What happens to the most probable kinetic energy and the energy of activation with an increase in temperature?

(N/A) As the temperature $(T)$ increases,the average kinetic energy of the molecules increases,which causes the most probable kinetic energy to increase. This is represented by a shift in the Maxwell-Boltzmann distribution curve to the right.
The energy of activation $(E_{a})$ is a characteristic property of a reaction and is generally considered independent of temperature for a given reaction. However,the fraction of molecules possessing energy equal to or greater than the activation energy increases significantly with an increase in temperature,which leads to an increase in the rate of reaction.
Note: The energy barrier itself does not change with temperature; rather,the distribution of molecular energies changes,allowing more molecules to overcome the existing energy barrier.