What happens to the pressure of a gas if its volume is halved while keeping the temperature constant?

When the volume of a gas is halved while keeping the temperature constant, the pressure of the gas will increase. This phenomenon is described by Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume at constant temperature.

According to Boyle's Law, if the volume decreases, the same number of gas molecules occupies a smaller space, resulting in more frequent collisions with the walls of the container. This increase in molecular collisions leads to an increase in pressure. Mathematically, this relationship can be expressed as P1V1 = P2V2, where P represents pressure and V represents volume. If the volume is reduced (halved, in this case), the pressure must increase to maintain the equality of the equation when temperature remains constant. Thus, halving the volume directly leads to a doubling of the pressure.