Which statement is true according to Gay-Lussac's law?

The statement that pressure increases with increasing temperature aligns perfectly with Gay-Lussac's law. This law describes the direct relationship between the pressure and temperature of a gas when the volume is held constant. As the temperature of a gas rises, its molecules move faster and collide with the walls of the container more forcefully and frequently. This increased kinetic activity results in an increase in pressure.

For example, if you take a sealed container of gas and heat it, the temperature rises, and consequently, the pressure inside that container also rises due to the enhanced molecular motion. This principle is crucial in various applications, including understanding how pressure cookers operate and why it is essential not to overheat sealed containers.

In contrast, the other options do not accurately reflect the relationship outlined by Gay-Lussac's law. One suggests that volume decreases with pressure decreases, which relates to Boyle's law, while another states that volume remains constant regardless of temperature, which does not apply in this context either. Finally, stating that pressure has no relationship with temperature directly contradicts the fundamental premise of Gay-Lussac's law. Thus, the correct statement that pressure increases with increasing temperature accurately captures the essence of Gay-Lussac's findings.