The wavy footage is the result of the vibrating vacuum pump causing the camera to oscillate. Apparently the physics camera did not like filming chemistry...
I think you could say the most energetic particles leave first and those that remain are the coldest particles. They leave sequentially based on their energy but the thermoprobe only reads the remaining particles in the liquid state. If you could measure the average heat of the container the energy change would reduce in Temp too for two reasons the entropic cost of changing state but also the change in heat capacity (this is like the inverse of the heating cause by squeezing a gas, but rather stretching a gas whilst making the liquid become gas)
Spot on. I'm not sure how much the adiabatic (de)compression of gasses applies here but water (as seen) certainly does some strange things at various pressures. Thanks for the insights!
Transcript: Here's a twist on something you may have seen in school. This is a beaker of room temperature water. Now watch what happens when we put the water in a vacuum chamber and SUCK all the air out. See, as you lower the atmospheric pressure on water, the boiling point of water decreases, so what you're looking at is water that's boiling, not on a stove, but at room temperature. But here's the twist that probably got overlooked in school: look at what's happening to the temperature of the water. See, in order for liquid water to change state to a gas, it needs energy. On your stove, the water gets that energy from the burner, but here, there's no energy source, so watch the thermometer. See, the only energy in the water is the heat it already has, so what's happening is the water that's changing state is actually robbing energy from the liquid that's getting left behind. As a result, you see the reading on the thermometer plummet as water boils off, taking with it the energy that's referred to, as the heat of vaporization.
It is not actually "robbing" energy from the water to become vapor. What is really happening is higher energy molecules separating from lower energy molecules.
It's likely they know all about this but if they put boiling chips or boba drink spheres/OrbitZ drink neutral bouyancy spheres in an evaporative boiling fluid like an industrial steam maker can you make more process steam faster, cool a volume of wwater faster, have higher velocity water continuous addition, a cheaper smaller steam generator, and greater fiscal efficiency
water cooling from boiling from the latent heat of vaporization, I commented, “It's likely they know all about this but if they put more bubble nucleation sites like boiling chips or boba drink spheres/OrbitZ drink neutral bouyancy spheres in an evaporative boiling fluid like an industrial steam maker or a volatile oil distillation apparatus, or a boiling distillation petroleum industry catalytic cracker can you make more process steam faster, cool a volume of water faster, have higher velocity water continuous addition, a cheaper smaller steam generator.oil cracker, and greater fiscal efficiency
A LONG time. Most of it will cool, then freeze then sublimate. Rough untested-guess, somewhere on the order of the same amount of time it would take the entire beaker to evaporate if was just left out in a room.
@@INTEGRALPHYSICSGreat demo! My guess is that it would be substantially faster in vacuum than just letting it evaporate at room temperature and normal atmospheric pressure. I'm basing this guess on the existence of the process known as "freeze drying". If the vacuum didn't speed up the process, why would manufacturers pay for the vacuum pump and the electricity to run it?
No energy is being taken from other molecules at all. Just molecules existing in different energy ranges, unable to break the surface tension bond between them. What the thermometer is reading, is the average energy level, and producing a temperature based on that. When pressure drops, the higher energy molecules, are now finally able to break that surface tension, and leave the beaker as a gas. When higher energy molecules leave the beaker as a gas, the average energy level inside the beaker drops, which means the temperature drops as well.
@@INTEGRALPHYSICS I never said it couldn't freeze. Just that boiling liquids, is just higher energy particles leaving the system, thereby leaving behind lower energy particles. It's why if you want to boil water continuously, you need to constantly supply energy to the system, to keep the energy level in the system at boiling point. Water being a great distributor of heat, exists in an energy gradiant, with a mix of high energy particles, and low energy particles. In most cases, the surface tension of the water, is what prevents the high energy particles from flying out of the system. Increase the energy in the system, and those high energy particles will then have enough energy to break the surface tension, and escape, thereby producing the effect known as boiling. It's why steam is hotter than the boiling water, because only the high energy particles are capable of leaving the system. Similar effect occurs when you decrease the pressure of the surrounding area. Surface tension of the water decreases along with pressure, making it easier for high energy particles at room temperature to leave the system. Because only high energy particles leave, thereby leaving behind low energy particles, you get a noticeable decrease in temperature of the water, because despite being in contact with solid surfaces, that exist outside of the vaccuum, those solid sufraces are poor heat conductors, and therefore simulating a closed system (but it should be noted, that because of all the solid surfaces, it's not a perfect closed system. If you turn off the vaccuum pump, and leave it at a specific level of vaccuum, the water will boil away, until the surface tension is capable of preventing particles from leaving. And yes, this does mean, potential of it freezing, if the vaccuum is high enough to be on the precipice of freezing temperature. It should be noted, that in a perfect vaccuum, the boiling point, and freezing point are exactly the same, and as a result, we'll have a solid to gas transition, similar to that of dry ice. I forget what the term is for said transition.
I'm not disagreeing. There is a statistical distribution of molecular temperature, and the more energetic molecules are going to escape first... My point however, is that if you do the math, the 24-2500J/g of energy required to create a state change in the liquid water must come from somewhere. Energy exchange between water molecules serves to provide the necessary heat of vaporization from the finite thermal energy within the liquid. The terms I think you are looking for are 'sublimation' at or below the 'triple point'.
So nothing to do with being in or out of direct sunlight .... space suits have cooling systems as well as heaters .... you're not directly exposed to the vacuum (not unless something has gone badly wrong) so you're not subject to this effect.... the simple matter is there's no atmosphere to store heat so when you're in the shadow you get cold and when you're in sunlight you get hot. Example the hull of the ISS can reach 120⁰c on the sunny side and as low as -160⁰c on the shadow side (also when 'behind' Earth during its 45 min 'night')
@@izzabelladogalini I was definitely only talking about unprotected biological matter. You can still freeze cuz the water will take the heat away as quick as the water can boil in the vacuum. Once the frozen water sublime's, and you're completely desiccated, then it will matter if you're in the sun or shade.
@@izzabelladogalini once you're frozen solid though , I think you might be able to heat up above freezing point and still be a block of ice, as the water just sublime's, but you'll have to check that, I'm not a hundred percent sure of that detail.
@@izzabelladogalini other detail I forgot to mention is the reason why, it's called the triple point of water, in a vacuum water boils at the freezing point.
True, but I got so many comments that the water was 'degassing' and not boiling, that I wanted to show the energy loss to vaporization in order to address the 'degassing' theory.
The wavy footage is the result of the vibrating vacuum pump causing the camera to oscillate.
Apparently the physics camera did not like filming chemistry...
I think you could say the most energetic particles leave first and those that remain are the coldest particles. They leave sequentially based on their energy but the thermoprobe only reads the remaining particles in the liquid state.
If you could measure the average heat of the container the energy change would reduce in Temp too for two reasons the entropic cost of changing state but also the change in heat capacity (this is like the inverse of the heating cause by squeezing a gas, but rather stretching a gas whilst making the liquid become gas)
Spot on. I'm not sure how much the adiabatic (de)compression of gasses applies here but water (as seen) certainly does some strange things at various pressures. Thanks for the insights!
Transcript:
Here's a twist on something you may have seen in school. This is a beaker of room temperature water. Now watch what happens when we put the water in a vacuum chamber and SUCK all the air out. See, as you lower the atmospheric pressure on water, the boiling point of water decreases, so what you're looking at is water that's boiling, not on a stove, but at room temperature. But here's the twist that probably got overlooked in school: look at what's happening to the temperature of the water. See, in order for liquid water to change state to a gas, it needs energy. On your stove, the water gets that energy from the burner, but here, there's no energy source, so watch the thermometer. See, the only energy in the water is the heat it already has, so what's happening is the water that's changing state is actually robbing energy from the liquid that's getting left behind. As a result, you see the reading on the thermometer plummet as water boils off, taking with it the energy that's referred to, as the heat of vaporization.
physics man approves
@@physicsman-rf2np oh thank god Physics Man approves, we were all terrified
That’s really interesting. It’s also an insight into how heatpumps and refrigerants work.
Need more content like this I love it
It is not actually "robbing" energy from the water to become vapor. What is really happening is higher energy molecules separating from lower energy molecules.
To clarify, the word boil doesn't refer to temperature but the transition to vapor. So, boiling hot is not redundant.
Thank you, I understand now why during vacuum distillation the temperature goes down in my reactors
Interesting phenomenon.
This is how the refrigerators works.
Also: ln(p2/p1)=(-ΔHvap/R)(1/T2-1/T1)
Ah yes, the triple point 🤓
Keep this experiment going long enough and it will cool off that far...
So essentially it'll freeze eventually
these shorts are always super interesting
It's likely they know all about this but if they put boiling chips or boba drink spheres/OrbitZ drink neutral bouyancy spheres in an evaporative boiling fluid like an industrial steam maker can you make more process steam faster, cool a volume of wwater faster, have higher velocity water continuous addition, a cheaper smaller steam generator, and greater fiscal efficiency
water cooling from boiling from the latent heat of vaporization, I commented, “It's likely they know all about this but if they put more bubble nucleation sites like boiling chips or boba drink spheres/OrbitZ drink neutral bouyancy spheres in an evaporative boiling fluid like an industrial steam maker or a volatile oil distillation apparatus, or a boiling distillation petroleum industry catalytic cracker can you make more process steam faster, cool a volume of water faster, have higher velocity water continuous addition, a cheaper smaller steam generator.oil cracker, and greater fiscal efficiency
how much time would it take to evaporate that whole beaker if continued?
A LONG time. Most of it will cool, then freeze then sublimate. Rough untested-guess, somewhere on the order of the same amount of time it would take the entire beaker to evaporate if was just left out in a room.
@@INTEGRALPHYSICSGreat demo! My guess is that it would be substantially faster in vacuum than just letting it evaporate at room temperature and normal atmospheric pressure. I'm basing this guess on the existence of the process known as "freeze drying". If the vacuum didn't speed up the process, why would manufacturers pay for the vacuum pump and the electricity to run it?
No energy is being taken from other molecules at all. Just molecules existing in different energy ranges, unable to break the surface tension bond between them. What the thermometer is reading, is the average energy level, and producing a temperature based on that.
When pressure drops, the higher energy molecules, are now finally able to break that surface tension, and leave the beaker as a gas. When higher energy molecules leave the beaker as a gas, the average energy level inside the beaker drops, which means the temperature drops as well.
Let this run a while and the water will freeze despite a surprisingly small loss of volume to gas.
@@INTEGRALPHYSICS I never said it couldn't freeze. Just that boiling liquids, is just higher energy particles leaving the system, thereby leaving behind lower energy particles. It's why if you want to boil water continuously, you need to constantly supply energy to the system, to keep the energy level in the system at boiling point.
Water being a great distributor of heat, exists in an energy gradiant, with a mix of high energy particles, and low energy particles. In most cases, the surface tension of the water, is what prevents the high energy particles from flying out of the system.
Increase the energy in the system, and those high energy particles will then have enough energy to break the surface tension, and escape, thereby producing the effect known as boiling. It's why steam is hotter than the boiling water, because only the high energy particles are capable of leaving the system.
Similar effect occurs when you decrease the pressure of the surrounding area. Surface tension of the water decreases along with pressure, making it easier for high energy particles at room temperature to leave the system.
Because only high energy particles leave, thereby leaving behind low energy particles, you get a noticeable decrease in temperature of the water, because despite being in contact with solid surfaces, that exist outside of the vaccuum, those solid sufraces are poor heat conductors, and therefore simulating a closed system (but it should be noted, that because of all the solid surfaces, it's not a perfect closed system.
If you turn off the vaccuum pump, and leave it at a specific level of vaccuum, the water will boil away, until the surface tension is capable of preventing particles from leaving. And yes, this does mean, potential of it freezing, if the vaccuum is high enough to be on the precipice of freezing temperature. It should be noted, that in a perfect vaccuum, the boiling point, and freezing point are exactly the same, and as a result, we'll have a solid to gas transition, similar to that of dry ice. I forget what the term is for said transition.
I'm not disagreeing. There is a statistical distribution of molecular temperature, and the more energetic molecules are going to escape first... My point however, is that if you do the math, the 24-2500J/g of energy required to create a state change in the liquid water must come from somewhere. Energy exchange between water molecules serves to provide the necessary heat of vaporization from the finite thermal energy within the liquid.
The terms I think you are looking for are 'sublimation' at or below the 'triple point'.
This is why you freeze in space,
not like because it's cold or something, it's because it's empty space.
So nothing to do with being in or out of direct sunlight .... space suits have cooling systems as well as heaters .... you're not directly exposed to the vacuum (not unless something has gone badly wrong) so you're not subject to this effect.... the simple matter is there's no atmosphere to store heat so when you're in the shadow you get cold and when you're in sunlight you get hot.
Example the hull of the ISS can reach 120⁰c on the sunny side and as low as -160⁰c on the shadow side (also when 'behind' Earth during its 45 min 'night')
@@izzabelladogalini I was definitely only talking about unprotected biological matter. You can still freeze cuz the water will take the heat away as quick as the water can boil in the vacuum. Once the frozen water sublime's, and you're completely desiccated, then it will matter if you're in the sun or shade.
@@izzabelladogalini once you're frozen solid though , I think you might be able to heat up above freezing point and still be a block of ice, as the water just sublime's, but you'll have to check that, I'm not a hundred percent sure of that detail.
@@izzabelladogalini other detail I forgot to mention is the reason why, it's called the triple point of water, in a vacuum water boils at the freezing point.
@@petevenuti7355 I'm well aware of what a triple point is .... funnily enough I mentioned it only this morning commenting on another video
do you mean that the energy is used for latent heat of vaporization ..not that it takes latent heat with it?
Thermal energy is drawn from all of the water in order to vaporize a small portion of the water. Meaning the water that remains actually cools.
But is it actually BOILING? I think it's just VAPORIZING
Pure physics
Why does the boiling point decrease when the atmospheric pressure around the beaker decrease
Evaporation is a cooling process
This is why evaporating sweat cools your skin.
Can you brew coffee or tea this way??
Not effectively. It's just ice cold water.
isn't this kind of bad for the vacuum pump?
That vacuum pump sucks...
Why is it bad?
@@BariumCobaltNitrog3n I guess the vacuum pump is designed to pump air, not water vapor
U did this with ice
True, but I got so many comments that the water was 'degassing' and not boiling, that I wanted to show the energy loss to vaporization in order to address the 'degassing' theory.
@@INTEGRALPHYSICS Boiling is the result of water turning into gas and that does indeed take a lot of energy to phase change. Great work, subscribed!
PV=nRT let's goooo
The ideal gas law doesn't apply to vaporizing liquids. The substance needs to be far from the liquid state for the ideal gas to apply.
@@carultch bro thought he did something 🤣
TH-camr discovers high school physics😂
Wonder what happens to a person. Look up the one and only time they tried.
There's no suit that can put a person in a vacuum.