Chemistry, 04.08.2019 22:30, kyliemorgan8623
Consider the following three-step representation of a reaction mechanism. step 1: a + b mc016-1.jpg ab (fast) and the rate = k[a][b] step 2: ab + b mc016-2.jpg ab2 (slow) and the rate = k[ab][b] step 3: ab2 + b mc016-3.jpg ab3 (fast) and the rate = k[ab2][b] overall: a + 3b mc016-4.jpg ab3 and the rate = k[a][b]2 which explains why the rate law for the overall equation is not the same as the rate equation for the rate-determining step?
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Consider the following three-step representation of a reaction mechanism. step 1: a + b mc016-1.jpg...
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