Calculate the equilibrium constant at \(750 \mathrm{~K}\) and 1 bar for the following reaction:

\[ \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CH}_{3} \mathrm{CHO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \]

Assume that the heat of reaction remains constant in the temperature range involved, given that the equilibrium constant \(K\) at \(298 \mathrm{~K}\) and 1 bar is \(1.1582 \times 10^{5}\). Use data table for standard heat of reaction.