At elevated temperatures, molecular hydrogen and molecular bromine react to partially form hydrogen bromide: H2 (g) + Br2 (g) 2HBr (g) A mixture of 0.682 mol of H2 and 0.440 mol of Br2 is combined in a reaction vessel with a volume of 2.00 L. At equilibrium at 700 K, there are 0.546 mol of H2 present. At equilibrium, there are ________ mol of Br2 present in the reaction vessel.

A) 0.000 B) 0.440 C) 0.546 D) 0.136 E) 0.304 A) 0.000 B) 0.440 C) 0.546 D) 0.136 E) 0.304

The value of Keq for the equilibrium CO2 (g) + 2H2 (g) CH3OH (g) Is 14.5 at 483 °C. What is the value of Keq for the equilibrium below? CO2 + H2 (g) CH3OH (g)

A) 7.30 B) 7.35 C) 0.136 D) 3.81 E) 6.90 × 10-2 A) 7.30 B) 7.35 C) 0.136 D) 3.81 E) 6.90 × 10-2

The equilibrium constant for the gas phase reaction N2 (g) + O2 (g) 2NO (g) Is Keq = 4.20 × 10-31 at 30 °C. At equilibrium, ________.

A) products predominate B) reactants predominate C) roughly equal amounts of products and reactants are present D) only products are present E) only reactants are present A) products predominate B) reactants predominate C) roughly equal amounts of products and reactants are present D) only products are present E) only reactants are present

In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H2O (g) CO2 (g) + H2 (g) In an experiment, 0.35 mol of CO and 0.40 mol of H2O were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.22 mol of CO remaining. Keq at the temperature of the experiment is ________.

A) 5.5 B) 0.75 C) 3.5 D) 0.28 E) 1.0 A) 5.5 B) 0.75 C) 3.5 D) 0.28 E) 1.0

The Keq for the equilibrium below is 7.16 × 10-2 at 440.0 °C. 2Cl2 (g) + 2H2O (g) 4HCl (g) + O2 (g) What is the value of Keq at this temperature for the following reaction? Cl2 (g) + H2O (g) 2HCl (g) + O2 (g)

A) 0.0716 B) 5.13 × 10-3 C) 0.268 D) 0.0376 E) 0.150 A) 0.0716 B) 5.13 × 10-3 C) 0.268 D) 0.0376 E) 0.150

Consider the following equilibrium. 2 SO2 (g) + O2 (g) 2 SO3 (g) The equilibrium cannot be established when ________ is/are placed in a 1.0-L container.

A) 0.25 mol SO2 (g)and 0.25 mol O2 (g) B) 0.75 mol SO2 (g) C) 0.25 mol of SO2 (g)and 0.25 mol of SO3 (g) D) 0.50 mol O2 (g)and 0.50 mol SO3 (g) E) 1.0 mol SO3 (g) A) 0.25 mol SO2 (g)and 0.25 mol O2 (g) B) 0.75 mol SO2 (g) C) 0.25 mol of SO2 (g)and 0.25 mol of SO3 (g) D) 0.50 mol O2 (g)and 0.50 mol SO3 (g) E) 1.0 mol SO3 (g)

Given the following reaction: CO (g) + 2 H2(g) CH3OH (g) In an experiment, 0.42 mol of CO and 0.42 mol of H2 were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.29 mol of CO remaining. Keq at the temperature of the experiment is ________.

A) 2.80 B) 0.357 C) 14.5 D) 17.5 E) none of the above A) 2.80 B) 0.357 C) 14.5 D) 17.5 E) none of the above

Exam 15: Chemical Equilibrium

At elevated temperatures, molecular hydrogen and molecular bromine react to partially form hydrogen bromide: H₂ (g) + Br₂(g) 2HBr (g) A mixture of 0.682 mol of H₂ and 0.440 mol of Br₂ is combined in a reaction vessel with a volume of 2.00 L. At equilibrium at 700 K, there are 0.546 mol of H₂ present. At equilibrium, there are ________ mol of Br₂ present in the reaction vessel.

(Multiple Choice)

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Question 61

The value of K_eq for the equilibrium CO₂ (g) + 2H₂ (g) CH₃OH (g) Is 14.5 at 483 °C. What is the value of K_eq for the equilibrium below? CO₂ + H₂ (g) CH₃OH (g)

(Multiple Choice)

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Question 62

The equilibrium constant for the gas phase reaction N₂ (g) + O₂ (g) 2NO (g) Is K_eq = 4.20 × 10^-31 at 30 °C. At equilibrium, ________.

(Multiple Choice)

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Question 63

The reaction below is exothermic: 2SO₂ (g) + O₂ (g) 2SO₃ (g) Le Châtelier's Principle predicts that ________ will result in an increase in the number of moles of SO₃ (g)in the reaction container.

(Multiple Choice)

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Question 64

The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is ________. (1) SO₂ (g) + (1/2)O₂ (g) SO₃ (g) (2) 2SO₃ (g) 2SO₂ (g) + O₂ (g)

(Multiple Choice)

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Question 65

For the endothermic reaction CaCO₃ (s) CaO (s) + CO₂ (g) Le Châtelier's principle predicts that ________ will result in an increase in the number of moles of CO₂.

(Multiple Choice)

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Question 66

The equilibrium expression for K_p for the reaction below is ________. N₂ (g) + O₂ (g) 2NO (g)

(Multiple Choice)

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Question 67

If the reaction quotient Q for a reaction is less than the value of the equilibrium constant K for that reaction at a given temperature, must be converted to for the system to reach equilibrium.

(Short Answer)

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Question 68

In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H₂O (g) CO₂ (g) + H₂ (g) In an experiment, 0.35 mol of CO and 0.40 mol of H₂O were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.22 mol of CO remaining. K_eq at the temperature of the experiment is ________.

(Multiple Choice)

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Question 69

In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Châtelier's principle?

(Multiple Choice)

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Question 70

The expression of K_eq for the following reaction will not include ________. A(g) + B (g) C (l) + D (g)

(Multiple Choice)

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Question 71

At equilibrium, ________.

(Multiple Choice)

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Question 72

The value of K_eq for the following reaction is 0.50: A (g) + 2B (g) C (g) + 4D (g) The value of K_eq at the same temperature for the reaction below is ________. A (g) + B (g) C (g) + 2D (g)

(Multiple Choice)

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Question 73

The K_eq for the equilibrium below is 7.16 × 10^-2 at 440.0 °C. 2Cl₂ (g) + 2H₂O (g) 4HCl (g) + O₂ (g) What is the value of K_eq at this temperature for the following reaction? Cl₂ (g) + H₂O (g) 2HCl (g) + O₂ (g)

(Multiple Choice)

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Question 74

Consider the following equilibrium. 2 SO₂ (g) + O₂ (g) 2 SO₃ (g) The equilibrium cannot be established when ________ is/are placed in a 1.0-L container.

(Multiple Choice)

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Question 75

If Reaction A + Reaction B = Reaction C, then K_cReaction C = ________.

(Essay)

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Question 76

The effect of a catalyst on an equilibrium is to ________.

(Multiple Choice)

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Question 77

Given the following reaction: CO (g) + 2 H₂(g) CH₃OH (g) In an experiment, 0.42 mol of CO and 0.42 mol of H₂ were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.29 mol of CO remaining. K_eq at the temperature of the experiment is ________.

(Multiple Choice)

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Question 78

The effect of a catalyst on a chemical reaction is to react with product, effectively removing it and shifting the equilibrium to the right.

(True/False)

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Question 79

Given the following reaction at equilibrium, if K_p = 1.10 at 250.0 °C, K_c = ________. PCl₅ (g) PCl₃ (g) + Cl₂ (g)

(Multiple Choice)

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Question 80

Showing 61 - 80 of 97

Exam 15: Chemical Equilibrium

The value of Keq for the equilibrium CO2 (g) + 2H2 (g) CH3OH (g) Is 14.5 at 483 °C. What is the value of Keq for the equilibrium below? CO2 + H2 (g) CH3OH (g)

The equilibrium constant for the gas phase reaction N2 (g) + O2 (g) 2NO (g) Is Keq = 4.20 × 10-31 at 30 °C. At equilibrium, ________.

The reaction below is exothermic: 2SO2 (g) + O2 (g) 2SO3 (g) Le Châtelier's Principle predicts that ________ will result in an increase in the number of moles of SO3 (g)in the reaction container.

The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is ________. (1) SO2 (g) + (1/2)O2 (g) SO3 (g) (2) 2SO3 (g) 2SO2 (g) + O2 (g)

For the endothermic reaction CaCO3 (s) CaO (s) + CO2 (g) Le Châtelier's principle predicts that ________ will result in an increase in the number of moles of CO2.

The equilibrium expression for Kp for the reaction below is ________. N2 (g) + O2 (g) 2NO (g)

If the reaction quotient Q for a reaction is less than the value of the equilibrium constant K for that reaction at a given temperature, ________ must be converted to ________ for the system to reach equilibrium.

In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Châtelier's principle?

The expression of Keq for the following reaction will not include ________. A(g) + B (g) C (l) + D (g)

At equilibrium, ________.

The value of Keq for the following reaction is 0.50: A (g) + 2B (g) C (g) + 4D (g) The value of Keq at the same temperature for the reaction below is ________. A (g) + B (g) C (g) + 2D (g)

The Keq for the equilibrium below is 7.16 × 10-2 at 440.0 °C. 2Cl2 (g) + 2H2O (g) 4HCl (g) + O2 (g) What is the value of Keq at this temperature for the following reaction? Cl2 (g) + H2O (g) 2HCl (g) + O2 (g)

Consider the following equilibrium. 2 SO2 (g) + O2 (g) 2 SO3 (g) The equilibrium cannot be established when ________ is/are placed in a 1.0-L container.

If Reaction A + Reaction B = Reaction C, then Kc Reaction C = ________.

The effect of a catalyst on an equilibrium is to ________.

Given the following reaction: CO (g) + 2 H2(g) CH3OH (g) In an experiment, 0.42 mol of CO and 0.42 mol of H2 were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.29 mol of CO remaining. Keq at the temperature of the experiment is ________.

The effect of a catalyst on a chemical reaction is to react with product, effectively removing it and shifting the equilibrium to the right.

Given the following reaction at equilibrium, if Kp = 1.10 at 250.0 °C, Kc = ________. PCl5 (g) PCl3 (g) + Cl2 (g)

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The value of K_eq for the equilibrium CO₂ (g) + 2H₂ (g) CH₃OH (g) Is 14.5 at 483 °C. What is the value of K_eq for the equilibrium below? CO₂ + H₂ (g) CH₃OH (g)

The equilibrium constant for the gas phase reaction N₂ (g) + O₂ (g) 2NO (g) Is K_eq = 4.20 × 10^-31 at 30 °C. At equilibrium, ________.

The reaction below is exothermic: 2SO₂ (g) + O₂ (g) 2SO₃ (g) Le Châtelier's Principle predicts that ________ will result in an increase in the number of moles of SO₃ (g)in the reaction container.

The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is ________. (1) SO₂ (g) + (1/2)O₂ (g) SO₃ (g) (2) 2SO₃ (g) 2SO₂ (g) + O₂ (g)

For the endothermic reaction CaCO₃ (s) CaO (s) + CO₂ (g) Le Châtelier's principle predicts that ________ will result in an increase in the number of moles of CO₂.

The equilibrium expression for K_p for the reaction below is ________. N₂ (g) + O₂ (g) 2NO (g)

If the reaction quotient Q for a reaction is less than the value of the equilibrium constant K for that reaction at a given temperature, must be converted to for the system to reach equilibrium.

The expression of K_eq for the following reaction will not include ________. A(g) + B (g) C (l) + D (g)

The value of K_eq for the following reaction is 0.50: A (g) + 2B (g) C (g) + 4D (g) The value of K_eq at the same temperature for the reaction below is ________. A (g) + B (g) C (g) + 2D (g)

The K_eq for the equilibrium below is 7.16 × 10^-2 at 440.0 °C. 2Cl₂ (g) + 2H₂O (g) 4HCl (g) + O₂ (g) What is the value of K_eq at this temperature for the following reaction? Cl₂ (g) + H₂O (g) 2HCl (g) + O₂ (g)

Consider the following equilibrium. 2 SO₂ (g) + O₂ (g) 2 SO₃ (g) The equilibrium cannot be established when ________ is/are placed in a 1.0-L container.

If Reaction A + Reaction B = Reaction C, then K_cReaction C = ________.

Given the following reaction: CO (g) + 2 H₂(g) CH₃OH (g) In an experiment, 0.42 mol of CO and 0.42 mol of H₂ were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.29 mol of CO remaining. K_eq at the temperature of the experiment is ________.

Given the following reaction at equilibrium, if K_p = 1.10 at 250.0 °C, K_c = ________. PCl₅ (g) PCl₃ (g) + Cl₂ (g)