Collision theory of reaction rate bimolecular reactions salient features.
`to` The reaction molecules are assumed to be hard spheres
`to` The reaction is postulated to occur when molecules collide with each other.
`to` The number of collisions per second per unit volume of the reaction mixture is known as collidion frequenxy (Z).
`to` For a biomolecular elementary reaction
`A+B yo` proudcts
Rate `=Z _(AB). e ^(-E_(a)//RT):Z _(AB)` = collision frequency.
`to` All collisions do not lead to produce formation.
`to` The collisions with surfficient kinetic energy (Threshold energy) are responsible for produect formation . These are called as effective collisions.
`to` To account for effective collisions a factor p called to probability factor or steric factor is introduced.
Rate `=PZ _(AB). e^(-e_(a)//RT)`
`to` The proper orientiation of reactant molecular lead to bond formation where as improper orientation makes them back and no product are formed.
`to` In this theory activation enerfgy and proper orientation of the molecules of the molecules to gather determine the createria for an effective collision and hence the rate of a chemical reaction.
