## Gibbs Free energy

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

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

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

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

### Gibbs Free energy

In the textbook it says the Gibbs free energy of the solid phase lies the lowest. If the entropy of a gas is the highest (compared to liquids and solids), shouldn't the free energy of the gas be the lowest at a certain temperature?

Matthew Lin 2C
Posts: 30
Joined: Fri Sep 29, 2017 7:06 am

### Re: Gibbs Free energy

Yes Gibbs free energy is lowest as a solid because it takes heat and a positive deltaH for the substance to go from a solid to a liquid and from a liquid to a gas. So even though the entropy might be greater as a gas, the enthalpy is higher so the overall G is higher in gases.

Return to “Gibbs Free Energy Concepts and Calculations”

### Who is online

Users browsing this forum: No registered users and 2 guests