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 125L tank with 45.mol of ethylene gas and 39.mol of water vapor. When the mixture has come to equilibrium she determines that it contains 21.mol of ethylene gas and 15.mol of water vapor. The engineer then adds another 23.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.