Question 1

A student determined the equilibrium concentration in the following equation by neglecting the x term in the denominator. Was she justified or not in this approximation and why? K  4.0  102   4.0  102    A) Yes, the concentration is much greater than K, so the x can be ignored. B) Yes, the value of x determined in this way is less than 0.05, so it can be ignored. C) No, the value of x determined in this way significantly reduces the denominator. D) No, the value of x can never be ignored in solving an algebra problem. E) No, the value of K is much less than 1, so x cannot be ignored." class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  Yes, the concentration is much greater than K, so the x can be ignored.
B)  Yes, the value of x determined in this way is less than 0.05, so it can be ignored.
C)  No, the value of x determined in this way significantly reduces the denominator.
D)  No, the value of x can never be ignored in solving an algebra problem.
E)  No, the value of K is much less than 1, so x cannot be ignored.

Question 2

Which statement about an equilibrium constant, K, and a reaction quotient, Q, for a reaction is correct?

Accepted Answer

A)  Values for each can be determined using units of moles/liter or atmospheres.
B)  K is the reciprocal of Q: K  1/Q.
C)  K always is larger than Q.
D)  Q always is larger than K.
E)  Q can never equal K.

Question 3

When can an x be ignored in solving an equilibrium expression derived from a RICE table?

Accepted Answer

A)  whenever it simplifies the calculation
B)  whenever it is very much smaller than the term it is added to or subtracted from
C)  whenever the equilibrium concentration for that species is relatively very small
D)  whenever it is raised to any power higher than 1
E)  never

Question 4

Which expression corresponds to the equilibrium constant for the reaction written as 2H2(g)   O2(g)  2(g)   O2(g)    2H2O2(g) ? A) [H2]2[O2] B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > 2H2O2(g) ?

Accepted Answer

A)  [H2]2[O2]
B)   2(g)   O2(g)    2H2O2(g) ? 
A)  [H2]2[O2] 
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2(g)   O2(g)    2H2O2(g) ? 
A)  [H2]2[O2] 
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2(g)   O2(g)    2H2O2(g) ? 
A)  [H2]2[O2] 
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2(g)   O2(g)    2H2O2(g) ? 
A)  [H2]2[O2] 
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" > C

Question 5

Consider the equilibrium A  B  B   C. What is significant about the equilibrium state in which [B]  [C]? A) [A]  K B) [A]  [B]  [C] C) [B]  [C]  K D) [A]  1/K E) [C]/[B]  K" class="answers-bank-image d-inline" rel="preload" > C. What is significant about the equilibrium state in which [B]  [C]?

Accepted Answer

A)  [A]  K
B)  [A]  [B]  [C]
C)  [B]  [C]  K
D)  [A]  1/K
E)  [C]/[B]  K

Question 6

One mole of solid ammonium carbamate (NH4CO2NH2) decomposes to form gaseous ammonia (NH3) and carbon dioxide. Write an expression for the equilibrium constant for this reaction.

Accepted Answer

K<sub>c</sub> <font face="symbol">...

Question 7

Which of the following reactions will not shift toward the reactants products when the pressure of the system is altered by changing the volume?

Accepted Answer

A)  2CO2(g)  2(g)    2 CO(g)   O2(g)  
B)  CaCO3(s)    CaO(s)   CO2(g)  
C)  N2(g)   3H2(g)    2NH3(g)  
D)  H2(g)   I2(g)    2HI(g)  
E)  2SO2(g)   O2(g)    2SO3(g) " class="answers-bank-image d-inline" rel="preload" > 2 CO(g)   O2(g) 
B)  CaCO3(s)  2(g)    2 CO(g)   O2(g)  
B)  CaCO3(s)    CaO(s)   CO2(g)  
C)  N2(g)   3H2(g)    2NH3(g)  
D)  H2(g)   I2(g)    2HI(g)  
E)  2SO2(g)   O2(g)    2SO3(g) " class="answers-bank-image d-inline" rel="preload" > CaO(s)   CO2(g) 
C)  N2(g)   3H2(g)  2(g)    2 CO(g)   O2(g)  
B)  CaCO3(s)    CaO(s)   CO2(g)  
C)  N2(g)   3H2(g)    2NH3(g)  
D)  H2(g)   I2(g)    2HI(g)  
E)  2SO2(g)   O2(g)    2SO3(g) " class="answers-bank-image d-inline" rel="preload" > 2NH3(g) 
D)  H2(g)   I2(g)  2(g)    2 CO(g)   O2(g)  
B)  CaCO3(s)    CaO(s)   CO2(g)  
C)  N2(g)   3H2(g)    2NH3(g)  
D)  H2(g)   I2(g)    2HI(g)  
E)  2SO2(g)   O2(g)    2SO3(g) " class="answers-bank-image d-inline" rel="preload" > 2HI(g) 
E)  2SO2(g)   O2(g)  2(g)    2 CO(g)   O2(g)  
B)  CaCO3(s)    CaO(s)   CO2(g)  
C)  N2(g)   3H2(g)    2NH3(g)  
D)  H2(g)   I2(g)    2HI(g)  
E)  2SO2(g)   O2(g)    2SO3(g) " class="answers-bank-image d-inline" rel="preload" > 2SO3(g)

Question 8

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

Accepted Answer

Heterogeneous equilibrium cons...

Question 9

The chemical equilibrium constant for the following reaction is 14.5. CH3OH(g)  3OH(g)    CO(g)   2H2(g)  What is the value of the equilibrium constant for the following reaction?       A) 3.81 B) 2.62  101 C) 7.25 D) 1.38  101 E) 6.90  102" class="answers-bank-image d-inline" rel="preload" > CO(g)   2H2(g) 
What is the value of the equilibrium constant for the following reaction? 3OH(g)    CO(g)   2H2(g)  What is the value of the equilibrium constant for the following reaction?       A) 3.81 B) 2.62  101 C) 7.25 D) 1.38  101 E) 6.90  102" class="answers-bank-image d-inline" rel="preload" > 3OH(g)    CO(g)   2H2(g)  What is the value of the equilibrium constant for the following reaction?       A) 3.81 B) 2.62  101 C) 7.25 D) 1.38  101 E) 6.90  102" class="answers-bank-image d-inline" rel="preload" > 3OH(g)    CO(g)   2H2(g)  What is the value of the equilibrium constant for the following reaction?       A) 3.81 B) 2.62  101 C) 7.25 D) 1.38  101 E) 6.90  102" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  3.81
B)  2.62  101
C)  7.25
D)  1.38  101
E)  6.90  102 A

Question 10

Which of the following is true regarding the effect of a catalyst on chemical equilibrium?

Accepted Answer

A)  Only the forward rate increases, so the quantity of products increases.
B)  Only the forward rate increases, but the quantity of products remains the same.
C)  Both the forward and reverse rates increase, and the quantity of products increases.
D)  Both the forward and reverse rates increase, but the quantity of products is unchanged.
E)  The effect varies depending on whether the reaction is endothermic or exothermic.

Question 11

Given the reaction below, which of the following would cause an increase in the concentration of reactants? 2HF(g)  2(g)   H2(g)    H° 12.0 kJ/mol I. removal of hydrogen II. addition of HF III. increasing the temperature of the reaction IV. an increase in the volume of the container A) I only B) II only C) III only D) IV only E) III and IV" class="answers-bank-image d-inline" rel="preload" > F2(g)   H2(g)  2(g)   H2(g)    H° 12.0 kJ/mol I. removal of hydrogen II. addition of HF III. increasing the temperature of the reaction IV. an increase in the volume of the container A) I only B) II only C) III only D) IV only E) III and IV" class="answers-bank-image d-inline" rel="preload" > H° 12.0 kJ/mol
I. removal of hydrogen
II. addition of HF
III. increasing the temperature of the reaction
IV. an increase in the volume of the container

Accepted Answer

A)  I only
B)  II only
C)  III only
D)  IV only
E)  III and IV

Question 12

The equilibrium constants for the two reactions are known: Mm 4L m 4L   [ML4]m4 Ka HL   H L Kb What must be the value of the equilibrium constant, Koverall for the following overall reaction? Mm  4HL   [ML4]m4  4H Koverall A) KaKb B) Ka  4Kb C) Ka  Kb4 D) KaKb4 E) KaKb1/4" class="answers-bank-image d-inline" rel="preload" > [ML4]m4 Ka
HL m 4L   [ML4]m4 Ka HL   H L Kb What must be the value of the equilibrium constant, Koverall for the following overall reaction? Mm  4HL   [ML4]m4  4H Koverall A) KaKb B) Ka  4Kb C) Ka  Kb4 D) KaKb4 E) KaKb1/4" class="answers-bank-image d-inline" rel="preload" > H L Kb
What must be the value of the equilibrium constant, Koverall for the following overall reaction?
Mm  4HL m 4L   [ML4]m4 Ka HL   H L Kb What must be the value of the equilibrium constant, Koverall for the following overall reaction? Mm  4HL   [ML4]m4  4H Koverall A) KaKb B) Ka  4Kb C) Ka  Kb4 D) KaKb4 E) KaKb1/4" class="answers-bank-image d-inline" rel="preload" > [ML4]m4  4H Koverall

Accepted Answer

A)  KaKb
B)  Ka  4Kb
C)  Ka  Kb4
D)  KaKb4
E)  KaKb1/4

Question 13

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.

Question 14

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, because the effects of the two processes cancel each other out.

Question 15

The equilibrium constant for the reaction below is 17.5. S(s)   3 O2(g)   3 O2(g)    2 SO3(g)  What is the value of the equilibrium constant for the following reaction? 6 SO3(g)    3S(s)   9 O2(g)  A) 1.87  104 B) 5.71  102 C) 17.5 D) 306 E) 5360" class="answers-bank-image d-inline" rel="preload" > 2 SO3(g) 
What is the value of the equilibrium constant for the following reaction?
6 SO3(g)   3 O2(g)    2 SO3(g)  What is the value of the equilibrium constant for the following reaction? 6 SO3(g)    3S(s)   9 O2(g)  A) 1.87  104 B) 5.71  102 C) 17.5 D) 306 E) 5360" class="answers-bank-image d-inline" rel="preload" > 3S(s)   9 O2(g)

Accepted Answer

A)  1.87  104
B)  5.71  102
C)  17.5
D)  306
E)  5360

Question 16

Which of the following can be predicted from the law of mass action?
I. At equilibrium, the ratio of concentrations of products to reactants, each raised to a power corresponding to the stoichiometric coefficient in the balanced reaction equation, will have a constant value at a given temperature.
II. The direction of the reaction given values for the reactant and product concentrations and the equilibrium constant.
III. The amounts of products that can be produced from a given amount of reactants.

Accepted Answer

A)  I only
B)  II and III
C)  I, II, and III
D)  I and II
E)  I and III C

Question 17

Calculate K for the following reaction, provided the concentration versus time graph shown below.  2A  2A   2B  3C   A) 0.50 B) 0.68 C) 1.1 D) 1.5 E) 2.8" class="answers-bank-image d-inline" rel="preload" > 2B  3C  2A   2B  3C   A) 0.50 B) 0.68 C) 1.1 D) 1.5 E) 2.8" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  0.50
B)  0.68
C)  1.1
D)  1.5
E)  2.8

Question 18

In the following reaction, which of the statements is true, given the concentrations of each species? C6H6(g)   3H2(g)  6H6(g)   3H2(g)    C6H12(g)  K  1.23103 [C6H6]  [H2]  0.170 M and [C6H12]  0.025 M A) More hydrogen must be consumed to achieve equilibrium. B) More cyclohexane (C6H12)  must form to achieve equilibrium. C) The reaction is at equilibrium. D) More benzene (C6H6)  must be formed to achieve equilibrium. E) Equilibrium cannot be established in the system." class="answers-bank-image d-inline" rel="preload" > C6H12(g)  K  1.23103
[C6H6]  [H2]  0.170 M and [C6H12]  0.025 M

Accepted Answer

A)  More hydrogen must be consumed to achieve equilibrium.
B)  More cyclohexane (C6H12)  must form to achieve equilibrium.
C)  The reaction is at equilibrium.
D)  More benzene (C6H6)  must be formed to achieve equilibrium.
E)  Equilibrium cannot be established in the system.

Question 19

If Q for a reaction is greater than K, the reaction will be ________. If Q for a reaction is less than K, the reaction will be ________. If Q for a reaction is equal to K, the reaction will be ________.

Accepted Answer

nonspontan...

Question 20

The reaction of bromine gas with chlorine gas, shown here, has a Kp value of 7.20. If a closed vessel was charged with the two reactants, each at an initial partial pressure of 0.500 atm, what would be the equilibrium partial pressure of BrCl(g)?
Br2(g) F1F1F1S1F1F1F10 Cl2(g)  2BrCl(g)

Accepted Answer

Exam 14: Chemical Equilibrium: How Much Product Does a Reaction Really Make

A student determined the equilibrium concentration in the following equation by neglecting the x term in the denominator. Was she justified or not in this approximation and why? K  4.0  10^² 

Correct Answer
verified

Which statement about an equilibrium constant, K, and a reaction quotient, Q, for a reaction is correct?

Correct Answer
verified

When can an x be ignored in solving an equilibrium expression derived from a RICE table?

Correct Answer
verified

Which expression corresponds to the equilibrium constant for the reaction written as 2H₂(g)  O₂(g) 2H₂O₂(g) ?

Correct Answer
verified
C

Consider the equilibrium A  B C. What is significant about the equilibrium state in which [B]  [C]?

Correct Answer
verified

One mole of solid ammonium carbamate (NH₄CO₂NH₂) decomposes to form gaseous ammonia (NH₃) and carbon dioxide. Write an expression for the equilibrium constant for this reaction.

Correct Answer
verified
K_c ...
View Answer

Which of the following reactions will not shift toward the reactants products when the pressure of the system is altered by changing the volume?

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 chemical equilibrium constant for the following reaction is 14.5. CH₃OH(g) CO(g)  2H₂(g) What is the value of the equilibrium constant for the following reaction?

Correct Answer
verified
A

Which of the following is true regarding the effect of a catalyst on chemical equilibrium?

Correct Answer
verified

Given the reaction below, which of the following would cause an increase in the concentration of reactants? 2HF(g) F₂(g)  H₂(g) H^° 12.0 kJ/mol I. removal of hydrogen II. addition of HF III. increasing the temperature of the reaction IV. an increase in the volume of the container

Correct Answer
verified

The equilibrium constants for the two reactions are known: M^m^ 4L^ [ML₄]^m^⁴ K_a HL H^ L^ K_b What must be the value of the equilibrium constant, K_overall for the following overall reaction? M^m^  4HL [ML₄]^m^⁴  4H^ K_overall

Correct Answer
verified

An equilibrium that strongly favors products has ________

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

The equilibrium constant for the reaction below is 17.5. S(s)  3 O₂(g) 2 SO₃(g) What is the value of the equilibrium constant for the following reaction? 6 SO₃(g) 3S(s)  9 O₂(g)

Correct Answer
verified

Correct Answer
verified
C

Calculate K for the following reaction, provided the concentration versus time graph shown below. 2A 2B  3C

Correct Answer
verified

In the following reaction, which of the statements is true, given the concentrations of each species? C₆H₆(g)  3H₂(g) C₆H₁₂(g) K  1.2310^³ [C₆H₆]  [H₂]  0.170 M and [C₆H₁₂]  0.025 M

Correct Answer
verified

If Q for a reaction is greater than K, the reaction will be . If Q for a reaction is less than K, the reaction will be . If Q for a reaction is equal to K, the reaction will be .

Correct Answer
verified
nonspontan...
View Answer

The reaction of bromine gas with chlorine gas, shown here, has a K_p value of 7.20. If a closed vessel was charged with the two reactants, each at an initial partial pressure of 0.500 atm, what would be the equilibrium partial pressure of BrCl(g)? Br₂(g)  Cl₂(g) 2BrCl(g)

Correct Answer
verified

Exam 14: Chemical Equilibrium: How Much Product Does a Reaction Really Make

A student determined the equilibrium concentration in the following equation by neglecting the x term in the denominator. Was she justified or not in this approximation and why? K  4.0  102 

Correct AnswerverifiedShow Answer

Which statement about an equilibrium constant, K, and a reaction quotient, Q, for a reaction is correct?

Correct AnswerverifiedShow Answer

When can an x be ignored in solving an equilibrium expression derived from a RICE table?

Correct AnswerverifiedShow Answer

Which expression corresponds to the equilibrium constant for the reaction written as 2H2(g)  O2(g) 2H2O2(g) ?

Correct AnswerverifiedC

Consider the equilibrium A  B C. What is significant about the equilibrium state in which [B]  [C]?

Correct AnswerverifiedShow Answer

One mole of solid ammonium carbamate (NH4CO2NH2) decomposes to form gaseous ammonia (NH3) and carbon dioxide. Write an expression for the equilibrium constant for this reaction.

Correct AnswerverifiedKc ...View AnswerShow Answer

Which of the following reactions will not shift toward the reactants products when the pressure of the system is altered by changing the volume?

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 chemical equilibrium constant for the following reaction is 14.5. CH3OH(g) CO(g)  2H2(g) What is the value of the equilibrium constant for the following reaction?

Correct AnswerverifiedA

Which of the following is true regarding the effect of a catalyst on chemical equilibrium?

Correct AnswerverifiedShow Answer

Given the reaction below, which of the following would cause an increase in the concentration of reactants? 2HF(g) F2(g)  H2(g) H° 12.0 kJ/mol I. removal of hydrogen II. addition of HF III. increasing the temperature of the reaction IV. an increase in the volume of the container

Correct AnswerverifiedShow Answer

The equilibrium constants for the two reactions are known: Mm 4L [ML4]m4 Ka HL H L Kb What must be the value of the equilibrium constant, Koverall for the following overall reaction? Mm  4HL [ML4]m4  4H Koverall

Correct AnswerverifiedShow Answer

An equilibrium that strongly favors products has ________

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

The equilibrium constant for the reaction below is 17.5. S(s)  3 O2(g) 2 SO3(g) What is the value of the equilibrium constant for the following reaction? 6 SO3(g) 3S(s)  9 O2(g)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedC

Calculate K for the following reaction, provided the concentration versus time graph shown below. 2A 2B  3C

Correct AnswerverifiedShow Answer

In the following reaction, which of the statements is true, given the concentrations of each species? C6H6(g)  3H2(g) C6H12(g) K  1.23103 [C6H6]  [H2]  0.170 M and [C6H12]  0.025 M

Correct AnswerverifiedShow Answer

If Q for a reaction is greater than K, the reaction will be ________. If Q for a reaction is less than K, the reaction will be ________. If Q for a reaction is equal to K, the reaction will be ________.

Correct Answerverifiednonspontan...View AnswerShow Answer

The reaction of bromine gas with chlorine gas, shown here, has a Kp value of 7.20. If a closed vessel was charged with the two reactants, each at an initial partial pressure of 0.500 atm, what would be the equilibrium partial pressure of BrCl(g)? Br2(g)  Cl2(g) 2BrCl(g)

Correct AnswerverifiedShow Answer

A student determined the equilibrium concentration in the following equation by neglecting the x term in the denominator. Was she justified or not in this approximation and why? K  4.0  10^² 

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Which expression corresponds to the equilibrium constant for the reaction written as 2H₂(g)  O₂(g) 2H₂O₂(g) ?

Correct Answer
verified
C

Correct Answer
verified

One mole of solid ammonium carbamate (NH₄CO₂NH₂) decomposes to form gaseous ammonia (NH₃) and carbon dioxide. Write an expression for the equilibrium constant for this reaction.

Correct Answer
verified
K_c ...
View Answer

Correct Answer
verified

Correct Answer
verified
Heterogeneous equilibrium cons...
View Answer

The chemical equilibrium constant for the following reaction is 14.5. CH₃OH(g) CO(g)  2H₂(g) What is the value of the equilibrium constant for the following reaction?

Correct Answer
verified
A

Correct Answer
verified

Given the reaction below, which of the following would cause an increase in the concentration of reactants? 2HF(g) F₂(g)  H₂(g) H^° 12.0 kJ/mol I. removal of hydrogen II. addition of HF III. increasing the temperature of the reaction IV. an increase in the volume of the container

Correct Answer
verified

The equilibrium constants for the two reactions are known: M^m^ 4L^ [ML₄]^m^⁴ K_a HL H^ L^ K_b What must be the value of the equilibrium constant, K_overall for the following overall reaction? M^m^  4HL [ML₄]^m^⁴  4H^ K_overall

Correct Answer
verified

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

The equilibrium constant for the reaction below is 17.5. S(s)  3 O₂(g) 2 SO₃(g) What is the value of the equilibrium constant for the following reaction? 6 SO₃(g) 3S(s)  9 O₂(g)

Correct Answer
verified

Correct Answer
verified
C

Correct Answer
verified

In the following reaction, which of the statements is true, given the concentrations of each species? C₆H₆(g)  3H₂(g) C₆H₁₂(g) K  1.2310^³ [C₆H₆]  [H₂]  0.170 M and [C₆H₁₂]  0.025 M

Correct Answer
verified

If Q for a reaction is greater than K, the reaction will be . If Q for a reaction is less than K, the reaction will be . If Q for a reaction is equal to K, the reaction will be .

Correct Answer
verified
nonspontan...
View Answer

The reaction of bromine gas with chlorine gas, shown here, has a K_p value of 7.20. If a closed vessel was charged with the two reactants, each at an initial partial pressure of 0.500 atm, what would be the equilibrium partial pressure of BrCl(g)? Br₂(g)  Cl₂(g) 2BrCl(g)

Correct Answer
verified