My pit bull ate an entire box of S.O.S. steel wool soap pads and shit iron oxide for a week.I suppose you can use this method,but it may change the odor of the Thermite just a bit.
If you're interested, theres a hydrothermal method can make iron oxide with interested properties. If you use a solution of iron chloride and a sugar (sucrose or glucose work well) and put the solution in a hydrothermal reactor you'll end up with iron oxide nano spheres surrounding a nano sized carbon ball scaffold. Filter and dry to powder and then heat to several hundred degrees burns on off the carbon leaving a hollow sphere of ironoxide. I'm curious to see if it make better thermite. I'll make some in a video in the near future probably
ThePharphis I realized I posted that with the wrong channel, I use it in my nanotech research on my other channel, the thought emporium. Same process, but I use it to make glowing nano particles
TheChemLife aha.. nanothermite is of what i recall created through an organo-electric process where the aluminium is formed among the iron oxide, being also very well mixed up upon being created
If you run a magnet through fine dry soil, particularly red soils you tend to pick up a noticeable amount of iron. These little pebbles tend to be very tiny from my experience, less than 1cm. I would imagine they would be easy to grind into a fine powder for oxidation by taking advantage of a large surface area!
This video also took way longer to make than i expected. Oh, well, better late than never. Do you guys like the longer more comprehensive video format? or do you prefer shorter videos (~4mins)?
I find that the easiest way to ignite thermite is with glycerine and potassium permanganate - it also gives an inherent time delay to allow you to walk away from it before the reaction starts and doesn't require any magnesium.
You can also perform the electrolysis inside, near candles. This drastically increases the chance for hydrogen combustion setting the entire room and you on fire. I don't know WHY you would want to set your face on fire, but you can.
I needed some ironoxide for my chemiluminescense experiment, I made it by a percipitation reaction. I mixed iron sulphate with sodiumhydroxide, than I removed the water and was left with ironoxide. It's a really fast way but the downside is that you need iron sulphate :)
Hint: "washing soda" is sodium carbonate. Ferrous Sulfate is sold as moss killer in hardware stores or garden stores. Cheap. Ferrous Hydroxide if Lye used, which oxidizes or use as is (thermite Al works with NiO, MnO, CuO, FeO). On thermal drying Fe3O4 formed.
NurdRage, you are not alone. I also have a PhD (of sorts) and am also easily impressed. i think its because I understand how amazing the process is behind what I am witnessing. I am still amazed by turbine engines for example. Drives my wife nuts.
***** u idiot iron oxide doesnt form on cars lol r u serious cars r made of aluminium and glass like from the beach i went to the beach once and there was sand which is also known as silicon dioxide, a covalent network substance (i.e. covalent molecules all covalently bonded to each-other as opposed to relying on IMFs), which can be turned into glass and iron oxide absolutely does form on cars as the (typically) nickel galvanising layer wears away and exposes iron which is then oxidised but u r a idiot nd no wonder u hav a shit car cos ur an idiot lol do u even no physics
nurd rage i really have respect for you . you made me tha i want to be a chemist i even built my own mini lab and i always watch evry video so thanks greetings from a twelve year old boy from malta
9+ minutes is amazing! This will be really interesting and I hope you continue with this style of video. I want to emphasize that I only want this if you have 9+ minutes of things to say about the subject. Don't let the pressure of needing a longer video compromise the excellence in quality that we have grown to love! Keep up the good work.
I work at an auto parts store, where we have a brake rotor lathe. I got just about all the iron filings I want! If your nearby store has a brake lathe, you might could ask for them to give you some. It just gets dumped in the dumpster anyway.
If you use steel wool wash it off with dish soap first (Dawn works best) cuz there's an oil on the steel wool to keep it from rusting. It speeds things up A LOT. lol I found this out looking for info on making old-timey DIY wood stain from steel wool and acetic acid.
Thank you so much for your videos! I found myself experimenting (successfully) with an old bit of iron/steel wool to see if I could get some rust. 1. I washed it in dish detergent to rid it of oil residue. 2. I immersed it in hydrogen peroxide solution (3%) in an empty water bottle. 3. Put it in window sill and added pinch of sodium chloride. 4. It worked in a week or so.
You can avoid that foaming when precipitating the iron, if you just use sodium hydroxide instead of baking soda. This doesn't release CO2 and you also dont get a mixture of iron hydroxide and carbonat. I personally prefer this method because it's somewhat cleaner and easier to work with. Also you don't need to dilute and decant it, since you can just let it sit for a few hours in a cold environment and then filter it.
i think he was going for more common home chemicals, also baking soda has that nice co2 bubbling as an indicator i guess, but yeah NaOH is probably best
I find that white vinegar is a useful catalyst and scrap iron for cans can be used. Iron (II) acetate is unstable to oxidation while iron (III) acetate breaks down into iron hydroxide, releasing the acetate for further reaction. With an ice cream container, a liter of vinegar and a few squashed cans you can make a kilo of oxide a week. Cheap white vinegar is factory made now and is literally just acetic acid. As a bonus the unreacted acid will evaporate off when you're done.
I like to come back to this video periodically whenever I have a new update, so here it is. In my case, the peroxide would the most expensive investment...until I found some septic treatment that is 15-20% hydrogen peroxide at $7 a gallon. However, even with shipping it's still cheaper to buy 20lbs of rust from a ceramics supply online, than it is to invest in the time and reagents. If youre sketchy on the quality, you can still make a weak pirranah solution to convert impurities into soluable or separable salts and particles. But I doubt the effort would be worth it. For those thinking that just adding peroxide to rust or iron with work, yes it will, but it's highly inefficient and the rust itself seems to be a catalyst to decompose the peroxide, meaning that as rust is created, the less peroxide their is to react and thus wasting your reagents. I have 15g of red rust I've been reacting under 50ml of the above concentration of peroxide going on six days. Since the rust I used is the result of three refinement and filtering steps (including magnetic and mass graduation) I doubt my sample is that impure that concentrated peroxide would continue to react almost a week later at an average temp of 80F. The only thing I can think of for it's continued reaction is that iron oxide has a catalytic property with H2O2 that would give a false positive for contaminates or continued oxidation of trace iron.
Most don’t know that steel wool is shipped coated with oil for rust protection. If you use it for anything like trying to rust it or anything else, you should wash it with acetone or lacquer thinner or similar. That’s probably why in this video it didn’t rust extremely well....
I haven't watched your video's in a few years because my computer broke and i simply could not check all my subscriptions on an xbox. I got a new computer recently and this is the first video I'm watching since then. I'm still amazed by the quality of your production and your attention to detail. Thank you
So I have no idea whether or not anyone will see this, but I just wanted to drop in. I am in High School and I am writing a paper for forensic science about dangerous chemicals/materials and whether or not we (The U.S) should place higher restrictions. My main argument is the restrictions we'd have to put in play to ban ONE thing: Thermite Hypothetically say that we put restrictions on the purchase of fine iron oxide and aluminum powders that most metallurgy workers use for their thermite (readily available from Wal-Mart and Amazon, as well as others). With this, you would need some form of permit saying you're a metallurgy worker or something similar. So because of these restrictions, obviously these powders would be a lot harder to get your hands on. I'm making a counter-argument to the proposal in favor of 'restricting' thermite and other chemicals. Using this video and the one where Cody's Lab made thermite with aluminum foil, I'm pressing the argument that thermite is something we pretty much can't do anything about. If we put limitations on the powders, it's worth mention that all someone needs is a sheet of aluminum foil and a box of steel wool to show you how unhappy they are. Not sure if anyone cares!
I realize this is an ancient video, but I wanted to add some observations of my own which I made recently. I have made iron oxide using the electrolytic method. I used sodium bicarbonate as an electrolyte, and did not observe the passivization effect you encountered. I did not want to use sodium chloride because the iron oxide was for another experiment (not thermite) and needed to be substantially chloride-free. The things I did differently from you: -my sacrificial anode was a piece of cast iron, not steel like your nail. I don't know if this has an effect, but thought I'd mention it -the electrolyte was diluted: 4% NaHCO3 -I used a low but constant current of 0.45A from my bench power supply. Yes it takes longer, but it worked.
An artis would tell you that Iron colors range from Indian red to black to yewwow to silver (goethite). You need Fe3O4, either heating Fe2O3 or FeO. You have water in your "Iron Oxide" and as you.know water doesn't help anhydrous reactions.
If you were to use a stainless steel nail in the electrolytic method, wouldnt it produce cancerogenic chromates ? (Since the chromium could easily be oxidized to chromium-(III)-ions which would then react with the bleach)
Found a nice way to remove the salt. Boil down the iron oxide tell dry in a pie tin and use a large magnet on the bottom. The iron oxide is easily rinsed with no loss.
I have 30lbs of railroad spikes, so I'm using the electrolitic process while running a bubbler through it. The extra oxygen from the bubbler helps to both react FeOH into FeO3, as well as prevent buildup on the electrodes. I had tried also to grind up and convert rust flakes accumulated from a junk car, and although this seems like a cheap source, it's actually such an inferior quality as to be almost useless. With the electrolytic process eventually all of the salt will be converted into NaHO, and this will still work as an electrolyte but it's less efficient as an electrolyte. So depending on when you decide to stop the reaction, it may become necessary to exchange the solution.
@@kayakMike1000 I made an error. Some of the the chlorine will be out gassed, while the majority will probably be reacted into ferric chloride and sodium chlorate.
If you use the thermal method and put either steel wool or turnings into a metal container with holes - you can ignite a portion and then air boil the rest until it stops melting and increasing its temperature. The resulting solid mass has to be broken up - After this its a case of using a hydraulic press and a screen. The big chunks are melted Iron chunks ranging from large to granular - The resulting powder ranging from dust to caster sugar size is your oxide - I have to say it is highly reactive and my preferred method as it is less messy. I found this by accident one day - It is called the Basic Oxygen Process - pioneered by a gentleman call William Kelly from my research - except it was Henry Bessemer was given all credit for the process and Kelly lost out, even though there is historical evidence that he contributed a lot to this process - I also made an instructable many years ago demonstrating this process in action.
A variable power supply was recommended, but I have old computer power supplies that can supply 3v, 5v, or 12v. I suspect that 12v will certainly go faster, but risks over-volting. Most PSUs can supply the most watts on the 5v rail, and 3v would end up being the most efficent, but will take longer and or require higher surface area for the anode and cathode.
Very informative, but I think I am out of my depth! Your descriptions are so scientific that I would need to go back to 8th grade and retake chemistry (beginning) Really want to learn this stuff but you are moving way fast for my simple ol' mind(60 yrs)
I think the most efficent way of seperating water from iron hydroxide is boiling off the water, also you can keep boiling after the water is gone to convert the iron hydroxides to iron oxide, i used this method for my experiment
5:17 for a second... I thought I was smart, then I remembered this is electrolytic and not galvanic. I cringed a little inside. Thanks for making me use my brain a little more than normal and jogging my memory. Much appreciated. I will forever remember my chemistry prof repeating, "I'm POSITIVE I have a cat in the garage." Over and over. Professor Nipe... thanks for being (sort of) helpful.
That red dye like iron oxide can be produced by taking Iron oxides produced in this video and putting them in a microwave oven rolled in fiberglass for 15-30 second intervals until it's done . The fiberglass is to protect the microwave oven's dish or any dish used from the heat produced by the iron oxide, which will glow red while being heated. Be careful not to unintentionally stain anything with the end product, because you either have to use Hydrochloric acid to clean it up or the object is fire engine red for the rest of eternity.
It would be a slower process but what about h202 and vinegar to dissolve the metal, then add naoh and filter? It’s more of a set and forget method and doesn’t take electricity it just takes time and household chemicals that aren’t as brutal as HCl
GREAT VIDEO!!! but just in case anyone needs IRON OXIDE for THERMITE, you can also go to a masonry supply store and buy it in bags. They literally sell bags of rust as dye for mortar
mayb u can cleensweep a mechanic-shop (iron oxide from welding and grinding) -or even a dockyard. I came across a bulkhead wall lately where large chunks of rust fell off.
How about this: 1, Steel wool into the grill separated from the fire so it only get really heated up. 2, Water+NaCl+the steel wool-->Fe2O3 3, Heat the powder upp to make the iron hydroxide get into iron. 4, Use magnet to separate Fe2O3. 5, You now have got pure Fe2O3. This should be an easy way to get many kilograms of Fe2O3.
Why You Didn't Try Sodium Hydroxide? It Will Oxidized The Iron To It Oxide & NaOH Regenerate, It Produced Hydrogen At The Copper Cathode, So it doesn't corroded.
@@cuocsongbinhyen3438 He Show Simple Way Of Getting Iron Oxides. Electrolytic Method, Where Iron Anode Is Corrode In Salt Or Sodium Hydroxide Solution. H2O = H - OH is broken to Hydrogen Gas At Cathode & Free Hydroxy Ion At Anode. But Iron Anode Corrode Away Into An Dark Insoluble Precipitate. Anode Corrosion Fe + 3 OH = Fe(OH)3 Dehydration 2 Fe(OH)3 = Fe2O3 - 3 H2O Salt, Caustic Soda (Sodium Hydroxide) Is Just Added To Make Water Conductive To Electricity. Sodium Bisulphate, Acetic Acid Will Only Cause Electroplating.
A couple comments from a fellow chemistry enthusiast: - You might notice the cell getting rather hot! This is because iron already "wants" to oxidize in water. It's rather slow without adding some extra incentive (like acid), though. You can force the reaction by adding more voltage (as shown), but this is very wasteful of electricity -- you already have solid, metallic electricity in the reaction, so it should be exothermic already; you're adding fire to fire. - The last time I was doing this, I used a hybrid method: As mentioned, neutral salts are handy, because they facilitate electrolysis without entering into the reaction itself (much). Rather than an unrelated salt like sodium chloride, suppose we started with a salt of the metal: ferrous chloride or sulfate. What's great about this is, if you have a neutral solution of a ferrous salt, it will precipitate Fe(OH)3 as soon as it is oxidized slightly (if fully oxidized, it would become one part Fe(OH)3 precipitate and two parts Fe(III) in solution). If we reduce the Fe(III) back to Fe(II) with more iron (which draws more iron back into solution, keeping the concentration constant), we have a catalytic reaction, which needs only air bubbling to speed up. You do want to do this with a large quantity of iron, so the surface area is reasonable. It will still take weeks to "digest" some kilograms of metal, but it can be left in a corner, forgotten, without taking up valuable fume hood or other lab space. The byproduct is a fine grained Fe(OH)3 with a reasonable light brown color (use it for staining concrete?). - Finally, all these methods produce some combination of hydration and incomplete oxidation (the black product from your electrolytic method is probably half magnetite, or some related hydrated intermediate). The final necessity is calcination. Use a furnace, torch or other heating method (charcoal fire?) to bring the material to red heat (about 700C). Stir it around and allow exposure to air. It should bubble and froth a bit, due to escaping gas (mostly steam). The finished product should be identical to the beautiful brown, almost purplish red product that's used commercially. Safety note: I once tried to ignite a thermite using the Fe(OH)3 directly. Although I didn't lose my eyebrows on that one, I can't say I recommend it for anyone! Since all rust is formed in the presence of water, always ensure your material is calcined before mixing it with other chemicals!
Tim Williams I actually did try an air bubbling method with a ferrous salt but it took way too long to get reasonable results. I didn't have enough iron oxide to make for a good video. The process does work, but i have viewers to appease ;) you are right about making sure the metals and oxides are as dry as possible, preferably with calcination. I'll see if i can cover that in the thermite video.
Hi. I just re-watched your video. I am wondering how to go about purifying some rust into pure iron oxide? I have a big heavy bucket full of big pieces of rust that have come off my old digger as thick layers. I would like to make a thermite mix from this.
NurdRage Hey NurdRage, this videos seems to be very good (like the others). I have just one question: To the third part (The electrolysis), how much voltage did you used? I really want to know :)
the higher the voltage the less electorate needed. I have found that for making rust it is better. just watch the amperage so you do not start to boil off the water and ignite the H2 and O2. I would start with 3.5 volts remember it is a " experiment " "Be ever vigilant"
Alright rust bluing. I use a bath of salt, vinegar, hydrogen peroxide to etch some of the knives I make. I recently saw a video where they guy was saying to do a proper "rust bluing", that you needed to put the steel into a boiling salt hydrogen peroxide bath and take it out, put it back in, take out, put it back in, etc. I've heard other knife makers say that putting the etched blade in hot (usually boiling water) will make the etch "set". My question is, at what temperature does the iron oxide change from Fe2O3 to the Fe3O4 form used for "rust bluing"? (I cant remember what they were exactly but it is something like that after heating). I'm not so hot on the idea of boiling the epoxy and micarta handle components I often use, but would let them sit in 160 degree water for a bit if that would do the trick.
There is a way to get fairly pure iron oxides for "free" (you still have to spend some money). Just buy a pack of peanut, there is a small package inside, it is iron oxides. The function of iron oxide in there is to consume the leftover oxygen after the peanut is sealed. Most likely the reaction is FeO --- Fe2O3.
and two birthday sparklers warped in 2 layers of cooking foil will start the reaction for tho having trouble getting mg ribbon. the foil traps a lot of wasted heat making them burn hotter
Great vid very informative, been using FE304 for a biochar fertilizer mix, it was expensive to buy here in Northern Thailand so I was looking at making it myself, you have put me off the idea, mission accomplished
If you used sodium bisulfate as the electrolyte, then why couldn't you have just raised the cathode up a bit and use a coiled wire for the anode so that the wire would dissolve but not be turned back to iron?
Sparklers are a very bad way to ignite thermite. You risk ingition too early by the sparks it throws, like when your standing right next to it with your hand over it.
Sodium hypochlorite + steel wool equals a dark brown mess in about a day. Found this when I was cleaning something a while back. Left the wool in the bleach over night. How pure is the dry powder left over? I also use Sodium hypochlorite to strip copper from other metals. Copper oxidizes slower than most, so done right i can separate the copper easily from the other oxidized metals.
Im making iron oxide from vinegar, Should I chemically clean it for a better burn? Also, What burns hotter, Iron oxide or copper? Would you do a video on the two different thermites? I find that just learning the different methods of making Iron oxide is very amazing.A very big fan.
3:50 That looks just like a Martian atmosphere. Interesting thing is that the real Martian Atmosphere does consist of some suspended iron oxide, which is what you're seeing in the video.
I understand the goal was to make iron(III) oxide. But, I was wondering if the electrolysis method, when dried heated in an anaerobic environment, produces iron(II) oxide, or magnetite, or something else. My last question is, what temperature is needed to convert the iron hydroxides to iron oxides. My goal is to make a magnetic powder to mix into a epoxy forming a composite material with magnetic properties, that can be easily formed.
i wish you could be my tutor i am studying a lot i love chemistry it blows my mine on how many chemicals that can be made someday i want to find someone that would help me i have problems with writhing equations thank you for your videos you are a very smart chemist i wish i was half as smart as you
if you are going to make your own youre probably better off using CuO2 as an oxidizer, as it should be easyer to make, though still Iron powder is probably cheeper and easyer just to buy.
This is the only video I've seen on RUclips that shows the reduction of iron oxide to metallic iron using electrolysis - even though that wasn't the intent of the video. I've found sources claiming that electrolysis of iron chloride can yield metallic iron, but I wasn't successful when I attempted it. I'm interested in reducing iron ore using electrolysis - would you have any information or tips to point me in the right direction? Thanks!
I'm using the electrolysis method and my water is noticably bluer then yours and has a clear layer on top but that might be because I used a lot of salt or because of me using an copper wire instead of a iron wire
what about boiling down urine and using for electrolyte? the urea with the salt somehow cooperate that it can get very concentrated so you get even more current.
I heard that if u heat up and evaporate all the water in ferric chloride it will decompose and make red iron oxide and chlorine gas. Could u do an episode on it?
Instead of using water and air to rust steel wool, would it not work to simply ignite the steel wool and let it burn in air to produce iron oxide, like you showed in another video?
Or even easier, just go to the beach and locate a patch of black sand, get out a magnet, and pick up all the Fe3O4 you want. Though you might want to pan it first to get the gold out before hitting it with a magnet.
is supposed to be for my solution is grey and black and very magnetic so it's basically a big mass of iron filings nanoparticulate at best and larger. I'm wondering if at this point I should pump some oxygen through it or perhaps some ozone although I know that it will oxidize with heat later on after I dry it I'm wondering if it would be easier to just do it now pumping some air oxygen or ozone through the solution
Why not precipitate the Fe(OH)3 with urea? I've never used it myself, but I remember my analitical chemistry book had a photo showing clean, well-formed, solid Fe(OH)3 that had been precipitated using urea. Maybe you can just filter that and it won't clog the filter paper.
Electrolysis breaks up H2O 6 times more easily than D2O or HDO. So take a few liters of water and start electrolysis. The more you will electrolyse it, the higher D2O concentration will be. Note that you will need to add some salt/base/acid to make electrolysis work so distill your final product to remove it.
My pit bull ate an entire box of S.O.S. steel wool soap pads and shit iron oxide for a week.I suppose you can use this method,but it may change the odor of the Thermite just a bit.
LOL
pit bull accelerated ferric chloride method haha
My pit bull eats everything and somehow survives near death every time
It's better than the smell of urea imo
Blim The Toolman that mean it smells good lmao
the cheapest way to get iron oxide is to buy a ford pick up
Lmao! You know what ford means dont ya?! Fix it again, tony.
@@lemuelseale1640 i thought Fix It Again Tony was the acronym of fiat.. ford was first on race day
Mark Short its a quote from the show king of the hill. I think from the character dale gribble lol
Ok
@@markshort9098 you obviously never drove my truck ,the only thing my truck will do first , is it will be my first truck to go to the scrap yard
Iron oxide is always available if you don´t want it and pretty complex to get when you really need it :/
Universal phenomenon, my friend.
If you're interested, theres a hydrothermal method can make iron oxide with interested properties. If you use a solution of iron chloride and a sugar (sucrose or glucose work well) and put the solution in a hydrothermal reactor you'll end up with iron oxide nano spheres surrounding a nano sized carbon ball scaffold. Filter and dry to powder and then heat to several hundred degrees burns on off the carbon leaving a hollow sphere of ironoxide. I'm curious to see if it make better thermite. I'll make some in a video in the near future probably
TheChemLife Seems cool. Any idea if this is commonly used in nano research or is it just one product from an older bit of research?
ThePharphis I realized I posted that with the wrong channel, I use it in my nanotech research on my other channel, the thought emporium. Same process, but I use it to make glowing nano particles
TheChemLife Cool, thanks for answering
TheChemLife Interesting! I don;t have a hydrothermal reactor or an easy means to reach several hundred degrees but the process does sound fascinating.
TheChemLife aha.. nanothermite is of what i recall created through an organo-electric process where the aluminium is formed among the iron oxide, being also very well mixed up upon being created
If you run a magnet through fine dry soil, particularly red soils you tend to pick up a noticeable amount of iron. These little pebbles tend to be very tiny from my experience, less than 1cm. I would imagine they would be easy to grind into a fine powder for oxidation by taking advantage of a large surface area!
“Yeah I’m still easily impressed despite having a PhD” 😂 this is my favorite science channel and I thank you greatly.
This video also took way longer to make than i expected. Oh, well, better late than never.
Do you guys like the longer more comprehensive video format? or do you prefer shorter videos (~4mins)?
NurdRage Longer videos with an in depth explanation. I can get more into the video and better understand your steps that way.
NurdRage NurdRage, I must know, is this your real voice?
I agree, I enjoy the chemistry.
NurdRage I wasn't even thinking about it as a turd solution until you mentioned it, then I began to laugh hysterically. Thank you for that. :)
NurdRage I like the longer videos.
I find that the easiest way to ignite thermite is with glycerine and potassium permanganate - it also gives an inherent time delay to allow you to walk away from it before the reaction starts and doesn't require any magnesium.
You can also perform the electrolysis inside, near candles. This drastically increases the chance for hydrogen combustion setting the entire room and you on fire.
I don't know WHY you would want to set your face on fire, but you can.
I laughed 😂
I needed some ironoxide for my chemiluminescense experiment, I made it by a percipitation reaction. I mixed iron sulphate with sodiumhydroxide, than I removed the water and was left with ironoxide. It's a really fast way but the downside is that you need iron sulphate :)
you can just use most metal salts like copper sulfate
@@uxleumas not for making iron oxide tho bruh
OKE DIT IS DE LAATSTE PLEK WAAR IK JOU OOIT HAD KUNNEN VERWACHTTEN
Yeah, thats like buying irun oxide but with a lot of extra work,lol
Hint: "washing soda" is sodium carbonate. Ferrous Sulfate is sold as moss killer in hardware stores or garden stores. Cheap. Ferrous Hydroxide if Lye used, which oxidizes or use as is (thermite Al works with NiO, MnO, CuO, FeO). On thermal drying Fe3O4 formed.
NurdRage, you are not alone. I also have a PhD (of sorts) and am also easily impressed. i think its because I understand how amazing the process is behind what I am witnessing. I am still amazed by turbine engines for example. Drives my wife nuts.
Typically, only those who do not understand something find it uninteresting.
Wayne Robinson Oh god - that means she WAS pregnant!
+Matthew Marting: I feel like somewhere in there, there's a joke about Matthew's android wife
@@sbaromski those two things arent really correlated imo?
you like turbofans or turbojets?
If you want iron oxide you can scrape the bottom off my piece of shit car
***** u idiot iron oxide doesnt form on cars lol r u serious cars r made of aluminium and glass like from the beach i went to the beach once and there was sand which is also known as silicon dioxide, a covalent network substance (i.e. covalent molecules all covalently bonded to each-other as opposed to relying on IMFs), which can be turned into glass and iron oxide absolutely does form on cars as the (typically) nickel galvanising layer wears away and exposes iron which is then oxidised but u r a idiot nd no wonder u hav a shit car cos ur an idiot lol do u even no physics
antiswattt3 please reread my post because I'm seeing that you obv dnt understnd wat i meant stfu u idiot lol ur mom
***** I love Jesus & God, He created ceverything. The Big Bang is a lie.
Did I do good, Senpai?
God told me the Earth is a torus. ;C
Roberto F Satan told me that the Earth is a triangular prism.
nurd rage i really have respect for you . you made me tha i want to be a chemist i even built my own mini lab and i always watch evry video so thanks greetings from a twelve year old boy from malta
Still doing chemistry?
Hope you're still nerd raging, 7 years later.
9+ minutes is amazing! This will be really interesting and I hope you continue with this style of video. I want to emphasize that I only want this if you have 9+ minutes of things to say about the subject. Don't let the pressure of needing a longer video compromise the excellence in quality that we have grown to love! Keep up the good work.
I work at an auto parts store, where we have a brake rotor lathe. I got just about all the iron filings I want!
If your nearby store has a brake lathe, you might could ask for them to give you some. It just gets dumped in the dumpster anyway.
If you use steel wool wash it off with dish soap first (Dawn works best) cuz there's an oil on the steel wool to keep it from rusting. It speeds things up A LOT. lol I found this out looking for info on making old-timey DIY wood stain from steel wool and acetic acid.
Thank you so much for your videos!
I found myself experimenting (successfully) with an old bit of iron/steel wool to see if I could get some rust.
1. I washed it in dish detergent to rid it of oil residue.
2. I immersed it in hydrogen peroxide solution (3%) in an empty water bottle.
3. Put it in window sill and added pinch of sodium chloride.
4. It worked in a week or so.
I'm not joking, I was actually looking for a blueberry pancake recipe. Might try this one day, though.
You can avoid that foaming when precipitating the iron, if you just use sodium hydroxide instead of baking soda. This doesn't release CO2 and you also dont get a mixture of iron hydroxide and carbonat. I personally prefer this method because it's somewhat cleaner and easier to work with. Also you don't need to dilute and decant it, since you can just let it sit for a few hours in a cold environment and then filter it.
i think he was going for more common home chemicals, also baking soda has that nice co2 bubbling as an indicator i guess, but yeah NaOH is probably best
LONGER VIDEOS PLEASE I LOVE SCIENCE
TacoPugs_ FTW YEAH SCIENCE BITCH!
Jesse Pinkman Yo yo yo!
Jesse Pinkman 3 to the 3 to the 6 to the 9!
represents the abq what uuup biaatch
I find that white vinegar is a useful catalyst and scrap iron for cans can be used. Iron (II) acetate is unstable to oxidation while iron (III) acetate breaks down into iron hydroxide, releasing the acetate for further reaction. With an ice cream container, a liter of vinegar and a few squashed cans you can make a kilo of oxide a week. Cheap white vinegar is factory made now and is literally just acetic acid. As a bonus the unreacted acid will evaporate off when you're done.
I like to come back to this video periodically whenever I have a new update, so here it is.
In my case, the peroxide would the most expensive investment...until I found some septic treatment that is 15-20% hydrogen peroxide at $7 a gallon. However, even with shipping it's still cheaper to buy 20lbs of rust from a ceramics supply online, than it is to invest in the time and reagents. If youre sketchy on the quality, you can still make a weak pirranah solution to convert impurities into soluable or separable salts and particles. But I doubt the effort would be worth it.
For those thinking that just adding peroxide to rust or iron with work, yes it will, but it's highly inefficient and the rust itself seems to be a catalyst to decompose the peroxide, meaning that as rust is created, the less peroxide their is to react and thus wasting your reagents. I have 15g of red rust I've been reacting under 50ml of the above concentration of peroxide going on six days. Since the rust I used is the result of three refinement and filtering steps (including magnetic and mass graduation) I doubt my sample is that impure that concentrated peroxide would continue to react almost a week later at an average temp of 80F. The only thing I can think of for it's continued reaction is that iron oxide has a catalytic property with H2O2 that would give a false positive for contaminates or continued oxidation of trace iron.
Most don’t know that steel wool is shipped coated with oil for rust protection. If you use it for anything like trying to rust it or anything else, you should wash it with acetone or lacquer thinner or similar. That’s probably why in this video it didn’t rust extremely well....
Are you aware that it looked like you were stirring around a turd?
I haven't watched your video's in a few years because my computer broke and i simply could not check all my subscriptions on an xbox. I got a new computer recently and this is the first video I'm watching since then. I'm still amazed by the quality of your production and your attention to detail. Thank you
So I have no idea whether or not anyone will see this, but I just wanted to drop in. I am in High School and I am writing a paper for forensic science about dangerous chemicals/materials and whether or not we (The U.S) should place higher restrictions. My main argument is the restrictions we'd have to put in play to ban ONE thing: Thermite
Hypothetically say that we put restrictions on the purchase of fine iron oxide and aluminum powders that most metallurgy workers use for their thermite (readily available from Wal-Mart and Amazon, as well as others). With this, you would need some form of permit saying you're a metallurgy worker or something similar. So because of these restrictions, obviously these powders would be a lot harder to get your hands on.
I'm making a counter-argument to the proposal in favor of 'restricting' thermite and other chemicals.
Using this video and the one where Cody's Lab made thermite with aluminum foil, I'm pressing the argument that thermite is something we pretty much can't do anything about. If we put limitations on the powders, it's worth mention that all someone needs is a sheet of aluminum foil and a box of steel wool to show you how unhappy they are.
Not sure if anyone cares!
Vinegar on steel wool forms perfect dust like iron oxide.
I realize this is an ancient video, but I wanted to add some observations of my own which I made recently. I have made iron oxide using the electrolytic method. I used sodium bicarbonate as an electrolyte, and did not observe the passivization effect you encountered. I did not want to use sodium chloride because the iron oxide was for another experiment (not thermite) and needed to be substantially chloride-free. The things I did differently from you:
-my sacrificial anode was a piece of cast iron, not steel like your nail. I don't know if this has an effect, but thought I'd mention it
-the electrolyte was diluted: 4% NaHCO3
-I used a low but constant current of 0.45A from my bench power supply. Yes it takes longer, but it worked.
I did it with sodium hydroxide and no current appeared, I turned into NaCl
2:44 *the forbidden cake mixture*
4:27 drying iron oxide on top of brake rotors, very appropriate
Nice observation. Very appropriate
Thank you Seth, very cool!
An artis would tell you that Iron colors range from Indian red to black to yewwow to silver (goethite). You need Fe3O4, either heating Fe2O3 or FeO. You have water in your "Iron Oxide" and as you.know water doesn't help anhydrous reactions.
If you were to use a stainless steel nail in the electrolytic method, wouldnt it produce cancerogenic chromates ?
(Since the chromium could easily be oxidized to chromium-(III)-ions which would then react with the bleach)
Found a nice way to remove the salt. Boil down the iron oxide tell dry in a pie tin and use a large magnet on the bottom. The iron oxide is easily rinsed with no loss.
I have 30lbs of railroad spikes, so I'm using the electrolitic process while running a bubbler through it. The extra oxygen from the bubbler helps to both react FeOH into FeO3, as well as prevent buildup on the electrodes.
I had tried also to grind up and convert rust flakes accumulated from a junk car, and although this seems like a cheap source, it's actually such an inferior quality as to be almost useless.
With the electrolytic process eventually all of the salt will be converted into NaHO, and this will still work as an electrolyte but it's less efficient as an electrolyte. So depending on when you decide to stop the reaction, it may become necessary to exchange the solution.
What happens to the chlorine?
@@kayakMike1000 I made an error. Some of the the chlorine will be out gassed, while the majority will probably be reacted into ferric chloride and sodium chlorate.
If you use the thermal method and put either steel wool or turnings into a metal container with holes - you can ignite a portion and then air boil the rest until it stops melting and increasing its temperature. The resulting solid mass has to be broken up - After this its a case of using a hydraulic press and a screen. The big chunks are melted Iron chunks ranging from large to granular - The resulting powder ranging from dust to caster sugar size is your oxide - I have to say it is highly reactive and my preferred method as it is less messy. I found this by accident one day - It is called the Basic Oxygen Process - pioneered by a gentleman call William Kelly from my research - except it was Henry Bessemer was given all credit for the process and Kelly lost out, even though there is historical evidence that he contributed a lot to this process - I also made an instructable many years ago demonstrating this process in action.
I understand nothing but for some reason I like your videos!
A variable power supply was recommended, but I have old computer power supplies that can supply 3v, 5v, or 12v.
I suspect that 12v will certainly go faster, but risks over-volting. Most PSUs can supply the most watts on the 5v rail, and 3v would end up being the most efficent, but will take longer and or require higher surface area for the anode and cathode.
Very informative, but I think I am out of my depth! Your descriptions are so scientific that I would need to go back to 8th grade and retake chemistry (beginning) Really want to learn this stuff but you are moving way fast for my simple ol' mind(60 yrs)
I think the most efficent way of seperating water from iron hydroxide is boiling off the water, also you can keep boiling after the water is gone to convert the iron hydroxides to iron oxide, i used this method for my experiment
5:17 for a second... I thought I was smart, then I remembered this is electrolytic and not galvanic. I cringed a little inside. Thanks for making me use my brain a little more than normal and jogging my memory. Much appreciated. I will forever remember my chemistry prof repeating, "I'm POSITIVE I have a cat in the garage." Over and over. Professor Nipe... thanks for being (sort of) helpful.
That red dye like iron oxide can be produced by taking Iron oxides produced in this video and putting them in a microwave oven rolled in fiberglass for 15-30 second intervals until it's done . The fiberglass is to protect the microwave oven's dish or any dish used from the heat produced by the iron oxide, which will glow red while being heated. Be careful not to unintentionally stain anything with the end product, because you either have to use Hydrochloric acid to clean it up or the object is fire engine red for the rest of eternity.
It would be a slower process but what about h202 and vinegar to dissolve the metal, then add naoh and filter? It’s more of a set and forget method and doesn’t take electricity it just takes time and household chemicals that aren’t as brutal as HCl
GREAT VIDEO!!! but just in case anyone needs IRON OXIDE for THERMITE, you can also go to a masonry supply store and buy it in bags. They literally sell bags of rust as dye for mortar
good place to start to look for it is at any big hard-where store in the concrete coloring part
I’ve learnt more from this guy than any science lesson I’ve had at school
mayb u can cleensweep a mechanic-shop (iron oxide from welding and grinding)
-or even a dockyard.
I came across a bulkhead wall lately where large chunks of rust fell off.
3 year sub, and all I do with my life anymore is school, youtube, and science! It's awesome! Keep it up!
How about this:
1, Steel wool into the grill separated from the fire so it only get really heated up.
2, Water+NaCl+the steel wool-->Fe2O3
3, Heat the powder upp to make the iron hydroxide get into iron.
4, Use magnet to separate Fe2O3.
5, You now have got pure Fe2O3.
This should be an easy way to get many kilograms of Fe2O3.
This would also be cheaper if you have or are a mechanic with a shop and a big bolt bucket where the bolts can be turned to iron oxide.
"Black crud become, red crud"
I love this.
Why You Didn't Try Sodium Hydroxide? It Will Oxidized The Iron To It Oxide & NaOH Regenerate, It Produced Hydrogen At The Copper Cathode, So it doesn't corroded.
Pls writting chemical
@@cuocsongbinhyen3438 He Show Simple Way Of Getting Iron Oxides. Electrolytic Method, Where Iron Anode Is Corrode In Salt Or Sodium Hydroxide Solution.
H2O = H - OH is broken to Hydrogen Gas At Cathode & Free Hydroxy Ion At Anode. But Iron Anode Corrode Away Into An Dark Insoluble Precipitate.
Anode Corrosion
Fe + 3 OH = Fe(OH)3
Dehydration
2 Fe(OH)3 = Fe2O3 - 3 H2O
Salt, Caustic Soda (Sodium Hydroxide) Is Just Added To Make Water Conductive To Electricity. Sodium Bisulphate, Acetic Acid Will Only Cause Electroplating.
A couple comments from a fellow chemistry enthusiast:
- You might notice the cell getting rather hot! This is because iron already "wants" to oxidize in water. It's rather slow without adding some extra incentive (like acid), though. You can force the reaction by adding more voltage (as shown), but this is very wasteful of electricity -- you already have solid, metallic electricity in the reaction, so it should be exothermic already; you're adding fire to fire.
- The last time I was doing this, I used a hybrid method:
As mentioned, neutral salts are handy, because they facilitate electrolysis without entering into the reaction itself (much). Rather than an unrelated salt like sodium chloride, suppose we started with a salt of the metal: ferrous chloride or sulfate.
What's great about this is, if you have a neutral solution of a ferrous salt, it will precipitate Fe(OH)3 as soon as it is oxidized slightly (if fully oxidized, it would become one part Fe(OH)3 precipitate and two parts Fe(III) in solution). If we reduce the Fe(III) back to Fe(II) with more iron (which draws more iron back into solution, keeping the concentration constant), we have a catalytic reaction, which needs only air bubbling to speed up.
You do want to do this with a large quantity of iron, so the surface area is reasonable. It will still take weeks to "digest" some kilograms of metal, but it can be left in a corner, forgotten, without taking up valuable fume hood or other lab space.
The byproduct is a fine grained Fe(OH)3 with a reasonable light brown color (use it for staining concrete?).
- Finally, all these methods produce some combination of hydration and incomplete oxidation (the black product from your electrolytic method is probably half magnetite, or some related hydrated intermediate). The final necessity is calcination. Use a furnace, torch or other heating method (charcoal fire?) to bring the material to red heat (about 700C). Stir it around and allow exposure to air. It should bubble and froth a bit, due to escaping gas (mostly steam).
The finished product should be identical to the beautiful brown, almost purplish red product that's used commercially.
Safety note: I once tried to ignite a thermite using the Fe(OH)3 directly. Although I didn't lose my eyebrows on that one, I can't say I recommend it for anyone! Since all rust is formed in the presence of water, always ensure your material is calcined before mixing it with other chemicals!
Tim Williams I actually did try an air bubbling method with a ferrous salt but it took way too long to get reasonable results. I didn't have enough iron oxide to make for a good video. The process does work, but i have viewers to appease ;)
you are right about making sure the metals and oxides are as dry as possible, preferably with calcination. I'll see if i can cover that in the thermite video.
Surprisingly great result with the electrolysis method :0
Hi.
I just re-watched your video.
I am wondering how to go about purifying some rust into pure iron oxide? I have a big heavy bucket full of big pieces of rust that have come off my old digger as thick layers. I would like to make a thermite mix from this.
NurdRage
Hey NurdRage, this videos seems to be very good (like the others).
I have just one question:
To the third part (The electrolysis), how much voltage did you used?
I really want to know :)
the higher the voltage the less electorate needed. I have found that for making rust it is better. just watch the amperage so you do not start to boil off the water and ignite the H2 and O2. I would start with 3.5 volts
remember it is a " experiment "
"Be ever vigilant"
Alright rust bluing.
I use a bath of salt, vinegar, hydrogen peroxide to etch some of the knives I make. I recently saw a video where they guy was saying to do a proper "rust bluing", that you needed to put the steel into a boiling salt hydrogen peroxide bath and take it out, put it back in, take out, put it back in, etc. I've heard other knife makers say that putting the etched blade in hot (usually boiling water) will make the etch "set".
My question is, at what temperature does the iron oxide change from Fe2O3 to the Fe3O4 form used for "rust bluing"? (I cant remember what they were exactly but it is something like that after heating). I'm not so hot on the idea of boiling the epoxy and micarta handle components I often use, but would let them sit in 160 degree water for a bit if that would do the trick.
There is a way to get fairly pure iron oxides for "free" (you still have to spend some money).
Just buy a pack of peanut, there is a small package inside, it is iron oxides.
The function of iron oxide in there is to consume the leftover oxygen after the peanut is sealed.
Most likely the reaction is FeO --- Fe2O3.
2nd one acid cardonate high water use ? Do you Heat it! Faster removal off h2o and transfer off at least a percent no?
Dude you should narrate horror movies. You have an awesome voice!
Lol thats not how his voice sounds
I have done electrolyisi of Iron in salt water years ago
Should try hydrogen peroxide & salt. Best solution I've found so far to make iron oxide.
and two birthday sparklers warped in 2 layers of cooking foil will start the reaction for tho having trouble getting mg ribbon.
the foil traps a lot of wasted heat making them burn hotter
Great vid very informative, been using FE304 for a biochar fertilizer mix, it was expensive to buy here in Northern Thailand so I was looking at making it myself, you have put me off the idea, mission accomplished
If you used sodium bisulfate as the electrolyte, then why couldn't you have just raised the cathode up a bit and use a coiled wire for the anode so that the wire would dissolve but not be turned back to iron?
Sparklers are a very bad way to ignite thermite. You risk ingition too early by the sparks it throws, like when your standing right next to it with your hand over it.
Sodium hypochlorite + steel wool equals a dark brown mess in about a day. Found this when I was cleaning something a while back. Left the wool in the bleach over night. How pure is the dry powder left over? I also use Sodium hypochlorite to strip copper from other metals. Copper oxidizes slower than most, so done right i can separate the copper easily from the other oxidized metals.
Im making iron oxide from vinegar, Should I chemically clean it for a better burn? Also, What burns hotter, Iron oxide or copper? Would you do a video on the two different thermites? I find that just learning the different methods of making Iron oxide is very amazing.A very big fan.
2:48 yep thought of that the first time i tried making some
I'm so glad you're back!
you should make a video about the black snake experiment. .. like do it but show different ways it could be done
Wouldn’t the chlorine gas react with the iron tho. When u electrolysis salt water.
3:50 That looks just like a Martian atmosphere. Interesting thing is that the real Martian Atmosphere does consist of some suspended iron oxide, which is what you're seeing in the video.
could you do a vid on how to make easy aluminium powder or filings for thermite?
I understand the goal was to make iron(III) oxide. But, I was wondering if the electrolysis method, when dried heated in an anaerobic environment, produces iron(II) oxide, or magnetite, or something else. My last question is, what temperature is needed to convert the iron hydroxides to iron oxides. My goal is to make a magnetic powder to mix into a epoxy forming a composite material with magnetic properties, that can be easily formed.
i wish you could be my tutor i am studying a lot i love chemistry it blows my mine on how many chemicals that can be made someday i want to find someone that would help me i have problems with writhing equations thank you for your videos you are a very smart chemist i wish i was half as smart as you
if you are going to make your own youre probably better off using CuO2 as an oxidizer, as it should be easyer to make, though still Iron powder is probably cheeper and easyer just to buy.
now THAT is an awesome teacher!
This is the science teacher we all wanted in high school but never came close to getting lol
iron oxide iron and oxygen molar mass 159.69gmo/l density 59.7 g/cm fe203-
what about aluminum powder...do you have a method for making that at home?
I'm studying chemical engineering because of you!
Is Iron Oxide not just rust from putting some iron in a tub of water? :0
This is the only video I've seen on RUclips that shows the reduction of iron oxide to metallic iron using electrolysis - even though that wasn't the intent of the video. I've found sources claiming that electrolysis of iron chloride can yield metallic iron, but I wasn't successful when I attempted it. I'm interested in reducing iron ore using electrolysis - would you have any information or tips to point me in the right direction? Thanks!
How do I dispose of the leftover chemicals?
THE STIR BAR IS AWESOME
I'm using the electrolysis method and my water is noticably bluer then yours and has a clear layer on top but that might be because I used a lot of salt or because of me using an copper wire instead of a iron wire
wrong polarity
thank you for sharing your knowlegde with us peaseants i will be a great chemist inventor one day ,thank you
I've used thermite before it's really fun to do :) but just do it away from anything flammable.
what about boiling down urine and using for electrolyte? the urea with the salt somehow cooperate that it can get very concentrated so you get even more current.
I heard that if u heat up and evaporate all the water in ferric chloride it will decompose and make red iron oxide and chlorine gas. Could u do an episode on it?
Instead of using water and air to rust steel wool, would it not work to simply ignite the steel wool and let it burn in air to produce iron oxide, like you showed in another video?
Or even easier, just go to the beach and locate a patch of black sand, get out a magnet, and pick up all the Fe3O4 you want. Though you might want to pan it first to get the gold out before hitting it with a magnet.
How can we make sodium hypochlorite
Hey where would I buy equipment for things like this like a hot plate and viles ect
Put some iron in water for a couple days...agitating a few times each day. Remove iron, filter water and the iron oxide will be in your enhancements
is supposed to be for my solution is grey and black and very magnetic so it's basically a big mass of iron filings nanoparticulate at best and larger. I'm wondering if at this point I should pump some oxygen through it or perhaps some ozone although I know that it will oxidize with heat later on after I dry it I'm wondering if it would be easier to just do it now pumping some air oxygen or ozone through the solution
Why not precipitate the Fe(OH)3 with urea?
I've never used it myself, but I remember my analitical chemistry book had a photo showing clean, well-formed, solid Fe(OH)3 that had been precipitated using urea. Maybe you can just filter that and it won't clog the filter paper.
How about a heavy water video, out of see water, which contains more of deuterium or regular water which contains less
Electrolysis breaks up H2O 6 times more easily than D2O or HDO. So take a few liters of water and start electrolysis. The more you will electrolyse it, the higher D2O concentration will be. Note that you will need to add some salt/base/acid to make electrolysis work so distill your final product to remove it.
Iron choride can be use in thermite