## Spontaneity

$\Delta G^{\circ} = -nFE_{cell}^{\circ}$

Chloe Alviz 1E
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Joined: Sat Aug 17, 2019 12:17 am

### Spontaneity

If the cell potential of a battery is positive, does it mean that that Gibbs Free Energy would be negative too?

205007651
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Joined: Tue Nov 13, 2018 12:17 am

### Re: Spontaneity

Yes your delta G will be negative based on the equation ΔG∘=−nFEcell

Sydney Myers 4I
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Joined: Fri Aug 09, 2019 12:17 am

### Re: Spontaneity

Since both are directly correlated with the spontaneity of the reaction, and they are inversely related, then it makes sense that if one is positive, the other must be negative and vice versa.

Posts: 53
Joined: Fri Aug 02, 2019 12:16 am

### Re: Spontaneity

Correct. Negative Gibbs free energy and positive cell potential both mean that the reaction is spontaneous.

RobertXu_2J
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Joined: Fri Aug 30, 2019 12:17 am

### Re: Spontaneity

Yes. From the equation ΔG∘=−nFEcell, you can see that if E.cell is positive, then the gibbs free energy would have to be negative, and if the change in gibbs free energy is negative, the reaction is spontaneous.

Jacob Villar 2C
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Joined: Sat Aug 17, 2019 12:18 am

### Re: Spontaneity

Yes, if delta G is negative and cell potential is positive, it means the reaction is spontaneous.

Emily Burghart 1k
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Joined: Wed Sep 18, 2019 12:17 am

### Re: Spontaneity

Yes, due to their inverse relationship in the equation $\Delta G\cdot=$ -nFEcell, when the cell potential of the battery is positive, the $\Delta G\cdot$
becomes negative

CosetteBackus_4F
Posts: 23
Joined: Wed Feb 20, 2019 12:18 am

### Re: Spontaneity

Because Gibbs free energy and cell potential are inversely related, if the cell potential is positive, Gibbs free energy will be negative, therefore the reaction is spontaneous.

ABombino_2J
Posts: 102
Joined: Thu Jul 11, 2019 12:15 am

### Re: Spontaneity

Yes, Delta G = -nFEcell so if Ecell is positive Delta G must be negative and therefore spontaneous. Also keep in mind a negative delta G and positive Ecell means that the battery is working well.

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