For a reaction

2H_2O_2 \xrightarrow [\textup{alkaline medium}] {I^-} 2H_2O + O_2

the proposed mechanism is as given below :

  1. H_2O_2 + I^- \rightarrow H_2O + I^-O \ (slow)
  2. H_2O_2 + I^O- \rightarrow H_2O + I^ + O_2 \ (fast)

(i)    Write rate law for the reaction

(ii)    Write the overall order of reaction.

(iii)    Out of steps a and 2, which one rate determining step?

 

 

 

 
 
 
 
 

Answers (1)

(i) Rate law:

\textup{Rate} = -\frac{1}{2}\frac{d[H_2O_2]}{dt} = k[H_2O_2][I^-]

(ii) Order w.r.t H_2O_2 = 1

    Order w.r.t  [I^-] = 1

    Overall order = 2

(iii) Step 1 is the rate determining step as it is the slowest step.

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