Question

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.

Answer 1

Answer:

The ideal gas model assumes that gas particles experience no intermolecular attractions.

At low temperature, gas particles move slowly.

At high pressures, gas particles are very close together.

The closeness of the gas particles and their low speed allow intermolecular forces to become important at high pressure and low temperature.

The intermolecular forces cause the gas to deviate from ideal behavior.

Explanation:

Answer 2

Answer:

Ideal gas explains the property of gas that has no inter-molecular attractions irrespective of temperature and pressure.

Explanation:

• 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.