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Which one of the following statements is true?

A. Some real gases have lower pressures than that calculated for the ideal gas because of attraction between molecules.

B. For a real gas, is always less than .

C. Some real gases have lower pressures than that calculated for the ideal gas because of the finite volume occupied by the molecules.

D. For a real gas, is always greater than .

E. Gases are likely to be more real and less ideal at high temperatures.

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Related questions

Which one of the following statements about the properties of gases is not correct?

A. At low temperatures, the attractive forces between molecules cause a real gas to deviate from ideal gas behavior.

B. At high pressures, the finite size of the molecules causes a real gas to deviate from ideal gas behavior.

C. The ratio PV/RT = 1 for one mole of an ideal gas.

D. The ratio PV/nRT < 1 because of repulsive interactions between the molecules.

E. The ratio PV/nRT > 1 because of the finite size of the molecules.

Which one of the following statements about the properties of gases is NOT correct?

a. At high pressures, the attractive forces between molecules cause a real gas to deviate from ideal gas behavior, and the van der Waals a factor adjusts for this.
b. At high pressures, the finite size of the molecules causes a real gas to deviate from ideal gas behavior, and the van der Waals b factor adjusts for this.
c. The ratio PV/RT = 1 for one mole of an ideal gas.
d. The ratio PV/nRT < 1 because of repulsive interactions between the molecules.
e. The ratio PV/nRT > 1 because of the finite size and repulsive force of the molecules.


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