while (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 75 L tank with 11. mol of ethylene gas and 22. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 4.5 mol of ethylene gas and 15.5 mol of water vapor. The engineer then adds another 7.3 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 (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 75 L tank with 11. mol of ethylene gas and 22. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 4.5 mol of ethylene gas and 15.5 mol of water vapor. The engineer then adds another 7.3 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: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 92QRT
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Transcribed Image Text:While ethanol (CH3CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene
(CH₂CH₂) with water vapor at elevated temperatures.
A chemical engineer studying this reaction fills a 75 L tank with 11. mol of ethylene gas and 22. mol of water vapor. When the mixture has come to equilibrium
he determines that it contains 4.5 mol of ethylene gas and 15.5 mol of water vapor.
The engineer then adds another 7.3 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
10
X
S
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