Question 1

For a chemical reaction at equilibrium, which of the following will change the value of the equilibrium constant K?
(I) Changing the temperature
(II) Changing the total concentration of reactants and products
(III) Changing the reaction coefficients

Accepted Answer

A)   I only
B)   II only
C)   III only
D)   I and II only
E)   I and III onlyF) C) and E)
G) All of the above

Question 2

Write the expression for the reaction quotient for the reaction Zn2+(aq)  + 2NH3(aq)  2+(aq)  + 2NH3(aq)    Zn(NH3) 2+(aq)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > Zn(NH3) 2+(aq)

Accepted Answer

A)   2+(aq)  + 2NH3(aq)    Zn(NH3) 2+(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   2+(aq)  + 2NH3(aq)    Zn(NH3) 2+(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2+(aq)  + 2NH3(aq)    Zn(NH3) 2+(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2+(aq)  + 2NH3(aq)    Zn(NH3) 2+(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2+(aq)  + 2NH3(aq)    Zn(NH3) 2+(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) A) and B)
G) A) and C) D

Question 3

The forward rate constant, kf, and reverse rate constant, kr, for a chemical reaction are not equal. Which of the following must be true?

Accepted Answer

A)   The reaction will be unable to achieve equilibrium.
B)   kf and kr will become equal as equilibrium is approached owing to concentration changes.
C)   kf and kr will become equal as equilibrium is approached owing to temperature changes.
D)   kf and kr will remain unequal but the rates will become equal owing to concentration changes.
E)   kf and kr will remain unequal but the rates will become equal owing to temperature changes.F) B) and C)
G) A) and C)

Question 4

What happens to the equilibrium between NO2(g)  and N2O4(g)  in inert argon when the volume is increased and additional argon is added to maintain a constant total pressure?

Accepted Answer

A)   The ratio of NO2 to N2O4 increases solely because of the increase in volume.
B)   The ratio of NO2 to N2O4 increases solely because of the addition of argon.
C)   The ratio of NO2 to N2O4 decreases solely because of the increase in volume.
D)   The ratio of NO2 to N2O4 decreases solely because of the addition of argon.
E)   The ratio of NO2 to N2O4 remains the same, as the effects of the two processes cancel.F) A) and D)
G) C) and E)

Question 5

For a particular hypothetical reaction, 2A + B  C, the value of G is 250 kJ/mol. What is the value of G for this reaction at 298 K when [A] = 0.60 M, [B] = 0.10 M, and [C] = 4.0  10-3 M?

Accepted Answer

A)   248 kJ/mol
B)   245 kJ/mol
C)   2775 kJ/mol
D)   250 kJ/mol
E)   255 kJ/molF) A) and B)
G) A) and D)

Question 6

Using the thermodynamic data below, determine the equilibrium constant for the conversion of oxygen to ozone at 2000 K. Substance H H   (kJ/mol)  G   (kJ/mol)  S (J/mol · K)  O2(g)  0 0 205.0 O3(g)  142.3 163.4 237.6 3O2(g)    2O3(g)  A)  2.04  107 B)  5.44  10-14 C)  2.67  10-8 D)  2.91  10-9 E)  3.65  10-12" class="answers-bank-image d-inline" rel="preload" > (kJ/mol)  G H   (kJ/mol)  G   (kJ/mol)  S (J/mol · K)  O2(g)  0 0 205.0 O3(g)  142.3 163.4 237.6 3O2(g)    2O3(g)  A)  2.04  107 B)  5.44  10-14 C)  2.67  10-8 D)  2.91  10-9 E)  3.65  10-12" class="answers-bank-image d-inline" rel="preload" > (kJ/mol)  S (J/mol · K) 
O2(g)  0 0 205.0
O3(g)  142.3 163.4 237.6
3O2(g)  H   (kJ/mol)  G   (kJ/mol)  S (J/mol · K)  O2(g)  0 0 205.0 O3(g)  142.3 163.4 237.6 3O2(g)    2O3(g)  A)  2.04  107 B)  5.44  10-14 C)  2.67  10-8 D)  2.91  10-9 E)  3.65  10-12" class="answers-bank-image d-inline" rel="preload" > 2O3(g)

Accepted Answer

A)   2.04  107
B)   5.44  10-14
C)   2.67  10-8
D)   2.91  10-9
E)   3.65  10-12F) C) and E)
G) A) and E)

Question 7

A reaction X + 2Y  3Z is started with 1.0 M Z and no X or Y. To calculate the equilibrium concentrations of all species using an ICE table, which of the following would you enter in the Z column for the C row?

Accepted Answer

A)   1.0 M
B)   1.0 M - x
C)   1.0 M - 3x
D)   1.0 M + 3x
E)   -3xF) A) and E)
G) A) and D)

Question 8

Consider the reaction of nitrogen and hydrogen gas under standard state conditions to form two moles of ammonia gas (NH3). Write the initial expression for Kc that would be derived from an ICE table if the concentrations of all species were as follows.
[N2] = 3 M
[H2] = 2 M
[NH3] = 1 M

Accepted Answer

Question 9

How and why are the expressions for homogeneous equilibrium constants different from the expressions for heterogeneous equilibrium constants?

Accepted Answer

Heterogeneous equilibrium cons...

Question 10

The values of H°rxn and S°rxn are shown for the following equilibrium reaction. What makes the equilibrium constant larger at low temperature? 2NO2(g)  H°rxn and S°rxn are shown for the following equilibrium reaction. What makes the equilibrium constant larger at low temperature? 2NO2(g)    N2O4(g)  H= -58.02 kJ/mol, S°-176.5 J/mol · K A)  The negative value of H is dominant at all temperatures. B)  The negative value of S° is dominant at all temperatures. C)  The negative value of S° is combined with the small value of T. D)  The negative value of H is combined with the small value of T." class="answers-bank-image d-inline" rel="preload" > N2O4(g)  H= -58.02 kJ/mol, S°-176.5 J/mol · K

Accepted Answer

A)   The negative value of H is dominant at all temperatures.
B)   The negative value of S° is dominant at all temperatures.
C)   The negative value of S° is combined with the small value of T.
D)   The negative value of H is combined with the small value of T.E) A) and D)
F) B) and C)

Question 11

As the temperature of an endothermic reaction is increased, the equilibrium constant __________

Accepted Answer

A)   always increases.
B)   always decreases.
C)   always stays the same.
D)   only increases when S° > 0.
E)   only increases when S° < 0.F) C) and E)
G) B) and D)

Question 12

As the temperature of a reaction with S° > 0 is increased, the equilibrium constant __________

Accepted Answer

A)   always increases.
B)   always decreases.
C)   always stays the same.
D)   only increases when H° > 0.
E)   only increases when H° < 0.F) B) and D)
G) A) and E)

Question 13

For the reaction of hydrogen and nitrogen gases at 30°C to form two moles of ammonia gas (NH3), the value of Kp is 4.5 F1F1F1S1F1F1F10 10-12. What is the value of Kc for the same reaction?

Accepted Answer

2.8 F1F1F1...

Question 14

Under what conditions are the values of Kc and Kp for a given gas-phase equilibrium the same?

Accepted Answer

A)   there is no change in the moles of gas in the reaction
B)   there is no change in the temperature during the reaction
C)   if the coefficients of the reactants and products are the same
D)   if the pressure remains constant
E)   if either Kc or Kp = 1F) C) and D)
G) B) and E)

Question 15

Several groups of general chemistry lab students measured the equilibrium constant for the same chemical equilibrium. In comparing their results, they found that they had different values because the temperatures of the experiments were different. Everyone was disappointed by the inconsistency, except for Dexter when he realized the measurements were made at different measured temperatures: "My esteemed colleagues," he said, "together we have sufficient data to determine two additional thermodynamic parameters and show the lab instructor what we know!" What two parameters did Dexter have in mind?

Accepted Answer

A)   "G" and "H"
B)   "G" and "S"
C)   "H" and "S"
D)   "E" and "S"
E)   This cannot be determined as there are no two thermodynamic parameters related to K and T.F) A) and B)
G) C) and D)

Question 16

Jane can accept that "G" = -RTlnK, but she cannot reconcile the relationship between "S" and lnK. Please explain it to her.

Accepted Answer

A)   "S" = R lnK - "H"/T
B)   "S" = +ln(K/R)  + "H"/T
C)   "S" = +R ln(K/T)  + "H"
D)   "S" = +R ln(K)  + "H"/T
E)   "S" = -R ln(K)  + "H"/TF) A) and E)
G) C) and E)

Question 17

For the chemical equilibrium aA + bB  cC, the value of the equilibrium constant, K, is 10. What is the value of the equilibrium constant for the following reaction? 2cC  2aA + 2bB

Accepted Answer

A)   0.10
B)   0.20
C)   0.010
D)   20
E)   10F) B) and D)
G) All of the above C

Question 18

An equilibrium that strongly favors products has __________

Accepted Answer

A)   a value of K  1.
B)   a value of K >> 1.
C)   a value of Q >> 1.
D)   a value of Q  1.
E)   K = Q.F) A) and C)
G) B) and D)

Question 19

A series of four equilibrium steps can be defined for the following overall reaction: Cu2+ + 4NH3 2+ + 4NH3   [Cu(NH3) 4]2+ Koverall Cu2+ + NH3   [Cu(NH3) ]2+ K1 [Cu(NH3) ]2+ + NH3   [Cu(NH3) 2]2+ K2 Etc)  What is true about K4? A)  K4 = Koverall B)  K4 = K1K2K3 C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > [Cu(NH3) 4]2+
Koverall
Cu2+ + NH3 2+ + 4NH3   [Cu(NH3) 4]2+ Koverall Cu2+ + NH3   [Cu(NH3) ]2+ K1 [Cu(NH3) ]2+ + NH3   [Cu(NH3) 2]2+ K2 Etc)  What is true about K4? A)  K4 = Koverall B)  K4 = K1K2K3 C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > [Cu(NH3) ]2+
K1
[Cu(NH3) ]2+ + NH3 2+ + 4NH3   [Cu(NH3) 4]2+ Koverall Cu2+ + NH3   [Cu(NH3) ]2+ K1 [Cu(NH3) ]2+ + NH3   [Cu(NH3) 2]2+ K2 Etc)  What is true about K4? A)  K4 = Koverall B)  K4 = K1K2K3 C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > [Cu(NH3) 2]2+
K2
Etc) 
What is true about K4?

Accepted Answer

A)   K4 = Koverall
B)   K4 = K1K2K3
C)   2+ + 4NH3   [Cu(NH3) 4]2+ Koverall Cu2+ + NH3   [Cu(NH3) ]2+ K1 [Cu(NH3) ]2+ + NH3   [Cu(NH3) 2]2+ K2 Etc)  What is true about K4? 
A)   K4 = Koverall 
B)   K4 = K1K2K3 
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2+ + 4NH3   [Cu(NH3) 4]2+ Koverall Cu2+ + NH3   [Cu(NH3) ]2+ K1 [Cu(NH3) ]2+ + NH3   [Cu(NH3) 2]2+ K2 Etc)  What is true about K4? 
A)   K4 = Koverall 
B)   K4 = K1K2K3 
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2+ + 4NH3   [Cu(NH3) 4]2+ Koverall Cu2+ + NH3   [Cu(NH3) ]2+ K1 [Cu(NH3) ]2+ + NH3   [Cu(NH3) 2]2+ K2 Etc)  What is true about K4? 
A)   K4 = Koverall 
B)   K4 = K1K2K3 
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) A) and E)
G) All of the above

Question 20

For the chemical equilibrium aA + bB  cC, the value of the equilibrium constant, K, is 10. What is the value of the equilibrium constant for the following reaction? cC  aA + bB

Accepted Answer

A)   0.10
B)   10
C)   1
D)   100
E)   -10F) B) and E)
G) None of the above A

Exam 16: Chemical Equilibrium

For a chemical reaction at equilibrium, which of the following will change the value of the equilibrium constant K? (I) Changing the temperature (II) Changing the total concentration of reactants and products (III) Changing the reaction coefficients

Correct Answer
verified

Write the expression for the reaction quotient for the reaction Zn²⁺(aq) + 2NH₃(aq) Zn(NH₃) ²⁺(aq)

Correct Answer
verified
D

The forward rate constant, k_f, and reverse rate constant, k_r, for a chemical reaction are not equal. Which of the following must be true?

Correct Answer
verified

What happens to the equilibrium between NO₂(g) and N₂O₄(g) in inert argon when the volume is increased and additional argon is added to maintain a constant total pressure?

Correct Answer
verified

For a particular hypothetical reaction, 2A + B  C, the value of G is 250 kJ/mol. What is the value of G for this reaction at 298 K when [A] = 0.60 M, [B] = 0.10 M, and [C] = 4.0  10^-³ M?

Correct Answer
verified

Using the thermodynamic data below, determine the equilibrium constant for the conversion of oxygen to ozone at 2000 K. Substance H (kJ/mol) G (kJ/mol) S (J/mol · K) O₂(g) 0 0 205.0 O₃(g) 142.3 163.4 237.6 3O₂(g) 2O₃(g)

Correct Answer
verified

A reaction X + 2Y  3Z is started with 1.0 M Z and no X or Y. To calculate the equilibrium concentrations of all species using an ICE table, which of the following would you enter in the Z column for the C row?

Correct Answer
verified

Consider the reaction of nitrogen and hydrogen gas under standard state conditions to form two moles of ammonia gas (NH₃). Write the initial expression for K_c that would be derived from an ICE table if the concentrations of all species were as follows. [N₂] = 3 M [H₂] = 2 M [NH₃] = 1 M

Correct Answer
verified

How and why are the expressions for homogeneous equilibrium constants different from the expressions for heterogeneous equilibrium constants?

Correct Answer
verified
Heterogeneous equilibrium cons...
View Answer

The values of H°_rxn and S°_rxn are shown for the following equilibrium reaction. What makes the equilibrium constant larger at low temperature? 2NO₂(g) N₂O₄(g) H= -58.02 kJ/mol, S°-176.5 J/mol · K

Correct Answer
verified

As the temperature of an endothermic reaction is increased, the equilibrium constant __________

Correct Answer
verified

As the temperature of a reaction with S° > 0 is increased, the equilibrium constant __________

Correct Answer
verified

For the reaction of hydrogen and nitrogen gases at 30°C to form two moles of ammonia gas (NH₃), the value of K_p is 4.5  10^-¹². What is the value of K_c for the same reaction?

Correct Answer
verified
2.8 F1F1F1...
View Answer

Under what conditions are the values of K_c and K_p for a given gas-phase equilibrium the same?

Correct Answer
verified

Correct Answer
verified

Jane can accept that "G" = -RTlnK, but she cannot reconcile the relationship between "S" and lnK. Please explain it to her.

Correct Answer
verified

For the chemical equilibrium aA + bB cC, the value of the equilibrium constant, K, is 10. What is the value of the equilibrium constant for the following reaction? 2cC 2aA + 2bB

Correct Answer
verified
C

An equilibrium that strongly favors products has __________

Correct Answer
verified

A series of four equilibrium steps can be defined for the following overall reaction: Cu²⁺ + 4NH₃ [Cu(NH₃) ₄]²⁺ K_overall Cu²⁺ + NH₃ [Cu(NH₃) ]²⁺ K₁ [Cu(NH₃) ]²⁺ + NH₃ [Cu(NH₃) ₂]²⁺ K₂ Etc) What is true about K₄?

Correct Answer
verified

For the chemical equilibrium aA + bB cC, the value of the equilibrium constant, K, is 10. What is the value of the equilibrium constant for the following reaction? cC aA + bB

Correct Answer
verified
A

Exam 16: Chemical Equilibrium

For a chemical reaction at equilibrium, which of the following will change the value of the equilibrium constant K? (I) Changing the temperature (II) Changing the total concentration of reactants and products (III) Changing the reaction coefficients

Correct AnswerverifiedShow Answer

Write the expression for the reaction quotient for the reaction Zn2+(aq) + 2NH3(aq) Zn(NH3) 2+(aq)

Correct AnswerverifiedD

The forward rate constant, kf, and reverse rate constant, kr, for a chemical reaction are not equal. Which of the following must be true?

Correct AnswerverifiedShow Answer

What happens to the equilibrium between NO2(g) and N2O4(g) in inert argon when the volume is increased and additional argon is added to maintain a constant total pressure?

Correct AnswerverifiedShow Answer

For a particular hypothetical reaction, 2A + B  C, the value of G is 250 kJ/mol. What is the value of G for this reaction at 298 K when [A] = 0.60 M, [B] = 0.10 M, and [C] = 4.0  10-3 M?

Correct AnswerverifiedShow Answer

Using the thermodynamic data below, determine the equilibrium constant for the conversion of oxygen to ozone at 2000 K. Substance H (kJ/mol) G (kJ/mol) S (J/mol · K) O2(g) 0 0 205.0 O3(g) 142.3 163.4 237.6 3O2(g) 2O3(g)

Correct AnswerverifiedShow Answer

A reaction X + 2Y  3Z is started with 1.0 M Z and no X or Y. To calculate the equilibrium concentrations of all species using an ICE table, which of the following would you enter in the Z column for the C row?

Correct AnswerverifiedShow Answer

Consider the reaction of nitrogen and hydrogen gas under standard state conditions to form two moles of ammonia gas (NH3). Write the initial expression for Kc that would be derived from an ICE table if the concentrations of all species were as follows. [N2] = 3 M [H2] = 2 M [NH3] = 1 M

Correct AnswerverifiedShow Answer

How and why are the expressions for homogeneous equilibrium constants different from the expressions for heterogeneous equilibrium constants?

Correct AnswerverifiedHeterogeneous equilibrium cons...View AnswerShow Answer

The values of H°rxn and S°rxn are shown for the following equilibrium reaction. What makes the equilibrium constant larger at low temperature? 2NO2(g) N2O4(g) H= -58.02 kJ/mol, S°-176.5 J/mol · K

Correct AnswerverifiedShow Answer

As the temperature of an endothermic reaction is increased, the equilibrium constant __________

Correct AnswerverifiedShow Answer

As the temperature of a reaction with S° > 0 is increased, the equilibrium constant __________

Correct AnswerverifiedShow Answer

For the reaction of hydrogen and nitrogen gases at 30°C to form two moles of ammonia gas (NH3), the value of Kp is 4.5  10-12. What is the value of Kc for the same reaction?

Correct Answerverified2.8 F1F1F1...View AnswerShow Answer

Under what conditions are the values of Kc and Kp for a given gas-phase equilibrium the same?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Jane can accept that "G" = -RTlnK, but she cannot reconcile the relationship between "S" and lnK. Please explain it to her.

Correct AnswerverifiedShow Answer

For the chemical equilibrium aA + bB cC, the value of the equilibrium constant, K, is 10. What is the value of the equilibrium constant for the following reaction? 2cC 2aA + 2bB

Correct AnswerverifiedC

An equilibrium that strongly favors products has __________

Correct AnswerverifiedShow Answer

A series of four equilibrium steps can be defined for the following overall reaction: Cu2+ + 4NH3 [Cu(NH3) 4]2+ Koverall Cu2+ + NH3 [Cu(NH3) ]2+ K1 [Cu(NH3) ]2+ + NH3 [Cu(NH3) 2]2+ K2 Etc) What is true about K4?

Correct AnswerverifiedShow Answer

For the chemical equilibrium aA + bB cC, the value of the equilibrium constant, K, is 10. What is the value of the equilibrium constant for the following reaction? cC aA + bB

Correct AnswerverifiedA

Correct Answer
verified

Write the expression for the reaction quotient for the reaction Zn²⁺(aq) + 2NH₃(aq) Zn(NH₃) ²⁺(aq)

Correct Answer
verified
D

The forward rate constant, k_f, and reverse rate constant, k_r, for a chemical reaction are not equal. Which of the following must be true?

Correct Answer
verified

What happens to the equilibrium between NO₂(g) and N₂O₄(g) in inert argon when the volume is increased and additional argon is added to maintain a constant total pressure?

Correct Answer
verified

For a particular hypothetical reaction, 2A + B  C, the value of G is 250 kJ/mol. What is the value of G for this reaction at 298 K when [A] = 0.60 M, [B] = 0.10 M, and [C] = 4.0  10^-³ M?

Correct Answer
verified

Using the thermodynamic data below, determine the equilibrium constant for the conversion of oxygen to ozone at 2000 K. Substance H (kJ/mol) G (kJ/mol) S (J/mol · K) O₂(g) 0 0 205.0 O₃(g) 142.3 163.4 237.6 3O₂(g) 2O₃(g)

Correct Answer
verified

Correct Answer
verified

Consider the reaction of nitrogen and hydrogen gas under standard state conditions to form two moles of ammonia gas (NH₃). Write the initial expression for K_c that would be derived from an ICE table if the concentrations of all species were as follows. [N₂] = 3 M [H₂] = 2 M [NH₃] = 1 M

Correct Answer
verified

Correct Answer
verified
Heterogeneous equilibrium cons...
View Answer

The values of H°_rxn and S°_rxn are shown for the following equilibrium reaction. What makes the equilibrium constant larger at low temperature? 2NO₂(g) N₂O₄(g) H= -58.02 kJ/mol, S°-176.5 J/mol · K

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

For the reaction of hydrogen and nitrogen gases at 30°C to form two moles of ammonia gas (NH₃), the value of K_p is 4.5  10^-¹². What is the value of K_c for the same reaction?

Correct Answer
verified
2.8 F1F1F1...
View Answer

Under what conditions are the values of K_c and K_p for a given gas-phase equilibrium the same?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
C

Correct Answer
verified

A series of four equilibrium steps can be defined for the following overall reaction: Cu²⁺ + 4NH₃ [Cu(NH₃) ₄]²⁺ K_overall Cu²⁺ + NH₃ [Cu(NH₃) ]²⁺ K₁ [Cu(NH₃) ]²⁺ + NH₃ [Cu(NH₃) ₂]²⁺ K₂ Etc) What is true about K₄?

Correct Answer
verified

Correct Answer
verified
A