Hi, I made pyrophoric iron once by heating rouge (fine Fe2O3) in a stream of hydrogen. It's described in a post on sciencemadness. It was a complete surprise, I didn't expect the iron to ignite. I love your videos, and am so glad you are continuing. You have had a tremendous impact.
I'm visiting family this week so there likely won't be a video. But i'll be back end of next week. I'm currently working out the steps to make Daraprim/Pyrimethamine from domestically available chemicals. I'm not sure if i'll actually make the chemical but it's a long-term project to think about.
JayMark2049 true, I'm the same way. however its the profession attributed to understanding this so thats why i suggested. and 001100AAAEA whats so bad about being a chemist?
+Akatosh x I love math and physics but I hate chemistry for some reason... it's too hard for me I guess!!! (Notice that I said "me", it could be easy for you idk)
I've been fascinated with this video for a while now and I've been working on making this myself. I thought I had done something wrong earlier because I was just left with a brown solution after adding the iron chloride to the oxalic acid even after it had completed cooled. I decided to pour the solution into a new container and the iron oxalate crystals began forming spontaneously and raining to the bottom of the flask. It was awesome to watch and it's still forming crystals after two hours. I can't thank you enough for the inspiration you have provided me from your videos and hard work.
Also, Iron(III) complexes with oxalate, to the extent that oxalate salts will act as rust removers and you can crystallize out (exceedingly soluble) double oxalates from solution.
I'm not a scientist, chemist or any ist. BUT I ALWAYS ENJOY YOUR VIDS. 50 YEARS AGO WISH YOU HAD BEEN MY SCIENCE TEACHER, COZ I ALWAYS LIKED THE SUBJECT, BUT MY SCIENCE TEACHER WAS A BORING SOD AND ONLY WANTED US TO KILL STUFF OR CUT UP EYE BALLS! IF HE WEREN'T GETTING US TO LOOK THROUGH HIS REFACTOR TELESCOPE! NICE BLOKE THOUGH.
Funny enough you can do this with almost any metal, oxygen is almost as reactive as fluorine, we just don’t see it, because it often forms tough passivation layers.
Here's a little trick for you; I don't know what you use for editing, but try to find a noise cleaner. The noise isn't the sound, but the image. It's to clean most of those little spots when the room becomes darker. Or you can also invest in a 20'000$ camera, up to you.
Is it possible to make one big chunk of the pyrophoric iron so that you would have a chuck of iron glowing red hot for a decent period of time? Like from the movie upside down...
I've been subbed for ages and usually have no idea what you're going on about yet for some reason I always enjoy these videos. Lol there is something wrong with me. :p Pretty experiments!
It would be better to first make a solution of oxalic acid. When one of the products is solid, you don't really want the reactant to be solid because its crystals will get caked with the product. That way you get particles of oxalic acid encased in iron(II) oxalate. Slowly dripping concentrated oxalic acid solution into a suitable solution of iron(II), while mixing it, will produce a very fine and reasonably pure product.
+Gareth Dean Im interested in the science and if it can be made through different methods. im sure there are places with the info but nurdrage has the best home chemistry videos on TH-cam.
Well you already made a thermite video but it you want to you can do it again I mean you got the aluminium (the foil) just ground it up into a powder :)
Would the direct reaction between an oxalic acid solution and iron be possible? I guess the main problem would be the precipitation of iron(II) oxalate on the surface of the nail which would slow down the reaction.
NurdRage, Referring to an article recently published in the Royal Soc. Chem's sister publication, 'Chemistry World', titled: "Environmentally Friendly Quantum Dots Make Their Mark", maybe you would like to synthesise indium phosphide nanoparticles?
Could you use finer iron like iron wool for a faster reaction, I am looking to make bulk quantities and got 10 lbs of iron wool on Ebay for $5, they priced the listing wrong .
So, if this would make good thermite, and he is using it on aluminum foil, could it happen that the reaction of the hot iron oxide and aluminum foil could start the thermite reaction and continue, if there was enough aluminum?
so he just changed the basic rule that i learnt..."never add water to acid" well makes sense...(yes i know you said its not a good idea for anhydrous acids)
Many chrome salts have a nice dark green, but also other colors. And I think the salts of Cobalt have many colors ranging from blue to red, also purple. Manganese is also quite colorful. Permanganates have a very intense purple color but the Manganese salts can also be green, brown and slightly pinkish. Transition metals in general produce any kind of imaginably colored salts.
+NurdRage can you make a video about how to synthesize your own oxalic acid like did with hydrochloric acid and also i don't have a blowtorch is there anything else I can use
+KnightKiller1000 Depends if you want the putty afterwards. The putty can be thinned with organic solvents and heating and the iron left to settle out.
Hello, NurdRage. Nice Pyrophoric Iron video. I wonder if you can make Iron (II) Oxalate using Iron Carbonates and Hydroxides And Oxalic Acid Dihydrate........
This process should also work with H2SO4, correct? Is my thinking correct that the acid could be poured off after iron oxalate recovery and used over and over again to make a pipeline of iron to iron oxalate? I suppose one would need to always ensure an excess of iron vs oxalic acid to prevent oxalate formation in the primary dissolution bath.
can you make ferrous sulfate into sulphuric acid? I heard it was doable by heating it up to decomposition temperatures (I'm unsure how high) and at which point it would produce sulphur dioxide and sulphur trioxide- which could be condensed and further processed into sulphuric acid. I was really hoping you could.confirm or debunk this.
Kane Rhodes yes, you can. Old chemists did this to obtain sulphuric acid, back in 1800. They decomposed it in FeO and SO3, and then absorbed the SO3 in water. The downside of this process is that it deals with SO3. When it comes in contact with air it instantly soaks up any water present and creates a heavy sulphuric acid fog. This reaction is also pretty violent. This is quite dangerous, and i would not recommend doing that.
Nice video NR :)) So other day I was making an Iron oxalate and when I started heating the beaker (containing FeSO4 and oxalic acid). Then some Iron oxalate precipitate and created a few little bangs in the beaker (I thought that my beaker will explode). Why it happened to me? Is there any scientific explanation of this? BTW sorry for my bad English.
@@RobertSzasz But as that reacts to form the iron oxide and provides a fairly high temp when it does the conversion, then it would have the heat and the Iron Oxide fe2 from that Pyrophoric Iron and would maybe continue with the thermite reaction once the correct aluminum/iron oxide ratio is reached? I am not a chemist so I may just not be getting it, but it just seems like it should flow along if the end result of the PI is fe2 and just would need aluminum and heat to go thermite.
@@peregrine1970 oxygen doesn't penetrate solids or piles of powder well. The reason thermite works is that the iron oxide and aluminium are well mixed together and iron oxide feeds oxygen to the aluminum.
NurdRage I'm not good when it comes to chemestry so I am unsure. I believe when I was in chemestry class in h.s I was told always use distilled water.... I just wanted to make sure that is what your suppose to use for people like me who are unsure. In your video you said wash it down with water.... Thank you for your feedback :)
Sup3rman1c Oh thanks. I guess I will just wait for high school. One more year and I will be 15 and go to a high school. That is why I want to know. Schools in Europe are at 15years and above (high schools). And I really love chemistry. But still thanks.
Would it be possible to somehow prepare this in a vial and use it as a means of starting a fire in a survival kit? Or is it too reactive to store for long periods of time.
I'm no expert on physics or chemical reactions, but my guess it would ignite no matter the temperature. Oxygen is extremely volatile, and as liquid even more than in gas form.
Hey NurdRage mix this pyroforic iron with Aluminium oxide will it spontaneously react wit the aluminium oxide or will it react only if it is exposed to air if the second case occurs than you have pyrophorik termite
+Magneto! Try "IChO 2010 preparatory problems" (www.icho2010.org/en/doc/the_preparatory_problems.pdf), the problem 37. You can scale amounts and when you want to prepare pure ferrite (not zinc ferrite) then just repleace ZnSO4 with FeSO4 in eqvimolar amount. In fact any soluble Fe(II) salt will work fine to produce fine ferrite pariticles.
+Ulim151 but the iron particles won't stay suspended in the liquid. i efficiant way would be to produce magnetite nano particles in solution by mixing fe(II) and Fe(III) soulutions in ammonia solution and the suspend them with fatty acids like oleic acid. the suspended nanoparticles can then be solved in unpolar liquids
TheMeilinger I wonder if you could just mix the iron oxalate with an oil and surfactant and then heat it to the iron oxalate's decomposition temperature to form the iron nano particles already in suspension.
not gonna work...... Aluminium isn't pyrophoric and you will need gold/silver powder(For better energy output)/tin/copper(cheaper but less useful) to create same effect.
1. I'm glad you have a glassware sponsor!
2. As someone who is hearing impaired, I especially appreciate that you caption your videos!
Hi, I made pyrophoric iron once by heating rouge (fine Fe2O3) in a stream of hydrogen. It's described in a post on sciencemadness. It was a complete surprise, I didn't expect the iron to ignite. I love your videos, and am so glad you are continuing. You have had a tremendous impact.
Where is the link?
I'm visiting family this week so there likely won't be a video. But i'll be back end of next week.
I'm currently working out the steps to make Daraprim/Pyrimethamine from domestically available chemicals. I'm not sure if i'll actually make the chemical but it's a long-term project to think about.
+NurdRage I hope you have a good time. I love your videos :)
+NurdRage Could you use a bunsen or lab burner in place of a propane torch when converting the Ferrous Oxalate to the Pyrophoric Iron? Great Video!
Have a good time with your family.
+NurdRage You took my advice to make pyrophoric iron. Nice! :D
if you do make daraprim, could you somehow switch the chlorine with another halogen and possibly make a new drug altogether?
These are the most interesting videos that I don't understand.
then become a chemist
+Akatosh x You don't need to be a chemist to understand these reactions. :)
+Akatosh x fuck that
JayMark2049 true, I'm the same way. however its the profession attributed to understanding this so thats why i suggested.
and 001100AAAEA whats so bad about being a chemist?
+Akatosh x I love math and physics but I hate chemistry for some reason...
it's too hard for me I guess!!!
(Notice that I said "me", it could be easy for you idk)
I've been fascinated with this video for a while now and I've been working on making this myself. I thought I had done something wrong earlier because I was just left with a brown solution after adding the iron chloride to the oxalic acid even after it had completed cooled. I decided to pour the solution into a new container and the iron oxalate crystals began forming spontaneously and raining to the bottom of the flask. It was awesome to watch and it's still forming crystals after two hours.
I can't thank you enough for the inspiration you have provided me from your videos and hard work.
You're a bright spark to come up with this method.
Wow. I learned something. Never seen this experiment before. Well done.
This is one of my favourites! I've made it somewhat often back then, because it looks so nice :)
I have no means or desire to do any of these experiments, but i love chemistry and i love watching your videos :-)
Wow, that ferrous oxalate is a beautiful shade of yellow.
Great for hand warmers too.
Also, Iron(III) complexes with oxalate, to the extent that oxalate salts will act as rust removers and you can crystallize out (exceedingly soluble) double oxalates from solution.
I'm not a scientist, chemist or any ist. BUT I ALWAYS ENJOY YOUR VIDS. 50 YEARS AGO WISH YOU HAD BEEN MY SCIENCE TEACHER, COZ I ALWAYS LIKED THE SUBJECT, BUT MY SCIENCE TEACHER WAS A BORING SOD AND ONLY WANTED US TO KILL STUFF OR CUT UP EYE BALLS! IF HE WEREN'T GETTING US TO LOOK THROUGH HIS REFACTOR TELESCOPE! NICE BLOKE THOUGH.
Oh yes, I love pyrophoric substances.
Chemistry is so cool. I totally missed out.
Funny enough you can do this with almost any metal, oxygen is almost as reactive as fluorine, we just don’t see it, because it often forms tough passivation layers.
Can you simulate Mark Watney's hydrazine into water experiment? :)
Gian Carlo Martinelli no, ci tiene alla sua pelle.
Here's a little trick for you;
I don't know what you use for editing, but try to find a noise cleaner.
The noise isn't the sound, but the image. It's to clean most of those little spots when the room becomes darker.
Or you can also invest in a 20'000$ camera, up to you.
It would be cool if you can show a video of silver plating. Not silver nitrate on copper like all the other silver plating videos on you tube.
can we make aluminium powder for flash powder like this ?
Omg wow this is so cool it gave me more info in my brain
Great video!
Is it possible to make one big chunk of the pyrophoric iron so that you would have a chuck of iron glowing red hot for a decent period of time? Like from the movie upside down...
in the next video you should teach us how to wear proper safety protocols
I know that using mag stirring seems like a great idea, but it has to scratch the hell out of your flask.
Note: FeC2O4 may not precipitate at 2:55 due to low Ph. It will work better if you use ammonium or sodium oxalate in place of oxalic acid.
be great to have sealed ampules of that for camping...
U can use FeSO4 instead of FeCl2, work as well ;)
2:50 And you use drain cleaner sulfuric acid XD
good flask. blow torch safe grade
I've been subbed for ages and usually have no idea what you're going on about yet for some reason I always enjoy these videos. Lol there is something wrong with me. :p Pretty experiments!
Fantastic, fun not enraging at all :)
During the end when you dumped it, how hot was it burning at?
It would be better to first make a solution of oxalic acid. When one of the products is solid, you don't really want the reactant to be solid because its crystals will get caked with the product. That way you get particles of oxalic acid encased in iron(II) oxalate. Slowly dripping concentrated oxalic acid solution into a suitable solution of iron(II), while mixing it, will produce a very fine and reasonably pure product.
I keep trying to read "Oxalate" as a hexadecimal number when I first see it.
254 + 662142 = 16695812
Chemistry has a bug.
+frtard
XD
+timewave02012 0xa1a7e
Where do the 254 and 16695812 come from?
Awesome
You said that the resulting iron oxide is pure. Does that mean that the magnetite that was present has also been converted to iron oxide?
+NurdRage can you please do a video about making potassium chlorate with electrolysis?
I always thought the sparks from grinding iron were caused but friction!
They probably are.
cool video. do you have any videos on making iodine or hydrogen peroxide?
+nickwoo2 You'd be better off buying peroxide than making it. Stuff is persnickety.
+Gareth Dean Doesn't mean we don't wanna see the process!
+Gareth Dean Im interested in the science and if it can be made through different methods. im sure there are places with the info but nurdrage has the best home chemistry videos on TH-cam.
*****
Good point. I myself think its production is rather dull, mostly electrolysis of clear solutions.
Gareth Dean
A lot of inorganic chemistry is "dull" like that. At least it's not asking to work with azidoazide azides!
if you were to add the aluminium under an inter athmosphere woud you get a self igniting thermite?
Well you already made a thermite video but it you want to you can do it again I mean you got the aluminium (the foil) just ground it up into a powder :)
Make fine thurmight
Damn that's fucking awesome! I really need youtube channels like yours.! Informative video ftw!.
How would you feel about making some super-fluid helium?
Is it possible to create large crystals of magnetite to demonstrate its magnetic strength?
Why do you use gravity filtration? Why not Buchner funnel (vacuum filtration)?
I don't have Ferrous Chloride. Will Ferrous Bueller do?
Is that an Extreme Q mini whip I see at 4:58? If not, that's uncanny...
you shhould do a collab with nile red
Magic!
Would the direct reaction between an oxalic acid solution and iron be possible? I guess the main problem would be the precipitation of iron(II) oxalate on the surface of the nail which would slow down the reaction.
Really?? Patrion is not enough? Now unskippable adds too??
What kind of iron is used in hand warmers
NurdRage,
Referring to an article recently published in the Royal Soc. Chem's sister publication, 'Chemistry World', titled: "Environmentally Friendly Quantum Dots Make Their Mark", maybe you would like to synthesise indium phosphide nanoparticles?
So, can this melt steel beams?
Could you use finer iron like iron wool for a faster reaction, I am looking to make bulk quantities and got 10 lbs of iron wool on Ebay for $5, they priced the listing wrong .
So, if this would make good thermite, and he is using it on aluminum foil, could it happen that the reaction of the hot iron oxide and aluminum foil could start the thermite reaction and continue, if there was enough aluminum?
I was wondering something similar. If you mixed with an aluminum power if it would make self-ignorating thermite
my brain now hurts
so he just changed the basic rule that i learnt..."never add water to acid"
well makes sense...(yes i know you said its not a good idea for anhydrous acids)
If cooper salts are blue, iron salts are yellow, then what metals have salts that are red? green? maybe even purple?
Many chrome salts have a nice dark green, but also other colors.
And I think the salts of Cobalt have many colors ranging from blue to red, also purple.
Manganese is also quite colorful. Permanganates have a very intense purple color but the Manganese salts can also be green, brown and slightly pinkish.
Transition metals in general produce any kind of imaginably colored salts.
Another reason why the PS4 is much better than the XBone.
+Militant Pacifist Pc master race, swaggot
+Queen Elizabeth II *pcmasterrace :D
Can you use this to make thermite
+NurdRage can you make a video about how to synthesize your own oxalic acid like did with hydrochloric acid and also i don't have a blowtorch is there anything else I can use
I'm wondering if there is a way to extract iron from "Thinking Putty?" If so could you do a video about it.
That would be super cool.
+KnightKiller1000 Depends if you want the putty afterwards. The putty can be thinned with organic solvents and heating and the iron left to settle out.
Hello, NurdRage. Nice Pyrophoric Iron video. I wonder if you can make Iron (II) Oxalate using Iron Carbonates and Hydroxides And Oxalic Acid Dihydrate........
Thought i saw a blue chrystal in the background ;)
Anyone tried pyrolysis of ferric oxalate?
Would that produce the fine iron needed to make magnetic ferrofluid?
Where did u get the reflux condenser and how does it work?
This process should also work with H2SO4, correct? Is my thinking correct that the acid could be poured off after iron oxalate recovery and used over and over again to make a pipeline of iron to iron oxalate? I suppose one would need to always ensure an excess of iron vs oxalic acid to prevent oxalate formation in the primary dissolution bath.
can you make ferrous sulfate into sulphuric acid?
I heard it was doable by heating it up to decomposition temperatures (I'm unsure how high)
and at which point it would produce sulphur dioxide and sulphur trioxide- which could be condensed and further processed into sulphuric acid.
I was really hoping you could.confirm or debunk this.
Kane Rhodes yes, you can. Old chemists did this to obtain sulphuric acid, back in 1800. They decomposed it in FeO and SO3, and then absorbed the SO3 in water. The downside of this process is that it deals with SO3. When it comes in contact with air it instantly soaks up any water present and creates a heavy sulphuric acid fog. This reaction is also pretty violent. This is quite dangerous, and i would not recommend doing that.
Since grinding dust is iron that's been burnt and thus some form of iron oxide, would it be possible to make thermite with it?
Idle curiosity: Is there a physics imposed limit on how fine iron oxide can become? (as in, a physical limit greater than one molecule)
Or as a recording medium...
Kids in Africa could have drank that hydrochloric acid
Can we use extemely fine powder of iron carbonatae
So you did all of that to make rust? Just kidding. Great vid!
? why not cool that co2 down to a solid?
Nice video NR :)) So other day I was making an Iron oxalate and when I started heating the beaker (containing FeSO4 and oxalic acid). Then some Iron oxalate precipitate and created a few little bangs in the beaker (I thought that my beaker will explode). Why it happened to me? Is there any scientific explanation of this? BTW sorry for my bad English.
Kinda makes me wonder. If you keep it in say an argon atmo, then add in the aluminum powder and then expose to oxygen. Self-igniting thermite?
No, you need the metal oxide to react with the aluminum
@@RobertSzasz But as that reacts to form the iron oxide and provides a fairly high temp when it does the conversion, then it would have the heat and the Iron Oxide fe2 from that Pyrophoric Iron and would maybe continue with the thermite reaction once the correct aluminum/iron oxide ratio is reached? I am not a chemist so I may just not be getting it, but it just seems like it should flow along if the end result of the PI is fe2 and just would need aluminum and heat to go thermite.
@@peregrine1970 oxygen doesn't penetrate solids or piles of powder well. The reason thermite works is that the iron oxide and aluminium are well mixed together and iron oxide feeds oxygen to the aluminum.
@@RobertSzasz Ahh... makes sense.
Shouldn't you always wash down with distilled water?
+Aaron orourke I don't think i said not to.
NurdRage I'm not good when it comes to chemestry so I am unsure. I believe when I was in chemestry class in h.s I was told always use distilled water.... I just wanted to make sure that is what your suppose to use for people like me who are unsure. In your video you said wash it down with water.... Thank you for your feedback :)
How do you know that your acid is 10M. I buy mine HCl (31%) as a special drain cleaner but it doesnt say rhe molarity.
Sup3rman1c Oh thanks. I guess I will just wait for high school. One more year and I will be 15 and go to a high school. That is why I want to know. Schools in Europe are at 15years and above (high schools). And I really love chemistry. But still thanks.
Would it be possible to somehow prepare this in a vial and use it as a means of starting a fire in a survival kit? Or is it too reactive to store for long periods of time.
I think that it would be suitable to store in a vacuüm.
Doesnt help, since it reacts with itself like said in the video.
Is it possible to make pyrophoric iron by displacing it from solution of iron sulfate with other metal like aluminium?
no, because the Aluminium poisons the iron surface, but you are right in thinking that it could do that...but not in this case.
Zinc or Magnesium maybe?
do you synthesize your own reagent grade chemicals or do you purchase them? and of so, what website do you recommend for glassware and or chemicals
Can this process work with other iron salts?
would it still ignite like that if it was cold?
+engelteir Yes, it reacts to oxygen.
+Lord Shagrax The activaton energy might be too low, if it was at room temperature :P
i was thinking it might just rust or something like that, maybe quickly. but not actually combust.
I'm no expert on physics or chemical reactions, but my guess it would ignite no matter the temperature. Oxygen is extremely volatile, and as liquid even more than in gas form.
+Lord Shagrax You don't understand what volatile means then.
Hey NurdRage mix this pyroforic iron with Aluminium oxide will it spontaneously react wit the aluminium oxide or will it react only if it is exposed to air if the second case occurs than you have pyrophorik termite
would this work with aluminum instead of iron
No
But Dr. Lithium! I want Iron(III) Chloride!!!!!!!!
Can I use oxalic acid ?
Yes. It actually is the dehydrate. It's always dehydrate.
I sometimes wish I could these, but then realize ill mess something up and probably die.
;-;
would this work with FeCl3?
is there a way to make ferrofluid from this?
+Magneto! you can use the Fe(II) solution for that
+Magneto! Try "IChO 2010 preparatory problems" (www.icho2010.org/en/doc/the_preparatory_problems.pdf), the problem 37. You can scale amounts and when you want to prepare pure ferrite (not zinc ferrite) then just repleace ZnSO4 with FeSO4 in eqvimolar amount. In fact any soluble Fe(II) salt will work fine to produce fine ferrite pariticles.
Ferrofluid is way easier to make. You can just take some iron powder and mix it with some light oil.
+Ulim151 but the iron particles won't stay suspended in the liquid. i efficiant way would be to produce magnetite nano particles in solution by mixing fe(II) and Fe(III) soulutions in ammonia solution and the suspend them with fatty acids like oleic acid. the suspended nanoparticles can then be solved in unpolar liquids
TheMeilinger I wonder if you could just mix the iron oxalate with an oil and surfactant and then heat it to the iron oxalate's decomposition temperature to form the iron nano particles already in suspension.
What's your job outside of TH-cam
Grant tompsen sent me.
Walter White should've done this instead of taking the iron from a toy.
Your comment is wrong in so many ways, that im not gonna bother.
ficolas2 So why'd you say something?
┌( ಠ‿ಠ)┘
Now make Thermite with it
not gonna work...... Aluminium isn't pyrophoric and you will need gold/silver powder(For better energy output)/tin/copper(cheaper but less useful) to create same effect.
5:46
♥