Chemiclint
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Daguin reaction -- production of HCl
Hi
can anyone enlighten me as to the Daguin reaction? Reading through a copy of Mellor - Inorganic and theoretical chemistry, p164, he makes reference
to the Daguin Co "treating a mixture of manganous and sodium chlorides with air containing about 10% sulphur dioxide" to form sodium sulphate and
hydrogen chloride, MnCl2 acting as a catalyst. Presuming it's mixing a sulphur dioxide flue with 10% residual O2 with salt and MnSO4/MnCl2 in a hot
reactor but then where's the H come from? Thinking steam
I'm assuming by the wording hydrogen chloride, not hydrochloric acid, that the HCl was gaseous/anhydrous. I haven't been able to find any info on the
web for this process, general historical information is available for the Marcheville-Daguin Co who where the largest producers of salt in France at
the time and had another interesting patent "Daguin (Engl. pat. 3669 1888) makes SO2 and air act upon chlorides the presence of MnO2, in order to
produce chlorine"
Personally more interested in HCl production side of it - Ideas?
[Edited on 25-9-2012 by Chemiclint]
EDITED: Changed title so that it is more clear what the OP wants.
[Edited on 25-9-12 by woelen]
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elementcollector1
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Nope.
Elements Collected:52/87
Latest Acquired: Cl
Next in Line: Nd
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woelen
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If you are interested in making HCl, then there are easier and much better ways. One option is to add NaCl to conc. H2SO4. If you don't have H2SO4,
then use NaHSO4 (pH minus for swimming pools) and mix this with NaCl and heat the mix. By careful heating you drive off HCl gas. The NaHSO4 in pH
minus usually is the monohydrate, so you get a mix of HCl and water vapor.
Yet another method is to take anhydrous CaCl2 (drying agent, can be found in hardware stores) and add the solid to concentrated hydrochloric acid (30%
or better). Slight heating drives off HCl gas and your solution becomes a very concentrated CaCl2 solution. The HCl can be dried by passing it through
a tube, filled with more CaCl2.
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Chemiclint
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Thanks woelen, Interested in it more based on reactions on an industrial scale/academic standpoint like burning pyrite (or sulphur) in excess air and
using commercial salt and requisite Mn catalyst to form HCl and the conditions under which such a reaction might proceed
Maybe from there to being able to use the HCl and suitable reductant to directly extract MnCl2 from MnO2 (either by direct reduction of MnO2 in an
acidic medium or consumption of the HClO derivitive from the soluton of Cl2 in water). Waste product would be relatevely inoccuous Na2SO4
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ScienceSquirrel
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I suspect that this was a large scale industrial process for treating flue gases.
The flue gas would contain water vapour and sulphur dioxide at several hundred degrees and this would be passed through a heated bed of the salts.
I suspect you would have to build a fairly hefty bit of kit to get this to work.
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Salmo
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Too much reagents to produce a cheap product h2so4 and NaCl is the way then you can dry the gas with an essicant like calcium chloride anyway HCl is
really useful but really nasty without a fumehood!
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