For the first-order reaction $N_2O_5 \text{ (in } CCl_4) \rightarrow 2NO_2 + \frac{1}{2}O_{2(g)}$,the rate constant is $6.2 \times 10^{-4} \, s^{-1}$. What will be the rate of reaction when $[N_2O_5] = 1.25 \, mol \, L^{-1}$?
- A$7.75 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}$
- B$6.35 \times 10^{-3} \, mol \, L^{-1} \, s^{-1}$
- C$5.15 \times 10^{-5} \, mol \, L^{-1} \, s^{-1}$
- D$3.85 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}$
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