Question 1

For which reaction will Kp = Kc?

Accepted Answer

A)  S(s) + O2(g) ⇌ SO2(g) 
B)  2 HgO(s) ⇌ Hg(l) + O2(g) 
C)  CaCO3(s) ⇌ CaO(s) + CO2(g) 
D)  H2CO3(s) ⇌ H2O(l) + CO2(g) 
E)  2 H2O(l) ⇌ 2 H2(g) + O2(g) F) B) and D)
G) None of the above

Question 2

The equilibrium constant for the reaction A(g) LB(g) is 102.A reaction mixture initially contains
[A] = 10.1 M and [B] = 0.0 M.Which statement is true at equilibrium?

Accepted Answer

A)  The reaction mixture contains [A] = 10.0 M and [B] = 0.10 M.
B)  The reaction mixture contains [A] = 0.10 M and [B] = 10.0 M.
C)  The reaction mixture contains [A] = 0.55 M and [B] = 0.55 M.
D)  The reaction mixture contains [A] = 1.0 M and [B] = 100.0 M.E) B) and D)
F) None of the above

Question 3

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

Accepted Answer

The equilibrium constant relates different concentrations of reactants and products to one another.Since the concentrations of liquids and solids are constant,their concentration(s)becomes part of the constant value of the equilibrium constant.

Question 4

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant.
H2(g) + Br2(g) ⇌ 2 HBr(g) Kc = 3.8 × 104
2 HBr(g) ⇌ H2(g) + Br2(g) Kc = ?

Accepted Answer

A)  1.9 × 104
B)  5.3 × 10-5
C)  2.6 × 10-5
D)  6.4 × 10-4
E)  1.6 × 103F) B) and D)
G) B) and E)

Question 5

At equilibrium in a 10.0 L vessel,there are 7.6 × 10-2 moles of SO2,8.6 × 10-2 moles of O2,and 8.2 × 10-2 moles of SO3.What is the equilibrium constant (Kc) for the reaction:
2SO2(g) + O2(g) ⇌ 2SO3(g)

Accepted Answer

A)  7.4 × 10-3
B)  12.5
C)  135
D)  13.5E) A) and C)
F) None of the above

Question 6

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 D)
G) D) and E)

Question 7

Kc is 1.67 × 1020 at 25°C for the formation of iron(III) oxalate complex ion:
Fe3+(aq) + 3 C2O42-(aq) ⇌ [Fe(C2O4) 3]3-(aq) .
If 0.0200 M Fe3+ is initially mixed with 1.00 M oxalate ion,what is the concentration of Fe3+ ion at equilibrium?

Accepted Answer

A)  1.44 × 10-22 M
B)  0.0100 M
C)  8.35 × 1019 M
D)  6.94 × 1021 ME) All of the above
F) A) and B)

Question 8

Consider the following reaction at equilibrium.What effect will adding water 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) C) and D)
G) A) and E)

Question 9

For the reaction: N2(g) + 2 O2(g) ⇌ 2 NO2(g) ,Kc = 8.3 × 10-10 at 25°C.What is the concentration of N2 gas at equilibrium when the concentration of NO2 is five times the concentration of O2 gas?

Accepted Answer

A)  3.3 × 10-11 M
B)  1.7 × 10-10 M
C)  6.0 × 109 M
D)  3.0 × 1010 ME) A) and D)
F) A) and C)

Question 10

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 E)
G) B) and C)

Question 11

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [PCl5]eq = 0.56 M,[PCl3]eq = 0.23 M,[Cl2]eq = 4.4 M.
PCl5(g) ⇌ PCl3(g) + Cl2(g)

Accepted Answer

A)  1.8
B)  0.93
C)  0.55
D)  1.1
E)  0.76F) C) and D)
G) A) and D)

Question 12

Express the equilibrium constant for the following reaction.
H2(g) + Br2(g) ⇌ 2 HBr(g)

Accepted Answer

A)  K = 2(g) + Br2(g) ⇌ 2 HBr(g)  
A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =  " class="answers-bank-image d-inline" rel="preload" >
B)  K = 2(g) + Br2(g) ⇌ 2 HBr(g)  
A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =  " class="answers-bank-image d-inline" rel="preload" >
C)  K = 2(g) + Br2(g) ⇌ 2 HBr(g)  
A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =  " class="answers-bank-image d-inline" rel="preload" >
D)  K = 2(g) + Br2(g) ⇌ 2 HBr(g)  
A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =  " class="answers-bank-image d-inline" rel="preload" >
E)  K = 2(g) + Br2(g) ⇌ 2 HBr(g)  
A)  K =   
B)  K =   
C)  K =   
D)  K =   
E)  K =  " class="answers-bank-image d-inline" rel="preload" >F) C) and D)
G) B) and E)

Question 13

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of SO3(g) .
2 SO2(g) + O2(g) ⇌ 2 SO3(g) Kc = 1.7 × 108
[SO2]eq = 0.0034 M [O2]eq = 0.0018 M

Accepted Answer

A)  1.9 M
B)  1.0 × 103 M
C)  0.53 M
D)  9.6 × 10-4 M
E)  0.73 MF) B) and E)
G) A) and D) A

Question 14

What will happen to the following exothermic reaction at equilibrium if the pressure is raised?
N2(g) + 3H2(g) ⇌ 2NH3(g)

Accepted Answer

A)  Less NH3 will be produced.
B)  More N2 and H2 will be produced.
C)  There will be no change in concentrations.
D)  More NH3 will be produced.E) All of the above
F) A) and D)

Question 15

Consider the following reaction at equilibrium.What effect will adding 1 atm of Ar to 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 D)
G) B) and C)

Question 16

Match the following.
-Q < K

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 17

Match the following.
-Q >> 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) C) and D)

Question 18

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of H2O(g) .
C2H4(g) + H2O(g) ⇌ C2H5OH(g) Kc = 9.0 × 103
[C2H4]eq = 0.015 M [C2H5OH]eq = 1.69 M

Accepted Answer

A)  9.9 × 10-7 M
B)  80.M
C)  1.0 M
D)  1.68 M
E)  0.013 MF) C) and D)
G) A) and B)

Question 19

The reaction below has a Kc value of 1.0 × 1012.What is the value of Kp for this reaction at 500 K?
2 SO2(g) + O2(g) ⇌ 2 SO3(g)

Accepted Answer

A)  4.2 × 10-11
B)  1.0 × 1012
C)  2.4 × 10-12
D)  4.1 × 1013
E)  2.4 × 1010F) A) and E)
G) A) and D)

Question 20

Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction:
PCl3(g) + Cl2(g) ⇌ PCl5(g) 
An equilibrium mixture at 450 K contains
PPCl3 = 0.124 atm,
PCl2 = 0.157 atm,and
PPCl5 = 1.30 atm.What is the value of Kp at this temperature?

Accepted Answer

A)  66.7
B)  1.50 × 10-2
C)  2.53 × 10-2
D)  1.02
E)  4.63F) B) and E)
G) A) and C) A

Exam 14: Chemical Equilibrium

For which reaction will K_p = K_c?

Correct Answer
verified

The equilibrium constant for the reaction A(g) LB(g) is 10².A reaction mixture initially contains [A] = 10.1 M and [B] = 0.0 M.Which statement is true at equilibrium?

Correct Answer
verified

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

Correct Answer
verified
The equilibrium constant relates different concentrations of reactants and products to one another.Since the concentrations of liquids and solids are constant,their concentration(s)becomes part of the constant value of the equilibrium constant.

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. H₂(g) + Br₂(g) ⇌ 2 HBr(g) K_c = 3.8 × 10⁴ 2 HBr(g) ⇌ H₂(g) + Br₂(g) K_c = ?

Correct Answer
verified

At equilibrium in a 10.0 L vessel,there are 7.6 × 10^-2 moles of SO₂,8.6 × 10^-2 moles of O₂,and 8.2 × 10^-2 moles of SO₃.What is the equilibrium constant (K_c)for the reaction: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)

Correct Answer
verified

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

K_c is 1.67 × 10²⁰ at 25°C for the formation of iron(III) oxalate complex ion: Fe³⁺(aq) + 3 C₂O₄^2-(aq) ⇌ [Fe(C₂O₄) ₃]^3-(aq) . If 0.0200 M Fe³⁺ is initially mixed with 1.00 M oxalate ion,what is the concentration of Fe³⁺ ion at equilibrium?

Correct Answer
verified

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

Correct Answer
verified

For the reaction: N₂(g) + 2 O₂(g) ⇌ 2 NO₂(g) ,K_c = 8.3 × 10^-10 at 25°C.What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is five times the concentration of O₂ gas?

Correct Answer
verified

Match the following. -K << 1

Correct Answer
verified

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [PCl₅]_eq = 0.56 M,[PCl₃]_eq = 0.23 M,[Cl₂]_eq = 4.4 M. PCl₅(g) ⇌ PCl₃(g) + Cl₂(g)

Correct Answer
verified

Express the equilibrium constant for the following reaction. H₂(g) + Br₂(g) ⇌ 2 HBr(g)

Correct Answer
verified

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of SO₃(g) . 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) K_c = 1.7 × 10⁸ [SO₂]_eq = 0.0034 M [O₂]_eq = 0.0018 M

Correct Answer
verified
A

What will happen to the following exothermic reaction at equilibrium if the pressure is raised? N₂(g) + 3H₂(g) ⇌ 2NH₃(g)

Correct Answer
verified

Consider the following reaction at equilibrium.What effect will adding 1 atm of Ar to the reaction mixture have on the system? 2 H₂S(g) + 3 O₂(g) ⇌ 2 H₂O(g) + 2 SO₂(g)

Correct Answer
verified

Match the following. -Q < K

Correct Answer
verified

Match the following. -Q >> 1

Correct Answer
verified

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of H₂O(g) . C₂H₄(g) + H₂O(g) ⇌ C₂H₅OH(g) K_c = 9.0 × 10³ [C₂H₄]_eq = 0.015 M [C₂H₅OH]_eq = 1.69 M

Correct Answer
verified

The reaction below has a K_c value of 1.0 × 10¹².What is the value of K_p for this reaction at 500 K? 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g)

Correct Answer
verified

Correct Answer
verified
A

Exam 14: Chemical Equilibrium

For which reaction will Kp = Kc?

Correct AnswerverifiedShow Answer

The equilibrium constant for the reaction A(g) LB(g) is 102.A reaction mixture initially contains [A] = 10.1 M and [B] = 0.0 M.Which statement is true at equilibrium?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedThe equilibrium constant relates different concentrations of reactants and products to one another.Since the concentrations of liquids and solids are constant,their concentration(s)becomes part of the constant value of the equilibrium constant.

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. H2(g) + Br2(g) ⇌ 2 HBr(g) Kc = 3.8 × 104 2 HBr(g) ⇌ H2(g) + Br2(g) Kc = ?

Correct AnswerverifiedShow Answer

At equilibrium in a 10.0 L vessel,there are 7.6 × 10-2 moles of SO2,8.6 × 10-2 moles of O2,and 8.2 × 10-2 moles of SO3.What is the equilibrium constant (Kc) for the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g)

Correct AnswerverifiedShow 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 = ?

Correct AnswerverifiedShow Answer

Kc is 1.67 × 1020 at 25°C for the formation of iron(III) oxalate complex ion: Fe3+(aq) + 3 C2O42-(aq) ⇌ [Fe(C2O4) 3]3-(aq) . If 0.0200 M Fe3+ is initially mixed with 1.00 M oxalate ion,what is the concentration of Fe3+ ion at equilibrium?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

For the reaction: N2(g) + 2 O2(g) ⇌ 2 NO2(g) ,Kc = 8.3 × 10-10 at 25°C.What is the concentration of N2 gas at equilibrium when the concentration of NO2 is five times the concentration of O2 gas?

Correct AnswerverifiedShow Answer

Match the following. -K << 1

Correct AnswerverifiedShow Answer

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [PCl5]eq = 0.56 M,[PCl3]eq = 0.23 M,[Cl2]eq = 4.4 M. PCl5(g) ⇌ PCl3(g) + Cl2(g)

Correct AnswerverifiedShow Answer

Express the equilibrium constant for the following reaction. H2(g) + Br2(g) ⇌ 2 HBr(g)

Correct AnswerverifiedShow Answer

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of SO3(g) . 2 SO2(g) + O2(g) ⇌ 2 SO3(g) Kc = 1.7 × 108 [SO2]eq = 0.0034 M [O2]eq = 0.0018 M

Correct AnswerverifiedA

What will happen to the following exothermic reaction at equilibrium if the pressure is raised? N2(g) + 3H2(g) ⇌ 2NH3(g)

Correct AnswerverifiedShow Answer

Consider the following reaction at equilibrium.What effect will adding 1 atm of Ar to the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)

Correct AnswerverifiedShow Answer

Match the following. -Q < K

Correct AnswerverifiedShow Answer

Match the following. -Q >> 1

Correct AnswerverifiedShow Answer

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of H2O(g) . C2H4(g) + H2O(g) ⇌ C2H5OH(g) Kc = 9.0 × 103 [C2H4]eq = 0.015 M [C2H5OH]eq = 1.69 M

Correct AnswerverifiedShow Answer

The reaction below has a Kc value of 1.0 × 1012.What is the value of Kp for this reaction at 500 K? 2 SO2(g) + O2(g) ⇌ 2 SO3(g)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedA

For which reaction will K_p = K_c?

Correct Answer
verified

The equilibrium constant for the reaction A(g) LB(g) is 10².A reaction mixture initially contains [A] = 10.1 M and [B] = 0.0 M.Which statement is true at equilibrium?

Correct Answer
verified

Correct Answer
verified
The equilibrium constant relates different concentrations of reactants and products to one another.Since the concentrations of liquids and solids are constant,their concentration(s)becomes part of the constant value of the equilibrium constant.

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. H₂(g) + Br₂(g) ⇌ 2 HBr(g) K_c = 3.8 × 10⁴ 2 HBr(g) ⇌ H₂(g) + Br₂(g) K_c = ?

Correct Answer
verified

At equilibrium in a 10.0 L vessel,there are 7.6 × 10^-2 moles of SO₂,8.6 × 10^-2 moles of O₂,and 8.2 × 10^-2 moles of SO₃.What is the equilibrium constant (K_c)for the reaction: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)

Correct Answer
verified

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

K_c is 1.67 × 10²⁰ at 25°C for the formation of iron(III) oxalate complex ion: Fe³⁺(aq) + 3 C₂O₄^2-(aq) ⇌ [Fe(C₂O₄) ₃]^3-(aq) . If 0.0200 M Fe³⁺ is initially mixed with 1.00 M oxalate ion,what is the concentration of Fe³⁺ ion at equilibrium?

Correct Answer
verified

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

Correct Answer
verified

For the reaction: N₂(g) + 2 O₂(g) ⇌ 2 NO₂(g) ,K_c = 8.3 × 10^-10 at 25°C.What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is five times the concentration of O₂ gas?

Correct Answer
verified

Correct Answer
verified

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [PCl₅]_eq = 0.56 M,[PCl₃]_eq = 0.23 M,[Cl₂]_eq = 4.4 M. PCl₅(g) ⇌ PCl₃(g) + Cl₂(g)

Correct Answer
verified

Express the equilibrium constant for the following reaction. H₂(g) + Br₂(g) ⇌ 2 HBr(g)

Correct Answer
verified

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of SO₃(g) . 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) K_c = 1.7 × 10⁸ [SO₂]_eq = 0.0034 M [O₂]_eq = 0.0018 M

Correct Answer
verified
A

What will happen to the following exothermic reaction at equilibrium if the pressure is raised? N₂(g) + 3H₂(g) ⇌ 2NH₃(g)

Correct Answer
verified

Consider the following reaction at equilibrium.What effect will adding 1 atm of Ar to 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

Correct Answer
verified

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of H₂O(g) . C₂H₄(g) + H₂O(g) ⇌ C₂H₅OH(g) K_c = 9.0 × 10³ [C₂H₄]_eq = 0.015 M [C₂H₅OH]_eq = 1.69 M

Correct Answer
verified

The reaction below has a K_c value of 1.0 × 10¹².What is the value of K_p for this reaction at 500 K? 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g)

Correct Answer
verified

Correct Answer
verified
A