In a bimolecular reaction,the steric factor P | vedclass

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(A) According to the collision theory,the rate constant $k$ is given by $k = P \cdot Z \cdot e^{-E_a/RT}$,where $P$ is the steric factor and $Z$ is th

Vedclass · Accepted Answer

$A, B$

Vedclass · Answer

(A) According to the collision theory,the rate constant $k$ is given by $k = P \cdot Z \cdot e^{-E_a/RT}$,where $P$ is the steric factor and $Z$ is the collision frequency.The experimental frequency factor $A_{exp}$ is equal to $P \cdot Z$.The Arrhenius equation predicts the frequency factor as $A_{calc} = Z$.Since $P = 4.5$ (which is $> 1$),we have $A_{exp} = 4.5 \cdot Z$,which means $A_{exp} > A_{calc}$. Thus,option $[B]$ is correct.The activation energy $E_a$ is an energy barrier and is independent of the steric factor $P$,which accounts for the orientation of molecules. Thus,option $[A]$ is correct.Option $[C]$ is incorrect because a reaction with $P > 1$ can proceed without a catalyst.Option $[D]$ is incorrect because the experimental value is higher,not lower.

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