The solubility of a gas in a liquid is directly proportional to its pressure, according to Henry’s law.
X=Kh*P, here X is mole fraction of a gas, Kh denotes henry’s law constant and P is partial pressure of the gas.
Important applications are as follows:
a) In the packaging of soda cans: To maximise the solubility of CO2 gas, soda water bottles are constantly packed at higher pressure.
b) Nitrogen is more soluble in our blood than Helium in deep-sea diving. The pressure in the deep sea is higher than at the water’s surface. When a diver tries to rapidly approach the water’s surface, pressure drops, and dissolved nitrogen returns to the blood, causing bubbles in veins. As a result, divers breathe oxygen mixed with helium.
According to Henry’s law, the solubility of a gas in a liquid is directly proportional to its pressure. Important applications are In the packaging of soda cans and in deep sea diving.
