According to Charles' Law, what relationship exists between gas volume and absolute temperature?

According to Charles' Law, the relationship between the volume of a gas and its absolute temperature is that the volume is directly proportional to the absolute temperature when the pressure is held constant. This means that as the absolute temperature of the gas increases, the volume also increases, provided that the pressure does not change.

This relationship can be succinctly represented in the equation V1/T1 = V2/T2, where V represents volume and T represents absolute temperature measured in Kelvin. Thus, if the temperature of a gas is increased, the gas molecules move more rapidly, leading to greater expansion and an increase in volume. This principle is fundamental in understanding how gases behave under different thermal conditions.

The other options do not accurately describe the relationship as outlined by Charles' Law. Specifically, discussing inverse proportionality or stating that temperature affects only pressure overlooks the established direct relationship between volume and temperature. Additionally, maintaining pressure while examining volume and temperature directly relates to the foundational principles of thermodynamics governing gas behavior.