For reactions M, N, O and P,the activation en | vedclass

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(D) According to the Arrhenius equation,the rate constant $K$ is given by $K = A \cdot e^{-E_a/RT}$.Taking the ratio of rate constants at two differen

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$P$

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(D) According to the Arrhenius equation,the rate constant $K$ is given by $K = A \cdot e^{-E_a/RT}$.Taking the ratio of rate constants at two different temperatures $T_1$ and $T_2$:$\ln(K_2/K_1) = \frac{E_a}{R} \cdot (\frac{1}{T_1} - \frac{1}{T_2})$.For a fixed temperature interval $(T_1 = 300 \ K, T_2 = 310 \ K)$,the ratio $K_{310}/K_{300}$ is directly proportional to the activation energy $E_a$.Therefore,the reaction with the highest activation energy will have the maximum value for the ratio $K_{310}/K_{300}$.Since the order of activation energy is $E_M Thus,the ratio $K_{310}/K_{300}$ will be maximum for reaction $P$.

For reactions $M, N, O$ and $P$,the activation energy order is $E_M < E_N < E_O < E_P$. For which reaction will the ratio $K_{310}/K_{300}$ be maximum?

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