Exam 3 Review:  Chapter 22:  Gas Laws

partial pressure (of a gas) - The pressure, i.e., the force applied uniformly against a container's surface, that one component gas of a mixture of gases would exert if it were alone, i.e., occupied the same volume as the gas mixture, in a container and was at the same temperature.  See Dalton's Law.

Boyle's law - The principle that at a constant temperature the volume of a confined ideal gas varies inversely with its pressure.

Dalton's Law - The principle that the pressure, i.e., the force applied uniformly against a container's surface, exerted by a mixture of gases equals the sum of the partial pressures of the gases in the mixture; the pressure of a gas in a mixture equals the pressure it would exert if it occupied the same volume alone at the same temperature.

Henry's Law - The principle that when a mixture of gases comes into contact with a liquid, a gas will dissolve into the liquid in proportion to its partial pressure and its solubility coefficient, and will diffuse until equilibrium is achieved (gases diffuse into and out of liquids from high to low partial pressure).

List:

9. The gases, nitrogen (N₂), oxygen (O₂), and carbon dioxide (CO₂), in order from largest to smallest solubility coefficient, i.e., from most to least soluble in water.

10. The gases, nitrogen (N₂), oxygen (O₂), and carbon dioxide (CO₂), in order from largest to smallest partial pressure in the atmosphere.

Describe:

8.  The effects of atmospheric pressure on the partial pressures of the gases nitrogen (N₂), oxygen (O₂), and carbon dioxide (CO₂), at:
     (a) sea level, (b) at high altitudes, and (c) under water during deep diving.