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Kinetic Collision Theory

Kinetic Theory is a theory that explains the behavior of gases.The gaseous particle are constantly moving and bombarding against the walls of the container. 

This means that the gas particles have kinetic energy. For a chemical reaction to occur between gaseous particles, the particles must collide.Kinetic Collision TheoryKinetic collisionSome of the assumptions made in the formulation of kinetic collision theory are thatGases consist of perfectly elastic particles and the walls of the containers are elastic too. 

It assumes that no energy is lost in collision and that there is ample space in the container for the gas particles to freely move around.The volume of the gas is assumed to be a fraction of the volume of the container.Another assumption is that these particles are not charged and there is no force of attraction or force of repulsion between the particles. 

Some of the observations from Boyle’s law, Gay-Lussacs law and Charles law on gases and the kinetic theory of gaseous particles areFor a chemical reaction to occur the gas particles must collide against each other.If there are more number of particles the number of collisions will increase.And if an external temperature is applied the particles move more vigorously and the collisions increase.However it is important to note that all collisions do not result in the required chemical reaction. For the reaction to occur, the particles must collide with a specific kinetic energy and in a specific angle.

I am planning to write more post on Lattice Enthalpy  and Lepton Number . Keep checking my blog.

The minimum kinetic energy required by the particles to ensure a successful collision reaction is called the activation energy and the specific angle that is required for a successful collision reaction is called correct special orientation. If the geometric orientation and the activation energy are not sufficient, the collisions may be fruitless.Conclusion for Kinetic Collision TheoryKinetic collision theory is a theory proposed to explain the behavior of gaseous particles and the reaction between gaseous particles. It states that for a reaction to occur the particles must collide with a specific minimum kinetic energy called activation energy and with a particular spatial orientation.