The initial$-$rate data in the table above were obtained for the reaction represented below. What is the experimental rate law for this reaction?

$2NO(g)+O_2(g)N{O}_2(g)$

A$)$ Rate $=k[NO][O_2]$

B$)$ Rate $=k[NO][O_2{]}^2$

$($C$)$ Rate $=k[NO{]}^2[O_2]$

D$)$ Rate $=k[NO{]}^2[O_2{]}^2$

E$)$ Rate $=k\frac{NO}{O_2}$