Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is: C2H4(g) + H2O(g) → C2H5OH(l) Water is present in excess. What is the percent yield when 42.7 g of ethylene is reacted, and 45.6 g of ethanol is collected
Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is: C2H4(g) + H2O(g) → C2H5OH(l) Water is present in excess. What is the percent yield when 42.7 g of ethylene is reacted, and 45.6 g of ethanol is collected
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter4: Stoichiometry
Section: Chapter Questions
Problem 4.14PAE: 4.14 The combustion of liquid chloroethylene, C2H3Cl, yields carbon dioxide, steam, and hydrogen...
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Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is:
C2H4(g) + H2O(g) → C2H5OH(l)
Water is present in excess. What is the percent yield when 42.7 g of ethylene is reacted, and 45.6 g of ethanol is collected?
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