Kinetic Theory of Gases

The kinetic theory is based on

The kinetic theory is based on six key assumptions: (1) Gases consist of a large number of tiny molecules in random motion, (2) Molecules are far apar

Pressure is caused by the constant

Pressure is caused by the constant bombardment of gas molecules on the walls of the container. Using Newton’s second law, the pressure is derived as $

The average kinetic energy of

The average kinetic energy of a gas molecule is directly proportional to the absolute temperature: $ \frac{1}{2} m \overline{c^2} = \frac{3}{2} kT $.

The root mean square (rms) speed

The root mean square (rms) speed is given by $ c_{\text{rms}} = \sqrt{\frac{3kT}{m}} = \sqrt{\frac{3RT}{M}} $. It represents the effective speed of ga

Energy is equally distributed among all

Energy is equally distributed among all degrees of freedom. Each degree of freedom contributes $ \frac{1}{2} kT $ to the energy of a molecule. A monat