Question

Collision theory is applicable to
(A) First order reactions
(B) Zero order reactions
(C) Bimolecular reactions
(D) Intramolecular reactions

Answer 1

Collision theory is used to predict the rates of chemical reactions, particularly for gases. It’s based upon the assumption that for a reaction to occur it is necessary for the reaction species (atoms or molecules) to come together or collide with one another.

Complete step by step answer:
According to the collision theory, the following criteria must be met in order for a chemical reaction to occur:
(1) Molecules must collide with sufficient energy known as activation energy, so that chemical bonds can break.
(2) Molecules must collide with the proper orientation.
(3) A collision that meets these two criteria, and that results in a chemical reaction is known as a successful collision or an effective collision.
Collision theory provides an explanation for how particles interact to cause a reaction and the formation of new products.
So from the above information, we get to know that collision theory is applicable to bi-molecular reactions and with molecularity greater than two. It is not applicable to uni-molecular reactions. The basic requirement for collision theory is that the reaction species (atoms, ions or molecules) must come together and collide in order for the reaction to occur. Collisions are possible in bi-molecular reactions.

So, the correct answer is Option C.

Note: The successful collision 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 product of the reaction increasing the concentration of reaction brings about more collisions and more temperature depicts more collisions, Hence, more successive collisions.
Collision theory is important as it is used to make predictions about how fast chemical reaction takes place. This theory helps the scientists to determine the reaction rates mathematically.