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During a phase transition (e.g., solid to liquid), the Gibbs Free Energy of the phases in question are equal, as the system is at equilibrium and the transition occurs at a constant temperature and pressure.

The Gibbs Free Energy (G) is defined by the equation $G = H - TS$, where $H$ is the enthalpy, $T$ is the absolute temperature, and $S$ is the entropy.

Gibbs Free Energy is often used to calculate the maximum amount of non-expansion work that can be done in a thermodynamic process, such as electrical work in a galvanic cell.

Gibbs Free Energy (G) is the thermodynamic potential that measures the maximum or reversible work that may be performed by a thermodynamic system at a constant temperature and pressure.

At equilibrium, the change in Gibbs Free Energy (ΔG) is zero, indicating that the system is at its lowest energy state for the given temperature and pressure conditions.

The sign of ΔG determines the direction of the chemical reaction; if ΔG is positive, the reaction proceeds in the reverse direction.

A reaction is spontaneous if the Gibbs Free Energy change (ΔG) is negative ($ΔG < 0$), meaning that the process can occur without being driven by an external force.