Question 1

Express the equilibrium constant for the following reaction. RbBrO3(s)⇌ RbBrO(s)+ O2(g)

Accepted Answer

A)  K =   
B)  K = [O2]-1 
C)  K =   
D)  K =   
E)  K = [O2] 
A)  K =   
B)  K = [O2]-1 
C)  K =   
D)  K =   
E)  K = [O2] E

Question 2

Consider the following reaction at equilibrium.What effect will removing NO2 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. D

Question 3

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [PBr5]eq = 0.56 M,[PBr3]eq = 0.23 M,[Br2]eq = 6.6 M. PBr5(g)⇌ PBr3(g)+ Br2(g)

Accepted Answer

A)  2.7 
B)  0.93 
C)  0.37 
D)  4.2 
E)  0.76 
A)  2.7 
B)  0.93 
C)  0.37 
D)  4.2 
E)  0.76 A

Question 4

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 5

Consider the following reaction at equilibrium.What effect will adding 2.3 mole of Rn to the reaction mixture have on the system? 2 H2S(g)+ 3 O2(g)⇌ 2 H2O(g)+ 2 SO2(g)

Accepted Answer

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

Question 6

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

Accepted Answer

A)  No effect will be observed. 
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. 
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 7

What is Δn for the following equation in relating Kc to Kp? N2(g)+ 3 F2(g)⇌ 2 NF3(g)

Accepted Answer

A)  4 
B)  -3 
C)  -2 
D)  2 
E)  0 
A)  4 
B)  -3 
C)  -2 
D)  2 
E)  0

Question 8

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO2(g). NH2COONH4(s)⇌ 2 NH3(g)+ CO2(g)Kc = 1.58 × 10-8
[NH3]eq = 2.3 × 10-3 M

Accepted Answer

A)  0.053 M 
B)  3.6 × 10-11 M 
C)  3.0 × 10-3 M 
D)  6.9 × 10-6 M 
E)  0.022 M 
A)  0.053 M 
B)  3.6 × 10-11 M 
C)  3.0 × 10-3 M 
D)  6.9 × 10-6 M 
E)  0.022 M

Question 9

Consider the following reaction: 2 H2O(g)+ 2 SO2(g)⇌ 2 H2S(g)+ 3 O2(g)
A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2.Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10-6.

Accepted Answer

A)  0.045 M 
B)  0.058 M 
C)  0.028 M 
D)  3.1 × 10-3 M 
E)  0.12 M 
A)  0.045 M 
B)  0.058 M 
C)  0.028 M 
D)  3.1 × 10-3 M 
E)  0.12 M

Question 10

Consider the following reaction and its equilibrium constant: I2(g)+ Br2(g)⇌ 2 IBr(g)Kc = 1.1 × 102
A reaction mixture contains 0.37 M I2,0.30 M Br2 and 3.5 M IBr.Which of the following statements is TRUE concerning this system?

Accepted Answer

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

Question 11

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 12

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

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 13

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of H2O(g). C2H4(g)+ H2O(g)⇌ C2H5OH(g)Kc = 9.0 × 103
[C2H4]eq = 0.015 M [C2H5OH]eq = 1.69 M

Accepted Answer

A)  9.9 × 10-7 M 
B)  80. M 
C)  1.0 M 
D)  1.68 M 
E)  0.013 M 
A)  9.9 × 10-7 M 
B)  80. M 
C)  1.0 M 
D)  1.68 M 
E)  0.013 M

Question 14

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 not at equilibrium. 
D)  All of the above are true. 
E)  None of the above is true. 
A)  If Q  K, it means the forward reaction will proceed to form more products. 
C)  If Q = K, it means the reaction is not at equilibrium. 
D)  All of the above are true. 
E)  None of the above is true.

Question 15

What is Δn 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)  1 
E)  4 
A)  -3 
B)  -1 
C)  -2 
D)  1 
E)  4

Question 16

Define dynamic equilibrium.

Accepted Answer

A)  no reactants react 
B)  no products are formed 
C)  the rate of the forward reaction is faster than the rate of the reverse reaction 
D)  the rate of the reverse reaction is faster than the rate of the forward reaction 
E)  the rate of the forward reaction equals the rate of the reverse reaction 
A)  no reactants react 
B)  no products are formed 
C)  the rate of the forward reaction is faster than the rate of the reverse reaction 
D)  the rate of the reverse reaction is faster than the rate of the forward reaction 
E)  the rate of the forward reaction equals the rate of the reverse reaction

Question 17

Express the equilibrium constant for the following reaction. Pb(NO3)2(aq)+ 2 NaI(aq)⇌ PbI2(s)+ 2 NaNO3(aq)

Accepted Answer

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

Question 18

Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction: PCl3(g)+ Cl2(g)⇌ PCl5(g)
An equilibrium mixture at 450 K contains   = 0.124 atm,   = 0.157 atm,and   = 1.30 atm.What is the value of Kp at this temperature?

Accepted Answer

A)  66.7 
B)  1.50 ×   
C)  2.53 × 10-2 
D)  1.02 
E)  4.63 
A)  66.7 
B)  1.50 ×   
C)  2.53 × 10-2 
D)  1.02 
E)  4.63

Question 19

Consider the following reaction at equilibrium.What effect will reducing the volume 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 20

Consider the following reaction at equilibrium.What effect will increasing the temperature 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.

Exam 15: Chemical Equilibrium

Express the equilibrium constant for the following reaction. RbBrO3(s)⇌ RbBrO(s)+ O2(g)

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

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [PBr5]eq = 0.56 M,[PBr3]eq = 0.23 M,[Br2]eq = 6.6 M. PBr5(g)⇌ PBr3(g)+ Br2(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

Consider the following reaction at equilibrium.What effect will adding 2.3 mole of Rn to the reaction mixture have on the system? 2 H2S(g)+ 3 O2(g)⇌ 2 H2O(g)+ 2 SO2(g)

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

What is Δn for the following equation in relating Kc to Kp? N2(g)+ 3 F2(g)⇌ 2 NF3(g)

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO2(g). NH2COONH4(s)⇌ 2 NH3(g)+ CO2(g)Kc = 1.58 × 10-8 [NH3]eq = 2.3 × 10-3 M

Consider the following reaction: 2 H2O(g)+ 2 SO2(g)⇌ 2 H2S(g)+ 3 O2(g) A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2.Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10-6.

Consider the following reaction and its equilibrium constant: I2(g)+ Br2(g)⇌ 2 IBr(g)Kc = 1.1 × 102 A reaction mixture contains 0.37 M I2,0.30 M Br2 and 3.5 M IBr.Which of the following statements is TRUE concerning this system?

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

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

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of H2O(g). C2H4(g)+ H2O(g)⇌ C2H5OH(g)Kc = 9.0 × 103 [C2H4]eq = 0.015 M [C2H5OH]eq = 1.69 M

Which of the following statements is TRUE?

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

Define dynamic equilibrium.

Express the equilibrium constant for the following reaction. Pb(NO3)2(aq)+ 2 NaI(aq)⇌ PbI2(s)+ 2 NaNO3(aq)

Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction: PCl3(g)+ Cl2(g)⇌ PCl5(g) An equilibrium mixture at 450 K contains = 0.124 atm, = 0.157 atm,and = 1.30 atm.What is the value of Kp at this temperature?

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

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

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Express the equilibrium constant for the following reaction. RbBrO₃(s)⇌ RbBrO(s)+ O₂(g)

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

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [PBr₅]_eq = 0.56 M,[PBr₃]_eq = 0.23 M,[Br₂]_eq = 6.6 M. PBr₅(g)⇌ PBr₃(g)+ Br₂(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

Consider the following reaction at equilibrium.What effect will adding 2.3 mole of Rn to the reaction mixture have on the system? 2 H₂S(g)+ 3 O₂(g)⇌ 2 H₂O(g)+ 2 SO₂(g)

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

What is Δn for the following equation in relating K_c to K_p? N₂(g)+ 3 F₂(g)⇌ 2 NF₃(g)

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO₂(g). NH₂COONH₄(s)⇌ 2 NH₃(g)+ CO₂(g)K_c = 1.58 × 10^-8 [NH₃]_eq = 2.3 × 10^-3 M

Consider the following reaction: 2 H₂O(g)+ 2 SO₂(g)⇌ 2 H₂S(g)+ 3 O₂(g) A reaction mixture initially contains 2.8 M H₂O and 2.6 M SO₂.Determine the equilibrium concentration of H₂S if K_c for the reaction at this temperature is 1.3 × 10^-6.

Consider the following reaction and its equilibrium constant: I₂(g)+ Br₂(g)⇌ 2 IBr(g)K_c = 1.1 × 10² A reaction mixture contains 0.37 M I₂,0.30 M Br₂and 3.5 M IBr.Which of the following statements is TRUE concerning this system?

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

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

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of H₂O(g). C₂H₄(g)+ H₂O(g)⇌ C₂H₅OH(g)K_c = 9.0 × 10³ [C₂H₄]_eq = 0.015 M [C₂H₅OH]_eq = 1.69 M

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

Express the equilibrium constant for the following reaction. Pb(NO₃)₂(aq)+ 2 NaI(aq)⇌ PbI₂(s)+ 2 NaNO₃(aq)

Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction: PCl₃(g)+ Cl₂(g)⇌ PCl₅(g) An equilibrium mixture at 450 K contains = 0.124 atm, = 0.157 atm,and = 1.30 atm.What is the value of K_p at this temperature?

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

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