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Author: Subject: Clorine gas WITHOUT sodium hypochlorite
AJKOER
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[*] posted on 23-9-2014 at 14:50


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
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[*] posted on 23-9-2014 at 14:55


Umm, the OP specified without NaClO.



As below, so above.

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Dan Vizine
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[*] posted on 23-9-2014 at 15:20



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
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[*] posted on 23-9-2014 at 16:24


Quote: Originally posted by Cheddite Cheese  
Umm, the OP specified without NaClO.


...and Mn...Cr would be more convenient to recharge...




"You're going to be all right, kid...Everything's under control." Yossarian, to Snowden
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AJKOER
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[*] posted on 23-9-2014 at 16:46


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
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[*] posted on 22-2-2015 at 09:14


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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[*] posted on 22-2-2015 at 09:43


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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[*] posted on 22-2-2015 at 09:55


blogfast25 thanks i will do this way.

[Edited on 22-2-2015 by stock]
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blogfast25
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[*] posted on 22-2-2015 at 10:58


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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