Question

What is Collision Theory?

Answer 1

What is Collision Theory?

=> For a chemical reaction to occur, the reacting particles must collide with one another.

Answer 2

Answer:

Explanation:

Collision theory states that when suitable particles of the reactant hit each other, only a certain amount of collisions result in a perceptible or notable change; these successful changes are called successful collisions. The successful collisions must have enough energy, also known as activation energy, at the moment of impact to break the pre-existing bonds and form all new bonds. This results in the products of the reaction. Increasing the concentration of the reactant brings about more collisions and hence more successful collisions. Increasing the temperature increases the average kinetic energy of the molecules in a solution, increasing the amount of collisions that have enough energy. Collision theory was proposed independently by Max Trautz in 1916 and William Lewis in 1918.

When a catalyst is involved in the collision between the reactant molecules, less energy is required for the chemical change to take place, and hence more collisions have sufficient energy for reaction to occur. The reaction rate therefore increases.

Collision theory is closely related to chemical kinetics.

Rate constant

The rate for a bimolecular gas-phase reaction, predicted by collision theory is

$r(T) =Kn _{A} n_{B} = Z exp \frac{- E_{a} }{RT}$