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In 1875, Josiah Gibbs proposed a thermodynamic quantity that combines enthalpy and entropy into a standard value, it was named Gibbs Free Energy.
SPONTANEOUS: G is negative (G< 0, Keq > 1)
NON-SPONTANEOUS: G is positive (G > 0, Keq < 1)
EQUILIBRIUM: G = 0 (Keq = 1)
It can also be used to calculate the K constant of a reaction using:
Application of Gibbs Free Energy in determining the spontaneity of a reaction
Gibbs free energy can be used as well in the Nernst equation to calculate standard cell potential
Endergonic - uses free energy, ΔG°>0
Exergonic - releases free energy, ΔG°<0
Endothermic - absorbs heat, ΔH°>0
Exothermic - releases heat, ΔH°<0
This can be used to determine spontaneity. Spontaneous reactions always have an excess of free energy
The most common formula using Gibbs free energy is:
It relates free energy to entropy and enthalpy
ΔG of formation
The Gibbs Free Energy of formation is the difference in free energy of the products minus reactants
The ΔG° of any free element in its standard state is zero
Gibbs Free Energy is defined as the energy associated with a chemical reaction that can be used to do work, its units are kJ/mol