Theory of collisions

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The theory of collisions - the theory of physical chemistry assuming that chemical reactions occur as a result of the collisions of reacting molecules.

According to the theory of collisions, the rate of reaction is proportional to the frequency of colliding of reacting molecules, where the proportional coefficient is a function of the decomposition of their kinetic energy and hence also their average velocity. This theory assumes that in order for a chemical bond to form or break, the energy of the collision must be greater than the activation energy of the reaction.

In the gas phase, according to the classical theory of perfect gas, particle velocity is a function of temperature. After combining the formula for the velocity dependence of the particle with the temperature with the definition of the rate constant, Svante Arrhenius derived the general constant binding formula from the temperature and activation energies of the chemical reactions occurring in the gas phase, called the Arrhenius equation.

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