Problem

Problem

The reaction, N2O5N_2O_5 (in CCl4CCl_4 ) →2NO2+1/2O2\rightarrow 2NO_2 + 1/2O_2 (g) is first order in N2O5N_2O_5 with rate constant 6.2×10−4 s−16.2 \times 10^{-4} \text{ s}^{-1} . What is the value of rate of reaction when [N2O5]=1.25 mol L−1[N_2O_5] = 1.25 \text{ mol L}^{-1} ? (a) 7.75×10−4 mol L−1 s−17.75 \times 10^{-4} \text{ mol L}^{-1} \text{ s}^{-1} (b) 6.35×10−3 mol L−1 s−16.35 \times 10^{-3} \text{ mol L}^{-1} \text{ s}^{-1} (c) 5.15×10−5 mol L−1 s−15.15 \times 10^{-5} \text{ mol L}^{-1} \text{ s}^{-1} (d) 3.85×10−4 mol L−1 s−13.85 \times 10^{-4} \text{ mol L}^{-1} \text{ s}^{-1}

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