state henry law and its application
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According to Henry’s law the solubility of gas in a liquid is directly proportional to the pressure of the gas
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
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
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important application
1. At high altitudes-the partial pressure of oxygen at high altitudes is less than the ground level.this results in low concentration of oxygen in the blood & tissues of the peoples
2. In scuba diving- during scuba diving,when the diver breaths in compressed air from the supply tank,more nitrogen dissolves in the blood & other body fluids because the pressure at that depth is far greater than the surface atmospheri
2. In scuba diving- during scuba diving,when the diver breaths in compressed air from the supply tank,more nitrogen dissolves in the blood & other body fluids because the pressure at that depth is far greater than the surface atmospheri
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Hey !!
Question = What is henry 's law and it's Application ?
Answer = It states that at a constant temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the Gas.
→ The most commonly used form of Henry's Law states that the partial pressure of a gas in vapour phase is proportional to the mole fraction of the gas (x) in the solution and is expressed as
P = Kh x
Here Kh is the Henry's constant and x is the mole fraction of the gas.
APPLICATIONS OF HENRY'S LAW
- To avoid the toxic effects of high concentration of nitrogen in the blood, the tanks used by scuba divers are filled with air diluted with helium (11.7% helium , 56.2% nitrogen and 32.1% oxygen)
- At high altitudes, low blood oxygen causes climbers to become weak and make them unable to think clearly, which are symptoms of a condition known as anoxia.
- To increase the solubility of CO₂ in soda water and soft drinks, the bottle is sealed under high pressure.
HOPE IT HELPS YOU !!
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