10.2 Gas Laws Including the Ideal Gas Law
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Gas Laws
| GAS LAWS | |
|---|---|
| Boyle’s Law(constant n, T) | PV = constant or P1V1 = P2V2 or P ∝ 1/V |
| Charles’ Law(constant n, P) |  |
| Avogadro’s Law(constant T, P) |  |
| Combined Gas Law |  |
| Better Combined Gas Law |  |
| Ideal Gas Law |  |
Kinetic Molecular Theory (Ideal Gas Theory)
| Kinetic Molecular Theory (Ideal Gas Theory) | |
|---|---|
| 1 | Gas molecules have negligible volume. |
| 2 | Gas molecules don’t have any attractive forces between themselves. |
| 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 ∝ T (KEavg = 3 / 2 RT) |
| Ideal Behavior |
|---|
| 1. Gases behave more ideally at low Pressure and high Temperature. |
| 2. Gases with less Intermolecular Forces tend to behave more ideally. |
Ideal Gas Law
PV = nRT R =0.08206 L.atm/mol.K
What is the volume of 2 moles of argon gas behaving ideally at a temperature of 298K and a pressure of 2.0atm?
What is the volume of 80g of argon gas behaving ideally at a temperature of 25°C and a pressure of 1520torr?
RMS Speed
What is the root mean square speed of O2 gas molecules at 273K?
