## Delta G

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

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

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

Kirsty Star 2H
Posts: 48
Joined: Fri Sep 28, 2018 12:24 am

### Delta G

How can you tell if increasing temperature will increase or decrease the stability of a molecule?

Heesu_Kim_1F
Posts: 60
Joined: Fri Sep 28, 2018 12:18 am

### Re: Delta G

The Gibbs free energy equation is (delta G) = (delta H) - (temperature)(delta S).
When (delta S) is positive and (delta H) is positive, then the reaction will be spontaneous at high temperature.
When (delta S) is positive and (delta H) is negative OR when (delta S) is negative and (delta H) is positive, the temperature will not affect spontaneity.
When (delta S) is negative and (delta H) is negative, then the reaction will be spontaneous at low temperature.
Hope this helps!

Theodore_Herring_1A
Posts: 60
Joined: Fri Sep 28, 2018 12:29 am

### Re: Delta G

The formula for Gibbs free energy is deltaG = deltaH - TdeltaS

If deltaG is negative, the reaction is spontaneous. If it is positive, the reaction is not spontaneous.

Thus, the higher the temperature, the lower the Gibbs free energy, making it more spontaneous, and thus less stable.

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