What happens to the pressure exerted by a given mass of gas if its absolute temperature is doubled while keeping its volume constant, according to Gay-Lussac's law?

💡 Solution & Explanation

Gay-Lussac's law states that the pressure of a fixed mass of gas at constant volume is directly proportional to its absolute temperature measured in Kelvin. Doubling the absolute temperature increases the average kinetic energy of the gas molecules proportionally, resulting in a doubling of the collision frequency and pressure exerted on the container walls. Pressure-temperature relationships form the foundational basis for constant-volume gas thermometers.