Quiz #4 – Writing and Calculating Keq

 

 

1. The equilibrium constant expression for the following reaction is

 

                        2Hg(l)  +  O2(g)               2HGO(s)

 

    A. Keq = 1/[O2]

 

    B. Keq = [O2]

 

    C. Keq = [2HgO] / [O2] [2Hg]

 

    D. Keq = [HgO]2 / [Hg]2[O2]

 

 

 

2.   Identify the equilibrium system that least favors the formation of products

 

    A. 2HgO(s)                 2Hg(l)  +  O2(g)                                             Keq = 1.2 x 10-22

    B. CH3COOH(aq)  +  H2O(l)               H3O+(aq) +  CH3COO-(aq)             Keq = 1.8 x 10-5

    C. 2NO(g)  +  O2(g)                      2NO2(g)                                                Keq = 6.5 x 105

    D. H2(g)  +  Cl2(g)                   2HCl(g)                                                  Keq = 1.8 x 1033

 

 

 

3. Consider the following equilibrium system

 

                        3O2(g)                  2O3(g)                  Keq = 1

 

    Which equation compares the concentration of oxygen and ozone?

 

    A. [O2] = [O3]2/5

    B. [O2] = [O3]

    C. [O2] = [O3]3/2

    D. [O2] 2/5 = [O3]

 

 

4. For which of the following equilibrium does Keq = [O2]

 

    A. O2(l)                     O2(g)

    B. 2O3(g)                   3O2(g)

    C. 2H2O(l)              2H2(g)  +  O2(g)

    D. 2Hg(s)  +  O2(g)                      2HgO(s)

 

 

5.  Consider the following equilibrium system at 25O C

 

                        2SO2(g)  +  O2(g)                 2SO3(g)

 

    At equilibrium, [SO2] is 4.00 x 10-3 mol/L and [SO3] is 2.33 x 10-3 mol/L.

    From this data, the Keq value for the above system is

 

    A. 6.85 x 10-3

    B. 1.18 x 10-2

    C. 84.8

    D. 146

 

 

6.Consider the following equilibrium system

 

                        PCl5(g)                     PCl3(g)  +  Cl2(g) 

 

    At equilibrium, [PCl5] is a 0.400 M. [PCl3] is 1.50 M and [Cl2] is 0.600 M. The Keq for the reaction is

 

    A. 0.360

    B. 0.444

    C. 0.900

    D. 2.25

 

 

7. Consider the following equilibrium

 

                                2H2S(g)                 2H2(g)   +  S2(g)

 

 

    At equilibrium, [H2S]  = 0.50 mol/L. [H2]  = 0.10 mol/L and [S2]  = 0.40 mol/L.

     The value of Keq is calculated using the ratio

 

    A  (0.10)(0.40)

            (0.50)

 

    B.  (0.10)2(0.40)

              (0.50)2

 

    C.     (0.50)         

        (0.10)(0.50)

 

    D.      (0.50)2

         (0.10)2(0.40)

 

 

8.  Consider the following equilibrium

 

                        2NO(g)  +  Cl2(g)                 2NOCl(g)          Keq  =  12 

 

     At equilibrium, [NOCl] = 1.60 mol/L  and [NO] = 0.80 mol/L. The [Cl2] is

 

    A. 0.17 mol/L

    B. 0.27 mol/L

    C. 0.33 mol/L

    D. 3.0   mol/L

 

 

9.  Consider the following equilibrium

 

                        I2(s)  +  H2O(l)                 H+(aq)  +  I-(aq)  +  HOI(aq)

 

    The equilibrium constant expression for the above system is

 

    A. Keq = [H+][I-]

 

    B. Keq = [H+][I-][HOI]

 

    C. Keq = [H+][I-][HOI]

                    [I2][H2O]

   

    D.  Keq = [H+][I-][HOI]

                        [H2O]

 

 

10. Consider the following equilibrium

 

                        2CO(g)  +  O2(g)                    2CO2(g)

 

    The ratio used to calculate the equilibrium constant is

 

    A. [2CO]2[O2]

           [2CO2]2

 

    B.    [2CO2]2

         [2CO]2[O2]

         

    C. [CO]2[O2]

           [CO2]2

 

    D.    [CO2]2

         [CO]2[O2]

 

 

 11. Consider the following equilibrium

 

                        2Fe(s)  +  3H2O(g)                      Fe2O3(s)  +  3H2(g)

 

      The equilibrium constant expression is

 

    A. Keq = [Fe2O3][H2]3

                   [Fe]2[H2O]3

 

    B. Keq =  [Fe2O3][3H2]

                   [2Fe] [3H2O]

 

    C. Keq = [H2]3

                 [H2O]3

 

    D. Keq = [H2]3

           

 

12. Consider the following equilibrium

 

                        4KO2(s)  +  2H2O(g)                       4KOH(s)  +  3O2(g)

 

     At equilibrium, the [N2O4] is equal to

 

    A.  0.133

          [NO2]

 

    B.  [NO2]

          0.133

 

    C.  0.133

          [NO2]2

 

    D.  [NO2]2

          0.133

 

 

13. Consider the following equilibrium

 

                        4KO2(s)  +  2H2O(g)                      4KOH(s)  +  3O2(g)

          

     The equilibrium constant expression is

 

    A. Keq = [KOH]4[O2]3

                   [KO2]4[H2O]2

 

    B. Keq = [O2]3

                 [H2O]2

 

    C. Keq = [KO2]4[H2O]2

                   [KOH]4[O2]3

                  

    D. Keq =  [H2O]2

                     [O2]3

 

14.  Consider the following equilibrium

 

                        C(s)  +  H2O(g)               CO(g)  +  H2(g)

 

     The contents of a 1.00 L container at equilibrium were analyzed and found to contain 0.20 mol C,

      0.20 mol H2O, 0.60 mol CO and 0.60 mol H2. The equilibrium constant is

 

 

    A. 0.11

    B. 0.56

    C. 1.8

    D. 9.0

 

 

 

15.  Consider the following equilibrium

 

                        N2O4(g)                 2NO2(g)          Keq = 4.61 x 10-3

 

     A 1.00 L container at equilibrium was analyzed and found to contain 0.0200 mol NO2.

     At equilibrium, the concentration of N2O4 is

 

    A. 0.0868 mol/L

    B. 0.230 mol/L

    C. 4.34 mol/L

    D. 11.5 mol/L

 

 

 

16.  Consider the following equilibrium

 

                        CH4(g)  +  H2O(g)                   CO(g)  +  3H2(g)             Keq= 5.7 

 

     At equilibrium, the [CH4] = 0.40 mol/L  [CO] = 0.30 mol/L and [H2] = 0.80 mol/L

     The [H2O] is

 

    A. 0.067 mol/L

    B. 0.11 mol/L

    C. 2.2 mol/L

    D. 5.3 mol/L

 

 

17. Consider the following equilibrium

 

                        H2(g)  +  I2(g)                        2HI(g)

 

     At equilibrium, the [H2] = 0.020 mol/L. [I2] = 0.020 mol/L and [HI] = 0.160 mol/L.

     The value of the equilibrium constant is

 

    A. 2.5 x 10-3

    B. 1.6 x 10-2

    C. 6.4 x 101

    D. 4.0 x 102

 

 

 

18. Consider the following constant expression

 

                        Keq = [Co2]

 

     Which one of the following equilibrium systems does the above expression represent?

 

    A. CO2(g)                  CO2(s)

    B. PbO(s)  + CO2(g)                 PbCO3(s)

    C. CaCO3(s)                          CaO(s) +  CO2(g)

    D. H2CO3(aq)                         H2O(l)  +  CO2(aq)

 

 

19. Given the following equilibrium system

                        Br2(g)                     Br2(l)

 

      The equilibrium constant expression for the above system is

 

    A. Keq = [BR2(l)]

                  [Br2(g)]

 

     B. Keq = [Br2(g)]

 

     C. Keq =      1 ­­­­__  

                    [Br2(g)]

 

    D. Keq = [BR2(g)] [Br2(g)]

                 

 

 

 

 

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