What is the difference between the transition state and activation energy?

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Solution

Difference between activation energy and transition state:
Transition state Activation energy
It is the highest potential energy along the reaction coordinate. It is the smallest amount of energy required for a reaction to take place.
It is a short-lived intermediate that decomposes to result in the products. The reactants need activation energy to generate an intermediate complex before the products are formed.

The representation of transition state and activation energy in the graph is given below:
$E_{a}$ represents as activation energy.

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Transition state	Activation energy
It is the highest potential energy along the reaction coordinate.	It is the smallest amount of energy required for a reaction to take place.
It is a short-lived intermediate that decomposes to result in the products.	The reactants need activation energy to generate an intermediate complex before the products are formed.