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(C) The Arrhenius equation is $k = A e^{-E_a/RT}$.Statement $A$ is incorrect because the Arrhenius equation is applicable to both elementary and compl

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$B$ and $C$ Only

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(C) The Arrhenius equation is $k = A e^{-E_a/RT}$.Statement $A$ is incorrect because the Arrhenius equation is applicable to both elementary and complex reactions.Statement $B$ is correct because $A$ (the frequency factor) has the same units as the rate constant $k$.Statement $C$ is correct because a lower activation energy $(E_a)$ results in a larger value of $e^{-E_a/RT}$,leading to a faster reaction rate.Statement $D$ is incorrect because $A$ and $E_a$ are generally considered temperature-independent constants for a given reaction.Statement $E$ is incorrect as $A$ and $E_a$ are independent parameters.Therefore,only statements $B$ and $C$ are correct.

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Explain the effect of an increase in temperature on the rate of reaction and the rate constant.

Fill in the blanks:
$1.$ Common collision means ......... phenomenon in species.
$2.$ In collision theory,activation energy and proper orientation of the molecules together determine the ......... for an effective collision.

If the rate constants of a reaction at $500 \ K$ and $700 \ K$ are $0.002 \ s^{-1}$ and $0.06 \ s^{-1}$,respectively,the value of activation energy is $(R=8.314 \ J \ mol^{-1} \ K^{-1}, \log 3=0.477)$.

For the gaseous reactions:
$A \to B$ $k_1 = 10^{15} e^{-25000 / 8.34 T}$
$C \to D$ $k_2 = 10^{14} e^{-15000 / 8.34 T}$
Calculate the approximate temperature at which $k_1 = k_2$ in $K$.

The rate of a reaction decreased by $3.555$ times when the temperature was changed from $40^{\circ} C$ to $30^{\circ} C$. The activation energy of the reaction is.........$kJ \, mol^{-1}$.
[Take; $R = 8.314 \, J \, mol^{-1} \, K^{-1}$,$\ln(3.555) = 1.268$]

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