The Gibbs energies of formation, \(\Delta G_{\mathrm{f}}^{\circ},\) for
\(\mathrm{Na}_{2} \mathrm{O}(\mathrm{s})\) and \(\mathrm{Na}_{2}
\mathrm{O}_{2}(\mathrm{s})\) are \(-379.09 \mathrm{kJ} \mathrm{mol}^{-1}\) and
\(-449.63 \mathrm{kJ} \mathrm{mol}^{-1}\)
respectively, at 298 K. Calculate the equilibrium constant for the reaction
below at \(298 \mathrm{K} .\) Is \(\mathrm{Na}_{2} \mathrm{O}_{2}(\mathrm{s})\)
thermodynamically stable with respect to \(\mathrm{Na}_{2}
\mathrm{O}(\mathrm{s})\) and \(\mathrm{O}_{2}(\mathrm{g})\) at \(298 \mathrm{K} ?\)
$$
\mathrm{Na}_{2} \mathrm{O}_{2}(\mathrm{s}) \longrightarrow \mathrm{Na}_{2}
\mathrm{O}(\mathrm{s})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{g})
$$