Formaldehyde $(C{H}_{2}O)$ is produced industrially by the catalytic oxidation of methanol $(C{H}_{3}OH)$ by the following reaction:

$C{H}_{3}OH+\frac{1}{2}{O}_{2}C{H}_{2}O+H_{2}O$

Unfortunately, under the conditions used to produce formaldehyde at a profitable rate, a significant portion of the formaldehyde can react with oxygen to produce $CO$ and $H_{2}O$ :

$C{H}_{2}O+\frac{1}{2}{O}_{2}CO+H_{2}O$

Assume that methanol and twice the reactor, that $90\%$ conversion of the methanol results, and that a $75\%$ yield of formaldehyde occurs. Determine the composition of the product gas leaving the reactor.