In the Deacon process for the manufacture of chlorine, $HCl$ and $O_2$ react to form $C{l}_2$ and $H_{2}O$ according to the reaction equation:

$4HCl+O_{2}2C{l}_2+2H_{2}O$

Sufficient air $(21$mol$\%O_2,79\%N_2)$ is fed to provide $35\%$ excess oxygen and the fractional conversion of $HCl$ is $85\%.$ If $100$molHCl is fed to the reactor:

$($a$)$ Draw and label a flowchart of the process and do a degree$-$of$-$freedom analysis.

$($b$)$ Calculate the mole fractions of the product stream components using atomic species balances in your calculation.

$($c$)$ Again calculate the mole fractions of the product stream components, only this time use the extent of reaction in the calculation.