Question 1

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. E

Question 2

Express the equilibrium constant for the following reaction: 2 CH3Cl(g)+ Cl2(g)⇔ 2 CH2Cl2(g)+ H2(g)

Accepted Answer

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

Question 3

Match the following.

-Q >> 1

Accepted Answer

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

Question 4

At a certain temperature, Kc equals 1.40 × 102 M-1 for the reaction: 2CO(g)+ O2(g)⇌ 2CO2(g)
If a 3.00 L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium, how many moles of CO are also present in the flask?

Accepted Answer

A) 0.555 mol 
B) 0.185 mol 
C) 0.107 mol 
D) 0.0114 mol 
A) 0.555 mol 
B) 0.185 mol 
C) 0.107 mol 
D) 0.0114 mol

Question 5

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 1.5 mol L-1, [H2]eq = 1.1 mol L-1, [NH3]eq = 0.47 mol L-1. N2(g)+ 3H2(g)⇌ 2NH3(g)

Accepted Answer

A) 3.5 M-2 
B) 0.28 M-2 
C) 9.1 M-2 
D) 0.11 M-2 
E) 0.78 M-2 
A) 3.5 M-2 
B) 0.28 M-2 
C) 9.1 M-2 
D) 0.11 M-2 
E) 0.78 M-2

Question 6

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? Fe3O4(s)+ CO(g)⇌ 3FeO(s)+ CO2(g)ΔH°= +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 7

Consider the following reaction at equilibrium. What effect will removing H2O 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 8

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 mol L-1, [I2]eq = 0.39 mol L-1, [HI]eq = 1.6 mol L-1. H2(g)+ I2(g)⇌ 2HI(g)

Accepted Answer

A) 2.1 × 10-2 
B) 29 
C) 47 
D) 3.4 × 10-2 
E) 8.7 × 10-2 
A) 2.1 × 10-2 
B) 29 
C) 47 
D) 3.4 × 10-2 
E) 8.7 × 10-2

Question 9

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [HCl]eq = 0.13 mol L-1, [HI]eq = 5.6 × 10-16 mol L-1, [Cl2]eq = 0.0019 mol L-1. 2HCl(g)+ I2(s)⇌ 2HI(g)+ Cl2(g)

Accepted Answer

A) 8.2 × 10-18 M 
B) 2.9 × 1031 M 
C) 1.2 × 1017 M 
D) 1.4 × 10-19 M 
E) 3.5 × 10-32 M 
A) 8.2 × 10-18 M 
B) 2.9 × 1031 M 
C) 1.2 × 1017 M 
D) 1.4 × 10-19 M 
E) 3.5 × 10-32 M

Question 10

The reaction below has a Kp value of 3.3 × 10-5 bar. What is the value of Kc for this reaction at 700 K? 2SO3(g)⇌ 2SO2(g)+ O2(g)

Accepted Answer

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

Question 11

For the following reaction, what is Δn required in the conversion of Kc to Kp? N2O4(g)⇌ 2NO2(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

Express the equilibrium constant for the following reaction: SO2(g) + H2O(l)⇌ H2SO3(aq)

Accepted Answer

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

Question 13

At a certain temperature, nitogen and hydrogen react to form ammonia: N2(g)+ 3H2(g)⇌ 2NH3(g)
When initial amounts of N2, H2, and NH3 are mixed, the concentration of NH3 increases. Which statement below is TRUE?

Accepted Answer

A) Kc c > Q 
C) Kc = Q 
D) Kc = Q = 0 
A) Kc c > Q 
C) Kc = Q 
D) Kc = Q = 0

Question 14

The following reaction is exothermic. Which change will shift the equilibrium to the left? 2SO2(g)+ O2(g)⇌ 2SO3(g)

Accepted Answer

A) raising the temperature 
B) decreasing the pressure 
C) increasing the volume 
D) all of the above 
E) none of the above 
A) raising the temperature 
B) decreasing the pressure 
C) increasing the volume 
D) all of the above 
E) none of the above

Question 15

Consider the following reaction: COCl2(g)⇌ CO(g)+ Cl2(g)
A reaction mixture initially contains 1.6 mol L-1 COCl2. Determine the equilibrium concentration of CO if Kc for the reaction at this temperature is 8.33 × 10-4 M. Calculate this based on the assumption that the answer is negligible compared to 1.6.

Accepted Answer

A) 4.2 × 10-4 mol L-1 
B) 1.5 × 10-3 mol L-1 
C) 3.7 × 10-2 mol L-1 
D) 2.1 × 10-2 mol L-1 
E) 1.3 × 10-3 mol L-1 
A) 4.2 × 10-4 mol L-1 
B) 1.5 × 10-3 mol L-1 
C) 3.7 × 10-2 mol L-1 
D) 2.1 × 10-2 mol L-1 
E) 1.3 × 10-3 mol L-1

Question 16

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. 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 17

Which of the following statements is TRUE?

Accepted Answer

A) Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction. 
B) The equilibrium constant for the forward reaction is equal to the equilibrium constant for the reverse reaction. 
C) A reaction quotient (Q)larger than the equilibrium constant (K)means that the reaction will favour the production of more products. 
D) Dynamic equilibrium indicates that the amount of reactants and products are equal. 
E) Dynamic equilibrium is established when K = 0. 
A) Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction. 
B) The equilibrium constant for the forward reaction is equal to the equilibrium constant for the reverse reaction. 
C) A reaction quotient (Q)larger than the equilibrium constant (K)means that the reaction will favour the production of more products. 
D) Dynamic equilibrium indicates that the amount of reactants and products are equal. 
E) Dynamic equilibrium is established when K = 0.

Question 18

For the following reaction, what is Δn required in the conversion of Kc to Kp? N2(g)+ 3H2(g)⇌ 2NH3(g)

Accepted Answer

A) 4 
B) -4 
C) -2 
D) 2 
E) 1 
A) 4 
B) -4 
C) -2 
D) 2 
E) 1

Question 19

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 20

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)= 0.0485 bar and P(trans-2-butene)= 0.165 bar 
B) P(cis-2-butene)= 0.0458 bar and P(trans-2-butene)= 0.156 bar 
C) P(cis-2-butene)= 0.0735 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)= 0.0485 bar and P(trans-2-butene)= 0.165 bar 
B) P(cis-2-butene)= 0.0458 bar and P(trans-2-butene)= 0.156 bar 
C) P(cis-2-butene)= 0.0735 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

Exam 14: Chemical Equilibrium

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

Express the equilibrium constant for the following reaction: 2 CH3Cl(g)+ Cl2(g)⇔ 2 CH2Cl2(g)+ H2(g)

Match the following. -Q >> 1

At a certain temperature, Kc equals 1.40 × 102 M-1 for the reaction: 2CO(g)+ O2(g)⇌ 2CO2(g) If a 3.00 L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium, how many moles of CO are also present in the flask?

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 1.5 mol L-1, [H2]eq = 1.1 mol L-1, [NH3]eq = 0.47 mol L-1. N2(g)+ 3H2(g)⇌ 2NH3(g)

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

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

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 mol L-1, [I2]eq = 0.39 mol L-1, [HI]eq = 1.6 mol L-1. H2(g)+ I2(g)⇌ 2HI(g)

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [HCl]eq = 0.13 mol L-1, [HI]eq = 5.6 × 10-16 mol L-1, [Cl2]eq = 0.0019 mol L-1. 2HCl(g)+ I2(s)⇌ 2HI(g)+ Cl2(g)

The reaction below has a Kp value of 3.3 × 10-5 bar. What is the value of Kc for this reaction at 700 K? 2SO3(g)⇌ 2SO2(g)+ O2(g)

For the following reaction, what is Δn required in the conversion of Kc to Kp? N2O4(g)⇌ 2NO2(g)

Express the equilibrium constant for the following reaction: SO2(g) + H2O(l)⇌ H2SO3(aq)

At a certain temperature, nitogen and hydrogen react to form ammonia: N2(g)+ 3H2(g)⇌ 2NH3(g) When initial amounts of N2, H2, and NH3 are mixed, the concentration of NH3 increases. Which statement below is TRUE?

The following reaction is exothermic. Which change will shift the equilibrium to the left? 2SO2(g)+ O2(g)⇌ 2SO3(g)

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. 2N2(g)+ O2(g)⇌ 2N2O(g)

Which of the following statements is TRUE?

For the following reaction, what is Δn required in the conversion of Kc to Kp? N2(g)+ 3H2(g)⇌ 2NH3(g)

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 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?

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

Express the equilibrium constant for the following reaction: 2 CH₃Cl(g)+ Cl₂(g)⇔ 2 CH₂Cl₂(g)+ H₂(g)

At a certain temperature, K_c equals 1.40 × 10² M^-1for the reaction: 2CO(g)+ O₂(g)⇌ 2CO₂(g) If a 3.00 L flask contains 0.400 mol of CO₂ and 0.100 mol of O₂ at equilibrium, how many moles of CO are also present in the flask?

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [N₂]_eq = 1.5 mol L^-1, [H₂]_eq = 1.1 mol L^-1, [NH₃]_eq = 0.47 mol L^-1. N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

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

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

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 mol L^-1, [I₂]_eq = 0.39 mol L^-1, [HI]_eq = 1.6 mol L^-1. H₂(g)+ I₂(g)⇌ 2HI(g)

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [HCl]_eq = 0.13 mol L^-1, [HI]_eq = 5.6 × 10^-16 mol L^-1, [Cl₂]_eq = 0.0019 mol L^-1. 2HCl(g)+ I₂(s)⇌ 2HI(g)+ Cl₂(g)

The reaction below has a K_p value of 3.3 × 10^-5bar. What is the value of K_c for this reaction at 700 K? 2SO₃(g)⇌ 2SO₂(g)+ O₂(g)

For the following reaction, what is Δn required in the conversion of K_c to K_p? N₂O₄(g)⇌ 2NO₂(g)

Express the equilibrium constant for the following reaction: SO₂₍_g₎ + H₂O(l)⇌ H₂SO₃(aq)

At a certain temperature, nitogen and hydrogen react to form ammonia: N₂(g)+ 3H₂(g)⇌ 2NH₃(g) When initial amounts of N₂, H₂, and NH₃ are mixed, the concentration of NH₃ increases. Which statement below is TRUE?

The following reaction is exothermic. Which change will shift the equilibrium to the left? 2SO₂(g)+ O₂(g)⇌ 2SO₃(g)

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. 2N₂(g)+ O₂(g)⇌ 2N₂O(g)

For the following reaction, what is Δn required in the conversion of K_c to K_p? N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

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 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?