Це відео не доступне.
Перепрошуємо.
Iron Oxide (Fe2O3) Synthesis on Large Scale Is A Huge Mess (Dealing With Chemical Waste)
Вставка
- Опубліковано 17 кві 2020
- In this Video I show how I turn my waste solutions of iron sulfate (FeSO4) into Iron Oxide (Fe2O3). This is definetly not a good way to get iron oxide, because it is a lot of work and you can buy it directly for cheap.
This Video is more to learn something about iron chemistry and practical synthetic chemistry, while at the same time doing something useful.
Here is a short outline of the process just using the reaction equations.
1. Hot filtration of iron sulfate solution to remove coal partikel from the steel.
2. Precipitation of the FeSO4 as Fe(OH)2 using Sodium Hydroxide (NaOH)
FeSO4(aq) + 2 NaOH(aq) --► Fe(OH)2(s) + Na2SO4(aq)
3. Letting the water dry up in air so the Fe2+ can oxidise zu Fe3+
2 Fe(OH)2 + O2 --► 2 FeO(OH) + H2O
4. Drying the FeO(OH) to yield Fe2O3
2 FeO(OH) --► Fe2O3 + H2O
What you need is a paint can mixer for a power drill to do your mixing.
Lol yeah or I just buy the Fe2O3 for much cheaper. :D
You need a plaster/mud/joint compound/paint mixing paddle on a drill
That would have helped lol :D
To wash the iron oxide, instead of filtering you could add as much water as you can to it, mix thoroughly, let it settle down, and decant as much of the clear liquid as you can. The time it takes to settle does not depend much on the amount of water. Repeat 2-3 times, and that should get rid of most of the sodium sulfate. Then you can just spread the sediment in a wide and shallow tray, cover with a cloth, and let it dry outdoors.
That would definetly be an option, but that would also produce a lot more waste water. At the same time the vacuum pump also wasted a lot of electricity, so I am not quite sure what would be better. Probably your option is a lot less messy.
@@EliasExperiments Sodium sulfate and sodium hydroxide are harmless to the environment, so the wash water can be just poured down the drain.
The sodium sulfate should not clog the filter. One reason why the second filtering was faster than the first one may be that the high pH causes the paper fibers to soften and swell, closing the pores. Another reason may be that the particles of iron oxide slowly recrystallize and aggregate while wet.
With the high pH and the filter paper is definetly an interesting idea. I certainly didn't think of that. I am not sure about the iron oxide recristallizing. If I knew a way to aggregate is more easily, that would be absolutely amazing.
@@EliasExperiments Unfortunately I cannot find the paper where I saw that discussion. In my recollection, it said that FeOOH is unstable and (very) slowly converts to Fe2O3 even in water suspension. If so, conversion would be faster by boling.
I am not so sure about that, cause I had the Fe(O)OH standing around for 8 month and nothing happend to it. Even after 5 hours at 250 °C in the backing oven most of it hadn't converted to Fe2O3.
@@EliasExperiments Yes, IIRC the conversion is VERY slow at ambient temperature, and was observed for nanoparticles -- that have a very large surface area over volume ratio.
I should try to find that paper again.
I may be mistaken, but I believe that you cannot turn Fe2O3 into FeOOH by mixing it with water; can you?. I believe that the equilibrium in Fe2O3 + H2O 2 FeOOH is very much skewed to the left; but there is a large energy barrier because of the crystal structures (that's why it takes more than 250C to dehydrate). and, at ambient temperatures, the conversion can only happen on the surface of the solid.
Yeah I also doubt that Fe2O3 will hydrolyse in water. Inorganic solid state reactions are just way to slow at ambient water temperatures. (Basically they pretty much won't work.) With nanoparticles it might be true, but nanoparticles are a real pain to work with, because they would go through every filter. I basically want as large crystals as I can get.
Thank you sir.
Most welcome!
@@EliasExperiments please give me your whatsapp number i need some help about making red oxide.
I can't share my phone number here in public youtube comments. If you want help you can contact me on skype or discord: Elias Chalwatzis
What happened at the very end of the video?????
I poured water over the reaction to cool it down again.
You should get some kitchen utensils like a potato masher egg beater rolling pin stong spatula for your experiments
Haha that could indeed be quite fun or usefull or both :D
Please make a video on how to make 99% red oxide from natural red oxide. Thank you
I am not entirely sure what you mean, but it is much easier and cheaper to just buy iron oxide then making it. So I would not recommend it.
Idk about useless, or how toxic those crystals are but they’d look real good in resin in a table top.
The crystals are quite harmles. They would indeed look quite cool in resin.
will this remove phosphates from water
Well maybe, but there are far more effective ways of removing phosphates from water.
@@EliasExperiments what ways are there
This document describes it extensively:
www.matec-conferences.org/articles/matecconf/pdf/2017/20/matecconf_spbw2017_07006.pdf
It has nothing to do with this video however. :D
I mean you could do it with Fe3+ or Fe2+, it would have helped if you formulated your question a bit more precise. :P
@@EliasExperiments Thanks, yep I was trying to find out about granular ferric oxide, but came across your channel, and your iron oxide looks similar. GFO is used in aquariums for phosphate removal. Thinking perhaps I could make my own GFO, LOL
Buying it, is certainly a lot cheaper and easier. :D
Get your gloves! Things are corrosive or irritating
Don't worry I am educated in what I am doing. ;-)