Ozone decomposes to oxygen gas. 2 O3(g) 3 O2(g) A proposed mechanism for this de

Question

Ozone decomposes to oxygen gas. 2 O3(g) 3 O2(g) A proposed mechanism for this decomposition is shown below. O3 O2 + O (fast, equilibrium) O3 + O 2 O2 (slow) What is the rate law derived from this mechanism?

Explanation / Answer

step 1 O3 ==> O2 + O (fast) step 2 O3 + O ==> 2 O2 (slow) The overall rate law can be determined from the slowest step, which is step 2 If you write the rate law based on the slow step, you can assume that the order with respect to each reactant is the same as the coefficient used in the slow step. rate = k[O3][O] Of course you cannot have a rate law that includes [O] because it is an intermediate, and not an actual reactant. The first step shows that O3 is involved in the formation of O, so when you do some substituting for O, you end up with a rate law that involves two molecules of O3 rate = k[O3]^2

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