The organic acid, ACOOH reacts reversibly with the alcohol, BOH, to form the ester ACOOB in the liquid phase according to the stoichiometric equation + + 2. The reverse reaction is much slower than the forward reaction under these operating conditions and so the reverse reaction can be neglected. The forward reaction is first order in ACOOH and second order in BOH and over-all third order. The reaction is to be carried out in solution in an ideal CSTR reactor. The reactor is to be operated isothermally at 298 K. The value of the rate constant k is 0.16 dm6/mol2-hr at 298 K, and the reaction has an activation energy of 25 kcal/mol. The initial concentration of ACOOH is 0.4 mol/dm3 and the initial concentration of BOH is 0.5 mol/dm3. The total inlet volumetric flow rate is 0.6 dm3/hr. (a) Use the CRE algorithm (mole balance, rate law, stoichiometry, etc.) to calculate the reactor volume needed to obtain a conversion of ACOOH of 80%? (b) Keeping the reactor volume constant as in (a), specify conditions (T, 0, CA0, and X) to double the moles of product ester produced per hour.