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

Question

Quizplus · Accepted Answer

The ratio PV/nRT is equal to 1 for an ideal gas, but deviates from the ideal behavior for real gases. This deviation is caused by attractive and/or repulsive interactions between the gas molecules. At high pressures, the finite size of the molecules causes repulsive interactions that lead to a lower compressibility than predicted by the ideal gas law. The van der Waals b factor takes this effect into account. At low temperatures, attractive forces between the molecules lead to a higher compressibility than predicted by the ideal gas law, and the van der Waals a factor compensates for this. Therefore, statement D is incorrect because it claims that the ratio PV/nRT is less than 1 due to repulsive interactions, when in fact it is greater than 1 due to the finite size of the molecules.

Which One of the Following Statements About the Properties of Gases