Class 11 › Physics › Physics Part II Kinetic Theory Class 11 Physics · Physics Part II · Chapter 5
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Browse all 60 kits → SummaryKinetic theory explains the behaviour of gases by treating them as large numbers of tiny molecules in rapid, random motion, with intermolecular forces negligible except during brief elastic collisions. Matter is made of atoms about an angstrom in size; in gases the molecules are far apart, so the mean free path is large. Gases at low pressure and high temperature obey the ideal-gas equation \(PV=\mu RT=k_B NT\), which embodies Boyle's law, Charles' law, Avogadro's hypothesis and Dalton's law of partial pressures. From the assumption of elastic molecular collisions with the walls, the pressure of an ideal gas is derived as \(P=\tfrac13 nm\overline{v^{2}}\), leading to the kinetic interpretation of temperature: the average translational kinetic energy of a molecule is \(\tfrac32 k_B T\), independent of the gas, and the root-mean-square speed is \(v_{rms}=\sqrt{3k_B T/m}\). The law of equipartition of energy assigns \(\tfrac12 k_B T\) to each degree of freedom, explaining the molar specific heats of monatomic, diatomic and polyatomic gases and of solids. The mean free path \(l=1/(\sqrt2\,\pi n d^{2})\) is the average distance a molecule travels between collisions and accounts for diffusion, viscosity and conduction in gases.
Molecular nature of matter Behaviour of gases and the ideal-gas equation Kinetic theory of an ideal gas and pressure Kinetic interpretation of temperature and rms speed Law of equipartition of energy Specific heat capacity of gases and solids Mean free path Key termsIdeal gas
A theoretical gas that obeys \(PV=\mu RT\) exactly at all pressures and temperatures; real gases approach it at low pressure and high temperature.
Boltzmann constant
The constant \(k_B=R/N_A=1.38\times10^{-23}\ \text{J K}^{-1}\) linking molecular energy to temperature.
Root-mean-square speed
The square root of the mean of the squared molecular speeds, \(v_{rms}=\sqrt{3k_B T/m}\).
Degree of freedom
An independent way in which a molecule can possess energy — translational, rotational or vibrational.
Law of equipartition of energy
In equilibrium, energy is shared equally among all degrees of freedom, each contributing \(\tfrac12 k_B T\).
Mean free path
The average distance a molecule travels between successive collisions, \(l=1/(\sqrt2\,\pi n d^{2})\).
Extra questions & answersQ1 State the basic assumptions of kinetic theory. Answer Q2 Write the kinetic expression for the pressure of an ideal gas. Answer Q3 State the kinetic interpretation of temperature. Answer Q4 Write the formula for the rms speed of gas molecules. Answer Q5 State the law of equipartition of energy. Answer Q6 How many degrees of freedom has a monatomic and a diatomic gas molecule? Answer Q7 Give the molar specific heats of a monatomic ideal gas. Answer Q8 Define mean free path and give its formula. Answer Q9 State Avogadro's hypothesis and how kinetic theory justifies it. Answer Q10 Why do lighter gases diffuse faster? Answer Try one from this chapter
In kinetic theory, collisions between gas molecules are assumed to be:
A Partially inelastic B Random in energy C Perfectly inelastic D Elastic
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