Question

In the equation $\mathrm{k}={\mathrm{Z}}_{\mathrm{AB}}{\mathrm{e}}^{\frac{-\mathrm{Ea}}{\mathrm{RT}}}$ what does ${\mathrm{e}}^{\frac{-\mathrm{Ea}}{\mathrm{RT}}}$represent?

Answer 1

Collision theory:

1. For a chemical reaction to begin, the reacting molecules must approach and collide. The bonds between the interacting molecules are severed as a result of these collisions, and the product is created with new bonds.
2. To explain the reaction rates in a gaseous state, Arrhenius presented a simple collision theory. Kinetic molecular theory or reaction rate collision theory is the name given to this theory.
3. Arrhenius equation is given by $\mathrm{k}={\mathrm{Z}}_{\mathrm{AB}}{\mathrm{e}}^{\frac{-\mathrm{Ea}}{\mathrm{RT}}}$where ${\mathrm{e}}^{\frac{-\mathrm{Ea}}{\mathrm{RT}}}$represents the fraction of molecules with an energy equal to or greater than Ea where Ea is the activation energy of reaction, T is temperature, and R is gas constant.

Therefore, ${\mathrm{e}}^{\frac{-\mathrm{Ea}}{\mathrm{RT}}}$signifies the fraction of molecules with an energy equal to or more than the activation energy.