Molecular chaos
In the kinetic theory of gases in physics, the molecular chaos hypothesis (also called Stosszahlansatz in the writings of Paul and Tatiana Ehrenfest[1][2]) is the assumption that the velocities of colliding particles are uncorrelated, and independent of position. This means the probability that a pair of particles with given velocities will collide can be calculated by considering each particle separately and ignoring any correlation between the probability for finding one particle with velocity v and probability for finding another velocity v' in a small region δr. James Clerk Maxwell introduced this approximation in 1867[3] although its origins can be traced back to his first work on the kinetic theory in 1860.[4][5]
The assumption of molecular chaos is the key ingredient that allows proceeding from the BBGKY hierarchy to Boltzmann's equation, by reducing the 2-particle distribution function showing up in the collision term to a product of 1-particle distributions. This in turn leads to Boltzmann's H-theorem of 1872,[6] which attempted to use kinetic theory to show that the entropy of a gas prepared in a state of less than complete disorder must inevitably increase, as the gas molecules are allowed to collide. This drew the objection from Loschmidt that it should not be possible to deduce an irreversible process from time-symmetric dynamics and a time-symmetric formalism: something must be wrong (Loschmidt's paradox). The resolution (1895) of this paradox is that the velocities of two particles after a collision are no longer truly uncorrelated. By asserting that it was acceptable to ignore these correlations in the population at times after the initial time, Boltzmann had introduced an element of time asymmetry through the formalism of his calculation.[citation needed]
Though the Stosszahlansatz is usually understood as a physically grounded hypothesis, it was recently highlighted that it could also be interpreted as a heuristic hypothesis. This interpretation allows using the principle of maximum entropy in order to generalize the ansatz to higher-order distribution functions.[7]
See also
[edit]References
[edit]- ^ Ehrenfest, Paul; Ehrenfest, Tatiana (2002). The Conceptual Foundations of the Statistical Approach in Mechanics. Courier Corporation. ISBN 9780486495040.
- ^ Brown, Harvey R.; Myrvold, Wayne (2008-09-08). "Boltzmann's H-theorem, its limitations, and the birth of (fully) statistical mechanics". arXiv:0809.1304 [physics.hist-ph].
- ^ Maxwell, J. C. (1867). "On the Dynamical Theory of Gases". Philosophical Transactions of the Royal Society of London. 157: 49–88. doi:10.1098/rstl.1867.0004. S2CID 96568430.
- ^ See:
- Maxwell, J.C. (1860) "Illustrations of the dynamical theory of gases. Part I. On the motions and collisions of perfectly elastic spheres," Philosophical Magazine, 4th series, 19 : 19–32.
- Maxwell, J.C. (1860) "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," Philosophical Magazine, 4th series, 20 : 21–37.
- ^ 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:1702.01411. Bibcode:2017SHPMP..57...53G. doi:10.1016/j.shpsb.2017.01.001. S2CID 38272381.
- ^
L. Boltzmann, "Weitere Studien über das Wärmegleichgewicht unter Gasmolekülen." Sitzungsberichte Akademie der Wissenschaften 66 (1872): 275-370.
English translation: Boltzmann, L. (2003). "Further Studies on the Thermal Equilibrium of Gas Molecules". The Kinetic Theory of Gases. History of Modern Physical Sciences. Vol. 1. pp. 262–349. Bibcode:2003HMPS....1..262B. doi:10.1142/9781848161337_0015. ISBN 978-1-86094-347-8. - ^ Chliamovitch, G.; Malaspinas, O.; Chopard, B. (2017). "Kinetic theory beyond the Stosszahlansatz". Entropy. 19 (8): 381. Bibcode:2017Entrp..19..381C. doi:10.3390/e19080381.
 | This article about statistical mechanics is a stub. You can help Wikipedia by expanding it. |