While ethanol is produced naturally by fermentation, e. g. in beer- and wine-making, industrially it is synthesized by reacting ethylene with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 1.5 L tank at 12 °C with of ethylene gas and 4.7 atm of water vapor. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains 1.16 atm of ethylene gas and 4.06 atm of water vapor. The engineer then adds another 1.2 atm 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.