If a mixture of \(1 \mathrm{~mol}\) of \(\mathrm{CO}(\mathrm{g}), 1 \mathrm{~mol}\) of \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\), and \(2 \mathrm{~mol}\) of \(\mathrm{He}(\mathrm{g})\) are fed into a reactor at 10 bar and \(1000 \mathrm{~K}\), the following reaction occurs to produce carbon dioxide and hydrogen gas:

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

The equilibrium constant for the reaction is 1.5. Calculate the degree of conversion and equilibrium composition of the reaction mixture, assuming that the mixture behaves like an ideal gas.