Methane is converted to hydrogen via the steam reforming reaction

$C{H}_4(g)+H_{2}O(g)>CO(g)+3H_2(g)$

Calculate the equilibrium composition for an equimolar feed of the reactants given that the equilibrium constant is given by the relation

$ln(K)=25\mathrm{.}8-\frac{24800}{T}.$ The temperature, $T$ is $600K$ and the pressure is $1$atm.

$($b$)$ What will be the effect of pressure on the equilibrium reaction composition? Calculate the compositions for $P=0\mathrm{.}5$atm and $P=1\mathrm{.}5$atm to support your conclusions.