Science Skool........Wow i am impressed. Not only is it a GREAT video but you actually replied and answered all the post below the video. That is very rare for chemistry videos. I got a question.......ULTRA ULTRA PURE anhydrous AlCl3 is white. But it is well know that MOST samples of anhydrous AlCl3 are somewhat yellow/brown due to FeCl3 impurities. I noticed inside, up on top of your apparatus, there is definitely a lot of white powder. But there is also some yellow tinted powder. The same goes for the AlCl3 you are collecting in the test tube. Although some times the camera does not show color the way it is in real life. So maybe it was all white with no yellow tint. If there was some yellow tint then where do you think the iron impurity came from? If that's what it is. I mean you got chlorine gas and aluminum foil. There was no SOLID iron metal in a GAS of chlorine. SO MY QUESTION IS THIS >>>>>>>>>> Do you think aluminum foil has trace amounts of iron in it???????????????????????????????? I mean if you are going to use the AlCl3 as a catalyst in like a freidel crafts reaction it wont matter if you got a little FeCl3 impurity in there. Both AlCl3 and FeCl3 can be used for the lewis acid catalyst but i am just curious.
I have looked at EVERY VIDEO on youtube where someone is reacting a halogen with a metal and this is the ONLY VIDEO with VALUBLE INFORMATION. I should be trying this experiment before the week is over. Hope it goes well. Although i am making AlBr3. I just need a pinch the first time i make it for a F.C. alkylation so that should be easy. But then i need a stoichiometric amount for the next F.C. reaction cause it is an acylation and that is a lot of AlBr3 needed for that.
@@michaelsambor5286 .............Well not good. I tried the same experiment in the video above only i used Br2 vapor instead of chlorine. It did not work. I think you need MORE HEAT when using bromine instead of chlorine. I finally had to heat the aluminum and shove it in a round bottom flask that had some bromine vapor in it to make some AlBr3. Then i was going to heat up the flask to get the excess bromine out of the flask. And then just use that flask for a friedel crafts reaction. I also alpha brominated some acetone. Unfortunately soon after that my son died and i got to depressed to do much more in the lab last winter. I did get out of bed to do 2 more experiments to try to get out of my funk. I used hypochlorous acid (bleach/AcOH) to oxidize isopropanol to acetone. And I dehydrogenated ethanol to make acetaldehyde. Next winter i will try to make AlCl3 using chlorine. I am going to finally buy a gas mask i think. Last winter i did not do much in the way of chemistry
@@waltersobchak7275 ...........I tried this experiment with aluminum and bromine vapor but i could not get it to work. I actually had to burn the aluminum in the bromine vapors. Just an FYI..................................Yeah i made some mercuric chloride last month. I want to take my methylamine and make a video on reductive amination with the carbonyl being acetone. To make N_methyl isopropylamine. OH MY GOD!!!!!!!!!!!!!!!!!! I got methylamine crystals. Looks like a lot but you know how that is. Looks like an ounce but ends up being 10 grams. I am shooting for 34 grams. So anything below 20 is going to make me unhappy. But still happy it worked at all. First attempt is always the worst.........lol.
Use Cl2 first then switch to Br2. Also Br2 needs to be in excess for it to work well. AlBr3 also won't sublime as easily, so it will form a glob instead. Try using flitter flake pyrotechnics aluminum. It is fine flakes of aluminum that ar very shiny and look like fish scales under a microscope.
Thank You very good! So....this is what happens inside hot water heaters with Aluminum Anode Rods? All the Aluminum dissolves into the water we drink, cook and shower with?.....How nice is that?
How to make Alcl3 for chemisty reactions. My version uses an actual steel pipe to roast it in and an ice cooled trap to collect it in. Uses course pyro flake aluminum and a chlorine generator fueled with HCl and TCCA or pool shock. This chemical is very moisture sensitive so great care must be taken to keep it dry.
Gas drying bottle filled with glass wool and CaCl2 pellets, a pyrolyis tube, a cold trap to crystallize the vapor, and a getter bottle to grab left over chlorine. It can easily be improvised without needing much actual glassware. However the reaction tube and plumbing to the trap need to be heat resistant. A steel pipe is ok for the reaction tube, just slowly heat it to allow the inner surface to passivate with FeCl3. ❤
I added a mixture of graphite powder and toothpaste with chloride as a temporary thermal paste to my led headlight which get insanely hot when turned on. No i regret it after watching this video. Ill check it again later and if got time ill upload a video of that
@@boozinga Though I am not an expert in thermal paste, toothpaste usually contains fluoride ions not chloride ions (though they're probably in there as well. However please don't confuse chloride ions with chlorine atoms, they are very different. I am not sure how effective it is as a thermal paste, but I am quite confident it won't react like the video :)
HOLLY CRAP I just looked it up and aluminum foil ...depending on what it is used for... is an alloy with only like 92 to 98 % aluminum. These impurities are mainly chromium, copper, iron, magnesium, manganese, silicon, titanium and zinc. MSDS for reynolds wrap is 96.9 % Aluminum / IRON 1% / silicon 1.1 %. I never would have guessed that. I thought ALL aluminum foil was like 99% aluminum with trace metal impurities.
Hi John Black Super Chemist - This is a really good question. I believe the colour you are seeing in the product is from the chlorine. At this point, the AlCl3 hadn't been isolated. The product was quite wet as well, so chlorinate water would often give a pale yellow/green colour, possibly even chlorine and water ligands. As this was high-grade pure aluminium it would have a negligible amount of iron and shouldn't give it the yellow colour you are referring to. However to prove this I would have had to attempt to purify it. Great question though, Alex.
@@scienceskool4734 ........Well you blew my THEORY out of the water....lmao. I JUST FOUND OUT YESTERDAY that HOUSEHOLD aluminum foil is not 99% aluminum in most cases. You OBVIOUSLY already knew and got good aluminum. I also did not realize the AlCl3 salt you made needed purified more. Although i was thinking the impurity was FeCl3 which is no big deal if you are just going to use the AlCl3 as a lewis acid catalyst in halogenation/friedel crafts reactions. AND Yeah your explanation is the only thing left that makes SENCE.. My NEXT GUESS was going to be that just like in an electrophilic aromatic substitution (halogenation of benzene say) the chlorine gas would react with the AlCl3 to make tetrachloroaluminate anion (AlCl4). But that would be a chloro LIGAND and your BIG BRAIN already mentioned that in your post that it MIGHT be ligands. I do NOT know but I am GUESSING that would be white in color and not yellow or green. And again i am TOTALLY GUESSING but i would think water ligands would not change its color to yellow/green. Don't get me wrong if a little water condensed out of the air and into the test tube some chloro and water ligands were exchanged but i just do not think it made the yellowish color. Although i have NEVER taken ligand theory (crystal field theory) so what do i know...lol. I REALLY LIKE your answer about the chlorine and water from the air. Even though NOW IN HINDSIGHT I can see YOUR answer is somewhat obvious, but without you bringing it up, i NEVER would have thought of it. I had tunnel vision thinking it was iron impurities. And i was obsess ed to prove it....lol. I am going to make an ANHYDROUS MX3 salt soon. Maybe i will pull a vacuum on the system before i let the halogen into where the metal is. Try to get the water out of the apparatus first and completely. Maybe even dry my glass in the oven first. . And keep the system closed (except for a drying tube). And use a RBF instead of a test tube so i can keep the collecting/distilled salt closed off to the outside atmosphere and the water contained in the atmosphere. . To tell you the truth i NEVER even thought of purifying the MX3 salt i will make until you just mentioned it in your post today.. I guess since AlCl3 and AlBr3 both sublime i GUESS I could just distill the salt after i make it using a short path distillation set up. ANYWAYS thanks for all the tips and help. I really learned a lot from your video and reply. AGAIN GREAT VIDEO!!!!!!!!! You know there are like only 5 videos on youtube about making ANHYDROUS MX3 salt but comparing those videos to yours like like comparing a lit match to the sun. . And THANK YOU VERY MUCH for answering my question. Not many channels do that. Thanks to you i am back on the RIGHT path again. HAVE A GREAT DAY BUDDY!!!!!!!!!!!
Hi John, I love your enthusiasm. Just clarifying one point, any complex of aluminium would give a white precipitate (offwhite occasionally) or colourless solution as aluminium is not a transition metal so there is no d orbital splitting and hence no colour. Keep enjoying your science. Alex.
@@scienceskool4734 ...........Thanks buddy. I wasn't sure. I mean i know in GENERAL CHEMISTRY i always read what you just said. But they never really mention ligands in general chemistry. I mean they do mention them but they usually only give the very basics in general chemistry 2. And maybe 2 sentences in text books in organic chemistry. And then 4 or 5 years ago i heard that some colleges put there classes on youtube. LIKE THE WHOLE SEMESTER OF CLASSES. So i took every class for organic chemistry 1 and 2 and biochemistry then i could not find any more HIGHER classes on youtube. And the only time ligands where mentioned was when he talked about grignards and how THF. or ether would form ligands with ether to help the reaction. Maybe he said 5 sentences. THAT IS THE SAME FOR THE D BLOCK METALS. It is like they just give you the bare minimum of information. I just say screw it I mean i am to old to learn everything about chemistry before i die. It is not like i am running out of stuff to learn I think i know as much about chemistry as someone who went to college for 3 years for chemistry. But i also think that is only like 20% of what there really is to learn. ANYWAYS I AM BABBING HERE..........So let me just say thanks cause i did wander the last 3 years if a dative bond in a molecule/ion could effect it's color. And you are saying it is still the metal that determines the color. And also the reason i am kind of enthusiastic is cause the last 4 years i had a channel and i recently quit that. IT WAS SO TIME CONSUMING. And any more it was more like having an unpaid job than being a fun hobby. I mean the last 4 years i have not really learned that much that was NEW cause i was always making videos or editing or posting or writing on my white board showing stuff for the videos. I mean don't get me wrong. i learned some new stuff but mostly in the last 4 years MOSTLY I just reviewed what i already new. But now i got time to learn some NEW stuff. I want to study some chemistry i never seen before. That is why i LOVE videos like the one YOU made here. It makes me go out and research and learn NEW stuff just so i can understand everything you are doing and saying. It is a shame the colleges do not put ALL there classes on line. Even if you can not ask questions it is SO MUCH EASIER TO LEARN WHEN A PERSON IS EXPLAINING IT. Well i am starting to babble again so i will stop here. Thanks again for the videos and all the info. I may know up to 3 years of college when it comes to books but I am DEFINITELY not that far in the lab So videos on people actually doing the experiment is so helpful and educational.
Hi C16H36BF4N - you would absolutely get FeCl3 anhydrous. I would make the chlorine in-situ by adding bleach and sulphuric acid and then add heated iron wool suspended in the chlorine gas.
Hi Paul Halloween - It should be possible to "melt" aluminium with a Bunsen flame as its melting point is around 660oC where as a Bunsen flame could be up to 1200-1400oC. As for burning, do you mean combustion? In which case, yes you could create aluminium oxide by reacting it with oxygen in a Bunsen flame.
Paul Frankenstein...........THIS IS A GREAT VIDEO. Are you the one i just sent a post to telling you about this video??????????? If so i see you already knew about it. You can burn any metal if it is thin enough and hot enough AND YOU HAVE AN OXIDIZER. So aluminum foil is definitely thin enough. And even methane/air(natural gas) burns 6 times as hot as the ignition temp of aluminum foil AND propane in air burns even hotter than that. So you definitely got enough heat with a bunsen burner. All you need last is an oxidizer like oxygen (from the air) or a halogen or etc. So if oxygen is the oxidizer you will PROBABLY make some kind of aluminum oxide. If chlorine is the oxidizer you will make anhydrous AlCl3. If bromine is the oxidizer you will make AlBr3. Combustion ALWAYS consist of 3 things. (1) Source material that burns like aluminum. (2) heat (3) oxidizer. You know Dr. Frankenstein's monster was named Adam Frankenstein. Are you any relation to either of them? LOL
Hi Drobin Huang. This would be an example of a redox reaction. The aluminium has been oxidised (Al --> Al3+ + 3e-) and the chlorine has been reduced (Cl2 + 2e- --> 2Cl-). I hope that helps
@@scienceskool4734 yeah but its a gas at that temperature right? also, are you aware of any temperature that cause aluminum chloride molecules to decompose?
Science Skool........Wow i am impressed. Not only is it a GREAT video but you actually replied and answered all the post below the video. That is very rare for chemistry videos. I got a question.......ULTRA ULTRA PURE anhydrous AlCl3 is white. But it is well know that MOST samples of anhydrous AlCl3 are somewhat yellow/brown due to FeCl3 impurities. I noticed inside, up on top of your apparatus, there is definitely a lot of white powder. But there is also some yellow tinted powder. The same goes for the AlCl3 you are collecting in the test tube. Although some times the camera does not show color the way it is in real life. So maybe it was all white with no yellow tint. If there was some yellow tint then where do you think the iron impurity came from? If that's what it is. I mean you got chlorine gas and aluminum foil. There was no SOLID iron metal in a GAS of chlorine. SO MY QUESTION IS THIS >>>>>>>>>> Do you think aluminum foil has trace amounts of iron in it???????????????????????????????? I mean if you are going to use the AlCl3 as a catalyst in like a freidel crafts reaction it wont matter if you got a little FeCl3 impurity in there. Both AlCl3 and FeCl3 can be used for the lewis acid catalyst but i am just curious.
I have looked at EVERY VIDEO on youtube where someone is reacting a halogen with a metal and this is the ONLY VIDEO with VALUBLE INFORMATION. I should be trying this experiment before the week is over. Hope it goes well. Although i am making AlBr3. I just need a pinch the first time i make it for a F.C. alkylation so that should be easy. But then i need a stoichiometric amount for the next F.C. reaction cause it is an acylation and that is a lot of AlBr3 needed for that.
hello how did it go?
@@michaelsambor5286 .............Well not good. I tried the same experiment in the video above only i used Br2 vapor instead of chlorine. It did not work. I think you need MORE HEAT when using bromine instead of chlorine. I finally had to heat the aluminum and shove it in a round bottom flask that had some bromine vapor in it to make some AlBr3. Then i was going to heat up the flask to get the excess bromine out of the flask. And then just use that flask for a friedel crafts reaction. I also alpha brominated some acetone. Unfortunately soon after that my son died and i got to depressed to do much more in the lab last winter. I did get out of bed to do 2 more experiments to try to get out of my funk. I used hypochlorous acid (bleach/AcOH) to oxidize isopropanol to acetone. And I dehydrogenated ethanol to make acetaldehyde. Next winter i will try to make AlCl3 using chlorine. I am going to finally buy a gas mask i think. Last winter i did not do much in the way of chemistry
@@johnblacksuperchemist2556 I’m following a link sir. I Got a bunch of Hg Cl2 maybe make some amalgam
@@waltersobchak7275 ...........I tried this experiment with aluminum and bromine vapor but i could not get it to work. I actually had to burn the aluminum in the bromine vapors. Just an FYI..................................Yeah i made some mercuric chloride last month. I want to take my methylamine and make a video on reductive amination with the carbonyl being acetone. To make N_methyl isopropylamine. OH MY GOD!!!!!!!!!!!!!!!!!! I got methylamine crystals. Looks like a lot but you know how that is. Looks like an ounce but ends up being 10 grams. I am shooting for 34 grams. So anything below 20 is going to make me unhappy. But still happy it worked at all. First attempt is always the worst.........lol.
Use Cl2 first then switch to Br2. Also Br2 needs to be in excess for it to work well. AlBr3 also won't sublime as easily, so it will form a glob instead. Try using flitter flake pyrotechnics aluminum. It is fine flakes of aluminum that ar very shiny and look like fish scales under a microscope.
Thank You very good! So....this is what happens inside hot water heaters with Aluminum Anode Rods? All the Aluminum dissolves into the water we drink, cook and shower with?.....How nice is that?
How to make Alcl3 for chemisty reactions. My version uses an actual steel pipe to roast it in and an ice cooled trap to collect it in. Uses course pyro flake aluminum and a chlorine generator fueled with HCl and TCCA or pool shock. This chemical is very moisture sensitive so great care must be taken to keep it dry.
AWESOME DIMOSTRATION!!! But, what is the names of apparatus (or eventually the parts of the apparatus)?
Gas drying bottle filled with glass wool and CaCl2 pellets, a pyrolyis tube, a cold trap to crystallize the vapor, and a getter bottle to grab left over chlorine. It can easily be improvised without needing much actual glassware. However the reaction tube and plumbing to the trap need to be heat resistant. A steel pipe is ok for the reaction tube, just slowly heat it to allow the inner surface to passivate with FeCl3. ❤
Hi! One question. Will the reaction be fast if say for example. The aluminum is buried in a bucket of chlorine instead of heating it in a tube.
Perfect Video on the best Channel
I added a mixture of graphite powder and toothpaste with chloride as a temporary thermal paste to my led headlight which get insanely hot when turned on. No i regret it after watching this video. Ill check it again later and if got time ill upload a video of that
LED heat sink structure is Aluminum.
@@boozinga Though I am not an expert in thermal paste, toothpaste usually contains fluoride ions not chloride ions (though they're probably in there as well. However please don't confuse chloride ions with chlorine atoms, they are very different. I am not sure how effective it is as a thermal paste, but I am quite confident it won't react like the video :)
no one:
no one:
captions:"can be sublimed by eating"
Super! Thank you very much!
Is the resulting substance anhydrous aluminum chloride?
Is chlorine corrosion on aluminum the worst of all metals?
New to chemistry and this got into my recommendations. What’s this kind of apparatus called?
HOLLY CRAP I just looked it up and aluminum foil ...depending on what it is used for... is an alloy with only like 92 to 98 % aluminum. These impurities are mainly chromium, copper, iron, magnesium, manganese, silicon, titanium and zinc. MSDS for reynolds wrap is 96.9 % Aluminum / IRON 1% / silicon 1.1 %. I never would have guessed that. I thought ALL aluminum foil was like 99% aluminum with trace metal impurities.
Hi John Black Super Chemist - This is a really good question. I believe the colour you are seeing in the product is from the chlorine. At this point, the AlCl3 hadn't been isolated. The product was quite wet as well, so chlorinate water would often give a pale yellow/green colour, possibly even chlorine and water ligands. As this was high-grade pure aluminium it would have a negligible amount of iron and shouldn't give it the yellow colour you are referring to. However to prove this I would have had to attempt to purify it. Great question though, Alex.
@@scienceskool4734 ........Well you blew my THEORY out of the water....lmao. I JUST FOUND OUT YESTERDAY that HOUSEHOLD aluminum foil is not 99% aluminum in most cases. You OBVIOUSLY already knew and got good aluminum. I also did not realize the AlCl3 salt you made needed purified more. Although i was thinking the impurity was FeCl3 which is no big deal if you are just going to use the AlCl3 as a lewis acid catalyst in halogenation/friedel crafts reactions. AND Yeah your explanation is the only thing left that makes SENCE.. My NEXT GUESS was going to be that just like in an electrophilic aromatic substitution (halogenation of benzene say) the chlorine gas would react with the AlCl3 to make tetrachloroaluminate anion (AlCl4). But that would be a chloro LIGAND and your BIG BRAIN already mentioned that in your post that it MIGHT be ligands. I do NOT know but I am GUESSING that would be white in color and not yellow or green. And again i am TOTALLY GUESSING but i would think water ligands would not change its color to yellow/green. Don't get me wrong if a little water condensed out of the air and into the test tube some chloro and water ligands were exchanged but i just do not think it made the yellowish color. Although i have NEVER taken ligand theory (crystal field theory) so what do i know...lol. I REALLY LIKE your answer about the chlorine and water from the air. Even though NOW IN HINDSIGHT I can see YOUR answer is somewhat obvious, but without you bringing it up, i NEVER would have thought of it. I had tunnel vision thinking it was iron impurities. And i was obsess
ed to prove it....lol. I am going to make an ANHYDROUS MX3 salt soon. Maybe i will pull a vacuum on the system before i let the halogen into where the metal is. Try to get the water out of the apparatus first and completely. Maybe even dry my glass in the oven first. . And keep the system closed (except for a drying tube). And use a RBF instead of a test tube so i can keep the collecting/distilled salt closed off to the outside atmosphere and the water contained in the atmosphere. . To tell you the truth i NEVER even thought of purifying the MX3 salt i will make until you just mentioned it in your post today.. I guess since AlCl3 and AlBr3 both sublime i GUESS I could just distill the salt after i make it using a short path distillation set up. ANYWAYS thanks for all the tips and help. I really learned a lot from your video and reply. AGAIN GREAT VIDEO!!!!!!!!! You know there are like only 5 videos on youtube about making ANHYDROUS MX3 salt but comparing those videos to yours like like comparing a lit match to the sun. . And THANK YOU VERY MUCH for answering my question. Not many channels do that. Thanks to you i am back on the RIGHT path again. HAVE A GREAT DAY BUDDY!!!!!!!!!!!
Hi John, I love your enthusiasm. Just clarifying one point, any complex of aluminium would give a white precipitate (offwhite occasionally) or colourless solution as aluminium is not a transition metal so there is no d orbital splitting and hence no colour. Keep enjoying your science. Alex.
@@scienceskool4734 ...........Thanks buddy. I wasn't sure. I mean i know in GENERAL CHEMISTRY i always read what you just said. But they never really mention ligands in general chemistry. I mean they do mention them but they usually only give the very basics in general chemistry 2. And maybe 2 sentences in text books in organic chemistry. And then 4 or 5 years ago i heard that some colleges put there classes on youtube. LIKE THE WHOLE SEMESTER OF CLASSES. So i took every class for organic chemistry 1 and 2 and biochemistry then i could not find any more HIGHER classes on youtube. And the only time ligands where mentioned was when he talked about grignards and how THF. or ether would form ligands with ether to help the reaction. Maybe he said 5 sentences. THAT IS THE SAME FOR THE D BLOCK METALS. It is like they just give you the bare minimum of information. I just say screw it I mean i am to old to learn everything about chemistry before i die. It is not like i am running out of stuff to learn I think i know as much about chemistry as someone who went to college for 3 years for chemistry. But i also think that is only like 20% of what there really is to learn. ANYWAYS I AM BABBING HERE..........So let me just say thanks cause i did wander the last 3 years if a dative bond in a molecule/ion could effect it's color. And you are saying it is still the metal that determines the color. And also the reason i am kind of enthusiastic is cause the last 4 years i had a channel and i recently quit that. IT WAS SO TIME CONSUMING. And any more it was more like having an unpaid job than being a fun hobby. I mean the last 4 years i have not really learned that much that was NEW cause i was always making videos or editing or posting or writing on my white board showing stuff for the videos. I mean don't get me wrong. i learned some new stuff but mostly in the last 4 years MOSTLY I just reviewed what i already new. But now i got time to learn some NEW stuff. I want to study some chemistry i never seen before. That is why i LOVE videos like the one YOU made here. It makes me go out and research and learn NEW stuff just so i can understand everything you are doing and saying. It is a shame the colleges do not put ALL there classes on line. Even if you can not ask questions it is SO MUCH EASIER TO LEARN WHEN A PERSON IS EXPLAINING IT. Well i am starting to babble again so i will stop here. Thanks again for the videos and all the info. I may know up to 3 years of college when it comes to books but I am DEFINITELY not that far in the lab So videos on people actually doing the experiment is so helpful and educational.
Does is produce more heat?
Can the aluminum chloride prepared in this way be used in friedel craft reactions, does it need to be very pure for friedel craft?
What do you want to synthetize?
So amazing
if i place iron wool do i get fecl3 anhydrous ? nice work ty
Hi C16H36BF4N - you would absolutely get FeCl3 anhydrous. I would make the chlorine in-situ by adding bleach and sulphuric acid and then add heated iron wool suspended in the chlorine gas.
Nice video. Is it possible to burn the aluminium foil with a Bunsen burner?
Hi Paul Halloween - It should be possible to "melt" aluminium with a Bunsen flame as its melting point is around 660oC where as a Bunsen flame could be up to 1200-1400oC. As for burning, do you mean combustion? In which case, yes you could create aluminium oxide by reacting it with oxygen in a Bunsen flame.
Paul Frankenstein...........THIS IS A GREAT VIDEO. Are you the one i just sent a post to telling you about this video??????????? If so i see you already knew about it. You can burn any metal if it is thin enough and hot enough AND YOU HAVE AN OXIDIZER. So aluminum foil is definitely thin enough. And even methane/air(natural gas) burns 6 times as hot as the ignition temp of aluminum foil AND propane in air burns even hotter than that. So you definitely got enough heat with a bunsen burner. All you need last is an oxidizer like oxygen (from the air) or a halogen or etc. So if oxygen is the oxidizer you will PROBABLY make some kind of aluminum oxide. If chlorine is the oxidizer you will make anhydrous AlCl3. If bromine is the oxidizer you will make AlBr3. Combustion ALWAYS consist of 3 things. (1) Source material that burns like aluminum. (2) heat (3) oxidizer. You know Dr. Frankenstein's monster was named Adam Frankenstein. Are you any relation to either of them? LOL
Hi, is there any name for this reaction??
Hi Drobin Huang. This would be an example of a redox reaction. The aluminium has been oxidised (Al --> Al3+ + 3e-) and the chlorine has been reduced (Cl2 + 2e- --> 2Cl-). I hope that helps
@@scienceskool4734 thx a lot
Which gas will liberate
There will be no gas liberated, only AlCl3 is produced.
@@scienceskool4734 yeah but its a gas at that temperature right? also, are you aware of any temperature that cause aluminum chloride molecules to decompose?
Tq