Rate of a reaction can be expressed by Arrhenius equation as k = A e^-E_a/RT . In this equation, E_a represents: - Chemistry MCQ AIEEE 2006 2026 | ExamTest.live

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Rate of a reaction can be expressed by Arrhenius equation as k = A e^{- E_{a} / RT} . In this equation, E_{a} represents:

A $the energy above which all the colliding molecules will react$
B $the energy below which colliding molecules will not react$
C $the total energy of the reacting molecules at a temperature, T$
D $the fraction of molecules with energy greater than the activation energy of the reaction$

Solution & Step-by-step Explanation

Activation energy (E_{a}) is the minimum excess energy that the reactant molecules must possess over their average energy to undergo a chemical reaction. Molecules with energy less than E_{a} will not result in a reaction upon collision.

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Rate of a reaction can be expressed by Arrhenius equation as k = A e^{- E_{a} / RT} . In this equation, E_{a} represents:

the energy above which all the colliding molecules will react

the energy below which colliding molecules will not react

the total energy of the reacting molecules at a temperature, T

the fraction of molecules with energy greater than the activation energy of the reaction

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