Hydrogen sulfide will react with water as shown in the following reactions. H2S(g) + H2O(l) H3O+(aq) + HS-(aq) K1 = 1.0 × 10-7 HS-(aq) + H2O(l) H3O+(aq) + S2-(aq) K2 = ? H2S(g) + 2H2O(l) 2H3O+(aq) + S2-(aq) K3 = 1.3 × 10-20 What is the value of K2?

A) 1.3 × 10-27 B) 2.3 × 10-7 C) 1.3 × 10-13 D) 7.7 × 1012 E) 7.7 × 1026 A) 1.3 × 10-27 B) 2.3 × 10-7 C) 1.3 × 10-13 D) 7.7 × 1012 E) 7.7 × 1026

The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br2(g) + Cl2(g) 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) Br2(g) + Cl2(g)

A) 2.97 × 10-4 B) 1.72 × 10-2 C) 3.45 × 10-2 D) 1.31 × 10-1 E) > 1.00 A) 2.97 × 10-4 B) 1.72 × 10-2 C) 3.45 × 10-2 D) 1.31 × 10-1 E) > 1.00

Nitrogen dioxide decomposes according to the reaction 2NO2(g) 2NO(g) + O2(g) Where Kp = 4.48 × 10-13 at 25°C. What is the value for Kc?

A) 1.81 × 10-16 B) 1.83 × 10-14 C) 4.48 × 10-13 D) 1.10 × 10-11 E) 1.11 × 10-9 A) 1.81 × 10-16 B) 1.83 × 10-14 C) 4.48 × 10-13 D) 1.10 × 10-11 E) 1.11 × 10-9

Hydrogen sulfide can be formed in the following reaction: H2(g) + S2(g) H2S(g) F1F1F1S1F1F1F10H°rxn = -92 kJ The equilibrium constant Kp = 106 at 1023 K. Estimate the value of Kp at 1218 K.

A) 5.05 B) 18.8 C) 34.7 D) 88.9 E) 598 A) 5.05 B) 18.8 C) 34.7 D) 88.9 E) 598

The following reaction is at equilibrium at one atmosphere, in a closed container. NaOH(s) + CO2(g) NaHCO3(s) Which, if any, of the following actions will decrease the total amount of CO2 gas present at equilibrium?

A) adding N2 gas to double the pressure B) adding more solid NaOH C) decreasing the volume of the container D) removing half of the solid NaHCO3 E) none of the above A) adding N2 gas to double the pressure B) adding more solid NaOH C) decreasing the volume of the container D) removing half of the solid NaHCO3 E) none of the above

Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO2(g) 2NO(g) + O2(g) F1F1F1S1F1F1F10H°rxn = +114 kJ Under which reaction conditions would you expect to produce the largest amount of oxygen?

A) high temperature, high pressure B) low temperature, high pressure C) high temperature, low pressure D) low temperature, low pressure E) none of the above, unless a catalyst is present A) high temperature, high pressure B) low temperature, high pressure C) high temperature, low pressure D) low temperature, low pressure E) none of the above, unless a catalyst is present

Exam 17: Equilibrium: the Extent of Chemical Reactions

Magnesium hydroxide is used in several antacid formulations. When it is added to water it dissociates into magnesium and hydroxide ions. Mg(OH)₂(s) Mg²⁺(aq) + 2OH^-(aq) The equilibrium constant at 25°C is 8.9 × 10^-12. One hundred grams of magnesium hydroxide is added to 1.00 L of water and equilibrium is established. What happens to the solution if another 10 grams of Mg(OH)₂are now added to the mixture?

(Multiple Choice)

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Question 81

The equilibrium constant, K_p, for the reaction CO(g) + H₂O(g) CO₂(g) + H₂(g) At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?

(Multiple Choice)

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Question 82

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 83

Hydrogen sulfide will react with water as shown in the following reactions. H₂S(g) + H₂O(l) H₃O⁺(aq) + HS^-(aq) K₁= 1.0 × 10^-7 HS^-(aq) + H₂O(l) H₃O⁺(aq) + S^2-(aq) K₂= ? H₂S(g) + 2H₂O(l) 2H₃O⁺(aq) + S^2-(aq) K₃= 1.3 × 10^-20 What is the value of K₂?

(Multiple Choice)

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Question 84

The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br₂(g) + Cl₂(g) 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) Br₂(g) + Cl₂(g)

(Multiple Choice)

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Question 85

For a gas-phase equilibrium, a change in the pressure of any single reactant or product will change K_p.

(True/False)

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Question 86

Changing the amount of a solid reactant or product in an equilibrium reaction will not affect the amounts of the other reactants and products present at equilibrium.

(True/False)

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Question 87

The reaction quotient, Q_c, for a reaction has a value of 75 while the equilibrium constant, K_c, has a value of 195. Which of the following statements is accurate?

(Multiple Choice)

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Question 88

Nitrogen dioxide decomposes according to the reaction 2NO₂(g) 2NO(g) + O₂(g) Where K_p = 4.48 × 10^-13 at 25°C. What is the value for K_c?

(Multiple Choice)

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Question 89

Consider the equilibrium reaction shown below. B₂(g) 2B(g) If the rate constants are: k_fwd = 7.00 × 10^-5 s^-1 and k_rev = 2.00 × 10^-5 L mol^-1 s^-1, what is the value of K_c under these conditions?

(Multiple Choice)

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Question 90

Hydrogen sulfide can be formed in the following reaction: H₂(g) + S₂(g) H₂S(g) H°_rxn = -92 kJ The equilibrium constant K_p = 106 at 1023 K. Estimate the value of K_p at 1218 K.

(Multiple Choice)

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Question 91

Consider the equilibrium reaction: N₂O₄(g) 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_p for the reaction?

(Multiple Choice)

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Question 92

The following reaction is at equilibrium at one atmosphere, in a closed container. NaOH(s) + CO₂(g) NaHCO₃(s) Which, if any, of the following actions will decrease the total amount of CO₂ gas present at equilibrium?

(Multiple Choice)

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Question 93

At a certain temperature the reaction CO₂(g) + H₂(g) CO(g) + H₂O(g) Has K_c = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?

(Multiple Choice)

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Question 94

A mixture 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium concentration of COBr₂was 0.233 M. What is the value of K_c for this reaction? CO(g) + Br₂(g) COBr₂(g)

(Multiple Choice)

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Question 95

Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO₂(g) 2NO(g) + O₂(g) H°_rxn = +114 kJ Under which reaction conditions would you expect to produce the largest amount of oxygen?

(Multiple Choice)

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Question 96

Write the mass-action expression, Q_c, for the following chemical reaction. NO(g) + Br₂(g) NOBr(g)

(Multiple Choice)

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Question 97

Consider the following gas-phase equilibrium reaction: N₂(g) + O₂(g) 2NO(g) K_c = 4.10 × 10^-4 at 2000°C If 1.0 mol of NO is introduced into a 1.0 L container at 2000°C, what is the concentration of NO when equilibrium is reached?

(Essay)

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Question 98

A chemical reaction has an equilibrium constant of 2 × 10⁶. If this reaction is at equilibrium, select the one correct conclusion that can be made about the reaction.

(Multiple Choice)

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Question 99

The equilibrium constant K_c for the reaction A(g) + B(g) C(g) Is 0.76 at 150°C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150°C, what will be the equilibrium concentration of C?

(Multiple Choice)

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Question 100

Showing 81 - 100 of 104

Exam 17: Equilibrium: the Extent of Chemical Reactions

The equilibrium constant, Kp , for the reaction CO(g) + H2O(g) CO2(g) + H2(g) At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?

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?

Hydrogen sulfide will react with water as shown in the following reactions. H2S(g) + H2O(l) H3O+(aq) + HS-(aq) K1 = 1.0 × 10-7 HS-(aq) + H2O(l) H3O+(aq) + S2-(aq) K2 = ? H2S(g) + 2H2O(l) 2H3O+(aq) + S2-(aq) K3 = 1.3 × 10-20 What is the value of K2?

The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br2(g) + Cl2(g) 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) Br2(g) + Cl2(g)

For a gas-phase equilibrium, a change in the pressure of any single reactant or product will change Kp.

Changing the amount of a solid reactant or product in an equilibrium reaction will not affect the amounts of the other reactants and products present at equilibrium.

The reaction quotient, Qc, for a reaction has a value of 75 while the equilibrium constant, Kc, has a value of 195. Which of the following statements is accurate?

Nitrogen dioxide decomposes according to the reaction 2NO2(g) 2NO(g) + O2(g) Where Kp = 4.48 × 10-13 at 25°C. What is the value for Kc?

Consider the equilibrium reaction shown below. B2(g) 2B(g) If the rate constants are: kfwd = 7.00 × 10-5 s-1 and krev = 2.00 × 10-5 L mol-1 s-1, what is the value of Kc under these conditions?

Hydrogen sulfide can be formed in the following reaction: H2(g) + S2(g) H2S(g) H°rxn = -92 kJ The equilibrium constant Kp = 106 at 1023 K. Estimate the value of Kp at 1218 K.

Consider the equilibrium reaction: N2O4(g) 2NO2(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?

The following reaction is at equilibrium at one atmosphere, in a closed container. NaOH(s) + CO2(g) NaHCO3(s) Which, if any, of the following actions will decrease the total amount of CO2 gas present at equilibrium?

At a certain temperature the reaction CO2(g) + H2(g) CO(g) + H2O(g) Has Kc = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?

A mixture 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium concentration of COBr2 was 0.233 M. What is the value of Kc for this reaction? CO(g) + Br2(g) COBr2(g)

Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO2(g) 2NO(g) + O2(g) H°rxn = +114 kJ Under which reaction conditions would you expect to produce the largest amount of oxygen?

Write the mass-action expression, Qc, for the following chemical reaction. NO(g) + Br2(g) NOBr(g)

Consider the following gas-phase equilibrium reaction: N2(g) + O2(g) 2NO(g) Kc = 4.10 × 10-4 at 2000°C If 1.0 mol of NO is introduced into a 1.0 L container at 2000°C, what is the concentration of NO when equilibrium is reached?

A chemical reaction has an equilibrium constant of 2 × 106. If this reaction is at equilibrium, select the one correct conclusion that can be made about the reaction.

The equilibrium constant Kc for the reaction A(g) + B(g) C(g) Is 0.76 at 150°C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150°C, what will be the equilibrium concentration of C?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

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The equilibrium constant, K_p, for the reaction CO(g) + H₂O(g) CO₂(g) + H₂(g) At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?

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?

Hydrogen sulfide will react with water as shown in the following reactions. H₂S(g) + H₂O(l) H₃O⁺(aq) + HS^-(aq) K₁= 1.0 × 10^-7 HS^-(aq) + H₂O(l) H₃O⁺(aq) + S^2-(aq) K₂= ? H₂S(g) + 2H₂O(l) 2H₃O⁺(aq) + S^2-(aq) K₃= 1.3 × 10^-20 What is the value of K₂?

The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br₂(g) + Cl₂(g) 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) Br₂(g) + Cl₂(g)

For a gas-phase equilibrium, a change in the pressure of any single reactant or product will change K_p.

The reaction quotient, Q_c, for a reaction has a value of 75 while the equilibrium constant, K_c, has a value of 195. Which of the following statements is accurate?

Nitrogen dioxide decomposes according to the reaction 2NO₂(g) 2NO(g) + O₂(g) Where K_p = 4.48 × 10^-13 at 25°C. What is the value for K_c?

Consider the equilibrium reaction shown below. B₂(g) 2B(g) If the rate constants are: k_fwd = 7.00 × 10^-5 s^-1 and k_rev = 2.00 × 10^-5 L mol^-1 s^-1, what is the value of K_c under these conditions?

Hydrogen sulfide can be formed in the following reaction: H₂(g) + S₂(g) H₂S(g) H°_rxn = -92 kJ The equilibrium constant K_p = 106 at 1023 K. Estimate the value of K_p at 1218 K.

Consider the equilibrium reaction: N₂O₄(g) 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_p for the reaction?

The following reaction is at equilibrium at one atmosphere, in a closed container. NaOH(s) + CO₂(g) NaHCO₃(s) Which, if any, of the following actions will decrease the total amount of CO₂ gas present at equilibrium?

At a certain temperature the reaction CO₂(g) + H₂(g) CO(g) + H₂O(g) Has K_c = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?

A mixture 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium concentration of COBr₂was 0.233 M. What is the value of K_c for this reaction? CO(g) + Br₂(g) COBr₂(g)

Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO₂(g) 2NO(g) + O₂(g) H°_rxn = +114 kJ Under which reaction conditions would you expect to produce the largest amount of oxygen?

Write the mass-action expression, Q_c, for the following chemical reaction. NO(g) + Br₂(g) NOBr(g)

Consider the following gas-phase equilibrium reaction: N₂(g) + O₂(g) 2NO(g) K_c = 4.10 × 10^-4 at 2000°C If 1.0 mol of NO is introduced into a 1.0 L container at 2000°C, what is the concentration of NO when equilibrium is reached?

A chemical reaction has an equilibrium constant of 2 × 10⁶. If this reaction is at equilibrium, select the one correct conclusion that can be made about the reaction.

The equilibrium constant K_c for the reaction A(g) + B(g) C(g) Is 0.76 at 150°C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150°C, what will be the equilibrium concentration of C?