The anion is formed, together with peroxocarbonate CO2−
4, at the negative electrode during electrolysis of molten lithium carbonate.[1] The anion can also be obtained by electrolysis of a saturated
solution of rubidium carbonate in water.
Potassium peroxydicarbonate K2C2O6 was obtained by Constam and von Hansen in 1895;[3] its crystal structure was determined only in 2002.It too can be
obtained by electrolysis of a saturated potassium carbonate solution at −20 °C. It is a light blue crystalline solid that decomposes at 141 °C,
releasing oxygen and carbon dioxide, and decomposes slowly at lower temperatures
sounds doable along with a dry ice bath of acetone any one tried this.AJKOER - 17-7-2018 at 06:10
A major part of a successful electrolysis, per my limited experience and readings, is the choice of the electrode material and its surface area.
What is the problem with graphite? Titanium passivates, which is a problem, but graphite doesn't. Plus graphite is cheap, available in thin plates and
is unreactive.
To address the corrosion issue with graphite rods (for lead pencils), I placed the electrode in a funnel with filter paper with the mouth of the
funnel in contact with the rest of the cell.
Also, maintaining a very cold solution during electrolysis may require stirring as well.
[Edited on 17-7-2018 by AJKOER]Cipher - 17-7-2018 at 06:45
Sounds impractical. How do you plan to hold solution cold for so long? Also if you try to reduce time by increasing electrolysis rate, it will just
heat up more. Also isn't graphite or carbon or it's impurities maybe catalyst in H2O2 decomposition? Has anybody tried reating C with H2O2? UTFSE!
