Background:

A customer is considering our company as a new supplier of ethylene. The customer

requires the production of $10,000mo\frac{l}{?}$ day of pure ethylene. The contract is potentially

quite lucrative, and the company could use the business. Luckily, Save the World

Industries, INC has access to a cheap supply of ethane $(C_2{H}_6).$ Ethane is not very

reactive, but can be dehydrogenated to ethylene $(C_2{H}_4)$ in a catalytic packed bed

reactor. However, if the dehydrogenation reaction proceeds too far, acetylene $(C_2{H}_2)$ is

made. Acetylene is highly reactive, expensive to separate from other components, and

an explosion hazard $($safety limit is $10$mol$\%).$

Reaction $1$: $C_2{H}_6(g)harr{C}_2{H}_4(g)+H_2(g)$

Reaction $2$: $C_2{H}_4(g)harr{C}_2{H}_2(g)+H_2(g)$

The R&D department suggests that we feed a $1$:$1$ molar ratio of ethane and steam to

the reactor. Steam acts as a diluent and is not part of the reaction network. The R&D

department suggests running the reactor at $1000K$ and $1$atm for sufficient time to

reach equilibrium. The business department wants to remind you that higher flow rates

lead to higher equipment costs, as does operating under vacuum $(<mn\; id="EditorElement\_2215980">1</mn>$atm $).$

Action items:

For a single pass, determine the reactor ethylene yield and ethylene selectivity at

these conditions.

Calculate the ethylene yield and ethylene selectivity at equilibrium as a function of

reactor temperature from $800$ to $1400K.$ Plot your results on a graph. Use enough

points to show the curve's shape.

Determine the effect of altering the reactor pressure between $0\mathrm{.}15$ and $4\mathrm{.}0$atm on

the ethylene yield and ethylene selectivity at equilibrium. Plot your results on a

graph.

Determine the effect of altering the feed ratio between $3$:$1$ and $1$:$3$ ethane:steam on

the ethylene yield and ethylene selectivity at equilibrium. Plot your results on a

graph.