Question

For the following reaction: A(g) + 2 B(g) ⇌ 2 C(g) Calculate the equilibrium constant K given the following information: The initial pressure of A is 2.755 bar and the initial pressure of B is 1.582 bar The equilibrium pressure of C is 0.460 bar B)For the following reaction: 2 A(g) + B(g) ⇌ C(g) Calculate the equilibrium constant K given the following information: The initial pressure of A is 2.772 bar and the initial pressure of B is 2.645 bar The equilibrium pressure of C is 0.739 bar C)For the following reaction: A(aq) + B(aq) ⇌ 2 C(aq) Given the following information, what is the equilibrium concentration of C in mol L-1? Initial concentration of A = 1.081 mol L-1 Initial concentration of B = 1.081 mol L-1 Initial concentration of C = 0 mol L-1 K = 6.1 x 10-5

Answer 1

              A(g) +    2 B(g) ⇌ 2 C(g)

I              2.755       1.582       0

C            -0.23       -2*0.23    2*0.23

E            2.525        1.122       0.46

          Kc    = [C]^2/[A][B]^2

                = (0.46)^2/2.525*(1.122)^2   = 0.067

B.

   2 A(g)    +    B(g)   ⇌ C(g)

I           2.772         2.645        0

C         -2*0.739     -0.739       0.739

E       1.294            1.906 0.739

      kc   =    [C]/[A]^2[B]

              =   0.739/(1.294)^2*1.906

               = 0.232

C.

        A(aq)    +    B(aq) ⇌ 2 C(aq)

I       1.081          1.081       0

C     -x                  -x            2x

E     1.081-x       1.081-x       2x

           Kc   = [C]^2/[A][B]

           6.1*10^-5   = (2x)^2/(1.081-x)(1.081-x)

          6.1*10^-5    = (2x/1.081-x)^2

          0.0078         = 2x/1.081-x

         0.0078*(1.081-x) = 2x

             x   = 0.0042

     [C]   = 2x    = 2*0.0042   = 0.0084M