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### Tendency of processes

Posted: Tue Feb 06, 2018 11:09 am
Do reactions/processes tend to go towards a lower gibbs free energy or a higher energy and why?

### Re: Tendency of processes

Posted: Tue Feb 06, 2018 11:24 am
When the Gibbs Free Energy of the reaction is less than 0, that means the forward reaction will be favorable, therefore making it spontaneous.

### Re: Tendency of processes

Posted: Tue Feb 06, 2018 2:56 pm
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.