## Gibbs energy

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

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

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

Jane Burgan 1C
Posts: 73
Joined: Fri Sep 28, 2018 12:15 am

### Gibbs energy

In lecture, professor Lavelle plugged in 0 for G in the equation deltaG=deltaH - TdeltaS to figure out at what temperature is G negative. Why does this work?

Schuyler_Howell_4D
Posts: 66
Joined: Fri Sep 28, 2018 12:28 am
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### Re: Gibbs energy

He used 0 for Gibbs Free energy to find the critical point at which the liquid and gas phase both exist. At this temperature deltaG is zero so, a temperature higher than the critical temp found will be spontaneous because deltaG is negative. A temperature lower will mean a positive deltaG so the reverse reaction is favored.