The rate of a reaction can be expressed by Arrhenius equation as, \(k = Ae^{–E_a/RT}\): In this equation, \(Ε_a\) represents
Answer & explanation
Correct answer: option 2
In the Arrhenius equation, \(k = Ae^{-E_a/RT}\), the symbol \(E_a\) represents the activation energy of the reaction.
The activation energy (\(E_a\)) is the minimum energy required for a reaction to occur. It represents the energy barrier that must be overcome for the reactant molecules to transform into products.
Considering this, the correct answer is (2) The energy below which colliding molecules will not react. The activation energy represents the threshold energy required for a successful collision to result in a reaction. Molecules with energies below the activation energy will not have sufficient energy to overcome this barrier and undergo the reaction.