Consider the following hypothetical molecular collisions and predict which of the following will form potential products, given the values for the energy of activation, Ea, and enthalpy of the reaction, ΔH, in combination with the molecular orientation.

The collision theory is defined as the rate of a reaction is proportional to the rate of reactant collisions.

Explanation:

The reacting species should collide with orientation that allows contract between the atoms that will become bonds together in the product.

The collision occurs with adequate energy to permit mutual penetration of the reacting species. The two physical factors based on the orientation and energy of collision, the following reaction with carbon monoxide with oxygen is considered.

2CO (g) + O2 (g) → 2CO2 (g)

After collision between the carbon monoxide and oxygen the reaction is

CO (g) + O2 (g) → CO2 (g) + O (g)

Based on the theories of chemical reaction the molecules collide with sufficient amount of energy an activated complex is formed.