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 75L tank with 36. Mol of ethylene gas and 9.5 mol of water vapor. When the mixture has come to equilibrium she determines that it contains 32.3 mol of ethylene gas and 5.8 mol of water vapor. The engineer then adds another 12. 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.