1) Define dynamic equilibrium.

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

2) Which of the following statements is FALSE?

A) When K >> 1, the forward reaction is favored and essentially goes to completion.

B) When K << 1, the reverse reaction is favored and the forward reaction does not proceed to a great extent.

C) When K ≈ 1, neither the forward or reverse reaction is strongly favored, and about the same amount of reactants and products exist at equilibrium.

D) K >> 1 implies that the reaction is very fast at producing products.

E) None of the above.

3) Give the direction of the reaction, if K >> 1.

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.

4) Give the direction of the reaction, if K << 1.

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.

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

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.

6) Express the equilibrium constant for the following reaction.

CH4(g) + 2 O2(g) –> CO2(g) + 2 H2O(g)

7) The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant.

H2(g) + Br2(g) <—-> HBr(g) Kc = 3.8 x 104

HBr(g) <—-> H2(g) + Br2(g) Kc = ?

A) 1.9 x 104

B) 5.3 x 10-5

C) 2.6 x 10-5

D) 6.4 x 10-4

E) 1.6 x 103

8) Express the equilibrium constant for the following reaction.

Pb(NO3)2(aq) + 2 NaI(aq) –> PbI2(s) + 2 NaNO3(aq)

9) Express the equilibrium constant for the following reaction.

4 Al(s) + 3 O2(g) –> 2 Al2O3(s)

10) Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [P4O10]eq = 2.000 moles, [P4]eq = 3.000 moles, [O2]eq = 4.000 M

P4O10(s) –> P4(s) + 5 O2(g)

A) 20.00

B) 4.000

C) 1.320

D) 1536

E) 1024

11) Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 3.6 M, [O2]eq = 4.1 M, [N2O]eq = 3.3 ? 10-18 M.

2 N2(g) + O2(g) ? 2 N2O(g)

A) 2.2 x 10-19

B) 4.5 x 1018

C) 2.0 x 10-37

D) 5.0 x 1036

E) 4.9 x 10-17

12) Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 1.5 M, [H2]eq = 1.1 M, [NH3]eq = 0.47 M.

N2(g) + 3 H2(g) –>2 NH3(g)

A) 3.5

B) 0.28

C) 9.1

D) 0.11

E) 0.78

13) Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [HCl]eq = 0.13 M, [HI]eq = 5.6 ? 10-16 M, [Cl2]eq = 0.0019 M.

2 HCl(g) + I2(s) ? 2 HI(g) + Cl2(g)

A) 8.2 x 10-18

B) 2.8 x 1031

C) 1.2 x 1017

D) 1.4 x 10-19

E) 3.5 x 10-32

14) Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [HCl]eq = 0.13 M, [HI]eq = 5.6 ? 10-16 M, [Cl2]eq = 0.0019 M.

2 HI(g) + Cl2(g) –> 2 HCl(g) + I2(s)

A) 8.2 x 10-18

B) 2.8 x 1031

C) 1.2 x 1017

D) 1.4 x 10-19

E) 3.5 x 10-32

15) Calculate the value of [N2]eq if [H2]eq = 2.0 M, [NH3]eq = 0.5 M, and Kc = 2.

N2(g) + 3 H2(g) –> 2 NH3(g)

A) 0.016 M

B) 0.031 M

C) 0.062 M

D) 0.40 M

E) 62.5 M

16) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO3(g).

2 SO2(g) + O2(g) –> 2 SO3(g) Kc = 1.7 ? 108

[SO2]eq = 0.0034 M [O2]eq = 0.0018 M

A) 1.9 M

B) 1.0 x 103 M

C) 0.53 M

D) 9.6 x 10-4 M

E) 0.73 M

17) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO2(g).

2 SO2(g) + O2(g) –> 2 SO3(g) Kc = 1.7 x 108

[SO3]eq = 0.0034 M [O2]eq = 0.0018 M

A) 2.8 x 1013 M

B) 1.88 M

C) 6.1 x 10-6 M

D) 1.0 x 103 M

E) 1.4 M

18) Which of the following is true about a system at equilibrium?

A) The concentration(s) of the reactant(s) is equal to the concentration(s) of the product(s).

B) No new product molecules are formed.

C) The concentration(s) of reactant(s) is constant over time.

D) The rate of the reverse reaction is equal to the rate of the forward reaction and both rates are equal to zero.

E) None of the above (A-D) is true.

19) For a particular system at a particular temperature there ______ equilibrium constant(s) and there _______ equilibrium position(s).

A) are infinite; is one

B) is one; are infinite

C) is one; is one

D) are infinite; are infinite

E) none of these

20) Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system?

CuS(s) + O2(g) –> Cu(s) + SO2(g)

A) The equilibrium constant will decrease.

B) No effect will be observed.

C) The reaction will shift to the right in the direction of products.

D) The equilibrium constant will increase.

E) The reaction will shift to the left in the direction of reactants.

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