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(B) The rate of a chemical reaction is proportional to the number of effective collisions,which depends on the fraction of molecules having energy gre

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The fraction of the molecules forming the activated complex doubles itself.

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(B) The rate of a chemical reaction is proportional to the number of effective collisions,which depends on the fraction of molecules having energy greater than or equal to the activation energy $(E_a)$.According to the Arrhenius equation,the fraction of molecules with energy $\geq E_a$ is given by $f = e^{-E_a/RT}$.For a $10^{\circ}C$ rise in temperature,this fraction approximately doubles,leading to a doubling of the reaction rate.Option $(A)$ is incorrect because the average speed $u$ is proportional to $\sqrt{T}$,so it does not double.Option $(C)$ is incorrect as concentration is independent of temperature.Option $(D)$ is incorrect because collision frequency increases only by a small factor (proportional to $\sqrt{T}$),not by a factor of $2$.

It is found that for every $10^{\circ}C$ rise in temperature,the rate of the reaction doubles itself. This is mainly because

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