Difficult
For the reaction $2NOBr(g) \rightarrow 2NO(g) + Br_2(g)$, the rate law is $r = k[NOBr]^2$. If the rate constant $k = 1.62 \times 10^{-2} \text{ L mol}^{-1} \text{ s}^{-1}$ and the concentration of $[NOBr] = 2 \times 10^{-3} \text{ mol L}^{-1}$, what is the rate of reaction?
- A$6.48 \times 10^{-8} \text{ mol L}^{-1} \text{ s}^{-1}$
- B$3.24 \times 10^{-8} \text{ mol L}^{-1} \text{ s}^{-1}$
- C$1.62 \times 10^{-8} \text{ mol L}^{-1} \text{ s}^{-1}$
- D$8.10 \times 10^{-8} \text{ mol L}^{-1} \text{ s}^{-1}$
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