Determine the rate law and the rate constant for the reaction below given the data

presented in the table.

$N_2(g)+O_2(g)-2NO(g)$

Experiment Initial $O_2$ Initial $N_2$ Initial Rate $(\frac{M}{s})$

Rate $=1\mathrm{.}2M^{-2}{s}^{-1}[N_2][O_2{]}^{\frac{1}{2}}$

Rate $=1\mathrm{.}2{10}^5{M}^{-\frac{1}{2}}{s}^{-1}[N_2][O_2{]}^{\frac{1}{2}}$

Rate $=1\mathrm{.}2{10}^5{M}^{-\frac{1}{2}}{s}^{-1}[N_2][O_2]$

Rate $=2\mathrm{.}4{10}^5{M}^{\frac{1}{2}}{s}^{-1}[N_2][O_2{]}^{\frac{1}{2}}$

Rate $=1{10}^6{M}^{-\frac{1}{2}}{s}^{-1}[N_2{]}^2[O_2{]}^{\frac{1}{2}}$