@mrgreenguytoo recycling^2 Lol you should try diy-ing crude oil, atleast you could spend another couple hundred days building a steel apparatus like for the sodium lmao. I mean I guess it's just a metal distillation setup with wood or whatever in the reactor, when I tried it, all I got was like wood vinegar and once I got tar which smelled horrible lmao
@@_-noxxon-_you can use plastics. It's much easier this way. of course some problems (like using pvc that generates chlorine) but it's most of the time much cleaner if you know what plastics you put in.
@@stasi0238 yeah plastics are possible but the issue is always that if your temperature is high like from a blowtorch, it cracks it into smaller stuff like in my case wood vinegar
i like this type of content because green can upload videos which are bit low effort but still interesting at a fast pace, and work on the main channel whenever he thinks he has a good project. instead of procrastinating for months or longer.
@@yourenevergonnaknowwhoiam yeah this is pretty much it! I have so many projects I've recorded over the past year that I either didn't quite complete, or wasn't cool enough for a main channel vid
Metallurgy student here. Put a vacuum on the retort. Alkali and earth alkali metals are volatile and can be distilled off from otherwise unfavorable reactions. They make magnesium from ferrosilicon this way. This should also dampen the reaction somewhat. You can even try freezing out the vapors on the lid and then melting the sodium out afterward.
Chemists...... Try having a much larger volume receiving apparatus first lol. Hot gasses plus small diameter tube leading to an even smaller restriction equals back pressure and boom. So long as you're able to maintain an inert atmosphere too, you should be fine.
One thing that i think would work without having to change much is to leave the longer tube on the reaction vessel and let the reaction do its thing. The longer portion will be cooler, letting the sodium vapors reflux in the top instead of coming on over. Once the reaction is over, you could then just use your torch to heat the top cooler portion to let it distill on over. This would give the sodium vapors room to expand and cool without them pouring out. You'd just have to lightly heat the top to keep any sodium buildup molten so it doesn't clog the outlet. Alternatively, you could have a longer distillation tube and submerge it much deeper in oil to catch and cool all of the vapors before they can escape. Forming tiny blobs of sodium in the bottom of the oil. You risk suckback with this method, but it wouldn't be that bad of a thing since the oil would coat the inside of the vessel and prevent any sodium from reacting and making it more recoverable later on. I've done a lot of what you're doing here in terms of building such an apparatus and have had a lot of success in making fairly large amounts of cesium metal. If you'd like more advice, just let me know. 🙂
Is it just me or do you doubt he made any potassium in that first aluminium+KOH fire test? I feel like the KOH just melted and then reacted violently with the aluminium like potassium hydroxide does with aluminium to form potassium aluminate. The potassium emission happened just because there was a lot of potassium ions there.
You probably won't reply since you're like working on a project right now or doing something else, but I absolutely LOVE your content and your videos really are inspiring me to do chemistry! Mostly probably just stuff like displacement reactions and stuff like that, I will NOT be doing stuff with acids. At least yet. Thanks for making your videos :)
Sodium has low melting point. If you can put together some dry 1,4-dioxane (difficult), you can boil that sodium sludge you got and sodium will float+melt, resulting in floating sodium spheres. You will let them cool down and this is how you separate sodium from whatever junk is also present. Toluene is easier to source and dry (usually dry enough to be used as is), but sodium do not float in it (still coalesce somehow, but on the bottom, together with all other oxide impurities).
I think the reason for the crucible damage is due to sodium reacting with the carbon. At such high temperatures the sodium is probably dissolving the graphite or catalysing some reaction with it.
I always thought it was possible to extract sodium metal from one of its componds using aluminum metal. I knew that elements with high reactivity (like cesium) could be extracted from there compounds with a lower reactive element (like lithium) in a still. But I didn't have the time or the knowledge to prove that aluminum could do the same. But thanks to you, I now know that it is totally possible. Thank you Nilegreen/Mr.Green guy
This kinda stuff kinda help with the gaps of main channel uploads :p your content is awesome and i love how whacky your setups tend to be, it's just relatable to when i also do styff on my own and it's always the whackiest setups to do whatever im doing (not chemistry tho)
Love the second channel, can't wait for the next video! Btw maybe you could use a bit of potassium hydroxide to lower the fusion point and stay close enough to the potassium boiling point but without it flash boiling
Oh man i always think your videos are funny but its really awesome your doing chem videos too! Ive been really enjoying the ones you make. When in a pinch i used to dissolve KOH in absolute ethanol and bubble CO2 through it. The hydroxide is soluble whereas the carbonate is insoluble in ethanol. Filter and wash with more absolute ethanol. Id throw it in a round bottom with a vacuum adapter and heat it on a warm water bath under vacuum for a few minutes. Should give anhydrous potassium carbonate. Probably more work than what it was worth but I was broke lol
Nurdrage has already solved your problem of lowering the activation energy. You need to try the menthol catalysed method he developed. Just switch out magnesium for aluminum and let us know how it goes.
This was so cool. The fact that you started with stuff you can get from a hardware store and grocery store (excluding the furnace, but you can technically make one of those using stuff from a hardware store also) and produced sodium metal is incredible.
In pyrotechnics they use an alloy of magnesium and aluminum called magnalium because it's brittle and easier to grind into a powder. Having a more reactive metal in the mix should lower the temperature that the reaction gets started. Using turnings instead of fine mesh aluminum should slow the reaction down as well.
If you can bleed a little argon into the vessel while doing the reaction you should be able to allow the sodium to not react with trace oxygen before cooling enough to condense. Or make the "condenser" pipe a lot longer to again give the sodium enough time to condense back to liquid. Very neat process though.
If I could make a suggestion? In many thermates (non-iron/aluminum metal redox reactions) there is a few percent of sulfur added to the mix because the formation of Aluminum sulfide is exothermic and can jumpstart the main reaction, thus lowering the activation energy for the whole reaction. Try between 2-3% sulfur and see if that gives you something you can light with a magnesium ribbon. Additionally, if you kept the longer reaction chamber, you would probably have less boil over of unreacted reagents into your oil bath. Headspace is a factor in all still designs and just because you're distilling metal is no reason to disregard that.
I did that but with sodium chloride and once it took it exploded. The sulfur does reduce the activation energy a bit. Another thing that might be better is using a flux of sorts to bring the melt point down, preferably something that doesn't change the overall reaction and something that will scavenge the aluminum oxide. Although a more typical thermite mixed with the carbonate thermite might actually be closer to ideal if it doesn't alloy well with the alkali.
if you store KOH in the open it converts into potassium carbonate by itself. Drying it in the closed oven was not a good idea, because it had no access to the CO2 in the air to convert the residual KOH. Air actually has lots of CO2 in it already, if you can wait a few days.
Might be a stupid suggestion, but to speed the reaction, you could use a solvent and do the work in solution. My first thought was Borax (anhydrous, baked first) which would melt at a low temp but you'd reduce out elemental boron before the Sodium, and metallic aluminum wouldnt dissolve in it anyhow. Another simpler Sodium salt would be great but one problem with aluminum is you're trapped by anion choices: Halogens will create scary AlX3 vapours, Nitrates will create NOx gas and aluminum oxide which will plug your reaction up, and anything hydroxy or oxy will give the same problem minus the NOx. I feel like the best solvent would be an aluminum salt but they're all either refractory or volatile as hell. Alternatively, (possibly) better idea would be to have an excess of aluminum which can allow the reaction to occur at the molten surface where the sodium salt sits on top - but AlO3 will build up and form a refractory layer that will stop the reaction and maybe go pop. I'm just rambling at this point, this clearly worked albiet in a slightly terrifying manner, Cool as shit, thanks for the content. Please wear gloves
Maybe try adding an inert salt to lower the temperature of the melt. The eutectic point can be a few hundred degrees lower than the pure salt. If good melting facilitates the reaction and temperature drives the reaction, maybe having it melt at a lower temperature will slow down the reaction. I imagine the added dilution might also give some thermal mass to yeet the massive spike in exothermic heat
Looked at a random post from 2017, what you might have there is pure sodium. Apparently the other products are aluminum oxide, and aluminum carbide. So, that fire when cleaning your station with water might be sodium making hydrogen, or aluminum carbide making methane gas, or likely both. But, apparently the carbide would be a solid during the reaction, and the oxide would be a liquid, meaning the only gas would just be pure sodium.
Instead of doing that, you could use a process outlined by nurdrage where he catalized the reaction of sodium hydroxide and magnesium with menthol to mass produce pretty clean sodium.
Potassium carbonate is making by burning wood or charcoal and mixing ash with water. Potassium carbonate is soluble in water and you can filter out this solution. That is what too many potassium compounds is made with potassium carbonate
I think you should make science "slop" for this channel. It could help greatly with the funding while keeping viewers engaded. Under slop I mean creating a vid where you talk about recent news and advancements in chemistry or in science general, reacting to TikTok hacks or just talk about the overall scene of science or about related UA-cam content you like.
You could carefully try using finer aluminium powder, this could lower the activation temperature to below sodiums boiling point, though equally it could just make the reaction way too violent, but seeing as sodium carbonate is so unreactive that might be unlikely
5:54 I'm sure you def know this but please do not stare at burning magnesium as it literally can tear holes in your cornea which isn't ideal if you want to maintain a perfect vision lol
Yeah it's a common concern. Not usually anywhere near as bad as people make it sound though. I've stared at a lot of burning magnesium over the years. Magnesium powder fireballs used to be used for flash photography and the main danger was burning your hand rather than burning your eyes. But yeah it is very very bright and gives off some UV
I wonder if you could use a HFVTTC for the ignition of sodium carbonate and aluminum. It would be cool to make a low pressure container filled with argon and the stuff for sodium production, and then blast it with extremely high temperature plasma.
I mean you could do the reaction under pressure. It would theoretically increase sodiums boiling point above 1000C. Unsure the pressure needed and youd want it to be argon
perhaps your reaction was to vigorous because of aluminium powder? I would try with aluminium foil or eaven thicker pieces of aluminium. this would probably slow down the reaction and it wouldn all just burst out of the aparatus
It frustrates me that UA-cam's been stupid towards a Quality Science channel! They cannot change how important this kind of informative content is *UA-cam would be stupid if they didn't support creators of this quality. The way UA-cam handles their community guidelines is mind numbingly absurd. Yet stuff like "G-string camping videos" get fully supported *don't get me wrong, I fully support G-string camping videos. Why do those videos get supported but someone can make a well edited informative video that covers a difficult topic.. and yet that's not supported? Quality true crime content struggles to get any support & that's just one example. UA-cam overly abuses their control over what videos get monetized or whats gets flagged or copyrighted, even when the creator did everything correctly to be fully covered under "fair use" rights. Yet UA-cam still makes these people go thru a bunch of nonsense, trying to communicate with UA-cams joke of an official review process. Some of these creators put in so much effort into their videos & they follow all of youtubes rules as much as possible followed, yet UA-cam still throws them thru the ringer. People should be allowed to cover these topics but they don't care. They hit them with limited adds, etc. It just really frustrates me that UA-cam is making it really hard for these creators. Even tho they bring so much value to their company. I don't think UA-cam realizes that a huge percentage of their viewers are adults.. Not everything has to be made for kids... Idk i hope UA-cam improves because they really are a great platform but they got to get their shit together and support these creators who bring so much to their platform.
This totally should have been a main channel video. I understand why you wouldn't want to upload after your last video though. Eventually UA-cam will come around.
Aluminium chloride reacts with water, producing aluminium hydroxide (hard to react with) and hydrochloric acid (volatile, dangerous). Because it's a byproduct that is annoying to handle, maybe that's one possible answer for that.
@@mrgreenguytoo Ah, I am stupid. So you basically first reduced carbon, then sodium... Still few g of NaCl could form eutectic to lower melting point, but I have no idea really.
Green manages to take a seemingly efficient process and makes it as inefficient and dangerous as possible.
Absolute cinema
Difference between playing around and being serious is recording the results
this truly is science
I dare you to breathe through a hose to generate the CO2 required. Gotta cut your carbon footprint lmao
I was considering it for a while haha
@mrgreenguytoo recycling^2
Lol you should try diy-ing crude oil, atleast you could spend another couple hundred days building a steel apparatus like for the sodium lmao. I mean I guess it's just a metal distillation setup with wood or whatever in the reactor, when I tried it, all I got was like wood vinegar and once I got tar which smelled horrible lmao
@@_-noxxon-_you can use plastics. It's much easier this way. of course some problems (like using pvc that generates chlorine) but it's most of the time much cleaner if you know what plastics you put in.
Why not adding carbonated water?
@@stasi0238 yeah plastics are possible but the issue is always that if your temperature is high like from a blowtorch, it cracks it into smaller stuff like in my case wood vinegar
i like this type of content because green can upload videos which are bit low effort but still interesting at a fast pace, and work on the main channel whenever he thinks he has a good project. instead of procrastinating for months or longer.
@@yourenevergonnaknowwhoiam yeah this is pretty much it! I have so many projects I've recorded over the past year that I either didn't quite complete, or wasn't cool enough for a main channel vid
@@mrgreenguytooyes I love this format. Codyslab and explosions&fire vibes
"I'm just gonna mix random chemicals together and hopefully i'll find something that works." Sounds about right
Metallurgy student here. Put a vacuum on the retort. Alkali and earth alkali metals are volatile and can be distilled off from otherwise unfavorable reactions. They make magnesium from ferrosilicon this way. This should also dampen the reaction somewhat. You can even try freezing out the vapors on the lid and then melting the sodium out afterward.
Great video! It sucks that UA-cam takes down all your content.
:)
think YT is worried about his clumsiness
As is tradition for second channels, you should rename this video "HUGE SODIUM DRAMA"
No slop names plewse
The sodium situation is wild
SODIUM IS COOKED
Sodium situation is insane
Genuinely haven't seen a second channel use titles like that.
Chemists...... Try having a much larger volume receiving apparatus first lol. Hot gasses plus small diameter tube leading to an even smaller restriction equals back pressure and boom. So long as you're able to maintain an inert atmosphere too, you should be fine.
The Sodium Metal Situation is CRAZY
Glad to be here for this 2nd channel, love your content
alternate title: jon snow does chemistry
One thing that i think would work without having to change much is to leave the longer tube on the reaction vessel and let the reaction do its thing. The longer portion will be cooler, letting the sodium vapors reflux in the top instead of coming on over. Once the reaction is over, you could then just use your torch to heat the top cooler portion to let it distill on over. This would give the sodium vapors room to expand and cool without them pouring out. You'd just have to lightly heat the top to keep any sodium buildup molten so it doesn't clog the outlet. Alternatively, you could have a longer distillation tube and submerge it much deeper in oil to catch and cool all of the vapors before they can escape. Forming tiny blobs of sodium in the bottom of the oil. You risk suckback with this method, but it wouldn't be that bad of a thing since the oil would coat the inside of the vessel and prevent any sodium from reacting and making it more recoverable later on.
I've done a lot of what you're doing here in terms of building such an apparatus and have had a lot of success in making fairly large amounts of cesium metal. If you'd like more advice, just let me know. 🙂
Is it just me or do you doubt he made any potassium in that first aluminium+KOH fire test? I feel like the KOH just melted and then reacted violently with the aluminium like potassium hydroxide does with aluminium to form potassium aluminate. The potassium emission happened just because there was a lot of potassium ions there.
You probably won't reply since you're like working on a project right now or doing something else, but I absolutely LOVE your content and your videos really are inspiring me to do chemistry! Mostly probably just stuff like displacement reactions and stuff like that, I will NOT be doing stuff with acids. At least yet. Thanks for making your videos :)
It's our boy NileGreen again
Sodium has low melting point. If you can put together some dry 1,4-dioxane (difficult), you can boil that sodium sludge you got and sodium will float+melt, resulting in floating sodium spheres. You will let them cool down and this is how you separate sodium from whatever junk is also present. Toluene is easier to source and dry (usually dry enough to be used as is), but sodium do not float in it (still coalesce somehow, but on the bottom, together with all other oxide impurities).
Thanks for re uploding old exprmental madness videos🎉
cozy atmosphere right here
thank you
Hope this doesn’t get age restricted or de-monetised 😢
Oh hi!
I'm here before this channel gets big.
I'll be a part of history books.
Yippie!!!
Dig ur content MrG been watching for a while now, don't be discouraged by YTs.. bs. Allot of us love science vids!
nd Shout out to Houston Jones
I think the reason for the crucible damage is due to sodium reacting with the carbon. At such high temperatures the sodium is probably dissolving the graphite or catalysing some reaction with it.
"there are bold chemists and old chemists never both"
Congrats ! Very cool to see that in these trying times
I always thought it was possible to extract sodium metal from one of its componds using aluminum metal. I knew that elements with high reactivity (like cesium) could be extracted from there compounds with a lower reactive element (like lithium) in a still. But I didn't have the time or the knowledge to prove that aluminum could do the same. But thanks to you, I now know that it is totally possible.
Thank you Nilegreen/Mr.Green guy
This guys lives my dream of sounding smart enough that makes throwing some chemicals together sound reasonable
This kinda stuff kinda help with the gaps of main channel uploads :p your content is awesome and i love how whacky your setups tend to be, it's just relatable to when i also do styff on my own and it's always the whackiest setups to do whatever im doing (not chemistry tho)
Justice for our boy Mr.Green!
Hey dude, I love your videos. Keep it up ❤
Love the second channel, can't wait for the next video!
Btw maybe you could use a bit of potassium hydroxide to lower the fusion point and stay close enough to the potassium boiling point but without it flash boiling
Oh man i always think your videos are funny but its really awesome your doing chem videos too! Ive been really enjoying the ones you make. When in a pinch i used to dissolve KOH in absolute ethanol and bubble CO2 through it. The hydroxide is soluble whereas the carbonate is insoluble in ethanol. Filter and wash with more absolute ethanol. Id throw it in a round bottom with a vacuum adapter and heat it on a warm water bath under vacuum for a few minutes. Should give anhydrous potassium carbonate. Probably more work than what it was worth but I was broke lol
I had a lot of trouble finding this channel. I'm happy I did
Nurdrage has already solved your problem of lowering the activation energy. You need to try the menthol catalysed method he developed. Just switch out magnesium for aluminum and let us know how it goes.
Could it be done same way with NaOH and Al to get Na?
This was so cool. The fact that you started with stuff you can get from a hardware store and grocery store (excluding the furnace, but you can technically make one of those using stuff from a hardware store also) and produced sodium metal is incredible.
I think it should be called a shotgun distillation
I actually like these types of videos, shame youtube takes them down
that was a very enjoyable watch, nice
just watched your vid in the main channel, came here as soon i learned you got a new channel
In pyrotechnics they use an alloy of magnesium and aluminum called magnalium because it's brittle and easier to grind into a powder. Having a more reactive metal in the mix should lower the temperature that the reaction gets started. Using turnings instead of fine mesh aluminum should slow the reaction down as well.
If you can bleed a little argon into the vessel while doing the reaction you should be able to allow the sodium to not react with trace oxygen before cooling enough to condense. Or make the "condenser" pipe a lot longer to again give the sodium enough time to condense back to liquid. Very neat process though.
Nice, I like these more in depth videos!
We have the same Chinese heating stirring round thing with the confusing labelling ! We're bros !
I love this guy so much. No homo but this is some of the best content I've seen in a while.
If I could make a suggestion? In many thermates (non-iron/aluminum metal redox reactions) there is a few percent of sulfur added to the mix because the formation of Aluminum sulfide is exothermic and can jumpstart the main reaction, thus lowering the activation energy for the whole reaction. Try between 2-3% sulfur and see if that gives you something you can light with a magnesium ribbon.
Additionally, if you kept the longer reaction chamber, you would probably have less boil over of unreacted reagents into your oil bath. Headspace is a factor in all still designs and just because you're distilling metal is no reason to disregard that.
I did that but with sodium chloride and once it took it exploded. The sulfur does reduce the activation energy a bit. Another thing that might be better is using a flux of sorts to bring the melt point down, preferably something that doesn't change the overall reaction and something that will scavenge the aluminum oxide. Although a more typical thermite mixed with the carbonate thermite might actually be closer to ideal if it doesn't alloy well with the alkali.
if you store KOH in the open it converts into potassium carbonate by itself. Drying it in the closed oven was not a good idea, because it had no access to the CO2 in the air to convert the residual KOH. Air actually has lots of CO2 in it already, if you can wait a few days.
Might be a stupid suggestion, but to speed the reaction, you could use a solvent and do the work in solution. My first thought was Borax (anhydrous, baked first) which would melt at a low temp but you'd reduce out elemental boron before the Sodium, and metallic aluminum wouldnt dissolve in it anyhow. Another simpler Sodium salt would be great but one problem with aluminum is you're trapped by anion choices: Halogens will create scary AlX3 vapours, Nitrates will create NOx gas and aluminum oxide which will plug your reaction up, and anything hydroxy or oxy will give the same problem minus the NOx. I feel like the best solvent would be an aluminum salt but they're all either refractory or volatile as hell.
Alternatively, (possibly) better idea would be to have an excess of aluminum which can allow the reaction to occur at the molten surface where the sodium salt sits on top - but AlO3 will build up and form a refractory layer that will stop the reaction and maybe go pop.
I'm just rambling at this point, this clearly worked albiet in a slightly terrifying manner, Cool as shit, thanks for the content.
Please wear gloves
These are some interesting thoughts!
Amazing to watch the lunch bad video and realize you've been telling us "I've never done this before" for over 10 years.
Maybe try adding an inert salt to lower the temperature of the melt. The eutectic point can be a few hundred degrees lower than the pure salt. If good melting facilitates the reaction and temperature drives the reaction, maybe having it melt at a lower temperature will slow down the reaction. I imagine the added dilution might also give some thermal mass to yeet the massive spike in exothermic heat
Looked at a random post from 2017, what you might have there is pure sodium. Apparently the other products are aluminum oxide, and aluminum carbide. So, that fire when cleaning your station with water might be sodium making hydrogen, or aluminum carbide making methane gas, or likely both. But, apparently the carbide would be a solid during the reaction, and the oxide would be a liquid, meaning the only gas would just be pure sodium.
This double mobile in one case is such a weird flex xD
If you have a sodastream you can just feed it into potassium hydroxide water. I've done it before and it works better than youd think!
Instead of doing that, you could use a process outlined by nurdrage where he catalized the reaction of sodium hydroxide and magnesium with menthol to mass produce pretty clean sodium.
where is the taste test
i already love this channel omg
Oh shit! It actually works in a janked up setup.
You could use a very long steel pipe as a condensation chamber
That is coola new method of making Sodium metal.
Potassium carbonate is making by burning wood or charcoal and mixing ash with water. Potassium carbonate is soluble in water and you can filter out this solution. That is what too many potassium compounds is made with potassium carbonate
12:21 got me acting up
I think you should make science "slop" for this channel. It could help greatly with the funding while keeping viewers engaded.
Under slop I mean creating a vid where you talk about recent news and advancements in chemistry or in science general, reacting to TikTok hacks or just talk about the overall scene of science or about related UA-cam content you like.
Science slop occurs when the mixture fails and turns into thick brown stuff
This is actually amazing.
this is more of a main channel video but with less editing XD
7:56 ohh nah, now where have I seen that before👀
PPE good 😂😮😊 great video.
You could carefully try using finer aluminium powder, this could lower the activation temperature to below sodiums boiling point, though equally it could just make the reaction way too violent, but seeing as sodium carbonate is so unreactive that might be unlikely
Yeah I thought about this, but the fact it doesn't even react when everything is molten tells me that a powder won't help it
nice! good job mrgreenguytoo!
The sodium situation is crazy
Interesting.I wonder if the same reagent substitutions work with the Nurdrage process.
if this channel does not blow up im prob going to be the only one constantly watching your second channel videos
let him cook youtube
5:54 I'm sure you def know this but please do not stare at burning magnesium as it literally can tear holes in your cornea which isn't ideal if you want to maintain a perfect vision lol
Yeah it's a common concern. Not usually anywhere near as bad as people make it sound though. I've stared at a lot of burning magnesium over the years. Magnesium powder fireballs used to be used for flash photography and the main danger was burning your hand rather than burning your eyes. But yeah it is very very bright and gives off some UV
Careful, sir. Dangerous stuff.
This feels appropriate for the first video I see here... Considering how salty the review team is on your main channel. :)
It would be cool if you hearted this comment. Great video
I wonder if you could use a HFVTTC for the ignition of sodium carbonate and aluminum. It would be cool to make a low pressure container filled with argon and the stuff for sodium production, and then blast it with extremely high temperature plasma.
I mean you could do the reaction under pressure. It would theoretically increase sodiums boiling point above 1000C. Unsure the pressure needed and youd want it to be argon
As someone smart once approximately said, I think Einstein, "The only difference between dicking around and science is writing it down."
Adam Savage.🤣
perhaps your reaction was to vigorous because of aluminium powder? I would try with aluminium foil or eaven thicker pieces of aluminium. this would probably slow down the reaction and it wouldn all just burst out of the aparatus
This video not getting enough views tells me a lot about the UA-cam algorithm
17:54, could you use a catalyst to lower the activation energy?
You should not have needed to upload to a second channel, but here we are, thanks youtube!
I came over from your rant video. You made 10 hours ago. I’ll check out what this is but then I’m gonna go watch the finals. See how it’s doing.
What if you bought some dry ice. Then evaporated it in a container connected into a balloon to extract the CO2.
couldve just bought pressurised co2
@@HerzaPop Hey.. exhaling into a tube was on the table. He's not made of money. See
@_-noxxon-_ comment.
😂😂😂
@HerzaPop Hey.. breathing through a tube was on the table. He's not made of money. See @_-noxxon-_ comment about that.
double the fun!
Channel 2 let's go!
hey would you mind sharing the link to the aluminium powder?
It frustrates me that UA-cam's been stupid towards a Quality Science channel! They cannot change how important this kind of informative content is *UA-cam would be stupid if they didn't support creators of this quality. The way UA-cam handles their community guidelines is mind numbingly absurd. Yet stuff like "G-string camping videos" get fully supported *don't get me wrong, I fully support G-string camping videos. Why do those videos get supported but someone can make a well edited informative video that covers a difficult topic.. and yet that's not supported? Quality true crime content struggles to get any support & that's just one example. UA-cam overly abuses their control over what videos get monetized or whats gets flagged or copyrighted, even when the creator did everything correctly to be fully covered under "fair use" rights. Yet UA-cam still makes these people go thru a bunch of nonsense, trying to communicate with UA-cams joke of an official review process. Some of these creators put in so much effort into their videos & they follow all of youtubes rules as much as possible followed, yet UA-cam still throws them thru the ringer. People should be allowed to cover these topics but they don't care. They hit them with limited adds, etc. It just really frustrates me that UA-cam is making it really hard for these creators. Even tho they bring so much value to their company. I don't think UA-cam realizes that a huge percentage of their viewers are adults.. Not everything has to be made for kids... Idk i hope UA-cam improves because they really are a great platform but they got to get their shit together and support these creators who bring so much to their platform.
Justice for spoon. They sell them at supermarkets.
Make fentanyl next!
This totally should have been a main channel video. I understand why you wouldn't want to upload after your last video though. Eventually UA-cam will come around.
I supporting you
How can I find the coat you're wearing?
Strange to hear an Australian switching between non-rhotic and rhotic English frequently
spoon and torch chemistry
Why didn't you use dry ice for the co2?
well, does this mean we'll get a new sodium ducky
Hmmm possibly some day
8:55 The internet demands that I say 'nice'.
@8:30 i wonder if the propane torch is stealing all the oxygen away from the magnesium so it cant burn as hot
He only owns 1 spoon, and he chose to be a chemist...
ChatGPT can't do math.
Why not use NaCl?
Aluminium chloride reacts with water, producing aluminium hydroxide (hard to react with) and hydrochloric acid (volatile, dangerous). Because it's a byproduct that is annoying to handle, maybe that's one possible answer for that.
Sodium chloride is even less reactive than sodium carbonate. I think it would be nearly impossible to get them to react at all
@@mrgreenguytoo Ah, I am stupid. So you basically first reduced carbon, then sodium... Still few g of NaCl could form eutectic to lower melting point, but I have no idea really.