Question 1

How is the reaction quotient different from an equilibrium constant for a given reaction?

Accepted Answer

The expression for both are identical.Ho...

Question 2

Consider the following reaction at equilibrium.What effect will adding more SO3 have on the system?
SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)

Accepted Answer

A)   The reaction will shift in the direction of products.
B)   The reaction will shift to decrease the pressure.
C)   No change will occur since SO3 is not included in the equilibrium expression.
D)   The reaction will shift in the direction of reactants.
E)   The equilibrium constant will decrease.

Question 3

Consider the following reaction at equilibrium.What effect will reducing the pressure have on the system?
C3H8(g) + 5 O2(g) ⇌ 3 CO2(g) + 4 H2O(l) ΔH° = -2220 kJ

Accepted Answer

A)   The reaction will shift to the right in the direction of products.
B)   The reaction will shift to the left in the direction of reactants.
C)   The equilibrium constant will increase.
D)   The equilibrium constant will decrease.
E)   No effect will be observed.

Question 4

In a reaction mixture containing only reactants,what is the value of Q?

Accepted Answer

A)   -1
B)   1
C)   ∞
D)   0
E)   It cannot be determined without concentrations.

Question 5

Consider the following reaction: Xe(g) + 2 F2(g) → XeF4(g) 
A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F2.If the equilibrium pressure of Xe is 0.34 atm,find the equilibrium constant (Kp) for the reaction.

Accepted Answer

A)   25
B)   0.12
C)   0.99
D)   8.3
E)   0.040

Question 6

The reaction below has a Kc value of 3.64 × 10-3.What is the value of Kp for this reaction at 25°C?
2 NaN3(s) ⇌ 2 Na(s) + 3 N2(g)

Accepted Answer

A)   131
B)   0.613
C)   8.90 × 10-2
D)   29.9
E)   53.2

Question 7

What is △n for the following equation in relating Kc to Kp?
P4(s) + 5 O2(g) ⇌ P4O10(s)

Accepted Answer

A)   3
B)   0
C)   -3
D)   -6
E)   -5

Question 8

Consider the following reaction at equilibrium.What effect will raising the pressure of the system from 5 atm to 8 atm?
2 NH3(g) ⇌ N2(g) + 3 H2(g)

Accepted Answer

A)   It will shift to the right
B)   It will shift to the left
C)   It will have no effect
D)   It will speed up the reaction
E)   It will slow down the reaction

Question 9

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. 2 SO2(g) + O2(g) ⇌ 2 SO3(g) Kc = 1.7 × 106
SO3(g) ⇌ 1/2 O2(g) + SO2(g) Kc = ?

Accepted Answer

A)   3.4 × 102
B)   8.5
C)   1.3 × 103
D)   1.2 × 10-6
E)   7.7 × 10-4

Question 10

The reaction below has a Kc value of 1.0 × 1012.What is the value of Kp for this reaction at 200 K?
2 SO2(g) + O2(g) ⇌ 2 SO3(g)

Accepted Answer

A)   6.1 × 10-14
B)   1.0 × 1012
C)   1.6 × 10-11
D)   1.6 × 1013
E)   6.1 × 1010

Question 11

For the following reaction of N2O4,the equilibrium constant is 0.593 at a particular temperature. N2O4(g) ⇌ 2 NO2(g) 
If the initial concentration of N2O4 is 0.880M,what are the equilibrium concentrations?

Accepted Answer

A)   [N2O4] = 0.705M, [NO2] = 0.350M
B)   [N2O4] = 0.678M, [NO2] = 0.404M
C)   [N2O4] = 0.332M, [NO2] = 1.094M
D)   [N2O4] = 0.586M, [NO2] = 0.588M
E)   [N2O4] = 0.000M, [NO2] = 1.760M

Question 12

Consider the following reaction at equilibrium.What effect will reducing the volume of the reaction mixture have on the system?
Xe(g) + 2 F2(g) → XeF4(g)

Accepted Answer

A)   The reaction will shift to the left in the direction of reactants.
B)   The equilibrium constant will increase.
C)   No effect will be observed.
D)   The reaction will shift to the right in the direction of products.
E)   The equilibrium constant will decrease.

Question 13

In which of the following reactions will Kc = Kp?

Accepted Answer

A)   H2(g)  + I2(g)  ⇌ 2 HI(g) 
B)   CH4(g)  + H2O(g)  ⇌ CO(g)  + 3 H2(g) 
C)   N2O4(g)  ⇌ 2NO2(g) 
D)   CO(g)  + 2 H2(g)  ⇌ CH3OH(g) 
E)   N2(g)  + 3 Cl2(g)  ⇌ 2 NCl3(g)

Question 14

The reaction below has a Kp value of 3.3 × 10-5.What is the value of Kc for this reaction at 700 K?
2 SO3(g) ⇌ 2 SO2(g) + O2(g)

Accepted Answer

A)   5.7 × 10-7
B)   1.7 × 106
C)   3.3 × 10-5
D)   3.0 × 104
E)   1.9 × 10-3

Question 15

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [C3H8]= 0.15 M,[O2] = 0.35 M,[CO2] = 1.3 M,[H2O] = 2.8 M C3H8(g) + 5 O2(g) ⇌ 3 CO2(g) + 4 H2O(g)

Accepted Answer

A)   1.7 × 105
B)   3.2 × 10-6
C)   6.7 × 103
D)   7.4 × 102
E)   6.1.9 × 10-4

Question 16

Consider the following reaction at equilibrium.What effect will reducing the pressure of the reaction mixture have on the system?
Xe(g) + 2 F2(g) → XeF4(g)

Accepted Answer

A)   The reaction will shift to the left in the direction of reactants.
B)   The equilibrium constant will increase.
C)   No effect will be observed.
D)   The reaction will shift to the right in the direction of products.
E)   The equilibrium constant will decrease.

Question 17

Why aren't solids or liquids included in an equilibrium expression?

Accepted Answer

The equilibrium constant relates differe...

Question 18

Give the direction of the reaction,if K ≈ 1.

Accepted Answer

A)   The forward reaction is favored.
B)   The reverse reaction is favored.
C)   Neither direction is favored.
D)   If the temperature is raised, then the forward reaction is favored.
E)   If the temperature is raised, then the reverse reaction is favored.

Question 19

Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(NOCl) eq = 0.22 atm,P(NO) eq = 0.10 atm,P(Cl2) eq = 0.20 atm. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g)

Accepted Answer

A)   1.0
B)   24
C)   4.1 × 102
D)   4.1 × 10-2
E)   0.97

Question 20

In which of the following reactions will Kc = Kp?

Accepted Answer

A)   4 NH3(g)  + 3 O2(g)  ⇌ 2 N2(g)  + 6 H2O(g) 
B)   SO3(g)  + NO(g)  ⇌ SO2(g)  + NO2(g) 
C)   2 N2(g)  + O2(g)  ⇌ 2 N2O(g) 
D)   2 SO2(g)  + O2(g)  ⇌ 2 SO3(g) 
E)   None of the above reactions have Kc = Kp.

Exam 16: Chemical Equilibrium

In a reaction mixture containing only reactants,what is the value of Q?

Correct AnswerverifiedShow Answer

Consider the following reaction at equilibrium.What effect will reducing the pressure of the reaction mixture have on the system? Xe(g) + 2 F2(g) → XeF4(g)

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Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(NOCl) eq = 0.22 atm,P(NO) eq = 0.10 atm,P(Cl2) eq = 0.20 atm. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g)

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What is △n for the following equation in relating Kc to Kp? P4(s) + 5 O2(g) ⇌ P4O10(s)

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Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [C3H8]= 0.15 M,[O2] = 0.35 M,[CO2] = 1.3 M,[H2O] = 2.8 M C3H8(g) + 5 O2(g) ⇌ 3 CO2(g) + 4 H2O(g)

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Consider the following reaction at equilibrium.What effect will reducing the volume of the reaction mixture have on the system? Xe(g) + 2 F2(g) → XeF4(g)

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The reaction below has a Kc value of 3.64 × 10-3.What is the value of Kp for this reaction at 25°C? 2 NaN3(s) ⇌ 2 Na(s) + 3 N2(g)

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Consider the following reaction at equilibrium.What effect will raising the pressure of the system from 5 atm to 8 atm? 2 NH3(g) ⇌ N2(g) + 3 H2(g)

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Give the direction of the reaction,if K ≈ 1.

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The reaction below has a Kp value of 3.3 × 10-5.What is the value of Kc for this reaction at 700 K? 2 SO3(g) ⇌ 2 SO2(g) + O2(g)

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For the following reaction of N2O4,the equilibrium constant is 0.593 at a particular temperature. N2O4(g) ⇌ 2 NO2(g) If the initial concentration of N2O4 is 0.880M,what are the equilibrium concentrations?

Correct AnswerverifiedShow Answer

Consider the following reaction at equilibrium.What effect will reducing the pressure have on the system? C3H8(g) + 5 O2(g) ⇌ 3 CO2(g) + 4 H2O(l) ΔH° = -2220 kJ

Correct AnswerverifiedShow Answer

In which of the following reactions will Kc = Kp?

Correct AnswerverifiedShow Answer

Why aren't solids or liquids included in an equilibrium expression?

Correct AnswerverifiedThe equilibrium constant relates differe...View AnswerShow Answer

Consider the following reaction at equilibrium.What effect will adding more SO3 have on the system? SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)

Correct AnswerverifiedShow Answer

Consider the following reaction: Xe(g) + 2 F2(g) → XeF4(g) A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F2.If the equilibrium pressure of Xe is 0.34 atm,find the equilibrium constant (Kp) for the reaction.

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In which of the following reactions will Kc = Kp?

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The reaction below has a Kc value of 1.0 × 1012.What is the value of Kp for this reaction at 200 K? 2 SO2(g) + O2(g) ⇌ 2 SO3(g)

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The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. 2 SO2(g) + O2(g) ⇌ 2 SO3(g) Kc = 1.7 × 106 SO3(g) ⇌ 1/2 O2(g) + SO2(g) Kc = ?

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How is the reaction quotient different from an equilibrium constant for a given reaction?

Correct AnswerverifiedThe expression for both are identical.Ho...View AnswerShow Answer

Correct Answer
verified

Consider the following reaction at equilibrium.What effect will reducing the pressure of the reaction mixture have on the system? Xe(g) + 2 F₂(g) → XeF₄(g)

Correct Answer
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Determine the value of K_p for the following reaction if the equilibrium concentrations are as follows: P(NOCl) _eq = 0.22 atm,P(NO) _eq = 0.10 atm,P(Cl₂) _eq = 0.20 atm. 2 NOCl(g) ⇌ 2 NO(g) + Cl₂(g)

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What is △n for the following equation in relating K_c to K_p? P₄(s) + 5 O₂(g) ⇌ P₄O₁₀(s)

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Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [C₃H₈]= 0.15 M,[O₂] = 0.35 M,[CO₂] = 1.3 M,[H₂O] = 2.8 M C₃H₈(g) + 5 O₂(g) ⇌ 3 CO₂(g) + 4 H₂O(g)

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Consider the following reaction at equilibrium.What effect will reducing the volume of the reaction mixture have on the system? Xe(g) + 2 F₂(g) → XeF₄(g)

Correct Answer
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The reaction below has a K_c value of 3.64 × 10^-3.What is the value of K_p for this reaction at 25°C? 2 NaN₃(s) ⇌ 2 Na(s) + 3 N₂(g)

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verified

Consider the following reaction at equilibrium.What effect will raising the pressure of the system from 5 atm to 8 atm? 2 NH₃(g) ⇌ N₂(g) + 3 H₂(g)

Correct Answer
verified

Correct Answer
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The reaction below has a K_p value of 3.3 × 10^-5.What is the value of K_c for this reaction at 700 K? 2 SO₃(g) ⇌ 2 SO₂(g) + O₂(g)

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For the following reaction of N₂O₄,the equilibrium constant is 0.593 at a particular temperature. N₂O₄(g) ⇌ 2 NO₂(g) If the initial concentration of N₂O₄ is 0.880M,what are the equilibrium concentrations?

Correct Answer
verified

Consider the following reaction at equilibrium.What effect will reducing the pressure have on the system? C₃H₈(g) + 5 O₂(g) ⇌ 3 CO₂(g) + 4 H₂O(l) ΔH° = -2220 kJ

Correct Answer
verified

In which of the following reactions will K_c = K_p?

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Correct Answer
verified
The equilibrium constant relates differe...
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Consider the following reaction at equilibrium.What effect will adding more SO₃ have on the system? SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g)

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Consider the following reaction: Xe(g) + 2 F₂(g) → XeF₄(g) A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F₂.If the equilibrium pressure of Xe is 0.34 atm,find the equilibrium constant (K_p) for the reaction.

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verified

In which of the following reactions will K_c = K_p?

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The reaction below has a K_c value of 1.0 × 10¹².What is the value of K_p for this reaction at 200 K? 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g)

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The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) K_c = 1.7 × 10⁶ SO₃(g) ⇌ 1/2 O₂(g) + SO₂(g) K_c = ?

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Correct Answer
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The expression for both are identical.Ho...
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