Q.The decomposition of $N_2O_5$ in $CCl_4$ is a first-order reaction with $k = 6.2 \times 10^{-4} \text{ min}^{-1}$ . If $[N_2O_5] = 1.25 \text{ mol L}^{-1}$ , the rate of reaction is:

7.75 \times 10^{-4} \text{ mol L}^{-1} \text{ min}^{-1}

4.96 \times 10^{-4} \text{ mol L}^{-1} \text{ min}^{-1}

8.25 \times 10^{-4} \text{ mol L}^{-1} \text{ min}^{-1}

1.25 \times 10^{-4} \text{ mol L}^{-1} \text{ min}^{-1}

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Q.The decomposition of N2O5N_2O_5N2​O5​ in CCl4CCl_4CCl4​ is a first-order reaction with k=6.2×10−4 min−1k = 6.2 \times 10^{-4} \text{ min}^{-1}k=6.2×10−4 min−1. If [N2O5]=1.25 mol L−1[N_2O_5] = 1.25 \text{ mol L}^{-1}[N2​O5​]=1.25 mol L−1, the rate of reaction is: