Question 1

The reaction below has a Kc value of 3.64 × 10-3.What is the value of Kp for this reaction at 25°C?
2 NaN3(s)⇌ 2 Na(s)+ 3 N2(g)

Accepted Answer

A)  131 
B)  0.613 
C)  8.90 × 10-2 
D)  29.9 
E)  53.2 
A)  131 
B)  0.613 
C)  8.90 × 10-2 
D)  29.9 
E)  53.2

Question 2

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [C3H8]= 0.15 M,[O2] = 0.35 M,[CO2] = 1.3 M,[H2O] = 2.8 M C3H8(g)+ 5 O2(g)⇌ 3 CO2(g)+ 4 H2O(g)

Accepted Answer

A)  1.7 × 105 
B)  3.2 × 10-6 
C)  6.7 × 103 
D)  7.4 × 102 
E)  6.1.9 × 10-4 
A)  1.7 × 105 
B)  3.2 × 10-6 
C)  6.7 × 103 
D)  7.4 × 102 
E)  6.1.9 × 10-4

Question 3

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. 
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 4

In which of the following reactions will Kc = Kp?

Accepted Answer

A)  4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H2O(g) 
B)  SO3(g) + NO(g) ⇌ SO2(g) + NO2(g) 
C)  2 N2(g) + O2(g) ⇌ 2 N2O(g) 
D)  2 SO2(g) + O2(g) ⇌ 2 SO3(g) 
E)  None of the above reactions have Kc = Kp. 
A)  4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H2O(g) 
B)  SO3(g) + NO(g) ⇌ SO2(g) + NO2(g) 
C)  2 N2(g) + O2(g) ⇌ 2 N2O(g) 
D)  2 SO2(g) + O2(g) ⇌ 2 SO3(g) 
E)  None of the above reactions have Kc = Kp.

Question 5

Consider the following reaction: Xe(g)+ 2 F2(g)→ XeF4(g)
A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F2.If the equilibrium pressure of Xe is 0.34 atm,find the equilibrium constant (Kp)for the reaction.

Accepted Answer

A)  25 
B)  0.12 
C)  0.99 
D)  8.3 
E)  0.040 
A)  25 
B)  0.12 
C)  0.99 
D)  8.3 
E)  0.040

Question 6

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 × 10-3 
A)  5.7 × 10-7 
B)  1.7 × 106 
C)  3.3 × 10-5 
D)  3.0 × 104 
E)  1.9 × 10-3

Question 7

For the following reaction of N2O4,the equilibrium constant is 0.593 at a particular temperature. N2O4(g)⇌ 2 NO2(g)
If the initial concentration of N2O4 is 0.880M,what are the equilibrium concentrations?

Accepted Answer

A)  [N2O4] = 0.705M, [NO2] = 0.350M 
B)  [N2O4] = 0.678M, [NO2] = 0.404M 
C)  [N2O4] = 0.332M, [NO2] = 1.094M 
D)  [N2O4] = 0.586M, [NO2] = 0.588M 
E)  [N2O4] = 0.000M, [NO2] = 1.760M 
A)  [N2O4] = 0.705M, [NO2] = 0.350M 
B)  [N2O4] = 0.678M, [NO2] = 0.404M 
C)  [N2O4] = 0.332M, [NO2] = 1.094M 
D)  [N2O4] = 0.586M, [NO2] = 0.588M 
E)  [N2O4] = 0.000M, [NO2] = 1.760M

Question 8

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 9

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

Accepted Answer

The expression for both are identical.Ho

Question 10

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 11

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. 
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 12

Consider the following reaction at equilibrium.What effect will raising the pressure of the system from 5 atm to 8 atm?
2 NH3(g)⇌ N2(g)+ 3 H2(g)

Accepted Answer

A)  It will shift to the right 
B)  It will shift to the left 
C)  It will have no effect 
D)  It will speed up the reaction 
E)  It will slow down the reaction 
A)  It will shift to the right 
B)  It will shift to the left 
C)  It will have no effect 
D)  It will speed up the reaction 
E)  It will slow down the reaction

Question 13

In a reaction mixture containing only reactants,what is the value of Q?

Accepted Answer

A)  -1 
B)  1 
C)  ∞ 
D)  0 
E)  It cannot be determined without concentrations. 
A)  -1 
B)  1 
C)  ∞ 
D)  0 
E)  It cannot be determined without concentrations.

Question 14

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 × 10-4 
A)  3.4 × 102 
B)  8.5 
C)  1.3 × 103 
D)  1.2 × 10-6 
E)  7.7 × 10-4

Question 15

What is △n for the following equation in relating Kc to Kp?
P4(s)+ 5 O2(g)⇌ P4O10(s)

Accepted Answer

A)  3 
B)  0 
C)  -3 
D)  -6 
E)  -5 
A)  3 
B)  0 
C)  -3 
D)  -6 
E)  -5

Question 16

The reaction below has a Kc value of 1.0 × 1012.What is the value of Kp for this reaction at 200 K?
2 SO2(g)+ O2(g)⇌ 2 SO3(g)

Accepted Answer

A)  6.1 × 10-14 
B)  1.0 × 1012 
C)  1.6 × 10-11 
D)  1.6 × 1013 
E)  6.1 × 1010 
A)  6.1 × 10-14 
B)  1.0 × 1012 
C)  1.6 × 10-11 
D)  1.6 × 1013 
E)  6.1 × 1010

Question 17

Consider the following reaction at equilibrium.What effect will reducing the pressure have on the system?
C3H8(g)+ 5 O2(g)⇌ 3 CO2(g)+ 4 H2O(l)ΔH° = -2220 kJ

Accepted Answer

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

Question 18

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

Accepted Answer

The equilibrium constant relates differe

Question 19

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 Cl2(g) ⇌ 2 NCl3(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 Cl2(g) ⇌ 2 NCl3(g)

Question 20

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 = 0.20 atm. 2 NOCl(g)⇌ 2 NO(g)+ Cl2(g)

Accepted Answer

A)  1.0 
B)  24 
C)  4.1 × 102 
D)  4.1 × 10-2 
E)  0.97 
A)  1.0 
B)  24 
C)  4.1 × 102 
D)  4.1 × 10-2 
E)  0.97

Exam 16: Chemical Equilibrium

The reaction below has a Kc value of 3.64 × 10-3.What is the value of Kp for this reaction at 25°C? 2 NaN3(s)⇌ 2 Na(s)+ 3 N2(g)

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [C3H8]= 0.15 M,[O2] = 0.35 M,[CO2] = 1.3 M,[H2O] = 2.8 M C3H8(g)+ 5 O2(g)⇌ 3 CO2(g)+ 4 H2O(g)

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)

In which of the following reactions will Kc = Kp?

Consider the following reaction: Xe(g)+ 2 F2(g)→ XeF4(g) A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F2.If the equilibrium pressure of Xe is 0.34 atm,find the equilibrium constant (Kp)for the reaction.

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)

For the following reaction of N2O4,the equilibrium constant is 0.593 at a particular temperature. N2O4(g)⇌ 2 NO2(g) If the initial concentration of N2O4 is 0.880M,what are the equilibrium concentrations?

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

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

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

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)

Consider the following reaction at equilibrium.What effect will raising the pressure of the system from 5 atm to 8 atm? 2 NH3(g)⇌ N2(g)+ 3 H2(g)

In a reaction mixture containing only reactants,what is the value of Q?

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 = ?

What is △n for the following equation in relating Kc to Kp? P4(s)+ 5 O2(g)⇌ P4O10(s)

The reaction below has a Kc value of 1.0 × 1012.What is the value of Kp for this reaction at 200 K? 2 SO2(g)+ O2(g)⇌ 2 SO3(g)

Consider the following reaction at equilibrium.What effect will reducing the pressure have on the system? C3H8(g)+ 5 O2(g)⇌ 3 CO2(g)+ 4 H2O(l)ΔH° = -2220 kJ

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

In which of the following reactions will Kc = Kp?

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 = 0.20 atm. 2 NOCl(g)⇌ 2 NO(g)+ Cl2(g)

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Introduction to Solutions and Aqueous Reactions

Thermochemistry

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Solutions

Chemical Kinetics

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Transition Metals and Coordination Compounds

Filters

The reaction below has a K_c value of 3.64 × 10^-3.What is the value of K_p for this reaction at 25°C? 2 NaN₃(s)⇌ 2 Na(s)+ 3 N₂(g)

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [C₃H₈]= 0.15 M,[O₂] = 0.35 M,[CO₂] = 1.3 M,[H₂O] = 2.8 M C₃H₈(g)+ 5 O₂(g)⇌ 3 CO₂(g)+ 4 H₂O(g)

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)

In which of the following reactions will K_c = K_p?

Consider the following reaction: Xe(g)+ 2 F₂(g)→ XeF₄(g) A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F₂.If the equilibrium pressure of Xe is 0.34 atm,find the equilibrium constant (K_p)for the reaction.

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)

For the following reaction of N₂O₄,the equilibrium constant is 0.593 at a particular temperature. N₂O₄(g)⇌ 2 NO₂(g) If the initial concentration of N₂O₄ is 0.880M,what are the equilibrium concentrations?

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

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)

Consider the following reaction at equilibrium.What effect will raising the pressure of the system from 5 atm to 8 atm? 2 NH₃(g)⇌ N₂(g)+ 3 H₂(g)

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 = ?

What is △n for the following equation in relating K_c to K_p? P₄(s)+ 5 O₂(g)⇌ P₄O₁₀(s)

The reaction below has a K_c value of 1.0 × 10¹².What is the value of K_p for this reaction at 200 K? 2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g)

Consider the following reaction at equilibrium.What effect will reducing the pressure have on the system? C₃H₈(g)+ 5 O₂(g)⇌ 3 CO₂(g)+ 4 H₂O(l)ΔH° = -2220 kJ

In which of the following reactions will K_c = K_p?

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 = 0.20 atm. 2 NOCl(g)⇌ 2 NO(g)+ Cl₂(g)