Methanol (CH;OH) and acetic acid (CH;COOH) react in the gas phase to produce methyl acetate (CH;COOCH;) and water vapor (H2O). The reaction is reversible and subject to equilibrium. The equilibrium constant at the reaction temperature of operation is determined by the mole fractions of the four species as: K = y -=5.00 yAB where A denotes methanol, B denotes acetic acid, C denotes methyl acetate, and D denotes water vapor. (a) Write down the balanced chemical reaction. (b) If the feed to the reactor contains 1 mole of methanol, 1 mole of acetic acid, and no other species, calculate the equilibrium fractional conversion. (c) If 75 moles of methanol are fed with certain amount of acetic acid and the reaction proceeds to equilibrium, what are the mole fractions of the product stream if the final methyl acetate produced is found to be 70 moles?