The rate law for the reaction
`2H_(2(g))+2NO_((g)) to N_(2(g))+2H_(2)O_((g))` is given by rate `=-=k[H_(2)][NO]^(2)`
The reaction occurs in the following two steps:
(a) `H_(2(g))+2NO_((g)) to N_(2)O_((g))_H_(2)O_((g))`
`N_(2)O_((g))+ H_(2(g)) to N_(2(g))+H_(2)O_((g))`
What is the rate of `N_(2)O` in the mechanism ? What is the molecularity of each of the elementary stpes ?

Explanation

Rate of `N_(2)O=K[N_(2)O][H_(2)O]`
Molecularity for 1st step is 3
Molecularity for 2nd step is 2.