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Difficulty: MediumDeviations of Real Gases from Ideal Gas Behavior

Under conditions of high pressure and low temperature, real gases exert a lower measured pressure than predicted by the ideal gas equation primarily because intermolecular attractive forces reduce the impact force of gas molecules hitting the container walls.

Answer: Answer

Answer

The statement is True.
The statement accurately describes why real gas pressure is lower than ideal gas pressure under high pressure and low temperature conditions: attractive forces between molecules diminish collision forces with the container walls.

Step-by-Step Solution

1
Identify the assumptions of ideal gas behavior regarding intermolecular forces.
The ideal gas model assumes there are no attractive or repulsive forces between gas molecules.
Kinetic molecular theory treats ideal gas particles as non-interacting point masses.
2
Analyze how real gas conditions (high pressure, low temperature) affect molecular interactions.
Molecules come close together at high pressure and move slower at low temperature, allowing intermolecular attractions to become significant.
Slower-moving, closely spaced particles experience significant van der Waals attractive forces.
3
Determine the impact of attractive forces on measured gas pressure.
Molecules approaching the wall are pulled backward by neighboring molecules, reducing wall collision force.
Reduced wall impact force directly decreases observed pressure below the calculated ideal value.

Key Concept

Intermolecular attraction causing pressure deviation in real gases
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Topics

Deviations of Real Gases from Ideal Gas Behavior

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