What determines thermodynamic stability?

Thermodynamic stability is primarily determined by the energy state of a system. The concept posits that a system is more stable when it is at a lower energy state, as systems tend to favor configurations that minimize energy. When a reaction occurs and products are formed, the difference in energy between reactants and products plays a crucial role in determining stability.

If the products of a reaction possess less energy than the reactants, the reaction is exothermic, and this lower energy state indicates greater thermodynamic stability. Conversely, a higher energy state suggests less stability. This principle reflects the fundamental concept that nature seeks the lowest possible energy configurations, which is key in evaluating the thermodynamic favorability of a reaction.

Factors such as reaction pathways, speed, and activation energy pertain to the kinetic aspects of reactions rather than their thermodynamic stability. Therefore, the defining characteristic of thermodynamic stability directly correlates to the energy levels of the reactants and products.