If a gas is compressed to half its volume at constant temperature, what happens to its pressure?

When a gas is compressed to half its volume while keeping the temperature constant, its pressure actually doubles. This behavior is a consequence of Boyle's Law, which states that for a fixed amount of gas at constant temperature, the pressure of the gas is inversely proportional to its volume. Mathematically, this is expressed as ( P \propto \frac{1}{V} ) or ( P \times V = k ), where ( k ) is a constant.

In practical terms, if you reduce the volume of the gas to half, the pressure exerted by the gas increases because the same number of gas molecules occupies a smaller space, resulting in more frequent collisions with the walls of the container. Consequently, when the volume is halved, the pressure must double in order to maintain the relationship defined by Boyle's Law.

Thus, as the volume decreases, the pressure increases, leading to the conclusion that if the gas volume is cut in half, its pressure will indeed double.