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.
Concept: Rate of a Chemical Reaction
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