The heated sample obviously reacts more quickly, indicating that more of the ions have the needed activation energy to make effective collisions. Also, as the ions move more quickly they are simply more likely to make collisions. Thus both statistics and energy are helpful when the temperature is raised in a reaction system.

The third comparison involves the addition of Mn²⁺ to one sample of oxalate solution before the reaction begins. Manganese(II) ion is a known catalyst for this reaction.

Well, that was fast! The slight yellow color which is visible in the catalyzed mixture is how all of the reactions eventually look if left for a long time. Although we can't say exactly how the catalyst works in this process, it is clear that there is a considerable effect on the rate. In some way more ions are able to make effective collisions in the same amount of time.