${\mathrm{CH}}_3\mathrm{OH}\text{, }$ methanol can be prepared from CO and ${\mathrm{H}}_2$

$\mathrm{CO}\left(\mathrm{g}\right)+2{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CH}}_3\mathrm{OH}\left(\mathrm{g}\right)$ The value of $K_p$ at 500 K is $6.23\times {10}^{-3}$

What total pressure (in atm) at equilibrium is required to convert $25\%$ of CO to ${\mathrm{CH}}_3\mathrm{OH}$ at 500 K If CO and ${\mathrm{H}}_2$ comes from

${\mathrm{CH}}_4\left(g\right)+{\mathrm{H}}_2\mathrm{O}\left(g\right)⟶\mathrm{CO}\left(g\right)+3{\mathrm{H}}_2\left(g\right)$

Give your answer excluding decimal places