Iodine reacts with a ketone in aqueous solution to give an iodoketone. The stoichiometric equation is I2 + ketone S iodoketone + H+ + I-. The rate of the reaction can be measured by measuring the disappearance of I2 with time. Some data for initial rates and initial concentrations follow: " d [I 2 ]> dt (mol " 1 L s–1) [I 2 ] (mol L " 1 ) [ketone] (mol L " 1 ) [H # ] (mol L " 1 ) 7 * 10 -5 5 * 10 -4 0.2 1.0 * 10 -2 7 * 10 -5 3 * 10 -4 0.2 1.0 * 10 -2 1.7 * 10 -4 5 * 10 -4 0.5 1.0 * 10 -2 5.4 * 10 -4 5 * 10 -4 0.5 3.2 * 10 -2 a. Find the order of the reaction with respect to I2, ketone, and H+ . b. Write a differential equation expressing your findings in part (a) and calculate the average rate coefficient. c. How long will it take to synthesize 10 -4 mol L -1 of the iodoketone starting with 0.5 mol L -1 of ketone and 10 -3 mol L -1 of I 2 if the H + concentration is held constant at 10 -1 mol L -1 ? Will the reaction go faster if we double the concentration of ketone? Of iodine? Of H + ? How long will it take to synthesize 10 -1 mol L -1 of the iodoketone if all conditions are the same as above?