CBSE Class 12 Chemistry Notes: Chemical Kinetics – Collision Theory of Rate of Reaction

Important Definitions:

Active Molecules:

• Those molecules which attain the minimum energy required for a chemical reaction.

Activation Energy:

• Minimum amount of energy required by a reactant molecule to participate in a reaction is called Activation energy.

Threshold Energy:

• Minimum amount of energy which must be associated with the molecules so that their collision results into product formation.
• Threshold energy = Activation energy + Energy Possessed by molecules.

Collision Frequency:

The number of collisions taking place per second per unit volume of the        reaction mixture is known as Collision Frequency Z.
Incase of binary collision Z = 10²⁵   to   10^28.

According to collision theory

• Reacting species must possess the adequate energy to overcome the energy barrier
• Reacting species must be properly oriented at the time of collision.
• Reactant → Activated Complex → Product
• The molecule which have sufficient activation energy from activated complex which decompose in product.
• Orientation of molecule:-

Example:

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