GibbsEnergieänderung

GibbsEnergieänderung, often denoted as ΔG, represents the change in Gibbs free energy during a process or chemical reaction. Gibbs free energy is a thermodynamic potential that measures the maximum amount of non-expansion work that can be extracted from a closed system at constant temperature and pressure. It is defined as G = H - TS, where H is the enthalpy, T is the absolute temperature, and S is the entropy.

The change in Gibbs free energy, ΔG, for a process at constant temperature and pressure is given by ΔG = ΔH - TΔS. This equation is fundamental in determining the spontaneity of a process. If ΔG is negative, the process is spontaneous and can occur without external energy input. If ΔG is positive, the process is non-spontaneous and requires energy input to proceed. If ΔG is zero, the system is at equilibrium.

The enthalpy change, ΔH, relates to the heat absorbed or released during the process, while the entropy change, ΔS, reflects the change in disorder or randomness. The interplay between these two factors, modulated by temperature, dictates whether a process will naturally occur. For instance, an exothermic reaction (negative ΔH) that increases disorder (positive ΔS) will be spontaneous at most temperatures. Conversely, an endothermic reaction (positive ΔH) that decreases disorder (negative ΔS) will likely be non-spontaneous. Understanding GibbsEnergieänderung is crucial in chemistry, biology, and materials science for predicting reaction feasibility and optimizing conditions.