where Pt is the total pressure, PO2 is the partial pressure of oxygen, PN2 is the partial pressure of nitrogen, and Px is the partial pressure of the remaining gases in the mixture. This law explains why the partial pressures of component gases in a mixture change proportionately to changes in ambient pressure even though their absolute concentrations remain constant. This law is fundamental to the understanding of decompression sickness and other breathing gas-related problems.
Henry's law states that the amount of gas dissolved in a given volume of fluid is proportional to the pressure of the gas with which it is in equilibrium. The formula is
Cx = Px X solubility where CX is the concentration of gas dissolved in a liquid and P X is the partial pressure of gas X. This law explains why more inert gas (e.g., nitrogen) dissolves in the diver's body as ambient pressure is increased with descent and, conversely, is released from tissue with ascent.
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