Which statement is incorrect according to the | vedclass

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(D) The Arrhenius equation is given by $k = A e^{-E_a / (RT)}$.$(1)$ The rate constant $k$ is a function of temperature $T$.$(2)$ As temperature $T$ i

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Activation energy and pre-exponential factors are temperature independent.

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(D) The Arrhenius equation is given by $k = A e^{-E_a / (RT)}$.$(1)$ The rate constant $k$ is a function of temperature $T$.$(2)$ As temperature $T$ increases,the fraction of molecules with energy greater than the threshold energy increases,leading to more effective collisions.$(3)$ In the standard Arrhenius model,the activation energy $E_a$ and the pre-exponential factor $A$ are considered to be temperature independent constants.$(4)$ Therefore,all statements $A$,$B$,and $C$ are correct according to the theory,while $D$ is technically an approximation but often treated as a correct premise in basic kinetics; however,if we look for the most accurate theoretical description,the Arrhenius equation assumes $E_a$ and $A$ are independent of $T$. Since the question asks for the incorrect statement,and all provided options are standard interpretations,there might be a misunderstanding. Re-evaluating: all statements are actually consistent with the basic Arrhenius model. Given the standard curriculum,this question is often flawed or implies that $A$ and $E_a$ might vary slightly with $T$ in complex systems. However,based on the provided options,none are strictly 'incorrect' in the context of the basic Arrhenius equation.

Which statement is incorrect according to the Arrhenius equation?

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