## Stability

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

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

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

Henry Krasner 1C
Posts: 64
Joined: Fri Sep 28, 2018 12:15 am

### Stability

What does it mean that if the Gibbs free energy is higher (larger positive number), it is less stable? How does being spontaneous (or a more negative number) equal to more stability?

Riya Shah 4H
Posts: 65
Joined: Wed May 02, 2018 3:00 am

### Re: Stability

You can look at it this way -
If a compound has more energy, its constituent atoms will have more energy. This energy will allow atoms to move around or break apart from each other thus making the compound unstable. Think of this situation as a kid who is hyped up on sugar, he or she will not sit quietly in one place but rather jump and run around.
Now, if a compound has less energy, it is more stable because the atoms will stay in their places. In this situation, the kid is very tired and wants to take rest, so he or she will remain at one place and not disturb the equilibrium of the surroundings.

Jonathan Pai 2I
Posts: 121
Joined: Fri Sep 28, 2018 12:27 am

### Re: Stability

Things with less energy are more stable, stuff with more energy are less stable. So if G is positive, that means energy is going up and it's less stable, versus if it was negative then it would become more stable.