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

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

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

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. Kc for this reaction is ________.

A) 0.723 mol L-1 B) 0.391 mol L-1 C) 0.212 mol L-1 D) 6.94 × 10-3 mol L-1 E) 1.92 × 10-4 mol L-1 A) 0.723 mol L-1 B) 0.391 mol L-1 C) 0.212 mol L-1 D) 6.94 × 10-3 mol L-1 E) 1.92 × 10-4 mol L-1

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. 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.

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

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

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.

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

Calculate the value of [N2]eq if [H2]eq = 2.0 mol L-1, [NH3]eq = 0.50 mol L-1, and Kc = 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 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

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)

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

Exam 14: Chemical Equilibrium

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 Br₂and 3.5 mol L^-1 IBr. Which of the following statements is TRUE concerning this system?

(Multiple Choice)

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Question 81

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

(Multiple Choice)

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Question 82

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. K_c for this reaction is ________.

(Multiple Choice)

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Question 83

For which reaction will K_p = K_c?

(Multiple Choice)

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Question 84

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 = ?

(Multiple Choice)

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Question 85

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

(Multiple Choice)

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Question 86

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

(Multiple Choice)

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Question 87

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)

(Multiple Choice)

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Question 88

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

(Multiple Choice)

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Question 89

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

(Multiple Choice)

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Question 90

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.

(Multiple Choice)

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Question 91

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

(Multiple Choice)

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Question 92

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)

(Multiple Choice)

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Question 93

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)

(Multiple Choice)

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Question 94

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 = ?

(Multiple Choice)

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Question 95

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

(Essay)

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Question 96

Which of the following statements is TRUE?

(Multiple Choice)

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Question 97

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

(Multiple Choice)

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Question 98

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 = ?

(Multiple Choice)

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Question 99

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)

(Multiple Choice)

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Question 100

Showing 81 - 100 of 123

Exam 14: Chemical Equilibrium

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

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

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. Kc for this reaction is ________.

For which reaction will Kp = Kc?

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 = ?

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

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

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

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

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

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

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

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)

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 = ?

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

Which of the following statements is TRUE?

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

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 = ?

For the following reaction, what is Δn required in the conversion of Kc to Kp? CH4(g)+ H2O(g)⇌ CO(g)+ 3H2(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 0.41 mol L^-1 I₂, 0.27 mol L^-1 Br₂and 3.5 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)

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. K_c for this reaction is ________.

For which reaction will K_p = K_c?

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 = ?

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

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

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)

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

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

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

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)

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)

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 = ?

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

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 = ?

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)