## Delta G

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

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

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

Nathan Mariano 2G
Posts: 68
Joined: Fri Sep 28, 2018 12:29 am

### Delta G

Dr. Lavelle mentioned that a positive delta H (endothermic reaction) is, the more that it does not favor the forward process in the equation (delta g = delta h - temperature x delta s). Why does a positive delta H not favor the forward process? I thought that endothermic reactions do favor forward reactions.

Max Hayama 4K
Posts: 63
Joined: Fri Sep 28, 2018 12:16 am

### Re: Delta G

Normally a negative deltaH indicates spontaneity assuming that delta S is positive or that the temperature of the reaction is low. This will result in a negative deltaG value most of the time.

Fiona Jackson 1D
Posts: 30
Joined: Fri Sep 28, 2018 12:22 am

### Re: Delta G

Hi! Also, a positive delta H in the equation deltaG=deltaH-TdeltaS would make it so the entropy and temperature term would have to be positive and greater that the delta H, making it more likely for delta G to be positive, and thus make the reaction not spontaneous.

Hedi Zappacosta 1E
Posts: 66
Joined: Fri Sep 28, 2018 12:27 am

### Re: Delta G

A negative delta H means that it is exothermic, and usually exothermic processes are favored because they don't require extra energy