## Spontaneity

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

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

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

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Jessica Helfond 2F
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### Spontaneity

How does Gibbs free energy relate to the spontaneity of a reaction?

Bruce Chen 2H
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### Re: Spontaneity

When delta G is negative, it is spontaneous. When it is positive, it is not.

Carissa Young 1K
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### Re: Spontaneity

Gibbs free energy can be used to determine the "spontaneity" of a reaction due to the fact Gibbs free energy change is the total energy change of the system.

Xingzheng Sun 2K
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### Re: Spontaneity

△G determines whether a reaction can happen spontaneously. Negative △G is spontaneous, and positive △G is not. It is also related to which way of reaction can be more stable. The lower △G is, the more stable it is.

Henry Dudley 1G
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### Re: Spontaneity

What does it mean if delta G is 0?

Danny Zhang 4L
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### Re: Spontaneity

I believe that the reaction is at equilibrium if delta G is zero.

Anmol_cheema_2F
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### Re: Spontaneity

When change in Gibbs free energy is negative, the reaction is spontaneous; when delta G is positive, the reaction is not spontaneous.

Desiree1G
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### Re: Spontaneity

If Gibbs is at 0 it is at equilibrium, if it is negative then it is exergonic meaning it is also spontaneous. If it is positive it is endergonic which means it is non-spontaneous. The lower the delta G is the more stable it is.

Erin Kim 2G
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### Re: Spontaneity

delta G= 0 is at equilibrium
delta G >0 is not spontaneous
delta G < 0 spontaneous

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