What is partial pressure of a gas in the atmospheric air, lungs, or blood Differ
ID: 176279 • Letter: W
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According to Dalton's law of partial pressures states that the total pressure of a mixture of gases is the sum of the partial pressures of its components. each gas in a mixture of gases exerts its own pressure as if all the other gases were not present. The total pressure of the mixture is calculated by simply adding all the partial pressures.
• (air)Atmospheric pressure equal to PO2+ PCO2 + PN2(nitrogen)
The partial pressure exerted by each component in the mixture can be determined by multiplying the percentage of that gas in the mixture by the total pressure of the mixture.
For example, to find the partial pressure of oxygen in the atmosphere, multiplying the percentage of the atmospheric air composed of oxygen (in our air 21% is oxygen) by the total atmospheric pressure (760 mmhg) so 21%x 760 = 159mmhg:
For carbon dioxide (which represent in our air 0.03%. We take that multiply it by 760 and we get
0.3x 760= 0.3
for nitrogen 79%in the air x 760= 600
so we talking about partial pressure so if we were asked what is the partial pressure of oxygen in the air. It's 159
Thehe partial pressure of oxygen in the air is 159. But in the alveoli. It's 105 and in arterial blood is 100 mm HG.
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