Calculate the equilibrium constant at \(1000 \mathrm{~K}\) and 1 bar for the following reaction:

\[ \mathrm{CO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2}(\mathrm{~g}) \]

Assuming that the heat of reaction remains constant in the temperature range involved. Given that Equilibrium constant \(K\) at \(298 \mathrm{~K}\) and 1 bar \(1.1582 \times 10^{5}\)

\[ \begin{aligned} \Delta H_{f, \mathrm{CO}}^{0} & =-110.532 \mathrm{~kJ} \\ \Delta H_{f, \mathrm{H}_{2} \mathrm{O}}^{0} & =-241.997 \mathrm{~kJ} \\ \Delta H_{f, \mathrm{CO}_{2}}^{0} & =-393.978 \mathrm{~kJ} \end{aligned} \]