74 mol L-1 
C)  0.465 mol L-1 
D)  2.42 × 10-2 mol L-1 
E)  9.70 × 10-2 mol L-1

Question 16

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 mol L-1 and 0. 075 mol L-1, respectively.

Accepted Answer

A)  [C6H12] = 0. 041 mol L-1, [CH3C5H9] = 0. 041 mol L-1 
B)  [C6H12] = 0. 159 mol L-1, [CH3C5H9] = 0. 116 mol L-1 
C)  [C6H12] = 0. 241 mol L-1, [CH3C5H9] = 0. 034 mol L-1 
D)  [C6H12] = 0. 253 mol L-1, [CH3C5H9] = 0. 022 mol L-1 
A)  [C6H12] = 0. 041 mol L-1, [CH3C5H9] = 0. 041 mol L-1 
B)  [C6H12] = 0. 159 mol L-1, [CH3C5H9] = 0. 116 mol L-1 
C)  [C6H12] = 0. 241 mol L-1, [CH3C5H9] = 0. 034 mol L-1 
D)  [C6H12] = 0. 253 mol L-1, [CH3C5H9] = 0. 022 mol L-1

Question 17

Match the following.
-K ≈ 1

Accepted Answer

A) reverse reaction is favoured 
B) reaction is at equilibrium 
C) reaction favours formation of more products 
D) reaction does not strongly favour reactants or products 
E) reaction has a larger amount of products than reactants
F)reaction will favour formation of reactants 
A) reverse reaction is favoured 
B) reaction is at equilibrium 
C) reaction favours formation of more products 
D) reaction does not strongly favour reactants or products 
E) reaction has a larger amount of products than reactants
F)reaction will favour formation of reactants

Question 18

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

Accepted Answer

The expressions for both are identical.

Question 19

Kc is 1.67 × 1020 mol3 L-3 at 25 °C for the formation of iron(III) oxalate complex ion: Fe3+(aq) + 3C2O42-(aq) ⇌ [Fe(C2O4)3]3-(aq)
If 0. 0200 mol L-1 Fe3+ is initially mixed with 1.00 mol L-1 oxalate ion, what is the concentration of Fe3+ ion at equilibrium?

Accepted Answer

A)  1.44 × 10-22 mol L-1 
B)  0.0100 mol L-1 
C)  8.35 × 1019 mol L-1 
D)  6.94 × 1021 mol L-1 
A)  1.44 × 10-22 mol L-1 
B)  0.0100 mol L-1 
C)  8.35 × 1019 mol L-1 
D)  6.94 × 1021 mol L-1

Question 20

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

Accepted Answer

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

Exam 14: Chemical Equilibrium

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

Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ⇌ 2IBr(g) Kc = 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?

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

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

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

Consider the following reaction and its equilibrium constant: 4CuO(s) + CH4(g) ⇌ CO2(g) + 4Cu(s) + 2H2O(g) Kc = 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?

Express the equilibrium constant for the following reaction: SO2(g) + H2O(l) ⇌ H2SO3(aq)

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

Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ⇌ 2IBr(g) Kc = 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?

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. 2NOCl(g) ⇌ 2NO(g) + Cl2(g)

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 Kc for the reaction at this temperature is 1.3 × 10-6 mol L-1.

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO2(g). N2O4(g) ⇌ 2NO2(g) Kc = 0.21 M [N2O4]eq = 1.34 mol L-1

For which of the following reactions will Kc = Kp?

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.

Dinitrogen tetroxide partially decomposes according to the following equilibrium: (g) ⇌ (g) A 1.000 L flask is charged with 6.00 × 10-2 mol of . At equilibrium, 3.21 × 10-2 mol of remains. for this reaction is ________.

Match the following. -K ≈ 1

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

Kc is 1.67 × 1020 mol3 L-3 at 25 °C for the formation of iron(III) oxalate complex ion: Fe3+(aq) + 3C2O42-(aq) ⇌ [Fe(C2O4)3]3-(aq) If 0. 0200 mol L-1 Fe3+ is initially mixed with 1.00 mol L-1 oxalate ion, what is the concentration of Fe3+ ion at equilibrium?

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

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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?

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

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

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

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?

Express the equilibrium constant for the following reaction: SO₂₍_g₎ + H₂O(l) ⇌ H₂SO₃(aq)

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)

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?

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)

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^-6mol L^-1.

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 = 1.34 mol L^-1

For which of the following reactions will K_c = K_p?

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.

Dinitrogen tetroxide partially decomposes according to the following equilibrium: (g) ⇌ (g) A 1.000 L flask is charged with 6.00 × 10^-2 mol of . At equilibrium, 3.21 × 10^-2 mol of remains. for this reaction is ________.

K_c is 1.67 × 10²⁰ mol³ L^-3 at 25 °C for the formation of iron(III) oxalate complex ion: Fe³⁺(aq) + 3C₂O₄^2-(aq) ⇌ [Fe(C₂O₄)₃]^3-(aq) If 0. 0200 mol L^-1 Fe³⁺ is initially mixed with 1.00 mol L^-1 oxalate ion, what is the concentration of Fe³⁺ ion at equilibrium?

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