Hydrogen peroxide may decompose to form water and oxygen gas according to the following reaction. 2H2O2(g) 2H2O(g) + O2(g) In a particular experiment, 1.75 moles of H2O2 were placed in a 2.5-L reaction chamber at 307ºC. After equilibrium was reached, 1.20 moles of H2O2 remained. What is Kc for the reaction?

A) 2.0 × 10-4 B) 2.3 × 10-2 C) 2.4 × 10-3 D) 5.5 × 10-3 E) 3.9 × 10-4 A) 2.0 × 10-4 B) 2.3 × 10-2 C) 2.4 × 10-3 D) 5.5 × 10-3 E) 3.9 × 10-4

The equilibrium constant KP at 427°C for the reaction N2(g) + 3H2(g) 2NH3(g) is 9.4 × 10-5. What is ΔG° for the reaction under these conditions? (R = 8.314 J/K • mol)

A) -33 kJ/mol B) -54 kJ/mol C) 54 kJ/mol D) 33 kJ/mol E) 1.3 J/mol A) -33 kJ/mol B) -54 kJ/mol C) 54 kJ/mol D) 33 kJ/mol E) 1.3 J/mol

Consider the following reactions and their associated equilibrium constants: A + 2B C K1 C D + E K2 For the reaction A + 2B D + E, having equilibrium constant Kc

A) Kc = K1 + K2. B) Kc = K1/K2. C) Kc = K1 - K2. D) Kc = (K1)(K2). E) Kc = K2/K1. A) Kc = K1 + K2. B) Kc = K1/K2. C) Kc = K1 - K2. D) Kc = (K1)(K2). E) Kc = K2/K1.

Calculate KP for the reaction 2NOCl(g) 2NO(g) + Cl2(g) at 400.°C if Kc at 400.°C for this reaction is 2.1 × 10-2. (R = 0.08206 L • atm/K • mol)

A) 6.4 × 10-3 B) 1.7 × 10-3 C) 0.69 D) 1.2 E) 3.8 × 10-4 A) 6.4 × 10-3 B) 1.7 × 10-3 C) 0.69 D) 1.2 E) 3.8 × 10-4

The following reaction is at equilibrium in a sealed container. N2(g) + 3H2(g) 2NH3(g); ΔH°rxn c?

A) Adding more NH3 B) Adding more N2 C) Increasing the pressure D) Lowering the temperature E) Adding a catalyst A) Adding more NH3 B) Adding more N2 C) Increasing the pressure D) Lowering the temperature E) Adding a catalyst

Exam 15: Chemical Equilibrium

Hydrogen peroxide may decompose to form water and oxygen gas according to the following reaction. 2H₂O₂(g) 2H₂O(g) + O₂(g) In a particular experiment, 1.75 moles of H₂O₂ were placed in a 2.5-L reaction chamber at 307ºC. After equilibrium was reached, 1.20 moles of H₂O₂ remained. What is K_c for the reaction?

(Multiple Choice)

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Question 121

A change in a concentration will not change the position of equilibrium.

(True/False)

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Question 122

The equilibrium constant K_P at 427°C for the reaction N₂(g) + 3H₂(g) 2NH₃(g) is 9.4 × 10^-5. What is ΔG° for the reaction under these conditions? (R = 8.314 J/K • mol)

(Multiple Choice)

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Question 123

For the common allotropes of carbon (graphite and diamond), C(gr) C(dia) with equilibrium constant K = 0.32. The molar volumes of graphite and diamond are, respectively, 5.30 cm³/mol and 3.42 cm³/mol; ΔH_f of diamond is 1.90 kJ/mol. These data suggest that the formation of diamond is favored at

(Multiple Choice)

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Question 124

Consider the following reactions and their associated equilibrium constants: A + 2B C K₁ C D + E K₂ For the reaction A + 2B D + E, having equilibrium constant K_c

(Multiple Choice)

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Question 125

What is defined as a fraction with product concentrations in the numerator and reactant concentrations in the denominator and with each concentration raised to a power equal to the corresponding stoichiometric coefficient in the balanced chemical equation?

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Question 126

Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached, the following partial pressures of three gases were measured: NO: 0.526 atm; Br₂ : 1.59 atm; NOBr: 7.68 atm. Calculate K_P for the reaction. 2NO(g) + Br₂(g) 2NOBr(g)

(Multiple Choice)

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Question 127

For the endothermic reaction A₂ (g) 2A(g), a snapshot of an equilibrium mixture of A(g) and A₂ (g) at low temperature may look as follows. (Each circle represents 1.0 mol of A atoms, and the volume of the box is 1.0 L.) If the temperature is raised, what might the new equilibrium system look like?

(Multiple Choice)

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Question 128

Calculate K_P for the reaction 2NOCl(g) 2NO(g) + Cl₂(g) at 400.°C if K_c at 400.°C for this reaction is 2.1 × 10^-2. (R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 129

The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ/mol at 25°C. What is K_P for the reaction H₂(g) + I₂(g) 2HI(g) at this temperature?

(Multiple Choice)

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Question 130

Calculate the equilibrium constant at 25°C for the reaction of methane with water to form carbon dioxide and hydrogen. The data below are values at 25°C.(R = 8.314 J/K • mol) CH₄(g) + 2H₂O(g) CO₂(g) + 4H₂(g)

(Multiple Choice)

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Question 131

Compounds A, B, and C react according to the following equation. 3A(g) + 2B(g) 2C(g) At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of K_c for this reaction?

(Multiple Choice)

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Question 132

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 133

Which of the following statements is incorrect regarding equilibrium?

(Multiple Choice)

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Question 134

For the reaction of A + B C + D + heat, the reverse reaction is exothermic.

(True/False)

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Question 135

For the following reaction at equilibrium, which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g) 2NO(g) + Br₂(g), ΔHº_rxn= 30 kJ/mol

(Multiple Choice)

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Question 136

Suppose 25.0 g of HI(g) is injected into a 4.00-L reaction vessel that contains 20.0 g of I₂(g). When the system comes to equilibrium at 400.ºC, what will be the total pressure inside the reaction vessel? (R = 0.08206 L • atm/K • mol) 2HI(g) H₂(g) + I₂(g), K_c = 0.0156 at 400.ºC

(Multiple Choice)

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Question 137

Which represents the correct relationship between the Gibbs free energy and the equilibrium constant?

(Multiple Choice)

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Question 138

The following reaction is at equilibrium in a sealed container. N₂(g) + 3H₂(g) 2NH₃(g); ΔH°_rxn< 0 Which, if any, of the following actions will increase the value of the equilibrium constant, K_c?

(Multiple Choice)

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Question 139

A(n) ________ means that the products of the reaction can react to form reactants.

(Short Answer)

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Question 140

Showing 121 - 140 of 146

Exam 15: Chemical Equilibrium

A change in a concentration will not change the position of equilibrium.

The equilibrium constant KP at 427°C for the reaction N2(g) + 3H2(g) 2NH3(g) is 9.4 × 10-5. What is ΔG° for the reaction under these conditions? (R = 8.314 J/K • mol)

For the common allotropes of carbon (graphite and diamond), C(gr) C(dia) with equilibrium constant K = 0.32. The molar volumes of graphite and diamond are, respectively, 5.30 cm3/mol and 3.42 cm3/mol; ΔHf of diamond is 1.90 kJ/mol. These data suggest that the formation of diamond is favored at

Consider the following reactions and their associated equilibrium constants: A + 2B C K1 C D + E K2 For the reaction A + 2B D + E, having equilibrium constant Kc

What is defined as a fraction with product concentrations in the numerator and reactant concentrations in the denominator and with each concentration raised to a power equal to the corresponding stoichiometric coefficient in the balanced chemical equation?

Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached, the following partial pressures of three gases were measured: NO: 0.526 atm; Br2 : 1.59 atm; NOBr: 7.68 atm. Calculate KP for the reaction. 2NO(g) + Br2(g) 2NOBr(g)

For the endothermic reaction A2 (g) 2A(g), a snapshot of an equilibrium mixture of A(g) and A2 (g) at low temperature may look as follows. (Each circle represents 1.0 mol of A atoms, and the volume of the box is 1.0 L.) If the temperature is raised, what might the new equilibrium system look like?

Calculate KP for the reaction 2NOCl(g) 2NO(g) + Cl2(g) at 400.°C if Kc at 400.°C for this reaction is 2.1 × 10-2. (R = 0.08206 L • atm/K • mol)

The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ/mol at 25°C. What is KP for the reaction H2(g) + I2(g) 2HI(g) at this temperature?

Calculate the equilibrium constant at 25°C for the reaction of methane with water to form carbon dioxide and hydrogen. The data below are values at 25°C.(R = 8.314 J/K • mol) CH4(g) + 2H2O(g) CO2(g) + 4H2(g)

Compounds A, B, and C react according to the following equation. 3A(g) + 2B(g) 2C(g) At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of Kc for this reaction?

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

Which of the following statements is incorrect regarding equilibrium?

For the reaction of A + B C + D + heat, the reverse reaction is exothermic.

For the following reaction at equilibrium, which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g) 2NO(g) + Br2(g), ΔHºrxn = 30 kJ/mol

Suppose 25.0 g of HI(g) is injected into a 4.00-L reaction vessel that contains 20.0 g of I2(g). When the system comes to equilibrium at 400.ºC, what will be the total pressure inside the reaction vessel? (R = 0.08206 L • atm/K • mol) 2HI(g) H2(g) + I2(g), Kc = 0.0156 at 400.ºC

Which represents the correct relationship between the Gibbs free energy and the equilibrium constant?

The following reaction is at equilibrium in a sealed container. N2(g) + 3H2(g) 2NH3(g); ΔH°rxn < 0 Which, if any, of the following actions will increase the value of the equilibrium constant, Kc?

A(n) ________ means that the products of the reaction can react to form reactants.

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The equilibrium constant K_P at 427°C for the reaction N₂(g) + 3H₂(g) 2NH₃(g) is 9.4 × 10^-5. What is ΔG° for the reaction under these conditions? (R = 8.314 J/K • mol)

For the common allotropes of carbon (graphite and diamond), C(gr) C(dia) with equilibrium constant K = 0.32. The molar volumes of graphite and diamond are, respectively, 5.30 cm³/mol and 3.42 cm³/mol; ΔH_f of diamond is 1.90 kJ/mol. These data suggest that the formation of diamond is favored at

Consider the following reactions and their associated equilibrium constants: A + 2B C K₁ C D + E K₂ For the reaction A + 2B D + E, having equilibrium constant K_c

Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached, the following partial pressures of three gases were measured: NO: 0.526 atm; Br₂ : 1.59 atm; NOBr: 7.68 atm. Calculate K_P for the reaction. 2NO(g) + Br₂(g) 2NOBr(g)

Calculate K_P for the reaction 2NOCl(g) 2NO(g) + Cl₂(g) at 400.°C if K_c at 400.°C for this reaction is 2.1 × 10^-2. (R = 0.08206 L • atm/K • mol)

The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ/mol at 25°C. What is K_P for the reaction H₂(g) + I₂(g) 2HI(g) at this temperature?

Calculate the equilibrium constant at 25°C for the reaction of methane with water to form carbon dioxide and hydrogen. The data below are values at 25°C.(R = 8.314 J/K • mol) CH₄(g) + 2H₂O(g) CO₂(g) + 4H₂(g)

Compounds A, B, and C react according to the following equation. 3A(g) + 2B(g) 2C(g) At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of K_c for this reaction?

For the following reaction at equilibrium, which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g) 2NO(g) + Br₂(g), ΔHº_rxn= 30 kJ/mol

Suppose 25.0 g of HI(g) is injected into a 4.00-L reaction vessel that contains 20.0 g of I₂(g). When the system comes to equilibrium at 400.ºC, what will be the total pressure inside the reaction vessel? (R = 0.08206 L • atm/K • mol) 2HI(g) H₂(g) + I₂(g), K_c = 0.0156 at 400.ºC

The following reaction is at equilibrium in a sealed container. N₂(g) + 3H₂(g) 2NH₃(g); ΔH°_rxn< 0 Which, if any, of the following actions will increase the value of the equilibrium constant, K_c?