Question 1

How is the reaction quotient used to determine whether a system is at equilibrium?

Accepted Answer

A)  The reaction quotient must be satisfied for equilibrium to be achieved.
B)  At equilibrium, the reaction quotient is undefined.
C)  The reaction is at equilibrium when Q eq.
D)  The reaction is at equilibrium when Q > Keq.
E)  The reaction is at equilibrium when Q = Keq.

Question 2

The equilibrium expression for Kp for the reaction below is __________. 2O3 (g)  p for the reaction below is __________. 2O3 (g)    3O2 (g)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > 3O2 (g)

Accepted Answer

A)   p for the reaction below is __________. 2O3 (g)    3O2 (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   p for the reaction below is __________. 2O3 (g)    3O2 (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   p for the reaction below is __________. 2O3 (g)    3O2 (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   p for the reaction below is __________. 2O3 (g)    3O2 (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   p for the reaction below is __________. 2O3 (g)    3O2 (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >

Question 3

In what year was Fritz Haber awarded the Nobel Prize in chemistry for his development of a process for synthesizing ammonia directly from nitrogen and hydrogen?

Accepted Answer

A)  1954
B)  1933
C)  1918
D)  1900
E)  1912

Question 4

At constant temperature, reducing the volume of a gaseous equilibrium mixture causes the reaction to shift in the direction that increases the number of moles of gas in the system.

Accepted Answer

A) True 
 B)False

Question 5

Which of the following expressions is the correct equilibrium-constant expression for the following reaction? CO2 (g) + 2H2 (g)  2 (g) + 2H2 (g)    CH3OH (g)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > CH3OH (g)

Accepted Answer

A)   2 (g) + 2H2 (g)    CH3OH (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   2 (g) + 2H2 (g)    CH3OH (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2 (g) + 2H2 (g)    CH3OH (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2 (g) + 2H2 (g)    CH3OH (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2 (g) + 2H2 (g)    CH3OH (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >

Question 6

Exactly 3.5 moles if N2O4 is placed in an empty 2.0-L container and allowed to reach equilibrium described by the equation
N2O4 (g)⇌ 2NO2 (g)
If at equilibrium the N2O4 is 25% dissociated, what is the value of the equilibrium constant for the reaction?

Accepted Answer

Question 7

The value of Keq for the equilibrium CO2 (g) + 2H2 (g)  eq 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? 1/2 CO2 + H2 (g)    1/2 CH3OH (g)  A) 7.30 B) 7.35 C) 0.136 D) 3.81 E) 6.90 × 10-2" class="answers-bank-image d-inline" rel="preload" > CH3OH (g) 
Is 14.5 at 483 °C. What is the value of Keq for the equilibrium below?
1/2 CO2 + H2 (g)  eq 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? 1/2 CO2 + H2 (g)    1/2 CH3OH (g)  A) 7.30 B) 7.35 C) 0.136 D) 3.81 E) 6.90 × 10-2" class="answers-bank-image d-inline" rel="preload" > 1/2 CH3OH (g)

Accepted Answer

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

Question 8

Pure __________ and pure __________ are excluded from equilibrium-constant expressions.

Accepted Answer

The answer of Pure __________ and pure __________ are excluded...

Question 9

The Keq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) + eq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) +   O2 (g)    SO3 (g)  What is the value of Keq at this temperature for the following reaction? 2SO2 (g) + O2 (g)    2SO3 (g)  A) 0.224 B) 0.335 C) 0.0125 D) 0.0560 E) 0.112" class="answers-bank-image d-inline" rel="preload" > O2 (g)  eq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) +   O2 (g)    SO3 (g)  What is the value of Keq at this temperature for the following reaction? 2SO2 (g) + O2 (g)    2SO3 (g)  A) 0.224 B) 0.335 C) 0.0125 D) 0.0560 E) 0.112" class="answers-bank-image d-inline" rel="preload" > SO3 (g) 
What is the value of Keq at this temperature for the following reaction?
2SO2 (g) + O2 (g)  eq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) +   O2 (g)    SO3 (g)  What is the value of Keq at this temperature for the following reaction? 2SO2 (g) + O2 (g)    2SO3 (g)  A) 0.224 B) 0.335 C) 0.0125 D) 0.0560 E) 0.112" class="answers-bank-image d-inline" rel="preload" > 2SO3 (g)

Accepted Answer

A)  0.224
B)  0.335
C)  0.0125
D)  0.0560
E)  0.112

Question 10

The equilibrium constant for the gas phase reaction N2 (g) + O2 (g)  2 (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" class="answers-bank-image d-inline" rel="preload" > 2NO (g) 
Is Keq = 4.20 × 10-31 at 30°C. At equilibrium, __________.

Accepted Answer

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

Question 11

At equilibrium, __________.

Accepted Answer

A)  all chemical reactions have ceased
B)  the rates of the forward and reverse reactions are equal
C)  the rate constants of the forward and reverse reactions are equal
D)  the value of the equilibrium constant is 1
E)  the limiting reagent has been consumed

Question 12

What role did Karl Bosch play in development of the Haber-Bosch process?

Accepted Answer

A)  He discovered the reaction conditions necessary for formation of ammonia.
B)  He originally isolated ammonia from camel dung and found a method for purifying it.
C)  Haber was working in his lab with his instructor at the time he worked out the process.
D)  He developed the equipment necessary for industrial production of ammonia.
E)  He was the German industrialist who financed the research done by Haber.

Question 13

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? 2SO2 (g) + O2 (g)  2 (g) + O2 (g)    2SO3 (g)  A) [SO3] / [SO2][O2] B) [SO2] / [SO3] C) [SO3]2 / [SO2]2[O2] D) [SO3]2 / [SO2]2[O2]2 E) [SO3] / [SO2][O2]2" class="answers-bank-image d-inline" rel="preload" > 2SO3 (g)

Accepted Answer

A)  [SO3] / [SO2][O2]
B)  [SO2] / [SO3]
C)  [SO3]2 / [SO2]2[O2]
D)  [SO3]2 / [SO2]2[O2]2
E)  [SO3] / [SO2][O2]2

Question 14

Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g)  2O4 (g)    2NO2 (g)  A 1.00-L flask is charged with 0.0400 mol of N2O4. At equilibrium at 373 K, 0.0055 mol of N2O4 remains. Keq for this reaction is __________. A) 2.2 × 10-4 B) 13 C) 0.22 D) 0.022 E) 0.87" class="answers-bank-image d-inline" rel="preload" > 2NO2 (g) 
A 1.00-L flask is charged with 0.0400 mol of N2O4. At equilibrium at 373 K, 0.0055 mol of N2O4 remains. Keq for this reaction is __________.

Accepted Answer

A)  2.2 × 10-4
B)  13
C)  0.22
D)  0.022
E)  0.87

Question 15

In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H2O (g)  2O (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 0.16 mol of CO remaining. Keq at the temperature of the experiment is __________. A) 5.5 B) 0.75 C) 0.93 D) 1.1 E) 1.0" class="answers-bank-image d-inline" rel="preload" > 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 0.16 mol of CO remaining. Keq at the temperature of the experiment is __________.

Accepted Answer

A)  5.5
B)  0.75
C)  0.93
D)  1.1
E)  1.0

Question 16

If the reaction quotient Q for a reaction is greater 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.

Accepted Answer

The answer of If the reaction quotient Q for a...

Question 17

Consider the following chemical reaction: H2 (g) + I2 (g)  2 (g) + I2 (g)    2HI (g)  At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.25 M, 0.035 M, and 0.55 M, respectively. The value of Keq for this reaction is __________. A) 23 B) 63 C) 0.0090 D) 5.1 E) 34" class="answers-bank-image d-inline" rel="preload" > 2HI (g) 
At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.25 M, 0.035 M, and 0.55 M, respectively. The value of Keq for this reaction is __________.

Accepted Answer

A)  23
B)  63
C)  0.0090
D)  5.1
E)  34

Question 18

Consider the following reaction at equilibrium. 2CO2 (g)  2 (g)    2CO (g) + O2 (g) ΔH° = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction __________. A) at high temperature and high pressure B) at high temperature and low pressure C) at low temperature and low pressure D) at low temperature and high pressure E) in the presence of solid carbon" class="answers-bank-image d-inline" rel="preload" > 2CO (g) + O2 (g) ΔH° = -514 kJ
Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction __________.

Accepted Answer

A)  at high temperature and high pressure
B)  at high temperature and low pressure
C)  at low temperature and low pressure
D)  at low temperature and high pressure
E)  in the presence of solid carbon

Question 19

Which one of the following will change the value of an equilibrium constant?

Accepted Answer

A)  changing temperature
B)  adding other substances that do not react with any of the species involved in the equilibrium
C)  varying the initial concentrations of reactants
D)  varying the initial concentrations of products
E)  changing the volume of the reaction vessel

Question 20

The equilibrium constant for the gas phase reaction N2 (g) + 3H2 (g)  2 (g) + 3H2 (g)    2NH3 (g)  Is Keq = 4.34 × 10-3 at 300°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" class="answers-bank-image d-inline" rel="preload" > 2NH3 (g) 
Is Keq = 4.34 × 10-3 at 300°C. At equilibrium, __________.

Accepted Answer

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

Exam 15: Chemical Equilibrium

How is the reaction quotient used to determine whether a system is at equilibrium?

Correct Answer
verified

The K_eq for the equilibrium below is 0.112 at 700.0°C. SO₂ (g) + O₂ (g) SO₃ (g) What is the value of K_eq at this temperature for the following reaction? 2SO₂ (g) + O₂ (g) 2SO₃ (g)

Correct Answer
verified

At equilibrium, __________.

Correct Answer
verified

In what year was Fritz Haber awarded the Nobel Prize in chemistry for his development of a process for synthesizing ammonia directly from nitrogen and hydrogen?

Correct Answer
verified

Pure and pure are excluded from equilibrium-constant expressions.

Correct Answer
verified

Which of the following expressions is the correct equilibrium-constant expression for the following reaction? CO₂ (g) + 2H₂ (g) CH₃OH (g)

Correct Answer
verified

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, __________.

Correct Answer
verified

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? 2SO₂ (g) + O₂ (g) 2SO₃ (g)

Correct Answer
verified

The equilibrium constant for the gas phase reaction N₂(g) + 3H₂ (g) 2NH₃ (g) Is K_eq= 4.34 × 10^-3 at 300°C. At equilibrium, __________.

Correct Answer
verified

Correct Answer
verified

Consider the following reaction at equilibrium. 2CO₂ (g) 2CO (g) + O₂ (g) ΔH° = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction __________.

Correct Answer
verified

Which one of the following will change the value of an equilibrium constant?

Correct Answer
verified

Dinitrogentetraoxide partially decomposes according to the following equilibrium: N₂O₄ (g) 2NO₂ (g) A 1.00-L flask is charged with 0.0400 mol of N₂O₄. At equilibrium at 373 K, 0.0055 mol of N₂O₄ remains. K_eq for this reaction is __________.

Correct Answer
verified

At constant temperature, reducing the volume of a gaseous equilibrium mixture causes the reaction to shift in the direction that increases the number of moles of gas in the system.

Correct Answer
verified

If the reaction quotient Q for a reaction is greater 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.

Correct Answer
verified

Consider the following chemical reaction: H₂ (g) + I₂ (g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H₂, I₂, and HI were 0.25 M, 0.035 M, and 0.55 M, respectively. The value of K_eq for this reaction is __________.

Correct Answer
verified

What role did Karl Bosch play in development of the Haber-Bosch process?

Correct Answer
verified

The equilibrium expression for K_p for the reaction below is __________. 2O₃(g) 3O₂(g)

Correct Answer
verified

Exactly 3.5 moles if N₂O₄ is placed in an empty 2.0-L container and allowed to reach equilibrium described by the equation N₂O₄ (g)⇌ 2NO₂(g) If at equilibrium the N₂O₄ is 25% dissociated, what is the value of the equilibrium constant for the reaction?

Correct Answer
verified

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? 1/2 CO₂ + H₂ (g) 1/2 CH₃OH (g)

Correct Answer
verified

Exam 15: Chemical Equilibrium

How is the reaction quotient used to determine whether a system is at equilibrium?

Correct AnswerverifiedShow Answer

The Keq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) + O2 (g) SO3 (g) What is the value of Keq at this temperature for the following reaction? 2SO2 (g) + O2 (g) 2SO3 (g)

Correct AnswerverifiedShow Answer

At equilibrium, __________.

Correct AnswerverifiedShow Answer

In what year was Fritz Haber awarded the Nobel Prize in chemistry for his development of a process for synthesizing ammonia directly from nitrogen and hydrogen?

Correct AnswerverifiedShow Answer

Pure __________ and pure __________ are excluded from equilibrium-constant expressions.

Correct AnswerverifiedShow Answer

Which of the following expressions is the correct equilibrium-constant expression for the following reaction? CO2 (g) + 2H2 (g) CH3OH (g)

Correct AnswerverifiedShow Answer

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, __________.

Correct AnswerverifiedShow Answer

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? 2SO2 (g) + O2 (g) 2SO3 (g)

Correct AnswerverifiedShow Answer

The equilibrium constant for the gas phase reaction N2 (g) + 3H2 (g) 2NH3 (g) Is Keq = 4.34 × 10-3 at 300°C. At equilibrium, __________.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Consider the following reaction at equilibrium. 2CO2 (g) 2CO (g) + O2 (g) ΔH° = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction __________.

Correct AnswerverifiedShow Answer

Which one of the following will change the value of an equilibrium constant?

Correct AnswerverifiedShow Answer

Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g) 2NO2 (g) A 1.00-L flask is charged with 0.0400 mol of N2O4. At equilibrium at 373 K, 0.0055 mol of N2O4 remains. Keq for this reaction is __________.

Correct AnswerverifiedShow Answer

At constant temperature, reducing the volume of a gaseous equilibrium mixture causes the reaction to shift in the direction that increases the number of moles of gas in the system.

Correct AnswerverifiedShow Answer

If the reaction quotient Q for a reaction is greater 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.

Correct AnswerverifiedShow Answer

Consider the following chemical reaction: H2 (g) + I2 (g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.25 M, 0.035 M, and 0.55 M, respectively. The value of Keq for this reaction is __________.

Correct AnswerverifiedShow Answer

What role did Karl Bosch play in development of the Haber-Bosch process?

Correct AnswerverifiedShow Answer

The equilibrium expression for Kp for the reaction below is __________. 2O3 (g) 3O2 (g)

Correct AnswerverifiedShow Answer

Exactly 3.5 moles if N2O4 is placed in an empty 2.0-L container and allowed to reach equilibrium described by the equation N2O4 (g)⇌ 2NO2 (g) If at equilibrium the N2O4 is 25% dissociated, what is the value of the equilibrium constant for the reaction?

Correct AnswerverifiedShow Answer

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? 1/2 CO2 + H2 (g) 1/2 CH3OH (g)

Correct AnswerverifiedShow Answer

Correct Answer
verified

The K_eq for the equilibrium below is 0.112 at 700.0°C. SO₂ (g) + O₂ (g) SO₃ (g) What is the value of K_eq at this temperature for the following reaction? 2SO₂ (g) + O₂ (g) 2SO₃ (g)

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Pure and pure are excluded from equilibrium-constant expressions.

Correct Answer
verified

Which of the following expressions is the correct equilibrium-constant expression for the following reaction? CO₂ (g) + 2H₂ (g) CH₃OH (g)

Correct Answer
verified

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, __________.

Correct Answer
verified

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? 2SO₂ (g) + O₂ (g) 2SO₃ (g)

Correct Answer
verified

The equilibrium constant for the gas phase reaction N₂(g) + 3H₂ (g) 2NH₃ (g) Is K_eq= 4.34 × 10^-3 at 300°C. At equilibrium, __________.

Correct Answer
verified

Correct Answer
verified

Consider the following reaction at equilibrium. 2CO₂ (g) 2CO (g) + O₂ (g) ΔH° = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction __________.

Correct Answer
verified

Correct Answer
verified

Dinitrogentetraoxide partially decomposes according to the following equilibrium: N₂O₄ (g) 2NO₂ (g) A 1.00-L flask is charged with 0.0400 mol of N₂O₄. At equilibrium at 373 K, 0.0055 mol of N₂O₄ remains. K_eq for this reaction is __________.

Correct Answer
verified

Correct Answer
verified

If the reaction quotient Q for a reaction is greater 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.

Correct Answer
verified

Consider the following chemical reaction: H₂ (g) + I₂ (g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H₂, I₂, and HI were 0.25 M, 0.035 M, and 0.55 M, respectively. The value of K_eq for this reaction is __________.

Correct Answer
verified

Correct Answer
verified

The equilibrium expression for K_p for the reaction below is __________. 2O₃(g) 3O₂(g)

Correct Answer
verified

Exactly 3.5 moles if N₂O₄ is placed in an empty 2.0-L container and allowed to reach equilibrium described by the equation N₂O₄ (g)⇌ 2NO₂(g) If at equilibrium the N₂O₄ is 25% dissociated, what is the value of the equilibrium constant for the reaction?

Correct Answer
verified

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? 1/2 CO₂ + H₂ (g) 1/2 CH₃OH (g)

Correct Answer
verified