I want to address a concern that people are mentioning about vapor pressure. When you put a liquid in a container that is bigger than the volume of the liquid, some of the liquid will form a vapor until the container reaches the vapor pressure of that liquid at that temperature. If it is a pure liquid (no air in the container) and all of the liquid doesn't evaporate, then the total pressure will be somewhere along the liquid/vapor line on the phase diagram. But, if there is air in the container, then the liquid will form a vapor and increase the pressure until the partial pressure of the vapor reaches the the point on the liquid/vapor line in the phase diagram. The point is that if you have a *pure* substance and you tell me the temperature and pressure of the container it is in, then I can tell you if it is a liquid, solid, vapor or gas. (Also note that if the temperature and pressure are on the solid/liquid/gas equilibrium lines on the phase diagram, then I can't tell you how much solid/liquid/gas you have unless you tell me how much energy you have input into the system and how much liquid you started with etc.)
> But, if there is air in the container, then the liquid will form a vapor and increase the pressure until the partial pressure of the vapor reaches the the point on the liquid/solid line in the phase diagram. I think you mean the liquid/gas line. On the solid/liquid line you can't be in equilibrium with a gaseous phase (unless you're exactly at the triple point).
Only critique here is the emphasis on a pure substance, you can do the same thing for binary mixtures very easily, only need 1 more piece of information which is the molar fraction and then I can tell you the amount that is in the liquid phase, the vapor phase, and the contributing partial pressures of each species. Vapor-liquid equilibrium diagrams aren't too difficult to read without a background in chemical engineering.
@@fat_pigeon Sublimation, transition from solid to gas. You can easily be on that equilibrium line without a triple point, easiest example is dry ice, frozen CO2.
The supercritical transition is still one of the coolest (heh) things I've ever seen. I've watched a lot of people using supercritical CO2 to make aerogel, and watching the meniscus just gradually disappear still blows my mind.
Watching those got me to build my own chamber just to see it myself. Really cool to start with solid CO2, watch it go to solid+liquid+gas, then liquid+gas, then supercritical fluid. Put some stuff in the chamber and shake it around and you can tell there's a fluid in there that's slowing down movement more than a gas but less than a liquid. The cloudiness that forms when it goes back to liquid+gas is also fun to watch, you can see it in this video but it doesn't last as long as it does with CO2.
This is so cool, as a refrigeration tech I too have been curious of the phase change of supercritical fluids. Our entire industry is largely based supercritical and subcooled fluids to transfer heat and rely on pressure changes to affect said state.
@@JustABeeInFPV absolutely my friend, a bit of chemistry, a bit of physics, a bunch of mechanics, electrical and plumbing. Get your gas ticket, you can install. Wire and supply gas to the furnace all eith 1 ticket. A buddy needs some electrical done, take out a permit and run the wire. Sister needs a new bathroom in the basement your ready to go. We can work on up to 600VAC with the ticket and like I said get you gas ticket which we can as Fridge Techs and you can do gas fitting.
@Praise Jesus, Repent or Likewise Perish its funny how there are different versions of your new testament. Doesn't that say something? Each version is different.
I mean it when I say your videos are very hard to pass on. Every one I see available hooks me and reels me in like a fish lol. Arguably some of the most enlightening and entertaining content on TH-cam or anywhere else for that matter. You're a gifted teacher and I've learned a lot without having to try!
Fun fact: Xenon gas is used in headlight bulbs called "High intensity discharge bulbs" or HID. Electricity is used to ignite the gas and keep it at a stable temperature. The temperature of the gas once ignited determines the color of the light being projected. You can have anything from amber (lower temps), to bright white (slightly higher), to blue (slightly higher), and more.
@@mikedejesus7064 Honestly, i don't know how it correlates with temperature, but the key point is that the light emitted in discharge lamps is due to ionization of the gas and not its temperature. Thats why its emissions spectrum is limited to a few frequencies unlike a black body radiation.
This clarifies so much physics, I had no idea. Your videos always bring something new! I’m 29, and really interested in science, and yet, you never fail to drop new knowledge with every video!
@@andybaldman I think it’s a mix of both… of course this channel is mostly concentrated in entertainment via science. But I’m sure there are channels within YT dedicated to more in depth explanation. School I think is good later on for finding better jobs but I never think it’s necessary to learn…
dude, your channel rocks. I;ve been repeatedly impressed with how you can tackle a highly complex topic with seemingly simple demonstrations. I've forwarded many videos to friends with "see, this is why this happens or works this way, etc"!
The cool thing is that as the supercritical fluid forms, the gas above and liquid below approach having the exact same refractive index, which is why the division between then becomes more and more difficult to discern.
The refractive index is merely a consequence or side effect of the density (for transparent homogeneous phases). We can no longer see the difference between the two phases because...there is no difference, they're absolutely identical :D Yeah I know it's a detail and in practice we can only compare the refractive index by looking at a sealed ampule, but I think it's even more mind blowing to realise the two phases *are* identical, than to only assume their refractive indexes (one of many properties) being equal
@@YounesLayachi Yes, that's exactly right. This is why I didn't concentrate on the state of them being the same because that's pointless. I focused on the two approaching having the same refractive index, and that's why they become more and more difficult to distinguish. Now this is, of course, due to their density (and other properties) approaching homogeneity, but it's still true that the refractive indices approaching equality makes them more difficult to distinguish. The smaller the difference in refractive index, the less light reflects on the boundary of the liquid and gas.
I believe what you said at 4:05 is not right...you should always talk about partial pressures - there is always some partial pressure of gaseous phase over liquid - the bold line in phase diagram just marks the point, when partial pressure of gas equal the surrounding pressure (in everyday life it is atmosferic pressure)
As a chemist, I have to agree with you. The property is called vapor pressure. For water at 25 °C, it's 3170 Pa. For ethanol, it's much higher -- 5950 Pa at 20 °C. Therefore, a vessel containing only ethanol (no air) would be under pressure of 6 kPa at 20 °C only from ethanol vapor. At boiling point, vapor pressure equals atmospheric pressure. That's why water boils at lower temperature when pressure is reduced (like on high mountain peaks) and at higher temperature when pressure is increased (like in a pressure cooker).
This post needs more attention. He said something wrong in the video, that doesn't even make sense -- without the air, you'd have zero pressure and that changes your position on the diagram. But if you meant water vapor only (no nitrogen etc) that's a direct contradiction.
I came here to make this comment, too. I think the problem was how it was presented. In a sealed container that is partially filled with liquid, there is always water vapor present above the liquid water. The concept of boiling means that almost all of the energy added is used to vaporize the liquid at that temp and pressure, which is measurable as the latent heat. Until the boiling point is reached, the energy increases the sensible heat of the liquid and vapor. Adding energy to a sealed container will vaporize water to cause the pressure to increase (following the vapor pressure curve) until the container ruptures or all the liquid is vaporized. After all liquid is vaporized then pressure increases per a non-ideal gas equation because water is not an ideal gas.
This channel has some of the most intuitive explanations (and demonstrations) of scientific concepts anywhere. I've said it before but for almost every video there's an "Oh! THAT'S how that works!" moment for me.
Everytime!!! Always so impressive! And thank you for saying the difference between gas and vapor. You ended a very long (friendly) debate between myself and one of my classmates from decades ago! I was so happy to send him this! And always such a pleasure to see your excitement about teaching... Absolutely contagious! Keep it up friend! I'll be sure to check out whatever you've got up your sleeve for the next video! Yeah science!
I find you channel extremely fascinating!!! Even though sometimes I don’t understand anything, I think that makes it even more interesting in some strange way
Hi! Great video! May I suggest something? Film it again having a diffuse light shining behind the vials. It can be a led behind a parchment paper. This will help visualize the phases as we do it in shadowsizing for two-phase flow.
Whoa. That vial is pressurized to 60 bar? That's almost 900 PSI. I wouldn't dare touch it, let alone cool it, heat it, etc. I didn't know a little glass container could hold that much pressure. Living & learning.
As a MSE undergrad, I've seen hundreds of phase diagrams in class, but never saw what a supercritical fluid actually looks like. As soon as I saw what was happening, it immediately became clear what was going on. Very cool!
Thanks for another great video! This reminds me when I was a sailor in a ship with a steam turbine for propulsion. We brought the feed water (very pure) up to 750 degrees at 550psi. This "dried" the water so that when it hit the turbine blades it didn't cause damage and was converted into a usable force. Fun stuff.
I like your videos a lot! Initially I did not enjoyed it but the quality of content and yor attitude conquered my heart and mind! Thank you very much for what you do!
I'm always enjoying your videos, so interesting! But I wonder if you may forgot to mention something around 4:20. Because materials, especially liquids possess a property called vapour pressure, causing the transition to a gas well below the boiling point in oder to establish a equilibrium between gas and liquid phase. This is also one of the reasons one can nicely smell liquors so easily. I'm just curious if you left it out on purpose. Anyway, keep up the great work!!
4:12 Well, if we had pure water surrounded by nothing but water vapor, extra water vapor would still come off of it. And the reason we see the vapor is because the partial pressure of the water vapor above the hot water greatly exceeds the vapor pressure that water would have at room temperature, and so the water vapor is at too high a pressure, and therefore condenses faster than it evaporates (the equilibrium is shifted towards condensation). And so this forms millions of tiny water droplets, which is visible.
We have a supercritical fluid extractor (S.F.E.) where I work. We use it to extract fat from liver powder and chlorophyll from alfalfa. The liver fat smells gross.
Currently taking thermodynamics and having to get used to the steam tables was super difficult for me. This is cool to see it demonstrated. "compressed liq. Saturated Mix, Superheated, and Super critical states"
I love seeing your videos, and trying to wrap my head around what I'm seeing, especially this. And I'm a little nervous that 60bar is being contained in that fragile-looking little ampule, I'd be afraid to handle it for fear it'll explode lol. One thing about water vapour though, I must mention, is that yes, even without air present, vapour still emerges off liquid water below 100°C. That's why it'll boil if you remove the air. There are a range of vapour pressures even below freezing, of course it's very low below freezingb(sublimation). Water will evaporate until there is equilibrium, then there is no net change of vapour/liquid and no boiling. This principle is used in heat pipes 👍
I think it’s cool that as the xenon approaches the critical point, the density of the vapor rises while the density of the liquid falls until they are equal with each other. That explains why the meniscus disappears the way that it does. The atoms in liquid phase and the atoms in vapor phase have no reason to stay separate so they just diffuse into each other. 3D phase diagrams are fascinating in that they also include density (or rather specific volume which is the inverse of density) along with temperature and pressure, showing how all three properties interact with each other.
Thanks for explaining the isolating the water part lol. That's got to be the most ignored part about that diagram that people just forget to teach it and cause a lot of confusion when solving vs seeing it
"It's not really a liquid not really a gas" *my second grade science class memories coming back to me and the joking that I didn't have back then fusing together* Ah a solid.
I really wonder what this would look like with food coloring introduced. Would it color the supercritical fluid, or would it just collect at the bottom, with a little bit of liquid that doesn't convert?
I can relate to this. I drag race utilizing nitrous oxide. The critical temperature is 36.5* C (97.7* F). Lots of fellow racers warm their nitrous oxide bottles to obtain a higher pressure inside the bottle. In order to spray through a fixed oriface, a pressure increase will flow more nitrous oxide and result in additional power. Of course too much nitrous will burn engine internals. I’ve seen friends (and I’ve done this myself) exceed the critical pressure, therefore spraying a gas/vapor instead of a liquid. It alters the Air/Fuel ratio (rich) and doesn’t make the full power potential. So any bottles temperatures exceeding 97.7 F will cause the bottles to release a vapor/ gas instead of a liquid.
Excellent. What is really tough for folks to understand is how we have learned that with exceptional high pressures we can now compress liquids and change their properrties.
Just a quick MASSIVE thank you for putting your Short Videos on a separate channel. I wish more TH-camrs would do this to keep my subscriptions from being overrun with Shorts.
Happy you come back to address the pressure issue. What you said in your video was correct of course but a little muddled for people who are not familiar with the subject. Another informative and fun vid.
This was one of your best videos. I'm a chemist, and as much as I've studied this stuff, supercritical states have always fascinated me, and you very rarely get to see them demonstrated so clearly.
By pressurizing a gas, you increase the density. And when it reaches the density of the liquid without any condensation, you get a supercritical fluid with a mixture of liquid and gas that can't be distinguished due to the same density.
Correction: The reason water begins to evaporate below boiling point is that the temperature only reflects the *average* kinetic energy, meaning some water particles are either moving faster or slower, according to a Normal Distribution. The part of the normal distribution whose kinetic energy exceeds the equivalent of the boiling point represents particles that will evaporate, if they are on the water surface. Excellent channel, by the way!
For those that play paintball with co2, you know that 88 degrees is when the velocity of the paintballs jumps because the co2 tank will be deliverying supercritical co2 instead of co2 gas,
im very interested in science and tech since i was a kid. i wish you have an animation in every thing that you say to be understandable easily because english is not my primary language and im a slow learner. more power to your channel
This particular video is much nice. Please post more on this. Probably this could be a life saver for high school students interested in physical chemistry.
Some boilers used to generate electricity are called super critical boilers. They operate at or above waters supercritical temp and pressures of 705.4 degrees f and 3206.2 psi respectively. They are known as forced-flow boilers, because in this state, natural circulation cannot occur due to the lack of distinction between density of water vs steam, meaning water wont flow down nor will steam rise to the top. Circulation is "forced" via mechanical means of a pump, offering even heat distribution among the entire volume of the steam/water medium
Nice video I was in IBM R&D Wets engineering had to explain to the operator's what was the process is. Video like this will help you with the explanation of process.
Literally every high school chemistry teacher ever: “There are three phases of matter: Solids, liquids and gases.” Then they would use gas and vapour interchangeably, making no distinction whatsoever. I had a grade 8 science teacher mention plasmas ONCE! It wasn’t until I had completed my second year of my Business degree that I even heard of supercriticals. So yeah, that’s three phases of matter I was never taught about in school. And oh yeah, I learned from Anton Petrov last year that there are 18 different kinds of water ice that occur in nature (only about five of which can be found on Earth), and that a 19th kind was recently discovered and produced in a lab. So yeah, the way I see it, there are 25 phases of matter. 26! I almost forgot about the experiment a few years ago that proved Hydrogen has a metallic phase.
@@louf7178 So would it not be the perfect time to learn these things to help a person chose a career so that he or she knows what post-secondary to pursue?
I knew all about super critical fluids, different types of ice, 1, 2, 3,4,5 6 and my fav, 7, and all sorts.... I didn't know the distinction between vapor and gas!!!!!!!!!!!!!!!!!! THANK YOU!
So I've been familiar with the concept of phase diagrams for more than 20 years, but obviously didn't understand them. My mind was blown several times in that video!
A supercritical liquid has long dark brown hair, a beard, a white t shirt and a backwards cap. Usually you can hear something that's sounds kinda like "WOOOOOO YEAH BABY"
It would also be worth mentioning/showing the vapour dome (P-v diagram). Not only is it neat for showing the phase transition, but also other stuff like the almost incompressible nature of most liquids, and of course the supercritical point at the peak of the vapour dome, where there is no longer a distinct set of boundaries to cross between liquid and gas.
Super cool stuff with actual theoretical explanation. Not for everyone but that's what make you a special youtuber, togheter with veritasium vsauce electroboom and such.
Few years back... I even heard that Supercritical water is inflammable when combines with distilled water and can be used to dispose the electronic waste without emitting radiation
A nice way to quantify how these phase change lines are valid only for pure, single component volumes, is to measure the temperature of dry ice. It is a common misconception (also a industry a lot!) that sublimating dry ice will always be at -78.5 C. Because our atmosphere has (thankfully) only a little amount of CO2, there will be additional diffusion of CO2 which cooles down the dry ice. This effect is commonly referred as the wet-bulb temperature. The physics are the same as the evaporating water from a pan discussed in this video and it is (was?) commonly used to measure the humidity in meteorology. If you make a good (dense) lump of dry ice and measure its temperature just in the room, you will measure a temperature which can be up to 20 degrees lower than the 'commonly' used sublimation temperature. Putting this in a semi-closed volume (simply a cup can sufficy, as CO2 is heavier than air), you will see that the temperature starts to rise as the CO2 concentration increases. I'm doing quantitative measurements of this effect for my master thesis. We have dry ice spheres hanging from a thermocouple, which I will place inside a fully controlled (temperature, pressure and composition) atmosphere. Preliminary results will be published at the ExHFT-10 conference this summer.
I want to address a concern that people are mentioning about vapor pressure. When you put a liquid in a container that is bigger than the volume of the liquid, some of the liquid will form a vapor until the container reaches the vapor pressure of that liquid at that temperature. If it is a pure liquid (no air in the container) and all of the liquid doesn't evaporate, then the total pressure will be somewhere along the liquid/vapor line on the phase diagram. But, if there is air in the container, then the liquid will form a vapor and increase the pressure until the partial pressure of the vapor reaches the the point on the liquid/vapor line in the phase diagram. The point is that if you have a *pure* substance and you tell me the temperature and pressure of the container it is in, then I can tell you if it is a liquid, solid, vapor or gas. (Also note that if the temperature and pressure are on the solid/liquid/gas equilibrium lines on the phase diagram, then I can't tell you how much solid/liquid/gas you have unless you tell me how much energy you have input into the system and how much liquid you started with etc.)
thanks for the clarification!
@The Action Lab = I’m old enough to remember Ammonia bubble lamps for Christmas tree bulbs.
> But, if there is air in the container, then the liquid will form a vapor and increase the pressure until the partial pressure of the vapor reaches the the point on the liquid/solid line in the phase diagram.
I think you mean the liquid/gas line. On the solid/liquid line you can't be in equilibrium with a gaseous phase (unless you're exactly at the triple point).
Only critique here is the emphasis on a pure substance, you can do the same thing for binary mixtures very easily, only need 1 more piece of information which is the molar fraction and then I can tell you the amount that is in the liquid phase, the vapor phase, and the contributing partial pressures of each species.
Vapor-liquid equilibrium diagrams aren't too difficult to read without a background in chemical engineering.
@@fat_pigeon Sublimation, transition from solid to gas. You can easily be on that equilibrium line without a triple point, easiest example is dry ice, frozen CO2.
The supercritical transition is still one of the coolest (heh) things I've ever seen. I've watched a lot of people using supercritical CO2 to make aerogel, and watching the meniscus just gradually disappear still blows my mind.
@@Flashisgreatfr yeah you're a kid
@@Flashisgreatfr Hey I’m a kid and did you know that I don’t give a f*ck?
NileRed did that also. That was the first time I've seen supercritical fluids in action!
@@thomasbodrey that's one of the places I've seen it, yeah. Such a cool thing to watch
Watching those got me to build my own chamber just to see it myself. Really cool to start with solid CO2, watch it go to solid+liquid+gas, then liquid+gas, then supercritical fluid. Put some stuff in the chamber and shake it around and you can tell there's a fluid in there that's slowing down movement more than a gas but less than a liquid. The cloudiness that forms when it goes back to liquid+gas is also fun to watch, you can see it in this video but it doesn't last as long as it does with CO2.
This is so cool, as a refrigeration tech I too have been curious of the phase change of supercritical fluids. Our entire industry is largely based supercritical and subcooled fluids to transfer heat and rely on pressure changes to affect said state.
Note to self: add refrigeration tech to list of cool jobs
@@JustABeeInFPV absolutely my friend, a bit of chemistry, a bit of physics, a bunch of mechanics, electrical and plumbing.
Get your gas ticket, you can install. Wire and supply gas to the furnace all eith 1 ticket. A buddy needs some electrical done, take out a permit and run the wire. Sister needs a new bathroom in the basement your ready to go.
We can work on up to 600VAC with the ticket and like I said get you gas ticket which we can as Fridge Techs and you can do gas fitting.
Most refrigerants except carbon dioxide do not ever inhabit the supercritical region. Superheated may have been the word you were looking for.
@Praise Jesus, Repent or Likewise Perish its funny how there are different versions of your new testament. Doesn't that say something? Each version is different.
Where can I buy Xenon?
I mean it when I say your videos are very hard to pass on. Every one I see available hooks me and reels me in like a fish lol. Arguably some of the most enlightening and entertaining content on TH-cam or anywhere else for that matter. You're a gifted teacher and I've learned a lot without having to try!
You always bring us the most epic thought-provoking videos I have ever seen on TH-cam!
I tip my hat to you Mr. Action Lab 🎩
This was a question I had in my mind for a long time but never got to search for an answer. This explanation is much more interesting than I expected!
Fun fact: Xenon gas is used in headlight bulbs called "High intensity discharge bulbs" or HID. Electricity is used to ignite the gas and keep it at a stable temperature. The temperature of the gas once ignited determines the color of the light being projected. You can have anything from amber (lower temps), to bright white (slightly higher), to blue (slightly higher), and more.
That was fun!
Its not the temperature of the gas, its the difference between the energy levels of the atoms of such gas
@@germánciliurczuk Wouldn't differing energy levels mean differing temperatures? I would think they'd correlate.
@@mikedejesus7064 Honestly, i don't know how it correlates with temperature, but the key point is that the light emitted in discharge lamps is due to ionization of the gas and not its temperature. Thats why its emissions spectrum is limited to a few frequencies unlike a black body radiation.
Headlight fluid
I’m guessing it grows a hair and beard, puts on a white tshirt, and gets a deeper voice along with a vernacular full of obscenities.
This clarifies so much physics, I had no idea. Your videos always bring something new! I’m 29, and really interested in science, and yet, you never fail to drop new knowledge with every video!
This is more chemistry than physics…
If you really want to learn, go to school. Watching TH-cam is not education. It’s entertainment. Education is an active process, not passive.
@@andybaldman I think it’s a mix of both… of course this channel is mostly concentrated in entertainment via science. But I’m sure there are channels within YT dedicated to more in depth explanation. School I think is good later on for finding better jobs but I never think it’s necessary to learn…
@@maoomph thermodynamics is physics
@@juanmariogarciarueda4628 ok bruh… all I said is it leans more in chemistry I never said it’s not physics.
I super appreciate your work and this channel. It often sorts out concept for me that have been rattling around in the back of my head for ages.
dude, your channel rocks. I;ve been repeatedly impressed with how you can tackle a highly complex topic with seemingly simple demonstrations. I've forwarded many videos to friends with "see, this is why this happens or works this way, etc"!
The cool thing is that as the supercritical fluid forms, the gas above and liquid below approach having the exact same refractive index, which is why the division between then becomes more and more difficult to discern.
The refractive index is merely a consequence or side effect of the density (for transparent homogeneous phases).
We can no longer see the difference between the two phases because...there is no difference, they're absolutely identical :D
Yeah I know it's a detail and in practice we can only compare the refractive index by looking at a sealed ampule, but I think it's even more mind blowing to realise the two phases *are* identical, than to only assume their refractive indexes (one of many properties) being equal
@@YounesLayachi Yes, that's exactly right. This is why I didn't concentrate on the state of them being the same because that's pointless. I focused on the two approaching having the same refractive index, and that's why they become more and more difficult to distinguish. Now this is, of course, due to their density (and other properties) approaching homogeneity, but it's still true that the refractive indices approaching equality makes them more difficult to distinguish. The smaller the difference in refractive index, the less light reflects on the boundary of the liquid and gas.
I believe what you said at 4:05 is not right...you should always talk about partial pressures - there is always some partial pressure of gaseous phase over liquid - the bold line in phase diagram just marks the point, when partial pressure of gas equal the surrounding pressure (in everyday life it is atmosferic pressure)
As a chemist, I have to agree with you. The property is called vapor pressure. For water at 25 °C, it's 3170 Pa. For ethanol, it's much higher -- 5950 Pa at 20 °C. Therefore, a vessel containing only ethanol (no air) would be under pressure of 6 kPa at 20 °C only from ethanol vapor.
At boiling point, vapor pressure equals atmospheric pressure. That's why water boils at lower temperature when pressure is reduced (like on high mountain peaks) and at higher temperature when pressure is increased (like in a pressure cooker).
And of course, there is evaporation occurring as well.
This post needs more attention. He said something wrong in the video, that doesn't even make sense -- without the air, you'd have zero pressure and that changes your position on the diagram. But if you meant water vapor only (no nitrogen etc) that's a direct contradiction.
This needs more likes. The community needs to know the correct answer.
I came here to make this comment, too. I think the problem was how it was presented.
In a sealed container that is partially filled with liquid, there is always water vapor present above the liquid water. The concept of boiling means that almost all of the energy added is used to vaporize the liquid at that temp and pressure, which is measurable as the latent heat. Until the boiling point is reached, the energy increases the sensible heat of the liquid and vapor. Adding energy to a sealed container will vaporize water to cause the pressure to increase (following the vapor pressure curve) until the container ruptures or all the liquid is vaporized. After all liquid is vaporized then pressure increases per a non-ideal gas equation because water is not an ideal gas.
Simply explained but still professionally. That’s why I love this dude
This channel has some of the most intuitive explanations (and demonstrations) of scientific concepts anywhere. I've said it before but for almost every video there's an "Oh! THAT'S how that works!" moment for me.
Everytime!!! Always so impressive! And thank you for saying the difference between gas and vapor. You ended a very long (friendly) debate between myself and one of my classmates from decades ago! I was so happy to send him this! And always such a pleasure to see your excitement about teaching... Absolutely contagious!
Keep it up friend!
I'll be sure to check out whatever you've got up your sleeve for the next video!
Yeah science!
I love this channel, I always learn new and interesting things
I find you channel extremely fascinating!!! Even though sometimes I don’t understand anything, I think that makes it even more interesting in some strange way
Hi! Great video! May I suggest something? Film it again having a diffuse light shining behind the vials. It can be a led behind a parchment paper. This will help visualize the phases as we do it in shadowsizing for two-phase flow.
Whoa. That vial is pressurized to 60 bar? That's almost 900 PSI. I wouldn't dare touch it, let alone cool it, heat it, etc.
I didn't know a little glass container could hold that much pressure.
Living & learning.
Yeah. It surprised me too.
Thats what I thought too. I want to know how he created it, or who did, and how?
yes a little scary. I wore safety glasses...
@@TheActionLab is there a way to buy it?
As a MSE undergrad, I've seen hundreds of phase diagrams in class, but never saw what a supercritical fluid actually looks like. As soon as I saw what was happening, it immediately became clear what was going on. Very cool!
I have seen triple point labs but I have not seen the critical point before! This is really neat. Just seeing the meniscus disappear.
I once tried to make super critical liquid, but it said I was doing it wrong...
Thanks for another great video! This reminds me when I was a sailor in a ship with a steam turbine for propulsion. We brought the feed water (very pure) up to 750 degrees at 550psi. This "dried" the water so that when it hit the turbine blades it didn't cause damage and was converted into a usable force. Fun stuff.
I like your videos a lot! Initially I did not enjoyed it but the quality of content and yor attitude conquered my heart and mind! Thank you very much for what you do!
Love your content and it's very educational
I learnt so much here because of your channel. As a science graduate i haven't learnt this much in my academics. Thanks to you.
I'm always enjoying your videos, so interesting!
But I wonder if you may forgot to mention something around 4:20. Because materials, especially liquids possess a property called vapour pressure, causing the transition to a gas well below the boiling point in oder to establish a equilibrium between gas and liquid phase. This is also one of the reasons one can nicely smell liquors so easily.
I'm just curious if you left it out on purpose. Anyway, keep up the great work!!
nile red + you is the best combo for better understanding
4:12 Well, if we had pure water surrounded by nothing but water vapor, extra water vapor would still come off of it. And the reason we see the vapor is because the partial pressure of the water vapor above the hot water greatly exceeds the vapor pressure that water would have at room temperature, and so the water vapor is at too high a pressure, and therefore condenses faster than it evaporates (the equilibrium is shifted towards condensation). And so this forms millions of tiny water droplets, which is visible.
We have a supercritical fluid extractor (S.F.E.) where I work. We use it to extract fat from liver powder and chlorophyll from alfalfa. The liver fat smells gross.
Currently taking thermodynamics and having to get used to the steam tables was super difficult for me. This is cool to see it demonstrated. "compressed liq. Saturated Mix, Superheated, and Super critical states"
I love seeing your videos, and trying to wrap my head around what I'm seeing, especially this. And I'm a little nervous that 60bar is being contained in that fragile-looking little ampule, I'd be afraid to handle it for fear it'll explode lol.
One thing about water vapour though, I must mention, is that yes, even without air present, vapour still emerges off liquid water below 100°C. That's why it'll boil if you remove the air. There are a range of vapour pressures even below freezing, of course it's very low below freezingb(sublimation). Water will evaporate until there is equilibrium, then there is no net change of vapour/liquid and no boiling. This principle is used in heat pipes 👍
I think it’s cool that as the xenon approaches the critical point, the density of the vapor rises while the density of the liquid falls until they are equal with each other. That explains why the meniscus disappears the way that it does. The atoms in liquid phase and the atoms in vapor phase have no reason to stay separate so they just diffuse into each other. 3D phase diagrams are fascinating in that they also include density (or rather specific volume which is the inverse of density) along with temperature and pressure, showing how all three properties interact with each other.
I love it. Where could I buy one of these to demonstrate this to my daughter? She's 9 and loves science! I looked online and didn't find much.
Were you sucessfull in bying one?
Thanks for explaining the isolating the water part lol. That's got to be the most ignored part about that diagram that people just forget to teach it and cause a lot of confusion when solving vs seeing it
I'm most surprised that little glass vessel can hold 60 atmospheres..that's almost 890 psi right?
Thick Pyrex
The supercritical becomes in so many ways, laws of physics, gravity, laws of molecular activities/nuclear science.
"It's not really a liquid not really a gas"
*my second grade science class memories coming back to me and the joking that I didn't have back then fusing together*
Ah a solid.
You mean moistcritikal?
W
make this the top comment
_'And then it just... Disappears.'_
I want to get a sealed jar of this to just mess with people now.
I really wonder what this would look like with food coloring introduced. Would it color the supercritical fluid, or would it just collect at the bottom, with a little bit of liquid that doesn't convert?
Great (and simple sounding) explanation for a very complicated process! Also love the visual demonstration with xenon gas! Great video, as always!
I can relate to this.
I drag race utilizing nitrous oxide.
The critical temperature is 36.5* C (97.7* F).
Lots of fellow racers warm their nitrous oxide bottles to obtain a higher pressure inside the bottle.
In order to spray through a fixed oriface, a pressure increase will flow more nitrous oxide and result in additional power.
Of course too much nitrous will burn engine internals.
I’ve seen friends (and I’ve done this myself) exceed the critical pressure, therefore spraying a gas/vapor instead of a liquid.
It alters the Air/Fuel ratio (rich) and doesn’t make the full power potential.
So any bottles temperatures exceeding 97.7 F will cause the bottles to release a vapor/ gas instead of a liquid.
Excellent. What is really tough for folks to understand is how we have learned that with exceptional high pressures we can now compress liquids and change their properrties.
I stumbled on to this channel a couple days ago. Now I'm hooked.
Just a quick MASSIVE thank you for putting your Short Videos on a separate channel. I wish more TH-camrs would do this to keep my subscriptions from being overrun with Shorts.
Happy you come back to address the pressure issue.
What you said in your video was correct of course but a little muddled for people who are not familiar with the subject.
Another informative and fun vid.
I want to thank you for the content and the excellent pronunciation, that helps a lot to non native English people
I remember learning about the conversion graph in chemistry class. It is really cool to see it again.
I knew all this stuff theoretically before. But in this vid I actually SAW the phenomenon for the first time! Thank you so much!
I saw a video of a guy who makes water freeze, evaporate, and be liquid, all at the same time and it's amazing.
This was one of your best videos. I'm a chemist, and as much as I've studied this stuff, supercritical states have always fascinated me, and you very rarely get to see them demonstrated so clearly.
The liquid being heated: "change the world, my final message, goodbye"
Great, it's already after 1am, now I'm gonna be on wikipedia and google for hours looking up supercritical fluids...
Nice video! I am running supercritical CO2 every working day! And I am still amazed by the diversity of possible applications!
Thank you for this demonstration!
I've only heard about these concepts. Watching a supercriticality for a first time..
Really worth it.. Thanks
By pressurizing a gas, you increase the density. And when it reaches the density of the liquid without any condensation, you get a supercritical fluid with a mixture of liquid and gas that can't be distinguished due to the same density.
Its the triple point at which it becomes supercritical, as at that point water exist in a transition state
I like the way you explain the chemistry.
Correction: The reason water begins to evaporate below boiling point is that the temperature only reflects the *average* kinetic energy, meaning some water particles are either moving faster or slower, according to a Normal Distribution. The part of the normal distribution whose kinetic energy exceeds the equivalent of the boiling point represents particles that will evaporate, if they are on the water surface.
Excellent channel, by the way!
So cool to see this stuff happening in real life instead of learning through tables/graphs like at school.
It still amazes me that Dimethyl Sulfoxide has a freezing point of 66.2F (19C).
For those that play paintball with co2, you know that 88 degrees is when the velocity of the paintballs jumps because the co2 tank will be deliverying supercritical co2 instead of co2 gas,
That was the coolest thing I've seen you demonstrate. Blew my mind. Like watching a mirage dissappear. So cool!
You're basically turning it into a rain cloud and then it rains and the cloud goes away, something which usually takes 5 hours is shown in one second
Wow - difficult to get your head around this - great stuff man.
im very interested in science and tech since i was a kid. i wish you have an animation in every thing that you say to be understandable easily because english is not my primary language and im a slow learner.
more power to your channel
This particular video is much nice. Please post more on this. Probably this could be a life saver for high school students interested in physical chemistry.
Some boilers used to generate electricity are called super critical boilers. They operate at or above waters supercritical temp and pressures of 705.4 degrees f and 3206.2 psi respectively. They are known as forced-flow boilers, because in this state, natural circulation cannot occur due to the lack of distinction between density of water vs steam, meaning water wont flow down nor will steam rise to the top. Circulation is "forced" via mechanical means of a pump, offering even heat distribution among the entire volume of the steam/water medium
Nice video I was in IBM R&D Wets engineering had to explain to the operator's what was the process is. Video like this will help you with the explanation of process.
action lab:
' not a liquid or a gas '
me:
' wait I~
there~
*theres a solid too*
LIQUID TURNS SUPERCRITICAL *woooooooh! YEAAAAAAAH BABY THAT'S WHAT WE'VE BEEN WAITING FOR*
It just disappears like the invisible man would disappear.
Literally every high school chemistry teacher ever: “There are three phases of matter: Solids, liquids and gases.”
Then they would use gas and vapour interchangeably, making no distinction whatsoever. I had a grade 8 science teacher mention plasmas ONCE! It wasn’t until I had completed my second year of my Business degree that I even heard of supercriticals. So yeah, that’s three phases of matter I was never taught about in school. And oh yeah, I learned from Anton Petrov last year that there are 18 different kinds of water ice that occur in nature (only about five of which can be found on Earth), and that a 19th kind was recently discovered and produced in a lab. So yeah, the way I see it, there are 25 phases of matter.
26! I almost forgot about the experiment a few years ago that proved Hydrogen has a metallic phase.
It's only secondary school --- scope of work.
@@louf7178 So would it not be the perfect time to learn these things to help a person chose a career so that he or she knows what post-secondary to pursue?
Best videos where you go straight to the point!
Action Labs: *Shows Phase Diagrams*
Chemical Engineers: *Vietnam Flashbacks*
I never get tired of watching that.
Neither Solid nor Liquid, he was a well-balanced masterpiece.
Man I look forward to these !
Nile Red’s Going Supercritical episode has him making a chamber to allow him to film the transition.
I knew all about super critical fluids, different types of ice, 1, 2, 3,4,5 6 and my fav, 7, and all sorts.... I didn't know the distinction between vapor and gas!!!!!!!!!!!!!!!!!! THANK YOU!
And when the already supercritical thing becomes further supercritical, it becomes someone special.
So I've been familiar with the concept of phase diagrams for more than 20 years, but obviously didn't understand them. My mind was blown several times in that video!
You can technically make real life potions with chemistry, it's just that most of them are poison potions
A supercritical liquid has long dark brown hair, a beard, a white t shirt and a backwards cap. Usually you can hear something that's sounds kinda like "WOOOOOO YEAH BABY"
4 years after graduating from school I see this video and finally get what they tried to show in schools 🙂
This is pretty cool. I too never witnessed the meniscus disappear
When liquid turns super critical is best to depersonalize, be objective and consider, and if necessary be assertive
It would also be worth mentioning/showing the vapour dome (P-v diagram). Not only is it neat for showing the phase transition, but also other stuff like the almost incompressible nature of most liquids, and of course the supercritical point at the peak of the vapour dome, where there is no longer a distinct set of boundaries to cross between liquid and gas.
this will be super cool to see this in slow motion with some high speed cameras !!
Super cool stuff with actual theoretical explanation. Not for everyone but that's what make you a special youtuber, togheter with veritasium vsauce electroboom and such.
Its really interesting how the water looks like it just vaporizes
Schrodinger's phase of matter.
I always wondered about steaming cups and water vs vapor vs temperature. It's confusing! The water phase diagram is really cool, so many forms
Do more of this gas properties videos
Really interesting, I'm also studying chemical engineering
58 bar , 860 psi in that small glass vessel. Great demonstration.
Few years back... I even heard that Supercritical water is inflammable when combines with distilled water and can be used to dispose the electronic waste without emitting radiation
A nice way to quantify how these phase change lines are valid only for pure, single component volumes, is to measure the temperature of dry ice.
It is a common misconception (also a industry a lot!) that sublimating dry ice will always be at -78.5 C. Because our atmosphere has (thankfully) only a little amount of CO2, there will be additional diffusion of CO2 which cooles down the dry ice. This effect is commonly referred as the wet-bulb temperature. The physics are the same as the evaporating water from a pan discussed in this video and it is (was?) commonly used to measure the humidity in meteorology.
If you make a good (dense) lump of dry ice and measure its temperature just in the room, you will measure a temperature which can be up to 20 degrees lower than the 'commonly' used sublimation temperature. Putting this in a semi-closed volume (simply a cup can sufficy, as CO2 is heavier than air), you will see that the temperature starts to rise as the CO2 concentration increases.
I'm doing quantitative measurements of this effect for my master thesis. We have dry ice spheres hanging from a thermocouple, which I will place inside a fully controlled (temperature, pressure and composition) atmosphere. Preliminary results will be published at the ExHFT-10 conference this summer.