A mixture of 1 mole of H_2 O and 1 mole of CO is taken in a 10 litre container and heated to 725 K. At equilibrium 40 % of water by mass reacts with…

A mixture of $\displaystyle 1$ mole of $\displaystyle \mathrm{H}_2 \mathrm{O}$ and $\displaystyle 1$ mole of CO is taken in a $\displaystyle 10$ litre container and heated to $\displaystyle 725$ K . At equilibrium $\displaystyle 40 \%$ of water by mass reacts with carbon monoxide according to the equation: $\displaystyle \mathrm{CO}(\mathrm{g})+\mathrm{H}_2 \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}_2(\mathrm{~g})+\mathrm{H}_2(\mathrm{~g})$. The equilibrium constant $\displaystyle \mathrm{K}_{\mathrm{c}} \times 10^2$ for the reaction is $\displaystyle \_\_\_\_$. (Nearest integer)