Gas Laws Quiz: Boyle's and Dalton's Law

Study Notes

Describes the relationship between the pressure and volume of a gas
At a constant temperature, pressure of a gas varies inversely with its volume
Gases always fill their container, therefore in a large container, the molecules of a gas will be far apart and the pressure will be low
If the volume of the container is reduced, the gas molecules will be forced closer together and the pressure will rise

States that the total pressure exerted by a mixture of gases is the sum of the pressures exerted independently by each gas in the mixture
Each gas in a mixture exerts a pressure called its partial pressure, which is proportional to the percentage of that gas in the gas mixture
Nitrogen (N2) makes up 79% of air and has a partial pressure of 597 mm Hg
Oxygen (O2) makes up 21% of air and has a partial pressure of 159 mm Hg
At high altitudes, partial pressures decline in direct proportion to the decrease in atmospheric pressure

States that when a gas is in contact with a liquid, the gas will dissolve in the liquid in proportion to its partial pressure
The greater the concentration of a particular gas in the gas phase, the more and the faster that gas will go into solution in the liquid
This principle is applied in gas exchange in the lungs and tissues
The direction and amount of gas movement is determined by its partial pressure in the two phases
The solubility of the gas and the temperature of the liquid also influence the amount of gas that will dissolve in a liquid
CO2 is most soluble in liquids
O2 is 1/20 as soluble as CO2
N2 is only half as soluble as O2
When a liquid's temperature rises, gas solubility decreases
Example: Soda drinks, the CO2 gas will slowly go flat if left in the fridge, but very quickly go flat if left at room temperature.