If the volume of a gas is halved during compression, what happens to its pressure?

When the volume of a gas is halved during compression, its pressure approximately doubles, according to Boyle’s Law. This law states that for a given amount of gas at a constant temperature, the pressure of the gas is inversely proportional to its volume. Therefore, if the volume decreases, the pressure must increase to maintain that balance.

In this scenario, halving the volume means that the gas particles are being forced closer together, which results in more frequent collisions with the walls of the container – this increase in collision frequency translates to an increase in pressure. Therefore, if the initial volume is reduced to half, the pressure will approximately double, demonstrating the direct relationship between volume and pressure in such situations.

Regarding the other options, they do not align with the principles outlined by Boyle's Law. For instance, the claim that the temperature remains constant does not apply unless it’s specified that the compression process occurs isothermally, which is not implied in the question. Similarly, the notion that mass is approximately doubled is inaccurate, as the mass of the gas remains constant regardless of changes in pressure or volume. Finally, the idea that pressure is approximately halved contradicts the fundamental inverse relationship established by Boyle's Law.