Kinetic theory of gases — FAQ

The kinetic theory explains the macroscopic properties of gases (like pressure and temperature) by modelling them as collections of tiny, constantly moving particles (molecules) that collide with each other and their container walls.

The absolute temperature of a gas is a direct measure of the average translational kinetic energy of its molecules. A higher temperature means that, on average, the gas molecules are moving faster and possess more kinetic energy.

No, real gases only approximate ideal gas behaviour. They behave most like ideal gases at high temperatures and low pressures, where intermolecular forces are weak and the volume of the molecules themselves is negligible compared to the total gas volume.

Mean square speed ($\overline{c^2}$) is the average of the squares of the speeds of all molecules. Root-mean-square speed ($c_{rms}$) is the square root of the mean square speed. $c_{rms}$ gives a better representation of the typical speed of a molecule than a simple average.