State Henry’s law correlating the pressure of a gas and its solubility in a solvent and mention two applications for the law.

Henry's law is one of the gas laws formulated by William Henry in 1803. It states: "At a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid.

Importance of this Law :-
(1) In Packing of soda cans :- To increase the solubility of CO2 gas in soda water , bottles of soda water is always packed under higher pressure.
(2) In Deep see diving: - As nitrogen is a more soluble gas in our blood and at deep see pressure increase so its solubility also increases, when scuba diver tries to come rapidly toward the surface of water, pressure decreased and Dissolved N2 gas comes back from the blood and make bubbles in his veins. It because bends .To avoid bends diver use oxygen diluted with helium because helium is less soluble in blood.

Importance of this Law :-
(1) In Packing of soda cans :- To increase the solubility of CO2 gas in soda water , bottles of soda water is always packed under higher pressure.
(2) In Deep see diving: - As nitrogen is a more soluble gas in our blood and at deep see pressure increase so its solubility also increases, when scuba diver tries to come rapidly toward the surface of water, pressure decreased and Dissolved N2 gas comes back from the blood and make bubbles in his veins. It because bends .To avoid bends diver use oxygen diluted with helium because helium is less soluble in blood.