(a) List two experimental conditions under which gases deviate from ideal behavior. (b) List two reasons why the gases deviate from ideal behavior. (c) Explain how the function \(P V / R T\) can be used to show how gases behave nonideally.

Two experimental conditions that can lead to gases deviating from ideal behavior are: 1. Low Temperature: Gases tend to deviate from ideal behavior at low temperatures because the intermolecular forces between the gas particles become significant, resulting in nonideal behavior. 2. High Pressure: Gases also deviate from ideal behavior when subjected to high pressure. Under high pressure, the volume of the gas molecules becomes significant relative to the total volume of the gas, causing deviations from ideal gas behavior.

Two reasons why gases deviate from ideal behavior are: 1. Intermolecular forces: Ideal gas assumptions ignore the presence of any intermolecular forces between gas particles. However, in reality, gas particles have some weak intermolecular forces (such as Van der Waals forces) which make the gases deviate from ideal behavior. 2. Molecular size: Ideal gas assumptions consider gas particles as point masses with negligible volume. In reality, gas particles have a finite size, and at high pressure or low temperature conditions, the volume occupied by the gas particles becomes significant, causing deviations from the ideal gas behavior.

The function \(PV/RT\) is useful in understanding the non-ideal behavior of gases. For an ideal gas, the product of its pressure (P), volume (V), and the inverse of the gas constant (R) and absolute temperature (T) should equal 1, i.e., \(PV/RT = 1\). However, under certain conditions, gases do not follow the ideal gas equation, and the value of \(PV/RT\) differs from 1. A value of \(PV/RT\) greater than 1 indicates a positive deviation from ideal behavior. This implies that the repulsive forces between the gas particles are dominating and causing the gas to occupy a larger volume than predicted by the ideal gas equation. A value of \(PV/RT\) less than 1 indicates a negative deviation from ideal behavior. This implies that the attractive forces between gas particles are significant, causing the gas to be compressed to a smaller volume than predicted by the ideal gas equation. By comparing the value of the \(PV/RT\) function with 1, it is possible to deduce and analyze the non-ideal behavior of gases.