The ideal gas law describes a relationship between pressure (P), volume (V), temperature and number of moles (n) in terms of the gas constant (R) for an ideal gas. The ratio of (PV) to (nT) should be equal to the gas constant as shown in the ideal gas equation PV = nRT. The ideal gas law assumes that the gas molecules are ideal and do not have any volume and that there are no forces acting on them except during collisions. It was designed to understand the effects of pressure, volume and temperature on gases while excluding the variables of real-world conditions.
The behavior of ideal gases under varying conditions of volume, temperature and pressure in the ideal gas law can be split into the following gas laws: Boyle’s law, Charles’ law and Avogadro’s law. Boyle’s law says that the pressure of an ideal gas at a constant temperature is inversely proportional to the volume of the gas. According to Charles’ law, at a constant pressure, temperature is directly proportional to the volume of an ideal gas. Avogadro’s law states that under the same conditions of temperature and pressure, volume is directly proportional to the number of moles. Finally, at a constant volume, pressure is directly proportional to temperature.