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The Rate Law for the Reaction - Chemistry

The rate law for the reaction

`2H_(2(g))+2NO_((g))->N_(2(g))+2H_2O_((g))`

is given by rate= `K[H_2][NO]^2`

The reaction occurs in the following two steps:

a. `H_(2(g)) +2NO_((g))->N_2O_((g))+H_2O_((g))`

b. `N_2O_((g))+H_(2(g))->N_(2(g))+H_2O_((g))`

What is the role of N2O in the mechanism? What is the molecularity of each of the elementary steps?

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Solution

a. Role of N2O: N2O acts as an intermediate since it is produced in first step and consumed in second step. 

b. The first step is trimolecular/termolecular. The second step is bimolecular.

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