For the given reaction, choose the correct expression of $$K_C$$ from the following: $$\text{Fe}^{3+}_{(aq)} + \text{SCN}^-_{(aq)} \rightleftharpoons (\text{FeSCN})^{2+}_{(aq)}$$

We need to write the equilibrium constant expression ($$K_C$$) for the reaction:

$$ Fe^{3+}_{(aq)} + SCN^-_{(aq)} \rightleftharpoons (FeSCN)^{2+}_{(aq)} $$

For a general reaction $$aA + bB \rightleftharpoons cC + dD$$ in solution, the equilibrium constant in terms of molar concentrations is:

$$ K_C = \frac{[C]^c[D]^d}{[A]^a[B]^b} $$

Products go in the numerator and reactants go in the denominator, each raised to the power of their stoichiometric coefficient.

Here, the stoichiometric coefficients are all 1:

- Product: $$[FeSCN^{2+}]$$ with coefficient 1

- Reactants: $$[Fe^{3+}]$$ with coefficient 1 and $$[SCN^-]$$ with coefficient 1

$$ K_C = \frac{[FeSCN^{2+}]}{[Fe^{3+}][SCN^-]} $$

The correct answer is Option (1): $$K_C = \frac{[FeSCN^{2+}]}{[Fe^{3+}][SCN^-]}$$.