The collision theory explains chemical reactions particularly gas-phase chemical reactions which occur when molecules collide with sufficient kinetic energy. The collision theory is based on the kinetic theory of gases. It assumes that for a reaction to occur it is necessary for the reacting species such as atoms or molecules to come together or collide with one another. The collision theory explain that when suitable particles of the reactant hit one another, just a specific division of the collisions cause any noticeable or substantial chemical change, these successful changes are called successful collisions. The successful collisions must have enough energy which is known as activation energy, at the moment of impact to break the prior bonds and form every single new bond. This results in the products of the reaction. Increasing the concentration of the reactant particles or raising the temperature which brings about more collisions and which results in more successful collisions, therefore increases the rate of a reaction.
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