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 5.0 L flask with 1.0 atm of ethylene gas and 3.0 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 0.58 atm of ethylene gas and 2.58 atm of water vapor. The engineer then adds another 1.0 atm of water, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. atm x10 G

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 5.0 L flask with 1.0 atm of ethylene gas and 3.0 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 0.58 atm of ethylene gas and 2.58 atm of water vapor. The engineer then adds another 1.0 atm of water, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. atm x10 G

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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