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COLLISION THEORY
General Introduction:-
Generally collision theory is the theory which explains about how chemical reaction takes place.The process of intermixing of reactants and striking between reacting species is called collision.The chemical reaction is only possible by collision of reacting species.During collision,large amount of kinetic energy is formed from the conversion of their potential energy.After vigorous collision,molecules are broken down into several fractions and they move with high speed so possessing high kinetic energy.
The chemical reaction in which molecular collision high in high rate takes place faster.It means higher molecular collision increases the rate of chemical reaction.Because for the chemical reaction and to convert reactants to products,reaction species must overcome the threshold energy.For this activation energy is needed which is the external source of energy.Due to the collision,liberated high amount of kinetic energy is used to overcome the threshold energy barrier.So reactants easily get converted into products.Now,to understand the collision theory properly,general assumptions can be made as follows:-
- Chemical reactions can occur only when collision between reacting molecules takes place.
- Increase in temperature and concentration of reacting molecules increases the rate of collision and hence rate of reaction also increases.
- Only effective collision can result the formation of products.(Effective collision is that collision which can form enough energy so that the activation energy gained can overcome the threshold energy barrier.)
- A collision results in a reaction only if the colliding particles are correctly oriented to one another.
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