A mixture of 1 mole of H₂O 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 carbon monoxide according to the equation: $\mathrm{CO}\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CO}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)$. The equilibrium constant ${\mathrm{K}}_{\mathrm{c}}\times {10}^2$for the reaction is _____________. (Nearest integer)

                                                              ${\mathrm{CO}}_{\left(\mathrm{g}\right)}+{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}\underset{ }{\rightleftharpoons }{\mathrm{CO}}_{2\left(\mathrm{g}\right)}+{\mathrm{H}}_{2\left(\mathrm{g}\right)}$
Initial concentrations  $(\mathrm{mole}.{\mathrm{lit}}^{-1})$   0.1       0.1                  0                 0
Reacted to reach equilibrium            -0.04     -0.04             +0.04       +0.04
Reacted to reach equilibrium            0.06        0.06              0.04          0.04
Equilibrium constant ${\mathrm{K}}_{\mathrm{C}}=\frac{{\left[{\mathrm{CO}}_2\right]}^1{\left[{\mathrm{H}}_2\right]}^1}{{\left[\mathrm{CO}\right]}^1{\left[{\mathrm{H}}_2\mathrm{O}\right]}^1}$
$\begin{array}{l}=\frac{(0.04)(0.04)}{(0.06)(0.06)}\\ =0.4444\end{array}$
Nearest integer of ${\mathrm{K}}_{\mathrm{C}}\times {10}^2=44$