Medium
For the reaction $2 \ NOBr_{(g)} \rightarrow 2 \ NO_{(g)} + Br_{2_{(g)}}$,the rate law is $r = k[NOBr]^{2}$. If the rate constant is $1.62 \ M^{-1} \ s^{-1}$ and the concentration of $NOBr$ is $2.00 \times 10^{-3} \ M$,what is the rate of reaction?
- A$6.48 \times 10^{-6} \ M \ s^{-1}$
- B$4.05 \times 10^{-5} \ M \ s^{-1}$
- C$2.46 \times 10^{-6} \ M \ s^{-1}$
- D$5.24 \times 10^{-6} \ M \ s^{-1}$
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