Ethanol is produced commercially by the hydration of ethylene:

C2H4 + H2O --> C2H5OH

Some of the product is converted to diethyl ether in the side reaction:

2 C2H5OH --> (C2H5)2O +H2O

The feed to the reactor contains ethylene, steam, and an inert gas. A sample of the reactor effluent gas is analyzed and found to contain 43.3 mole % ethylene, 2.5 % ethanol, .14 % ether, 9.3 % inerts, and the balance water.

A) Take as a basis 100 mole of effluent gas, draw and label a flowchart, and do a degree-of-freedom analysis based on atomic species to prove that the system has zero degrees of freedom. Your first attempt is likely to yield D. F. = -1 meaning that either you counted one too many independent balances, you forgot to label one unknown variable, or the problem statement contains one redundant - and possibly inconsistent - process variable specification.

B) Calculate the molar composition of the reactor feed, the percentage conversion of ethylene, the fractional yield of ethanol, and the selectivity of ethanol production in relative to ether production.

C) The percentage conversion of ethylene you calculated should be very low. Why do you think the reactor would be designed to consume so little of the reactant? (Hint: if the reaction mixture remained in the reactor long enough to use up most of the ethylene, what would the main product contituent probably be?) What additional processing steps are likely to take place downstream from the reactor?