Amixture initially contains a, b, and c in the following concentrations: [a] = 0.350 m , [b] = 0.650 m , and [c] = 0.300 m . the following reaction occurs and equilibrium is established: a+2b⇌c at equilibrium, [a] = 0.220 m and [c] = 0.430 m . calculate the value of the equilibrium constant, kc.

The value of equilibrium constant, for the given reaction is 12.85.

Explanation:

For the given chemical equation:

At t = 0      0.350M     0.650M      0.300M

At  (0.350 - x)    (0.650 - 2x)     (0.300 + x)

We are given:

Equilibrium concentration of A = 0.220 M

Forming an equation for concentration of A at equilibrium:

Thus, the concentration of B at equilibrium becomes =

Equilibrium concentration of C = 0.430 M

The expression of for the given chemical equation is:

Putting values in above equation:

Hence, the value of equilibrium constant, for the given reaction is 12.85.

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