Question

The decomposition of ozone in the stratosphere can occur by the following two-step mechanism:             Step...

The decomposition of ozone in the stratosphere can occur by the following two-step mechanism:

            Step 1: Br + O3 → BrO + O2

            Step 2: BrO + O → Br + O2

This question has multiple parts. Be sure to answer all of them!

(A) What is the overall reaction when steps 1 and 2 are added together?

(B) What is the intermediate in this reaction?

(C) What is the catalyst in this reaction?

(D) What is the molecularity of the first step?

(E) If step 1 were the rate determining, the slowest step, what would be the rate law for this reaction?

(F) If step 2 were the rate determining, the slowest step, what would be the rate law for this reaction?

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Homework Answers

Answer #1

A. adding step 1 and step 2 we have:

Br + O3 + BrO + O → BrO + O2 + Br + O2

Eliminating Br and BrO from both side we get

O3 + O → O2 + O2

Or, O3 + O → 2O2   This is overall reaction.

B. Here in step 1 BrO is produced which destroyed in step 2. So BrO is the intermidiate.

C. In step 1 Br reacts with O3 and at the end of the reaction at step 2, Br is reproduced. So Br is the catalyst.

D. Molecularity is the total number of coefficient of reactant. So molecularity of step 1 is 2. [2 reactants]

E. If step 1 is the rate determining step, then rate = K1 [Br] [O3] , where K1 is rate constant of step 1 and [X] is the concentration of X.

F. If step 2 is the rate determining step, then rate = K2 [BrO] [O] , where K2 is rate constant of step

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