## Gibs Free Energy and Enthalpy

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

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

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

VivianaHF2L
Posts: 29
Joined: Fri Sep 28, 2018 12:20 am

### Gibs Free Energy and Enthalpy

How does the negative enthalpy help prove that most spontaneous reactions are exothermic. In other words what are the connections between them?

Andre_Galenchik_2L
Posts: 69
Joined: Fri Sep 28, 2018 12:23 am

### Re: Gibs Free Energy and Enthalpy

Using the equation Delta G = Delta H - T Delta S, knowing that the reaction is exothermic would increase the chances of Delta G being negative and thus spontaneous.

makenzie2K
Posts: 31
Joined: Fri Sep 28, 2018 12:20 am

### Re: Gibs Free Energy and Enthalpy

As mentioned above, knowing that the deltaH value is negative makes the possibility of deltaG being negative possible. Though, in order for this to occur we must also know that T*deltaS is either some positive number OR a negative number that is LESS than deltaH (meaning deltaH>T*deltaS). In any other case, deltaG would not result in a negative number.