Calculate the equilibrium constant, $K$, at $298 \mathrm{~K}$ for the reaction
$$
\mathrm{H}_{2} \mathrm{O}(\mathrm{D}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g})
$$
The standard Gibbs energy change of formation of $\mathrm{H}_{2} \mathrm{O}(\mathrm{l})$ at $298 \mathrm{~K}$ is - $237.1 \mathrm{~kJ} \mathrm{~mol}^{-1}$. (Section 15.3)