9.1 Pressure and Kinetic Molecular Theory of Gases
Properties of Gases
Gases have no definite shape or volume.
(Liquids have a definite volume but no definite shape. Solids have definite shape and volume.)
Pressure = Force / Area P = F / A SI Unit is the Pascal
1atm = 760torr = 760mmHg = 101,325Pa = 101.325kPa
| Kinetic Molecular Theory (Ideal Gas Theory) | |
|---|---|
| 1 | Gas atoms/molecules occupy negligible volume compared to the space between atoms/molecules. |
| 2 | Gas molecules don’t experience attractive or repulsive forces between one another. |
| 3 | All collisions are elastic (no loss of kinetic energy). |
| 4 | A gas is composed of a large number of atoms/molecules in random motion. |
| 5 | KEavg α T (KEavg = 3/2RT) |
| Ideal Behavior | 1. Gases behave more ideally at low Pressure and high Temperature. |
|---|
| 2. Gases with less Intermolecular Forces tend to behave more ideally. |