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 75 L tank with 10. mol of ethylene gas and 5.4 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 6.8 mol of ethylene gas and 2.2 mol of water vapor. The engineer then adds another 1.4 mol of water, 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 75 L tank with 10. mol of ethylene gas and 5.4 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 6.8 mol of ethylene gas and 2.2 mol of water vapor. The engineer then adds another 1.4 mol of water, 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 ?
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.101PAE: 12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to...
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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 75 L tank with 10. mol of ethylene gas and 5.4 mol of water vapor. When the mixture
has come to equilibrium he determines that it contains 6.8 mol of ethylene gas and 2.2 mol of water vapor.
The engineer then adds another 1.4 mol of water, 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
x10
O
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