## delta G vs. standard Gibbs free energy

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

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

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

Virpal Gill 1B
Posts: 32
Joined: Thu Jul 27, 2017 3:00 am

### delta G vs. standard Gibbs free energy

I am confused on the use of $\Delta G$ and $\Delta G^{\circ}$. I know that when $\Delta G$ is negative the reaction is spontaneous, but does this also apply to $\Delta G^{\circ}$? What is $\Delta G^{\circ}$ used for?

Lindsay Kester 2L
Posts: 29
Joined: Thu Jul 27, 2017 3:00 am

### Re: delta G vs. standard Gibbs free energy

They're almost the same thing! ∆G° is just defined in terms of the standard molar Gibbs energies of the reactants and products; it's the difference in energy between the pure products and the pure reactants that won't change as the reaction proceeds.