While ethanol (CH₂CH₂OH) 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 17. mol of ethylene gas and 13. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 7.9 mol of ethylene gas and 3.9 mol of water vapor. The engineer then adds another 3.3 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 X

While ethanol (CH₂CH₂OH) 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 17. mol of ethylene gas and 13. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 7.9 mol of ethylene gas and 3.9 mol of water vapor. The engineer then adds another 3.3 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 X

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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