Activation energy is crucial for initiating chemical reactions, determining reaction rates, and forming activated complexes.
Activation energy is the energy required to start a chemical reaction. It is essential because reactant molecules need energy to overcome intermolecular forces and collide to initiate the reaction.
The activation energy determines the rate of the reaction; higher activation energy leads to slower reactions. Heat energy from the surroundings is commonly the source of activation energy for chemical reactions.
Activated complex, an unstable arrangement of atoms at the peak of the activation energy barrier, plays a crucial role in determining whether reactants will form products or remain unchanged after collision.
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