Calculate \(\Delta G^{0}\) for the hydrogenation of ethylene at \(298 \mathrm{~K}\) using the following data:

\(\Delta G_{f, 298}^{0}\) for \(\mathrm{C}_{2} \mathrm{H}_{4}=68.12 \mathrm{~kJ} / \mathrm{mol}\)

\(\Delta G_{f, 298}^{0}\) for \(\mathrm{C}_{2} \mathrm{H}_{6}=-32.89 \mathrm{~kJ} / \mathrm{mol}\).

The reaction involved is

\[ \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{~g})+\mathrm{H}_{2}(\mathrm{~g}) \rightarrow \mathrm{C}_{2} \mathrm{H}_{6}(\mathrm{~g}) \]