## Delta G equal Zero [ENDORSED]

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

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

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

Mishta Stanislaus 1H
Posts: 45
Joined: Fri Sep 29, 2017 7:04 am

### Delta G equal Zero

Des delta G and delta S have to equal zero for a reaction to be reversible? Can someone explain the reason?

Harsha 1J
Posts: 30
Joined: Fri Sep 29, 2017 7:05 am

### Re: Delta G equal Zero

No, I don't thing so. When delta G is zero is just means that there are equal amounts of products and reactants.

Lily Guo 1D
Posts: 64
Joined: Fri Sep 29, 2017 7:03 am

### Re: Delta G equal Zero  [ENDORSED]

Not necessarily, but delta G = 0 does mean that the reaction is at equilibrium.

Wenjie Dong 2E
Posts: 53
Joined: Fri Jun 23, 2017 11:40 am

### Re: Delta G equal Zero

Lily Guo 1D wrote:Not necessarily, but delta G = 0 does mean that the reaction is at equilibrium.

Agree.

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

### Re: Delta G equal Zero

Do you mean spontaneous? So for a reaction to be spontaneous the Delta G is negative while the Delta Stotal is positive for it to be spontaneous. I'm not sure what you mean by reversible, unless you are talking about if the forward reaction is favorable. Can you elaborate? Hope this helps.