Calculate the equilibrium constant, K for the following reaction at 400K?
`2NOCl_((g))iff2NO_((g))+Cl_(2(g))`
Given that `Delta_(r)H^(0)=80.0KJmol^(-1)` and `Delta_(r)S^(0)=120JK^(-1)mol^(-1)` at 400 K.

Explanation

To calculate the equilibrium constant \( K \) for the reaction

\[ 2 \text{NOCl}_{(g)} \iff 2 \text{NO}_{(g)} + \text{Cl}_{2(g)} \]

at 400 K, we will use the Gibbs free energy change (\( \Delta G^\circ \)) and the relationship between \( \Delta G^\circ \) and the equilibrium constant \( K \).

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