To properly absorb and understand the physiological processes involved in breathing, incorporating a simple, different physical laws governing the gas. This is a reminder level terminal S.

I – Ideal Gas Law
Gases are compressible, and expand at an elevated temperature. This law, called the ideal gas law, relates the pressure P, volume V and temperature T of a gas in the following formula:

PV = nRT where

  • n represents the number of molecules per gram of gas,
  • R is the gas constant
  • T is expressed in absolute temperature (T c 273 °)

Note that under physiological conditions “normal” correspond to 1 atmosphere is 760mmHg at 0 ° c

II – The law of partial pressures, or Dalton’s law
The gas pressure is the representation of the currency turmoil of gas molecules on the walls of its container. Each gas acts independently of others, so that the sum of partial pressures of each gas is the total pressure.

Note P total = P gas 1 gas 2 + P +…+ P gas n
Or more simply: P = ΣP Total partial

III – Act of Henry
Gas will tend to balance the pressure in the gaseous state and pressure as a dissolved in a liquid with which it is connected. This phenomenon allows the expulsion of carbon dioxide dissolved in blood at the end, the latter comprising a pressure wound greater than the ambient air.
The relationship is as follows:

V = (P/760) Qa

Where V is the volume of gas dissolved in ml, P the partial pressure of dissolved gas (mmHg), Q the volume of liquid in which gas is dissolved and the solubility coefficient of gas. (0.023 for oxygen, 0.49 for CO2, standard conditions (1 atmosphere, 37 ° C)).

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