I love this!! Such a great visual for Charles' Law. Is that just a regular balloon you used? I thought that it would have cracked at such low temps! Thanks.
Paperclip Physics. First, thanks for the follow! Yes, this was just a regular balloon. I must admit that these balloons sometimes do pop if your warm them up too rapidly. As you would suspect, the balloon is very brittle at 77 K and will shatter if you drop it or strike it. We'll be adding a video soon demonstrating this loss of elasticity at very low temperatures.
Would you say that there is water underground? Would you also say that there is air underground? Is it cooler or hotter underground? If you are on the beach and it's mid summer and it's 2pm and the temperature is 102 degrees F, and your feet are burning on the sand... and you dig a hole and stand in it, is the hole where you stand, hotter or cooler? Do all things increase in volume in heat and contract in cold?
You sure can! You can see an example at ruclips.net/video/vRo9zNjN7tI/видео.html where I demonstrate the application of Charles' Law to crush cans (and even a 55 gallon steel drum) that have been filled with steam and are then rapidly cooled.
I didn't understood one thing, liquid nitrogen temperature is same as room temperature then why the volume of balloon decreased in liquid nitrogen and not in room temperature and balloon came in same form at the exact room temperature after taking it out from nitrogen. Explain Please i am preparing for test
Charles Law describes the relationship between the volume of a gas and its temperature. It states that the volume of a gas is proportional to its temperature. This means that when a gas is cold, it has a smaller volume thank when it is hot.
Great question! An ideal gas is a theoretical model that we use to help describe the behavior of gases. Generally, an 'ideal gas' is one that fits the behavior predicted by the Ideal Gas Law, PV=nRT Under the conditions that I carried out this demonstration, the gas does behave 'ideally' until its gets cold enough, and the gas particles slow down enough, to begin to have significant interparticle interactions and ultimately to become a liquid. So to answer your question: You get to see both kinds of behavior here, ideal gas behavior when the gas is warm in the expanded balloon, and real gas behavior as the volume decreases and the gas becomes a liquid.
Hello, I have a question because the gas decreased, so how is it still Charles Law as I thought the gas in Charles law is supposed to remain the same according to the Volume/ Temperature equation ? Please Respond Thank you have a good day
Charles Law says that the volume of a gas is directly proportional to its temperature. That is, the volume will increase as the temperature goes up and decrease as the temperature goes down. In this demonstration the gas whose properties we are observing is the air that is inside the balloon. At room temperature (about 22 degrees Celsius that day) the balloon was inflated to its maximum volume. When we cool the gas inside the balloon to -196 Celsius by immersing into the liquid nitrogen we saw the volume of the gas inside the balloon decrease (the balloon deflated). What is constant in the demonstration is the pressure and the moles of gas inside the balloon. Hope that answers your question and thanks for watching our video.
@@michaelducey8313 ohh okay I get it now I was really confused with Charles Law, but I understand now thank you for taking your time to answer my question take care
@@michaelducey8313 sir, i want to know that how the pressure is constant in here . i mean what is the part in here that we are sure here is it constant.i mean which pressure is constant? inside of balloon or outside of it.
@@reduanahmed3513 This is a great question! The pressure is constant outside the balloon and that pressure is that of the atmosphere (which doesn't change significantly over the few minutes it took me to record this demonstration).
@@MWSUChemistryDepartment To call this a demonstration of Charles' law is misleading -- the expected volume when chilling form 298 K to 77 K is 77/298 = 0.258 or 25.8% of the original volume. Clearly, the volume reduction as seen in the video is much greater than that, which is due to the fact the the air inside the balloon is being liquified and thus is not behaving like and ideal gas and therefore not an illustration of Charle's law. An alternative would be cooling the balloon to dry ice temperature, where the air inside the balloon would remain in a gaseous state - in this case the volume would be 194.7 K/298 K = 0.653 or 65.3% of the original volume -- not as dramatic a change, but an accurate illustration of Charle's law.
![I.N "HALLUCINATION" | [Stray Kids : SKZ-PLAYER]](http://i.ytimg.com/vi/n5B5q1Hwt_U/mqdefault.jpg)
It's good to see these classes in practice.
Our Chemistry teacher legit showed this in our class 💀
Excellent demonstration!
This was awesome to watch and really helped my homeschool students in understanding Charles’ law in practice -Thank You! :)
Appreciate your effort !! Keep doing more practical experiment ahead !
I never believed my teacher before seeing this video
Thankyou so much teacher❤❤
Best explanation ever of Charles law thankyou sir
Great information about Charles’s law!
hello there , concise , right to the point , awesome
Excellent video!
Thanks a lot, I've learned so much ☺️
I love this!! Such a great visual for Charles' Law. Is that just a regular balloon you used? I thought that it would have cracked at such low temps! Thanks.
Paperclip Physics. First, thanks for the follow! Yes, this was just a regular balloon. I must admit that these balloons sometimes do pop if your warm them up too rapidly. As you would suspect, the balloon is very brittle at 77 K and will shatter if you drop it or strike it. We'll be adding a video soon demonstrating this loss of elasticity at very low temperatures.
@@MWSUChemistryDepartment Hi @MWSU Chemistry Department, can anybody tell me where to get such a see-through dewar flask? Best regards from Germany!
Good job sir 👍👍
I LOVE THIS GUY! NOW I CAN DO ME HOMEWORK YAY!!!
cool
Yes very cool
I love this! 🔥
I love to see experiments its really very interesting
This was fun to watch 😂
Would you say that there is water underground? Would you also say that there is air underground? Is it cooler or hotter underground? If you are on the beach and it's mid summer and it's 2pm and the temperature is 102 degrees F, and your feet are burning on the sand... and you dig a hole and stand in it, is the hole where you stand, hotter or cooler? Do all things increase in volume in heat and contract in cold?
Amazing 👌
AMAZING
ME ]e wondering why did one of the balloon burst? Like how come its volume increase more than what it was initially (before putting it into nitrogen)?
❤❤
so wonderful
Love this video but did no one tell you yet that Charles's Law is Charles' Law?
It's very interesting it was so nice
We're glad you enjoyed it!
Thank you sir so much
Next time, put those balloons in a small, closed container together and let them duke it out for the real estate inside the container. 😈
Looks soooooo fun and helpful things
Awesome 👏,
Its funny...I now understand why people back then thought science was witchcraft🤣
Can we do this with water
You sure can! You can see an example at ruclips.net/video/vRo9zNjN7tI/видео.html where I demonstrate the application of Charles' Law to crush cans (and even a 55 gallon steel drum) that have been filled with steam and are then rapidly cooled.
How do you get liquid nitrogen?
I didn't understood one thing, liquid nitrogen temperature is same as room temperature then why the volume of balloon decreased in liquid nitrogen and not in room temperature and balloon came in same form at the exact room temperature after taking it out from nitrogen.
Explain Please i am preparing for test
The temperature of the liquid nitrogen is only 77 K while the temperature of the room is about 298 K. So the liquid nitrogen is much colder.
@@MWSUChemistryDepartment ohk Thanks❤️
This is super neat……but what is Charles law?
Charles Law describes the relationship between the volume of a gas and its temperature. It states that the volume of a gas is proportional to its temperature. This means that when a gas is cold, it has a smaller volume thank when it is hot.
Is it ideal gas or real gas what's the difference between them
Great question! An ideal gas is a theoretical model that we use to help describe the behavior of gases. Generally, an 'ideal gas' is one that fits the behavior predicted by the Ideal Gas Law, PV=nRT Under the conditions that I carried out this demonstration, the gas does behave 'ideally' until its gets cold enough, and the gas particles slow down enough, to begin to have significant interparticle interactions and ultimately to become a liquid. So to answer your question: You get to see both kinds of behavior here, ideal gas behavior when the gas is warm in the expanded balloon, and real gas behavior as the volume decreases and the gas becomes a liquid.
You look scared from the balloon HAHAHAA! I GET SCARED TOO!!
Is that cold water and hot water??
Cold nitrogen
Super
Hello, I have a question because the gas decreased, so how is it still Charles Law as I thought the gas in Charles law is supposed to remain the same according to the Volume/ Temperature equation ?
Please Respond
Thank you
have a good day
Charles Law says that the volume of a gas is directly proportional to its temperature. That is, the volume will increase as the temperature goes up and decrease as the temperature goes down. In this demonstration the gas whose properties we are observing is the air that is inside the balloon. At room temperature (about 22 degrees Celsius that day) the balloon was inflated to its maximum volume. When we cool the gas inside the balloon to -196 Celsius by immersing into the liquid nitrogen we saw the volume of the gas inside the balloon decrease (the balloon deflated). What is constant in the demonstration is the pressure and the moles of gas inside the balloon. Hope that answers your question and thanks for watching our video.
@@michaelducey8313 ohh okay I get it now I was really confused with Charles Law, but I understand now thank you for taking your time to answer my question take care
@@michaelducey8313 sir, i want to know that how the pressure is constant in here . i mean what is the part in here that we are sure here is it constant.i mean which pressure is constant? inside of balloon or outside of it.
@@reduanahmed3513 This is a great question! The pressure is constant outside the balloon and that pressure is that of the atmosphere (which doesn't change significantly over the few minutes it took me to record this demonstration).
@@MWSUChemistryDepartment To call this a demonstration of Charles' law is misleading -- the expected volume when chilling form 298 K to 77 K is 77/298 = 0.258 or 25.8% of the original volume. Clearly, the volume reduction as seen in the video is much greater than that, which is due to the fact the the air inside the balloon is being liquified and thus is not behaving like and ideal gas and therefore not an illustration of Charle's law. An alternative would be cooling the balloon to dry ice temperature, where the air inside the balloon would remain in a gaseous state - in this case the volume would be 194.7 K/298 K = 0.653 or 65.3% of the original volume -- not as dramatic a change, but an accurate illustration of Charle's law.
Hi @MWSU Chemistry Department, can anybody tell me where to get such a see-through dewar flask? Best regards from Germany!
❤
I love it, so ridiculous
He looks like Messi fr
No matter the scientific law. Theres always a Bollywood movie that could break it
So ridiculously
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