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Distillation: Vapor–Liquid Equilibria01:01

Distillation: Vapor–Liquid Equilibria

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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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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.
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Phase Diagrams02:39

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A phase diagram combines plots of pressure versus temperature for the liquid-gas, solid-liquid, and solid-gas phase-transition equilibria of a substance. These diagrams indicate the physical states that exist under specific conditions of pressure and temperature and also provide the pressure dependence of the phase-transition temperatures (melting points, sublimation points, boiling points). Regions or areas labeled solid, liquid, and gas represent single phases, while lines or curves represent...
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Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and standard pressure, a piece of dry ice (solid CO2) sublimes, appearing to gradually disappear without ever forming any liquid. Snow and ice sublimate at temperatures below the melting point of water, a slow process that may be accelerated by winds and the reduced atmospheric pressures at high altitudes. When solid iodine is warmed, the solid sublimes...
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Phase Transitions: Melting and Freezing02:39

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Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy becomes large enough to partially overcome the forces holding the molecules or ions of the solid in their fixed positions, and the solid begins the process of transitioning to the liquid state or melting. At this point, the temperature of the solid stops rising, despite the continual input of heat, and it remains constant until all of the solid is...
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The phase of a given substance depends on the pressure and temperature. Thus, plots of pressure versus temperature showing the phase in each region provide considerable insights into the thermal properties of substances. Such plots are known as phase diagrams. For instance, in the phase diagram for water (Figure 1), the solid curve boundaries between the phases indicate phase transitions (i.e., temperatures and pressures at which the phases coexist).
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Thermodynamic models for predicting and correlating solid-liquid phase equilibrium.

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  • 1National Engineering Research Center of Industrial Crystallization Technology, School of Chemical Engineering and Technology, Tianjin University, Tianjin 300072, China. wangna224@tju.edu.cn.

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Thermodynamic models are crucial for predicting substance behavior and optimizing chemical processes. This review details widely used models for solubility prediction, highlighting their strengths, limitations, and future development needs.

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Area of Science:

  • Chemical Engineering
  • Physical Chemistry
  • Materials Science

Background:

  • Thermodynamic models are essential for predicting substance behavior under varying temperatures.
  • Accurate prediction of solid-liquid phase equilibria reduces experimental costs and enhances product design efficiency.
  • Current models for solubility prediction have limitations, necessitating a comprehensive review.

Purpose of the Study:

  • To review widely used thermodynamic models in chemical engineering.
  • To detail the applicability and predictive performance of these models across diverse systems.
  • To identify key limitations and challenges associated with current thermodynamic models.

Main Methods:

  • Literature review of established thermodynamic models.
  • Analysis of model performance for organic compounds, inorganic salts, and multicomponent mixtures.
  • Discussion of specific solubility scenarios and successful prediction contexts.

Main Results:

  • Various thermodynamic models exhibit different applicability and predictive performance.
  • Models show varying success in predicting solubility for different compound types and mixtures.
  • Key limitations and challenges in current model development are identified.

Conclusions:

  • Thermodynamic models are vital but require further development for broader applicability.
  • Future models should be modular, comprehensible, and easily updatable for industrial use.
  • Improved models will enhance efficiency in process development, optimization, and design.