According to Boyle's Law, what happens to pressure in a closed system when temperature increases?

Boyle's Law specifically describes the relationship between the pressure and volume of a gas at constant temperature. However, it must be noted that the scenario presented requires an understanding of the gas laws that include temperature, particularly Charles's Law, which states that at constant volume, the pressure of a gas is directly proportional to its absolute temperature.

When temperature increases in a closed system, gas molecules gain kinetic energy, causing them to move more vigorously. As the temperature rises, if the volume of the container remains the same (which is typically the case in a closed system where the volume is fixed), the increased kinetic energy results in more frequent and forceful collisions of the gas molecules with the walls of the container. This leads to an increase in pressure.

Therefore, in a closed system where the temperature is increased, the correct response is that pressure increases, reflecting the direct relationship between temperature and pressure in gases.