APII Study Guides

Respiratory Study Guide

Gas Laws


Dalton Law of Partial Pressure

The total pressure of a gas mixture is the sum of the pressures exerted by the independent gases.

(ie. Total Pressure = PO2 + P CO2)

(atmospheric pressure= 1 atmosphere = 760 mmHg)

The partial pressure is proportional to its percentage in the total gas mixture.

P is proportional to gas in mixture


Henry’s Law

When a mixture of gases is in contact with a liquid each gases will dissolve in the proportion to its partial pressure

It is also dependent on its solubility.

Both gases will move from an area of high concentration to an area of low concentration.


Bohr effect

Declining pH (increase acid) results in the increase of O2 unloading.


Haldane Effect

¯ (low) PO2 of blood, the more room for PCO2


­ (increasing) PCO2


Boyle's Law

Movement of air is based on:

change in volume a change in pressure a flow of gases