Question 1

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.

Accepted Answer

A) True 
 B)False

Question 2

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

Accepted Answer

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

Question 3

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.

Accepted Answer

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

Question 4

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

Accepted Answer

A)   c, 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." class="answers-bank-image d-inline" rel="preload" >
B)   c, 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." class="answers-bank-image d-inline" rel="preload" >
C)   c, 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." class="answers-bank-image d-inline" rel="preload" >
D)   c, 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." class="answers-bank-image d-inline" rel="preload" >
E)  None of these choices are correct.F) All of the above
G) A) and B)

Question 5

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?

Accepted Answer

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 −1F) C) and E)
G) A) and B)

Question 6

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?

Accepted Answer

A)  As equilibrium is reestablished, the partial pressure of carbon disulfide increases.
B)  As equilibrium is reestablished, the partial pressure of methane, CH 4, decreases.
C)  As equilibrium is reestablished, the partial pressure of hydrogen decreases.
D)  As equilibrium is reestablished, the partial pressure of hydrogen sulfide decreases.
E)  As equilibrium is reestablished, all the partial pressures will decrease.F) A) and C)
G) All of the above

Question 7

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

Accepted Answer

A) True 
 B)False

Question 8

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?

Accepted Answer

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.F) D) and E)
G) A) and B)

Question 9

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

Accepted Answer

A)   c, for the following chemical reaction. 3ClO2−(aq)  ⇄ 2ClO3−(aq)  + Cl−(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   c, for the following chemical reaction. 3ClO2−(aq)  ⇄ 2ClO3−(aq)  + Cl−(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   c, for the following chemical reaction. 3ClO2−(aq)  ⇄ 2ClO3−(aq)  + Cl−(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   c, for the following chemical reaction. 3ClO2−(aq)  ⇄ 2ClO3−(aq)  + Cl−(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   c, for the following chemical reaction. 3ClO2−(aq)  ⇄ 2ClO3−(aq)  + Cl−(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) C) and E)
G) A) and B)

Question 10

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

Accepted Answer

A)   c, for the following chemical reaction. Zn(s)  + 2Ag+(aq)  ⇄ Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   c, for the following chemical reaction. Zn(s)  + 2Ag+(aq)  ⇄ Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   c, for the following chemical reaction. Zn(s)  + 2Ag+(aq)  ⇄ Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   c, for the following chemical reaction. Zn(s)  + 2Ag+(aq)  ⇄ Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   c, for the following chemical reaction. Zn(s)  + 2Ag+(aq)  ⇄ Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) B) and E)
G) A) and B)

Question 11

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?

Accepted Answer

A)  0.038 M
B)  0.14 M
C)  0.28 M
D)  1.18 M
E)  2.4 MF) C) and D)
G) All of the above B

Question 12

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.

Accepted Answer

A) True 
 B)False

Question 13

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?

Accepted Answer

A)  3.55 × 10 −3
B)  1.24
C)  1.47
D)  282
E)  325F) B) and E)
G) A) and C) D

Question 14

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?

Accepted Answer

A)  2.5 × 10 −7
B)  6.5 × 10 −4
C)  1.6 × 10 −2
D)  1.7
E)  None of these choices are correct.F) A) and B)
G) C) and D)

Question 15

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

Accepted Answer

A)  all of the reactants and products are gases.
B)  in the reaction equation, the number of moles of gaseous products equals the number of moles of gaseous reactants.
C)  in the reaction equation, the number of moles of gaseous products is greater than the number of moles of gaseous reactants.
D)  in the reaction equation, the number of moles of gaseous products is smaller than the number of moles of gaseous reactants.
E)  in the reaction equation, the total number of moles of reactants equals that of the products.F) A) and D)
G) All of the above

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 Kp 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?

Accepted Answer

A)  0.16 atm
B)  0.31 atm
C)  3.1 atm
D)  7.7 atm
E)  7.8 atmF) D) and E)
G) B) and D)

Question 17

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

Accepted Answer

A) True 
 B)False

Question 18

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?

Accepted Answer

A)  10.0 g hydrogen remains
B)  10.9 g hydrogen remains
C)  15.0 g hydrogen remains
D)  19.9 g hydrogen remains
E)  Need to know the equilibrium constant in order to calculate the answer.F) B) and D)
G) A) and B)

Question 19

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?

Accepted Answer

A)  The partial pressure of hydrogen will decrease.
B)  The partial pressure of hydrogen will increase.
C)  The partial pressure of hydrogen will be unchanged.
D)  K p needs to be known before a prediction can be made.
E)  Both K p and the temperature need to be known before a prediction can be made.F) C) and E)
G) B) and E)

Question 20

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

Accepted Answer

A)  K p = K c
B)  K p = RT × K c
C)  K p = ( RT × K c) −1
D)  K p = K c / RT
E)  K p = RT / K cF) A) and D)
G) A) and B) B

Exam 17: Equilibrium: the Extent of Chemical Reactions

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.

Correct Answer
verified

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?

Correct Answer
verified

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.

Correct Answer
verified

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)

Correct Answer
verified

Correct Answer
verified

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?

Correct Answer
verified

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

Correct Answer
verified

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?

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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?

Correct Answer
verified
B

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.

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?

Correct Answer
verified
D

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?

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

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?

Correct Answer
verified

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?

Correct Answer
verified
B

Exam 17: Equilibrium: the Extent of Chemical Reactions

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.

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedB

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.

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedD

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedB

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.

Correct Answer
verified

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?

Correct Answer
verified

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.

Correct Answer
verified

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)

Correct Answer
verified

Correct Answer
verified

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?

Correct Answer
verified

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

Correct Answer
verified

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?

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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?

Correct Answer
verified
B

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?

Correct Answer
verified
D

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?

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

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?

Correct Answer
verified
B