Determine the value of kc for the following reaction if the equilibrium concentrations are as follows

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)

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

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 × 104

HBr(g) –> H2(g) + Br2(g) Kc =   ?

  • A) 1.9 × 104
  • B) 5.3 × 10-5
  • C) 2.6 × 10-5
  • D) 6.4 × 10-4
  • E) 1.6 × 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 × 10-19
  • B) 4.5 × 1018
  • C) 2.0 × 10-37
  • D) 5.0 × 1036
  • E) 4.9 × 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 × 10-18
  • B) 2.8 × 1031
  • C) 1.2 × 1017
  • D) 1.4 × 10-19
  • E) 3.5 × 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 × 10-18
  • B) 2.8 × 1031
  • C) 1.2 × 1017
  • D) 1.4 × 10-19
  • E) 3.5 × 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 × 103 M
  • C) 0.53 M
  • D) 9.6 × 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 × 108

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

  • A) 2.8 × 1013 M
  • B) 1.88 M
  • C) 6.1 × 10-6 M
  • D) 1.0 × 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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