Recent content by AnathemaXI

I'm just saying, that just because the oxidation potentials of Cl- ad H2O are close, the Cl will appear b/c of it's high reactivity. But if we're electrolyzing FeF2, the products of the H2O reaction will appear at the anode since there is a big difference between it and the Fe products. Am I on...

Oh ok, so it's just because the Cl and hydrogen potentials are so close, that going a little over will create the Cl in the end. So if the reduction potentials are fairly far apart, the water products will form instead eve if it is slow? Such as Fe3+ + e => Fe2+?

What exactly is the difference between a concentration cell and galvanic/voltaic cell? How do you know what are the half reactions? Also, is the ion and electron flow the same found in voltaic cells or is it the opposite? My biggest question of electrolysis has to do with Cl species...

In the example I'm thinking about it refers to an electrochemical cell, a closed one at that. The molarities of the of the solutions are not at standard conditions so it is not at equilibrium. I'll give you the whole picture b/c maybe that would help more. I was given the problem that a student...

I've just about had it with these salt bridges. It's such an easy concept but there are too many questions about it. I understand that the salt bridge enables the flow of ions for the cathodes and anodes by neutralizing charges, but if you use a different salt bridge (Say zinc nitrate instead...