The Gas Laws
If we make several plausible assumptions, the macroscopic properties of a gas can be expressed simply in terms of three gas laws. The assumptions are:
All collisions that take place between the molecules of a gas or between the gas molecules and the walls of the container are elastic, so the total kinetic energy of the gas is conserved. In addition the time of each collision is zero.
The volume the the actual gas molecules is small compared with the volume of the container. In fact calculations indicate the actual volume of the gas molecules is of the order of 1% of the volume of the container under normal conditions – room temperature and atmospheric pressure.
There are no forces between the gas molecules or between the gas molecules and the walls of the container.
The motion of the gas molecules is random, with no preferred direction. There is no bulk movement of the gas.
Under these conditions a gas will obey three simple laws.
The Pressure Law: The pressureof a fixed mass of gas increases linearly with temperatureat constant volume. This can be expressed as
Charles's Law: The volumeof a fixed mass of gas increases linearly with temperatureat constant pressure. This can be written as
Boyle's Law: The pressureof a fixed mass of gas is inversely proportional to the volumeat constant temperature. This can be expressed as