Maxwell–Boltzmann distribution

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Maxwell–Boltzmann
Probability density function
Maxwell-Boltzmann distribution pdf.svg
Cumulative distribution function
Maxwell-Boltzmann distribution cdf.svg
Parameters
Support
PDF
CDF where erf is the error function
Mean
Mode
Variance
Skewness
Ex. kurtosis
Entropy

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

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 (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 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. Ideal plasmas, which are ionized gases of sufficiently low density, frequently also have particle distributions that are partially or entirely Maxwellian.[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.

Distribution function[edit]

Assuming the system of interest contains a large number of particles, the fraction of the particles within an infinitesimal element of three-dimensional velocity space, d, centered on a velocity vector of magnitude , is d, in which

where is the particle mass and is the product of Boltzmann's constant and thermodynamic temperature.

The speed probability density functions of the speeds of a few noble gases at a temperature of 298.15 K (25 °C). The y-axis is in s/m so that the area under any section of the curve (which represents the probability of the speed being in that range) is dimensionless.

One can write the element of velocity space as d = ddd, for velocities in a standard Cartesian coordinate system, or as d = dd in a standard spherical coordinate system, where d is an element of solid angle. Here is given as a probability distribution function, properly normalized so that d over all velocities equals one. In plasma physics, the probability distribution is often multipled by the particle density, so that the integral of the resulting distribution function equals the density.

Undergraduate students are likely to work with the Maxwellian distribution function for particles moving in only one direction. If this direction is , then one has

which can be obtained by integrating the three-dimensional form given above over and .

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 . 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:

With the Darwin–Fowler method of mean values the Maxwell–Boltzmann distribution is obtained as an exact result.[clarification needed]

Typical speeds[edit]

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]

  • The most probable speed, vp, is the speed most likely to be possessed by any molecule (of the same mass m) in the system and corresponds to the maximum value or mode of f(v). To find it, we calculate the derivative df/dv, set it to zero and solve for v:

    with the solution:

    (the second solution representing the "least probable speed").

    R is the gas constant and M is molar mass of the substance, and thus may be calculated as a product of particle mass, m, and Avogadro constant, Na:

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

  • The mean speed is the expected value of the speed distribution, setting :
  • The mean square speed is the second-order raw moment of the speed distribution. The "root mean square speed" is the square root of the mean square speed, corresponding to the speed of a particle with median kinetic energy, setting :

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

where is the adiabatic index, f is the number of degrees of freedom of the individual gas molecule. For the example above, diatomic nitrogen (approximating air) at 300 K, [9] and

the true value for air can be approximated by using the average molar weight of air (29 g/mol), yielding 347 m/s at 300 K (corrections for variable humidity are of the order of 0.1% to 0.6%).

Derivation and related distributions[edit]

Maxwell–Boltzmann statistics[edit]

The original derivation in 1860 by James Clerk Maxwell was an argument based on molecular collisions of the Kinetic theory of gases as well as certain symmetries in the speed distribution function; Maxwell also gave an early argument that these molecular collisions entail a tendency towards equilibrium.[5][10] After Maxwell, Ludwig Boltzmann in 1872[11] also derived the distribution on mechanical grounds and argued that gases should over time tend toward this distribution, due to collisions (see H-theorem). He later (1877)[12] derived the distribution again under the framework of statistical thermodynamics. The derivations in this section are along the lines of Boltzmann's 1877 derivation, starting with result known as Maxwell–Boltzmann statistics (from statistical thermodynamics). Maxwell–Boltzmann statistics gives the average number of particles found in a given single-particle microstate, under certain assumptions, the logarithm of the fraction of particles in a given microstate is proportional to the ratio of the energy of that state to the temperature of the system:

The assumptions of this equation are that the particles do not interact, and that they are classical; this means that each particle's state can be considered independently from the other particles' states. Additionally, the particles are assumed to be in thermal equilibrium.[1][13]

This relation can be written as an equation by introducing a normalizing factor:

 

 

 

 

(1)

where:

  • 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.

The denominator in Equation (1) is simply a normalizing factor so that the ratios add up to unity — in other words it is a kind of partition function (for the single-particle system, not the usual partition function of the entire system).

Because velocity and speed are related to energy, Equation (1) can be used to derive relationships between temperature and the speeds of gas particles. All that is needed is to discover the density of microstates in energy, which is determined by dividing up momentum space into equal sized regions.

Distribution for the momentum vector[edit]

The potential energy is taken to be zero, so that all energy is in the form of kinetic energy. The relationship between kinetic energy and momentum for massive non-relativistic particles is

 

 

 

 

(2)

where p2 is the square of the momentum vector p = [pxpypz]. We may therefore rewrite Equation (1) as:

 

 

 

 

(3)

where Z is the partition function, corresponding to the denominator in Equation (1). Here m is the molecular mass of the gas, T is the thermodynamic temperature and k is the Boltzmann constant. This distribution of is proportional to the probability density function fp for finding a molecule with these values of momentum components, so:

 

 

 

 

(4)

The normalizing constant can be determined by recognizing that the probability of a molecule having some momentum must be 1. Integrating the exponential in (4) over all px, py, and pz yields a factor of

So that the normalized distribution function is:

   (6)

The distribution is seen to be the product of three independent normally distributed variables , , and , with variance . Additionally, it can be seen that the magnitude of momentum will be distributed as a Maxwell–Boltzmann distribution, with . The Maxwell–Boltzmann distribution for the momentum (or equally for the velocities) can be obtained more fundamentally using the H-theorem at equilibrium within the Kinetic theory of gases framework.

Distribution for the energy[edit]

The energy distribution is found imposing

 

 

 

 

(7)

where is the infinitesimal phase-space volume of momenta corresponding to the energy interval . Making use of the spherical symmetry of the energy-momentum dispersion relation , this can be expressed in terms of as

 

 

 

 

(8)

Using then (8) in (7), and expressing everything in terms of the energy , we get

and finally

   (9)

Since the energy is proportional to the sum of the squares of the three normally distributed momentum components, this distribution is a gamma distribution; in particular, it is a chi-squared distribution with three degrees of freedom.

By the equipartition theorem, this energy is evenly distributed among all three degrees of freedom, so that the energy per degree of freedom is distributed as a chi-squared distribution with one degree of freedom:[14]

where is the energy per degree of freedom. At equilibrium, this distribution will hold true for any number of degrees of freedom. For example, if the particles are rigid mass dipoles of fixed dipole moment, they will have three translational degrees of freedom and two additional rotational degrees of freedom. The energy in each degree of freedom will be described according to the above chi-squared distribution with one degree of freedom, and the total energy will be distributed according to a chi-squared distribution with five degrees of freedom. This has implications in the theory of the specific heat of a gas.

The Maxwell–Boltzmann distribution can also be obtained by considering the gas to be a type of quantum gas for which the approximation ε >> k T may be made.

Distribution for the velocity vector[edit]

Recognizing that the velocity probability density fv is proportional to the momentum probability density function by

and using p = mv we get

which is the Maxwell–Boltzmann velocity distribution. The probability of finding a particle with velocity in the infinitesimal element [dvxdvydvz] about velocity v = [vxvyvz] is

Like the momentum, this distribution is seen to be the product of three independent normally distributed variables , , and , but with variance . It can also be seen that the Maxwell–Boltzmann velocity distribution for the vector velocity [vxvyvz] is the product of the distributions for each of the three directions:

where the distribution for a single direction is

Each component of the velocity vector has a normal distribution with mean and standard deviation , so the vector has a 3-dimensional normal distribution, a particular kind of multivariate normal distribution, with mean and standard deviation .

Distribution for the speed[edit]

The Maxwell–Boltzmann distribution for the speed follows immediately from the distribution of the velocity vector, above. Note that the speed is

and the volume element in spherical coordinates

where and are the spherical coordinate angles of the velocity vector. Integration of the probability density function of the velocity over the solid angles yields an additional factor of . The speed distribution with substitution of the speed for the sum of the squares of the vector components:

See also[edit]

References[edit]

  1. ^ a b Statistical Physics (2nd Edition), F. Mandl, Manchester Physics, John Wiley & Sons, 2008, ISBN 9780471915331
  2. ^ University Physics – With Modern Physics (12th Edition), H.D. Young, R.A. Freedman (Original edition), Addison-Wesley (Pearson International), 1st Edition: 1949, 12th Edition: 2008, ISBN 978-0-321-50130-1
  3. ^ Encyclopaedia of Physics (2nd Edition), R.G. Lerner, G.L. Trigg, VHC publishers, 1991, ISBN 3-527-26954-1 (Verlagsgesellschaft), ISBN 0-89573-752-3 (VHC Inc.)
  4. ^ N.A. Krall and A.W. Trivelpiece, Principles of Plasma Physics, San Francisco Press, Inc., 1986, among many other texts on basic plasma physics
  5. ^ a b See:
    • Maxwell, J.C. (1860 A): Illustrations of the dynamical theory of gases. Part I. On the motions and collisions of perfectly elastic spheres. The London, Edinburgh, and Dublin Philosophical Magazine and Journal of Science, 4th Series, vol.19, pp.19-32. [1]
    • Maxwell, J.C. (1860 B): Illustrations of the dynamical theory of gases. Part II. On the process of diffusion of two or more kinds of moving particles among one another. The London, Edinburgh, and Dublin Philosophical Magazine and Journal of Science, 4th Ser., vol.20, pp.21-37. [2]
  6. ^ H.J.W. Müller-Kirsten (2013), Basics of Statistical Physics, 2nd ed., World Scientific, ISBN 978-981-4449-53-3, Chapter 2.
  7. ^ Raymond A. Serway; Jerry S. Faughn & Chris Vuille (2011). College Physics, Volume 1 (9th ed.). p. 352. ISBN 9780840068484. 
  8. ^ The calculation is unaffected by the Nitrogen being diatomic. Despite the larger heat capacity (larger internal energy at the same temperature) of diatomic gases relative to monatomic gases, due to their larger number of degrees of freedom, is still the mean translational kinetic energy. Nitrogen being diatomic only affects the value of the molar mass M = 28 g/mol. See e.g. K. Prakashan, Engineering Physics (2001), 2.278.
  9. ^ Nitrogen at room temperature is considered a "rigid" diatomic gas, with two rotational degrees of freedom additional to the three translational ones, and the vibrational degree of freedom not accessible.
  10. ^ Gyenis, Balazs (2017). "Maxwell and the normal distribution: A colored story of probability, independence, and tendency towards equilibrium". Studies in History and Philosophy of Modern Physics. 57: 53–65. arXiv:1702.01411Freely accessible. Bibcode:2017SHPMP..57...53G. doi:10.1016/j.shpsb.2017.01.001. 
  11. ^ Boltzmann, L., "Weitere studien über das Wärmegleichgewicht unter Gasmolekülen." Sitzungsberichte der Kaiserlichen Akademie der Wissenschaften in Wien, mathematisch-naturwissenschaftliche Classe, 66, 1872, pp. 275–370.
  12. ^ Boltzmann, L., "Über die Beziehung zwischen dem zweiten Hauptsatz der mechanischen Wärmetheorie und der Wahrscheinlichkeitsrechnung respektive den Sätzen über das Wärmegleichgewicht." Sitzungsberichte der Kaiserlichen Akademie der Wissenschaften in Wien, Mathematisch-Naturwissenschaftliche Classe. Abt. II, 76, 1877, pp. 373–435. Reprinted in Wissenschaftliche Abhandlungen, Vol. II, pp. 164–223, Leipzig: Barth, 1909.
  13. ^ McGraw Hill Encyclopaedia of Physics (2nd Edition), C.B. Parker, 1994, ISBN 0-07-051400-3
  14. ^ Laurendeau, Normand M. (2005). Statistical thermodynamics: fundamentals and applications. Cambridge University Press. p. 434. ISBN 0-521-84635-8. , Appendix N, page 434

Further reading[edit]

  • Physics for Scientists and Engineers – with Modern Physics (6th Edition), P. A. Tipler, G. Mosca, Freeman, 2008, ISBN 0-7167-8964-7
  • Thermodynamics, From Concepts to Applications (2nd Edition), A. Shavit, C. Gutfinger, CRC Press (Taylor and Francis Group, USA), 2009, ISBN 978-1-4200-7368-3
  • Chemical Thermodynamics, D.J.G. Ives, University Chemistry, Macdonald Technical and Scientific, 1971, ISBN 0-356-03736-3
  • Elements of Statistical Thermodynamics (2nd Edition), L.K. Nash, Principles of Chemistry, Addison-Wesley, 1974, ISBN 0-201-05229-6
  • 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.

External links[edit]