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For a consecutive reaction, if the rate constant for the second step \mathrm{(B \rightarrow C)} is much Greater than the rate constant for the first step \mathrm{(A \rightarrow B)},what will be the overall rate expression for the formation of \mathrm{C} ?

Option: 1

\mathrm{R a t e=k_{1}(A)}


Option: 2

\mathrm{Rate =k_{2}[B]}


Option: 3

\mathrm{Rate =k_{1}k_{2}[A]}


Option: 4

\mathrm{Rate=\left(k_{1}+k_{2}\right)[A] }


Answers (1)

best_answer

In a consecutive reaction, the overall rate of formation of \mathrm{C} is determined by the rate constants of both steps The rate expression will be the product of the rate constants i.e \mathrm{k_{1},k_{2}[A]}.

 

Posted by

jitender.kumar

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