A chemist is studying the properties of a gas under various conditions. He observes that when the gas is at room temperature and low pressure, it behaves as an ideal gas. When the gas is cooled to 10 kelvin and is placed under high pressure, however, it deviates significantly from an ideal gas. Explain these observations.

Ideal gases assumes that the gases would experience no inter-molecular attraction and collision with other gases.
These gases are perfectly exhibiting elastic collision in nature.
The particle of gases moves slowly at lower temperature and the gases would become close when they exhibit high pressure.
The "closeness of the gas-particle" and "low-speed characteristics" are the important observations noted.
The inter-molecular forces deviate the property of gases from ideal gas behavior.

pstnonsonjoku pstnonsonjoku · Answer 2 · 2021-09-21T18:27:16+02:00

Gases obey the ideal gas law only at high temperature and low pressure. At low temperature and high pressure, gases deviate from ideal behavior.

According to the ideal gas law, the molecules of a gas do not experience any kind of inter-molecular association hence they remain far apart from each other.

This is only applicable at high temperature and low pressure. At high pressure and low temperature, inter-molecular interactions become significant and gases deviate from ideal behavior.

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