At 400ºC, Kc = 64 for the equilibrium H2(g)+ I2(g) 2HI(g).If 3.00 mol H2 and 3.00 mol I2 are introduced into an empty 4.0 L vessel, find the equilibrium concentration of HI at 400ºC.

A) 0.15 M B) 1.2 M C) 2.4 M D) 4.8 M E) 5.8 M A) 0.15 M B) 1.2 M C) 2.4 M D) 4.8 M E) 5.8 M

The equilibrium constant expression for the reaction 2BrF5 (g) Br2 (g)+ 5F2 (g)is

A) Kc = [Br2] [F2] / [BrF5] B) Kc = [Br2] [F2]5 / [BrF5]2 C) Kc = [Br2] [F2]2 / [BrF5]5 D) Kc = [BrF5]2 / [Br2][F2]5 E) Kc = 2[BrF5]2 / ([Br2] × 5[F2]5) A) Kc = [Br2] [F2] / [BrF5] B) Kc = [Br2] [F2]5 / [BrF5]2 C) Kc = [Br2] [F2]2 / [BrF5]5 D) Kc = [BrF5]2 / [Br2][F2]5 E) Kc = 2[BrF5]2 / ([Br2] × 5[F2]5)

Concerning the following reaction at equilibrium: 3Fe(s)+ 4H2O(g) Fe3O4(s)+ 4H2(g), increasing the concentration of the Fe(s)would:

A) Shift the equilibrium to the right B) Shift the equilibrium to the left C) Increase the value of the equilibrium constant, K D) Decrease the value of the equilibrium constant, K E) No change A) Shift the equilibrium to the right B) Shift the equilibrium to the left C) Increase the value of the equilibrium constant, K D) Decrease the value of the equilibrium constant, K E) No change

The solubility of silver bromide can be increased by dissolving it in a solution containing the thiosulfate anion. AgBr(s) Ag+ (aq)+ Br- (aq)K1 = 7.7 x 10-13 Ag+(aq)+ 2S2O32- (aq) Ag(S2O3)23- (aq)K2 = 4.7 x 1013 What is the value of the equilibrium constant for the overall reaction? AgBr(s)+ 2S2O32-(aq) Ag(S2O3)23-(aq)+ Br-(aq)

A) 3.6 x 10-9 B) 12.4 x 1013 C) 4.7 x 10-9 D) 4.7 x 1013 E) 36 A) 3.6 x 10-9 B) 12.4 x 1013 C) 4.7 x 10-9 D) 4.7 x 1013 E) 36

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to increase? 2NOBr(g) 2NO(g)+ Br2(g), $\Delta$Hºrxn= 30 kJ/mol

A) Lower the temperature. B) Remove some NO. C) Remove some NOBr. D) Compress the gas mixture into a smaller volume. E) Add a catalyst A) Lower the temperature. B) Remove some NO. C) Remove some NOBr. D) Compress the gas mixture into a smaller volume. E) Add a catalyst

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

For the reaction at equilibrium: 3Fe(s)+ 4H2O(g) Fe3O4(s)+ 4H2(g), removing some of the product, Fe3O4(s), would:

A) Shift the equilibrium to the right B) Shift the equilibrium to the left C) Increase the value of the equilibrium constant, K D) Decrease the value of the equilibrium constant, K E) No change A) Shift the equilibrium to the right B) Shift the equilibrium to the left C) Increase the value of the equilibrium constant, K D) Decrease the value of the equilibrium constant, K E) No change

The equilibrium constants for the chemical reaction N2(g)+ O2(g) 2NO(g)are KP = 1.1 × 10-3 and 3.6 × 10-3 at 2,200 K and 2,500 K, respectively. Which one of these statements is true?

A) The reaction is exothermic, $\Delta$Hº P is less than Kc by a factor of (RT). D) The total pressure at 2,200 K is the same as at 2,500 K. E) Higher total pressure shifts the equilibrium to the left. A) The reaction is exothermic, $\Delta$Hº P is less than Kc by a factor of (RT). D) The total pressure at 2,200 K is the same as at 2,500 K. E) Higher total pressure shifts the equilibrium to the left.

The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO2 (aq)+ H2O (l) H2CO3 (aq) Which one of the following is the correct equilibrium constant expression (Kc)for this reaction?

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

Exam 14: Chemical Equilibrium

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant after ammonia was added to the system.

(Short Answer)

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Question 61

At 400ºC, K_c = 64 for the equilibrium H₂(g)+ I₂(g) 2HI(g).If 3.00 mol H₂ and 3.00 mol I₂ are introduced into an empty 4.0 L vessel, find the equilibrium concentration of HI at 400ºC.

(Multiple Choice)

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Question 62

The equilibrium constant expression for the reaction 2BrF₅(g) Br₂(g)+ 5F₂(g)is

(Multiple Choice)

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Question 63

Calculate K_c for the reaction 2HI(g) H₂(g)+ I₂(g)given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I₂] = 0.60 mol/L, [H₂] = 0.27 mol/L.

(Multiple Choice)

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Question 64

Concerning the following reaction at equilibrium: 3Fe(s)+ 4H₂O(g) Fe₃O₄(s)+ 4H₂(g), increasing the concentration of the Fe(s)would:

(Multiple Choice)

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Question 65

A reaction with an equilibrium constant K_c = 1.5 x 10^-25 would consist of which of the following at equilibrium:

(Multiple Choice)

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Question 66

The solubility of silver bromide can be increased by dissolving it in a solution containing the thiosulfate anion. AgBr(s) Ag⁺(aq)+ Br^-(aq)K₁ = 7.7 x 10^-13 Ag⁺(aq)+ 2S₂O₃^2-(aq) Ag(S₂O₃)₂^3-(aq)K₂ = 4.7 x 10¹³ What is the value of the equilibrium constant for the overall reaction? AgBr(s)+ 2S₂O₃^2-(aq) Ag(S₂O₃)₂^3-(aq)+ Br^-(aq)

(Multiple Choice)

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Question 67

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br₂ concentration to increase? 2NOBr(g) $For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to increase? 2NOBr(g) 2NO(g)+ Br2(g), \Delta Hºrxn= 30 kJ/mol$ 2NO(g)+ Br₂(g), $\Delta$ Hº_rxn= 30 kJ/mol

(Multiple Choice)

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Question 68

In which of these gas-phase equilibria is the yield of products increased by increasing the total pressure on the reaction mixture?

(Multiple Choice)

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Question 69

Consider the reaction N₂(g)+ 3H₂(g) 2NH₃(g).If we use a catalyst, which way will the reaction shift?

(Essay)

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Question 70

What is the correct equilibrium constant expression for this reaction? 2HI(g) H₂(g)+ I₂(g)

(Essay)

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Question 71

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 72

When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the products by CuO(s)+ H₂(g) $When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the products by CuO(s)+ H2(g) H2O(g)+ Cu(s) \Delta Hºrxn = -2.0 kJ/mol$ H₂O(g)+ Cu(s) $\Delta$ Hº_rxn = -2.0 kJ/mol

(Multiple Choice)

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Question 73

Equilibrium constants are known for the following reactions: S(s)+ ³/₂O₂(g) SO₃(g)K_c = 9.2 × 10²³ SO₃(g) SO₂(g)+ ¹/₂O₂(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 74

For the reaction at equilibrium: 3Fe(s)+ 4H₂O(g) Fe₃O₄(s)+ 4H₂(g), removing some of the product, Fe₃O₄(s), would:

(Multiple Choice)

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Question 75

The equilibrium constants for the chemical reaction N₂(g)+ O₂(g) 2NO(g)are K_P = 1.1 × 10^-3 and 3.6 × 10^-3 at 2,200 K and 2,500 K, respectively. Which one of these statements is true?

(Multiple Choice)

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Question 76

The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO₂(aq)+ H₂O (l) H₂CO₃(aq) Which one of the following is the correct equilibrium constant expression (K_c)for this reaction?

(Multiple Choice)

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Question 77

Given the following data for the reaction: A(g)+ 2B(s) AB₂(g) Is the reaction endothermic or exothermic?

(Short Answer)

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Question 78

The K_c for the reaction CO₂(g)+ H₂(g) H₂O(g)+ CO(g)is 1.6 at about 990ºC.Calculate the number of moles of carbon dioxide in the final equilibrium system obtained by initially adding 1.00 mol of H₂, 2.00 mol of CO₂, 0.750 mol of H₂O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

(Short Answer)

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Question 79

For the reaction H₂(g)+ I₂(g) 2HI(g), K_P = K_c.

(True/False)

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Question 80

Showing 61 - 80 of 109

Exam 14: Chemical Equilibrium

Consider the following equilibrium, 4NH3(g)+ 3O2(g) 2N2(g)+ 6H2O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant after ammonia was added to the system.

At 400ºC, Kc = 64 for the equilibrium H2(g)+ I2(g) 2HI(g).If 3.00 mol H2 and 3.00 mol I2 are introduced into an empty 4.0 L vessel, find the equilibrium concentration of HI at 400ºC.

The equilibrium constant expression for the reaction 2BrF5 (g) Br2 (g)+ 5F2 (g)is

Calculate Kc for the reaction 2HI(g) H2(g)+ I2(g)given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, [H2] = 0.27 mol/L.

Concerning the following reaction at equilibrium: 3Fe(s)+ 4H2O(g) Fe3O4(s)+ 4H2(g), increasing the concentration of the Fe(s)would:

A reaction with an equilibrium constant Kc = 1.5 x 10-25 would consist of which of the following at equilibrium:

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to increase? 2NOBr(g) 2NO(g)+ Br2(g), Δ\DeltaΔ Hºrxn= 30 kJ/mol

In which of these gas-phase equilibria is the yield of products increased by increasing the total pressure on the reaction mixture?

Consider the reaction N2(g)+ 3H2(g) 2NH3(g).If we use a catalyst, which way will the reaction shift?

What is the correct equilibrium constant expression for this reaction? 2HI(g) H2(g)+ I2(g)

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)

When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the products by CuO(s)+ H2(g) H2O(g)+ Cu(s) Δ\DeltaΔ Hºrxn = -2.0 kJ/mol

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

For the reaction at equilibrium: 3Fe(s)+ 4H2O(g) Fe3O4(s)+ 4H2(g), removing some of the product, Fe3O4(s), would:

The equilibrium constants for the chemical reaction N2(g)+ O2(g) 2NO(g)are KP = 1.1 × 10-3 and 3.6 × 10-3 at 2,200 K and 2,500 K, respectively. Which one of these statements is true?

The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO2 (aq)+ H2O (l) H2CO3 (aq) Which one of the following is the correct equilibrium constant expression (Kc)for this reaction?

Given the following data for the reaction: A(g)+ 2B(s) AB2(g) Is the reaction endothermic or exothermic?

The Kc for the reaction CO2(g)+ H2(g) H2O(g)+ CO(g)is 1.6 at about 990ºC.Calculate the number of moles of carbon dioxide in the final equilibrium system obtained by initially adding 1.00 mol of H2, 2.00 mol of CO2, 0.750 mol of H2O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

For the reaction H2(g)+ I2(g) 2HI(g), KP = Kc.

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Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant after ammonia was added to the system.

At 400ºC, K_c = 64 for the equilibrium H₂(g)+ I₂(g) 2HI(g).If 3.00 mol H₂ and 3.00 mol I₂ are introduced into an empty 4.0 L vessel, find the equilibrium concentration of HI at 400ºC.

The equilibrium constant expression for the reaction 2BrF₅(g) Br₂(g)+ 5F₂(g)is

Calculate K_c for the reaction 2HI(g) H₂(g)+ I₂(g)given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I₂] = 0.60 mol/L, [H₂] = 0.27 mol/L.

Concerning the following reaction at equilibrium: 3Fe(s)+ 4H₂O(g) Fe₃O₄(s)+ 4H₂(g), increasing the concentration of the Fe(s)would:

A reaction with an equilibrium constant K_c = 1.5 x 10^-25 would consist of which of the following at equilibrium:

Consider the reaction N₂(g)+ 3H₂(g) 2NH₃(g).If we use a catalyst, which way will the reaction shift?

What is the correct equilibrium constant expression for this reaction? 2HI(g) H₂(g)+ I₂(g)

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)

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

For the reaction at equilibrium: 3Fe(s)+ 4H₂O(g) Fe₃O₄(s)+ 4H₂(g), removing some of the product, Fe₃O₄(s), would:

The equilibrium constants for the chemical reaction N₂(g)+ O₂(g) 2NO(g)are K_P = 1.1 × 10^-3 and 3.6 × 10^-3 at 2,200 K and 2,500 K, respectively. Which one of these statements is true?

The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO₂(aq)+ H₂O (l) H₂CO₃(aq) Which one of the following is the correct equilibrium constant expression (K_c)for this reaction?

Given the following data for the reaction: A(g)+ 2B(s) AB₂(g) Is the reaction endothermic or exothermic?

The K_c for the reaction CO₂(g)+ H₂(g) H₂O(g)+ CO(g)is 1.6 at about 990ºC.Calculate the number of moles of carbon dioxide in the final equilibrium system obtained by initially adding 1.00 mol of H₂, 2.00 mol of CO₂, 0.750 mol of H₂O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

For the reaction H₂(g)+ I₂(g) 2HI(g), K_P = K_c.