State henry's law and its applications.

Henry's Law

1. Henry's law states that the partial pressure of a gas in the vapour phase is proportional to a mole fraction of the gas in the solution.
2. The mathematical formula is: $\mathrm{P}={\mathrm{K}}_{\mathrm{H}}\mathrm{C}$ where C= concentration or mole fraction of dissolved gas, K_H= Henry's law constant and P= partial pressure of dissolved gas.
3. Applications:

• Henry's law in respiration: The main application of Henry's law in respiratory physiology is that gases will dissolve in the alveoli and bloodstream during gas exchange.
• The amount of oxygen that dissolves in the bloodstream is directly proportional to the partial pressure of oxygen in the alveoli air.
• Henry's law in carbonated soft drinks: (a) The carbonated drink is almost pure carbon dioxide at a pressure slightly higher than the atmospheric pressure.
• When the bottle is opened some of the gas escapes giving a specific pop, this is due to the lower pressure above the liquid and carbon dioxide comes out as bubbles.
• It is applied in deep-sea diving as well.

Therefore, Henry's law states the relationship between partial pressure and the concentration of gases.