Chapter 5 Solution of Thermodynamics
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Transcript of Chapter 5 Solution of Thermodynamics
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Chapter 5 Solution of Thermodynamics:
Theory and applications
Chemical Engineering Thermodynamics
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5.1 Fundamental Property Relation5.2 The Chemical Potential and Phase Equilibria5.3 Partial Properties of Solution 5.4 Ideal Gas Mixture5.5 Fugacity and Fugacity Coefficient: Pure Species and Species in Mixture/Solution5.6 Fugacity Coefficient of Gas Mixture from the Virial Equation of State5.7 Ideal Solution and Excess Properties5.8 Liquid Phase Properties from VLE data5.9 Property Changes of Mixing5.10 Heat Effects of Mixing Process
Chapter Outline
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Multi-component gases and liquids commonly undergoes composition changes by separationand mixing processes.
This chapter gives the thermodynamics applications of both gas mixtures and liquid solutions.
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5.1 Fundamental Property Relation
The definition of the chemical potential of species i in the mixture of any closed system:
jnTPi
i nnG
,,
the Gibbs energy which is the function of temperature, pressure and number of molesof the chemical species present.
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5.2 The Chemical Potential and Phase Equilibria
For a closed system consists of 2 phase inequilibrium, the mass transfer between phases may occur.
At the same P and T, the chemical potential of each species of multiple phases in equilibriumis the same for all species.
iii
.......
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5.3 Partial Properties in Solution
Partial molar property of species i in solution:
jnTPi
i nnM
M,,
iM
In a mixture solution:1) A solution properties, 2) The partial properties base on components in a solution,
iiiiiGSHVM ,,,
Pure-species properties, iiiiiGSHVM ,,,
GSHVM ,,,
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In a solution of liquids, its properties:
ii iMxM
iiiiiGSHVM ,,,GSHVM ,,,
For a binary solution, its properties:
2211MxMxM
Similarly, for separate x1 and x2;
2121
MMxMM 2211
MMMxM
(See Example 11.3)
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In a ideal gas mixture, partial molar propertiesof a species (except volume) is equal to its molar properties of the species as a pure ideal gas when the temperature is the mixture temperature and the pressure equal to its partial pressure in the mixture.
i
ig
i
ig pTMPTM ,,
5.4 Ideal Gas Mixture
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Partial pressure of a species i in ideal-gas mixture:
PyVRTy
piig
i
i
Hence, for enthalpy;ig
ii i
ig HyH
For entropy; i ii
ig
ii i
ig yyRSyS ln
For Gibbs energy;
i iiii i
ig PyyRTTyG ln
integration constant
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5.5 Fugacity and Fugacity Coefficient: Pure Species and Species in Gas Mixture or Solution of Liquids
PRTTGi
ig
iln
For pure species in ideal-gas state;
For pure species in real-gas state;
iii fRTTG ln
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Pfi
iwhere
is called fugacity coefficient of pure species.
R
i
iig
iiG
Pf
RTGG ln
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For species i in a mixture of real gases or in asolution of liquids, in equilibrium;
iiifff ˆ....ˆˆ
The fugacity of each species is the same in all phases.
For vapor-liquid equilibrium,
l
i
v
iff ˆˆ
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Pyf
i
i
i
ˆˆ
Fugacity coefficient of species i in gas mixture;
For species in gas mixture or solution of liquids,
Pxf
i
i
i
ˆˆ
Fugacity coefficient of species i in solution;
For species i in ideal-gas mixture, 1ˆ ig
i
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5.6 Fugacity Coefficient for Gas Mixture from the Virial Equation of State
j ijikjiikkkyyB
RTP 2
21ˆln
i, j, k are run over all species in gas mixture.
kkiiikikBBB 2 jjiiijij
BBB 2
0kk
0jj
0ii
etc.,ikki
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cij
ijcij
ij P
BRTB
ˆ
6.1
0 422.0083.0
rij
ij TB
10ˆijijijijBBB
2.4
1 172.0139.0
rij
ij TB
2ji
ij
ijcjcicijkTTT 1
2/1
cij
cijcij
cij V
RTZP
2cjci
cij
ZZZ
33/13/1
2
cjci
cij
VVV
(Examples 11.7, 11.8 & 11.9)
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5.7 Ideal Solution and Excess Properties
EM is defined as the difference between theactual value of solution and value from ideal solution;
idE MMM
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5.8 Liquid Phase Properties from VLE data
In a vapor which a gas mixture and a liquid solution coexist in vapor/liquid equilibrium,
For species i in vapor mixture,
Similar for species i in solution,
Pyf v
ii
v
iˆ
Pyf v
ii
l
iˆ
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In vapor-liquid equilibrium, vapor is assumed ideal gas, hence,
1ˆ ig
i
Pyffi
v
i
l
i ˆˆ
Thus, fugacity of species i (in both the liquidand vapor phases) is equal to the partialpressure of species i in the vapor phase.
Pyf11
Pyf22
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In an ideal solution,
ii
id
ifxf ˆ
By introducing a activity coefficient;
id
i
i
ii
i
i f
ffxf
ˆ
ˆˆ
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This is a mixing process for a binary system.The 2 pure species both atT and P initially separatedby a partition, and then allow to mix.
5.9 Property Changes of Mixing
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As mixing occurs,expansion accompanied by movement of piston so that P is constant.
Heat is added or removed to maintain the constant T.
When mixing is completed,the volume changed as measured by piston displacement.
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Thus, the volume change of mixing, and the enthalpy change of mixing are found from the measured quantities and .
Association with , is called the heat effect of mixing per mole of solution.
tV
VH
Q
Q
Property changes of mixing is given by;
ii
iMxMM GSHVM ,,,
H
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212211 nn
VVxVxVV
t
For volume in binary system;
For enthalpy in binary system;
212211 nn
QHxHxHH
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5.10 Heat Effects of Mixing
Heat of mixing per mole of solution;
ii
iHxHH
Solving for binary systems;
HHxHxH 2211
This equation provides the calculation of theenthalpies of binary mixture for pure species 1 and 2.
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Heat of mixing are similar in many respectto heat of reaction. When a mixture is formed,energy change occurs because interaction between the force fields of the molecules.
However, the heat of mixing are generallyMuch smaller than heats of reaction.
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Heats of Solution
When solids or gases are dissolved in liquids,the heat effect is called the heat of solution. This heat of solution is based on the dissolution of 1 mol of solute.
If species 1 is the solute, x1 is the moles ofsolute per mole of solution. Since, is the heat effect of mixing per mole of solution, is the heat effect of mixing per mole of solute.
HH~
1
~
x
HH
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Mixing processes are presented by physical-change equations, same like chemical-reactionequations.
When 1 mol of LiCl(s) is mixed with 12 mol of H2O, the process;
O)LiCl(12H)O(12H)LiCl( 22 ls
LiCl(12H2O) means a solution of 1 mol of LiCl dissolved in 12 mol of H2O, giving heat effectof the process at 25°C and 1 bar; J 33,614
~ H
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(Try Example 12.4, 12.5, 12.6, 12.7, 18.12.9)
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Tutorial 5
Smith et al., (2006)
Problem 11.19Problem 11.37Problem 12.32Problem 12.46Problem 12.59
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Assignment 5Smith et al., (2006)
Problem 11.18Problem 11.25Problem 11.40Problem 12.30Problem 12.33