6. The acid-catalyzed reaction of acetone, CH3COCH3, with iodine can be represen

Question

6. The acid-catalyzed reaction of acetone, CH3COCH3, with iodine can be represented by the equation H + CH3COCH3 + I2 -> CH2ICOCH3 + H+ + I– It is found experimentally that the reaction is first-order with respect to both acetone and the hydrogen ion. The rate of the reaction is independent of the iodine concentration. Which of the following conclusions could be drawn from the experimental results?

1. The uncatalyzed reaction would have a different pathway.

2. Iodine is involved in the rate-determining step.

3. The reaction takes place stepwise.

A. 1 only B. 2 only C. 3 only D. 1 and 3 E. 1, 2, and 3

Explanation / Answer

1. The uncatalyzed reaction would have a different pathway: You can never predict any hypothetical data for an uncatalyzed reaction mechanistic pathway, just by looking at the catalyzed reaction. So, this can't be deduced.

2. Iodine is involved in the rate-determining step.Not true. If I2 was invloved, then the rate of the reaction would definitely depend on the I2 to some order.

3. The reaction takes place stepwise. this is a possibility because the I2 concentration does not affect the reaction, so most likely the stepwise mechanism involves a step with acetone and H+ which is the slowest/rate determining step, that's why involved in the reaction rate and the other step being the faster step which involves the I2, that's why the rate is independent of I2 concentration.

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