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翻訳と辞書　辞書検索 [ 開発暫定版 ] スポンサード リンク Virial expansion ： ウィキペディア英語版 Virial expansion The classical virial expansion expresses the pressure of a many-particle system in equilibrium as a power series in the density. The virial expansion, introduced in 1901 by Heike Kamerlingh Onnes, is a generalization of the ideal gas law. He wrote that for a gas containing $N$ atoms or molecules, :$$ \frac = \rho + B_2(T) \rho^2 +B_3(T) \rho^3+ \cdots, where $p$ is the pressure, $k\_B$ is the Boltzmann constant, $T$ is the absolute temperature, and $\backslash rho\; \backslash equiv\; N/V$ is the number density of the gas. Note that for a gas containing a fraction $n$ of $N\_A$ (Avogadro's number) molecules, truncation of the virial expansion after the first term leads to $pV\; =\; n\; N\_A\; k\_B\; T\; =\; nRT$, which is the ideal gas law. Writing $\backslash beta=(k\_T)^$, the virial expansion can be written as :$\backslash frac=1+\backslash sum\_^B\_(T)\backslash rho^$. The virial coefficients $B\_i(T)$ are characteristic of the interactions between the particles in the system and in general depend on the temperature $T$. Virial expansion can also be applied to aqueous ionic solutions, as shown by Harold Friedman. == See also == *Virial theorem *Statistical mechanics *Equation of state 抄文引用元・出典: フリー百科事典『 ウィキペディア（Wikipedia）』 ■ウィキペディアで「Virial expansion」の詳細全文を読む スポンサード リンク 翻訳と辞書 : 翻訳のためのインターネットリソース Copyright(C) kotoba.ne.jp 1997-2016. All Rights Reserved.