10.0 mL of a 0.100 mol L−1 solution of a metal ion M2+ is mixed with 10.0 mL of a 0.100 mol L−1 solution of a substance L. The following equilibrium is established: M2+(aq) + 2L(aq) ⇄ ML22+(aq) At equilibrium the concentration of L is found to be 0.0100 mol L−1. What is the equilibrium concentration of ML22+, in mol L−1?

A) 0.100 mol L −1 B) 0.050 mol L −1 C) 0.025 mol L −1 D) 0.0200 mol L −1 E) 0.0100 mol L −1 A) 0.100 mol L −1 B) 0.050 mol L −1 C) 0.025 mol L −1 D) 0.0200 mol L −1 E) 0.0100 mol L −1

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

A) Adding a catalyst B) Adding more N 2 C) Increasing the pressure D) Lowering the temperature E) None of these choices are correct. A) Adding a catalyst B) Adding more N 2 C) Increasing the pressure D) Lowering the temperature E) None of these choices are correct.

Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C17H35COOH ⇄ (C17H35COOH)2 ΔH°rxn = −172 kJ The equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium constant at 38°C.

A) 4.7 × 10 5 B) 2.6 × 10 4 C) 1.9 × 10 3 D) 3.2 × 10 2 E) 18 A) 4.7 × 10 5 B) 2.6 × 10 4 C) 1.9 × 10 3 D) 3.2 × 10 2 E) 18

The reaction of nitric oxide to form dinitrogen oxide and nitrogen dioxide is exothermic. 3NO(g) ⇄ N2O(g) + NO2(g) + heat What effect will be seen if the temperature of the system at equilibrium is raised by 25°C?

A) The partial pressure of NO will increase. B) The partial pressure of NO will decrease. C) The partial pressure of NO 2 will increase. D) The partial pressures of NO and N 2O will increase. E) All three partial pressures will increase. A) The partial pressure of NO will increase. B) The partial pressure of NO will decrease. C) The partial pressure of NO 2 will increase. D) The partial pressures of NO and N 2O will increase. E) All three partial pressures will increase.

What is the mass-action expression, Qc, for the following chemical reaction? 4H3O+(aq) + 2Cl−(aq) + MnO2(s) ⇄ Mn2+(aq) + 6H2O(l) + Cl2(g)

A) B) C) D) E) None of these choices are correct. A) B) C) D) E) None of these choices are correct.

Exam 17: Equilibrium: the Extent of Chemical Reactions

At 25°C, the equilibrium constant K_c for the reaction 2A(aq) ⇄ B(aq) + C(aq) Is 65. If 2.50 mol of A is added to enough water to prepare 1.00 L of solution, what will the equilibrium concentration of A be?

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(Multiple Choice)

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Question 1

Correct Answer:

Verified

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?

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(Multiple Choice)

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Question 2

Correct Answer:

Verified

A mixture of 0.600 mol of bromine and 1.600 mol of iodine is placed into a rigid 1.000-L container at 350°C. Br₂(g) + I₂(g) ⇄ 2IBr(g) When the mixture has come to equilibrium, the concentration of iodine monobromide is 1.190 M. What is the equilibrium constant for this reaction at 350°C?

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(Multiple Choice)

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Question 3

Correct Answer:

Verified

For a gas-phase equilibrium, a change in the pressure of any single reactant or product will affect the amounts of other substances involved in the equilibrium.

(True/False)

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Question 4

10.0 mL of a 0.100 mol L⁻¹ solution of a metal ion M²⁺ is mixed with 10.0 mL of a 0.100 mol L⁻¹ solution of a substance L. The following equilibrium is established: M²⁺(aq) + 2L(aq) ⇄ ML₂²⁺(aq) At equilibrium the concentration of L is found to be 0.0100 mol L⁻¹. What is the equilibrium concentration of ML₂²⁺, in mol L⁻¹?

(Multiple Choice)

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Question 5

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 6

Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C₁₇H₃₅COOH ⇄ (C₁₇H₃₅COOH)₂ΔH°_rxn = −172 kJ The equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium constant at 38°C.

(Multiple Choice)

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Question 7

The equilibrium constant, K_p, has a value of 6.5 × 10⁻⁴ at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl₂(g) ⇄ 2NOCl(g) What is the value of K_c?

(Multiple Choice)

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Question 8

Increasing the initial amount of the limiting reactant in a reaction will increase the value of the equilibrium constant, K_c.

(True/False)

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Question 9

Hydrogen iodide, HI, is formed in an equilibrium reaction when gaseous hydrogen and iodine gas are heated together. If 20.0 g of hydrogen and 20.0 g of iodine are heated, forming 10.0 g of hydrogen iodide, what mass of hydrogen remains unreacted?

(Multiple Choice)

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Question 10

If all of the coefficients in the balanced equation for an equilibrium reaction are doubled, then the value of the equilibrium constant, K_c, will also be doubled.

(True/False)

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Question 11

Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g) + 2H₂(g) ⇄ CH₃OH(g) A reaction vessel contains the three gases at equilibrium with a total pressure of 1.00 atm. What will happen to the partial pressure of hydrogen if enough argon is added to raise the total pressure to 1.4 atm?

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Question 12

Write the mass-action expression, Q_c, for the following chemical reaction. 3ClO₂⁻(aq) ⇄ 2ClO₃⁻(aq) + Cl⁻(aq)

(Multiple Choice)

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Question 13

The two equilibrium constants for the same reaction, K_c and K_p, will always equal one another when

(Multiple Choice)

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Question 14

The reaction of nitric oxide to form dinitrogen oxide and nitrogen dioxide is exothermic. 3NO(g) ⇄ N₂O(g) + NO₂(g) + heat What effect will be seen if the temperature of the system at equilibrium is raised by 25°C?

(Multiple Choice)

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Question 15

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 16

Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N₂(g) + O₂(g) ⇄ 2NO(g) The equilibrium constant K_p for the reaction is 0.0025 at 2127°C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?

(Multiple Choice)

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Question 17

The reaction system CS₂(g) + 4H₂(g) ⇄ CH₄(g) + 2H₂S(g) Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled?

(Multiple Choice)

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Question 18

Write the mass-action expression, Q_c, for the following chemical reaction. Zn(s) + 2Ag⁺(aq) ⇄ Zn²⁺(aq) + 2Ag(s)

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Question 19

What is the mass-action expression, Q_c, for the following chemical reaction? 4H₃O⁺(aq) + 2Cl⁻(aq) + MnO₂(s) ⇄ Mn²⁺(aq) + 6H₂O(l) + Cl₂(g)

(Multiple Choice)

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Question 20

Showing 1 - 20 of 98

Exam 17: Equilibrium: the Extent of Chemical Reactions

At 25°C, the equilibrium constant Kc for the reaction 2A(aq) ⇄ B(aq) + C(aq) Is 65. If 2.50 mol of A is added to enough water to prepare 1.00 L of solution, what will the equilibrium concentration of A be?

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

A mixture of 0.600 mol of bromine and 1.600 mol of iodine is placed into a rigid 1.000-L container at 350°C. Br2(g) + I2(g) ⇄ 2IBr(g) When the mixture has come to equilibrium, the concentration of iodine monobromide is 1.190 M. What is the equilibrium constant for this reaction at 350°C?

For a gas-phase equilibrium, a change in the pressure of any single reactant or product will affect the amounts of other substances involved in the equilibrium.

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?

Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C17H35COOH ⇄ (C17H35COOH)2 ΔH°rxn = −172 kJ The equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium constant at 38°C.

The equilibrium constant, Kp, has a value of 6.5 × 10−4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl2(g) ⇄ 2NOCl(g) What is the value of Kc?

Increasing the initial amount of the limiting reactant in a reaction will increase the value of the equilibrium constant, Kc.

Hydrogen iodide, HI, is formed in an equilibrium reaction when gaseous hydrogen and iodine gas are heated together. If 20.0 g of hydrogen and 20.0 g of iodine are heated, forming 10.0 g of hydrogen iodide, what mass of hydrogen remains unreacted?

If all of the coefficients in the balanced equation for an equilibrium reaction are doubled, then the value of the equilibrium constant, Kc, will also be doubled.

Write the mass-action expression, Qc, for the following chemical reaction. 3ClO2−(aq) ⇄ 2ClO3−(aq) + Cl−(aq)

The two equilibrium constants for the same reaction, Kc and Kp, will always equal one another when

The reaction of nitric oxide to form dinitrogen oxide and nitrogen dioxide is exothermic. 3NO(g) ⇄ N2O(g) + NO2(g) + heat What effect will be seen if the temperature of the system at equilibrium is raised by 25°C?

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

The reaction system CS2(g) + 4H2(g) ⇄ CH4(g) + 2H2S(g) Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled?

Write the mass-action expression, Qc, for the following chemical reaction. Zn(s) + 2Ag+(aq) ⇄ Zn2+(aq) + 2Ag(s)

What is the mass-action expression, Qc, for the following chemical reaction? 4H3O+(aq) + 2Cl−(aq) + MnO2(s) ⇄ Mn2+(aq) + 6H2O(l) + Cl2(g)

Keys to the Study of Chemistry: Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Three 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

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 Reaction Direction

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

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At 25°C, the equilibrium constant K_c for the reaction 2A(aq) ⇄ B(aq) + C(aq) Is 65. If 2.50 mol of A is added to enough water to prepare 1.00 L of solution, what will the equilibrium concentration of A be?

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?

A mixture of 0.600 mol of bromine and 1.600 mol of iodine is placed into a rigid 1.000-L container at 350°C. Br₂(g) + I₂(g) ⇄ 2IBr(g) When the mixture has come to equilibrium, the concentration of iodine monobromide is 1.190 M. What is the equilibrium constant for this reaction at 350°C?

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?

Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C₁₇H₃₅COOH ⇄ (C₁₇H₃₅COOH)₂ΔH°_rxn = −172 kJ The equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium constant at 38°C.

The equilibrium constant, K_p, has a value of 6.5 × 10⁻⁴ at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl₂(g) ⇄ 2NOCl(g) What is the value of K_c?

Increasing the initial amount of the limiting reactant in a reaction will increase the value of the equilibrium constant, K_c.

If all of the coefficients in the balanced equation for an equilibrium reaction are doubled, then the value of the equilibrium constant, K_c, will also be doubled.

Write the mass-action expression, Q_c, for the following chemical reaction. 3ClO₂⁻(aq) ⇄ 2ClO₃⁻(aq) + Cl⁻(aq)

The two equilibrium constants for the same reaction, K_c and K_p, will always equal one another when

The reaction of nitric oxide to form dinitrogen oxide and nitrogen dioxide is exothermic. 3NO(g) ⇄ N₂O(g) + NO₂(g) + heat What effect will be seen if the temperature of the system at equilibrium is raised by 25°C?

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

The reaction system CS₂(g) + 4H₂(g) ⇄ CH₄(g) + 2H₂S(g) Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled?

Write the mass-action expression, Q_c, for the following chemical reaction. Zn(s) + 2Ag⁺(aq) ⇄ Zn²⁺(aq) + 2Ag(s)

What is the mass-action expression, Q_c, for the following chemical reaction? 4H₃O⁺(aq) + 2Cl⁻(aq) + MnO₂(s) ⇄ Mn²⁺(aq) + 6H₂O(l) + Cl₂(g)