Question

How does Gay-Lussac’s Law explain the use of a pressure cooker?

Answer 1

Hint: Inside a pressure cooker the food that you need to cook sits in water. As the temperature of the fluid water is expanded, water fume (water in its gas state) is created. The air can't extend in light of the fact that the tires are basically a fixed-volume compartment, so the pressure increments – this is Gay-Lussac's Law!

Complete step by step answer:
Joseph Louis Gay-Lussac's was a French scientist and physicist who found in \[1802\] that in the event that you keep the volume of a gas consistent, (for example, in a shut holder), and you apply heat, the pressure of the gas will increment. This is on the grounds that the gases have more dynamic energy, making them hit the dividers of the holder with more force (bringing about more noteworthy pressure).
Inside a pressure cooker the food that you need to cook sits in water. As the temperature of the fluid water is expanded, water fume (water in its gas state) is delivered. This fume can't get away from the pressure cooker – which means the volume isn't evolving. The pressure of the water fume continues to ascend until the temperature of the water and the water fume surpass the ordinary limit of water (\[100{\text{ }}^\circ C\]). At this higher temperature food can be cooked a lot quicker. Extreme meat additionally comes out considerably more delicate subsequent to being cooked in a pressure cooker.
Gay-Lussac's law holds that at steady volume, \[P \propto T\]. At \[1{\text{ }}atm\] pressure we realize that the limit of water (the temperature at which the fume pressure of the water is equivalent to \[1{\text{ }}atm\]) is equivalent to \[100{\text{ }}^\circ C\]. On the off chance that we increment the surrounding pressure, the limit of the water should increment, and undoubtedly it does, so you can cook at temperatures \[ > 100{\text{ }}^\circ C\] and possibly lessen cooking time.
Gay-Lussac's law is a gas law which expresses that the pressure applied by a gas (of a given mass and kept at a steady volume) differs straightforwardly with the supreme temperature of the gas. At the end of the day, the pressure applied by a gas is corresponding to the temperature of the gas when the mass is fixed and the volume is consistent.

Note:
This law was detailed by the French scientist Joseph Gay-Lussac in the year\[1808\]. The numerical articulation of Gay-Lussac's law can be composed as follows:
\[P \propto T\]; \[\frac{P}{T} = {\text{ }}k\]
Where: \[P\] is the pressure applied by the gas, \[T\] is the outright temperature of the gas, \[k\] is a constant.