CHEE 311 J.S. Parent 1 8. Solute (1) / Solvent (2) Systems 12.7 SVNA Until now, all the components we have considered in VLE calculations have been below their critical temperature. Their pure component liquid fugacity is calculated using: Our VLE equation that describes the distribution of each component between liquid and vapour has the form: How do we deal with components that, at the temperature of interest, are above T c and no longer have a P i sat ? RT ) P P ( V exp P f sat i liq i sat i sat i liq i RT ) P P ( V exp P x f x P ˆ y sat i l sat i sat i i i l i i i v i i i
8. Solute (1) / Solvent (2) Systems 12.7 SVNA. Until now, all the components we have considered in VLE calculations have been below their critical temperature. Their pure component liquid fugacity is calculated using: - PowerPoint PPT Presentation
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CHEE 311 J.S. Parent 1
8. Solute (1) / Solvent (2) Systems 12.7 SVNA
Until now, all the components we have considered in VLE calculations have been below their critical temperature. Their pure component liquid fugacity is calculated using:
Our VLE equation that describes the distribution of each component between liquid and vapour has the form:
How do we deal with components that, at the temperature of interest, are above Tc and no longer have a Pi
sat?
RT
)PP(VexpPf
sati
liqisat
isati
liqi
RT
)PP(VexpPx
fxPˆysati
lsati
satiii
liii
vii
i
CHEE 311 J.S. Parent 2
VLE Above the Critical Point of Pure Components
CHEE 311 J.S. Parent 3
Pure Species Fugacity of a Solute
The difficulty in handling a component that is above its critical temperature or simply unstable as a pure liquid is to define a pure component fugacity for the purpose of VLE calculations.
While this component must have a liquid solution fugacity, f1
l, it does not havea pure liquid fugacity, f1
l atx1 = 1.
The tangent line at x1=0 isthe Henry’s constant, k1.It is useful for predicting the mixture fugacity of a dilutecomponent, but it cannotbe extrapolated to x1=1with any degree of accuracy.
CHEE 311 J.S. Parent 4
Pure Component Fugacity of a Solute
The pure component fugacity of a solute is calculated from a combination of Henry’s Law and an activity coefficient model.
Recall that Henry’s Law may be used to represent the mixture fugacity of a minor (xi<0.02) component in a liquid.
defines the Henry’sconstant
andis accurate as longas x1 < 0.02
Unfortunately, we cannot extrapolate the above equation to x1 = 1 to give us the pure component f1.
An activity coefficient model can refine this approach
1
l1
0x1 x
f̂limk1
11l1 xkf̂
CHEE 311 J.S. Parent 5
Pure Component Fugacity of a Solute
Recall that the activity coefficient is the ratio of the mixture fugacity of a component to its ideal solution fugacity:
At infinite dilution (x10), the activity coefficient becomes:
Since the pure component fugacity is a constant at a given T, we can write this expression as:
Using the definition of the Henry’s Constant, ki, we have:
or 12.34
l11
l1
0x1
0x1
fx
f̂limlim11
1
l1
0xl1
1 xf̂
limf
1
1
l1
11
f
k
1
1l1
kf
l11
l1
1 fx
f̂
CHEE 311 J.S. Parent 6
Pure Component Fugacity of a Solute
Equation 12.34 is a rigorous thermodynamic equation,
12.34
for the fugacity of a “pure” solute. However, it is evaluated at P2sat
(where x1 = 0) and its use requires us to assume that pressure has an insignificant influence on the solute’s fugacity.
To apply 12.34, we require a Henry’s constant for the system at the temperature of interest, ki(T), and an excess Gibbs energy model for the system, also at the T of interest.
1
1l1
kf
CHEE 311 J.S. Parent 7
VLE Relationship for a Supercritical Component
Consider a system where one component is above Tc (species 1) and the other component is below Tc (species 2).
The equilibrium relationship for component 2 is unchanged:
or
However, component 1 is handled differently, using a Henry’s constant (k1) and the infinite dilution activity coefficient (1
). Both are properties specific to this mixture.
12.36
RT
)PP(VexpPxPˆy
sat2
lsat2
sat222
v22
2
1
111
v11
kxPˆy
sat22222 PxPy
CHEE 311 J.S. Parent 8
Solute (1) / Solvent (2) Systems: Example
Carbon Dioxide(1) / n-butane(2) at 71C
0
10
20
30
40
50
60
70
80
90
0.000 0.200 0.400 0.600 0.800 1.000
x1, y1
Pre
ss
ure
(b
ar)
P-x1
P-y1
CHEE 311 J.S. Parent 9
9. Phase Stability and Liquid-Liquid Equilibria
Throughout the course we have developed methods of calculating the thermodynamic properties of different systems:
Gibbs energy of pure vapours and liquids Gibbs energy of ideal and real mixtures Definition of vapour liquid equilibrium conditions
As we apply these methods, we assume that the phases are stable.
Recall our calculation of the Gibbs energy of a hypothetical liquid while developing Raoult’s law.
In our flash calculations that we calculated Pdew and Pbubble before assuming that two phases exist
A slight extension of the thermodynamic theory covered in CHEE 311 provides us with a means of assessing the stability of a phase.
Answers the question: “Will the system actually exist in the state I have chosen?”
CHEE 311 J.S. Parent 10
Phase Stability
A system at equilibrium has minimized the total Gibbs energy. Under some conditions (relatively low P, high T) it assumes a
vapour state Under others (relatively high P, low T) the system exists as a
liquid Mixtures at specific temperatures and pressures exist as a
liquid and vapour in equilibrium
Consider the mixing of two, pure liquids. We can observe two behaviours:
complete miscibility which creates a single liquid phase partial miscibility which creates two liquid phases
» in the extreme case, these phases may be considered completely immiscible.
CHEE 311 J.S. Parent 11
Stability and the Gibbs Energy of Mixing
We have already discussed the property changes of mixing, in particular the Gibbs energy of mixing.
Before After
GA GB G
nA moles nB moles nA + nB moles liquid A liquid B of mixture
The Gibbs energy of mixing is defined as:
which in terms of mole fractions becomes:
+
BBAABAmixBA GnGnG)nn(G)nn(
BBAAmix GxGxGG
CHEE 311 J.S. Parent 12
Stability and the Gibbs Energy of Mixing
The mixing of liquids changes the Gibbs energy of the system by:
Clearly, this quantity must be negative if mixing is to occur, meaning that the mixed state is lower in Gibbs energy than the unmixed state.
i
iiimix xlnxRTG
CHEE 311 J.S. Parent 13
Stability Criterion Based on Gmix
If the system can lower its Gibbs energy by splitting a single liquid phase into two liquids, it will proceed towards this multiphase state.
A criterion for single phase stability can be derived from a knowledge of the composition dependence of Gmix.
For a single phase to be stable at a given temperature, pressure and composition:
Gmix and its first and second derivatives must be continuous functions of x1
The second derivative of Gmix must satisfy:
14.50
dx
)RT/G(d21
mix2
CHEE 311 J.S. Parent 14
Phase Stability Example: Phenol-WaterTemp 298 K Composition: Phase Property Data: