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Distillation: Vapor–Liquid Equilibria01:01

Distillation: Vapor–Liquid Equilibria

4.3K
Distillation is a separation technique that takes advantage of the boiling point properties of disparate elements in a mixture. To perform distillation, we begin by heating a miscible mixture of two liquids with a significant difference in boiling points (at least 20°C). As the solution heats up and reaches the bubble point of the more volatile component, some molecules of the more volatile component transition into the gas phase and travel upward into the condenser, which is a glass tube...
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Thermodynamics: Activity Coefficient01:24

Thermodynamics: Activity Coefficient

2.7K
Activity is the measure of the effective concentration of the species in solution. It can be expressed as the product of the molar concentration of the species and its activity coefficient. The activity coefficient is a dimensionless quantity and depends on the total ionic strength of the solution.
The activity coefficient is a measure of the deviation from ideal behavior. When the ionic strength of the solution is minimal, the activity coefficient of an ionic species is close to unity, making...
2.7K
Intermolecular Forces and Physical Properties02:56

Intermolecular Forces and Physical Properties

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26.4K
Clausius-Clapeyron Equation02:35

Clausius-Clapeyron Equation

62.3K
The equilibrium between a liquid and its vapor depends on the temperature of the system; a rise in temperature causes a corresponding rise in the vapor pressure of its liquid. The Clausius-Clapeyron equation gives the quantitative relation between a substance’s vapor pressure (P) and its temperature (T); it predicts the rate at which vapor pressure increases per unit increase in temperature.
62.3K
Van der Waals Equation01:10

Van der Waals Equation

6.1K
The ideal gas law is an approximation that works well at high temperatures and low pressures. The van der Waals equation of state (named after the Dutch physicist Johannes van der Waals, 1837−1923) improves it by considering two factors.
First, the attractive forces between molecules, which are stronger at higher densities and reduce the pressure, are considered by adding to the pressure a term equal to the square of the molar density multiplied by a positive coefficient a. Second, the volume...
6.1K
Mixtures of Gases: Dalton's Law of Partial Pressures and Mole Fractions03:03

Mixtures of Gases: Dalton's Law of Partial Pressures and Mole Fractions

43.5K
Unless individual gases chemically react with each other, the individual gases in a mixture of gases do not affect each other’s pressure. Each gas in a mixture exerts the same pressure that it would exert if it were present alone in the container. The pressure exerted by each individual gas in a mixture is called its partial pressure.
43.5K

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相关实验视频

Updated: Jan 11, 2026

High-pressure Sapphire Cell for Phase Equilibria Measurements of CO2/Organic/Water Systems
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High-pressure Sapphire Cell for Phase Equilibria Measurements of CO2/Organic/Water Systems

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对二元混合物的新热力学函数:共摩尔体积.

Kristian Polanco Olsen1, Bjørn Hafskjold2, Anders Lervik3

  • 1PoreLab, Department of Physics, Norwegian University of Science and Technology, N-7491 Trondheim, Norway.

The Journal of chemical physics
|November 14, 2025
PubMed
概括

这项研究引入了共摩尔体积,将部分摩尔体积与内在分子体积联系起来. 这种新的热力学变量为混合物特性提供了更清晰的物理解释.

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科学领域:

  • 热力学是一种热力学.
  • 物理化学 物理化学
  • 计算化学计算化学

背景情况:

  • 部分摩尔体积是标准的热力学特性,但缺乏直观的物理意义.
  • 传统的部分摩尔体积代表体积导数,而不是实际占用的分子空间.
  • 通过模拟计算的内在体积提供了分子空间的直接测量.

研究的目的:

  • 开发一种新的理论,将部分摩尔体积与内在分子体积连接起来.
  • 定义一种新的热力学变量,即共体积,将这两个概念联系起来.
  • 为了提供更直观的物理解释混合物中的热力学特性.

主要方法:

  • 开发一个新的热力学理论.
  • 欧勒定理对同质函数的应用.
  • 使用分子动力学模拟与沃罗诺伊测样来确定内在体积.

主要成果:

  • 建立了一个理论框架,将部分摩尔体积与内在 (Voronoi) 体积联系起来.
  • 引入了共体积作为一种新的热力学变量.
  • 通过分子动力学模拟,证明了共体积的有效性.

结论:

  • 共同体积成功地弥合了传统热力学特性和物理确定分子体积之间的差距.
  • 这种新变量为混合物中成分的空间贡献提供了更好的洞察力.
  • 在双相流系统中,共同分子体积与共同运动速度之间存在关系.