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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 100 L tank with 22. mol of ethylene gas and 46. mol of water vapor. When the mixture has come to equilibrium she determines that it contains 4.0 mol of ethylene gas and 28. mol of water vapor. The engineer then adds another 12. 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 0 x10 X

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 100 L tank with 22. mol of ethylene gas and 46. mol of water vapor. When the mixture has come to equilibrium she determines that it contains 4.0 mol of ethylene gas and 28. mol of water vapor. The engineer then adds another 12. 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 0 x10 X

Chemistry: The Molecular Science
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 61QRT
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While ethanol (CH3CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH₂ CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 100 L tank with 22. mol of ethylene gas and 46. mol of water vapor. When the mixture has come to equilibrium she determines that it contains 4.0 mol of ethylene gas and 28. mol of water vapor. The engineer then adds another 12. 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 X
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 (CH₂ CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 100 L tank with 22. mol of ethylene gas and 46. mol of water vapor. When the mixture has come to equilibrium she determines that it contains 4.0 mol of ethylene gas and 28. mol of water vapor. The engineer then adds another 12. 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 X
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