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## Ignore words

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Low Temperature
Particles slow down at low temperatures. Low temp means more interactions with other molecules (chilling) making it non ideal
High Pressure
High pressures mean molecules are hitting a "smaller wall" so they are forced closer together = molecules interacting (can collide and the molecules won't travel in straight lines, not ideal)
Larger Molecules
The larger the molecules, the less ideal the gas will act (more unideal it will act). This can be related to volume. Given a certain volume container, larger particles take up more space, so there is less free space.
intermolecular attractions
the attraction of molecules to one another
Ideal Gases situations
Gases are more likely to be ideal in, very high temperatures, very large volumes/containers, low pressures, where they can move freely and not be attracted to each other
Ideal Gases Bad situations
Gases are more likely to be less ideal in, super low temperatures, small volumes, high pressure, where theres intermolecular interactions, limited free space (has to do with volumes)
a in real gas equation
Gases are more likely to be ideal at high pressures. "a" is the correction to the real gas to balance out the intermolecular interactions between the molecules. The stronger the molecular forces, the bigger "a" is
b in real gas equation
b has to do with particle size. If the particles are really big that means there is less free space in the container (volume). So if the particles are large, we must have bigger…
IMFs
From Strongest to weakest:
Density Formula
Density= (mw)(P)/(RT)
MW= grams(RT)/(P)
Molecular mass formula
effusion
A process by which gas particles pass through a tiny opening
Diffusion
Ability of gases to mix