Determine the Rate Law and the Value of K for the Following

Determine the rate law and the value of k for the following reaction using the data provided:
2N₂O₅(g) → 4NO₂(g) + O₂(g) [N₂O₅]_i (M) Initial Rate (M^-1 s^-1)
$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ 0.093 $\quad$ 4.84 × 10^-4
$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ 0.186 $\quad$ 9.67 × 10^-4
$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ 0.279 $\quad$ 1.45 × 10^-3

A) Rate = 5.6 × 10^-2 M^-1 s^-1[N₂O₅]²
B) Rate = 6.0 × 10^-1 M^-2 s^-1[N₂O₅]³
C) Rate = 1.6 × 10^-3 M^1/2 s^-1[N₂O₅]^1/2
D) Rate = 1.7 × 10^-2 M^-1/2 s^-1[N₂O₅]^3/2
E) Rate = 5.2 × 10⁻³ s^-1[N₂O₅]