1. The Behavior of Gases

2. Factors Affecting Gas Pressure
Amount of Gas – Adding gas increases gas particles, increases collisions, and therefore increases pressure
Volume – Decreasing the volume of the container increases the number of collisions and raises the pressure
Temperature – Raising the temperature of a gas causes the particles to move faster and run into each other more often

3. Boyle’s Law Pressure-Volume Relationship
For a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure
Decrease volume/Increase pressure
Increase volume/Decrease pressure
P1 V1 = P2 V2

5. Charles’s Law Temperature-Volume Relationship
The volume of a mixed mass of a gas is directly proportional to its Kelvin temperature if the pressure is kept constant
Increase temperature/Increase volume
Decrease temperature/Decrease volume
V1 V2
T1 T2 =

7. Gay-Lussac’s Temperature-Pressure Relationship
Pressure of a gas is directly proportional to the Kelvin temperature if the volume remains constant
P1 P2
T1 T2 =

9. Combined Gas Law Single expression that combines the three gas laws
P1 V1 P2 V2
T T2 =

10. Ideal Gas Law R or P V = nRT
Equation that expresses how much gas is in a system
Moles of gas (n)
Ideal gas constant (R) = 8.31
P V
T n R =
or P V = nRT

11. Partial Pressure of Gas
At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressure of the component of gas
Ptotal = P1 + P2 + P3 + ………..

13. Graham’s Law
Diffusion – the tendency of molecules to move toward areas of lower concentration
Effusion – the process in which gas escapes through a tiny hole in its container
Graham’s Law – the rate of effusion of a gas is inversely proportional to the square root of the gas’s molar mass
RateA Molar massB
RateB Molar massA =