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Maxwell–Boltzmann distribution

In physics (in particular in statistical mechanics), the Maxwell–Boltzmann distribution, or Maxwell(ian) distribution, is a particular probability distribution named after James Clerk Maxwell and Ludwig Boltzmann.

This article is about particle energy levels and velocities. For system energy states, see Boltzmann distribution.

Parameters

(where exp is the exponential function)

(where erf is the error function)

It was first defined and used for describing particle speeds in idealized gases, where the particles move freely inside a stationary container without interacting with one another, except for very brief collisions in which they exchange energy and momentum with each other or with their thermal environment. The term "particle" in this context refers to gaseous particles only (atoms or molecules), and the system of particles is assumed to have reached thermodynamic equilibrium.[1] The energies of such particles follow what is known as Maxwell–Boltzmann statistics, and the statistical distribution of speeds is derived by equating particle energies with kinetic energy.


Mathematically, the Maxwell–Boltzmann distribution is the chi distribution with three degrees of freedom (the components of the velocity vector in Euclidean space), with a scale parameter measuring speeds in units proportional to the square root of (the ratio of temperature and particle mass).[2]


The Maxwell–Boltzmann distribution is a result of the kinetic theory of gases, which provides a simplified explanation of many fundamental gaseous properties, including pressure and diffusion.[3] The Maxwell–Boltzmann distribution applies fundamentally to particle velocities in three dimensions, but turns out to depend only on the speed (the magnitude of the velocity) of the particles. A particle speed probability distribution indicates which speeds are more likely: a randomly chosen particle will have a speed selected randomly from the distribution, and is more likely to be within one range of speeds than another. The kinetic theory of gases applies to the classical ideal gas, which is an idealization of real gases. In real gases, there are various effects (e.g., van der Waals interactions, vortical flow, relativistic speed limits, and quantum exchange interactions) that can make their speed distribution different from the Maxwell–Boltzmann form. However, rarefied gases at ordinary temperatures behave very nearly like an ideal gas and the Maxwell speed distribution is an excellent approximation for such gases. This is also true for ideal plasmas, which are ionized gases of sufficiently low density.[4]


The distribution was first derived by Maxwell in 1860 on heuristic grounds.[5] Boltzmann later, in the 1870s, carried out significant investigations into the physical origins of this distribution. The distribution can be derived on the ground that it maximizes the entropy of the system. A list of derivations are:

m is the particle mass;

k is the ;

Boltzmann constant

T is ;

thermodynamic temperature

is a probability distribution function, properly normalized so that over all velocities is unity.

For a system containing a large number of identical non-interacting, non-relativistic classical particles in thermodynamic equilibrium, the fraction of the particles within an infinitesimal element of the three-dimensional velocity space d 3v, centered on a velocity vector of magnitude , is given by


One can write the element of velocity space as , for velocities in a standard Cartesian coordinate system, or as in a standard spherical coordinate system, where is an element of solid angle and


The Maxwellian distribution function for particles moving in only one direction, if this direction is x, is


Recognizing the symmetry of , one can integrate over solid angle and write a probability distribution of speeds as the function[6]


This probability density function gives the probability, per unit speed, of finding the particle with a speed near v. This equation is simply the Maxwell–Boltzmann distribution (given in the infobox) with distribution parameter The Maxwell–Boltzmann distribution is equivalent to the chi distribution with three degrees of freedom and scale parameter


The simplest ordinary differential equation satisfied by the distribution is:


or in unitless presentation:

gas constant

The mean speed , most probable speed (mode) vp, and root-mean-square speed can be obtained from properties of the Maxwell distribution.


This works well for nearly ideal, monatomic gases like helium, but also for molecular gases like diatomic oxygen. This is because despite the larger heat capacity (larger internal energy at the same temperature) due to their larger number of degrees of freedom, their translational kinetic energy (and thus their speed) is unchanged.[7]


For diatomic nitrogen (N2, the primary component of air)[8] at room temperature (300 K), this gives


In summary, the typical speeds are related as follows:


The root mean square speed is directly related to the speed of sound c in the gas, by


The average relative velocity


The integral can easily be done by changing to coordinates and

Limitations[edit]

The Maxwell–Boltzmann distribution assumes that the velocities of individual particles are much less than the speed of light, i.e. that . For electrons, the temperature of electrons must be K.

Ni is the expected number of particles in the single-particle microstate i,

N is the total number of particles in the system,

Ei is the energy of microstate i,

the sum over index j takes into account all microstates,

T is the equilibrium temperature of the system,

k is the .

Boltzmann constant

Quantum Boltzmann equation

Maxwell–Boltzmann statistics

Maxwell–Jüttner distribution

Boltzmann distribution

Rayleigh distribution

Kinetic theory of gases

Physics for Scientists and Engineers – with Modern Physics (6th Edition), P. A. Tipler, G. Mosca, Freeman, 2008,  0-7167-8964-7

ISBN

Thermodynamics, From Concepts to Applications (2nd Edition), A. Shavit, C. Gutfinger, CRC Press (Taylor and Francis Group, USA), 2009,  978-1-4200-7368-3

ISBN

Chemical Thermodynamics, D.J.G. Ives, University Chemistry, Macdonald Technical and Scientific, 1971,  0-356-03736-3

ISBN

Elements of Statistical Thermodynamics (2nd Edition), L.K. Nash, Principles of Chemistry, Addison-Wesley, 1974,  0-201-05229-6

ISBN

Ward, CA & Fang, G 1999, "Expression for predicting liquid evaporation flux: Statistical rate theory approach", Physical Review E, vol. 59, no. 1, pp. 429–40.

Rahimi, P & Ward, CA 2005, "Kinetics of Evaporation: Statistical Rate Theory Approach", International Journal of Thermodynamics, vol. 8, no. 9, pp. 1–14.

from The Wolfram Demonstrations Project at Mathworld

"The Maxwell Speed Distribution"