Ideal vs Real Gas
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Re: Ideal vs Real Gas
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.
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.
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Re: Ideal vs Real Gas
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.
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Re: Ideal vs Real Gas
One could use the van der waals equation to see the difference between real and ideal gases.
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Re: Ideal vs Real Gas
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.
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Re: Ideal vs Real Gas
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.
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