Problem 2 Your boss asks you to isothermally carry out a liquid-phase, irreversible reaction A B with the following rate law: - r = kC with k = 0.20 L(mol*min)! a. Starting with a mole balance (& assumptions), calculate the time it would take a batch reactor to process your feed to achieve 95% conversion. The batch reactor is initially charged with 10 mol of pure A and the reactor size is 2L. b. Again starting with a mole balance, calculate the residence time t (reactor volume/flow rate through reactor) it would take a PFR to process your feed to achieve 95% conversion. The PFR has an inlet feed of pure A at a rate of 10 mol/min and the volumetric flow rate is 2 L/min. c. Compare your results in a) and b) and explain their relationship. d. Starting with a mole balance (& assumptions), calculate the volume it would take for a CSTR to process your feed (from part b) to achieve 95% conversion. e. Calculate the residence time for the CSTR in part d and compare it to part b. Which reactor yields the higher conversion given the same residence time? f. Now suppose instead that the reaction exhibits negative second-order kinetic behavior (i.e. -r= kC ?). How does this influence your decision in e) and why? Which reactor yields the higher conversion, given the same residence time? g. If the given reaction exhibited zero-order kinetic behavior (i.e. n = 0) instead, how does this influence your decision in e) and why? Briefly explain your conclusion