You do a very superb job at explaining several topics. You condense a lot of material in to quick video. How you vary you voice, hand movements, and the rate that you present make it easy to learn. This is probably one of the most enjoyable science tutorial I watched.
Hey Kyle, thank you for your question. A confusing one indeed. Although your reasoning makes sense, that is not what they mean. The volume of the container remains the same in both cases. In the ideal case, we assume that the molecules have no volume and so the volume of the container with those "volumeless" molecules is just V. However in the real case, the molecules do have volume and so the total volume is the volume of the container plus the volume of molecules, so we have V + V_molecules.
Therefore, Since V < V + V_molecules, we see that the volume in the real case is larger than the volume in the ideal case. Hope that helped! Sorry for the late response! Next time, post the question under the video on my website so that I can respond quicker!
do have volume. So the new volume of our system becomes (volume of container) + (volume of molecules) and since (volume of molecules) is no longer zero, that extra number will give us a larger overall volume.
Exactly. The book probably means that because the real gas molecules are attracted towards one another, they will pull each other closer and therefore decrease the overall volume.
I love you, may God bless your wonderfully brilliant mind. I'm blabbering stuff I know, it's just that I wanna say THANK YOU. I was in tears of frustration before this video and at the end I was really smiling.
thanx...initially i couldnt understand why the volume of real gasses is more than ideal gas but after you gave the example regarding the cup of water i understood it...once again thanx
No problem. Do you understand it now? I think the confusion lies in your understanding of what they mean by the volume of container. You're thinking that once you add the volume of gas, the volume of the container should technically decrease because you have less empty space. Although this is the case so to speak, this is not the case that they are considering. They are saying just simply take the volume of the container and add the volume of gas to get the real volume.
Imagine a cup of water filled completely to the edge of the cup.. If you place a few marbles (the molecules) into the cup, the cup will overflow. That is because the the additional volume of those marbles (the molecules) creates a larger overall volume of (water) + (marbles).
Great explanation! Totally understood it. Thanks to your videos, I've got a distinction in my exam. Keep up the good work. I bet the videos will help many other students like me :)
Sir, I just want to clarify one thing. You said on this video (2:34) that "I claim that the Kinetic Theory breaks down", which basically means that you've conducted so many experiments to prove that the theory really does break down on this certain conditions. Thanks
A claim is not a theory, which means it does not need any proof. However, for a claim to become a theory, you are absolutely correct, it needs proof in the form of experiments. :-)
Hey! Sure thing. An ideal gas has no volume due to the molecules. In other words, for any ideal gas, we make the assumption (which comes from the Kinetic Molecular Theory) that our molecules contain zero volume. So when we measure the volume of the container, we do not take the molecules into consideration.. Mathematically.. (volume of container) + (volume of molecules) = (volume of container) + 0 = volume of container. This is for an ideal condition. But for REAL gases, the molecules
Thanks for this lesson, But I have an question : it is about real gases mixture extends in old well , and how to find the pressure and the composition in the bottom?
I appreciate your video, but I just have a quick question. Is the "V" in the term "Preal + n^2a/V^2" (the ideal pressure term) referring to the real volume or the ideal volume? Thanks in advance.
standard conditions and standard temperature and pressure are 2 different things: standard conditions are 25 c and 1 atm but standard temperature and pressure (STP) are 0 c (273 k) and 1 atm.
You do a very superb job at explaining several topics. You condense a lot of material in to quick video.
How you vary you voice, hand movements, and the rate that you present make it easy to learn.
This is probably one of the most enjoyable science tutorial I watched.
Hey Kyle, thank you for your question. A confusing one indeed. Although your reasoning makes sense, that is not what they mean. The volume of the container remains the same in both cases. In the ideal case, we assume that the molecules have no volume and so the volume of the container with those "volumeless" molecules is just V. However in the real case, the molecules do have volume and so the total volume is the volume of the container plus the volume of molecules, so we have V + V_molecules.
Therefore, Since V < V + V_molecules, we see that the volume in the real case is larger than the volume in the ideal case. Hope that helped! Sorry for the late response! Next time, post the question under the video on my website so that I can respond quicker!
You went over this in the clearest way possible. Much appreciated.
do have volume. So the new volume of our system becomes (volume of container) + (volume of molecules) and since (volume of molecules) is no longer zero, that extra number will give us a larger overall volume.
Exactly. The book probably means that because the real gas molecules are attracted towards one another, they will pull each other closer and therefore decrease the overall volume.
I love you, may God bless your wonderfully brilliant mind. I'm blabbering stuff I know, it's just that I wanna say THANK YOU. I was in tears of frustration before this video and at the end I was really smiling.
Best explanation I found [and the last I will look for]. Thank you.
thanx...initially i couldnt understand why the volume of real gasses is more than ideal gas but after you gave the example regarding the cup of water i understood it...once again thanx
Let me know if that helps. If not, dont be shy! Maybe Ill put out another video explaining just that!
No problem. Do you understand it now? I think the confusion lies in your understanding of what they mean by the volume of container. You're thinking that once you add the volume of gas, the volume of the container should technically decrease because you have less empty space. Although this is the case so to speak, this is not the case that they are considering. They are saying just simply take the volume of the container and add the volume of gas to get the real volume.
Imagine a cup of water filled completely to the edge of the cup.. If you place a few marbles (the molecules) into the cup, the cup will overflow. That is because the the additional volume of those marbles (the molecules) creates a larger overall volume of (water) + (marbles).
Wow that's an ingenious way to imagine it
Great explanation! Totally understood it. Thanks to your videos, I've got a distinction in my exam. Keep up the good work. I bet the videos will help many other students like me :)
awesome is just not the word!!.....got all my concepts so clear!!! thnk u!
Yash Jain glad to hear it :)
You have explained well,thank you
Very impressive I understood every piece of it
Thank you very much, Sir....This lecture really helped me a lot :)
Sir, I just want to clarify one thing. You said on this video (2:34) that "I claim that the Kinetic Theory breaks down", which basically means that you've conducted so many experiments to prove that the theory really does break down on this certain conditions. Thanks
A claim is not a theory, which means it does not need any proof. However, for a claim to become a theory, you are absolutely correct, it needs proof in the form of experiments. :-)
Indeed Sir, I just wanted to clarify it though. Overall, you did a really great job there. Hope to see more. *Clap clap
Jovert Baniel Thank you :)
Thanks for watching
Awesome work...I have got it....iam a 11th grader.....thanks a lo!
Hello sir .. i really like ur video .. u taught very well thanx
Amazing explanation!! You helped me a lot!!
this was absolutely incredible, thank you
Thanks Bill!
hi..i dont understand how the volume of real gases is higher than volume of ideal. could you explain further?
Hey! Sure thing. An ideal gas has no volume due to the molecules. In other words, for any ideal gas, we make the assumption (which comes from the Kinetic Molecular Theory) that our molecules contain zero volume. So when we measure the volume of the container, we do not take the molecules into consideration.. Mathematically.. (volume of container) + (volume of molecules) = (volume of container) + 0 = volume of container. This is for an ideal condition. But for REAL gases, the molecules
Useful
Perfection!! Thanks dude.
Thank you brother .... Your are amazing .....you helped alot :)
this was really helpful! thank you :)
looking ahead for more useful videos :D
Thanks for the help!
man you're the best
This video was very helpfull you should upload more videos on other topics as well........
Way ahead of you! :)
Thanks for this lesson, But I have an question : it is about real gases mixture extends in old well , and how to find the pressure and the composition in the bottom?
perfect explanation!
l want to ask about an equation used to calculated the the amont of gas dissolved in its liquid. .and the gas is under 9bar pressure
I appreciate your video, but I just have a quick question. Is the "V" in the term "Preal + n^2a/V^2" (the ideal pressure term) referring to the real volume or the ideal volume? Thanks in advance.
is 0C considered high temp? Since most gases exhibit ideal behavior at high T and low P?
You are amazing thank you
really magnificent👏👏👏👏
How will the temperature remain constant when pressure is increased although there will be more collisions that will cause heat due to friction
sorry anyone know the names a and b please and what they relate to thanks
Fantastic !
thanks!
we wanna see more lectures not only in chemistry but also in maths and physics =)
I have 6x more lectures in physics than in chemistry ;)
thanks bro so helpful
whats the great teacher
nice explain
Very good
how can i drive the equation of real gases???
such a boss.
Mohammed Kamareddine :-)
thanks :)
thanks man
isn't 0 C and 1 atm considered "normal conditions"
i thought standard conditions was 25 C and 1 atm
standard conditions and standard temperature and pressure are 2 different things:
standard conditions are 25 c and 1 atm
but standard temperature and pressure (STP) are 0 c (273 k) and 1 atm.
I like your shirt.
Thankyou.
You're welcome!
Vreal < Videal
(Y)
Like it
my problem is solved..haha
👍🏻✌🏻️👌🏻😘
Perfection!! Thanks dude.
whats the great teacher