The Theoretical Model of the Reaction Process

     In our lives, there is no harm on trying things; likewise to the Chemists who proposed a theoretical model known as collision theory which states that molecules must collide in order to react. The kinetic energy of the molecules can be used to break bonds leading to chemical reactions upon collision. If molecules are moving slowly, they have little kinetic energy that they merely bounce off without any reaction It is because not all collisions are effective. If it leads to a formation of products, then it is a effective collision. If every collision leads to a reaction, chemical reactions would be thousands of times faster than they really are.

     There are two factors that determine the effectiveness of a collision: the energy of the colliding particles and the orientation of the molecules at the time of collision Effective collisions depend on the colliding particles having sufficient kinetic energy to achieve the threshold energy or minimum energy required for a chemical reaction to occur This minimum energy is called activation energy. As the temperature is increased, the frequency collision is increase and more reactant particles acquire kinetic energies that exceed the activation energy.