@@Shelby_itachi P=pressure V=volume n=number of gas molecules T=temperature(above absolute zero) R=a constant(depends on the units of all the other measurements, and the amount of gas) Once everything has been been determined, the equation remains true no matter what you do: E.g. double the temp and keep the volume constant, then the pressure will double. Or double the amount of gas at the same pressure and temp, then the volume will double. Etc.
@@Shelby_itachi for example I have P₁V = nRT₁ as eq 1 and P₂V=nRT₂ as eq 2 let V, n, R be const eq 1 divide eq 2 we can get P₁/T₁ = P₂/T₂ this is Gay-Lussac's law
People often question whether these things are ever applicable. At the refinery where I work, it is essential to operators, which are pretty well paying jobs in the area.
Why did the water get drawn into the bottle? I would think that the air would get hotter and expand causing pressure to build and prevent water from moving in. Or is the candle burning the oxygen and that is removing volume? If that’s the case wouldn’t the heat produced offset the change in volume?
Awesome question. Initially, things do get hotter with the burning candle. However, as oxygen is changed into carbon dioxide and water vapour, the candle slowly extinguished. Two things happen here, one is that the temperature drops and therefore the pressure as well. The other is that some of the water vapour condenses on the glass which reduces the pressure as well. Hope this helps.
Volume is inversely proportional to pressure because if it is inverse then it will be easier because as pressure increase the inversed volume will increase, but in reality it decrease
If cont volume is inversely proportional to the constant pressure.. does that mean change in internal energy is inversely proportional to the change in heat capacity..? (Bcoz delta H = Qp and delta U =Qv
History of the Ideal Gas Law
ua-cam.com/video/55pLYP8qpdM/v-deo.html
I just use PV=nRT and derive the rest if needed.
Great way to do it. Only need to remember one equation 👍
Yup, that's the way I learned it back in the day. 👍
can u elaborate more pls
@@Shelby_itachi P=pressure
V=volume
n=number of gas molecules
T=temperature(above absolute zero)
R=a constant(depends on the units of all the other measurements, and the amount of gas)
Once everything has been been determined, the equation remains true no matter what you do:
E.g. double the temp and keep the volume constant, then the pressure will double. Or double the amount of gas at the same pressure and temp, then the volume will double. Etc.
@@Shelby_itachi
for example I have
P₁V = nRT₁ as eq 1
and
P₂V=nRT₂ as eq 2
let V, n, R be const
eq 1 divide eq 2 we can get
P₁/T₁ = P₂/T₂ this is Gay-Lussac's law
Thank you so much, I’ve been struggling to learn this for a while 🙏
You’re welcome 😊
Damn. Understood this in a single watch, thank you!
You’re welcome 👍
Thanks for nice and quick short, good for a little recap
Glad you liked it!
Interested in a Sample Problem for the combined gas law? Find it here: ua-cam.com/video/kD22EQXClhc/v-deo.html
Thank you brother🦄
THANKS MY G
You’re welcome
Oh! Thank you so much sirr💖 i got it in one go😄
Great 👍
THANK you sir you explained them easily
You’re welcome 👍
I used IFCE tables including the initial, final, change, and effect to find them
People often question whether these things are ever applicable. At the refinery where I work, it is essential to operators, which are pretty well paying jobs in the area.
This is great information. Thank you for the comment.
I was half expecting the joke about cole
Why did the water get drawn into the bottle? I would think that the air would get hotter and expand causing pressure to build and prevent water from moving in. Or is the candle burning the oxygen and that is removing volume? If that’s the case wouldn’t the heat produced offset the change in volume?
Awesome question. Initially, things do get hotter with the burning candle. However, as oxygen is changed into carbon dioxide and water vapour, the candle slowly extinguished. Two things happen here, one is that the temperature drops and therefore the pressure as well. The other is that some of the water vapour condenses on the glass which reduces the pressure as well. Hope this helps.
@@PhysicsTeacherYT Interesting, thanks for clarifying👍🏻
Thank you so much sir ❤
You’re welcome 👍
Volume is inversely proportional to pressure because if it is inverse then it will be easier because as pressure increase the inversed volume will increase, but in reality it decrease
If cont volume is inversely proportional to the constant pressure.. does that mean change in internal energy is inversely proportional to the change in heat capacity..? (Bcoz delta H = Qp and delta U =Qv
Thank you 😅
You’re welcome 👍
ah just realized you are talking about gases only, cool infos to know
bro saved me 3 weeks
Glad I could help
Tq bro❤❤
Thank you 👍
PV= nRT is enough to remember
Yes. Definitely. Once you know the ideal gas law, you can use proportionalities to come up with the rest.
🎉
My father was sitting besidee me he also understood this concept
That’s awesome! I’m glad you could both enjoy my video.
How did the third experiment work?
super da
And then theres the vander waals gas equation. What a monstrosity.
Flashbacks of thermodynamics 😱
Didn't know about Fay Lussac's Law. TIL.
PV = nRT is the most important equation in engineering. If you forget this equation, get a different career.
Awesome. Is that for any engineering or is it most important for a specific engineering background?
@@PhysicsTeacherYT mechanical or
any engineering which has thermodynamics. Most of, if not all gaa calculations involve PC=nRT.
Gay lussac's law
Batter than 20 or 30 minutes lecture 😂😂😂
😒"laws"...all these are common sense
Agree
Why is it Gay - lussac 😂
Named after the French Chemist in the 19th century, Joseph Louis Gay-Lussac