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The respiratory system seems to have many Laws and Effects
and rules. Here they are, all in one place:
 | Boyles Law (p. 712):
 | P1V1 = P2V2 |
| This means that (if temperature is constant), if you
have an enclosed space and the volume changes, the pressure does, too, but
in a manner according to the original state. So if the thoracic cavity
has a certain volume and pressure, when you change the volume (for example,
increase it for inspiration), the pressure will change as well (in this
example, decrease) so that the V * P is constant. |
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| Dalton's Law (p. 718):
| This law simply says that if you add up all the
partial pressures of the components of a gas, they will sum to the total
pressure of the gas as a whole. It also defines partial pressure as a
component of the total pressure. |
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| Henry's Law (p. 719):
| This law says that each component of a gas will
diffuse into a liquid at a rate proportional to its partial pressure.
So the higher the pressure, the more of that gas that will enter the liquid. |
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| Bohr effect (p. 725):
| This says that oxygen unloading happens more readily
(where it is needed) when CO2 and hydrogen ion concentration is
higher. This does relate to the fact that Hb carries O2
better when it doesn't also have to carry CO2 or H+,
but that specific detail is part of the Haldane effect. |
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| Haldane effect (p. 726):
| This relates to the fact that Hb carries CO2
or H+ better when it isn't also carrying O2. It
also says the opposite (that Hb carries O2 better when it doesn't
also have to carry CO2 or H+). |
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| lung compliance (p. 715):
| The compliance, or stretchiness, of lung tissue
relates to how its total volume changes in relationship to the pressure
applied to change its volume. This should make sense because if a lot
of pressure is needed, the lung musn't be very stretchy. So, C =
ΔV / ΔP , where the P is actually the
transpulmonary pressure, measured as intra-alveolar pressure - intrapleural
pressure |
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