While ethanol (CH CH2OH) 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 3.7 atm of ethylene gas and 4.8 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 2.95 atm of ethylene gas and 4.05 atm of water vapor The engineer then adds another 1.2 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. m atm x10 ? Explanation Check O 2019 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy X

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