Question 1

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 × 10-4F) A) and C)
G) C) and D)

Question 2

An equilibrium mixture of CO,O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0100 M O2.At this temperature,Kc equals 1.4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g) .
What is the equilibrium concentration of CO?

Accepted Answer

A)   7.1 × 10-7 M
B)   8.4 × 10-4 M
C)   1.4 × 10-2 M
D)   1.2 × 10-1 ME) A) and C)
F) A) and B)

Question 3

Which of the following statements is TRUE?

Accepted Answer

A)   Reaction quotient is the concentration of the products raised to the stoichiometric coefficients divided by the concentration of the reactants raised to their stoichiometric coefficients, measured at any point in the reaction.
B)   Reaction quotient is the concentration of the reactants raised to the stoichiometric coefficients divided by the concentration of the products raised to their stoichiometric coefficients, measured at any point in the reaction.
C)   Reaction quotient is the concentration of the products raised to the stoichiometric coefficients divided by the concentration of the reactants raised to their stoichiometric coefficients, measured at equilibrium.
D)   Reaction quotient is the concentration of the reactants raised to the stoichiometric coefficients divided by the concentration of the products raised to their stoichiometric coefficients, measured at equilibrium.
E)   Reaction quotient is the concentration of the products raised to the stoichiometric coefficients divided by the concentration of the reactants raised to their stoichiometric coefficients, at the point both are equal.F) A) and D)
G) A) and C)

Question 4

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 = 0.11 atm. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g)

Accepted Answer

A)   1.8
B)   44
C)   2.3 × 102
D)   2.3 × 10-2
E)   0.53F) A) and D)
G) A) and E)

Question 5

The equilibrium constant,Kp,equals 3.40 for the isomerization reaction: cis-2-butene ⇌ trans-2-butene.
If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene,what is the equilibrium pressure of each gas?

Accepted Answer

A)   P(cis-2-butene)  = 0.0426 atm and P(trans-2-butene)  = 0.145 atm
B)   P(cis-2-butene)  = 0.0471 atm and P(trans-2-butene)  = 0.160 atm
C)   P(cis-2-butene)  = 0.0735 atm and P(trans-2-butene)  = 0.250 atm
D)   P(cis-2-butene)  = 0.0898 atm and P(trans-2-butene)  = 0.305 atmE) C) and D)
F) B) and D)

Question 6

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 M,[Br2]eq = 0.39 M,[HBr]eq = 1.6 M. H2(g) + Br2(g) ⇌ 2 HBr(g)

Accepted Answer

A)   2.1 × 10-2
B)   29
C)   47
D)   3.4 × 10-2
E)   8.7 × 10-2F) C) and D)
G) B) and C)

Question 7

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

Question 8

Cyclohexane,C6H12,undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane,CH3C5H9, according to the equation: C6H12 ⇌ CH3C5H9
If Kc = 0.143 at 25°C for this reaction,find the equilibrium concentrations of C6H12 and CH3C5H9 if the initial concentrations are 0.200 M and 0.075 M,respectively.

Accepted Answer

A)   [C6H12] = 0.041 M, [CH3C5H9] = 0.041 M
B)   [C6H12] = 0.159 M, [CH3C5H9] = 0.116 M
C)   [C6H12] = 0.241 M, [CH3C5H9] = 0.034 M
D)   [C6H12] = 0.253 M, [CH3C5H9] = 0.022 ME) C) and D)
F) B) and C)

Question 9

Define Le Chatelier's Principle.

Accepted Answer

Le Chatelier's Principle state...

Question 10

Consider the following reaction at equilibrium.What effect will decreasing the temperature have on the system? CO2(g) + 2 H2O(l) ⇌ CH4(g) + 2 O2(g) ΔH° = +890 kJ

Accepted Answer

A)   The reaction will shift to the left in the direction of reactants.
B)   The equilibrium constant will decrease.
C)   The equilibrium constant will increase.
D)   The reaction will shift to the right in the direction of products.
E)   No effect will be observed.F) B) and D)
G) None of the above

Question 11

Explain dynamic equilibrium.Use the generic reaction A(g)⇌ B(g)to explain.

Accepted Answer

In this reaction,dynamic equilibrium mea...

Question 12

The reaction below has a Kp value of 41.What is the value of Kc for this reaction at 400 K? N2(g) + 3 H2(g) ⇌ 2 NH3(g)

Accepted Answer

A)   3.8 × 10-2
B)   4.4 × 104
C)   26
D)   2.3 × 10-5
E)   41F) B) and C)
G) C) and D)

Question 13

Calculate P [NO]eq,if P [NOCl]eq = 0.33 atm,P [Cl2]eq = 0.50 atm,and Kp = 1.9 × 10-2. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g)

Accepted Answer

A)   1.7 atm
B)   0.0042 atm
C)   0.30 atm
D)   0.064 atm
E)   0.087 atmF) A) and C)
G) A) and D)

Question 14

Express the equilibrium constant for the following reaction. 4 CH3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)

Accepted Answer

A)   K = 3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)  
A)   K =   
B)   K =      
C)   K =      
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
B)   K =   3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)  
A)   K =   
B)   K =      
C)   K =      
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
C)   K =   3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)  
A)   K =   
B)   K =      
C)   K =      
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
D)   K = 3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)  
A)   K =   
B)   K =      
C)   K =      
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
E)   K = 3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)  
A)   K =   
B)   K =      
C)   K =      
D)   K =   
E)   K =  " class="answers-bank-image d-inline" rel="preload" >F) A) and C)
G) A) and D)

Question 15

Why is an equilibrium constant unitless?

Accepted Answer

Each concentration or pressure for a rea...

Question 16

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. A(g) + B(g) ⇌ AB(g) Kc = 0.24
AB(g) + A(g) ⇌ A2B(g) Kc = 3.8
2 A(g) + B(g) ⇌ A2B(g) Kc = ?

Accepted Answer

A)   4.0
B)   0.91
C)   3.6
D)   16
E)   0.063F) C) and E)
G) C) and D)

Question 17

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 1.5 M,[H2]eq = 1.1 M,[NH3]eq = 0.47 M. N2(g) + 3 H2(g) ⇌ 2 NH3(g)

Accepted Answer

A)   3.5
B)   0.28
C)   9.1
D)   0.11
E)   0.78F) C) and D)
G) A) and D)

Question 18

Express the equilibrium constant for the following reaction. 2 P4(s) + 10 O2(g) ⇌ 2 P4O10(s)

Accepted Answer

A)   K = 4(s) + 10 O2(g) ⇌ 2 P4O10(s)  
A)   K =   
B)   K =   
C)   K =   
D)   K = [O2]10 
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
B)   K = 4(s) + 10 O2(g) ⇌ 2 P4O10(s)  
A)   K =   
B)   K =   
C)   K =   
D)   K = [O2]10 
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
C)   K = 4(s) + 10 O2(g) ⇌ 2 P4O10(s)  
A)   K =   
B)   K =   
C)   K =   
D)   K = [O2]10 
E)   K =  " class="answers-bank-image d-inline" rel="preload" >
D)   K = [O2]10
E)   K = 4(s) + 10 O2(g) ⇌ 2 P4O10(s)  
A)   K =   
B)   K =   
C)   K =   
D)   K = [O2]10 
E)   K =  " class="answers-bank-image d-inline" rel="preload" >F) C) and D)
G) D) and E)

Question 19

Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)

Accepted Answer

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

Question 20

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. N2O4(g) ⇌ 2 NO2(g) Kc = 1.46
3 N2O4(g) ⇌ 6 NO2(g) Kc = ?

Accepted Answer

A)   1.46
B)   0.322
C)   3.11
D)   1.13
E)   5.40F) A) and C)
G) None of the above

Exam 15: Chemical Equilibrium

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. A(g) + B(g) ⇌ AB(g) Kc = 0.24 AB(g) + A(g) ⇌ A₂B(g) K_c = 3.8 2 A(g) + B(g) ⇌ A₂B(g) K_c = ?

Correct Answer
verified

Calculate P [NO]_eq,if P [NOCl]_eq = 0.33 atm,P [Cl₂]_eq = 0.50 atm,and K_p = 1.9 × 10^-2. 2 NOCl(g) ⇌ 2 NO(g) + Cl₂(g)

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
verified

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [N₂]_eq = 1.5 M,[H₂]_eq = 1.1 M,[NH₃]_eq = 0.47 M. N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)

Correct Answer
verified

Express the equilibrium constant for the following reaction. 4 CH₃Cl(g) + 2 Cl₂(g) ⇔ 4 CH₂Cl₂(g) + 2 H₂(g)

Correct Answer
verified

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 M,[Br₂]_eq = 0.39 M,[HBr]_eq = 1.6 M. H₂(g) + Br₂(g) ⇌ 2 HBr(g)

Correct Answer
verified

Why is an equilibrium constant unitless?

Correct Answer
verified
Each concentration or pressure for a rea...
View Answer

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 = ?

Correct Answer
verified

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 = 0.11 atm. 2 NOCl(g) ⇌ 2 NO(g) + Cl₂(g)

Correct Answer
verified

Express the equilibrium constant for the following reaction. 2 P₄(s) + 10 O₂(g) ⇌ 2 P₄O₁₀(s)

Correct Answer
verified

Which of the following statements is TRUE?

Correct Answer
verified

The equilibrium constant,K_p,equals 3.40 for the isomerization reaction: cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene,what is the equilibrium pressure of each gas?

Correct Answer
verified

Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system? 2 H₂S(g) + 3 O₂(g) ⇌ 2 H₂O(g) + 2 SO₂(g)

Correct Answer
verified

Define Le Chatelier's Principle.

Correct Answer
verified
Le Chatelier's Principle state...
View Answer

The reaction below has a K_p value of 41.What is the value of K_c for this reaction at 400 K? N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)

Correct Answer
verified

Correct Answer
verified

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. N₂O₄(g) ⇌ 2 NO₂(g) K_c = 1.46 3 N₂O₄(g) ⇌ 6 NO₂(g) K_c = ?

Correct Answer
verified

Explain dynamic equilibrium.Use the generic reaction A(g)⇌ B(g)to explain.

Correct Answer
verified
In this reaction,dynamic equilibrium mea...
View Answer

Consider the following reaction at equilibrium.What effect will decreasing the temperature have on the system? CO₂(g) + 2 H₂O(l) ⇌ CH₄(g) + 2 O₂(g) ΔH° = +890 kJ

Correct Answer
verified

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0100 M O₂.At this temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g) + O₂(g) ⇌ 2 CO₂(g) . What is the equilibrium concentration of CO?

Correct Answer
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Exam 15: Chemical Equilibrium

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. A(g) + B(g) ⇌ AB(g) Kc = 0.24 AB(g) + A(g) ⇌ A2B(g) Kc = 3.8 2 A(g) + B(g) ⇌ A2B(g) Kc = ?

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Calculate P [NO]eq,if P [NOCl]eq = 0.33 atm,P [Cl2]eq = 0.50 atm,and Kp = 1.9 × 10-2. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g)

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)

Correct AnswerverifiedShow Answer

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 1.5 M,[H2]eq = 1.1 M,[NH3]eq = 0.47 M. N2(g) + 3 H2(g) ⇌ 2 NH3(g)

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Express the equilibrium constant for the following reaction. 4 CH3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)

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Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 M,[Br2]eq = 0.39 M,[HBr]eq = 1.6 M. H2(g) + Br2(g) ⇌ 2 HBr(g)

Correct AnswerverifiedShow Answer

Why is an equilibrium constant unitless?

Correct AnswerverifiedEach concentration or pressure for a rea...View AnswerShow Answer

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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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 = 0.11 atm. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g)

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Express the equilibrium constant for the following reaction. 2 P4(s) + 10 O2(g) ⇌ 2 P4O10(s)

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Which of the following statements is TRUE?

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The equilibrium constant,Kp,equals 3.40 for the isomerization reaction: cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene,what is the equilibrium pressure of each gas?

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Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)

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Define Le Chatelier's Principle.

Correct AnswerverifiedLe Chatelier's Principle state...View AnswerShow Answer

The reaction below has a Kp value of 41.What is the value of Kc for this reaction at 400 K? N2(g) + 3 H2(g) ⇌ 2 NH3(g)

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Correct AnswerverifiedShow Answer

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. N2O4(g) ⇌ 2 NO2(g) Kc = 1.46 3 N2O4(g) ⇌ 6 NO2(g) Kc = ?

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Explain dynamic equilibrium.Use the generic reaction A(g)⇌ B(g)to explain.

Correct AnswerverifiedIn this reaction,dynamic equilibrium mea...View AnswerShow Answer

Consider the following reaction at equilibrium.What effect will decreasing the temperature have on the system? CO2(g) + 2 H2O(l) ⇌ CH4(g) + 2 O2(g) ΔH° = +890 kJ

Correct AnswerverifiedShow Answer

An equilibrium mixture of CO,O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0100 M O2.At this temperature,Kc equals 1.4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g) . What is the equilibrium concentration of CO?

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The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. A(g) + B(g) ⇌ AB(g) Kc = 0.24 AB(g) + A(g) ⇌ A₂B(g) K_c = 3.8 2 A(g) + B(g) ⇌ A₂B(g) K_c = ?

Correct Answer
verified

Calculate P [NO]_eq,if P [NOCl]_eq = 0.33 atm,P [Cl₂]_eq = 0.50 atm,and K_p = 1.9 × 10^-2. 2 NOCl(g) ⇌ 2 NO(g) + Cl₂(g)

Correct Answer
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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_c for the following reaction if the equilibrium concentrations are as follows: [N₂]_eq = 1.5 M,[H₂]_eq = 1.1 M,[NH₃]_eq = 0.47 M. N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)

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Express the equilibrium constant for the following reaction. 4 CH₃Cl(g) + 2 Cl₂(g) ⇔ 4 CH₂Cl₂(g) + 2 H₂(g)

Correct Answer
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Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 M,[Br₂]_eq = 0.39 M,[HBr]_eq = 1.6 M. H₂(g) + Br₂(g) ⇌ 2 HBr(g)

Correct Answer
verified

Correct Answer
verified
Each concentration or pressure for a rea...
View Answer

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 = ?

Correct Answer
verified

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 = 0.11 atm. 2 NOCl(g) ⇌ 2 NO(g) + Cl₂(g)

Correct Answer
verified

Express the equilibrium constant for the following reaction. 2 P₄(s) + 10 O₂(g) ⇌ 2 P₄O₁₀(s)

Correct Answer
verified

Correct Answer
verified

The equilibrium constant,K_p,equals 3.40 for the isomerization reaction: cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene,what is the equilibrium pressure of each gas?

Correct Answer
verified

Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system? 2 H₂S(g) + 3 O₂(g) ⇌ 2 H₂O(g) + 2 SO₂(g)

Correct Answer
verified

Correct Answer
verified
Le Chatelier's Principle state...
View Answer

The reaction below has a K_p value of 41.What is the value of K_c for this reaction at 400 K? N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)

Correct Answer
verified

Correct Answer
verified

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. N₂O₄(g) ⇌ 2 NO₂(g) K_c = 1.46 3 N₂O₄(g) ⇌ 6 NO₂(g) K_c = ?

Correct Answer
verified

Correct Answer
verified
In this reaction,dynamic equilibrium mea...
View Answer

Consider the following reaction at equilibrium.What effect will decreasing the temperature have on the system? CO₂(g) + 2 H₂O(l) ⇌ CH₄(g) + 2 O₂(g) ΔH° = +890 kJ

Correct Answer
verified

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0100 M O₂.At this temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g) + O₂(g) ⇌ 2 CO₂(g) . What is the equilibrium concentration of CO?

Correct Answer
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