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**Advanced Thermodynamics Note 11 Solution Thermodynamics: Applications**

Lecturer: 郭修伯

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**Liquid-phase properties from VLE data**

Fugacity For species i in the vapor mixture: Vapor/liquid equilibrium: The vapor phase is assumed an ideal gas: Therefore: The fugacity of species i (in both the liquid and vapor phases) is equal to the partial pressure of species i in the vapor phase. Its value increases from zero to Pisat for pure species i

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Fig. 12.1 Table 12.1 The first three columns are P-x1-y1 data. Columns 4 and 5 are: Column 6 is:

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Fig 12.3 Fig 12.2 Henry’s constant, the limiting slope of the curve at xi = 0. Henry’s law expresses: , it is approximate valid for small values of xi

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**Henry’s law Lewis/Randall rule Gibbs/Duhem equation x1 → 0 x2 → 1**

Gibbs/Duhem equation for binary mixture at const. T and P: The Lewis/Randall rule, Division by dx1 when x1 = 1, limit

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Excess Gibbs energy Table 12.2 Column 6:

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Fig. 12.5 Positive deviation from Raoult’s law behavior: The dimensionless excess Gibbs energy: The value of GE/RT is zero at both x1= 0 and x1 =1

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**From Fig 12.5(b), linear relation:**

Similarly, The Margules equations Limiting conditions:

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VLE data for diethyl ketone (1) / n-hexane (2) at 65°C are given in the first three columns of Table Reduce the data. Table 12.4 Fig 12.7 The solid lines. Not consistency! Omit Barker’s method Fig 12.7(b) for (GE/x1x2RT) fitting:

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**Models for the excess Gibbs energy**

weak GE/RT = f (T, P, composition) At constant T: Data fitting, convenient, but only for binary system The Redlich/Kister expansion The Margules equation The van Laar equation

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**Local composition models**

Can be applied to multi-component systems The Wilson equation: The NRTL(Non-Random-Two-Liquid) equation: The UNIQUAC equation and the UNIFAC method: App. H.

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**Property changes of mixing**

Excess properties The M change of mixing Because of their direct measurability, V and H are the property changes of mixing of major interest.

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Fig 12.10

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The excess enthalpy (heat of mixing) for liquid mixture of species 1 and 2 at fixed T and P is represented by the equation: Determine expressions for and as functions of xi. The partial properties:

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Fig 12.13 1. Each ΔM is zero for a pure species. 2. The Gibbs energy change of mixing ΔG is always positive. 3. The entropy change of mixing ΔS is positive.

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**Heat effects of mixing processes**

Heat of mixing: For binary systems: When a mixture is formed, a similar energy change occurs because interactions between the force fields of like and unlike molecules are different. Heat of solution based on 1 mol of solute dissolve in liquids:

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**Calculate the heat of formation of LiCl in 12 mol of H2O at 25°C.**

Fig 12.14

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A single-effect evaporator operating at atmospheric pressure concentrates a 15% (by weight) LiCl solution to 40%. The feed enters the evaporator at the rate of 2 kg/s at 25°C. The normal boiling point of a 40% LiCl solution is about 132°C, and its specific heat is estimated as 2.72 kJ/kg °C. What is the heat transfer rate in the evaporator? Feed at 25°C 2 kg/s 15% LiCl 1.25 kg superheated steam at 132°C and 1 atm 0.75 kg 40% LiCl at 132°C Q The energy balance: the total enthalpy of the product streams minus the total enthalpy of the feed stream liquid water is vaporized and heated to 132°C 0.75 kg of 40% LiCl solution is heated to 132°C mixing of 0.45 kg of water with 0.30 kg of LiCl(s) to form a 40% solution at 25°C separation of 2 kg of a 15% LiCl solution into its pure constituents at 25°C

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**Enthalpy/concentration diagrams**

The enthalpy/concentration (Hx) diagram Fig 12.17

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Solid NaOH at 70°F is mixed with H2O at 70°F to produce a solution containing 45% NaOH at 70°F. How much heat must be transferred per pound mass of solution formed? Energy balance: 45% NaOH: on the basis of 1 (lbm): 0.45(lbm) of solid NaOH dissolved in 0.55 (lbm) of H2O. Fig 12.19, x1 = 0: Fig 12.19, x1 = 45%:

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