While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 50 L tank with 9.0 mol of ethylene gas and 11. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 4.9 mol of ethylene gas and 6.9 mol of water vapor. The engineer then adds another 3.0 mol of ethylene, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. mol
While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 50 L tank with 9.0 mol of ethylene gas and 11. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 4.9 mol of ethylene gas and 6.9 mol of water vapor. The engineer then adds another 3.0 mol of ethylene, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. mol
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 54P
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Transcribed Image Text:While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene
(CH,CH,) with water vapor at elevated temperatures.
A chemical engineer studying this reaction fills a 50 L tank with 9.0 mol of ethylene gas and 11. mol of water vapor. When the mixture has come to equilibrium
he determines that it contains 4.9 mol of ethylene gas and 6.9 mol of water vapor.
The engineer then adds another 3.0 mol of ethylene, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is
reached the second time. Round your answer to 2 significant digits.
|mol
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