For the reaction $2NOBr(g) \rightarrow 2NO(g) + Br_2(g)$, the rate law is $r = k[NOBr]^2$. If the rate constant $k = 1.62 \text{ M}^{-1} \text{ s}^{-1}$ and the concentration of $NOBr$ is $5 \times 10^{-3} \text{ M}$, what is the rate of the reaction?

• A
  $4.05 \times 10^{-5} \text{ M s}^{-1}$
• B
  $4.05 \times 10^{-6} \text{ M s}^{-1}$
• C
  $1.62 \times 10^{-5} \text{ M s}^{-1}$
• D
  $8.10 \times 10^{-6} \text{ M s}^{-1}$