Noun
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Gibbs free energy (uncountable)
(physics, chemistry, thermodynamics) The difference between the enthalpy of a system and the product of its entropy and absolute temperature: a measure of the useful work obtainable from a thermodynamic system at constant temperature and pressure.
Δ
G
=
Δ
H
−
T
Δ
S
{\displaystyle \Delta G=\Delta H-T\Delta S}
and
G
=
H
−
T
S
{\displaystyle G=H-TS}
where G is Gibbs free energy, H is enthalpy, T is temperature, and S is entropy.
A reaction will be a spontaneous process at a certain temperature if the products have a lower Gibbs free energy (an exergonic reaction ) even if the enthalpy of the products is higher. Source: Internet
A spontaneous electrochemical reaction (change in Gibbs free energy less than zero) can be used to generate an electric current in electrochemical cells. Source: Internet
As shown in the previous section, the change in Gibbs free energy for an electrochemical cell can be related to the cell potential. Source: Internet
From a thermodynamics point of view, at the melting point the change in Gibbs free energy (ΔG) of the material is zero, but the enthalpy (H) and the entropy (S) of the material are increasing (ΔH, ΔS > 0). Source: Internet
In equilibrium, the Gibbs free energy must be zero. Source: Internet
Melting occurs when the Gibbs free energy of the liquid becomes lower than the solid for that material. Source: Internet