## delta g vs delta g°

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

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

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

Ian Morris 3C
Posts: 101
Joined: Wed Sep 18, 2019 12:18 am

### delta g vs delta g°

What is the difference between Delta g vs delta g°.
thanks

605110118
Posts: 75
Joined: Wed Sep 18, 2019 12:21 am

### Re: delta g vs delta g°

Delta G naught is for a standard reaction ya silly goose! The normal delta g is for the overall reaction! hope that helps .

Hannah Lee 2F
Posts: 117
Joined: Thu Jul 11, 2019 12:15 am

### Re: delta g vs delta g°

ΔG, Gibbs free energy, is the energy associated with a given chemical rxn and released from a spontaneous process (negative value) that can be used to do work. The relationship between ΔG and ΔG°is shown via the equation: ΔG = ΔG°+ RTlnQ.

ΔG° is the free energy of reaction at fixed, STANDARD STATE conditions. It is equal to the difference between standard free E of (pure) products - standard free E of (pure) reactants. Again, this is calculated under very specific conditions, while ΔG can be at any given condition. It can be calculated via: ΔG°= —RTlnK.

At equilibrium, ΔG = 0 (but not necessarily ΔG° = 0). Only when [products] = [reactants] (and thus K = 1) does ΔG° = 0, which is very rare.