## Spontaneous Directions [ENDORSED]

Abigail Volk 1F
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### Spontaneous Directions

How do you predict the spontaneous direction of a redox reaction using standard reduction potentials.

David Minasyan 1C
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### Re: Spontaneous Directions

If the standard potential is positive (it'll make delta G negative bc of delta G = -nFE) so it'll be spontaneous.

Guangyu Li 2J
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### Re: Spontaneous Directions

The values of standard potential can help us determine whether the process is spontaneous. When Eo is >0 the process is spontaneous and tend to produce products while when Eo <0 the process is not spontaneous and tend to produce the reactants.

Hope this helps!

Meredith Steinberg 2E
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Joined: Thu Jul 13, 2017 3:00 am

### Re: Spontaneous Directions

Redox reactions are spontaneous when standard potential is positive. This makes sense if you think about the equation G=-nFE. If E is positive, G will be negative, indicating a spontaneous process.

204918982
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### Re: Spontaneous Directions

standard potential has to be positive for the reaction to be spontaneous

Ivy Lu 1C
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### Re: Spontaneous Directions

You want the standard potential of the reaction to be positive because that would make deltaG be negative (deltaG=-nFE) and k be greater than 1.

Rachel Lu_dis1H
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### Re: Spontaneous Directions

Because of the equation deltaG= -nFE, E (standard reduction potential) must be positive in order for the reaction to be spontaneous. When E is positive, deltaG is negative (when deltaG is negative the reaction is spontaneous).

Tatiana Hage 2E
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### Re: Spontaneous Directions  [ENDORSED]

If the standard potential is positive, ∆G is negative and the reaction has a spontaneous tendency to form products.
If the standard potential is negative, ∆G is positive and the reverse of the cell reaction is spontaneous, so the cell reaction has a spontaneous tendency to form reactants.