Consider the following reaction: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) A solution is made containing an initial [Fe3+] of 1.2×10−3 M and an initial [SCN−] of 8.0×10−4 M . At equilibrium, [FeSCN2+]= 1.8×10−4 M .

The question is incomplete, here is the complete question:

Consider the following reaction: A solution is made containing an initial of 1.2×10⁻³ M and an initial [SCN⁻] of 8.0×10⁻⁴ M . At equilibrium, [FeSCN²⁺]= 1.8×10⁻⁴ M.

Calculate the value of the equilibrium constant (Kc).

The value of for above equation is 284.63

Explanation:

We are given:

Initial concentration of

Initial concentration of

Equilibrium concentration of

The given chemical equation follows:

Initial:                            

At eqllm:                  x

Equilibrium concentration of

Equilibrium concentration of

The expression of for above equation follows:

Putting values in above equation, we get:

Hence, the value of for above equation is 284.63

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