1. Gas Laws

2. Kinetic Theory (Gases)
1. Gas particles do not attract or repel each other
2. Gas particles are much smaller than the distances between them
3. Gas particles are in constant, random motion
4. No kinetic energy is lost when gas particles collide with each other or the walls of their container
5. All gases have the same average kinetic energy at a given temperature

3. Properties of Gases Based on ideal gases and kinetic theory
FLUID – capable of flowing
No definite shape or volume
* expand to fill container
* takes the shape of the container
Transmit and exert pressure in all directions

4. Ideal Gases
describe the behavior of gases under “ideal” condition according to kinetic theory
includes a 4th variable/factor affecting gases

5. Formula: PV = nRT
P = pressure in atmospheres V = volume in liters n = # of moles R = gas constant = L atm/mol K T = temperature in Kelvin (change ° C to K  + 273)

6. EX: A sample of 11.4 moles of dry ice (solid CO2) becomes gas at room temperature (25 °C). Calculate the volume of CO2 if pressure is 9.62 atm.

7. EX: Average lung capacity of humans is 4000 mL
EX: Average lung capacity of humans is 4000 mL. Assuming you breathe pure oxygen, how many moles of O2 gas can your lungs hold at 37°C (body temperature) and 827 mm pressure?

8. Molar Volume
Volume of gas in a mole
22.4 L/mol (conversion)
At STP

9. STP Standard temperature and pressure
Standard temperature: 0°C (aka 273 K)
Standard pressure: 1 atm