Select the correct statement.

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(C) According to the Arrhenius equation,$k = A e^{-E_{a} / RT}$,where $k$ is the rate constant,$A$ is the frequency factor,$E_{a}$ is the activation e

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Rate constant of all the elementary reactions increases with increase in temperature.

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(C) According to the Arrhenius equation,$k = A e^{-E_{a} / RT}$,where $k$ is the rate constant,$A$ is the frequency factor,$E_{a}$ is the activation energy,$R$ is the gas constant,and $T$ is the temperature in Kelvin. As the temperature $T$ increases,the term $e^{-E_{a} / RT}$ increases,which leads to an increase in the rate constant $k$ for all elementary reactions. Option $A$ and $B$ depend on the sign of $\Delta C_{p}$,which varies for different reactions. Option $D$ is incorrect because activation energy is generally considered independent of temperature for elementary reactions.

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The time required for $10 \%$ completion of a first order reaction at $298 \,K$ is equal to that required for its $25 \%$ completion at $308 \,K$. If the value of $A$ is $4 \times 10^{10} \,s^{-1}$,calculate $k$ at $318 \,K$ and $E_a$.

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According to the collision theory,which of the following statements is $NOT$ correct?

For an exothermic reaction $A \rightarrow B$,the activation energy of $A$ is $17 \, kJ/mol$. The heat of reaction is $40 \, kJ$. Calculate the activation energy for the reverse reaction $B \rightarrow A$.

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