Question 1

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. 
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 2

For the isomerization reaction:
Butane ⇌ isobutane
Kp equals 25 at 500°C.If the initial pressures of butane and isobutane are 20.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

Accepted Answer

A) P(butane)= 0.77 atm and P(isobutane)= 19.2 atm 
B) P(butane)= 0.80 atm and P(isobutane)= 20.atm 
C) P(butane)= 19.2 atm and P(isobutane)= 0.77 atm 
D) P(butane)= 20 atm and P(isobutane)= 0.80 atm 
A) P(butane)= 0.77 atm and P(isobutane)= 19.2 atm 
B) P(butane)= 0.80 atm and P(isobutane)= 20.atm 
C) P(butane)= 19.2 atm and P(isobutane)= 0.77 atm 
D) P(butane)= 20 atm and P(isobutane)= 0.80 atm

Question 3

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. 
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 4

Consider the following reaction and its equilibrium constant:
I2(g)⇌ 2I(g)Kp = 0.209
A reaction mixture contains 0.89 atm I2 and 1.77 atm I.Which of the following statements is true concerning this system?

Accepted Answer

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

Question 5

Express the equilibrium constant for the following reaction.
2 P(g)+ 3 Cl2(g)⇌ 2 PCl3(g)

Accepted Answer

A) K =   
B) K =   
C) K =   
D) K =   
E) K =   
A) K =   
B) K =   
C) K =   
D) K =   
E) K =

Question 6

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) 0.78 
A) 3.5 
B) 0.28 
C) 9.1 
D) 0.11 
E) 0.78

Question 7

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 H2(g)⇌ 2 NH3(g) 
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 H2(g)⇌ 2 NH3(g)

Question 8

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. 
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.

Question 9

Calculate the value of [N2]eq if [H2]eq = 2.0 M,[NH3]eq = 0.5 M,and Kc = 2.
N2(g)+ 3 H2(g)⇌ 2 NH3(g)

Accepted Answer

A) 0.016 M 
B) 0.031 M 
C) 0.062 M 
D) 0.40 M 
E) 62.5 M 
A) 0.016 M 
B) 0.031 M 
C) 0.062 M 
D) 0.40 M 
E) 62.5 M

Question 10

Why is an equilibrium constant unitless?

Accepted Answer

Each concentration or pressure

Question 11

What is △n for the following equation in relating Kc to Kp?
2 SO2(g)+ O2(g)⇌ 2 SO3(g)

Accepted Answer

A) 3 
B) -1 
C) -2 
D) 2 
E) 1 
A) 3 
B) -1 
C) -2 
D) 2 
E) 1

Question 12

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

Accepted Answer

The expression for both is identical.How

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

For the isomerization reaction: Butane ⇌ isobutane K_p equals 25 at 500°C.If the initial pressures of butane and isobutane are 20.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

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

Consider the following reaction and its equilibrium constant: I₂(g)⇌ 2I(g)K_p = 0.209 A reaction mixture contains 0.89 atm I₂ and 1.77 atm I.Which of the following statements is true concerning this system?

Express the equilibrium constant for the following reaction. 2 P(g)+ 3 Cl₂(g)⇌ 2 PCl₃(g)

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

In which of the following reactions will K_c = K_p?

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

Calculate the value of [N₂]_eq if [H₂]_eq = 2.0 M,[NH₃]_eq= 0.5 M,and K_c = 2. N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g)

Why is an equilibrium constant unitless?

What is △n for the following equation in relating K_c to K_p? 2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g)

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

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Exam 14: Chemical Equilibrium

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

For the isomerization reaction: Butane ⇌ isobutane Kp equals 25 at 500°C.If the initial pressures of butane and isobutane are 20.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

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

Consider the following reaction and its equilibrium constant: I2(g)⇌ 2I(g)Kp = 0.209 A reaction mixture contains 0.89 atm I2 and 1.77 atm I.Which of the following statements is true concerning this system?

Express the equilibrium constant for the following reaction. 2 P(g)+ 3 Cl2(g)⇌ 2 PCl3(g)

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)

In which of the following reactions will Kc = Kp?

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

Calculate the value of [N2]eq if [H2]eq = 2.0 M,[NH3]eq = 0.5 M,and Kc = 2. N2(g)+ 3 H2(g)⇌ 2 NH3(g)

Why is an equilibrium constant unitless?

What is △n for the following equation in relating Kc to Kp? 2 SO2(g)+ O2(g)⇌ 2 SO3(g)

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

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Liquids, Solids, and Intermolecular Forces

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Chemical Kinetics

Acids and Bases

Aqueous Ionic Equilibrium

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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)

For the isomerization reaction: Butane ⇌ isobutane K_p equals 25 at 500°C.If the initial pressures of butane and isobutane are 20.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

Consider the following reaction and its equilibrium constant: I₂(g)⇌ 2I(g)K_p = 0.209 A reaction mixture contains 0.89 atm I₂ and 1.77 atm I.Which of the following statements is true concerning this system?

Express the equilibrium constant for the following reaction. 2 P(g)+ 3 Cl₂(g)⇌ 2 PCl₃(g)

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

In which of the following reactions will K_c = K_p?

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

Calculate the value of [N₂]_eq if [H₂]_eq = 2.0 M,[NH₃]_eq= 0.5 M,and K_c = 2. N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g)

What is △n for the following equation in relating K_c to K_p? 2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g)