| P | = Pressure of the Gas (SI: Pa = M/m2; 1 atm =101.3 kPa) |
| V | = Volume of the Gas (SI: m3; 1 liter = 10-3 m3 = 1000 cm3) |
| T | = Temperature of the Gas (SI: K; oC = K - 273.15) |
| N | = Number of molecules in the Gas |
| k | = Boltzmann's Constant (SI: k = 1.38x10 -23 J/K) |
| n | = number of gram moles in the Gas |
| R | = Universal Gas Constant ( R = 8.314 J/mole/K) |
| NA | = 6.022x1023 molecules/mole (Avogadro's Number) |
| M | = Molecular Weight of the Gas in grams per mole |
| m | = mass of the Gas (SI: kg; 1 g = 10-3 kg) |
