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## Homework Statement

I DO understand the two following points.:

1. If the redox potential of a redox reaction is positive, then the redox reaction is spontaneous.

2. If the redox potential of a redox reaction is negative, then the redox reaction is NOT spontaneous/non-spontaneous.

What I am NOT 100 percent sure I understand is what a redox potential of 0 (so neither positive nor negative) means (since most, if not all, sources don't seem to mention that). I've been told that it means that the system is at equilibrium, which does make sense to me, but being told that, I have another (sub)question to inquire about this further. (See part 3, below.)

## Homework Equations

http://chem.libretexts.org/Core/Phy...es_of_Chemical_Equilibria/Dynamic_equilibrium

## The Attempt at a Solution

Basically, a redox reaction with a potential of 0 means the system in question is ALWAYS in DYNAMIC equilibrium (and never static equilibrium), since redox reactions ALWAYS have motion between reactants and products, albeit at an equal and constant rate, when the redox potential of a redox reaction is 0, right?

If I'm wrong, please correct me.

Any input would be GREATLY appreciated!

P.S.

"Potentials" = "Potential differences", right?