Question 1

For the following reaction, what is Δn required in the conversion of Kc to Kp? 2SO2(g) + O2(g) ⇌ 2SO3(g)

Accepted Answer

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

Question 2

Which of the following statements is TRUE?

Accepted Answer

A)  If Q  K, it means the forward reaction will proceed to form more products. 
C)  If Q = K, it means the reaction is at equilibrium. 
D)  If Q > K, it means the reaction is shifted to the right. 
A)  If Q  K, it means the forward reaction will proceed to form more products. 
C)  If Q = K, it means the reaction is at equilibrium. 
D)  If Q > K, it means the reaction is shifted to the right.

Question 3

Express the equilibrium constant for the following reaction: 2NH3(g) ⇔ N2(g) + 3H2(g)

Accepted Answer

A)  KP =   
B)  KP =   
C)  KP =   
D)  KP =   
E)  KP =   
A)  KP =   
B)  KP =   
C)  KP =   
D)  KP =   
E)  KP =

Question 4

Match the following.
-Q = K

Accepted Answer

A) reverse reaction is favoured 
B) reaction is at equilibrium 
C) reaction favours formation of more products 
D) reaction does not strongly favour reactants or products 
E) reaction has a larger amount of products than reactants
F)reaction will favour formation of reactants 
A) reverse reaction is favoured 
B) reaction is at equilibrium 
C) reaction favours formation of more products 
D) reaction does not strongly favour reactants or products 
E) reaction has a larger amount of products than reactants
F)reaction will favour formation of reactants

Question 5

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

Accepted Answer

A)  KP =   
B)  KP =   
C)  KP =   
D)  KP=   
E)  KP =   
A)  KP =   
B)  KP =   
C)  KP =   
D)  KP=   
E)  KP =

Question 6

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. N2O4(g) ⇌ 2NO2(g) K = 1.46
2N2O4(g) ⇌ 4NO2(g) K = ?

Accepted Answer

A)  2.13 
B)  0.685 
C)  3.11 
D)  1.46 
E)  1.13 
A)  2.13 
B)  0.685 
C)  3.11 
D)  1.46 
E)  1.13

Question 7

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

Accepted Answer

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

Question 8

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of CO2(g). NH2COONH4(s) ⇌ 2NH3(g) + CO2(g) Kc = 1.58 × 10-8 M3
[NH3]eq = 2.9 × 10-3 mol L-1

Accepted Answer

A)  0.053 mol L-1 
B)  4.6 × 10-11 mol L-1 
C)  1.9 × 10-3 mol L-1 
D)  5.4 × 10-6 mol L-1 
E)  0.022 mol L-1 
A)  0.053 mol L-1 
B)  4.6 × 10-11 mol L-1 
C)  1.9 × 10-3 mol L-1 
D)  5.4 × 10-6 mol L-1 
E)  0.022 mol L-1

Question 9

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? Xe(g) + 2F2(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. 
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 10

For the following reaction, what is △n required in the conversion of Kc to Kp? P4(s) + 5O2(g) ⇌ P4O10(s)

Accepted Answer

A)  3 
B)  4 
C)  -4 
D)  5 
E)  -5 
A)  3 
B)  4 
C)  -4 
D)  5 
E)  -5

Question 11

Consider the following reaction at equilibrium. What effect will adding some C have on the system? CO2(g) + C(graphite) ⇌ 2CO(g)

Accepted Answer

A)  No effect will be observed since C is not included in the equilibrium expression. 
B)  The equilibrium constant will decrease. 
C)  The reaction will shift to the left in the direction of reactants. 
D)  The equilibrium constant will increase. 
E)  The reaction will shift to the right in the direction of products. 
A)  No effect will be observed since C is not included in the equilibrium expression. 
B)  The equilibrium constant will decrease. 
C)  The reaction will shift to the left in the direction of reactants. 
D)  The equilibrium constant will increase. 
E)  The reaction will shift to the right in the direction of products.

Question 12

For which of the following reactions will ∆n = -2?

Accepted Answer

A)  H2(g) + I2(g) ⇌ 2HI(g) 
B)  CH4(g) + H2O(g) ⇌ CO(g) + 3H2(g) 
C)  N2O4(g) ⇌ 2NO2(g) 
D)  2SO2(g) + O2(g) ⇌ 2SO3(g) 
E)  N2(g) + 3H2(g) ⇌ 2NH3(g) 
A)  H2(g) + I2(g) ⇌ 2HI(g) 
B)  CH4(g) + H2O(g) ⇌ CO(g) + 3H2(g) 
C)  N2O4(g) ⇌ 2NO2(g) 
D)  2SO2(g) + O2(g) ⇌ 2SO3(g) 
E)  N2(g) + 3H2(g) ⇌ 2NH3(g)

Question 13

The equilibrium constant is given for two of the reactions below. Determine the value of the missing equilibrium constant. A(g) + 2B(g) ⇌ AB2(g) Kc = 59
AB2(g) + B(g) ⇌ AB3(g) Kc = ?
A(g) + 3B(g) ⇌ AB3(g) Kc = 478

Accepted Answer

A)  3.5 × 10-5 
B)  2.8 × 104 
C)  8.1 
D)  0.12 
E)  89 
A)  3.5 × 10-5 
B)  2.8 × 104 
C)  8.1 
D)  0.12 
E)  89

Question 14

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

Accepted Answer

A)  KP =   
B)  KP =   
C)  KP =   
D)  KP =   
E)  Kp =   
A)  KP =   
B)  KP =   
C)  KP =   
D)  KP =   
E)  Kp =

Question 15

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO2(g). N2O4(g) ⇌ 2NO2(g) Kc = 0.21 M
[N2O4]eq = 0.039 mol L-1

Accepted Answer

A)  1.22 mol L-1 
B)  9.0 × 10-2 mol L-1 
C)  7.8 × 10-2 mol L-1 
D)  8.2 × 10-3 mol L-1 
E)  11 mol L-1 
A)  1.22 mol L-1 
B)  9.0 × 10-2 mol L-1 
C)  7.8 × 10-2 mol L-1 
D)  8.2 × 10-3 mol L-1 
E)  11 mol L-1

Question 16

Match the following.
-Q < K

Accepted Answer

A) reverse reaction is favoured 
B) reaction is at equilibrium 
C) reaction favours formation of more products 
D) reaction does not strongly favour reactants or products 
E) reaction has a larger amount of products than reactants
F)reaction will favour formation of reactants 
A) reverse reaction is favoured 
B) reaction is at equilibrium 
C) reaction favours formation of more products 
D) reaction does not strongly favour reactants or products 
E) reaction has a larger amount of products than reactants
F)reaction will favour formation of reactants

Question 17

The equilibrium constant, Kp, equals 3.40 for the isomerization reaction: cis-2-butene ⇌ trans-2-butene
If a flask initially contains 0.250 bar of cis-2-butene and 0. 165 bar of trans-2-butene, what is the equilibrium pressure of each gas?

Accepted Answer

A)  P(cis-2-butene) = 0.0 485 bar and P(trans-2-butene) = 0. 165 bar 
B)  P(cis-2-butene) = 0.0 458 bar and P(trans-2-butene) = 0. 156 bar 
C)  P(cis-2-butene) = 0.0 735 bar and P(trans-2-butene) = 0.250 bar 
D)  P(cis-2-butene) = 0. 0943 bar and P(trans-2-butene) = 0. 321 bar 
A)  P(cis-2-butene) = 0.0 485 bar and P(trans-2-butene) = 0. 165 bar 
B)  P(cis-2-butene) = 0.0 458 bar and P(trans-2-butene) = 0. 156 bar 
C)  P(cis-2-butene) = 0.0 735 bar and P(trans-2-butene) = 0.250 bar 
D)  P(cis-2-butene) = 0. 0943 bar and P(trans-2-butene) = 0. 321 bar

Question 18

Consider the following reaction: NO(g) + SO3(g) ⇌ NO2(g) + SO2(g)
A reaction mixture initially contains 1.24 bar NO and 0.92 bar SO3. Determine the equilibrium pressure of NO2 if Kp for the reaction at this temperature is 0.0118.

Accepted Answer

A)  0.32 bar 
B)  1.32 bar 
C)  0.10 bar 
D)  0.74 bar 
E)  0.022 bar 
A)  0.32 bar 
B)  1.32 bar 
C)  0.10 bar 
D)  0.74 bar 
E)  0.022 bar

Question 19

Consider the following reaction and its equilibrium constant: 4CuO(s) + CH4(g) ⇌ CO2(g) + 4Cu(s) + 2H2O(g) Kc = 1.10
A reaction mixture contains 0.22 mol L-1 CH4, 0.67 mol L-1 CO2 and 1.3 mol L-1 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. 
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.

Question 20

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [PCl5]eq = 0.56 mol L-1, [PCl3]eq = 0.23 mol L-1, [Cl2]eq = 4.4 mol L-1. PCl5(g) ⇌ PCl3(g) + Cl2(g)

Accepted Answer

A)  1.8 M 
B)  0.93 M 
C)  0.55 M 
D)  1.1 M 
E)  0.76 M 
A)  1.8 M 
B)  0.93 M 
C)  0.55 M 
D)  1.1 M 
E)  0.76 M

Exam 14: Chemical Equilibrium

For the following reaction, what is Δn required in the conversion of Kc to Kp? 2SO2(g) + O2(g) ⇌ 2SO3(g)

Which of the following statements is TRUE?

Express the equilibrium constant for the following reaction: 2NH3(g) ⇔ N2(g) + 3H2(g)

Match the following. -Q = K

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

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. N2O4(g) ⇌ 2NO2(g) K = 1.46 2N2O4(g) ⇌ 4NO2(g) K = ?

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

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of CO2(g). NH2COONH4(s) ⇌ 2NH3(g) + CO2(g) Kc = 1.58 × 10-8 M3 [NH3]eq = 2.9 × 10-3 mol L-1

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

For the following reaction, what is △n required in the conversion of Kc to Kp? P4(s) + 5O2(g) ⇌ P4O10(s)

Consider the following reaction at equilibrium. What effect will adding some C have on the system? CO2(g) + C(graphite) ⇌ 2CO(g)

For which of the following reactions will ∆n = -2?

The equilibrium constant is given for two of the reactions below. Determine the value of the missing equilibrium constant. A(g) + 2B(g) ⇌ AB2(g) Kc = 59 AB2(g) + B(g) ⇌ AB3(g) Kc = ? A(g) + 3B(g) ⇌ AB3(g) Kc = 478

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

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO2(g). N2O4(g) ⇌ 2NO2(g) Kc = 0.21 M [N2O4]eq = 0.039 mol L-1

Match the following. -Q < K

The equilibrium constant, Kp, equals 3.40 for the isomerization reaction: cis-2-butene ⇌ trans-2-butene If a flask initially contains 0.250 bar of cis-2-butene and 0. 165 bar of trans-2-butene, what is the equilibrium pressure of each gas?

Consider the following reaction: NO(g) + SO3(g) ⇌ NO2(g) + SO2(g) A reaction mixture initially contains 1.24 bar NO and 0.92 bar SO3. Determine the equilibrium pressure of NO2 if Kp for the reaction at this temperature is 0.0118.

Consider the following reaction and its equilibrium constant: 4CuO(s) + CH4(g) ⇌ CO2(g) + 4Cu(s) + 2H2O(g) Kc = 1.10 A reaction mixture contains 0.22 mol L-1 CH4, 0.67 mol L-1 CO2 and 1.3 mol L-1 H2O. Which of the following statements is TRUE concerning this system?

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [PCl5]eq = 0.56 mol L-1, [PCl3]eq = 0.23 mol L-1, [Cl2]eq = 4.4 mol L-1. PCl5(g) ⇌ PCl3(g) + Cl2(g)

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry Ii: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

For the following reaction, what is Δn required in the conversion of K_c to K_p? 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)

Express the equilibrium constant for the following reaction: 2NH₃(g) ⇔ N₂(g) + 3H₂(g)

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

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. N₂O₄(g) ⇌ 2NO₂(g) K = 1.46 2N₂O₄(g) ⇌ 4NO₂(g) K = ?

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

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of CO₂(g). NH₂COONH₄(s) ⇌ 2NH₃(g) + CO₂(g) K_c = 1.58 × 10^-8M³ [NH₃]_eq = 2.9 × 10^-3 mol L^-1

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

For the following reaction, what is △n required in the conversion of K_c to K_p? P₄(s) + 5O₂(g) ⇌ P₄O₁₀(s)

Consider the following reaction at equilibrium. What effect will adding some C have on the system? CO₂(g) + C(graphite) ⇌ 2CO(g)

The equilibrium constant is given for two of the reactions below. Determine the value of the missing equilibrium constant. A(g) + 2B(g) ⇌ AB₂(g) K_c = 59 AB₂(g) + B(g) ⇌ AB₃(g) K_c = ? A(g) + 3B(g) ⇌ AB₃(g) K_c = 478

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

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO₂(g). N₂O₄(g) ⇌ 2NO₂(g) K_c = 0.21 M [N₂O₄]_eq = 0.039 mol L^-1

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 bar of cis-2-butene and 0. 165 bar of trans-2-butene, what is the equilibrium pressure of each gas?

Consider the following reaction: NO(g) + SO₃(g) ⇌ NO₂(g) + SO₂(g) A reaction mixture initially contains 1.24 bar NO and 0.92 bar SO₃. Determine the equilibrium pressure of NO₂ if K_p for the reaction at this temperature is 0.0118.

Consider the following reaction and its equilibrium constant: 4CuO(s) + CH₄(g) ⇌ CO₂(g) + 4Cu(s) + 2H₂O(g) K_c = 1.10 A reaction mixture contains 0.22 mol L^-1 CH₄, 0.67 mol L^-1 CO₂and 1.3 mol L^-1 H₂O. Which of the following statements is TRUE concerning this system?

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [PCl₅]_eq = 0.56 mol L^-1, [PCl₃]_eq = 0.23 mol L^-1, [Cl₂]_eq = 4.4 mol L^-1. PCl₅(g) ⇌ PCl₃(g) + Cl₂(g)