Question 1

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

Accepted Answer

A) The forward reaction is favoured. 
B) The reverse reaction is favoured. 
C) Neither direction is favoured. 
D) If the temperature is raised,then the forward reaction is favoured. 
E) If the temperature is raised,then the reverse reaction is favoured. 
A) The forward reaction is favoured. 
B) The reverse reaction is favoured. 
C) Neither direction is favoured. 
D) If the temperature is raised,then the forward reaction is favoured. 
E) If the temperature is raised,then the reverse reaction is favoured.

Question 2

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 3.6 mol L-1,[O2]eq = 4.1 mol L-1,[N2O]eq = 3.3 × 10-18 mol L-1. 
$\quad$$\quad$2N2(g)+ O2(g)⇌ 2N2O(g)

Accepted Answer

A) 2.2 × 10-19  
B) 4.5 × 1018  
C) 2.0 × 10-37 
D) 5.0 × 1036 
E) 4.9 × 10-17  
A) 2.2 × 10-19  
B) 4.5 × 1018  
C) 2.0 × 10-37 
D) 5.0 × 1036 
E) 4.9 × 10-17

Question 3

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of SO3(g). 
$\quad$$\quad$2SO2(g)+ O2(g)⇌ 2SO3(g)$\quad$$\quad$Kc = 1.7 × 108 M-1
$\quad$$\quad$[SO2]eq = 0.0034 mol L-1 $\quad$$\quad$[O2]eq = 0.0018 mol L-1

Accepted Answer

A) 1.9 mol L-1 
B) 1.0 × 103 mol L-1 
C) 0.53 mol L-1 
D) 9.6 × 10-4 mol L-1 
E) 0.73 mol L-1 
A) 1.9 mol L-1 
B) 1.0 × 103 mol L-1 
C) 0.53 mol L-1 
D) 9.6 × 10-4 mol L-1 
E) 0.73 mol L-1

Question 4

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

Question 5

Consider the following reaction at equilibrium.What effect will adding some C have on the system? 
$\quad$$\quad$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 6

Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system? 
$\quad$$\quad$$\quad$CuS(s)+ O2(g)⇌ Cu(s)+ SO2(g)

Accepted Answer

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

Question 7

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. 
$\quad$H2(g)+ Br2(g)⇌ 2HBr$\quad$$\quad$(g)K = 3.8 × 104
$\quad$4HBr(g)⇌ 2H2(g)+ 2Br2$\quad$ (g)K = ?

Accepted Answer

A) 1.9 × 104 
B) 5.1 × 10-3 
C) 2.6 × 10-5 
D) 6.9 × 10-10 
E) 1.6 × 103 
A) 1.9 × 104 
B) 5.1 × 10-3 
C) 2.6 × 10-5 
D) 6.9 × 10-10 
E) 1.6 × 103

Question 8

Express the equilibrium constant for the following reaction: 
$\quad$$\quad$P4(s)+ 5O2(g)? P4O10(s)

Accepted Answer

A) Kc = $\frac { \left[ \mathrm { P } _ { 4 } \right] \left[ \mathrm { O } _ { 2 } \right] ^ { 5 } } { \left[ \mathrm { P } _ { 4 } \mathrm { O } _ { 10 } \right] }$ 
B) Kc = $\frac { \left[ \mathrm { P } _ { 4 } \mathrm { O } _ { 10 } \right] } { \left[ \mathrm { P } _ { 4 } \right] \left[ \mathrm { O } _ { 2 } \right] ^ { 5 } }$ 
C) Kc = [O2]-5 
D) Kc = [O2]5 
E) Kc = $\frac { \left[ \mathrm { P } _ { 4 } \mathrm { O } _ { 10 } \right] } { \left[ \mathrm { P } _ { 4 } \right] \left[ \mathrm { O } _ { 2 } \right] ^ { 1 / 5 } }$ 
A) Kc = $\frac { \left[ \mathrm { P } _ { 4 } \right] \left[ \mathrm { O } _ { 2 } \right] ^ { 5 } } { \left[ \mathrm { P } _ { 4 } \mathrm { O } _ { 10 } \right] }$ 
B) Kc = $\frac { \left[ \mathrm { P } _ { 4 } \mathrm { O } _ { 10 } \right] } { \left[ \mathrm { P } _ { 4 } \right] \left[ \mathrm { O } _ { 2 } \right] ^ { 5 } }$ 
C) Kc = [O2]-5 
D) Kc = [O2]5 
E) Kc = $\frac { \left[ \mathrm { P } _ { 4 } \mathrm { O } _ { 10 } \right] } { \left[ \mathrm { P } _ { 4 } \right] \left[ \mathrm { O } _ { 2 } \right] ^ { 1 / 5 } }$

Question 9

Consider the following reaction,equilibrium pressures,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of H2. 
$\quad$D2(g)+ H2(g)⇌ 2HD(g)$\quad$$\quad$ Kp = 1.80
$\quad$P(D2)eq = 1.1 × 10-3 bar $\quad$$\quad$P(HD)eq = 2.7 × 10-3 bar

Accepted Answer

A) 2.7 bar 
B) 1.4 bar 
C) 0.73 bar 
D) 3.7 × 10-3 bar 
E) 8.1 × 10-4 bar 
A) 2.7 bar 
B) 1.4 bar 
C) 0.73 bar 
D) 3.7 × 10-3 bar 
E) 8.1 × 10-4 bar

Question 10

Explain dynamic equilibrium.Use the generic reaction A(g)⇌ B(g)to explain.

Accepted Answer

In this reaction,dynamic equilibrium mea

Question 11

Cyclohexane (C6H12)undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane (MCP)according to the equation: C6H12 ⇌ MCP
If Kc = 0.143 at 25 °C for this reaction,predict the direction in which the system will shift if the initial concentrations of C6H12 and MCP are 0.0400 mol L-1 and 0.0200 mol L-1,respectively.The system

Accepted Answer

A) will shift left. 
B) will shift right. 
C) is already at equilibrium. 
D) is not at equilibrium and will remain in an unequilibrated state. 
A) will shift left. 
B) will shift right. 
C) is already at equilibrium. 
D) is not at equilibrium and will remain in an unequilibrated state.

Question 12

In a reaction mixture containing reactants and products,each at a concentration of 1 mol L-1,what is the value of Q?

Accepted Answer

A) -1 
B) 1 
C) ∞ 
D) 0 
E) Q = K 
A) -1 
B) 1 
C) ∞ 
D) 0 
E) Q = K

Question 13

For which of the following reactions will Kc = Kp?

Accepted Answer

A) H2(g)+ I2(g)⇌ 2HI(g) 
B) CH4(g)+ H2O(g)⇌ CO(g)+ 3H2(g) 
C) N2O4(g)⇌ 2NO2(g) 
D) CO(g)+ 2H2(g)⇌ CH3OH(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) CO(g)+ 2H2(g)⇌ CH3OH(g) 
E) N2(g)+ 3H2(g)⇌ 2NH3(g)

Question 14

Consider the following reaction at equilibrium.What effect will increasing the temperature have on the system? 
Fe3O4(s)+ CO(g)⇌ 3FeO(s)+ CO2(g)ΔrH°= +35.9 kJ

Accepted Answer

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

Question 15

Consider the following reaction and its equilibrium constant: 
SO2(g)+ NO2(g)⇌ SO3(g)+ NO(g)Kc = 0.33
A reaction mixture contains 0.39 mol L-1 SO2,0.14 mol L-1 NO2 ,0.11 mol L-1 SO3 and 0.14 mol L-1 NO.Which of the following statements is TRUE concerning this system?

Accepted Answer

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

Question 16

The decomposition of ammonia is 2NH3(g)→ N2(g)+ 3H2(g).If Kp is 1.5 × 103 bar2 at 400 °C,what is the partial pressure of ammonia at equilibrium when the partial pressure of N2(g)is 0.10 bar and that of H2(g)is 0.15 bar?

Accepted Answer

A) 2.2 × 10-7 bar 
B) 4.7 × 10-4 bar 
C) 2.1 × 103 bar 
D) 4.4 × 106 bar 
A) 2.2 × 10-7 bar 
B) 4.7 × 10-4 bar 
C) 2.1 × 103 bar 
D) 4.4 × 106 bar

Question 17

The reaction below has a Kp value of 41 bar-2.What is the value of Kc for this reaction at 400 K? 
$\quad$N2(g)+ 3H2(g)⇌ 2NH3(g)

Accepted Answer

A) 2.4 × 10-2 M-2 
B) 4.4 × 104 M-2 
C) 41 M-2 
D) 2.3 × 10-5 M-2 
E) 1.9 × 104 M-2 
A) 2.4 × 10-2 M-2 
B) 4.4 × 104 M-2 
C) 41 M-2 
D) 2.3 × 10-5 M-2 
E) 1.9 × 104 M-2

Question 18

For the isomerization reaction: 
$\quad$butane ⇌ isobutane
Kp equals 25.0 at 500 °C.If the initial pressures of butane and isobutane are 20.0 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 19

Identify the change that will always shift the equilibrium to the right.

Accepted Answer

A) remove reactant 
B) increase product 
C) remove product 
D) increase pressure 
E) increase volume 
A) remove reactant 
B) increase product 
C) remove product 
D) increase pressure 
E) increase volume

Question 20

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

Accepted Answer

The equilibrium constant relat

Exam 14: Chemical Equilibrium

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

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 3.6 mol L-1,[O2]eq = 4.1 mol L-1,[N2O]eq = 3.3 × 10-18 mol L-1. \quad\quad 2N2(g)+ O2(g)⇌ 2N2O(g)

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

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

Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system? \quad\quad\quad CuS(s)+ O2(g)⇌ Cu(s)+ SO2(g)

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. \quad H2(g)+ Br2(g)⇌ 2HBr \quad\quad (g)K = 3.8 × 104 \quad 4HBr(g)⇌ 2H2(g)+ 2Br2 \quad (g)K = ?

Express the equilibrium constant for the following reaction: \quad\quad P4(s)+ 5O2(g)? P4O10(s)

Consider the following reaction,equilibrium pressures,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of H2. \quad D2(g)+ H2(g)⇌ 2HD(g) \quad\quad Kp = 1.80 \quad P(D2)eq = 1.1 × 10-3 bar \quad\quad P(HD)eq = 2.7 × 10-3 bar

Explain dynamic equilibrium.Use the generic reaction A(g)⇌ B(g)to explain.

In a reaction mixture containing reactants and products,each at a concentration of 1 mol L-1,what is the value of Q?

For which of the following reactions will Kc = Kp?

Consider the following reaction at equilibrium.What effect will increasing the temperature have on the system? Fe3O4(s)+ CO(g)⇌ 3FeO(s)+ CO2(g)ΔrH°= +35.9 kJ

Consider the following reaction and its equilibrium constant: SO2(g)+ NO2(g)⇌ SO3(g)+ NO(g)Kc = 0.33 A reaction mixture contains 0.39 mol L-1 SO2,0.14 mol L-1 NO2 ,0.11 mol L-1 SO3 and 0.14 mol L-1 NO.Which of the following statements is TRUE concerning this system?

The decomposition of ammonia is 2NH3(g)→ N2(g)+ 3H2(g).If Kp is 1.5 × 103 bar2 at 400 °C,what is the partial pressure of ammonia at equilibrium when the partial pressure of N2(g)is 0.10 bar and that of H2(g)is 0.15 bar?

The reaction below has a Kp value of 41 bar-2.What is the value of Kc for this reaction at 400 K? \quad N2(g)+ 3H2(g)⇌ 2NH3(g)

For the isomerization reaction: \quad butane ⇌ isobutane Kp equals 25.0 at 500 °C.If the initial pressures of butane and isobutane are 20.0 atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

Identify the change that will always shift the equilibrium to the right.

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

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Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [N₂]_eq = 3.6 mol L^-1,[O₂]_eq = 4.1 mol L^-1,[N₂O]_eq = 3.3 × 10^-18 mol L^-1. $\quad$ $\quad$ 2N₂(g)+ O₂(g)⇌ 2N₂O(g)

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

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

Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system? $\quad$ $\quad$ $\quad$ CuS(s)+ O₂(g)⇌ Cu(s)+ SO₂(g)

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. $\quad$ H₂(g)+ Br₂(g)⇌ 2HBr $\quad$ $\quad$ (g)K = 3.8 × 10⁴ $\quad$ 4HBr(g)⇌ 2H₂(g)+ 2Br₂ $\quad$ (g)K = ?

Express the equilibrium constant for the following reaction: $\quad$ $\quad$ P₄(s)+ 5O₂(g)? P₄O₁₀(s)

Consider the following reaction,equilibrium pressures,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of H₂. $\quad$ D₂(g)+ H₂(g)⇌ 2HD(g) $\quad$ $\quad$ K_p = 1.80 $\quad$ P(D₂)_eq = 1.1 × 10^-3bar $\quad$ $\quad$ P(HD)_eq = 2.7 × 10^-3 bar

In a reaction mixture containing reactants and products,each at a concentration of 1 mol L^-1,what is the value of Q?

For which of the following reactions will K_c = K_p?

Consider the following reaction at equilibrium.What effect will increasing the temperature have on the system? Fe₃O₄(s)+ CO(g)⇌ 3FeO(s)+ CO₂(g)Δ_rH°= +35.9 kJ

Consider the following reaction and its equilibrium constant: SO₂(g)+ NO₂(g)⇌ SO₃(g)+ NO(g)K_c = 0.33 A reaction mixture contains 0.39 mol L^-1 SO₂,0.14 mol L^-1 NO₂,0.11 mol L^-1 SO₃ and 0.14 mol L^-1 NO.Which of the following statements is TRUE concerning this system?

The decomposition of ammonia is 2NH₃(g)→ N₂(g)+ 3H₂(g).If K_p is 1.5 × 10³ bar² at 400 °C,what is the partial pressure of ammonia at equilibrium when the partial pressure of N₂(g)is 0.10 bar and that of H₂(g)is 0.15 bar?

The reaction below has a K_p value of 41 bar^-2.What is the value of K_c for this reaction at 400 K? $\quad$ N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

For the isomerization reaction: $\quad$ butane ⇌ isobutane K_p equals 25.0 at 500 °C.If the initial pressures of butane and isobutane are 20.0 atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?