|
|
| Line 1: |
Line 1: |
| {{Thermodynamics|cTopic=[[Thermodynamic system|Systems]]}}
| | Hi and then there. Let me start by introducing the author, her name is Eartha. Her husband doesn't like it method she does but what she really likes doing for you to draw 3d graphics but she can't make it her line of work. New Hampshire has for ages been my living place. Filing is how i support our neighbors but soon my husband and I will start this business. His wife and he maintain a [http://Www.Guardian.Co.uk/search?q=web+presence web presence]. You might in order to be check it out: http://www.unsignedsuperstar.com/index.php?do=/profile-93442/info/<br><br>Also visit my web-site; [http://www.unsignedsuperstar.com/index.php?do=/profile-93442/info/ diamond video role] |
| An '''ideal gas''' is a [[Scientific theory|theoretical]] [[gas]] composed of a set of randomly moving, non-interacting [[point particle]]s. The ideal gas concept is useful because it obeys the [[ideal gas law]], a simplified [[equation of state]], and is amenable to analysis under [[statistical mechanics]].
| |
| | |
| At normal conditions such as [[standard temperature and pressure]], most [[real gas]]es behave qualitatively like an ideal gas. Many gases such as [[nitrogen]], [[oxygen]], [[hydrogen]], [[noble gases]], and some heavier gases like [[carbon dioxide]] can be treated like ideal gases within reasonable tolerances.<ref name=boles>{{Cite book|title=Thermodynamics: An Engineering Approach |edition=Fourth | isbn = 0-07-238332-1|last1=Cengel|first1= Yunus A.|last2=Boles|first2=Michael A.|page=89}}</ref> Generally, a gas behaves more like an ideal gas at higher [[temperature]] and lower [[pressure]],<ref name=boles/> as the [[work (physics)|work]] which is against intermolecular forces becomes less significant compared with the particles' [[kinetic energy]], and the size of the molecules becomes less significant compared to the empty space between them.
| |
| | |
| The ideal gas model tends to fail at lower temperatures or higher pressures, when intermolecular forces and molecular size become important. It also fails for most heavy gases, such as many [[refrigerant]]s,<ref name=boles/> and for gases with strong intermolecular forces, notably [[water vapor]]. At some point of low temperature and high pressure, [[real gas]]es undergo a [[phase transition]], such as to a [[liquid]] or a [[solid]]. The model of an ideal gas, however, does not describe or allow phase transitions. These must be modeled by more complex [[equation of state|equations of state]].
| |
| | |
| The ideal gas model has been explored in both the [[Newtonian dynamics]] (as in "[[kinetic theory]]") and in [[quantum mechanics]] (as a "[[gas in a box]]"). The ideal gas model has also been used to model the behavior of electrons in a metal (in the [[Drude model]] and the [[free electron model]]), and it is one of the most important models in [[statistical mechanics]].
| |
| | |
| ==Types of ideal gas==
| |
| | |
| There are three basic classes of ideal gas:
| |
| | |
| * the classical or [[Maxwell-Boltzmann statistics|Maxwell-Boltzmann]] ideal gas,
| |
| * the ideal quantum [[Bose gas]], composed of [[bosons]], and
| |
| * the ideal quantum [[Fermi gas]], composed of [[fermions]].
| |
| | |
| The classical ideal gas can be separated into two types: The classical thermodynamic ideal gas and the ideal quantum Boltzmann gas. Both are essentially the same, except that the classical thermodynamic ideal gas is based on classical [[statistical mechanics]], and certain thermodynamic parameters such as the [[entropy]] are only specified to within an undetermined additive constant. The ideal quantum Boltzmann gas overcomes this limitation by taking the limit of the quantum Bose gas and quantum Fermi gas in the limit of high temperature to specify these additive constants. The behavior of a quantum Boltzmann gas is the same as that of a classical ideal gas except for the specification of these constants. The results of the quantum Boltzmann gas are used in a number of cases including the [[Sackur-Tetrode equation]] for the entropy of an ideal gas and the [[Saha ionization equation]] for a weakly ionized [[plasma (physics)|plasma]].
| |
| | |
| ==Classical thermodynamic ideal gas==
| |
| | |
| The thermodynamic properties of an ideal gas can be described by two equations:
| |
| The [[equation of state]] of a classical ideal gas is the [[ideal gas law]]
| |
| :<math>PV = nRT\,</math>
| |
| This equation is derived from [[Boyle's Law]]: <math>V = k/P</math> (at constant T and n); [[Charles's Law]]: <math>V = bT</math> (at constant P and n); and [[Avogadro's Law]]: <math>V = an</math> (at constant T and P). By combining the three laws, it would demonstrate that <math>3V = kba \left( \frac{Tn}{P} \right)</math> which would mean that <math>V = \left( \frac{kba}{3} \right) \left( \frac{Tn}{P} \right)</math>.
| |
| | |
| Under ideal conditions, <math>V = R \left( \frac{Tn}{P} \right)</math> ;
| |
| that is,
| |
| <math>PV = nRT</math>.
| |
| | |
| The [[internal energy]] of an ideal gas given by: :<math>U = \hat{c}_V nRT </math>
| |
| | |
| where
| |
| :* <math>P</math> is the [[pressure]]
| |
| :* <math>V</math> is the [[Volume (thermodynamics)|volume]]
| |
| :* <math>n</math> is the [[amount of substance]] of the gas (in moles)
| |
| :* <math>R</math> is the [[gas constant]] (8.314 [[joule|J]]·[[kelvin|K]]<sup>−1</sup>[[mole (unit)|mol]]<sup>-1</sup>)
| |
| :* <math>T</math> is the [[absolute temperature]]
| |
| :* <math>k</math> is a constant used in Boyle's Law
| |
| :* <math>b</math> is a proportionality constant; equal to <math>V/T</math>
| |
| :* <math>a</math> is a proportionality constant; equal to <math>V/n</math>
| |
| :* <math>U</math> is the [[internal energy]]
| |
| :* <math>\hat{c}_V</math> is the dimensionless specific [[heat capacity]] at constant volume, ≈ 3/2 for [[monatomic gas]], 5/2 for [[diatomic]] gas and 3 for more complex molecules.
| |
| In order to switch from macroscopic quantities (left hand side of the following equation) to microscopic ones (right hand side), we use
| |
| :<math>nR=N k_B\ </math>
| |
| where
| |
| :* <math>N</math> is the number of gas particles
| |
| :* <math>k_B</math> is the [[Boltzmann constant]] (1.381×10<sup>−23</sup>J·K<sup>−1</sup>).
| |
| | |
| The probability distribution of particles by velocity or energy is given by the [[Maxwell speed distribution]].
| |
| | |
| The ideal gas law is an extension of experimentally discovered [[gas laws]]. Real [[fluid]]s at low [[density]] and high [[temperature]] approximate the behavior of a classical ideal gas. However, at lower temperatures or a higher density, a real fluid deviates strongly from the behavior of an ideal gas, particularly as it [[Condensation|condenses]] from a gas into a liquid or as it [[deposition (phase transition)|deposits]] from a gas into a solid. This deviation is expressed as a [[compressibility factor]].
| |
| | |
| The ideal gas model depends on the following assumptions:
| |
| :* The molecules of the gas are indistinguishable, small, hard spheres
| |
| :* All collisions are elastic and all motion is frictionless (no energy loss in motion or collision)
| |
| :* Newton's laws apply
| |
| :* The average distance between molecules is much larger than the size of the molecules
| |
| :* The molecules are constantly moving in random directions with a distribution of speeds
| |
| :* There are no attractive or repulsive forces between the molecules or the surroundings
| |
| | |
| The assumption of spherical particles is necessary so that there are no rotational modes allowed, unlike in a diatomic gas. The following three assumptions are very related: molecules are hard, collisions are elastic, and there are no inter-molecular forces. The assumption that the space between particles is much larger than the particles themselves is of paramount importance, and explains why the ideal gas approximation fails at high pressures.
| |
| | |
| ==Heat capacity==
| |
| The [[Heat capacity#Heat capacity of compressible bodies|heat capacity]] at constant volume of ''n'' = 1 / R mole of any gas (so that ''n R ='' 1 J·K<sup>−1</sup>), including an ideal gas is:
| |
| | |
| :<math>\hat{c}_V=T\left(\frac{\partial S}{\partial T}\right)_V=\left(\frac{\partial U}{\partial T}\right)_V </math> | |
| | |
| where ''S'' is the [[entropy]]. This is the dimensionless heat capacity at constant volume, which is generally a function of temperature due to intermolecular forces. For moderate temperatures, the constant for a monatomic gas is <math>\hat{c}_V=3/2</math> while for a diatomic gas it is <math>\hat{c}_V=5/2</math>. It is seen that macroscopic measurements on heat capacity provide information on the microscopic structure of the molecules.
| |
| | |
| The heat capacity at constant pressure of 1/R mole of ideal gas is:
| |
| | |
| :<math>\hat{c}_p =T\left(\frac{\partial S}{\partial T}\right)_p= \left(\frac{\partial H}{\partial T}\right)_p = \hat{c}_V+1</math>
| |
| | |
| where <math>H=U+pV</math> is the [[enthalpy]] of the gas.
| |
| | |
| Sometimes, a distinction is made between an ideal gas, where <math>\hat{c}_V</math> and <math>\hat{c}_p</math> could vary with temperature, and a [[perfect gas]], for which this is not the case.
| |
| | |
| ==Entropy==
| |
| Using the results of [[thermodynamics]] only, we can go a long way in determining the expression for the [[entropy]] of an ideal gas. This is an important step since, according to the theory of [[thermodynamic potential]]s, if we can express the entropy as a function of ''U'' (U is a thermodynamic potential), volume ''V'' and the number of particles ''N'', then we will have a complete statement of the thermodynamic behavior of the ideal gas. We will be able to derive both the ideal gas law and the expression for internal energy from it.
| |
| | |
| Since the entropy is an [[exact differential]], using the [[chain rule]], the change in entropy when going from a reference state 0 to some other state with entropy ''S'' may be written as <math>\Delta S</math> where:
| |
| | |
| :<math>\Delta S = \int_{S_0}^{S}dS
| |
| =\int_{T_0}^{T} \left(\frac{\partial S}{\partial T}\right)_V\!dT
| |
| +\int_{V_0}^{V} \left(\frac{\partial S}{\partial V}\right)_T\!dV | |
| </math>
| |
| | |
| where the reference variables may be functions of the [[number of particles]] ''N''. Using the definition of the [[heat capacity]] at constant volume for the first differential and the appropriate [[Maxwell's relations|Maxwell relation]] for the second we have:
| |
| | |
| :<math>\Delta S
| |
| =\int_{T_0}^{T} \frac{C_v}{T}\,dT+\int_{V_0}^{V}\left(\frac{\partial P}{\partial T}\right)_VdV.
| |
| </math>
| |
| | |
| Expressing <math>C_V</math> in terms of <math>\hat{c}_V</math> as developed in the above section, differentiating the ideal gas equation of state, and integrating yields:
| |
| | |
| :<math>\Delta S
| |
| = \hat{c}_VNk\ln\left(\frac{T}{T_0}\right)+Nk\ln\left(\frac{V}{V_0}\right)
| |
| </math>
| |
| | |
| which implies that the entropy may be expressed as:
| |
| | |
| :<math>S= Nk\ln\left(\frac{VT^{\hat{c}_v}}{f(N)}\right)
| |
| </math>
| |
| | |
| where all constants have been incorporated into the logarithm as ''f(N)'' which is some function of the particle number ''N'' having the same dimensions as <math>VT^{\hat{c}_v}</math> in order that the argument of the logarithm be dimensionless. We now impose the constraint that the entropy be extensive. This will mean that when the extensive parameters (''V'' and ''N'') are multiplied by a constant, the entropy will be multiplied by the same constant. Mathematically:
| |
| | |
| :<math>S(T,aV,aN)=a S(T,V,N).\,</math>
| |
| | |
| From this we find an equation for the function ''f(N)''
| |
| | |
| :<math>af(N)=f(aN).\,</math>
| |
| | |
| Differentiating this with respect to ''a'', setting ''a'' equal to unity, and then solving the differential equation yields ''f(N)'':
| |
| | |
| :<math>f(N)=\Phi N\,</math>
| |
| | |
| where <math>\Phi</math> which may vary for different gases, but will be independent of the thermodynamic state of the gas. It will have the dimensions of <math>VT^{\hat{c}_v}/N</math>. Substituting into the equation for the entropy:
| |
| | |
| :<math>\frac{S}{Nk} = \ln\left(\frac{VT^{\hat{c}_v}}{N\Phi}\right).\,</math> | |
| | |
| and using the expression for the internal energy of an ideal gas, the entropy may be written:
| |
| | |
| :<math>\frac{S}{Nk} = \ln\left[\frac{V}{N}\,\left(\frac{U}{\hat{c}_v k N}\right)^{\hat{c}_v}\,\frac{1}{\Phi}\right]</math>
| |
| | |
| Since this is an expression for entropy in terms of ''U'', ''V'', and ''N'', it is a fundamental equation from which all other properties of the ideal gas may be derived.
| |
| | |
| This is about as far as we can go using thermodynamics alone. Note that the above equation is flawed — as the temperature approaches zero, the entropy approaches negative infinity, in contradiction to the [[third law of thermodynamics]]. In the above "ideal" development, there is a critical point, not at absolute zero, at which the argument of the logarithm becomes unity, and the entropy becomes zero. This is unphysical. The above equation is a good approximation only when the argument of the logarithm is much larger than unity — the concept of an ideal gas breaks down at low values of ''V/N''. Nevertheless, there will be a "best" value of the constant in the sense that the predicted entropy is as close as possible to the actual entropy, given the flawed assumption of ideality. A quantum-mechanical derivation of this constant is developed in the derivation of the [[Sackur-Tetrode equation]] which expresses the entropy of a monatomic <math>(\hat{c}_v=3/2)</math> ideal gas. In the Sackur-Tetrode theory the constant depends only upon the mass of the gas particle. The Sackur-Tetrode equation also suffers from a divergent entropy at absolute zero, but is a good approximation for the entropy of a monatomic ideal gas for high enough temperatures.
| |
| | |
| ==Thermodynamic potentials==
| |
| {{Main|Thermodynamic potentials}}
| |
| Expressing the entropy as a function of ''T'', ''V'', and ''N'':
| |
| | |
| :<math>\frac{S}{kN}=\ln\left( \frac{VT^{\hat{c}_V}}{N\Phi}\right)</math>
| |
| | |
| The [[chemical potential]] of the ideal gas is calculated from the corresponding equation of state (see [[thermodynamic potential]]):
| |
| | |
| :<math>\mu=\left(\frac{\partial G}{\partial N}\right)_{T,P}</math>
| |
| | |
| where ''G'' is the [[Gibbs free energy]] and is equal to <math>U+PV-TS</math> so that:
| |
| | |
| :<math>\mu(T,V,N)=kT\left(\hat{c}_P-\ln\left(\frac{VT^{\hat{c}_V}}{N\Phi}\right)\right)</math>
| |
| | |
| The thermodynamic potentials for an ideal gas can now be written as functions of ''T'', ''V'', and ''N'' as:
| |
| | |
| :{|
| |
| |-
| |
| |<math>U\,</math>
| |
| |
| |
| |<math>=\hat{c}_V NkT\,</math>
| |
| |-
| |
| |<math>A=\,</math>
| |
| |<math>U-TS\,</math>
| |
| |<math>=\mu N-NkT\,</math>
| |
| |-
| |
| |<math>H=\,</math>
| |
| |<math>U+PV\,</math>
| |
| |<math>=\hat{c}_P NkT\,</math>
| |
| |-
| |
| |<math>G=\,</math>
| |
| |<math>U+PV-TS\,</math>
| |
| |<math>=\mu N\,</math>
| |
| |}
| |
| | |
| where, as before, <math>\hat{c}_P=\hat{c}_V+1</math>. The most informative way of writing the potentials is in terms of their natural variables, since each of these equations can be used to derive all of the other thermodynamic variables of the system. In terms of their natural variables, the thermodynamic potentials of a single-species ideal gas are:
| |
| | |
| :<math>U(S,V,N)=\hat{c}_V N k \left(\frac{N\Phi}{V}\,e^{S/Nk}\right)^{1/\hat{c}_V}</math>
| |
| :<math>A(T,V,N)=NkT\left(\hat{c}_V-\ln\left(\frac{VT^{\hat{c}_V}}{N\Phi}\right)\right)</math>
| |
| :<math>H(S,P,N)=\hat{c}_P Nk\left(\frac{P\Phi}{k}\,e^{S/Nk}\right)^{1/\hat{c}_P}</math>
| |
| :<math>G(T,P,N)=NkT\left(\hat{c}_P-\ln\left(\frac{kT^{\hat{c}_P}}{P\Phi}\right)\right)</math>
| |
| | |
| In [[statistical mechanics]], the relationship between the [[Helmholtz free energy]] and the [[partition function (statistical mechanics)|partition function]] is fundamental, and is used to calculate the [[thermodynamic properties]] of matter; see [http://clesm.mae.ufl.edu/wiki.pub/index.php/Configuration_integral_%28statistical_mechanics%29 configuration integral] for more details.
| |
| | |
| ==Speed of sound==
| |
| {{Main|Speed of sound}}
| |
| The speed of sound in an ideal gas is given by
| |
| :<math>c_{sound} = \sqrt{\left(\frac{\partial P}{\partial \rho}\right)_{s}} = \sqrt{\frac{\gamma P}{\rho}}=\sqrt{\frac{\gamma R T}{M}} </math>
| |
| where
| |
| :<math>\gamma \,</math> is the [[adiabatic index]] <math>(\hat{c}_P/\hat{c}_V)</math>
| |
| :<math>s \,</math> is the [[entropy]] per particle of the gas.
| |
| :<math>\rho \,</math> is the [[mass density]] of the gas.
| |
| :<math>P \,</math> is the [[pressure]] of the gas.
| |
| :<math>R \,</math> is the [[universal gas constant]]
| |
| :<math>T \,</math> is the [[temperature]]
| |
| :<math>M \,</math> is the [[molar mass]] of the gas.
| |
| | |
| == Table of ideal gas equations ==
| |
| See [[Table of thermodynamic equations#Ideal gas|Table of thermodynamic equations: Ideal gas]].
| |
| | |
| ==Ideal quantum gases==
| |
| | |
| In the above mentioned Sackur-Tetrode equation, the best choice of the entropy constant was found to be proportional to the quantum [[thermal wavelength]] of a particle, and the point at which the argument of the logarithm becomes zero is roughly equal to the point at which the average distance between particles becomes equal to the thermal wavelength. In fact, [[Quantum mechanics|quantum]] theory itself predicts the same thing. Any gas behaves as an ideal gas at high enough temperature and low enough density, but at the point where the [[Sackur-Tetrode equation]] begins to break down, the gas will begin to behave as a quantum gas, composed of either [[bosons]] or [[fermions]]. (See the [[gas in a box]] article for a derivation of the ideal quantum gases, including the ideal Boltzmann gas.)
| |
| | |
| Gases tend to behave as an ideal gas over a wider range of pressures when the temperature reaches the [[Boyle temperature]].
| |
| | |
| ===Ideal Boltzmann gas===
| |
| | |
| The ideal Boltzmann gas yields the same results as the classical thermodynamic gas, but makes the following identification for the undetermined constant Φ:
| |
| | |
| :<math>\Phi = \frac{T^{3/2}\Lambda^3}{g}</math>
| |
| | |
| where Λ is the [[thermal de Broglie wavelength]] of the gas and ''g'' is the [[degenerate energy level|degeneracy]] of states.
| |
| | |
| ===Ideal Bose and Fermi gases===
| |
| | |
| An ideal [[Bose gas|gas of bosons]] (e.g. a [[photon gas]]) will be governed by [[Bose-Einstein statistics]] and the distribution of energy will be in the form of a [[Bose-Einstein distribution]]. An ideal [[Fermi gas|gas of fermions]] will be governed by [[Fermi-Dirac statistics]] and the distribution of energy will be in the form of a [[Fermi-Dirac distribution]].
| |
| | |
| ==See also==
| |
| *[[Compressibility factor]]
| |
| *[[Dynamical billiards]] - billiard balls as a model of an ideal gas
| |
| *[[Table of thermodynamic equations]]
| |
| *[[Scale-free ideal gas]]
| |
| | |
| ==References==
| |
| {{Reflist}}
| |
| | |
| {{DEFAULTSORT:Ideal Gas}}
| |
| <!-- [[Category:Thermodynamics]] redundant -->
| |
| [[Category:Ideal gas| ]]
| |