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 5.6 mol of ethylene gas and 7.7 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 2.3 mol of ethylene gas and 4.4 mol of water vapor. The engineer then adds another 2.8 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 75 L tank with 5.6 mol of ethylene gas and 7.7 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 2.3 mol of ethylene gas and 4.4 mol of water vapor. The engineer then adds another 2.8 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

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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