Consider the following reaction:
Fe3+(aq)+SCN−(aq) <> FeSCN2+(aq)
A solution is made containing an initial [Fe3+] of 1.1 x 10^−3 M and an initial [SCN−] of 7.8 x 10^−4 M . At equilibrium, [FeSCN2+]= 1.6 x 10^−4 M .
Part A) Calculate the value of the equilibrium constant (Kc).
Express your answer using two significant figures.

The value of the equilibrium constant is .

Explanation:

Initially

           0

At equilibrium :

           x

The concentration of at equilibrium is given ,x=

The expression of an equilibrium constant is given as;

Putting value of x:

The value of the

The value of the equilibrium constant is .

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