* Electrochemical Series: Potassium sits higher in the electrochemical series than hydrogen. This means potassium has a greater tendency to lose electrons and form positive ions (cations).

* Reactivity Trends: Reactivity generally increases as you move down a group in the periodic table. Potassium is below hydrogen in Group 1 (alkali metals).

* Reaction with Water: Potassium reacts vigorously with water, releasing hydrogen gas and generating heat. This reaction is much more violent than the reaction of hydrogen with water.

Example:

* Potassium: 2K(s) + 2H₂O(l) → 2KOH(aq) + H₂(g)

* Hydrogen: H₂(g) + ½O₂(g) → H₂O(l)

In summary, potassium's position in the periodic table, its greater tendency to lose electrons, and its vigorous reaction with water all point to its higher reactivity compared to hydrogen.