Explain the reasons why real gases deviate from ideal behavior.
Answers
Explanation:
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.
Answer:
Gases deviate from the ideal gas behaviour because their molecules have forces of attraction between them.
Kinetic theory can explain this.
1). The volume occupied by gas molecules is negligibly less as compared to the volume occupied by the specific 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 that gas.
2).The forces of attraction between gas molecules are negligible.
The second assumption is not valid when the pressure is high and temperature is low. But at high pressure or low temperature when the total volume of gas is miniscule, the forces of attraction become high and cannot be ignored.