The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N2(g) + O2(g) 2NO(g) At 2000.°C, the equilibrium constant, Kc, has a value of 4.10 × 10-4. What is the value of KP? (R = 0.08206 L • atm/K • mol)

A) 2.17 × 10-8 B) 4.10 × 10-4 C) 7.65 × 10-2 D) 2.20 ×10-6 E) 2.44 ×103 A) 2.17 × 10-8 B) 4.10 × 10-4 C) 7.65 × 10-2 D) 2.20 ×10-6 E) 2.44 ×103

Consider the following equilibria: 2SO3(g) 2SO2(g) + O2(g) Kc = 2.3 × 10-7 2NO3(g) 2NO2(g) + O2(g) Kc = 1.4 × 10-3 Calculate the equilibrium constant for the reaction SO2(g) + NO3(g) SO3(g) + NO2(g).

A) 78 B) 1.3 × 10-2 C) 1.6 × 10-4 D) 3.2 × 10-10 E) 6.1 × 103 A) 78 B) 1.3 × 10-2 C) 1.6 × 10-4 D) 3.2 × 10-10 E) 6.1 × 103

Sodium carbonate, Na2CO3(s), may be prepared by heating sodium bicarbonate, NaHCO3(s). 2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g) KP = 0.23 at 100ºC If a sample of NaHCO3 is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be?

A) 0.46 atm B) 0.96 atm C) 0.23 atm D) 0.48 atm E) 0.11 atm A) 0.46 atm B) 0.96 atm C) 0.23 atm D) 0.48 atm E) 0.11 atm

What is KP at 298 K for the following reaction? (R = 8.314 J/K • mol) SO2(g) + NO2(g) → SO3(g) + NO(g)

A) 6.99 × 10-7 B) 5.71 × 10-8 C) 14.2 D) 475 E) 1.42 × 106 A) 6.99 × 10-7 B) 5.71 × 10-8 C) 14.2 D) 475 E) 1.42 × 106

For the reaction H2(g) + Br2(g) 2HBr(g), Kc = 81.4 at 385ºC. If [H2] = [Br2] = [HBr] = 2.4 × 10-4M at 385ºC, which one of the following is correct?

A) [H2] and [HBr] decrease as the system moves toward equilibrium. B) The system is at equilibrium. C) [H2] and [Br2] increase as the system approaches equilibrium. D) [HBr] increases as the system approaches equilibrium. E) [HBr] and [Br2] increases as the system approaches equilibrium. A) [H2] and [HBr] decrease as the system moves toward equilibrium. B) The system is at equilibrium. C) [H2] and [Br2] increase as the system approaches equilibrium. D) [HBr] increases as the system approaches equilibrium. E) [HBr] and [Br2] increases as the system approaches equilibrium.

At 500°C the equilibrium constant, KP , is 4.00 × 10-4 for the equilibrium: 2HCN(g) H2(g) + C2N2(g) What is Kp for the following reaction? H2(g) + C2 N2(g) 2HCN(g)

A) 2.00 × 10-4 B) -4.00 × 10-4 C) 1.25 × 103 D) 2.50 × 103 E) 4.00 × 104 A) 2.00 × 10-4 B) -4.00 × 10-4 C) 1.25 × 103 D) 2.50 × 103 E) 4.00 × 104

The equilibrium constant for the reaction Ni(s) + 4CO(g) Ni(CO)4(g) is 5.0 × 104 at 25ºC. What is the equilibrium constant for the following reaction? Ni(CO)4(g) Ni(s) + 4CO(g)?

A) 2.0 × 10-5 B) 2.5 × 109 C) 5.0 × 104 D) 5.0 × 10-4 E) 2.0 × 10-3 A) 2.0 × 10-5 B) 2.5 × 109 C) 5.0 × 104 D) 5.0 × 10-4 E) 2.0 × 10-3

Exam 15: Chemical Equilibrium

A quantity of liquid methanol, CH₃OH, is introduced into a rigid 3.00-L vessel, the vessel is sealed, and the temperature is raised to 500 K. At this temperature, the methanol vaporizes and decomposes according to the reaction CH₃OH(g) CO(g) + 2 H₂(g), K_c= 6.90 × 10^-2 If the concentration of H₂ in the equilibrium mixture is 0.426 M, what mass of methanol was initially introduced into the vessel?

(Multiple Choice)

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Question 101

Equilibrium constants are known for the following reactions: S(s) + (3/2)O₂(g) SO₃(g) K_c = 9.2 × 10²³ SO₃(g) SO₂(g) + (1/2)O₂(g) K_c = 4.8 × 10^-4 Thus, for the reaction S(s) + O₂(g) SO₂(g), K_c = 4.4 × 10²⁰.

(True/False)

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Question 102

The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N₂(g) + O₂(g) 2NO(g) At 2000.°C, the equilibrium constant, K_c, has a value of 4.10 × 10^-4. What is the value of K_P? (R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 103

Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH₄I(s) NH₃(g) + HI(g) At 400°C, K_P = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.

(Multiple Choice)

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Question 104

Consider this reaction at equilibrium: 2H₂O₂(g) 2H₂O(g) + O₂(g), ΔHº_rxn = -210 kJ/mol If the volume of the system is expanded at constant temperature, what change will occur in the position of the equilibrium?

(Multiple Choice)

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Question 105

Consider the following equilibria: 2SO₃(g) 2SO₂(g) + O₂(g) K_c = 2.3 × 10^-7 2NO₃(g) 2NO₂(g) + O₂(g) K_c = 1.4 × 10^-3 Calculate the equilibrium constant for the reaction SO₂(g) + NO₃(g) SO₃(g) + NO₂(g).

(Multiple Choice)

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Question 106

For the reaction PCl₃(g) + Cl₂(g) PCl₅(g) at a particular temperature, K_c = 32.4. Suppose a system at that temperature is prepared with [PCl₅] = 0.50 M, [Cl₂] = 0.4 M, and [PCl₃] = 0.10 M. Which of the following is correct?

(Multiple Choice)

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Question 107

Sodium carbonate, Na₂CO₃(s), may be prepared by heating sodium bicarbonate, NaHCO₃(s). 2NaHCO₃(s) Na₂CO₃(s) + CO₂(g) + H₂O(g) K_P = 0.23 at 100ºC If a sample of NaHCO₃ is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be?

(Multiple Choice)

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Question 108

What is K_P at 298 K for the following reaction? (R = 8.314 J/K • mol) SO₂(g) + NO₂(g) → SO₃(g) + NO(g)

(Multiple Choice)

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Question 109

Which is the correct equilibrium constant expression for the following reaction? FeO(s) + H₂(g) Fe(s) + H₂O(g)

(Multiple Choice)

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Question 110

For the reaction H₂(g) + Br₂(g) 2HBr(g), K_c = 81.4 at 385ºC. If [H₂] = [Br₂] = [HBr] = 2.4 × 10^-4^M at 385ºC, which one of the following is correct?

(Multiple Choice)

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Question 111

What is the name for Q_c?

(Multiple Choice)

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Question 112

Consider the reaction: 2A(g) + B(g) → 2C(g) If ΔG° = 50.0 kJ/mol at T = 25°C and P_A = P_B = 1 atm and P_C = 2 atm, what is the value of ΔG? (R = 8.314 J/K • mol)

(Multiple Choice)

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Question 113

The data below refer to the following reaction: 2NO(g) + I₂(g) 2NOI(g) Find the concentration of I₂ when the system reaches equilibrium.

(Short Answer)

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Question 114

A temperature increase favors an endothermic reaction.

(True/False)

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Question 115

At 500°C the equilibrium constant, K_P , is 4.00 × 10^-4 for the equilibrium: 2HCN(g) H₂(g) + C₂N₂(g) What is K_p for the following reaction? H₂(g) + C₂ N₂(g) 2HCN(g)

(Multiple Choice)

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Question 116

Consider the equilibrium: A(s) B(s) + C(g); ΔH°_rxn> 0 Predict and explain how or whether the following actions would affect this equilibrium. a. adding more solid A b. lowering the temperature c. increasing the pressure on the system by reducing its volume d. adding helium gas to increase the total pressure

(Essay)

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Question 117

What is the expression for the partial pressure of "A" for the following reaction under ideal conditions? A(g) B(g)

(Multiple Choice)

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Question 118

The equilibrium constant for the reaction Ni(s) + 4CO(g) Ni(CO)₄(g) is 5.0 × 10⁴ at 25ºC. What is the equilibrium constant for the following reaction? Ni(CO)₄(g) Ni(s) + 4CO(g)?

(Multiple Choice)

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Question 119

Which is the correct equilibrium constant expression for the following reaction? 2BrCl₃(g) Br₂(g) + 3Cl₂(g)

(Multiple Choice)

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Question 120

Showing 101 - 120 of 146

Exam 15: Chemical Equilibrium

Equilibrium constants are known for the following reactions: S(s) + (3/2)O2(g) SO3(g) Kc = 9.2 × 1023 SO3(g) SO2(g) + (1/2)O2(g) Kc = 4.8 × 10-4 Thus, for the reaction S(s) + O2(g) SO2(g), Kc = 4.4 × 1020.

The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N2(g) + O2(g) 2NO(g) At 2000.°C, the equilibrium constant, Kc, has a value of 4.10 × 10-4. What is the value of KP? (R = 0.08206 L • atm/K • mol)

Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH4I(s) NH3(g) + HI(g) At 400°C, KP = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.

Consider this reaction at equilibrium: 2H2O2(g) 2H2O(g) + O2(g), ΔHºrxn = -210 kJ/mol If the volume of the system is expanded at constant temperature, what change will occur in the position of the equilibrium?

Consider the following equilibria: 2SO3(g) 2SO2(g) + O2(g) Kc = 2.3 × 10-7 2NO3(g) 2NO2(g) + O2(g) Kc = 1.4 × 10-3 Calculate the equilibrium constant for the reaction SO2(g) + NO3(g) SO3(g) + NO2(g).

For the reaction PCl3(g) + Cl2(g) PCl5(g) at a particular temperature, Kc = 32.4. Suppose a system at that temperature is prepared with [PCl5] = 0.50 M, [Cl2] = 0.4 M, and [PCl3] = 0.10 M. Which of the following is correct?

Sodium carbonate, Na2CO3(s), may be prepared by heating sodium bicarbonate, NaHCO3(s). 2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g) KP = 0.23 at 100ºC If a sample of NaHCO3 is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be?

What is KP at 298 K for the following reaction? (R = 8.314 J/K • mol) SO2(g) + NO2(g) → SO3(g) + NO(g)

Which is the correct equilibrium constant expression for the following reaction? FeO(s) + H2(g) Fe(s) + H2O(g)

For the reaction H2(g) + Br2(g) 2HBr(g), Kc = 81.4 at 385ºC. If [H2] = [Br2] = [HBr] = 2.4 × 10-4M at 385ºC, which one of the following is correct?

What is the name for Qc?

Consider the reaction: 2A(g) + B(g) → 2C(g) If ΔG° = 50.0 kJ/mol at T = 25°C and PA = PB = 1 atm and PC = 2 atm, what is the value of ΔG? (R = 8.314 J/K • mol)

The data below refer to the following reaction: 2NO(g) + I2(g) 2NOI(g) Find the concentration of I2 when the system reaches equilibrium.

A temperature increase favors an endothermic reaction.

At 500°C the equilibrium constant, KP , is 4.00 × 10-4 for the equilibrium: 2HCN(g) H2(g) + C2N2(g) What is Kp for the following reaction? H2(g) + C2 N2(g) 2HCN(g)

What is the expression for the partial pressure of "A" for the following reaction under ideal conditions? A(g) B(g)

The equilibrium constant for the reaction Ni(s) + 4CO(g) Ni(CO)4(g) is 5.0 × 104 at 25ºC. What is the equilibrium constant for the following reaction? Ni(CO)4(g) Ni(s) + 4CO(g)?

Which is the correct equilibrium constant expression for the following reaction? 2BrCl3(g) Br2(g) + 3Cl2(g)

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Equilibrium constants are known for the following reactions: S(s) + (3/2)O₂(g) SO₃(g) K_c = 9.2 × 10²³ SO₃(g) SO₂(g) + (1/2)O₂(g) K_c = 4.8 × 10^-4 Thus, for the reaction S(s) + O₂(g) SO₂(g), K_c = 4.4 × 10²⁰.

The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N₂(g) + O₂(g) 2NO(g) At 2000.°C, the equilibrium constant, K_c, has a value of 4.10 × 10^-4. What is the value of K_P? (R = 0.08206 L • atm/K • mol)

Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH₄I(s) NH₃(g) + HI(g) At 400°C, K_P = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.

Consider this reaction at equilibrium: 2H₂O₂(g) 2H₂O(g) + O₂(g), ΔHº_rxn = -210 kJ/mol If the volume of the system is expanded at constant temperature, what change will occur in the position of the equilibrium?

Consider the following equilibria: 2SO₃(g) 2SO₂(g) + O₂(g) K_c = 2.3 × 10^-7 2NO₃(g) 2NO₂(g) + O₂(g) K_c = 1.4 × 10^-3 Calculate the equilibrium constant for the reaction SO₂(g) + NO₃(g) SO₃(g) + NO₂(g).

For the reaction PCl₃(g) + Cl₂(g) PCl₅(g) at a particular temperature, K_c = 32.4. Suppose a system at that temperature is prepared with [PCl₅] = 0.50 M, [Cl₂] = 0.4 M, and [PCl₃] = 0.10 M. Which of the following is correct?

What is K_P at 298 K for the following reaction? (R = 8.314 J/K • mol) SO₂(g) + NO₂(g) → SO₃(g) + NO(g)

Which is the correct equilibrium constant expression for the following reaction? FeO(s) + H₂(g) Fe(s) + H₂O(g)

For the reaction H₂(g) + Br₂(g) 2HBr(g), K_c = 81.4 at 385ºC. If [H₂] = [Br₂] = [HBr] = 2.4 × 10^-4^M at 385ºC, which one of the following is correct?

What is the name for Q_c?

Consider the reaction: 2A(g) + B(g) → 2C(g) If ΔG° = 50.0 kJ/mol at T = 25°C and P_A = P_B = 1 atm and P_C = 2 atm, what is the value of ΔG? (R = 8.314 J/K • mol)

The data below refer to the following reaction: 2NO(g) + I₂(g) 2NOI(g) Find the concentration of I₂ when the system reaches equilibrium.

At 500°C the equilibrium constant, K_P , is 4.00 × 10^-4 for the equilibrium: 2HCN(g) H₂(g) + C₂N₂(g) What is K_p for the following reaction? H₂(g) + C₂ N₂(g) 2HCN(g)

The equilibrium constant for the reaction Ni(s) + 4CO(g) Ni(CO)₄(g) is 5.0 × 10⁴ at 25ºC. What is the equilibrium constant for the following reaction? Ni(CO)₄(g) Ni(s) + 4CO(g)?

Which is the correct equilibrium constant expression for the following reaction? 2BrCl₃(g) Br₂(g) + 3Cl₂(g)