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Given the following reaction mechanism: H2O2 to H2O+O   O+CF2Cl2 to ClO+CF2Cl     ClO+O3 to Cl+2O2    Cl+CF2Cl to...

Given the following reaction mechanism:

H2O2 to H2O+O  

O+CF2Cl2 to ClO+CF2Cl    

ClO+O3 to Cl+2O2   

Cl+CF2Cl to CF2Cl2

Steps:

1. Rate = k[H2O2]

2. Rate = k[O][CF2Cl2]

3. Rate = k[ClO][O3]

4. Rate = k[Cl][CF2Cl]

Which step would be the rate-limiting step if the reaction is found to be 1st order?

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Answer #1

H2O2 ----> H2O+O                          -----(1)

O+CF2Cl2 ----> ClO+CF2Cl             ----(2)

ClO+O3 ----> Cl+2O2                     ----(3)

Cl+CF2Cl ----> CF2Cl2                   ------(4)

On adding all these we get the overall equation as

H2O2 + O3 ---> H2O + 2O2

Given that the reaction is found to be 1st order so it involves one molecule of the reactant.among the given equations the rate with reactant is r = k[H2O2] (order with respect to H2O2 is 1)

We know that the slowest step is the rate determining step which involves one molecule of H2O2

So (i) is the slowest step of this reaction

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