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Generalized Correlations for Gases (Lee-Kesler)
By: Santosh Koirala Manoj Joshi
Lauren BillingsCory Klemashevich
The Generalized Correlation for Gases
• The generalized Pitzer’s correlation is a three-parameter corresponding states method for estimating thermodynamic properties of pure, nonpolar fluids . For the compressibility factor Z, it takes the form
Z = Z0 + ω Z1
where,
Z0 = Compressibility factor for fluids of nearly spherical molecules,
ω = Pitzer's acentric factor, and
Z1 = Corrects for nonspherical intermolecular forces.
• Appendix E provides values of Z0 and Z1 (Lee-Kessler correlations), from which Z can be calculated and, hence, the molar volume can be computed.
Virial equationsThe Virial equation (up to the second Virial coefficient) provides an approximation of Z and the equation is:
c
c
RT
BPB ˆ
2.41
6.10
10
172.0139.0
422.0083.0
ˆ
r
r
TB
TB
BBB
RT
BPZ 1
r
r
T
PBZ
ˆ1
Cont……
The virial equation (up to the Third coefficient) also provides an approximation of Z. Such virial equation is:
2
22
2
2
ˆˆ
1
ˆ
ˆ
1
ZT
PC
ZT
PBZ
TR
CPC
RT
BPB
V
C
V
BZ
r
r
r
r
c
c
c
c
5.107.21
5.100
10
00242.05539.002676.0
00313.02432.001407.0
ˆ
rr
rr
TTC
TTC
CCC
2.41
6.10
10
172.0139.0
422.0083.0
ˆ
r
r
TB
TB
BBB
Example Problem
Determine the molar volume of n-butane at 510 K and 25 bar by each of the following:
a) The ideal-gas equation, b) The generalized compressibility-factor correlation, c) Generalized correlation for using eq. 3.61, d) Equation 3.68 the third virial coefficient equation.
a
B
131.696,125
)510)(14.83( molcmP
RTV
A. By the Ideal Gas equation:
B. From the values of Tc and Pc given in Table B.1 of App. B
13
10
7.480,125
)510)(14.83)(873(.
873.0
molcmP
ZRTV
ZZZ
2.41
6.10
10
172.0139.0
422.0083.0
ˆ
ˆ1
ˆ
1
r
r
r
r
c
c
TB
TB
BBB
T
PBZ
RT
BPB
RT
BPZ
P 25barT 510KPc 37.96barTc 425.1KPr 0.658587987Tr 1.199717713ω 0.2
B0 -0.232344991B1 0.058943546
-0.220556282
Z 0.878925087
R 83.14cm3bar/molKV 1490.706167cm3/mol
Here, Excel was used to calculate the volume using second virial coefficient equation.
C. Using the Second Virial Equation
B
P 25barT 510KPc 37.96barTc 425.1K
Pr 0.658587987 Z (Guess)Z
(Calculated)Tr 1.199717713 1 0.889316ω 0.2 0.889316 0.876994
0.876994 0.875453B0 -0.232344991 0.875453 0.875258B1 0.058943546 0.875258 0.875233
-0.220556282 0.875233 0.875230.87523 0.875229
C0 0.03312865 0.875229 0.875229C1 0.006760336 0.875229 0.875229
0.034480717 0.875229 0.8752290.875229 0.8752290.875229 0.875229
R 83.14cm3bar/molK 0.875229 0.875229V 1484.438039cm3/mol 0.875229 0.875229
0.875229 0.8752290.875229 0.875229
5.107.21
5.100
10
2.41
6.10
10
2
22
2
2
00242.05539.002676.0
00313.02432.001407.0
ˆ
172.0139.0
422.0083.0
ˆ
ˆˆ
1
ˆ
ˆ
1
rr
rr
r
r
r
r
r
r
c
c
c
c
TTC
TTC
CCC
TB
TB
BBB
ZT
PC
ZT
PBZ
TR
CPC
RT
BPB
V
C
V
BZ
This is the third coefficient virial equation for the same problem. Again Excel was used to obtain the solution. The solution is again very close to the value obtained by the Lee-Kesler method.
D. Using Second and Third Virial coefficient
CC
C
Where the Virial Equation Applies
• The second coefficient virial equation works at low pressures where Z is a linear function. It is used when an approximation of a non ideal gas is needed, but at non extreme temperatures and pressures.
• The third virial coefficient equation provides another correction to the virial equation.
This graph shows the difference obtained for the Z0 value for the Lee/Kesler correlation vs. the virial coefficient equation.