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 75L tank with 16.mol of ethylene gas and 27.mol of water vapor. When the mixture has come to equilibrium she determines that it contains 9.6mol of ethylene gas and 20.6mol of water vapor. The engineer then adds another 9.0mol 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

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