6.2.5

Sketch and explain qualitatively the Maxwell–Boltzmann energy distribution curve for a fixed amount of gas at different temperatures and its consequences for changes in reaction rate.

Since temperature is a measure of average kinetic energy of the particles, the increase in temperature leads to an overall increase in the rate of reaction. Therefore a greater number of particles will have energy above the activation energy.

The area under both curves is equal (signifying the number of particles) but the curve at 310K has slightly more particles with energy greater than the activation energy. This is because at higher temperatures particles have an increase in average kinetic energy, which means higher collision frequency. Therefore more successful collisions taking place hence increase in rate of reaction.