| Term | Definition |
|---|
| 1/2 m [c2] = 3kT / 2 | equation linking the average molecular kinetic energy of a gas to absolute temperature (T) |
| 1.38 x 10-27 J K-1 | value of k (Boltzmann constant) |
| mean square speed | what is c2 called? |
| + 273 | how is temperature in K different to temperature in deg C? |
| pV = nRT | ideal gas equation |
| pV = nRT | equation relating the number of moles of molecules in a gas and its pressure |
| pV = nRT | equation relating a gas' pressure and its volume |
| the molar gas constant | what is R? |
| 6.02 x 10 23 molecules | how many molecules does 1 mole of a gas contain? |
| R = 6.02 x 10 23 x k | equation for R |
| 8.31 J K-1 mol-1 | value of R |
| p2V2 / T2 = p1V1 / T1 | equation for a situation where a change in a gas' pressure or volume has occurred |
| p = F / a | equation for pressure |
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