) threshold. Even a small increase in temperature results in a large increase in the fraction of particles that possess enough kinetic energy to overcome the energy barrier, resulting in more successful collisions per unit of time. 5. Summary of Key Factors Change in Parameter Effect on Peak ( vmpv sub m p end-sub Effect on Distribution Shape Shifts right Flatter and broader Decrease Temp ( ) Shifts left Taller and narrower Lighter Gas ( ) Shifts right Flatter and broader Heavier Gas ( ) Shifts left Taller and narrower

The extension questions build on this foundation, moving from static graphs to dynamic chemistry. The central idea is that for a chemical reaction to occur, particles must collide with enough energy to overcome the ((E_a)), the minimum energy for a reaction. The fraction of particles meeting this requirement is directly tied to the Maxwell-Boltzmann distribution. This is the crucial link between the graph and the real world of reaction rates: a reaction proceeds only when enough particles have energy ≥ (E_a).

represents the relative number of molecules or the probability density. The X-axis represents molecular speed ( ) or kinetic energy ( KEcap K cap E

![Description: Two curves. Curve at T1 is taller and narrower, peak at lower speed. Curve at T2 is shorter, broader, peak at higher speed. Shaded area beyond a certain high speed (Ea) is larger for T2.]