One mole of \(\mathrm{H}_2 \mathrm{O}\) and one mole of \(\mathrm{CO}\) are taken in 10 litre vessel and heated to \(725 \mathrm{~K}\). At equilibrium \(40 \%\) of water (by mass) reacts with \(\mathrm{CO}\) according to the equation,
\(\mathrm{H}_2 \mathrm{O}(\mathrm{g})+\mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{H}_2(\mathrm{~g})+\mathrm{CO}_2(\mathrm{~g})\)
Calculate the equilibrium constant for the reaction.