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?