Question

Explain collision theory of reaction rates of biomolecular gases.

Answer 1

Solution:-

Collision theory of reaction rates of biomolecular gases states that-

1. Molecules must collide in order to react.
   
2. In order to effectively initiate a reaction, the molecules in the collisions must have sufficient energy to bring about disruptions in the bonds of molecules.
   
3. A rise in temperature will cause the molecules to move faster and collide more vigorously, increasing the likelihood of bond cleavages and rearrangements greatly.
   
4. The reactions containing neutral molecules cannot take place at all until they have acquired the activation energy needed to stretch, bend or distort one or more bonds.
   

For a bimolecular elementary reaction,

$A+B⟶\text{Product}$

The rate of reaction is-

$R=Z_{AB}{e}^{-\frac{E_a}{RT}}$

where $Z_{AB}$ represents the collision frequency of reactants $A$ and $B$ and $e^{-\frac{E_a}{RT}}$ represents the fraction of molecules with energies equal to or greater than the activation energy of the reaction.