Spontaneous Directions [ENDORSED]

[Abigail Volk 1F]

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

[David Minasyan 1C]

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]

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.

The example of 14.5 can help you better understand this point.

Hope this helps!

[Meredith Steinberg 2E]

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]

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

[Ivy Lu 1C]

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]

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]

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.