The equilibrium constant of the reaction ${\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)+\mathrm{CO}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$, is 0.44 at 1259 K. The value of equilibrium constant of the reaction

${\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)+\mathrm{CO}\left(\mathrm{g}\right)$

will be

$K_{\text{new }}=1/K_{\text{old }}=1/0.44=2.27$

a number that represents the proportionality of the reactant and product concentrations at equilibrium in a reversible chemical reaction at a certain temperature.