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

Gay-Lussac's law states that for a given mass of gas at constant volume, the pressure of the gas is directly proportional to its absolute temperature (measured in Kelvin). This means that as the temperature of the gas increases, the kinetic energy of the gas molecules also increases, causing them to collide with the walls of their container more frequently and with greater force. This results in an increase in pressure.

When considering this relationship, it is important to note that the situation must involve a constant volume; otherwise, the results would differ. Therefore, under conditions where the volume is held constant, an increase in temperature leads to a direct increase in the pressure of the gas, illustrating the core principle of Gay-Lussac's law.