[maxvortex]

If i use MnSO4.H20 to make one part of the cell battery (electrode) and if i apply charge voltage of cca. 1.5V to the cell, this MnSO4 should be transformed/converted to permanganate. Is this correct ?
On discharge it should convert back to MnS04... 

The electrolyte is KOH solution.

Max

[Borek]

If i use MnSO4.H20 to make one part of the cell battery (electrode) and if i apply charge voltage of cca. 1.5V to the cell, this MnSO4 should be transformed/converted to permanganate. Is this correct ?

I doubt. Not every cell is rechargeable.

[maxvortex]

OK. but from the chemical point of view..
What chemical reaction would be triggered if I apply electric charge to this cell ?

Max

[Arkcon]

So, the electrolysis of MnSO₄, in water, then?  Consider what happens to water, in an electrolysis cell.  Also consider what happens to an NaCl solution during electrolysis.  Something similar could happen to manganese sulfate, depending on the electronegativity of the ions.

[maxvortex]

One cell is from iron and one should be manganese sulphate.
Electrolyte is KOH solution, not pure water.

max

[Arkcon]

Are you applying a current (that's called electrolysis,) or are you drawing a current (that what makes a battery)?  Which one you're doing will effect a different result.  You are not permitted to rewrite the laws of chemistry by sheer force of your will.   

[maxvortex]

:-).
I'm charging and discharging the cell.
The same process like in some rechargeable battery.

[Arkcon]

Interesting ... OK, describe the two cells and the two electrode materials,.  And we'll try to determine the half reactions for each for both charging and discharging.

[maxvortex]

Yea, its interesting but it's not working.
The college has test it in few different situations but the only thing that is working is when you add bunch of additives and when you use nacl.

Btw.
I'v found some different terms regarding, well... maybe the same stuff.
E.g. is the manganese sulfate the same as the manganese sulfonates ?
I know it's dumb question but what a hell :-)
 

[Borek]

http://en.wikipedia.org/wiki/Sulfonate

As I wrote earlier, not every cell is reversible. Oxidation of Mn to permanganate is not easy, as one of the intermediate products is a solid MnO₂, which can be quite difficult to oxidize further electrolytically.

[maxvortex]

http://en.wikipedia.org/wiki/Sulfonate

I read this but can you explain a bit further....?

If i would like to try to make permanganate from manganate, what would be the simplest way ?
I dont have laboratory equipment so i must try to make this with some home/basic stuff.

Max

[Borek]

I read this but can you explain a bit further....?

Short version: sulfate and sulfonate are different things.

[maxvortex]

I understand this, but can you tell me main differences...

[vmelkon]

I understand this, but can you tell me main differences...

The difference is the molecule. Sulfate has a sulfur atom onto which there are 4 oxygen atoms bonded. Two of the oxygens have a charge of -1 and so, the entire anion has a charge of -2.

The sulfonate anion also has a sulfur atom at the center and there are 3 oxygen atoms and a R group. One of the oxygen atoms has a charge of -1 and so, the entire anion has a charge of -1. The R represent a radical such as methyl, ethyl or some other carbon based collection.