What happens to the volume of a gas when it is heated at constant pressure, according to Charles's Law?

According to Charles's Law, when the temperature of a gas is increased at constant pressure, the volume of the gas also increases. This law states that the volume of a given mass of gas is directly proportional to its absolute temperature (measured in Kelvin) when pressure is held constant. Mathematically, Charles's Law is expressed as V1/T1 = V2/T2, where V represents volume and T represents temperature.

As the temperature of the gas rises, the kinetic energy of the gas molecules increases, causing them to move more rapidly and collide with the walls of the container with greater force. This increased movement pushes the walls of the container outward (in the case of a flexible container) or results in an increase in the overall volume the gas occupies if the container's volume can change.

When reviewing the other options, it's evident that they do not align with the principles of gas behavior as described by Charles's Law. The decrease in volume, constancy of volume, or condensation into a liquid occurs under different conditions or scenarios and does not apply when the gas is heated at a constant pressure.