If the temperature of a gas decreases, what happens if the pressure remains constant?

When the temperature of a gas decreases while keeping the pressure constant, the gas occupies a smaller volume. This behavior can be explained by Charles's Law, which states that under constant pressure, the volume of a gas is directly proportional to its absolute temperature (measured in Kelvin). Mathematically, this is expressed as V/T = k, where V is the volume, T is the absolute temperature, and k is a constant.

Thus, if the temperature decreases, the volume must also decrease in order to maintain the relationship defined by Charles's Law. This means that as the temperature drops, the gas particles have less kinetic energy, causing them to move closer together, which results in a decrease in volume.