I've come across the question "what is the origin of activation energy in a chemical reaction?"
My attempted answer:
Ea=RT^2(dlnK/dT) Activation energy - minimum energy needed to start a chemical reaction (sensitive to temperature). The more molecules with energy > Ea, the more frequent successful collisions and the faster the rate of reaction. Ea is the energy difference between reactants and transition state, which separates reactants from products.
I don't really know what the question is asking; someone please help me?