Formaldehyde $(CH{O}_2)$ is produced industrially by the catalytic oxidation of methanol $(C{H}_{3}OH)$ by the following reaction:

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

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 $H_{2}O$ :

$C{H}_{2}O+\frac{1}{2}{O}_2$cdotsCO$+H_{2}O$

Assume that methanol and twice the stoichiometric amount of air needed for complete oxidation of the $C{H}_{3}OH$ are fed to the reactor, that $90\%$ conversion of the methanol to formaldehyde results, and that a $75\%$ yield of formaldehyde occurs $[$based on the theoretical production of $C{H}_{2}O$ by Reaction $(1)].$ Determine the composition of the product gas leaving the reactor.

$[7]$