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.
The partial pressure of SO4 in a bottle of NO2, CO2, and SO2, is 7.32 atm.
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.
1.6 ATM