Orsa
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Producing high % CO
I need to get high levels of CO. I currently burn charcoal with air at 300 deg cel.
If i add pore oxygen O2 only what will happen?
Help
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rikkitikkitavi
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If you look at the equlibrium reaction
CO2 + C = 2 CO it is strongly shifted to the left at T < 600 C.
On the other hand , it is so strongly shifted to the right @ > 1000 C that the gases contain < 1 % CO2.
However , the reaction is endothermic, so in practise it is made like this.
Take a long steel tube and fill it with coal.
Ignite the coal at one end and inject air so the coal starts burning. This way there will be a zone where the coal is burning to CO2, and after that
zone the hot CO2 will react with hot C according to above reaction. And once the CO is formed it doesnt shift back unless it is oxidized.
Out from the tube comes almost pure CO and N2.
You will of course need to experiment a bit with airflows, amount of coal e t c to get the highest yield of CO.
/rickard
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PHILOU Zrealone
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If I remember wel heating salts of formic acid and of oxalic acid dry in a flame provide CO!
2NaO2CH --> Na2O + 2CO + H2O (2NaOH + 2CO)
On the other hand...
CO + NaOH --> NaO2CH
NaO2C-CO2Na --> Na2O + CO2 + CO (Na2CO3 + CO)
PH Z
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madscientist
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PH Z, could you provide more details on that reaction you mentioned:
NaOH + CO ----> NaO2CH
Does it merely involve passing carbon monoxide over sodium hydroxide pellets, or is heat, or something else, necessary?
I weep at the sight of flaming acetic anhydride.
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PHILOU Zrealone
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Don't know if it works on dry pellets but a warm solution of concentrated NaOH fixes CO quite fast to make Na formate!You can imagine the first
reaction to be the acid base reaction to get the salt!
C=O + H2O --> H-CO-OH
PH Z
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DDTea
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I think that one of the easiest ways would be to dehydrate Formic Acid with Concentrated Sulfuric Acid...
HCOOH + H2SO4 --> CO + H2SO4.H2O
From the book War Gases, the lab procedure is as follows...
Concentrated Sulfuric Acid is placed in a flask closed with a three-holed stopper. One of the holes carries a tap funnel, another a thermometer
and the third a gas delivery tube. The flask is heated to 100*C. and industrial formic acid (About 98%) is allowed to flow in slowly while the
temperature of the liquid is maintained at 100*C. From 175g Formic Acid, 100g Carbon Monoxide is obtained.
[Edited on 26-2-2003 by Samosa]
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symboom
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Carbon monoxide is conveniently produced in the laboratory by the dehydration of formic acid, for example with sulfuric acid. Another method is
heating a mixture of powdered zinc metal and calcium carbonate, which releases CO and leaves behind zinc oxide and calcium oxide:
Zn + CaCO3 → ZnO + CaO + CO
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Panache
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apparently there's a gas heater in a very depressing household somewhere in country victoria that is a good source of CO.
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subsecret
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Could this amount of CO react with methanol to form acetic acid? I figured it might be a better way to produce the acetic acid as opposed to
distilling a mixture of sodium acetate and sulfuric acid.
Gas Generator --> Gas Washing Bottle with methanol --> CO Absorption Device
Would this be a reasonable path to take for acetic acid?
Fear is what you get when caution wasn't enough.
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Adas
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Quote: Originally posted by Awesomeness  | Could this amount of CO react with methanol to form acetic acid? I figured it might be a better way to produce the acetic acid as opposed to
distilling a mixture of sodium acetate and sulfuric acid.
Gas Generator --> Gas Washing Bottle with methanol --> CO Absorption Device
Would this be a reasonable path to take for acetic acid? |
You need a special catalyst for that.
Rest In Pieces!
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UnintentionalChaos
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| Quote: Originally posted by Awesomeness | Could this amount of CO react with methanol to form acetic acid? I figured it might be a better way to produce the acetic acid as opposed to
distilling a mixture of sodium acetate and sulfuric acid.
Gas Generator --> Gas Washing Bottle with methanol --> CO Absorption Device
Would this be a reasonable path to take for acetic acid? |
Yes, if you're an acetic acid producing plant. It is an important industrial synthetic route using precious metal catalysts and operating at pressure.
http://en.wikipedia.org/wiki/Monsanto_process
http://en.wikipedia.org/wiki/Cativa_process
Department of Redundancy Department - Now with paperwork!
'In organic synthesis, we call decomposition products "crap", however this is not a IUPAC approved nomenclature.' -Nicodem
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subsecret
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So many of the seeming easy routes to organic compounds involve pretty complicated equipment. 
[Edited on 23-8-2013 by Awesomeness]
Fear is what you get when caution wasn't enough.
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12AX7
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Funny, years ago when I operated a metal melting furnace in the backyard, I once had a good fire going (hot coals, from real wood), then stoked it up
with some fresh charcoal. As the charge heated up, a great, eerily blue flame was produced: obviously, CO burning as it left the furnace. The
furnace was supplied air with a vacuum cleaner in reverse, so if you want a *lot* of CO, fast, well...
Tim
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AJKOER
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OK, if one needs CO for a reaction, I would consider the following sealed chamber approach. Mix Oxalic acid and Carbon and heat in the chamber to
generate the required CO. Reactions and references:
1. Thermal decomposition of H2C2O4 (see http://pubs.acs.org/doi/abs/10.1021/jp9638191 ):
H2C2O4 ---> H2O + CO + CO2
Another source clearly indicates the need for H2SO4 and heating to 90 C to effect this reaction (see http://books.google.com/books?id=AugDAAAAMBAJ&pg=PA759&a... ).
2. Reaction of Carbon heated to over 800 C with CO2 (see http://oxygen.atomistry.com/equilibrium_2co_co2_c.html ):
2CO ⇔ CO2 + C
3. Limit the reaction temperature to under 1500 C as (see http://oxygen.atomistry.com/equilibrium_co_h2o_co2_h2.html ):
CO + H2O ⇔ CO2 + H2
Caution: I believe there is limited explosion potential from heating H2C2O4 and C, but will not rule it out as Oxalic acid is, itself, a poor primary
explosive. Interestingly, Urea on heating with H2C2O4 may explode (see http://books.google.com/books?id=4ewS-AqdCM0C&pg=PA803&a... ). However, employing Oxalic acid dihydrate ( H2C2O4.2H2O) may reduce the
explosion hazard, in any event, based on my research.
[Edited on 4-10-2013 by AJKOER]
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