And its only 30 degrees, if my hand could somehow resist the high pressure i could dip it in this supercritical fluid, i wonder what would it feel like.
It's a very interesting question, and you've gotten me to want to speculate about this using what I know about fluid flow of varying Reynolds numbers (basically a scale factor for how fluid flow behaves). Imagine holding your hand out a car window and feel how the air moves around your hand. Then, imagine dragging your hand through water and how that feels. In many ways, the turbulence around your skin is very similar, just to different degrees. The water, being denser and thus possessing more momentum for any given speed, sort of wobbles around your hand in a slow motion sense, compared to the "noise" type feeling that less dense air does. Both examples would be relatively high Reynolds number flows, as the main effects you would feel would be momentum-based. This is distinct from low Reynolds number flow, which would be sort of like dragging your hand through honey (little to no bumpy sensations of turbulence but lots of drag). With a supercritical fluid, the sensation around your hand could be every degree between these two extremes, since supercritical fluids can be "tuned" with varying temperature and pressure. If you could somehow address High Pressure Nervous Syndrome (theoretically possible since the cause of this syndrome is not exactly known), you could slowly subject the human body to compression up to the 80 atmosphere supercritical pressure while the person would breathe a helium mixture with around half a percent composition of oxygen (anything much higher would cause oxygen toxicity. Even nitrogen is toxic at these pressures). From there, varying the temperature would be a very interesting experience for you could be initially be standing in a vat of liquid CO2 and high pressure (probably mostly helium for health reasons?) gases. You would initially observe a typical reflective surface of the liquid in which you would be standing. This liquid would be a denser version of something that vaguely felt like water but had none of the surface tension properties of it. You could probably attempt to cup the stuff in your hands but it would be extremely difficult to keep in your hands, due to the much lower surface tension compared to water. It would quickly pour out strangely smoothly, as liquid CO2 droplets would be extremely tiny due to its low surface tension. Breathing might actually be an issue at liquid-CO2 pressures, though, since your lungs would probably form a condensation of liquid CO2 on their inner surface instead of escaping your lungs upon exhale. However, since your lungs would be above supercritical temperature, I'm thinking the CO2 could escape your lungs relatively normally and then form a cloudy CO2 vapor in the now-cool pre-supercritical temperature chamber, like breathing on a cold day. Water vapor would also escape your lungs in a cloud as normal, since you'd still be at pressures low enough for water to continue existing as a liquid and not one of the exotic weirdo Ice## phases. I don't know whether liquid CO2 and liquid water are miscible. If they are, then the CO2 could probably dissolve in the water droplets and escape normally. As the temperature rose in the room, that shiny water-like surface would begin to "fuzz out" much like what divers observe when they shine a flashlight off the surface of an undersea brine lake. At the point of supercriticality (once all the liquid has reached that temperature) you would no longer be able to splash your hands in the surface, but you would certainly feel a density shift (like some kind of added turbulence to your hands) and you would probably be effectively mixing up the quickly-disappearing surface with the surrounding air. I'd be very interested to see how distorted your hand would look as the density of this fluid would be varying all around your hands (since temperature distribution would not be uniform). You'd probably want to make sure you're breathing through some breathing apparatus because you do not want that amount of supercritical CO2 entering your lungs. If you thought excess CO2 gas caused a suffocating sensation, supercritical CO2 would probably be a different world of discomfort. I'm not sure what kind of filter would keep supercritical CO2 out of your lungs, but you'd pretty much likely have to breathe in a completely airtight system. Basically I think this whole scenario would be possible. It'd be super expensive, probably unhealthy at the very least, but definitely possible.
TheFerruccio Very interesting. Supercritical CO2 would probably be unlike any else liquid we can dip our hands in in normal conditions. Sure, there are liquids with very low surface tension but the combination of supercritical CO2 properties would be special.
The feeling on our skin would probably be especially interesting. I'm thinking it could probably be somewhat simulated by trying to find a liquid of very low density we can put our hands safely in (that might actually be difficult), and have it somehow mix with much higher density liquids, then pass our hand through the interface and feel that non-instantaneous shift in fluid properties.
This is so cool!! You actually see the point at which liquid CO2 can no longer be a liquid and see it happen before your eyes. But not like a liquid in a chamber whose pressure is decreased until it boils; then you just see it boiling away and maybe freezing. In this case, the critical temperature is reached and the temperature and pressure are still increasing. The liquid stops boiling because of the pressure and you kind of see it just reach the same density as the gas and it takes on an intermediate form right before your eyes!! I want a small chamber like that...one that's not going to explode and kill me.
Why even look at Jupiter? Venus is nearly totally surrounded by this stuff at the surface Its surface temperature is over 400 °C, pressure over 90 atmospheres, and the atmosphere is 96% CO2
Ah thank you. I’ve been trying to imagine what the in between layers of gas giants could act like. Because with all of the pressure from the gas above, and giant hydrogen oceans below i thought there couldn’t be a clear line between the two. Though this probably isn’t exactly what it would look like without the same temperatures and density’s it gives me a vague sense of what it could be like.
Hi, yes you can fill a container completely with liquid CO2, if the container is cooled during the filling process. If not the temperature will rise due to the Joules Thomsen effect. The pressure would be (at 70F = 21°C) about 60 Bar.
To actually pass through the critical point, the vapor-liquid mensicus needs to stay in the middle of the vessel (equal volumes of the liquid and gas) at the moment that the two phases merge. If the meniscus drops, you are evaporating all the liquid before you hit the critical point, and your density is a bit low. Conversely, if you start with too much material in the vessel, then the liquid level rises and you pass by the critical point in the compressed liquid side of the phase diagram. Agitating the fluid in the vessel by rocking it works very well to show that the densities of the two phases approach each other as the fluid approaches the critical point.
I'd not say right at the middle of the vessel. The actual level at which heating up make it passes through critical point can be calculated based on the critical molar volume of the substance.
The turbidity is caused by small temperature differentials around the critical point where liquid is boiling then recondensing quickly. At equilibrium there would be no turbidity.
Hi Flachzange. I've been reading about producing methane directly from reaction of hydrogen with supercritical CO2. If the gas in your container were hydrogen and the hydrogen and CO2 were in the correct proportions could you create that reaction safely in your container? I think the temperature has to be raised above 300degrees centigrade and some form of catalyst may be needed. The aim behind that idea on a large/world scale is: if you can create methane (natural gas we use in the home) synthetically from hydrogen (electolysis of water) and CO2 (captured from industrial processes) additional carbon is not added to the atmosphere by the ongoing continuous burning of the fossil fuel for energy. The electricity for the electrolysis is coming from a renewable energy source, solar, wind or hydro.
Industrial volumes of CO2 are 'cracked' off of hydrocarbons (natural gas in particular) coming out of the ground to begin with. You would be starting from high energy, going to liquid CO2, then back to high energy. The energy would have to come from somewhere. If you can find a good way to capture atmospheric CO2 and purify it then yes it would work.
That happens because with the temperature, the pressure rises. The liquid water lowers its density, the density of the gaseous water rises til the critical point where the density of both is the same.
this is what rocky core of uranus consists of! It has stone and ice, and its surrounded by layer of supercritical fluid. Who knows what swimming in those would feel like (if you have some special suit that would prevent you from getting crushed, that is :) )?
@mrjazzycharon2 Earth's atmospheric pressure is too low to support supercritical fluids at room temperature. For example, the supercritical point of water can be found in the deepest ocean trenches from undersea vents called 'smokers', at pressures that would crush any human being, at around 330C in temperature.
the pressure it's kept constant at about 73 atm for CO2, the temperature in this case is increased to reach that supercritical point, google 'phase diagram for CO2' it will make more sense to look at the graph.
one of techniques that I can propose - you my use high pressure pVT cell (or any container that can persist high pressures) - (1) - if you fill the cell with CO2 and have a second vent, air should go out of the cell (if the vent is at the top) because higher CO2 density. After that you have only CO2 in the cell. if you can keep constant temperature, by increasing the pressure in the cell you can reach "vapor curve", i.e. dew point of CO2 (which at 70F is 58 bar).
I tried to imagine before what supercritical fluid in the interior of gas planets would look like, interesting to actually see it. I wonder what it would feel like to touch it? More like a fluid, or more like putting your hand in the wind?
At higher pressures it will only return to the liquid phase if the temperature is below the critical temperature. Otherwise it will stay supercritical.
It lacks certain qualities of a liquid. There is no surface tension, and no clear boundary between liquid-like and gas-like states of matter. The supercritical carbon dioxide looks like a roiling sea, except that a roiling sea is an interaction between wind and water very different in composition. With supercritical carbon dioxide the "sea" and the "wind" are the same substance. en.wikipedia.org/wiki/Supercritical_fluid
@@Flachzange1337 That happens because with the temperature, the pressure rises. The liquid water lowers its density, the density of the gaseous water rises til the critical point where the density of both is the same. now you see?
How nice of your vedeo! It helps me to understand the state of 'supercritical'. Can I ask you that where was this experiment conducted? At the school, Institute or somewhere..?
+MrJJunSang Because I want to use your video at my presentation in the school. And I want to identify the source, not only URL but also the place or organization.
At that moment CO2 will have vapour and liquid phase. You have to decrease volume until the pressure starts to increase again (that is the moment when the last bubble of gas turned to liquid). Or, in other words, the pressure in 2-phase states remains constant when you're changing only volume.
What is happening when it suddenly turns cloudy looking? Is that when the supercritical liquid is cooled to the point where it starts condensing into a liquid again?
I don't understand the message in the video that says when the chamber is filled with more co2 the fluid level increases with higher temperature. How does increasing temperature increase the amount of fluid??
Raising the temperature doesn't add more liquid, it causes the fluid to expand. As the liquid phase is much denser than the gaseous phase it expands at a higher rate and compresses the vapor, so the level rises. On the other hand, in the beginning of the video the vapor is not yet saturated, so the liquid starts to evaporate, which decreases its level. In reality both processes of expansion and evaporation occur simultaneously in all displayed cases, it is just a matter of which one would prevail over the other. I would assume that at a certain liquid/gas proportion the level would remain constant during heating until the critical point is reached.
I feel you. 5 years ago I was watching supercritical liquids being used in drycleaning, and laughing my ass off. In 2019 there's one machine using CO2 in Canada and in Amsterdam. I'm a drycleaner btw
yes i have made this by myself. Maybe i am makeing a bigger one in the future but then to figure out how a electrical discharge behaves in liquid (and supercritical) gases.
Does anybody know where I can buy that small glas tubes filled with supercritical CO2 in europe of from europe? Sending this in plane maybe could be problematic
Hello; I have been looking everywhere for answers to these I guess unusual questions. Please help if you can or send me to the person who can, if you know of somebody. 1. Assuming you have a container that can withstand the pressures, can you fill a container completely full of liquid co2? 2. If you can, what pressure would it exert at say 70 degrees F. Note: I be leave you probably can and the pressure would be whatever the vapor pressure Would be at that temperatur
very informative interesting video im curious if there was only liquid co2 at the very bottom of the cylinder like a few ml and the rest existed as a gas and it was heated in the same way would it still reach super critical phase? im thinking on a larger scale for instance 50 gallons with only 1 or 2 gallons liquid
It's really really great video! Our team make a video about thermodynamics now. Could we use this video as references...? It's really helpful to make viewers understand about thermodynamics...!! Of course we will mark your name on our video. Could you allow to use this video...?
+Evgeni Sergeev I would think that in a P-V diagram it would be a verticle line (with the X-axis being Volume). As for the answer regarding the liquid level which some people have asked - why does the level of liquid rise on heating - Imagine the Guassian-like dome (with the inside of the dome showing a mixture of liquid and vapor; the left side of the dome signifying liquid and the right side of the dome signifying vapour). THe initial ratio of the masses of liquid to vapour defines the dryness fraction (denoted as x). THe line inside the dome on which this lies is determied by the intiial pressure and temperature. From this initial location, as heat is added isochorically, we move up the line. If the initial point is to the left of the maxima of the dome, the final point is more towards the lower vapour fraction. That would mean that the liquid fraction increases and the level of liquid actually rises (Which is seen in the video). If the initial point x is on the right of the dome maxima, then the reverse happens - the final point x is on the higher vapour fraction and consequently the amount of liquid decreases. When sufficiently heated, the final point may rise above the pressure at which the maxima of the dome occurs (which is the cricial pressure). Above this pressure, liquid and vapour coexist.
@@CoolMusicsChannel Certainly. But on a P-T diagram you will then have to go along the isochore, which is not difficult to do in a P-V or infact a T-V diagram. Fundamentals still apply though
A good question. I find that nearly all of the videos and explanations that cover the critical point and supercritical fluids out there tend to avoid or brush over the critical point itself and fail to explain in simple terms what is happening at the molecular level. I scrolled down many comments on many videos and didn't really see a single good question that addressed that, until I saw yours of course. Well I happen to have design experience with supercritical fluids, specifically as a working fluid for waste heat recovery, so I wanted to give you a brief explanation. At the critical point of a fluid, the molecules are being squeezed together to just the right distance from each other, such that they effectively all 'vibrate' in phase. It's a function of the Van Der Waals radii and the fluid in question (hence why different CP for different fluids) and one other interesting property at the critical point; the internal energy U is 0, because at the CP the molecules are vibrating in phase, therefore there are effectively no molecules acting against each other in simplistic terms. This is what causes many of the interesting properties, such as opacity. The in-phase vibration of the fluid at the critical point means light has a hard time passing through the fluid due to the much higher chance of interaction with molecules. Other effects include sudden asymptotic drop in the speed of sound through it, massive increase in specific heat capacity, and significant instability, by which I mean in a transient system where fluid flows, it is very hard to control and predict. In a nutshell, at the CP, the fluid acts like a macroscopic molecule.
I forgot to add; when the fluid passes through the critical point and becomes supercritical, internal energy increases and it falls out of phase, therefore transparency returns. Hope this helps!
Thanks, this question goes along with my last one, If you can fill the tank completely can you now change the entire liquid content in the tank to a gas by only raising/lowering Temperature or pressure? I am curious if it can Be done with a container being full (or if not, how full would it work) before the saturation level of the vapor would become so high that it would force the vapor to liquid form.
that thing was a gas, supercritical fluids do not exist at normal atmospheric pressures, the pressure in the container of this video is way above this pressure (about 73 times larger in the case of CO2).
In the first example the level of liquid CO2 decreases as the temperature increases. I'm wondering why in the second example when the chamber is filled with more liquid CO2 the fluid level increases (instead of decreasing) with higher temperature.
By adding more CO2 you bring the pressure up above the critical point. So instead of boiling, it expands to fill the vacuum. I think that once it fully fills the vacuum it’d be considered a super critical fluid.
Above critical pressure, it cannot boil. Above critical temperature it cannot condense. So this is what happens when it’s first brought above critical pressure then brought above critical temperature.
you're probably think of the famous supler fluid video. What people forget is taht the liquid didn't actually pass through the ceramic bottom. It went up the side of the container.
No. When he says he adds Co2. That's a way of saying he's raising the pressure. The pressure would also increase as he increases the temperature. The only constant during this experiment is the volume of the chamber.
And its only 30 degrees, if my hand could somehow resist the high pressure i could dip it in this supercritical fluid, i wonder what would it feel like.
It would feel like pain! Jk actually an interesting question
It's a very interesting question, and you've gotten me to want to speculate about this using what I know about fluid flow of varying Reynolds numbers (basically a scale factor for how fluid flow behaves). Imagine holding your hand out a car window and feel how the air moves around your hand. Then, imagine dragging your hand through water and how that feels. In many ways, the turbulence around your skin is very similar, just to different degrees. The water, being denser and thus possessing more momentum for any given speed, sort of wobbles around your hand in a slow motion sense, compared to the "noise" type feeling that less dense air does. Both examples would be relatively high Reynolds number flows, as the main effects you would feel would be momentum-based. This is distinct from low Reynolds number flow, which would be sort of like dragging your hand through honey (little to no bumpy sensations of turbulence but lots of drag). With a supercritical fluid, the sensation around your hand could be every degree between these two extremes, since supercritical fluids can be "tuned" with varying temperature and pressure.
If you could somehow address High Pressure Nervous Syndrome (theoretically possible since the cause of this syndrome is not exactly known), you could slowly subject the human body to compression up to the 80 atmosphere supercritical pressure while the person would breathe a helium mixture with around half a percent composition of oxygen (anything much higher would cause oxygen toxicity. Even nitrogen is toxic at these pressures). From there, varying the temperature would be a very interesting experience for you could be initially be standing in a vat of liquid CO2 and high pressure (probably mostly helium for health reasons?) gases. You would initially observe a typical reflective surface of the liquid in which you would be standing. This liquid would be a denser version of something that vaguely felt like water but had none of the surface tension properties of it. You could probably attempt to cup the stuff in your hands but it would be extremely difficult to keep in your hands, due to the much lower surface tension compared to water. It would quickly pour out strangely smoothly, as liquid CO2 droplets would be extremely tiny due to its low surface tension. Breathing might actually be an issue at liquid-CO2 pressures, though, since your lungs would probably form a condensation of liquid CO2 on their inner surface instead of escaping your lungs upon exhale. However, since your lungs would be above supercritical temperature, I'm thinking the CO2 could escape your lungs relatively normally and then form a cloudy CO2 vapor in the now-cool pre-supercritical temperature chamber, like breathing on a cold day. Water vapor would also escape your lungs in a cloud as normal, since you'd still be at pressures low enough for water to continue existing as a liquid and not one of the exotic weirdo Ice## phases. I don't know whether liquid CO2 and liquid water are miscible. If they are, then the CO2 could probably dissolve in the water droplets and escape normally.
As the temperature rose in the room, that shiny water-like surface would begin to "fuzz out" much like what divers observe when they shine a flashlight off the surface of an undersea brine lake. At the point of supercriticality (once all the liquid has reached that temperature) you would no longer be able to splash your hands in the surface, but you would certainly feel a density shift (like some kind of added turbulence to your hands) and you would probably be effectively mixing up the quickly-disappearing surface with the surrounding air. I'd be very interested to see how distorted your hand would look as the density of this fluid would be varying all around your hands (since temperature distribution would not be uniform). You'd probably want to make sure you're breathing through some breathing apparatus because you do not want that amount of supercritical CO2 entering your lungs. If you thought excess CO2 gas caused a suffocating sensation, supercritical CO2 would probably be a different world of discomfort. I'm not sure what kind of filter would keep supercritical CO2 out of your lungs, but you'd pretty much likely have to breathe in a completely airtight system.
Basically I think this whole scenario would be possible. It'd be super expensive, probably unhealthy at the very least, but definitely possible.
TheFerruccio
Very interesting. Supercritical CO2 would probably be unlike any else liquid we can dip our hands in in normal conditions. Sure, there are liquids with very low surface tension but the combination of supercritical CO2 properties would be special.
The feeling on our skin would probably be especially interesting. I'm thinking it could probably be somewhat simulated by trying to find a liquid of very low density we can put our hands safely in (that might actually be difficult), and have it somehow mix with much higher density liquids, then pass our hand through the interface and feel that non-instantaneous shift in fluid properties.
It would feel like when you put your hand in a stargate
This is so cool!! You actually see the point at which liquid CO2 can no longer be a liquid and see it happen before your eyes. But not like a liquid in a chamber whose pressure is decreased until it boils; then you just see it boiling away and maybe freezing. In this case, the critical temperature is reached and the temperature and pressure are still increasing. The liquid stops boiling because of the pressure and you kind of see it just reach the same density as the gas and it takes on an intermediate form right before your eyes!! I want a small chamber like that...one that's not going to explode and kill me.
Just to think supercritical fluids are deep within Jupiter's atmosphere. Super interesting world.
Why even look at Jupiter? Venus is nearly totally surrounded by this stuff at the surface
Its surface temperature is over 400 °C, pressure over 90 atmospheres, and the atmosphere is 96% CO2
@@purpleapple4052 venus is surrounded by supercritical fluids?
@@_apsis i assume it is since the temperature, pressure and composition all would be supercritical
Metallic hydrogen
So that's what it looks like.
Ah thank you. I’ve been trying to imagine what the in between layers of gas giants
could act like.
Because with all of the pressure from the gas above, and giant hydrogen oceans below i thought there couldn’t be a clear line between the two.
Though this probably isn’t exactly what it would look like without the same temperatures and density’s it gives me a vague sense of what it could be like.
Some of the best footage out there of this
Great examples of Critical Opalescence as it goes supercritical! I wish I had found this video last fall.
I want to become an alien just so i could feel supercritical fluids
Hi,
yes you can fill a container completely with liquid CO2, if the container is cooled during the filling process. If not the temperature will rise due to the Joules Thomsen effect.
The pressure would be (at 70F = 21°C) about 60 Bar.
To actually pass through the critical point, the vapor-liquid mensicus needs to stay in the middle of the vessel (equal volumes of the liquid and gas) at the moment that the two phases merge. If the meniscus drops, you are evaporating all the liquid before you hit the critical point, and your density is a bit low. Conversely, if you start with too much material in the vessel, then the liquid level rises and you pass by the critical point in the compressed liquid side of the phase diagram. Agitating the fluid in the vessel by rocking it works very well to show that the densities of the two phases approach each other as the fluid approaches the critical point.
I'd not say right at the middle of the vessel. The actual level at which heating up make it passes through critical point can be calculated based on the critical molar volume of the substance.
Four years later and I want to thank you for single handedly making me understand how to relate what I just saw and this graph. 😂
awesome. i love seeing that transition with the raining CO2.
2:30 looks amazing and rather scary. Imagine swimming in it!
I would rather not swim in it because it is insanely hot
@@thranse9964 30 degrees??
You'd fall through to the bottom lol it's still gas like, despite being liquid like
The turbidity is caused by small temperature differentials around the critical point where liquid is boiling then recondensing quickly. At equilibrium there would be no turbidity.
near the critical point, even in equilibrium, thermal fluctuations will be large and we'd see them as turbidity. Check out "critical opalescence"
Hi Flachzange. I've been reading about producing methane directly from reaction of hydrogen with supercritical CO2. If the gas in your container were hydrogen and the hydrogen and CO2 were in the correct proportions could you create that reaction safely in your container? I think the temperature has to be raised above 300degrees centigrade and some form of catalyst may be needed. The aim behind that idea on a large/world scale is: if you can create methane (natural gas we use in the home) synthetically from hydrogen (electolysis of water) and CO2 (captured from industrial processes) additional carbon is not added to the atmosphere by the ongoing continuous burning of the fossil fuel for energy. The electricity for the electrolysis is coming from a renewable energy source, solar, wind or hydro.
Industrial volumes of CO2 are 'cracked' off of hydrocarbons (natural gas in particular) coming out of the ground to begin with. You would be starting from high energy, going to liquid CO2, then back to high energy. The energy would have to come from somewhere. If you can find a good way to capture atmospheric CO2 and purify it then yes it would work.
It looks alot like 'clouds' in the sky, very cool
yes. You can see the pressure gage in my other video about this apparatus.
nice video of something I could not figure out!
That happens because with the temperature, the pressure rises. The liquid water lowers its density, the density of the gaseous water rises til the critical point where the density of both is the same.
this is what rocky core of uranus consists of! It has stone and ice, and its surrounded by layer of supercritical fluid. Who knows what swimming in those would feel like (if you have some special suit that would prevent you from getting crushed, that is :) )?
@mrjazzycharon2 Earth's atmospheric pressure is too low to support supercritical fluids at room temperature. For example, the supercritical point of water can be found in the deepest ocean trenches from undersea vents called 'smokers', at pressures that would crush any human being, at around 330C in temperature.
the pressure it's kept constant at about 73 atm for CO2, the temperature in this case is increased to reach that supercritical point, google 'phase diagram for CO2' it will make more sense to look at the graph.
one of techniques that I can propose - you my use high pressure pVT cell (or any container that can persist high pressures) - (1) - if you fill the cell with CO2 and have a second vent, air should go out of the cell (if the vent is at the top) because higher CO2 density. After that you have only CO2 in the cell.
if you can keep constant temperature, by increasing the pressure in the cell you can reach "vapor curve", i.e. dew point of CO2 (which at 70F is 58 bar).
I tried to imagine before what supercritical fluid in the interior of gas planets would look like, interesting to actually see it. I wonder what it would feel like to touch it? More like a fluid, or more like putting your hand in the wind?
It's not liquid, not vapour (gas) - it's something of the two at the same time. Fascinating
It's gaseous with the solubility of a liquid and the properties of common gasses
What happens if we increase the pressure of a supercritical fluid? Why doesn't it return to the liquid phase?
Thank you !
At higher pressures it will only return to the liquid phase if the temperature is below the critical temperature. Otherwise it will stay supercritical.
Flachzange1337 Thanks for the quick reply!
A great video and an awesome phenomenon!
It lacks certain qualities of a liquid. There is no surface tension, and no clear boundary between liquid-like and gas-like states of matter. The supercritical carbon dioxide looks like a roiling sea, except that a roiling sea is an interaction between wind and water very different in composition. With supercritical carbon dioxide the "sea" and the "wind" are the same substance.
en.wikipedia.org/wiki/Supercritical_fluid
supun gamlath you need to lower the pressure, or the temperature to turn supercritical to liquid
@@Flachzange1337 That happens because with the temperature, the pressure rises. The liquid water lowers its density, the density of the gaseous water rises til the critical point where the density of both is the same. now you see?
How nice of your vedeo! It helps me to understand the state of 'supercritical'. Can I ask you that where was this experiment conducted? At the school, Institute or somewhere..?
+MrJJunSang Because I want to use your video at my presentation in the school. And I want to identify the source, not only URL but also the place or organization.
+MrJJunSang
Hi, i made this experiment at home.
So the source is: Stephan Passon
I knew it! The Smoke Monster from Lost is a supercritical fluid!
I always knew it!
And some point it SEEMS to not get supercritical at all…..
im so confused, can you explain this, im just a 13 year old boy trying to figure how this transition happens
I'm a 19 year old boy trying to figure out how this transition happens.
With high conditions of température and pressure, matter become supercritical
th-cam.com/video/Bl36JCi_hMk/w-d-xo.html
At that moment CO2 will have vapour and liquid phase. You have to decrease volume until the pressure starts to increase again (that is the moment when the last bubble of gas turned to liquid). Or, in other words, the pressure in 2-phase states remains constant when you're changing only volume.
What is happening when it suddenly turns cloudy looking? Is that when the supercritical liquid is cooled to the point where it starts condensing into a liquid again?
I don't understand the message in the video that says when the chamber is filled with more co2 the fluid level increases with higher temperature. How does increasing temperature increase the amount of fluid??
+deadeyejac it's the other way around.
Raising the temperature doesn't add more liquid, it causes the fluid to expand. As the liquid phase is much denser than the gaseous phase it expands at a higher rate and compresses the vapor, so the level rises. On the other hand, in the beginning of the video the vapor is not yet saturated, so the liquid starts to evaporate, which decreases its level.
In reality both processes of expansion and evaporation occur simultaneously in all displayed cases, it is just a matter of which one would prevail over the other. I would assume that at a certain liquid/gas proportion the level would remain constant during heating until the critical point is reached.
I wonder what such a thing feels like to move through
Beautiful demonstration
2011 was a fucking decade ago. fuck me i feel old
I feel you. 5 years ago I was watching supercritical liquids being used in drycleaning, and laughing my ass off. In 2019 there's one machine using CO2 in Canada and in Amsterdam. I'm a drycleaner btw
What is the difference between supercritical and supercritical fluids? Because I was looking on the internet then I can't find the answer...
What would happen if we drank liquid CO2
Having the temp behind the gas doesn't help, and what about the pressure reading?
What happens with pressure when the gas is in supercritical phase and we continue to increase the temperature? Will the chamber blowup?
yes i have made this by myself. Maybe i am makeing a bigger one in the future but then to figure out how a electrical discharge behaves in liquid (and supercritical) gases.
Can you do the same but with the water?
Does anybody know where I can buy that small glas tubes filled with supercritical CO2 in europe of from europe?
Sending this in plane maybe could be problematic
local black market might sell them
Hello; I have been looking everywhere for answers to these I guess unusual questions. Please help if you can or send me to the person who can, if you know of somebody. 1. Assuming you have a container that can withstand the pressures, can you fill a container completely full of liquid co2? 2. If you can, what pressure would it exert at say 70 degrees F. Note: I be leave you probably can and the pressure would be whatever the vapor pressure Would be at that temperatur
very informative interesting video
im curious if there was only liquid co2 at the very bottom of the cylinder like a few ml and the rest existed as a gas and it was heated in the same way would it still reach super critical phase?
im thinking on a larger scale for instance 50 gallons with only 1 or 2 gallons liquid
At the supercritical point, CO2 stops being a fluid or vapor, and just becomes. It is existence.
Have you measured the experiment pressure?
Is there any supercritical fluid at room temperature and pressure? How does it feel to touch supercritical fluids?
sCO2 can be used for decaffeination/caffeine extraction/. See a general article on Wiki -en.wikipedia.org/wiki/Supercritical_carbon_dioxide#Solvent
Is the supercritical CO2 the opaque and cloudy stuff?
Under Jupiters harsh windy atmosphere lies this stuff, supercritical fluids and under that, a possibly solid core.
also venus
It's really really great video!
Our team make a video about thermodynamics now.
Could we use this video as references...?
It's really helpful to make viewers understand about thermodynamics...!!
Of course we will mark your name on our video.
Could you allow to use this video...?
What's the path on the phase diagram that this moves through?
+Evgeni Sergeev I would think that in a P-V diagram it would be a verticle line (with the X-axis being Volume).
As for the answer regarding the liquid level which some people have asked - why does the level of liquid rise on heating -
Imagine the Guassian-like dome (with the inside of the dome showing a mixture of liquid and vapor; the left side of the dome signifying liquid and the right side of the dome signifying vapour). THe initial ratio of the masses of liquid to vapour defines the dryness fraction (denoted as x). THe line inside the dome on which this lies is determied by the intiial pressure and temperature. From this initial location, as heat is added isochorically, we move up the line. If the initial point is to the left of the maxima of the dome, the final point is more towards the lower vapour fraction. That would mean that the liquid fraction increases and the level of liquid actually rises (Which is seen in the video). If the initial point x is on the right of the dome maxima, then the reverse happens - the final point x is on the higher vapour fraction and consequently the amount of liquid decreases.
When sufficiently heated, the final point may rise above the pressure at which the maxima of the dome occurs (which is the cricial pressure). Above this pressure, liquid and vapour coexist.
@@localhost123456 but isnt p/Temp be the right thing for a phase diagram? (Volume const)
@@CoolMusicsChannel Certainly. But on a P-T diagram you will then have to go along the isochore, which is not difficult to do in a P-V or infact a T-V diagram. Fundamentals still apply though
What is the equation of conditions of supercritical fluid?
Both pressure and temperature must be above the critical point.
Okay thank you , all my doubts cleared
Why does it become no longer transparent at some point?
A good question. I find that nearly all of the videos and explanations that cover the critical point and supercritical fluids out there tend to avoid or brush over the critical point itself and fail to explain in simple terms what is happening at the molecular level. I scrolled down many comments on many videos and didn't really see a single good question that addressed that, until I saw yours of course. Well I happen to have design experience with supercritical fluids, specifically as a working fluid for waste heat recovery, so I wanted to give you a brief explanation. At the critical point of a fluid, the molecules are being squeezed together to just the right distance from each other, such that they effectively all 'vibrate' in phase. It's a function of the Van Der Waals radii and the fluid in question (hence why different CP for different fluids) and one other interesting property at the critical point; the internal energy U is 0, because at the CP the molecules are vibrating in phase, therefore there are effectively no molecules acting against each other in simplistic terms. This is what causes many of the interesting properties, such as opacity. The in-phase vibration of the fluid at the critical point means light has a hard time passing through the fluid due to the much higher chance of interaction with molecules. Other effects include sudden asymptotic drop in the speed of sound through it, massive increase in specific heat capacity, and significant instability, by which I mean in a transient system where fluid flows, it is very hard to control and predict. In a nutshell, at the CP, the fluid acts like a macroscopic molecule.
I forgot to add; when the fluid passes through the critical point and becomes supercritical, internal energy increases and it falls out of phase, therefore transparency returns. Hope this helps!
@onetrickhorse Thanks for your informative explanation!
@@squirrel4727 You are very welcome. Keep asking questions! :)
Thank you for showing this to us.
How much pressure can you go with your device?
Amazing, so cool.. thanks :)
Why it becomes white?
Thanks, this question goes along with my last one, If you can fill the tank completely can you now change the entire liquid content in the tank to a gas by only raising/lowering Temperature or pressure? I am curious if it can Be done with a container being full (or if not, how full would it work) before the saturation level of the vapor would become so high that it would force the vapor to liquid form.
that thing was a gas, supercritical fluids do not exist at normal atmospheric pressures, the pressure in the container of this video is way above this pressure (about 73 times larger in the case of CO2).
So this is what it looks like when liquid turn into super saiyan.
Hi! very nice experiment! Did you make this device by yourself?
is liquid nitrogen an example of supercritical fluid? (I may be wrong)
no. thats an example of a liquid. from some quick searches nitrogen goes supercritical at −147°c and 34 bars.
what happen if you drink it
Venus is covered with stuff in this state
Can someone explain why the hell the fluid level increases instead of decreases when there is a greater amount of CO2 inside?
are you asking why the fluid level increases when CO2 is added?
In the first example the level of liquid CO2 decreases as the temperature increases. I'm wondering why in the second example when the chamber is filled with more liquid CO2 the fluid level increases (instead of decreasing) with higher temperature.
By adding more CO2 you bring the pressure up above the critical point. So instead of boiling, it expands to fill the vacuum. I think that once it fully fills the vacuum it’d be considered a super critical fluid.
Above critical pressure, it cannot boil. Above critical temperature it cannot condense. So this is what happens when it’s first brought above critical pressure then brought above critical temperature.
Our company is currently developing an instrument which can read the viscosity of supercritical fluids.
Замечательное видео 👍
That is real time or slow camera?
Supercritical fluid? Nah.
Gliquid.
you're probably think of the famous supler fluid video. What people forget is taht the liquid didn't actually pass through the ceramic bottom. It went up the side of the container.
how much energy is required to turn CO2 into supercritical fluid?
Not sure if this is the answer you’re looking for but at least 73atm and 31°C
Hmm I don't know, maybe this is why Jupiter has stripes because supercritical fluid layer behaves so strangely.
who receives credit for this footage?
I build this setup and made the video also by myself
As part of an institutional lab project or as a tinkering project at home?
At that time (6 years ago) it was just a home project.
At what temp and pressure point do you pass it through the POT
This is badass thanks for posting!
from hash oil to this?
？気体と液体の区別良くわかんね！ということは今は圧力が高いから液体と気体との比率が変わっているのかな？
液体、空いた空間、気圧はゼロ気圧か大気圧かは不明
液体と空間は温度？圧力？により気体が発生。
空間に液体の物質が気体に変わり空間に充満。
液体と気体は圧力？により気体に変わり続けているけど、もう、空間は無いから液体の空間を圧縮してると、境界がみえなくなる。
次に液体と気体が均等？(液体は逃げる為に気体は増え続けている)となると液体と気体が混合している？気体の空間が混合物に変化して満たしていく、混合は運動によって成り立っているから止まると元に戻る。
なのかな？良くわからん
カゲロウができるのは気体が濃く濃密な気体が空間を満たしているのは間違いないと思う？
液体が減っているのは気体に変わっているのと圧縮されているから？
気体と液体がまじって液体でも気体でも無い物質、液体でも気体でもある物質に満たされた。さらに続けると装置が破損するから？
じゃ液体でも気体でもあるし無い物質を作て何をしようとしてるのだろうね！
良く分からないから、憶測での発言
0:43 magic is real.
CO2 is an excellent refrigerant. But we need to apply good security practices.
I'm working on that now
is pressure constant the whole time?
No. When he says he adds Co2. That's a way of saying he's raising the pressure. The pressure would also increase as he increases the temperature. The only constant during this experiment is the volume of the chamber.
Does the pressure increase or decrease during this transition?
increase
big up a la sup 1 de janson
The final demonstration gives me anxiety.
The atmosphere of Venus...
Excellent video.
That’s amazing to see
1:36 is my favorite moment
OMG.. i need the pressure of it..
CO2 with an identity crisis
Studying for Chemistry finals, found this video...
well how is it going 3 years after :)
oh so thats y the water level is rising
There’s no water in it
Nice video!
Toluene
Well they are just doing a mosh pit.
This lecture th-cam.com/video/Bl36JCi_hMk/w-d-xo.html
mentions this video and explains it if you are interested.
Thx man for this video
thx for the video :)
reminds me of clouds
This may be the future of ThC extration as a standard. May be even for home boys
Интересный опыт.