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?

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

Consider the following reaction and its equilibrium constant: I2(g)⇌ 2I(g)Kp = 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. 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.

At 900.0 K, the equilibrium constant (Kp)for the following reaction is 0.345 bar-1: 2SO2 + O2(g)→ 2SO3(g) At equilibrium, the partial pressure of SO2 is 35.0 bar and that of O2 is 15.9 bar. The partial pressure of SO3 is ________ bar.

A) 82.0 B) 4.21 × 10-3 C) 192 D) 6.20 × 10-4 E) 40.2 A) 82.0 B) 4.21 × 10-3 C) 192 D) 6.20 × 10-4 E) 40.2

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.

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

For the reaction: N2(g)+ 2O2(g)⇌ 2NO2(g), Kc = 8.3 × 10-10 M-1 at 25 °C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is five times the concentration of O2 gas?

A) 3.3 × 10-11 mol L-1 B) 1.7 × 10-10 mol L-1 C) 6.0 × 109 mol L-1 D) 3.0 × 1010 mol L-1 A) 3.3 × 10-11 mol L-1 B) 1.7 × 10-10 mol L-1 C) 6.0 × 109 mol L-1 D) 3.0 × 1010 mol L-1

At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2ICl(g)⇌ I2(g)+ Cl2(g) What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0 L flask?

A) 0.14 mol L-1 B) 0.17 mol L-1 C) 0.27 mol L-1 D) 0.34 mol L-1 A) 0.14 mol L-1 B) 0.17 mol L-1 C) 0.27 mol L-1 D) 0.34 mol L-1

Exam 14: Chemical Equilibrium

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?

(Multiple Choice)

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Question 41

Consider the following reaction at equilibrium. What effect will reducing the pressure of the reaction mixture have on the system? Xe(g)+ 2F₂(g)⇌ XeF₄(g)

(Multiple Choice)

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Question 42

Phosphorus trichloride and phosphorus pentachloride equilibrate in the presence of molecular chlorine according to the following reaction: (g)+ (g)→ (g) An equilibrium mixture at 450 K contains = 0.124 bar, = 0.157 bar, and = 1.30 bar. What is the value of K_p at this temperature?

(Multiple Choice)

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Question 43

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?

(Multiple Choice)

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Question 44

Define Le Châtelier's principle.

(Essay)

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Question 45

At 900.0 K, the equilibrium constant (K_p)for the following reaction is 0.345 bar^-1: 2SO₂ + O₂(g)→ 2SO₃(g) At equilibrium, the partial pressure of SO₂ is 35.0 bar and that of O₂ is 15.9 bar. The partial pressure of SO₃ is ________ bar.

(Multiple Choice)

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Question 46

Match the following. -K << 1

(Multiple Choice)

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Question 47

For the isomerization reaction: butane ⇌ isobutane K_p equals 25.0 at 500 °C. If the initial pressures of butane and isobutane are 20.0 atm and 0.0 atm, respectively, what are the pressures of the two gases at equilibrium?

(Multiple Choice)

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Question 48

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

(Multiple Choice)

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Question 49

The decomposition of ammonia is 2NH₃(g)→ N₂(g)+ 3H₂(g). If K_p is 1.5 × 10³ bar² at 400 °C, what is the partial pressure of ammonia at equilibrium when the partial pressure of N₂(g)is 0.10 bar and that of H₂(g)is 0.15 bar?

(Multiple Choice)

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Question 50

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

(Multiple Choice)

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Question 51

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

(Multiple Choice)

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Question 52

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

(Multiple Choice)

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Question 53

Why is a thermodynamic equilibrium constant unitless?

(Essay)

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Question 54

Cyclohexane, C₆H₁₂, undergoes a molecular rearrangement in the presence of AlCl₃ to form methylcyclopentane, CH₃C₅H_9, according to the equation: C₆H₁₂ ⇌ CH₃C₅H₉ If K_c = 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.

(Multiple Choice)

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Question 55

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

(Multiple Choice)

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Question 56

For the reaction: N₂(g)+ 2O₂(g)⇌ 2NO₂(g), K_c = 8.3 × 10^-10 M^-1at 25 °C. What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is five times the concentration of O₂ gas?

(Multiple Choice)

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Question 57

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

(Multiple Choice)

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Question 58

At a certain temperature the equilibrium constant, K_c, equals 0.11 for the reaction: 2ICl(g)⇌ I₂(g)+ Cl₂(g) What is the equilibrium concentration of ICl if 0.45 mol of I₂ and 0.45 mol of Cl₂ are initially mixed in a 2.0 L flask?

(Multiple Choice)

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Question 59

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? Xe(g)+ 2F₂(g)⇌ XeF₄(g)

(Multiple Choice)

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Question 60

Showing 41 - 60 of 123

Exam 14: Chemical Equilibrium

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?

Consider the following reaction at equilibrium. What effect will reducing the pressure of the reaction mixture have on the system? Xe(g)+ 2F2(g)⇌ XeF4(g)

Phosphorus trichloride and phosphorus pentachloride equilibrate in the presence of molecular chlorine according to the following reaction: (g)+ (g)→ (g) An equilibrium mixture at 450 K contains = 0.124 bar, = 0.157 bar, and = 1.30 bar. What is the value of Kp at this temperature?

Consider the following reaction and its equilibrium constant: I2(g)⇌ 2I(g)Kp = 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?

Define Le Châtelier's principle.

At 900.0 K, the equilibrium constant (Kp)for the following reaction is 0.345 bar-1: 2SO2 + O2(g)→ 2SO3(g) At equilibrium, the partial pressure of SO2 is 35.0 bar and that of O2 is 15.9 bar. The partial pressure of SO3 is ________ bar.

Match the following. -K << 1

For the isomerization reaction: butane ⇌ isobutane Kp equals 25.0 at 500 °C. If the initial pressures of butane and isobutane are 20.0 atm and 0.0 atm, respectively, what are the pressures of the two gases at equilibrium?

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

The decomposition of ammonia is 2NH3(g)→ N2(g)+ 3H2(g). If Kp is 1.5 × 103 bar2 at 400 °C, what is the partial pressure of ammonia at equilibrium when the partial pressure of N2(g)is 0.10 bar and that of H2(g)is 0.15 bar?

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

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

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

Why is a thermodynamic equilibrium constant unitless?

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

For the reaction: N2(g)+ 2O2(g)⇌ 2NO2(g), Kc = 8.3 × 10-10 M-1 at 25 °C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is five times the concentration of O2 gas?

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

At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2ICl(g)⇌ I2(g)+ Cl2(g) What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0 L flask?

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? Xe(g)+ 2F2(g)⇌ XeF4(g)

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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?

Consider the following reaction at equilibrium. What effect will reducing the pressure of the reaction mixture have on the system? Xe(g)+ 2F₂(g)⇌ XeF₄(g)

Phosphorus trichloride and phosphorus pentachloride equilibrate in the presence of molecular chlorine according to the following reaction: (g)+ (g)→ (g) An equilibrium mixture at 450 K contains = 0.124 bar, = 0.157 bar, and = 1.30 bar. What is the value of K_p at this temperature?

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?

At 900.0 K, the equilibrium constant (K_p)for the following reaction is 0.345 bar^-1: 2SO₂ + O₂(g)→ 2SO₃(g) At equilibrium, the partial pressure of SO₂ is 35.0 bar and that of O₂ is 15.9 bar. The partial pressure of SO₃ is ________ bar.

For the isomerization reaction: butane ⇌ isobutane K_p equals 25.0 at 500 °C. If the initial pressures of butane and isobutane are 20.0 atm and 0.0 atm, respectively, what are the pressures of the two gases at equilibrium?

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

The decomposition of ammonia is 2NH₃(g)→ N₂(g)+ 3H₂(g). If K_p is 1.5 × 10³ bar² at 400 °C, what is the partial pressure of ammonia at equilibrium when the partial pressure of N₂(g)is 0.10 bar and that of H₂(g)is 0.15 bar?

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

For the reaction: N₂(g)+ 2O₂(g)⇌ 2NO₂(g), K_c = 8.3 × 10^-10 M^-1at 25 °C. What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is five times the concentration of O₂ gas?

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

At a certain temperature the equilibrium constant, K_c, equals 0.11 for the reaction: 2ICl(g)⇌ I₂(g)+ Cl₂(g) What is the equilibrium concentration of ICl if 0.45 mol of I₂ and 0.45 mol of Cl₂ are initially mixed in a 2.0 L flask?

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? Xe(g)+ 2F₂(g)⇌ XeF₄(g)