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How do I remove the oxygen from a boron oxide molecule

Anonymous Wed 25 Aug 23:52:55 2021 No.13561625 View Reply Original Report

Quoted By: >>13562002 >>13562349 >>13562416

I have to remove the oxygen from B2O3 and I know that the combustion of it with Mg makes pure boron, but you have to use acid to take out the impurities and I'm looking for another way to do it

Anonymous

Anonymous Thu 26 Aug 2021 01:35:39 No.13561970 Report

Quoted By:

very small tweezers

Anonymous

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Anonymous Thu 26 Aug 2021 01:43:51 No.13562002 Report

Quoted By: >>13565434 >>13565752

>>13561625
you can reduce any substance with any other substance as long as the Gibbs free energy of the reaction, effectively the useful work done on the system is negative. If you wanted to reduce Boron with carbon, its doable at a high enough temperature, carbon would be pretty easy to remove too as the excess would just burns in air and forms a gas

Anonymous

Anonymous Thu 26 Aug 2021 03:04:37 No.13562349 Report

Quoted By: >>13562394

>>13561625
An excess of timethylsilyl fluoride, you would get TMS-O-TMS and BF3. BF3 has the strongest single bond in chemistry.

Anonymous

Anonymous Thu 26 Aug 2021 03:14:46 No.13562394 Report

Quoted By:

>>13562349
Again.

It might be a little kinetically slow, but that method might work. You could also use HF, either in water or as a gas. If you're actually looking to do this in the laboratory, it won't be a fun process. If you choose any of the above methods (particularly TMS-F), you will need a glove box/schlenk line, HF training, and a variety of other safety measures. Fluorine will absolutely molest you, so don't fuck with it unless you know exactly what you're doing.

Anonymous

Anonymous Thu 26 Aug 2021 03:22:08 No.13562416 Report

Quoted By:

>>13561625
Try using concentrated hydrogen chloride. And then use hydrogen to reduce it.

Anonymous

Anonymous Thu 26 Aug 2021 19:40:24 No.13565434 Report

Quoted By:

>>13562002
can you delve a little deeper into this? I don't quite understand it. some example? I am looking for an environmentally friendly method

Anonymous

Anonymous Thu 26 Aug 2021 19:42:27 No.13565442 Report

Quoted By: >>13565470

(OP) I must clarify that I am looking for pure boron and not oxygen

Anonymous

Anonymous Thu 26 Aug 2021 19:51:32 No.13565470 Report

Quoted By: >>13565475 >>13565485

>>13565442
Always keep to the sinoliest procedure. The anon suggesting HF isnt thinking about safety or how you'd actually deliver that to a vessel containing your reactants.

You know you need magnesium and combustion to make it work. Can you powderize the magnesium with your b2o3 and use conc sulfuric acid to start the reaction?

Anonymous

Anonymous Thu 26 Aug 2021 19:52:42 No.13565475 Report

Quoted By:

>>13565470
>sinoliest
Jesus I'm drunk
*Simplest

Anonymous

Anonymous Thu 26 Aug 2021 19:56:35 No.13565485 Report

Quoted By: >>13565661

>>13565470
The combustion of boric oxide with magnesium makes termite. The acid is only to dissolve the residues. On an industrial scale I think combustion would be the most sinister

Anonymous

Anonymous Thu 26 Aug 2021 20:41:47 No.13565661 Report

Quoted By: >>13565666 >>13565721

>>13565485
Yea but he's not doing it industrially and handling hf is infinitely worse purely from waste handling, safety, ppe, etc
Combustion doesn't have to be violent. Other reducing agents are probably as exothermic.

Anonymous

Anonymous Thu 26 Aug 2021 20:43:23 No.13565666 Report

Quoted By: >>13565716

>>13565661
Also is there another metal that would happily take that oxygen without being so volatile?

Anonymous

Anonymous Thu 26 Aug 2021 21:03:22 No.13565716 Report

Quoted By:

>>13565666
almost any metal if you convert the B2O3 into B (OH) 3. you make it react with heat and there would be pure boron and hydroxide from the metal you put.

Anonymous

Anonymous Thu 26 Aug 2021 21:05:04 No.13565721 Report

Quoted By: >>13565739

>>13565661
Like he could do this thermite reaction on his backyard by touching it off like you would regular thermite. He could then collect the resultants and find a way to filter magnesium oxide from pure boron.

Anonymous

Anonymous Thu 26 Aug 2021 21:12:21 No.13565739 Report

Quoted By:

>>13565721
yes you can, you have to be very careful that the boron does not react again with the oxygen in the air, and the acid serves to dissolve the reactant metal and decant the boron

Anonymous

Anonymous Thu 26 Aug 2021 21:15:57 No.13565752 Report

Quoted By: >>13565770

>>13562002
(OP)
I am going to use this method. Undoubtedly the most efficient, I can reuse the carbon by separating it from the CO2 gas and I would not have to use acid to purify the boron. Heat is not a problem because boron has a boiling point of 4000 ° C at 1 atm. Now I have to do the calculations of the entropy and enthalpy of the reaction to know the amount of temperature I need for the B203 to react with the C and that would be all. Thank you very much anon

Anonymous

Anonymous Thu 26 Aug 2021 21:20:59 No.13565770 Report

Quoted By:

>>13565752
Tbh that sounds harder than just lighting off boron and magnesium. The magnesium oxide is soluble in virtually any acid while boron isn't.

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