## Ideal vs real gases

$PV=nRT$

Funmi Baruwa
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### Ideal vs real gases

How do you know if the gas is ideal or if it’s real?

Nick Pascua 2L
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### Re: Ideal vs real gases

For a gas to be considered ideal, it would have to have negligible volume (which can't really be present in real life since all gases possess some sort of volume within a system), the particles would have to be move randomly and have to be equally sized with no form of intermolecular forces between other particles, and would have to have elastic collisions without a transfer of energy.

With that being said, we use the ideal gas law for accurate calculations and theoretical information whereas real gases we can't assume that they will be consistent in all environmental scenarios.

Colin Juett 2F
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### Re: Ideal vs real gases

Ideal gases do not actually exist, they are just when we treat the real gases as if they had no intermolecular interactions. In lecture today, Dr. Lavelle said we will treat all gases as if they were ideal.

Kaitlyn Hernandez 3I
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### Re: Ideal vs real gases

Ideal gases are exactly that: they're ideal and theoretical and they follow all of the gas laws regardless of the conditions they're in. I believe that the ideal gas law really helps us with calculations about properties and behaviors of gases.

Kiran Marla
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### Re: Ideal vs real gases

As other people mentioned, all gases will be treated as ideal. This is because this allows us to use the equation PV=nRT in order to change between pressure and concentration, which helps find equilibrium concentrations and make conclusions about a chemical reaction.

Posts: 90
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### Re: Ideal vs real gases

I think in this class Lavelle said that we will assume that all gases are ideal gases so we can use the equation but this may not be the case in future classes :)

Janelle Gokim 3B
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### Re: Ideal vs real gases

In lecture, Dr. Lavelle mentioned that an ideal gas wouldn't be able condense into a liquid state and would instead remain in it's gaseous form. This doesn't necessarily apply to the gases we are working with, in fact, most of the time it is possible for those intermolecular forces to develop among the molecules, however, we treat all of them as if they are ideal so we can make use of the ideal gas law, PV=nRT.

KhanTran3K
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### Re: Ideal vs real gases

Ideal gases have a set of rules that are not likely to occur in real life. This includes the fact that all atoms and molecules in the gas are not interacting with each other, and are moving randomly. With this, in comparison to real gases, ideal gases are used in calculations such as with the ideal gas law, PV=nRT. Hope this helps!

SavannahScriven_1F
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### Re: Ideal vs real gases

When we consider a real gas to be ideal, we assume it does not condense into a liquid when the temperature is reduced. In other words, we ignore the attractive forces between the gas molecules (intermolecular forces).

Mackenzie Stockton 2H
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### Re: Ideal vs real gases

I believe in lecture Dr. Lavelle said that an ideal gas is defined as a gas that does not undergo a phase change to a liquid when it is cooled. I believe that for this class, we assume all gases (assuming that they are a gas for a specific T and not a liquid that was cooled) are ideal and we can use PV=nRT for any gas. Most gases are not ideal and condense into a liquid, but for this class we just treat them as ideal.

Sheryl Ocampo 1D
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### Re: Ideal vs real gases

I don't think ideal gases actually exist, but for the purposes of our class we just treat gases as if they were ideal

Inderpal Singh 2L
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### Re: Ideal vs real gases

Dr. Lavelle said that for this class we should assume that the gases given are ideal :) in reality, I don't think there are many ideal gases.

Kaleb Tuliau 3E
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Joined: Tue Nov 05, 2019 12:18 am

### Re: Ideal vs real gases

I believe in professor Lavelle's class we want to assume that all gases are ideal gases. Unless told otherwise :)