GibbsReaktionsenergie

GibbsReaktionsenergie, also known as Gibbs free energy change, is a thermodynamic potential that measures the maximum or minimum amount of work a thermodynamic system can perform at a constant temperature and pressure. It is a key indicator in determining the spontaneity of a chemical reaction or a physical process. The Gibbs free energy change, denoted by the symbol ΔG, is defined by the equation ΔG = ΔH - TΔS, where ΔH represents the enthalpy change, T is the absolute temperature in Kelvin, and ΔS is the entropy change.

A negative ΔG indicates that a process is spontaneous or exergonic, meaning it releases energy and can proceed without external input. A positive ΔG signifies that a process is non-spontaneous or endergonic, requiring energy input to occur. If ΔG is zero, the system is at equilibrium, and there is no net change occurring.

In chemical reactions, ΔG helps predict whether reactants will transform into products under given conditions. It takes into account both the change in internal energy (enthalpy) and the change in disorder (entropy) of the system. Therefore, a reaction that is endothermic (absorbs heat) can still be spontaneous if the increase in entropy is large enough to make ΔG negative. Conversely, an exothermic reaction might not be spontaneous if the accompanying decrease in entropy results in a positive ΔG. Understanding Gibbs free energy is crucial in various fields, including chemistry, biology, and engineering, for predicting and controlling the direction of natural processes.