Boyle's Law describes the relationship between the pressure and volume of a gas — the pressure exerted by a gas held at a constant temperature varies inversely with the volume of the gas. For example, if the volume is halved, the pressure is doubled; and if the volume is doubled, the pressure is halved.
Pressure exerted by a given quantity of gas decreases when the gas is allowed to expand and occupy a larger area — reflects the pressure changes that occur with expansion and contraction of the chest cavity.
Stated as a formula:
P1/V1=P2/V2 (at constant temperature)
V1 = the original volume, V2 = new volume, P1 = original pressure, and P2 = new pressure.
If volume is halved, pressure is doubled;
and if volume is doubled, pressure is halved.
At a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid.
Solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
Example: Soft drinks — before the can of carbonated soda is opened, the gas above the drink is almost pure carbon dioxide at a pressure slightly higher than atmospheric pressure. The soda itself contains dissolved carbon dioxide. When the can is opened, some of this gas escapes, giving the hiss or "pop". Because the partial pressure of carbon dioxide above the liquid is now lower, some of the dissolved carbon dioxide comes out of solution as bubbles. If a glass of the drink is left in the open, the concentration of carbon dioxide in solution will come into equilibrium with the carbon dioxide in the air, and the drink will go "flat".
What you use Henry's Law for: to calculate the concentration of a gas in solution under pressure.
p is the partial pressure of the solute in the gas above the solution,
c is the concentration of the solute and
kH is a constant with the dimensions of pressure divided by concentration
The constant, known as the Henry's law constant,
depends on the solute, the solvent and the temperature.
The solubility of a gas in a liquid is directly proportional
to the partial pressure of the gas above the liquid.
The volume of a gas is directly proportional to its temperature.
Charles' Law (aka the law of volumes) is an experimental gas law which describes how gases tend to expand when heated, assuming that pressure remains constant, the volume and absolute temperature of a certain quantity of a gas are directly proportional.
Temperature = Constant x Volume or
Volume = Constant x Temperature or
Volume/Temperature = Constant
At constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its temperature on the absolute temperature scale (i.e. the gas expands as the temperature increases).
As absolute temperature increases,
volume of the gas also increases in proportion.
Dalton's — used to determine the individual pressures of each gas in a mixture of gases.
The pressure of a mixture of gases is equal to the sum of the pressures of all of the constituent gases alone.
Dalton's law (also called Dalton's law of partial pressures) states that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases.
PTotal is the total pressure of the atmosphere,
PGas is the pressure of the gas mixture in the atmosphere,
PH2O is the water pressure at that temperature
Pressure of a mixture of gases is equal to the sum
of pressures of all of the constituent gases.
3 Phases of Respiration
Muscles for Inhaling and Exhaling (Inspiration and Expiration)
The Respiratory Membrane
Four Gas Laws
Lung/Breathing Conditions & Illness