Choose the correct molecularity and rate law for each of the elementary reactions shown below.

$($a$)NO(g)+O(g)N{O}_2(g)$

Rate Law:

Rate $=k[NO{]}^2[O{]}^2$

Rate $=k[N{O}_2{]}^2$

Rate $=k[N{O}_2]$

Rate $=k[NO][O]$

Molecularity:

Rate $=k[N{O}_2{]}^2$

Rate $=k[N{O}_2]$

Rate $=k[NO][O]$

$($b$)NOC{l}_2(g)NO(g)+C{l}_2(g)$

Rate Law:

$($c$)C{H}_4(g)+Cl(g)C{H}_3(g)+HCl(g)$

Rate Law:

Rate $=k[C{H}_4{]}^2[Cl{]}^2$

Molecularity:

Rate $=k[C{H}_3][HCl]$

Rate $=k[C{H}_4][Cl]$

Rate $=k[C{H}_3{]}^2[HCl{]}^2$

$($d$)2C{H}_{3}O(g)C\frac{H_3}{O}OC{H}_3(g)$

Rate Law:

Rate $=k[C{H}_{3}O]$

Rate $=k[C\frac{H_3}{O}OCH]$

Rate $=k[C{H}_{3}O{]}^2$

Rate $=k[C\frac{H_3}{O}OCH{]}^2$

$($e$)N_2{O}_4(g)2N{O}_2(g)$

Rate Law:

Rate $=k[N{O}_2{]}^2$

Rate $=k[N_2{O}_4{]}^2$

Rate $=k[N{O}_2]$

Rate $=k[N_2{O}_4]$

Molecularity:

Rate $=k[N_2{O}_4{]}^2$

Rate $=k[N{O}_2]$

Rate $=k[N_2{O}_4]$