What happens to gas volume when it is heated, assuming constant pressure?

When a gas is heated while maintaining constant pressure, its volume increases. This phenomenon is described by Charles's Law, which states that the volume of a gas is directly proportional to its absolute temperature when pressure is held constant.

As temperature rises, the kinetic energy of the gas molecules increases, causing them to move more vigorously. This increased motion forces the molecules to occupy a greater volume, resulting in expansion. Thus, if the initial volume of the gas is V1 at temperature T1, and it is heated to temperature T2, the final volume V2 can be expressed as V2 = V1 * (T2/T1), assuming the pressure remains constant.

In contrast, if the gas were to operate under conditions where pressure changes without constant pressure being maintained, other relationships involving pressure and volume would come into play, which leads to the other options not aligning with the behavior of gas under these specified conditions.