| Law | Formula | Meaning | Example |
| Boyle's law | PV=k or P1V1=P2V2 | Pressure is inversely related to volume. | Pressure goes up, volume goes down- and vice versa! |
| Charles's Law | V/T=k or V1/T1= V2/T2 | Gas volume is directly related to Kelvin temp. | Temperature goes up, volume will go up |
| Gay-Lussac's Law | P/T or P1/T1= P2/T2 | Pressure is directly related to Kelvin temperature. | Temperature goes up, Pressure will go up |
| Combined gas law | PV/T=k or P1V1/T1 = P2V2/T2 | Relates pressure, temperature, and volume. | |
| Dalton's law of partial pressures | Pt=P1 + P2 + P3... | The pressure of a gas that is made up of a mixture of gases is the sum of the pressures of each individual gas component. | 24 apples = 9 apples + 8 apples + 7 apples |
| Gases collected by water displacement | P atm= Pgas+PH2O | Not really a law, used when a gas is present with water vapor. | The air |
| Avogadro's Law | V = kn | Gas volume is directly proportional to the number of moles of gas at a constant temperature and pressure. | all gases |
| The Ideal Gas Constant | R = PV/nT (explained below) | Combination of above gas laws | Relates volume, number of moles, and temperature. |
The ideal gas constant changes according to which unit is used for pressure. Although the SI unit for pressure is pascals, the more common unit is atmospheres(atm). The ideal gas constant is found by calculating the volume of one mole at standard temperature and pressure (STP) of an ideal gas. At STP, the volume of any ideal gas at one mole is 22.41410 L(or the standard molar volume of a gas).After substituting the values into the equation:
R = PV/nT, R = {(1 atm * 22.41410L)/(1 mol * 273 K)} = 0.0821*{(L*atm)/(mol*k)}
| Units of R | Value of R | Pressure Units(P) |
| {(L * mmHg)/(mol * K)} | 62.4 | mmHg (millimeters of Mercury |
| {(L * atm)/(mol * K)} | 0.0821 | atm (atmospheres) |
| {(L * kPa)/(mol * K)} | 8.314 | kPa (kilopascals) |
For links to the rest of the site look below
Homepage
An Explanation of the Kinetic-Molecular Theory
An Explanation of Pressure
Whitney's View on Chemistry?
A short Quiz
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