Partial pressure of a gas applied to respiration is explained by Dalton's Law. It states that in every mixture of gas, each individual gas has its own pressure that makes up the total pressure of gas.
The pressure of each gas in a mixture is called the partial pressure of that gas.
Explain the partial and multiple correlation
If not present (and the intra-alveolar pressure equaled atmospheric pressure) the lungs would collapse.
The partial pressure is the pressure exerted by just one gas in the mixture.
The partial pressure is the pressure exerted by just one gas in the mixture.
The partial pressure is the pressure exerted by just one gas in the mixture.
The partial pressure is the pressure exerted by just one gas in the mixture.
As you create a partial vacuum in the top part of the straw, the weight of the entire atmosphere above the glass applies a pressure of 15 PSI on the liquid surface. This pressure pushes the liquid up the straw until the pressure in the straw returns to 15 PSI too. If you keep creating the partial vacuum the air pressure will push the liquid all the way to the top of the straw and out.
The partial pressure of SO4 in a bottle of NO2, CO2, and SO2, is 7.32 atm.
At a cellular level it is strictly diffusion by way of partial pressure differences. (With animals that's oxygen disappearing and CO2 appearing within the cell.)
The partial pressure is the pressure exerted by just one gas in the mixture.
The Partial Pressure of Oxygen in ambient air in Denver (610mmHg) is 128.1mmHg.