Gibbs Free Energy [ENDORSED]

$\Delta G^{\circ}= \Delta H^{\circ} - T \Delta S^{\circ}$

$\Delta G^{\circ}= -RT\ln K$

$\Delta G^{\circ}= \sum \Delta G_{f}^{\circ}(products) - \sum \Delta G_{f}^{\circ}(reactants)$

Kirsty Star 2H
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Gibbs Free Energy

Under what conditions do ΔG and ΔG° = 0 respectively?

Chem_Mod
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Re: Gibbs Free Energy  [ENDORSED]

∆G will only equal zero at equilibrium.

∆G˚ is equal to zero in the unusual situation that K (equilibrium constant) is equal to 1 at that temperature. It is unusual because K=1 means that for a simple reaction (R--> P) the concentrations of both the reactant and product are equal. This implies these two compounds have the same Standard Gibbs Free Energy.

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