Final answer:
Keeping a reaction from reaching equilibrium is not something that occurs spontaneously. Spontaneity in reactions means they naturally progress toward equilibrium, signified by a minimized free energy. Changes in conditions can shift the equilibrium, but these are induced changes, not spontaneous.
Step-by-step explanation:
Keeping a reaction from reaching equilibrium does not occur spontaneously. Spontaneity in chemical reactions refers to the natural progression of a reaction towards equilibrium without the need for external intervention. A reaction is considered spontaneous when it releases free energy, indicated by a negative Gibbs Free Energy (ΔG), and moves towards a more stable state characterized by a minimized free energy.
Reactions spontaneously proceed in the direction that establishes equilibrium, which is defined where the system's free energy is at its lowest. When a system is in a non-equilibrium state (when the reaction quotient Q ≠ the equilibrium constant K), it will spontaneously adjust until equilibrium is achieved. However, external conditions such as temperature and concentration changes can shift the equilibrium, forcing the reaction to readjust to a new state of equilibrium. This shift is not spontaneous but induced by the change in conditions.