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In the van der Waals equation, what does the term (a)/(V²) signify?

1. The pressure exerted by the gas and (V - nb) the volume occupied by the gas. At low pressures, when the gas occupies a large volume, the intermolecular distances are significant, leading to negligible intermolecular forces, and the gas behaves ideally. Hence, this explanation is valid.
2. At high pressures, the intermolecular distances decrease, causing intermolecular forces to have a notable effect, resulting in deviations from ideal gas behavior. Therefore, this explanation is invalid.
3. The constants a and b, known as van der Waals coefficients, depend on the type of gas and are unaffected by temperature, making this statement accurate.
4. The pressure P + (a)/(V²) is not less than P, so this explanation is incorrect.

Correct answer: The constants a and b, known as van der Waals coefficients, depend on the type of gas and are unaffected by temperature, making this statement accurate.

Solution

The term ( rac{a}{V²}) in the van der Waals equation signifies the pressure exerted by the gas due to intermolecular forces, which becomes significant at high pressures and low volumes, causing deviations from ideal gas behavior.

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