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AJKOER
Radically Dubious
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Having generated Chlorine via the reaction:
MnO2 + 4 HCl → MnCl2 + Cl2 + 2 H2O
Upon adding Na2CO3 to the MnCl2 and also NaClO based on the following reported reaction:
MnSO4 + NaClO + Na2CO3 → MnO2↓ + NaCl + Na2SO4 + CO2 (reference: https://www.google.com/url?sa=t&source=web&rct=j&... )
One may be able to recycle the MnCl2, for those with NaClO. The reaction probably proceeds this way as it is known that MnCO3 is unstable and on
heating to 200 C, for example:
MnCO3 → MnO + CO2
and I would guess the action of NaClO on MnO to proceed as follows:
NaClO + MnO → MnO2 + NaCl
So my suggested recycle reaction is possibly:
MnCl2+ NaClO + Na2CO3 → MnO2↓ + 3 NaCl + CO2
[Edited on 23-9-2014 by AJKOER]
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Metacelsus
International Hazard
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Umm, the OP specified without NaClO.
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Dan Vizine
National Hazard
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Cheddite Cheese,
Why would you want to do any electrolysis when life can (probably) be easier? That's the bottom line.
If you have all the time in the world a lot of things may seem attractive. If you're trying to get something done, use the most direct route.
I'm currently working on making thorium from the oxide. I had to start with the nitrate because that's what I could get. If I had access to the oxide
directly, I'd never have done the extra work. It's just not efficient.
[Edited on 23-9-2014 by Dan Vizine]
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S.C. Wack
bibliomaster
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...and Mn...Cr would be more convenient to recharge...
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AJKOER
Radically Dubious
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Yes, as I noted "for those with NaClO".
My intent was for those performing a demo of Chlorine generation with MnO2, so that they may possibly (?) recycle their 'waste' MnCl2 (although I
suspect, this is rarely done in practice as my reaction, involving readily available and cheap ingredients, isn't even available on the internet in
the form I cited).
Interestingly, my first and last equation if correct, taken together, imply a net reaction where one is seemingly performing Cl2 generation via the
action of HCl on bleach (but, of course, we are physically not), albeit in a seemingly wastful fashion with the inclusion of Na2CO3. And, lets not
forget, of course, MnO2, acting seemingly as a catalyst(?) here:
MnO2 + 4 HCl → MnCl2 + Cl2 + 2 H2O
MnCl2+ NaClO + Na2CO3 → MnO2↓ + 3 NaCl + CO2
Implied Net:
4 HCl + NaClO + Na2CO3 --MnO2→ Cl2 + 2 H2O + 3 NaCl + CO2
With very cold HCl and NaClO, the net reaction is most likely accurate, as the action of HCl on hypochlorite is fast as is also the reaction with
carbonate, and I would guess MnO2 does not get much involved, but at higher temperatures, probably more engaged and partially consumed.
[Edit] This actually may be a better demo on issues with 'Net' reaction thinking. Often, in practice, ostensible net reactions are not even so
identified. My practice is to always disclose intermediate reactions for feasibility issues (like associated/required operating conditions) so that
the user can properly assess the accuracy (relating to yield, safety issues like possible detonation,..) of the professed net reaction itself.
[Edited on 24-9-2014 by AJKOER]
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stock
Harmless
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The standard laboratory preparation of dry Cl2 is to simply heat CuCl2 strongly
if i am strongly heating Iron(II) chloride i will get chlorine gas?
[Edited on 22-2-2015 by stock]
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blogfast25
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Quote: Originally posted by stock  | The standard laboratory preparation of dry Cl2 is to simply heat CuCl2 strongly
if i am strongly heating Iron(II) chloride i will get chlorine gas?
[Edited on 22-2-2015 by stock] |
LOL.
STANDARD???
Stop spreading misinformation: there are at least THREE much easier room temperature methods, had you bothered to look it up you'd have known this. Or
had you read this thread!
[Edited on 22-2-2015 by blogfast25]
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stock
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blogfast25 thanks i will do this way.
[Edited on 22-2-2015 by stock]
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blogfast25
International Hazard
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Stock:
Unless you have very decent equipment, thermal decomposition of cupric chloride is NOT your friend.
Look into MnO2 + HCl:
MnO2 + 4 HCl === > MnCl2 + Cl2 + 2 H2O
Dry batteries contain MnO2 and HCl is 'patio cleaner'.
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