Why do gases deviate from their ideal gas behaviour?
Answers
Explanation:
Real gases deviate from ideal behaviour because their particles (atoms for inert gases or molecules) occupy some finite space and do exert interactive forces among them. ... In ideal behaviour, gas particles don't occupy space and do not have any interaction, as assumed in the kinetic theory of gases.
Explanation:
The volume occupied by gas molecules is negligibly small as compared to the volume occupied by the gas.
The first assumption is valid only at low pressures and high temperature, when the volume occupied by the gas molecules is negligible as compared to the total volume of the gas. But at low temperature or at high pressure, the molecules being in compressible the volumes of molecules are no more negligible as compared to the total volume of the gas.
The forces of attraction between gas molecules are negligible.
The second assumption is not valid when the pressure is high and temperature is low.
Gases deviate from the ideal gas behaviour because their molecules have forces of attraction between them. At high pressure the molecules of gases are very close to each other so the molecular interactions start operating and these molecules do not strike the walls of the container with full impact