Ethanol can be produced using a chemical reaction by starting with the hydrocarbon ethylene. The hydration of ethylene $($:$C_2{H}_{5}OH\}$ creates ethanol, but some of the The feed to the reactor contains a gas mixture of ethylene and water at $225C.$ Ethylene enters at $138mo\frac{l}{h}r,$ and water enters at $305mo\frac{l}{h}.$ The fractional conversion of ethylene is $71\mathrm{.}2\%.$ The selectivity, which is defined as the ratio of ethanol production to diethyl ether production, is $2\mathrm{.}83.$

$($a$)$ Draw and label a process flow diagram. Clearly number each stream.

$($b$)$ Calculate the component molar flow rates $(mo\frac{l}{h})$ of the stream exiting the reactor.

$($c$)$ Calculate the fractional yield of ethanol $($ratio of ethanol produced to the ethylene consumed$).$

$($d$)$ Emmanuel, a clever engineer, adjusts the reactor conditions to double the selectivity. Will the molar flow rate of water exiting the reactor increase, decrease, or stay the same?