Iodine reacts with a ketone in aqueous solution to give an iodoketone. The stoichiometric equation is
I2 + ketone → 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[l2]/dt (mol-1 L s-1) | [l2] (mol L-1) | [ketone] (mol L-1) | [H+ ] (mol L-1) |
7 X 10- 5 | 5 X 10-4 | 0.2 | 1.0 X 10-2 |
7 X 10- 5 | 3 X 10-4 | 0.2 | 1.0 X 10-2 |
1.7 X 10-4 | 5 X 10-4 | 0.5 | 1.0 X 10-2 |
5.4 X 10-4 | 5 X 10-4 | 0.5 | 3.2 X 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 I2 if the H+ concentration is held con stant 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?
d. Propose a mechanism consistent with the experimental results.
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