In a chemical laboratory, it is proposed to carry out the reaction

\[ \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(\mathrm{g}) \]

at 1 bar and \(298 \mathrm{~K}\). Calculate the standard Gibbs free energy change at \(298 \mathrm{~K}\) and predict whether it is feasible to carry out the given reaction or not. If possible, calculate the equilibrium constant.