Give a detailed account of the Collision theory of reaction rates of biomolecular reaction.

Explanation

According to collision theory, the reactant molecules are assumed to be hard spheres and reaction occur only when molecules . collide each other. The number of collisions per second per unit volume of the reaction mixture is known as collision, frequency (Z). Activation energy also effects the rate chemical reactions. For a bimolecular elementary reaction.
`A + B to "Product"`
Rate of reaction is
Rate `= Z_("AB")e^(-E_(a)// Rt)`
Where `Ze_(AB)` represents the collision frequency of reactants. `A and B and e^(-E_(a)// RT)` represents the fraction of molecules with energies equal to or greater than `E_(a)`.
All collisions do not lead to the formation of products. The collisions in which the molecules having threshold energy and proper orientation leads to the formation of products. Such collisions are called effective collisions.
If the colliding molecules have improper orientation they bounce back and no reaction takes place.
To account for effective collisions a new factor .p. called probability or steric factor is introduced
Rate `=PZ_("AB") e^(-E_(a) // RT)`
Thus, in collision theory activation energy and proper orientation of the molecules together determine the criteria for an effective collision and hence the rate of a chemical reaction.