## Tendency of processes

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

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

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

manasa933
Posts: 72
Joined: Fri Sep 29, 2017 7:04 am

### Tendency of processes

Do reactions/processes tend to go towards a lower gibbs free energy or a higher energy and why?

Nehal Banik
Posts: 64
Joined: Thu Jul 13, 2017 3:00 am

### Re: Tendency of processes

When the Gibbs Free Energy of the reaction is less than 0, that means the forward reaction will be favorable, therefore making it spontaneous.

OliviaShearin2E
Posts: 37
Joined: Fri Sep 29, 2017 7:05 am

### Re: Tendency of processes

Manasa pointed out that a reaction will be spontaneous at low Gibbs energy, but as a whole reactions will proceed until they are at equilibrium where ΔG=0. Since ΔG = ΔGº + RT lnQ and ΔGº= -RT lnK, ΔG=0 when Q=K. Essentially, the reaction tries to minimize its Gibbs free energy as it proceeds towards equilibrium. A spontaneous process (ΔG<0) means that the forward reaction taking place will bring the reaction closer to equilibrium, and a nonspontaneous process (ΔG>0) means that the reverse reaction taking place will bring the reaction closer to equilibrium.