A mixture initially contains A, B, and C in the following concentrations: [A] = 0.600 M , [B] = 1.30 M , and [C] = 0.500 M . The following reaction occurs and equilibrium is established: A+2B⇌C At equilibrium, [A] = 0.410 M and [C] = 0.690 M . Calculate the value of the equilibrium constant, Kc.

Explanation:

Chemical equation for the given reaction is as follows.

Initial :    0.6       1.30           0.5

Final :   (0.6 - x)  (1.30 - 2x)  (0.5 + x)

It is given that at equilibrium, [A] = 0.410 M.

So,    x = (0.600 - 0.410)

           = 0.19 M

Hence, [B] will also be calculated as follows.

       [B] =

             = 0.92

Now, we will calculate the value of equilibrium constant as follows.

                  =      

                  =

                  = 1.988

Thus, we can conclude that the value of the equilibrium constant, is 1.988.

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