Question 1

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of NO2(g) .
N2O4(g) ⇌ 2 NO2(g)  Kc = 0.21
[N2O4]eq = 0.039 M

Accepted Answer

A)  1.22 M
B)  9.0 × 10-2 M
C)  7.8 × 10-2 M
D)  8.2 × 10-3 M
E)  11 MF) A) and E)
G) None of the above

Question 2

Consider the following reaction at equilibrium.What effect will adding more H2S 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 left.
B)  No change will be observed.
C)  The equilibrium constant will decrease.
D)  The equilibrium constant will increase.
E)  The reaction will shift in the direction of products.F) B) and C)
G) None of the above

Question 3

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of CO.
CO(g) + 2 H2(g) ⇌ CH3OH(l) Kp = 2.25 × 104
P(H2) eq = 0.52 atm

Accepted Answer

A)  8.3 × 104 atm
B)  1.2 × 10-5 atm
C)  6.25 × 10-3 atm
D)  8.5 × 10-5 atm
E)  1.6 × 10-4 atmF) B) and E)
G) D) and E)

Question 4

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.F) D) and E)
G) A) and E)

Question 5

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 × 10-3F) All of the above
G) C) and D)

Question 6

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant.
2 HD(g) ⇌ H2(g) + D2(g) Kc = 0.28
2 H2(g) + 2 D2(g) ⇌ 4 HD(g) Kc = ?

Accepted Answer

A)  7.8 × 10-2
B)  3.6
C)  0.53
D)  13
E)  1.9F) B) and D)
G) D) and E)

Question 7

Match the following.
-K ≈ 1

Accepted Answer

A)  Reaction will favor formation of reactants.
B)  Reaction does not strongly favor reactants or products.
C)  Reaction favors formation of more products.
D)  Reaction has a larger amount of products than reactants.
E)  Reaction is at equilibrium.F) A) and B)
G) A) and C)

Question 8

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)  0.63F) B) and D)
G) A) and C)

Question 9

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [HCl]eq = 0.13 M,[HI]eq = 5.6 × 10-16 M,[Cl2]eq = 0.0019 M.
2 HCl(g) + I2(s) ⇌ 2 HI(g) + Cl2(g)

Accepted Answer

A)  8.2 × 10-18
B)  2.9 × 1031
C)  1.2 × 1017
D)  1.4 × 10-19
E)  3.5 × 10-32F) A) and B)
G) All of the above

Question 10

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) B) and D)
G) B) and C)

Question 11

Consider the following reaction and its equilibrium constant:
4 CuO(s) + CH4(g) ⇌ CO2(g) + 4 Cu(s) + 2 H2O(g) Kc = 1.10
A reaction mixture contains 0.22 M CH4,0.67 M CO2 and 1.3 M H2O.Which of the following statements is true concerning this system?

Accepted Answer

A)  The reaction will shift in the direction of products.
B)  The equilibrium constant will increase.
C)  The reaction quotient will increase.
D)  The reaction will shift in the direction of reactants.
E)  The system is at equilibrium.F) C) and D)
G) None of the above

Question 12

Express the equilibrium constant for the following reaction.
P4(s) + 5 O2(g) ⇌ P4O10(s)

Accepted Answer

A)  K = 4(s) + 5 O2(g) ⇌ P4O10(s)  
A)  K =   
B)  K =   
C)  K = [O2]-5 
D)  K = [O2]5 
E)  K =  " class="answers-bank-image d-inline" rel="preload" >
B)  K = 4(s) + 5 O2(g) ⇌ P4O10(s)  
A)  K =   
B)  K =   
C)  K = [O2]-5 
D)  K = [O2]5 
E)  K =  " class="answers-bank-image d-inline" rel="preload" >
C)  K = [O2]-5
D)  K = [O2]5
E)  K = 4(s) + 5 O2(g) ⇌ P4O10(s)  
A)  K =   
B)  K =   
C)  K = [O2]-5 
D)  K = [O2]5 
E)  K =  " class="answers-bank-image d-inline" rel="preload" >F) C) and E)
G) B) and C)

Question 13

Consider the following reaction and its equilibrium constant:
I2(g) + Br2(g) ⇌ 2 IBr(g) Kc = 1.1 × 102
A reaction mixture contains 0.41 M I2,0.27 M Br2 and 3.5 M IBr.Which of the following statements is true concerning this system?

Accepted Answer

A)  The reaction will shift in the direction of products.
B)  The reaction will shift in the direction of reactants.
C)  The reaction quotient will decrease.
D)  The equilibrium constant will increase.
E)  The system is at equilibrium.F) C) and D)
G) B) and E)

Question 14

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.F) B) and E)
G) A) and B)

Question 15

Consider the following reaction:
CO2(g) + C(graphite) ⇌ 2 CO(g) 
A reaction mixture initially contains 0.56 atm CO2 and 0.32 atm CO.Determine the equilibrium pressure of CO if Kp for the reaction at this temperature is 2.25.

Accepted Answer

A)  0.83 atm
B)  0.31 atm
C)  0.26 atm
D)  0.58 atm
E)  0.42 atmF) All of the above
G) D) and E)

Question 16

Can the Kp and Kc for a reaction ever have the same value? Why or why not?

Accepted Answer

K_p and K_c are equal for reaction...

Question 17

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 = 0.081 atm.
2 NOCl(g) ? 2 NO(g) + Cl2(g)

Accepted Answer

A)  3.7 × 10-2
B)  60.
C)  27
D)  1.7 × 10-2
E)  1.8 × 10-3F) C) and D)
G) C) and E)

Question 18

Express the equilibrium constant for the following reaction.
2 Na(s) + 2 H2O(l) ⇌ 2 NaOH(aq) + H2(g)

Accepted Answer

A)  K = 2O(l) ⇌ 2 NaOH(aq) + H2(g)  
A)  K =   
B)  K = [H2][NaOH]-2 
C)  K =   
D)  K = [H2][NaOH]2 
E)  K =  " class="answers-bank-image d-inline" rel="preload" >
B)  K = [H2][NaOH]-2
C)  K = 2O(l) ⇌ 2 NaOH(aq) + H2(g)  
A)  K =   
B)  K = [H2][NaOH]-2 
C)  K =   
D)  K = [H2][NaOH]2 
E)  K =  " class="answers-bank-image d-inline" rel="preload" >
D)  K = [H2][NaOH]2
E)  K = 2O(l) ⇌ 2 NaOH(aq) + H2(g)  
A)  K =   
B)  K = [H2][NaOH]-2 
C)  K =   
D)  K = [H2][NaOH]2 
E)  K =  " class="answers-bank-image d-inline" rel="preload" >F) A) and E)
G) A) and B)

Question 19

The equilibrium constant is equal to 5.00 at 1300 K for the reaction:
2 SO2(g) + O2(g) ⇌ 2 SO3(g) .
If initial concentrations are [SO2] = 6.00 M,[O2] = 0.45 M,and [SO3] = 9.00 M,the system is

Accepted Answer

A)  at equilibrium.
B)  not at equilibrium and will remain in an unequilibrated state.
C)  not at equilibrium and will shift to the left to achieve an equilibrium state.
D)  not at equilibrium and will shift to the right to achieve an equilibrium state.E) A) and B)
F) None of the above

Question 20

Which statement is true for the following reaction at equilibrium at 25 C?
H2(g) + Br2(g) ⇌ HBr(g) ;K = 1.9 × 1019

Accepted Answer

A)  Concentration of HBr is high.
B)  Concentration of H2 and Br2 are high.
C)  The rate of the reaction is very slow.
D)  The reverse reaction does not happen.E) B) and C)
F) A) and D)

Exam 14: Chemical Equilibrium

Express the equilibrium constant for the following reaction. P4(s) + 5 O2(g) ⇌ P4O10(s)

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Which statement is true for the following reaction at equilibrium at 25 C? H2(g) + Br2(g) ⇌ HBr(g) ;K = 1.9 × 1019

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Consider the following reaction and its equilibrium constant: 4 CuO(s) + CH4(g) ⇌ CO2(g) + 4 Cu(s) + 2 H2O(g) Kc = 1.10 A reaction mixture contains 0.22 M CH4,0.67 M CO2 and 1.3 M H2O.Which of the following statements is true concerning this system?

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Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [HCl]eq = 0.13 M,[HI]eq = 5.6 × 10-16 M,[Cl2]eq = 0.0019 M. 2 HCl(g) + I2(s) ⇌ 2 HI(g) + Cl2(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 = 0.081 atm. 2 NOCl(g) ? 2 NO(g) + Cl2(g)

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Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of NO2(g) . N2O4(g) ⇌ 2 NO2(g) Kc = 0.21 [N2O4]eq = 0.039 M

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Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of CO. CO(g) + 2 H2(g) ⇌ CH3OH(l) Kp = 2.25 × 104 P(H2) eq = 0.52 atm

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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)

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Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ⇌ 2 IBr(g) Kc = 1.1 × 102 A reaction mixture contains 0.41 M I2,0.27 M Br2 and 3.5 M IBr.Which of the following statements is true concerning this system?

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The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO2(g) + O2(g) ⇌ 2 SO3(g) . If initial concentrations are [SO2] = 6.00 M,[O2] = 0.45 M,and [SO3] = 9.00 M,the system is

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The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. 2 HD(g) ⇌ H2(g) + D2(g) Kc = 0.28 2 H2(g) + 2 D2(g) ⇌ 4 HD(g) Kc = ?

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

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Match the following. -K ≈ 1

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

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Consider the following reaction: CO2(g) + C(graphite) ⇌ 2 CO(g) A reaction mixture initially contains 0.56 atm CO2 and 0.32 atm CO.Determine the equilibrium pressure of CO if Kp for the reaction at this temperature is 2.25.

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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) Kc = 3.8 2 A(g) + B(g) ⇌ A2B(g) Kc = ?

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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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Can the Kp and Kc for a reaction ever have the same value? Why or why not?

Correct AnswerverifiedKp and Kc are equal for reaction...View AnswerShow Answer

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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Express the equilibrium constant for the following reaction. 2 Na(s) + 2 H2O(l) ⇌ 2 NaOH(aq) + H2(g)

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Express the equilibrium constant for the following reaction. P₄(s) + 5 O₂(g) ⇌ P₄O₁₀(s)

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Which statement is true for the following reaction at equilibrium at 25 C? H2(g) + Br2(g) ⇌ HBr(g) ;K = 1.9 × 10¹⁹

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Consider the following reaction and its equilibrium constant: 4 CuO(s) + CH₄(g) ⇌ CO₂(g) + 4 Cu(s) + 2 H₂O(g) K_c = 1.10 A reaction mixture contains 0.22 M CH₄,0.67 M CO₂and 1.3 M H₂O.Which of the following statements is true concerning this system?

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Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [HCl]_eq = 0.13 M,[HI]_eq = 5.6 × 10^-16 M,[Cl₂]_eq = 0.0019 M. 2 HCl(g) + I₂(s) ⇌ 2 HI(g) + Cl₂(g)

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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 = 0.081 atm. 2 NOCl(g) ? 2 NO(g) + Cl₂₍g)

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Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of NO₂(g) . N₂O₄(g) ⇌ 2 NO₂(g) K_c = 0.21 [N₂O₄]_eq = 0.039 M

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Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of CO. CO(g) + 2 H₂(g) ⇌ CH₃OH(l) K_p = 2.25 × 10⁴ P(H₂) _eq = 0.52 atm

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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)

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Consider the following reaction and its equilibrium constant: I₂(g) + Br₂(g) ⇌ 2 IBr(g) K_c = 1.1 × 10² A reaction mixture contains 0.41 M I₂,0.27 M Br₂and 3.5 M IBr.Which of the following statements is true concerning this system?

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The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) . If initial concentrations are [SO₂] = 6.00 M,[O₂] = 0.45 M,and [SO₃] = 9.00 M,the system is

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The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. 2 HD(g) ⇌ H₂(g) + D₂(g) K_c = 0.28 2 H₂(g) + 2 D₂(g) ⇌ 4 HD(g) K_c = ?

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

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Consider the following reaction: CO₂(g) + C(graphite) ⇌ 2 CO(g) A reaction mixture initially contains 0.56 atm CO₂ and 0.32 atm CO.Determine the equilibrium pressure of CO if K_p for the reaction at this temperature is 2.25.

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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 = ?

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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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Can the K_p and K_c for a reaction ever have the same value? Why or why not?

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K_p and K_c are equal for reaction...
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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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Express the equilibrium constant for the following reaction. 2 Na(s) + 2 H₂O(l) ⇌ 2 NaOH(aq) + H₂(g)

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