Gay lussac law example

Learn about Gay-Lussac's law, which states that the pressure and temperature of an ideal gas are directly proportional, under constant mass and volume.

gay-lussac formula

See examples of how this law applies to everyday situations and solve problems with formulas. Gay Lussac’s law is typically applied to ideal gases under controlled conditions. Here are some examples of Gas Lussac’s law in daily life: 1. Pressure Cooker. 2. Boiling Water: 3. Aerosol Cans. 4. Bullet Firing. 5. Water Heater.

6. Car Tire Pressure. 7. Balloons Expanding in the Sun. 8. Fire Extinguishers. 9. Basketball Inflation. Learn how pressure and temperature of a gas are proportional at constant volume and mass. See the formula, graph, and a solved problem involving a pressurized aerosol can. Learn how Gay Lussac’s Law of Thermodynamics relates pressure and temperature of a gas with constant volume.

See examples of pressure cooker, tyre bursting, fire extinguisher, aerosol spray and bullet working based on this law. Gay-Lussac's gas law is a special case of the ideal gas law where the volume of the gas is held constant. When the volume is held constant, the pressure exerted by a gas is directly proportional to the absolute temperature of the gas.

We assume a constant volume and a constant number of moles. Note: Gay-Lussac's Law uses kelvin for temperature units , while the pressure units can be any pressure unit mm Hg , atm , etc. For Gay-Lussac's Law, we need to have kelvin for temperature. But we are given celsius. So we must convert those numbers to kelvin! A scientist has a mL chamber with a fixed amount of carbon dioxide gas.

The scientist noted the pressure to be atm but forgot to write down the temperature in the chamber.

If the new pressure is atm, and the new temperature is 50K, what was the original temperature in the chamber? It is a law describing the properties of gases. It is also sometimes referred to as Amonton's law or the pressure-temperature law. The law states that:. An amount of gas in a closed container at a constant volume has a pressure that will vary proportionally to the absolute temperature.

Let's think about the gas molecules in a closed system. If the temperature increases, the molecules of gas will have more energy. They will move around more and expand. This causes an increase in pressure. If the temperature decreases, the molecules lose energy and are closer together. So, the pressure decrease. A great example of Gay-Lussac's law is the tires on your vehicle. If the tire has no punctures and a good seal, it is a closed container.

There is a specific amount of gas or mass of gas in that container. In the winter, the pressure in tires often drops due to cold temperatures. The amount of gas did not change, but as the temperature drops so does the pressure. The Gay-Lussac law has an intriguing history. It is named after the french physical chemist Joseph-Louis Gay-Lussac. But he was actually the first person to publish Charles' Law.

So, why did we call Charles' Law after Jacques Charles? It turns out Charles discovered his law but never published his work. Gay-Lussac found the unpublished work and credited Charles. Interestingly, at the same time, John Dalton had determined Charles Law on his own. So, what about the Gay-Lussac law? It had already been discovered over years earlier by Guillaume Amontons.

But, because of the technology at the time, Amontons could only work with air.