According to Gay-Lussac's Law, how does temperature affect gas pressure?

The correct assertion regarding the relationship between temperature and gas pressure, as described by Gay-Lussac's Law, is that pressure is directly proportional to temperature measured in Kelvin. This law states that, for a given amount of gas at constant volume, if the temperature of the gas increases, the pressure will also increase. This relationship is due to the kinetic molecular theory, which indicates that as the temperature of the gas rises, the average kinetic energy of the gas molecules increases, causing them to collide with the walls of the container more forcefully and more frequently, thus increasing the pressure.

In contrast, the notion that pressure is inversely proportional to temperature misrepresents the law, as an increase in temperature leads to an increase in pressure, not a decrease. The idea that pressure remains constant regardless of temperature overlooks the insights provided by Gay-Lussac's Law and disregards empirical observations related to gas behavior. Lastly, the assertion that temperature has no effect on gas pressure directly contradicts the fundamental principles of thermodynamics and gas behavior.