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12 Cards in this Set
- Front
- Back
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Partial Pressure
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The pressure contributed by each gas in the atmosphere
All partial pressures together add up to 760 mm Hg |
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Normal Partial Pressures
In pulmonary vein plasma |
PCO2 = 40 mm Hg
PO2 = 100 mm Hg PN2 = 573 mm Hg |
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The Gas Laws
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Diffusion occurs in response to concentration gradients
Rate of diffusion depends on physical principles, or gas law. |
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Dalton’s Law and Partial Pressures
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Atmospheric pressure (760 mm Hg)
Produced by air molecules bumping into each other Each gas contributes to the total pressure In proportion to its number of molecules (Dalton’s law) |
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Dalton’s Law:
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Total pressure of a gas mixture is = to the sum of the pressures that each gas in the mixture would exert independently.
Partial pressure: The pressure that an particular gas exerts independently. PATM = PN2 + P02 + PC02 + PH20= 760 mm Hg. |
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Henry’s Law
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When gas under pressure comes in contact with liquid
Gas dissolves in liquid until equilibrium is reached At a given temperature Amount of a gas in solution is proportional to partial pressure of that gas |
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tidal volume
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the volume of gas inspired or expired in unforced respiratory cycle
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lung capacity
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measurements of the sum of two or more long volumes
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total lung capacity
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total amount of gas in the lungs after a maximum inspiration
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vital capacity
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maximum amount of gas that can be expired after a maximum inspiration
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anatomic dead space
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volume of air remaining in conducting passages
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diffusion
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the net transport of molecules from an area of higher concentration to an area of lower concentration
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