What occurs to the gas pressure when a fixed mass of gas is compressed into a smaller volume at constant temperature?

When a fixed mass of gas is compressed into a smaller volume while maintaining a constant temperature, the pressure of the gas rises. This increase in pressure can be explained by considering the behavior of gas particles.

As the volume of the container decreases, the same number of gas particles occupies a smaller space. With the same amount of energy and a constant temperature, these particles are forced closer together. As a result, they collide with the walls of the container more frequently. According to the ideal gas law, which relates pressure, volume, and temperature, this leads to an increase in pressure.

The relationship between pressure and volume is described by Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume when temperature is held constant. Therefore, compressing the gas into a smaller volume directly results in an increase in the pressure experienced by the gas, since the gas particles are impacting the walls of the container more often within the confined space.