The reaction between NO and `Cl_(2)` takes place in the following two steps :
I `{:(" "k_(1)), (NO + Cl_(2) hArr NOCl_(2)), (" "k_(2)), (" ""fast"):}`
II. `NOCl_(2)underset("fast")overset(k_(2))rarr2NOCl`
The rate law of overall reaction,
`2NO+Cl_(2)to2NOCl` can be given by:

Options

A. rate= `k[NO]^(2)[Cl_(2)]`
B. rate= `k[NO][Cl_(2)]`
C. rate= k[NOCl][NO]
D. rate = `k[NO][Cl_(2)]^(2)`

Answer

A