$[25]$ Methane is oxidized to produce formaldehyde and water vapor in a continuous reactor,

$C{H}_4(g)+O_2(g)$HCHO$(g)+H_{2}O(v)$

A competing reaction also occurs in the reactor, which is the combustion of methane,

$C{H}_4(g)+2O_2(g)C{O}_2(g)+2H_{2}O(v)$

$20mo\frac{l}{h}$ of $C{H}_4$ is fed to a reactor. Pure $O_2$ is fed in excess at $30mo\frac{l}{h}\mathrm{.}60\%$ of the methane remains

unreacted and exits the reactor. Of the converted methane, $3mo{l}^{m}C{H}_4$ is oxidized to form HCHO

for $1molo{f}_{C{H}_4}$ burned to $C{O}_2($formaldehyde and carbon dioxide are in a ratio of $3$ to $1).$

$($a$)[15]$ Draw and label the flowchart with a basis including units.

$($b$)[10]$ Perform degree of freedom analysis on the reactor.

$($c$)[15]$ Write down the equations and specifications.

$($d$)[10]$ Calculate the molar flow rates of the components in the reactor exit stream.