Consider the reversible reaction: 2NO2(g) N2O4(g) If the concentrations of both NO2 and N2O4 are 0.016 mol L-1, what is the value of Qc?

A) 0.016 B) 0.50 C) 1.0 D) 2.0 E) 63 A) 0.016 B) 0.50 C) 1.0 D) 2.0 E) 63

Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + O2(g) NO2(g) (2) 2NO2(g) 2NO(g) + O2(g) Which one of the following is the correct relationship between the equilibrium constants K1 and K2?

A) K2 = 2/K1 B) K2 = (1/K1)2 C) K2 = -K1/2 D) K2 = 1/(2K1) E) K2 = 1/(2K1)2 A) K2 = 2/K1 B) K2 = (1/K1)2 C) K2 = -K1/2 D) K2 = 1/(2K1) E) K2 = 1/(2K1)2

Hydrogen bromide will dissociate into hydrogen and bromine gases. 2HBr(g) H2(g) + Br2(g) F1F1F1S1F1F1F10H°rxn = 68 kJ What effect will a temperature increase of 50°C have on this system at equilibrium?

A) The partial pressure of hydrogen bromide will increase. B) The partial pressure of hydrogen will increase. C) The partial pressure of hydrogen bromide and bromine will increase. D) There will be no effect on the partial pressure of any of the gases. E) Need to know the initial pressure, volume, and temperature before any of the above predictions can be made. A) The partial pressure of hydrogen bromide will increase. B) The partial pressure of hydrogen will increase. C) The partial pressure of hydrogen bromide and bromine will increase. D) There will be no effect on the partial pressure of any of the gases. E) Need to know the initial pressure, volume, and temperature before any of the above predictions can be made.

The following reaction is at equilibrium in a closed container. CuSO4.5H2O(s) CuSO4(s) + 5H2O(g) Which, if any, of the following actions will lead to an increase in the pressure of H2O present at equilibrium?

A) increasing the volume of the container B) decreasing the volume of the container C) adding a catalyst D) removing some solid CuSO4 E) none of the above A) increasing the volume of the container B) decreasing the volume of the container C) adding a catalyst D) removing some solid CuSO4 E) none of the above

Exam 17: Equilibrium: the Extent of Chemical Reactions

In water, the following equilibrium exists: H⁺(aq) + OH^-(aq) H₂O(l) In pure water at 25 °C, the concentration of H⁺ ions is 1.00 × 10^-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

Free

(Multiple Choice)

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Question 1

Correct Answer:

Verified

Although a system may be at equilibrium, the rate constants of the forward and reverse reactions will in general be different.

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(True/False)

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Question 2

Correct Answer:

Verified

True

A chemical reaction will reach equilibrium when the limiting reactant is used up.

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(True/False)

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Question 3

Correct Answer:

Verified

False

At a high temperature, the following reaction has an equilibrium constant of 1.0 × 10². H₂(g) + F₂(g) 2HF(g) If 1.00 mol of each of H₂ and F₂ are allowed to come to equilibrium in a 10.0 L vessel, calculate the equilibrium amounts of H₂ and HF.

(Short Answer)

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Question 4

Consider the reversible reaction: 2NO₂(g) N₂O₄(g) If the concentrations of both NO₂and N₂O₄ are 0.016 mol L^-1, what is the value of Q_c?

(Multiple Choice)

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Question 5

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 6

Unless H°_rxn = 0, a change in temperature will affect the value of the equilibrium constant K_c.

(True/False)

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Question 7

Consider the equilibrium H₂(g) + Br₂(g) 2HBr(g) To a 20.0 L flask are added 0.100 moles of H₂ and 0.200 moles of HBr. The equilibrium constant for this reaction is 989. Calculate the number of moles of Br₂ in the flask when equilibrium is established. Make any reasonable approximation, clearly stating what that approximation is.

(Essay)

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Question 8

About half of the sodium carbonate produced is used in making glass products because it lowers the melting point of sand, the major component of glass. When sodium carbonate is added to water it hydrolyses according to the following reactions. CO₃^2-(aq) + H₂O(l) HCO₃^-(aq) + OH^-(aq) K₁ HCO₃^-(aq) + H₂O(l) H₂CO₃(aq) + OH^-(aq) K₂ These can be combined to yield CO₃^2-(aq) + 2H₂O(l) H₂CO₃(aq) + 2OH^-(aq) K₃ What is the value of K₃?

(Multiple Choice)

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Question 9

At 850°C, the equilibrium constant K_p for the reaction C(s) + CO₂(g) 2CO(g) Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?

(Multiple Choice)

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Question 10

When a reaction system reaches equilibrium, the forward and reverse reactions stop.

(True/False)

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Question 11

Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + O₂(g) NO₂(g) (2) 2NO₂(g) 2NO(g) + O₂(g) Which one of the following is the correct relationship between the equilibrium constants K₁ and K₂?

(Multiple Choice)

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Question 12

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?

(Multiple Choice)

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Question 13

Hydrogen bromide will dissociate into hydrogen and bromine gases. 2HBr(g) H₂(g) + Br₂(g) H°_rxn = 68 kJ What effect will a temperature increase of 50°C have on this system at equilibrium?

(Multiple Choice)

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Question 14

Write the mass-action expression, Q_c, for the following chemical reaction. Fe³⁺(aq) + 3OH^-(aq) Fe(OH)₃(s)

(Multiple Choice)

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Question 15

For some gas-phase reactions, K_p = K_c.

(True/False)

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Question 16

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 17

The following reaction is at equilibrium in a closed container. CuSO₄.5H₂O(s) CuSO₄(s) + 5H₂O(g) Which, if any, of the following actions will lead to an increase in the pressure of H₂O present at equilibrium?

(Multiple Choice)

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Question 18

If all the reactants and products in an equilibrium reaction are in the gas phase, then K_p = K_c.

(True/False)

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Question 19

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 20

Showing 1 - 20 of 104

Exam 17: Equilibrium: the Extent of Chemical Reactions

In water, the following equilibrium exists: H+(aq) + OH-(aq) H2O(l) In pure water at 25 °C, the concentration of H+ ions is 1.00 × 10-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

Although a system may be at equilibrium, the rate constants of the forward and reverse reactions will in general be different.

A chemical reaction will reach equilibrium when the limiting reactant is used up.

At a high temperature, the following reaction has an equilibrium constant of 1.0 × 102. H2(g) + F2(g) 2HF(g) If 1.00 mol of each of H2 and F2 are allowed to come to equilibrium in a 10.0 L vessel, calculate the equilibrium amounts of H2 and HF.

Consider the reversible reaction: 2NO2(g) N2O4(g) If the concentrations of both NO2 and N2O4 are 0.016 mol L-1, what is the value of Qc?

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

Unless H°rxn = 0, a change in temperature will affect the value of the equilibrium constant Kc.

At 850°C, the equilibrium constant Kp for the reaction C(s) + CO2(g) 2CO(g) Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?

When a reaction system reaches equilibrium, the forward and reverse reactions stop.

Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + O2(g) NO2(g) (2) 2NO2(g) 2NO(g) + O2(g) Which one of the following is the correct relationship between the equilibrium constants K1 and K2?

Hydrogen bromide will dissociate into hydrogen and bromine gases. 2HBr(g) H2(g) + Br2(g) H°rxn = 68 kJ What effect will a temperature increase of 50°C have on this system at equilibrium?

Write the mass-action expression, Qc , for the following chemical reaction. Fe3+(aq) + 3OH-(aq) Fe(OH)3(s)

For some gas-phase reactions, Kp = Kc.

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

The following reaction is at equilibrium in a closed container. CuSO4.5H2O(s) CuSO4(s) + 5H2O(g) Which, if any, of the following actions will lead to an increase in the pressure of H2O present at equilibrium?

If all the reactants and products in an equilibrium reaction are in the gas phase, then Kp = Kc.

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

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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In water, the following equilibrium exists: H⁺(aq) + OH^-(aq) H₂O(l) In pure water at 25 °C, the concentration of H⁺ ions is 1.00 × 10^-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

At a high temperature, the following reaction has an equilibrium constant of 1.0 × 10². H₂(g) + F₂(g) 2HF(g) If 1.00 mol of each of H₂ and F₂ are allowed to come to equilibrium in a 10.0 L vessel, calculate the equilibrium amounts of H₂ and HF.

Consider the reversible reaction: 2NO₂(g) N₂O₄(g) If the concentrations of both NO₂and N₂O₄ are 0.016 mol L^-1, what is the value of Q_c?

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

Unless H°_rxn = 0, a change in temperature will affect the value of the equilibrium constant K_c.

At 850°C, the equilibrium constant K_p for the reaction C(s) + CO₂(g) 2CO(g) Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?

Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + O₂(g) NO₂(g) (2) 2NO₂(g) 2NO(g) + O₂(g) Which one of the following is the correct relationship between the equilibrium constants K₁ and K₂?

Hydrogen bromide will dissociate into hydrogen and bromine gases. 2HBr(g) H₂(g) + Br₂(g) H°_rxn = 68 kJ What effect will a temperature increase of 50°C have on this system at equilibrium?

Write the mass-action expression, Q_c, for the following chemical reaction. Fe³⁺(aq) + 3OH^-(aq) Fe(OH)₃(s)

For some gas-phase reactions, K_p = K_c.

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

The following reaction is at equilibrium in a closed container. CuSO₄.5H₂O(s) CuSO₄(s) + 5H₂O(g) Which, if any, of the following actions will lead to an increase in the pressure of H₂O present at equilibrium?

If all the reactants and products in an equilibrium reaction are in the gas phase, then K_p = K_c.

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