Page 1 of 1

Ideal vs Real Gas

Posted: Wed Jan 09, 2019 10:14 am
by Courtney McHargue 1I
What's the physical and chemical difference between ideal and real gases?

Re: Ideal vs Real Gas

Posted: Wed Jan 09, 2019 10:17 am
by Ashley Kim
Ideal gases and real gases have no physical/chemical differences!

Rather, ideal gases are theoretical (meaning they do NOT exist). They fit perfectly into the equation PV=nRT, meaning that their particles obtain a negligible volume and have no attractive forces. However, this is not true for real gases (which do exist). Gas particles obtain a small volume, and they have small attractive forces.

Re: Ideal vs Real Gas

Posted: Wed Jan 09, 2019 3:20 pm
by Christopher Anisi 2K
In addition, ideal gases are supposed to have elastic collisions with their respective molecules meaning that no energy is lost when they interact with one another! A real gas acts like an ideal gas during the conditions of high temperature and a low pressure.

Re: Ideal vs Real Gas

Posted: Wed Jan 09, 2019 4:06 pm
by Philipp_V_Dis1K
One could use the van der waals equation to see the difference between real and ideal gases.

Re: Ideal vs Real Gas

Posted: Wed Jan 09, 2019 10:23 pm
by haleyervin7
For purposes of calculation, do we always assume it is an ideal gas?

Re: Ideal vs Real Gas

Posted: Thu Jan 10, 2019 10:12 am
by lindsey_ammann_4E
haleyervin7 wrote:For purposes of calculation, do we always assume it is an ideal gas?

For the purposes of this class, we need to assume that a gas is an ideal gas in order to use the idea gas equation. If the problem requires calculations, it's safe to assume it's an ideal gas.

Re: Ideal vs Real Gas

Posted: Thu Jan 10, 2019 11:39 am
by Jonny Schindler 1A
The equation for the ideal gas law can be modified to correct for characteristics of a specific gas. It can incorporate the attraction between gas molecules as well as the volume of the gas molecules.