Which law explains the relationship between pressure and temperature at constant volume?

The law that explains the relationship between pressure and temperature at constant volume is Gay-Lussac's Law. This law states that for a given amount of gas at constant volume, the pressure of the gas is directly proportional to its absolute temperature. This means that as the temperature of the gas increases, the pressure also increases, provided the volume does not change.

The rationale behind this relationship lies in the kinetic theory of gases, which states that the temperature of a gas is a measure of the average kinetic energy of its particles. When the temperature rises, the particles move more vigorously, leading to an increase in pressure against the walls of the container, given that the volume is held constant.

In contrast, Dalton's Law pertains to the partial pressures of gases in a mixture, Charles' Law deals with the volume and temperature relationship at constant pressure, and Boyle's Law relates pressure and volume at a constant temperature. Each of these laws addresses different aspects of gas behavior under varying conditions, reinforcing that Gay-Lussac's Law is the appropriate choice for this specific relationship.