March 08, 2021, 02:05:12 PM
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Topic: Rate determining step  (Read 100 times)

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Offline Roy16

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Rate determining step
« on: February 05, 2021, 07:26:22 AM »
Hi, I am currently studying on the iodination of acetone. I have discovered that acetone and H+ both have an order of reaction of 1 while I2 has a zero order. This results in a raw law of: k[acetone]1[H+]1. I have attached an image for reference.

However, given a reaction mechanism (attached below), the 2nd elementary step was known to be the rate determining step (rds). Since it contains an intermediate, I substituted it with [acetone] and [H+] (derived from the first step). But, this leaves me with a rate law of: k[acetone][H+][H2O], which is not equal to the experimentally determined rate law.

Is water meant to be in the rate law? Or is there some misconception that I'm having?

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