Question

Collision theory is applicable to:
[A] First order reactions
[B] Zero order reactions
[C] Bimolecular reactions
[D] Intramolecular reactions

Answer 1

HINT: According to the collision theory, for a reaction to occur the particles must collide. It also affects the rate of the reaction and thus the reactants affect it too. Using this you can answer the given question.

COMPLETE STEP BY STEP SOLUTION: To answer this firstly let's discuss the collision theory.
According to the collision theory, particles must collide with one another to undergo a chemical reaction. Only a certain amount of collisions result in a notable change when particles of the reactant hit each other. We call these successful changes as successful collisions. To break the pre-existing bonds and form a new bond, the reactants should have certain energy to overcome the energy barrier of the existing bonds and it is known as the activation energy. This results in the formation of products of the reaction.
For collisions to be successful, the reacting particle must collide with sufficient energy and in proper orientation.
Collision theory is applicable for bimolecular reactions where the reactant particles can collide with each other. However, it is also applicable for pseudo unimolecular reactions as they follow second order kinetics at very low pressure. It is applicable for bimolecular reactions following second order kinetics.

Therefore, the correct answer is option [C] bimolecular reactions

NOTE: The rate of collision depends upon certain factors. We can describe these factors as-
- Concentration of the reactant – Upon increasing the concentration of the reactant, the number of collisions increases thus, the rate of successful collisions also increases.
- Temperature – Upon increasing the temperature, the average kinetic energy of the molecules in the solution increases and thus increases the collisions.
- Catalyst – When we add a catalyst, less energy is required for the chemical change to take place and more collisions have sufficient energy to take the reaction forward thus increasing the reaction rate.