[{"@context":"http:\/\/schema.org\/","@type":"BlogPosting","@id":"https:\/\/wiki.edu.vn\/en\/wiki40\/thermodynamic-beta-wikipedia\/#BlogPosting","mainEntityOfPage":"https:\/\/wiki.edu.vn\/en\/wiki40\/thermodynamic-beta-wikipedia\/","headline":"Thermodynamic beta – Wikipedia","name":"Thermodynamic beta – Wikipedia","description":"From Wikipedia, the free encyclopedia Measure of the coldness of a system “Coldness” redirects here. For the abstract noun, see","datePublished":"2014-04-26","dateModified":"2014-04-26","author":{"@type":"Person","@id":"https:\/\/wiki.edu.vn\/en\/wiki40\/author\/lordneo\/#Person","name":"lordneo","url":"https:\/\/wiki.edu.vn\/en\/wiki40\/author\/lordneo\/","image":{"@type":"ImageObject","@id":"https:\/\/secure.gravatar.com\/avatar\/c9645c498c9701c88b89b8537773dd7c?s=96&d=mm&r=g","url":"https:\/\/secure.gravatar.com\/avatar\/c9645c498c9701c88b89b8537773dd7c?s=96&d=mm&r=g","height":96,"width":96}},"publisher":{"@type":"Organization","name":"Enzyklop\u00e4die","logo":{"@type":"ImageObject","@id":"https:\/\/wiki.edu.vn\/wiki4\/wp-content\/uploads\/2023\/08\/download.jpg","url":"https:\/\/wiki.edu.vn\/wiki4\/wp-content\/uploads\/2023\/08\/download.jpg","width":600,"height":60}},"image":{"@type":"ImageObject","@id":"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/thumb\/8\/8a\/ColdnessScale.svg\/250px-ColdnessScale.svg.png","url":"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/thumb\/8\/8a\/ColdnessScale.svg\/250px-ColdnessScale.svg.png","height":"260","width":"250"},"url":"https:\/\/wiki.edu.vn\/en\/wiki40\/thermodynamic-beta-wikipedia\/","about":["Wiki"],"wordCount":4702,"articleBody":"From Wikipedia, the free encyclopediaMeasure of the coldness of a system“Coldness” redirects here. For the abstract noun, see Cold.  SI temperature\/coldness conversion scale: Temperatures in Kelvin scale are shown in blue (Celsius scale in green, Fahrenheit scale in red), coldness values in gigabyte per nanojoule are shown in black. Infinite temperature (coldness zero) is shown at the top of the diagram; positive values of coldness\/temperature are on the right-hand side, negative values on the left-hand side.In statistical thermodynamics, thermodynamic beta, also known as coldness, is the reciprocal of the thermodynamic temperature of a system:\u03b2=1kBT{displaystyle beta ={frac {1}{k_{rm {B}}T}}} (where T is the temperature and kB is Boltzmann constant).[1]It was originally introduced in 1971 (as K\u00e4ltefunktion “coldness function”) by Ingo M\u00fcller\u00a0[de], one of the proponents of the rational thermodynamics school of thought,[2] based on earlier proposals for a “reciprocal temperature” function.[3][4]Thermodynamic beta has units reciprocal to that of energy (in SI units, reciprocal joules, [\u03b2]=J\u22121{displaystyle [beta ]={textrm {J}}^{-1}}). In non-thermal units, it can also be measured in byte per joule, or more conveniently, gigabyte per nanojoule;[5] 1 K\u22121 is equivalent to about 13,062 gigabytes per nanojoule; at room temperature: T = 300K, \u03b2 \u2248 44\u00a0GB\/nJ \u2248 39\u00a0eV\u22121 \u2248 2.4\u00d71020\u00a0J\u22121. The conversion factor is 1 GB\/nJ = 8ln\u20612\u00d71018{displaystyle 8ln 2times 10^{18}} J\u22121.Table of ContentsDescription[edit]Advantages[edit]Statistical interpretation[edit]Connection of statistical view with thermodynamic view[edit]See also[edit]References[edit]Description[edit]Thermodynamic beta is essentially the connection between the information theory and statistical mechanics interpretation of a physical system through its entropy and the thermodynamics associated with its energy. It expresses the response of entropy to an increase in energy. If a system is challenged with a small amount of energy, then \u03b2 describes the amount the system will randomize.Via the statistical definition of temperature as a function of entropy, the coldness function can be calculated in the microcanonical ensemble from the formula\u03b2=1kBT=1kB(\u2202S\u2202E)V,N{displaystyle beta ={frac {1}{k_{rm {B}}T}},={frac {1}{k_{rm {B}}}}left({frac {partial S}{partial E}}right)_{V,N}}(i.e., the partial derivative of the entropy S with respect to the energy E at constant volume V and particle number N).Advantages[edit]Though completely equivalent in conceptual content to temperature, \u03b2 is generally considered a more fundamental quantity than temperature owing to the phenomenon of negative temperature, in which \u03b2 is continuous as it crosses zero whereas T has a singularity.[6]In addition, \u03b2 has the advantage of being easier to understand causally: If a small amount of heat is added to a system, \u03b2 is the increase in entropy divided by the increase in heat. Temperature is difficult to interpret in the same sense, as it is not possible to “Add entropy” to a system except indirectly, by modifying other quantities such as temperature, volume, or number of particles.Statistical interpretation[edit]From the statistical point of view, \u03b2 is a numerical quantity relating two macroscopic systems in equilibrium. The exact formulation is as follows. Consider two systems, 1 and 2, in thermal contact, with respective energies E1 and E2. We assume E1 + E2 = some constant E. The number of microstates of each system will be denoted by \u03a91 and \u03a92. Under our assumptions \u03a9i depends only on Ei. We also assume that any microstate of system 1 consistent with E1 can coexist with any microstate of system 2 consistent with E2. Thus, the number of microstates for the combined system is\u03a9=\u03a91(E1)\u03a92(E2)=\u03a91(E1)\u03a92(E\u2212E1).{displaystyle Omega =Omega _{1}(E_{1})Omega _{2}(E_{2})=Omega _{1}(E_{1})Omega _{2}(E-E_{1}).,}We will derive \u03b2 from the fundamental assumption of statistical mechanics:When the combined system reaches equilibrium, the number \u03a9 is maximized.(In other words, the system naturally seeks the maximum number of microstates.) Therefore, at equilibrium,ddE1\u03a9=\u03a92(E2)ddE1\u03a91(E1)+\u03a91(E1)ddE2\u03a92(E2)\u22c5dE2dE1=0.{displaystyle {frac {d}{dE_{1}}}Omega =Omega _{2}(E_{2}){frac {d}{dE_{1}}}Omega _{1}(E_{1})+Omega _{1}(E_{1}){frac {d}{dE_{2}}}Omega _{2}(E_{2})cdot {frac {dE_{2}}{dE_{1}}}=0.}But E1 + E2 = E impliesdE2dE1=\u22121.{displaystyle {frac {dE_{2}}{dE_{1}}}=-1.}So\u03a92(E2)ddE1\u03a91(E1)\u2212\u03a91(E1)ddE2\u03a92(E2)=0{displaystyle Omega _{2}(E_{2}){frac {d}{dE_{1}}}Omega _{1}(E_{1})-Omega _{1}(E_{1}){frac {d}{dE_{2}}}Omega _{2}(E_{2})=0}i.e.ddE1ln\u2061\u03a91=ddE2ln\u2061\u03a92at equilibrium.{displaystyle {frac {d}{dE_{1}}}ln Omega _{1}={frac {d}{dE_{2}}}ln Omega _{2}quad {mbox{at equilibrium.}}}The above relation motivates a definition of \u03b2:\u03b2=dln\u2061\u03a9dE.{displaystyle beta ={frac {dln Omega }{dE}}.}Connection of statistical view with thermodynamic view[edit]When two systems are in equilibrium, they have the same thermodynamic temperature T. Thus intuitively, one would expect \u03b2 (as defined via microstates) to be related to T in some way. This link is provided by Boltzmann’s fundamental assumption written asS=kBln\u2061\u03a9,{displaystyle S=k_{rm {B}}ln Omega ,}where kB is the Boltzmann constant, S is the classical thermodynamic entropy, and \u03a9 is the number of microstates. Sodln\u2061\u03a9=1kBdS.{displaystyle dln Omega ={frac {1}{k_{rm {B}}}}dS.}Substituting into the definition of \u03b2 from the statistical definition above gives\u03b2=1kBdSdE.{displaystyle beta ={frac {1}{k_{rm {B}}}}{frac {dS}{dE}}.}Comparing with thermodynamic formuladSdE=1T,{displaystyle {frac {dS}{dE}}={frac {1}{T}},}we have\u03b2=1kBT=1\u03c4{displaystyle beta ={frac {1}{k_{rm {B}}T}}={frac {1}{tau }}}where \u03c4{displaystyle tau } is called the fundamental temperature of the system, and has units of energy.See also[edit]References[edit]^ J. Meixner (1975) “Coldness and Temperature”, Archive for Rational Mechanics and Analysis 57:3, 281-290 abstract.^ M\u00fcller, I., “Die K\u00e4ltefunktion, eine universelle Funktion in der Thermodynamik w\u00e4rmeleitender Fl\u00fcssigkeiten”.  Archive for Rational Mechanics and Analysis  40 (1971), 1\u201336 (“The coldness, a universal function in thermoelastic bodies”,  Archive for Rational Mechanics and Analysis 41:5, 319-332).^ Day, W.A. and Gurtin, Morton E. (1969) “On the symmetry of the conductivity tensor and other restrictions in the nonlinear theory of heat conduction”, Archive for Rational Mechanics and Analysis 33:1, 26-32 (Springer-Verlag)  abstract.^ J. Castle, W. Emmenish, R. Henkes, R. Miller, and J. Rayne (1965) Science by Degrees: Temperature from Zero to Zero (Westinghouse Search Book Series, Walker and Company, New York).^ P. Fraundorf (2003) “Heat capacity in bits”, Amer. J. Phys. 71:11, 1142-1151.^ Kittel, Charles; Kroemer, Herbert (1980), Thermal Physics (2\u00a0ed.), United States of America: W. H. Freeman and Company, ISBN\u00a0978-0471490302"},{"@context":"http:\/\/schema.org\/","@type":"BreadcrumbList","itemListElement":[{"@type":"ListItem","position":1,"item":{"@id":"https:\/\/wiki.edu.vn\/en\/wiki40\/#breadcrumbitem","name":"Enzyklop\u00e4die"}},{"@type":"ListItem","position":2,"item":{"@id":"https:\/\/wiki.edu.vn\/en\/wiki40\/thermodynamic-beta-wikipedia\/#breadcrumbitem","name":"Thermodynamic beta – Wikipedia"}}]}]