(a) List two experimental conditions under which gases deviate from ideal behavior. (b) List two reasons why the gases deviate from ideal behavior.

(1) High Pressure: Under high pressure, the volume occupied by the gas becomes comparable to the volume of the gas particles themselves. This causes the ideal gas law (PV=nRT) to give inaccurate predictions for the behavior of the gas. (2) Low Temperature: At low temperatures, intermolecular forces between gas particles become significant. These forces cause the gas particles to experience attractive or repulsive forces, which lead to deviations from the ideal gas law predictions.

(1) Intermolecular forces: The ideal gas law is based on the assumption that gas particles do not interact with each other. However, in reality, gas particles do experience attractive and repulsive forces (e.g., Van der Waals forces) that can affect their behavior and lead to deviations from the ideal gas law predictions. (2) Finite volume of gas particles: Another assumption of the ideal gas law is that gas particles have negligible volume compared to the volume of the container they occupy. However, under conditions such as high pressure or low temperature, the volume occupied by the gas particles can become significant compared to the container volume. This will also lead to deviations from the ideal gas law's predictions.