Q.For the gaseous reaction $2N_2O_5(g) \rightarrow 4NO_2(g) + O_2(g)$ , the rate of reaction can be expressed in terms of pressure. If the initial pressure is $P_0$ and the total pressure at time $t$ is $P_t$ , the rate constant $k$ for this first-order reaction is:

k = \frac{2.303}{t} \log \frac{P_0}{2P_0 - P_t}

k = \frac{2.303}{t} \log \frac{P_0}{P_t}

k = \frac{2.303}{t} \log \frac{2P_0}{3P_0 - P_t}

k = \frac{2.303}{t} \log \frac{2P_0}{P_0 - P_t}

The correct solution involves applying the fundamental concept to derive the final value step by step...

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