GayLussactörvény

GayLussac's Law, also known as the pressure-temperature law, describes the relationship between the pressure and temperature of a gas at constant volume. It states that for a fixed amount of gas, the pressure is directly proportional to its absolute temperature, provided the volume remains unchanged. This means that as the temperature of the gas increases, its pressure also increases proportionally, and conversely, as the temperature decreases, the pressure decreases.

Mathematically, GayLussac's Law can be expressed as P/T = k, where P is the pressure, T is the absolute temperature (in Kelvin), and k is a constant. This implies that if a gas undergoes a change in temperature from T1 to T2, its pressure will change from P1 to P2 such that P1/T1 = P2/T2.

This law is a specific case of the ideal gas law, which combines the relationships between pressure, volume, temperature, and the amount of gas. GayLussac's Law is particularly useful in understanding how gases behave in closed containers where the volume cannot change, such as in a sealed tank or a tire. It explains phenomena like why a tire pressure increases on a hot day or why a sealed aerosol can can explode if heated. The law is named after the French chemist Joseph Louis Gay-Lussac, who is credited with its discovery.