A mixture of 1 mole of $\mathrm{H}_{2} \mathrm{O}$ and 1 mole of $\mathrm{CO}$ is taken in a 10 litre container and heated to $725 \mathrm{~K}$. At equilibrium $40 \%$ of water by mass reacts with carbon monoxide according to the equation :

$\mathrm{CO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2}(\mathrm{~g})$.

The equilibrium constant $\mathrm{K}_{\mathrm{c}} \times 10^{2}$ for the reaction is ____________. (Nearest integer)