Ethanol can be produced using a chemical reaction by starting with the hydrocarbon ethylene. The hydration of ethylene $($C$2$H$4+$ H$20->$ C$2$H$5$OH$)$ creates ethanol, but some of the ethanol is converted to diethyl ether by a second reaction $(2$ C$2$H$5$OH $->($C$2$H$5)20+$ H$20).$

The feed to the reactor contains a gas mixture of ethylene and water at $225\backslash$deg C$.$ Ethylene enters at $138$ mol$/$hr$,$ and water enters at $305$ mol$/$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 $($mol$/$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?