Real vs Ideal Gases
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- Опубліковано 11 вер 2024
- Ideal gases don't really exist. But under Low Pressure and at High Temperatures many gases are close to ideal. That makes the Ideal Gas Law really usefully in many real world situations. Most of the gases in air are close to ideal at STP (except CO2).
Awesome visualization app: phet.colorado....
Here’s why:
1. For the ideal gas law we assume that molecules don’t take up any space. But they really do. This doesn’t matter as much at low pressure where they are spread out. We have mostly empty space. But increase the pressure, the volume occupied by molecules starts to matter.
2. For Ideal Gases we assume that molecules don’t attract or repel each other. This works well at higher temperatures. Molecules are moving fast so it’s more difficult to interact. But lower the temperature, now they can interact. Dipole-dipole, Van der Waals forces, or even hydrogen bonding.
So in short gases are ideal at lower pressures and higher temperatures.
The good news is we have equations to deal with the other situations, they are just a bit more complicated. For example, Van der Waals equation (en.wikipedia.o...) or
the Peng-Robinson Equation of State ( en.m.wikipedia...)
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shouldnt high temp make the pressure higher?
I'm focusing on Gas Laws. So this was helpful.😊👍
Glad it was helpful! This app is helpful to to visualize what happens when you change different variables:
phet.colorado.edu/en/simulations/gas-properties
I’ve seen this question so many times and I always get it wrong. Thanks Dr B I’m going to remember this now!
Excellent, it is a good one to remember!
Thank you! This was really helpful!
Glad it was helpful!
cool !!! really appreciate your efforts
Thanks a lot!
thank you!!
You're welcome!
What program it is
Here you go!
phet.colorado.edu/en/simulations/gas-properties
Why did the views go
This video is still pretty new but I expect it will start getting views next semester!