
Rahimi, A., Talaie, M. (2017). Introduction of a Novel TwoDimensional Equation of State to Predict Gas Equilibrium Adsorption in HighlyNonideal Systems. Gas Processing, 5(2), 112. doi: 10.22108/gpj.2018.100147.1004Abdolazim Rahimi; Mohamad Reza Talaie. "Introduction of a Novel TwoDimensional Equation of State to Predict Gas Equilibrium Adsorption in HighlyNonideal Systems". Gas Processing, 5, 2, 2017, 112. doi: 10.22108/gpj.2018.100147.1004Rahimi, A., Talaie, M. (2017). 'Introduction of a Novel TwoDimensional Equation of State to Predict Gas Equilibrium Adsorption in HighlyNonideal Systems', Gas Processing, 5(2), pp. 112. doi: 10.22108/gpj.2018.100147.1004Rahimi, A., Talaie, M. Introduction of a Novel TwoDimensional Equation of State to Predict Gas Equilibrium Adsorption in HighlyNonideal Systems. Gas Processing, 2017; 5(2): 112. doi: 10.22108/gpj.2018.100147.1004
Introduction of a Novel TwoDimensional Equation of State to Predict Gas Equilibrium Adsorption in HighlyNonideal Systems
Article 2, Volume 5, Issue 2, Autumn 2017, Page 112
PDF (916.5 K)
DOI: 10.22108/gpj.2018.100147.1004
Authors
Abdolazim Rahimi^{1}; Mohamad Reza Talaie ^{} ^{2}
^{1}Department of Chemical Engineering, College of Engineering, University of Isfahan, Isfahan, Iran
^{2}Department of Chemical Engineering, College of Engineering, University of Isfahan, Isfahan, Iran Department of Chemical Engineering, School of Chemical, Petroleum and Gas Engineering, Shiraz University, Shiraz, Iran
Abstract
Abstract
The accurate calculations of adsorption equilibrium for multicomponent gas systems are of great importance in many applications. In this paper, five twodimensional equations of state 2DEOS, i.e. Van der Waals, Eyring, ZhouGhasemRobinson, SoaveRedlichKwong and PengRobinson, were examined to find out their abilities to predict adsorption equilibrium for pure and multicomponent gas adsorption systems. Also, a new 2DEOS named RahimiTalaie (RT) was developed for accurately predicting adsorption equilibrium of the gas mixtures having highly nonideal behavior. The pure parameters of all these equations were obtained by fitting 2DEOS into pure gasadsorption equilibrium data, and then the mixture parameters were calculated by recommended mixing rules. It was concluded that all equations were capable of accurately predicting pure adsorption equilibrium. However, among the six abovementioned 2DEOSs, RT was more successful to provide more accurate prediction of gasmixture adsorption equilibrium, especially for the mixture showing azeotrope behavior.
Keywords
Equilibrium calculation; gas adsorption; twodimensional equation of state; nonideal mixture
Full Text
Introduction
The prediction of adsorption equilibrium plays a crucial part in an adsorption bed design. One of the most important approaches to calculate gas adsorption equilibrium is using twodimensional equations of state. Many attempts have been made to develop twodimensional equations of state and apply them to perform gas adsorption equilibrium calculations. Hill (1946) described a systematic thermodynamic treatment for mobile and monolayer adsorption of gas mixtures on homogeneous surfaces. They defined a surface fugacity for each component and they have utilized Van der Waals (VDW) EOS to predict adsorption equilibrium for binary gas mixtures [1]. Payne et al. (1968) derived a twodimensional equation of state from the HirschfelderEyring modification of VDW and applied it to predict high pressure adsorption equilibrium of pure and mixed hydrocarbons on charcoal [2]. Friederich and Mullins (1972) have used VDW to predict adsorption equilibrium of a mixture of hydrocarbons on carbon black [3]. Patrekiejew et al. (1977) have developed the twodimensional forms of Eyring, RedlichKwong (RK) and PengRobinson (PR) EOSs using statistical mechanics [4]. Konno et al. (1985) have obtained an isotherm equation by modifying PR EOS [5]. Zhou (1994) introduced a general twodimensional equation of state (ZGR) and derived the fugacity equations to describe the adsorbed phase for adsorption from gas mixtures [6]. The results of ZGR has been compared with those of multicomponent Langmuir model and ideal solution theory and found out that ZGR produced better results in multicomponent gas adsorption systems. Zheng et al. (1998) proposed a modified twodimensional VDW EOS model for the prediction of multicomponent gas adsorption isotherms from corresponding singlecomponent adsorption equilibrium data. Then, they employed this equation to predict adsorption isotherms of CO–CO_{2} mixtures and CO_{2}–N_{2} mixtures on Cu(I)–NaY zeolite [7]. Pan (2004) applied 2D EOS of ZGR and PR using new mixing rules to predict the adsorption of pure gas and several binary mixtures of gases on a carbon bed utilizing. A new computational algorithm has been developed for this purpose [8]. Fitzgerald et al. (2005) employed 2DEOS of ZGR to predict the adsorption of a mixture of gases on wet Tiffany coal [9]. In that work, a modified form of Van der Waals equation was developed by adding a new term. The four key parameters of this equation were obtained based on fitting to adsorption equilibrium data of pure gases using nonlinear regression method. In addition, the results of this equation are compared with those of VDW, Eyring, ZGR, SRK and PR for adsorption equilibrium of several pure and binary systems. The main objective of the present study is to compare the results obtained by twodimensional EOS of VDW, Eyring, ZGR, SRK and PR in predicting equilibrium adsorption of pure gases and the mixtures of gases. The sets of experimental data on pure and mixture gas adsorption found in literature were introduced in tables 2 and 3. Also, it was intended to develop a powerful 2DEOS which is capable of producing more accurate results for predicting equilibrium adsorption of highly nonideal gas mixtures.
Development of RT 2D EOS
The following general 2D EOS can be developed from threedimensional equations of state (3D EOS) [10]:
(1)
Where π, A, T, R and w are spreading pressure, surface area of the adsorbent, absolute temperature, universal gas constant and the material amount adsorbed per mass of adsorbent. α and β are two parameters of this equations. Applying different values of U, W and m, which are mentioned in table 1, one can generate different types of 2DEOSs.
Table 1. The values of W, U and m for generating different types of EOSs.
w
U
m
2DEOS
0
0
0
VDW
0
0
Eyring
0
0
ZGR
0
1
1
SRK
2
1
1
PR
VW equation can be obtained by using the following equation for :
(2)
In the righthand side of the above equation, the first and second terms show repulsive and attractive energy of adsorption. By investigating equilibrium adsorption of different systems employing VDW, It was revealed that repulsive term is underpredicted and the attractive term is overpredicted overall. Thus, in order to modify these terms, the following corrections were added to the righthand side of equation 32:
(3)
(4)
Where λ is an additional parameter of the new 2D EOS. Using these two terms, the best results were obtained amongst the numerous different terms tested. As a result, the following equation was obtained for the term :
(5)
The main difference between RT and VDW is the addition of the third parameter of λ.
Mixing rule
For RT equation the following common mixing rule were applied [11]:
(6)
(7)
(8)
(9)
(10)
Where are mole fractions of the components i and j, and are the binary correction factors which can be determined by fitting the results into mixture experimental data. However, in this study these parameters were set equal to zero. Also α, β and λ are the mixture parameters and α_{i}, β_{i}, and λ_{i} are the pure parameters of the 2D EOS.
Fugacity coefficients in adsorbed phase
The fugacity coefficient relation can be derived using the following thermodynamic equation [11]:
(11)
Where Z_{a} is the compressibility factor for twodimensional adsorbate phase which is defined as follows:
(12)
Where a is defined as:
(13)
Using the above equations the following general relations for mixture fugacity coefficient of the new EOS were found:
(14)
Where Q_{1}, Q_{2} and δ are:
(15)
(16)
(17)
The term w_{j} in the above equations denotes the mass of component j in the adsorbatephase mixture. It should be differentiated from w_{jj} which is the mass of component j in the pure adsorbate phase. The fugacity coefficient relations for pure components were obtained by taking i=j=1 in the equations, as follows:
(18)
Where and w_{ii }are Fugacity coefficient and the mass of component i in the pure adsorbed phase.
For :
(19)
(20)
(21)
For :
(22)
(23)
Equilibrium calculation for purecomponent system
The equilibrium relation for pure component is in the following form:
(24)
Where isfugacity of component i in the pure gas phase. Also, k_{i} is the henry’s constant for singlecomponent adsorption which is the ratio of at very low pressures (P→0).
Taking logarithm from both sides of equation 24 yields:
(25)
Substituting the relation for pure component fugacity coefficient in adsorbed phase gives:
(26)
Knowing the values of temperature, pressure and also the parameters of α_{i}, β_{i}, k_{i} and λ_{i}, one can determine the total amount of the adsorbed phase (w_{ii}). The fugacity of pure component i in gas phase, , was calculated using 3D PR equation of state.
Determination of optimum parameters
In order to determine singlecomponent parameters,α_{i}, β_{i}, k_{i} and λ_{i}, the adsorption equilibrium several sets of experimental data found in literature for pure component adsoprtion on a particular adsorbents were used as shown in tables 2 and 3. These parameters were calculated by fitting w_{ii }determined by the 2D EOS to the experimental data for the pure systems. Then, using the mixing rules one can find the EOS parameters for a multicomponent system with a given composition.
Equilibrium calculation for a multicomponent system
The equilibrium relations used in equilibrium adsorption calculations of a multicomponent system are:
(27)
Where N_{C} is the number of components. Knowing temperature, pressure and composition one can determine gasphase composition {y_{i}} and adsorbed –phase composition {w_{i}}. Determining the multicomponent parameters of α, β and λ using the mixing rules one can calculate (using equation 14) and , which is the fugacity of component i in the gasphase mixture (using 3D PR). Substituting these values into the set of equilibrium relations (equation 27), the following system of Nc equations for N_{C} variables which are the amount of each component in adsorbed mixture (w_{i}) was obtained:
(28)
Solving the above using the iterative Newton numerical method equations one can determine the mass of each component in the adsorbed mixture (w_{i}).
Result and Discussion
The adsorption equilibrium data predicted by new 2D EOS (RT) were compared to the ones collected from literature. In order to conduct equilibrium calculations for a multicomponent system, the parameters of single component adsorption of all respective constituents are required. It means that a set of adsorption equilibrium data for a multicomponent system on a specific adsorbent cannot be employed until the singlecomponent equilibrium data of all components on that particular adsorbent are available. These data are necessary to find the singlecomponent parameters. This fact created a huge restriction on the adsorption equilibrium data released in literature. In this regard, the appropriate sets of data were collected by an extensive literature survey. In this study, 24 sets of purecomponent data containing 441 equilibrium points and 15 sets of binary data comprising 175 equilibrium points were used to compare the performances of different 2D EOSs. Table 4 compares the predictions of various 2D EOSs with each other and reported their respective relative average deviations (%RAD) which are defined as:
(29)
Where and are the calculated and experimental amount of adsorbed phase of pure component i respectively.
Table 2. The comparison of relative average deviations in predicting singlecomponent adsorption equilibrium data using various 2D EOSs.
Ref
T(K)
Adsorbate
Adsorbent
%RAD
NP
System
RT
PR
SRK
ZGR
EYRING
VDW
[12]
298.15
iC_{4}H_{10}
13X
2.88
2.92
2.94
2.84
2.86
2.90
16
1
[12]
298.15
C_{2}H_{4}
13X
3.61
4.69
4.75
4.08
4.55
5.04
30
2
[12]
323.15
iC_{4}H_{10}
13X
1.48
1.47
1.48
1.67
1.59
1.48
16
3
[12]
323.15
C_{2}H_{4}
13X
2.77
2.67
2.66
2.99
2.77
2.70
25
4
[12]
298.15
C_{2}H_{6}
13X
1.97
3.46
3.32
4.61
2.32
2.92
31
5
[12]
323.15
C_{2}H_{6}
13X
2.63
2.77
2.67
3.00
1.75
2.47
20
6
[12]
298.15
CO_{2}
13X
2.69
4.84
5.06
4.11
4.87
5.44
20
7
[12]
323.15
CO_{2}
13X
2.69
2.56
2.56
3.00
2.77
2.65
17
8
[13]
300
CH_{4}
13X
0.54
0.52
0.53
4.07
1.95
0.54
18
9
[13]
300
C_{3}H_{8}
13X
1.83
1.86
1.74
2.36
1.74
2.57
15
10
[13]
300
CH_{4}
5A
4.00
3.94
3.95
4.63
3.94
3.95
18
11
[13]
300
C_{2}H_{6}
5A
0.82
1.23
1.18
2.26
1.21
0.91
15
12
[13]
300
C_{3}H_{8}
5A
5.58
5.74
5.65
5.23
5.34
6.13
12
13
[14]
293
CO_{2}
13X
2.11
1.98
2.44
2.20
2.59
3.81
38
14
[14]
293
C_{2}H_{6}
13X
0.55
1.64
1.43
2.90
1.28
0.76
30
15
[15]
423
C_{3}H_{8}
4A
2.37
1.99
2.15
6.67
4.35
2.44
5
16
[15]
423
C_{3}H_{6}
4A
2.99
3.01
3
3.21
3.06
2.99
20
17
[15]
473
C_{3}H_{8}
4A
2.25
2.24
2.24
2.50
2.12
2.25
5
18
[15]
473
C_{3}H_{6}
4A
2.70
2.78
2.76
3.68
3.06
2.71
18
19
[16]
298
O_{2}
10X
0.51
0.50
0.50
0.59
0.53
0.50
19
20
[16]
298
N_{2}
10X
0.26
0.33
0.34
0.25
0.30
0.35
19
21
[17]
298
CH_{4}
Norit R1
.49
1.64
1.82
3.12
0.60
2.04
12
22
[17]
298
N_{2}
Norit R1
.69
0.76
0.79
5.18
2.03
.84
10
23
[17]
298
CO_{2}
Norit R1
1.63
2.87
3.07
3.28
1.58
3.36
12
24




2.09
2.51
2.54
3.14
2.47
2.67
441
TOTALL
Table 3. The comparison of relative average deviations in predicting multicomponent adsorption equilibrium data using various 2D EOSs.
Quantities
P (KPa)
T (K)
Adsorbent
Adsorbate
NAME
wi
137.8
298.15
13X Zeolite
iC_{4}H_{10}(1)C_{2}H_{4}(2)
A
w
wi
137.8
323.15
13X Zeolite
iC_{4}H_{10}(1)C_{2}H_{4}(2)
B
w
wi
137.8
298.15
13X Zeolite
iC_{4}H_{10}(1)C_{2}H_{6}(2)
C
w
wi
137.8
323.15
13X Zeolite
iC_{4}H_{10}(1)C_{2}H_{6}(2)
D
w
wi
137.8
298.15
13X Zeolite
C_{2}H_{4}(1)CO_{2}(2)
E
w
wi
137.8
323.15
13X Zeolite
C_{2}H_{4}(1)CO_{2}(2)
F
w
wi
345
300
13X Zeolite
CH_{4}(1)C_{3}H_{8}(2)
G
w
wi
345
300
5A Zeolite
CH_{4}(1)C_{2}H_{6}(2)
H
w
wi
345
300
5A Zeolite
C_{2}H_{6}(1)C_{3}H_{8}(2)
I
w
wi
101.3
293
13X Zeolite
CO_{2} (1)C_{2}H_{6}(2)
J
w
wi
84.6198.41
423
4A Zeolite
C_{3}H_{6}(1)C_{3}H_{8}(2)
K
w
wi
102.93118.99
473
4A Zeolite
C_{3}H_{6}(1)C_{3}H_{8}(2)
L
w
wi
6.3828.65
298
10X Zeolite
O_{2}(1)N_{2}(2)
M
w
w_{i}
1515975
298
Activated carbon
CH_{4}(1)N_{2}(2)
N
w
w_{i}
985916
298
Activated carbon
CH_{4}(1)CO_{2}(2)
O
w
wi
OVERALL
w
ref
NP
RT
PR
SRK
ZGR
Eyring
VDW
%RAD
[12]
10
5.69
19.77
22.25
22.70
23.35
24.65
2.20
3.21
3.54
3.50
3.70
3.86
[12]
8
5.24
9.80
16.99
10.30
9.25
8.28
2.52
4.32
3.71
4.29
4.62
3.97
[12]
10
32.21
49.51
44.03
38.16
36.54
37.43
6.07
6.69
6.79
6.77
6.38
6.38
[12]
7
22.51
34.24
33.24
30.04
29.81
31.57
5.39
4.03
3.97
4.86
4.03
4.25
[12]
6
12.70
20.57
15.36
9.67
10.24
11.51
1.06
8.03
5.82
3.18
4.00
5.72
[12]
5
8.64
17.13
14.06
18.84
8.87
9.04
1.25
5.75
4.20
1.24
1.55
3.00
[13]
8
26.95
50.97
50.91
18.45
26.67
43.94
3.41
1.90
1.71
3.88
2.99
1.68
[13]
27
14
14.77
14.18
13.45
13.71
13.90
6.04
8.35
7.64
6.06
6.24
6.62
[13]
16
22.32
19.88
20.72
21.40
21.33
20.21
6.72
7.22
6.99
6.94
6.99
6.90
[14]
6
10.25
49.31
40.4
7.23
10.09
9.90
1.81
14.21
9.31
4.19
5.030
5.09
[15]
7
11.18
11.52
9.25
14.13
12.20
11.37
2.32
4.06
3.15
2.77
2.64
2.88
[15]
6
10.85
8.98
9.46
14.82
12.50
10.89
2.97
3.80
3.45
3.99
3.44
3.26
[16]
11
10.08
10.79
11.27
6.92
33.64
11.19
2.34
4.01
3.49
9.43
18.85
1.74
[17]
24
9.51
10.60
10.56
8.37
10.46
16.64
3.69
6.16
4.54
5.78
4.12
3.72
[17]
24
18.33
20.44
20.11
18.72
18.13
22.66
2.82
6.14
4.66
3.55
2.64
3.50
175
15.04
20.79
20.22
16.36
18.22
19.10
3.87
6.11
5.17
5.13
5.37
4.44
As expected, the results obtained by all EOSs are in good agreement with the experimental data for purecomponent systems. Adsorption of propane on zeolite 5A using VDW having %RAD of 6.13 is the worst case. This table shows that RT EOS having the total relative average error of 2.09 demonstrates the best performance, while the highest total average error is associated with ZRG having the error of 3.14. Using the optimum values of the singlecomponent parameters (α_{i}, β_{i}, k_{i} and λ_{i}) obtained through the calculations related to table 4, the multicomponent parameters (α, β and λ) were determined. Table 5 shows the relative average deviations, %RAD (wi) and %RAD(w), of different 2D EOSs for binary systems. These relative errors were calculated using the following equations:
(30)
(31)
Where N_{C} is the total number of components and N_{p} is the total number of equilibrium points in a set of data. The superscript c and e stand for calculated and experimental respectively. w and w_{i} are total amount of adsorbed phase and the amount of component i in adsorbed phase respectively.
As it is apparent from Table 3, RT equation of state having %RAD (w_{i})=15.04 and %RAD(w)=3.87 reveals the best prediction among the others. PR is ranked as the worst having %RAD (w_{i})=20.79 and %RAD(w)=6.11. The good prediction of highlynonideal systems where shows azeotropic behavior is the primary advantage of the new EOS. In order to demonstrate this capability, three sets of experimental data showing highlynonideal behavior were selected to be compared with the predictions of different EOSs. For each case the singlecomponent parameters and %RAD for various EOSs are shown through the tables. Also, the variation of one component (w_{i}) and total (w) adsorbed amounts were plotted versus mole fraction of one component. Because of the limitation of the data released in literature on gas adsorption, the following three cases were considered.
Case 1: Adsorption of isobuteneethylene on zeolite 13X
Table 4. The singlecomponent parameters and %RAD for various EOSs
Adsorbate
2DEOS
NP
10^{4 }α_{i}
β_{i}
Ln k_{i}
λ_{i}
%AAD
P (KPa)
T (K)
Ref
Isobutane
VDW
16
2.286
0.4074
8.554

2.90
24137.84
298.15
[12]
Eyring
16
0.0452
0.3680
8.953

2.86
24137.84
298.15
ZGR
16
1.829
0.3439
9.993

2.84
24137.84
298.15
SRK
16
3.782
0.4135
9.069

2.94
24137.84
298.15
PR
16
4.416
0.4104
9.126

2.92
24137.84
298.15
RT
16
1.872
0.3912
8.405
0.3912
2.88
24137.84
298.15
Ethylene
VDW
30
0.4643
0.2362
5.065

5.04
24137.84
298.15
[12]
Eyring
30
0.6790
0.2093
5.612

4.55
24137.84
298.15
ZGR
30
1.802
0.1973
6.627

4.08
24137.84
298.15
SRK
30
0.6323
0.2405
5.129

4.75
24137.84
298.15
PR
30
0.7564
0.2396
5.157

4.69
24137.84
298.15
RT
30
0.3001
0.2559
6.131
2.406
3.61
24137.84
298.15
Figure 1. The variation of adsorbate mole fraction of isobutene versus gas mole fraction of isobutene.
Figure 2. the variation of total amount of adsorbate versus gas mole fraction of isobutene.
Case 2: Adsorption of carbon dioxideethylene on zeolite 13X
Table 5. The singlecomponent parameters and %RAD for various EOSs
Adsorbate
2DEOS
NP
10^{4 }α_{i}
β_{i}
Ln k_{i}
λ_{i}
%AAD
P (KPa)
T (K)
Ref
Ethylene
VDW
25
6.322
0.2108
3.887

2.70
67137.87
323.15
[12]
Eyring
25
6.527
0.1968
4.375

2.77
67137.87
323.15
ZGR
25
20.170
0.1942
5.335

2.99
67137.87
323.15
SRK
25
7.511
0.2236
3.926

2.66
67137.87
323.15
PR
25
8.822
0.2233
3.951

2.67
67137.87
323.15
RT
25
1.497
0.2479
4.210
1.419
2.77
67137.87
323.15
Carbon dioxide
VDW
17
8.398
0.0966
4.0477

2.65
0.44137.84
323.15
[12]
Eyring
17
1.120
0.1180
4.4618

2.77
0.44137.84
323.15
ZGR
17
11.470
0.1265
5.3763

3
0.44137.84
323.15
SRK
17
8.481
0.1333
4.0770

2.56
0.44137.84
323.15
PR
17
9.670
0.1356
4.1082

2.56
0.44137.84
323.15
RT
17
2.571
0.1505
4.2643
1.080
2.69
0.44137.84
323.15
Figure 3. The variation of adsorbate mole fraction of ethylene versus gas mole fraction of ethylene.
Figure 4. The variation of total amount of adsorbate versus gas mole fraction of ethylene.
Case 3: Adsorption of Nitrogenoxygen on zeolite 10X
Table 6. The singlecomponent parameters and %RAD for various EOSs
Adsorbate
2DEOS
NP
10^{4 }α_{i}
β_{i}
Ln k_{i}
λ_{i}
%AAD
P (KPa)
T (K)
Ref
Oxygen
VDW
25
12.6552
0.5593
1.852

0.505
92.9212.39
273.15
[16]
Eyring
25
67.6354
0.8062
1.368

0.537
92.9212.39
273.15
ZGR
25
128.2308
0.9011
0.3409

0.592
92.9212.39
273.15
SRK
25
11.0082
0.4634
1.855

0.504
92.9212.39
273.15
PR
25
10.7484
0.4289
1.858

0.503
92.9212.39
273.15
RT
25
32.0132
0.7882
1.831
1.244
0.510
92.9212.39
273.15
Nitrogen
VDW
17
10.8017
5.00E05
0.3447

0.351
99.5212.4
273.15
[16]
Eyring
17
0.9828
0.1212
0.0285

0.307
99.5212.4
273.15
ZGR
17
12.3812
0.1370
0.9070

0.253
99.5212.4
273.15
SRK
17
9.2520
0.0917
0.3313

0.342
99.5212.4
273.15
PR
17
9.7411
0.1022
0.3143

0.333
99.5212.4
273.15
RT
17
18.4780
0.4298
0.8526
3.199
0.262
99.5212.4
273.15
Figure 5. the variation of adsorbate mole fraction of oxygen versus gas mole fraction of oxygen.
Figure 6. The variation of total amount of adsorbate versus gas mole fraction of oxygen.
As it can be seen from figures 1 through 6 for all cases, especially for case 1, the performance of the RT EOS outreaches the rest significantly.
References
Hill, T.L. (1946). Theory of Multimolecular Adsorption from a Mixture of Gases, J. Chem. Phys., 14, 268–275.
Payne, H.K., Sturdevent, G.A. & Leland, T.W. (1963). Improved TwoDimensional Equation of State to Predict Adsorption of Pure and Mixed Hydrocarbons, Ind. Eng. Chem. Fundam., 7, 363–374.
Friederich, R.O. & Mullins, J.C. (1972). Adsorption Equilibria of Binary Hydrocarbon Mixtures on Homogeneous Carbon Black at 25° C, Ind. Eng. Chem. Fundam., 11, 439–445.
Patrykiejew, A., Jaroniec, M. & Rudzinski, W. (1978). Twodimensional Mobile Films of Gases on Solids: Adorption of Threedimensional Equation of state to Physical Adsorption of Single Gases on Homogenous Surfaces, Chem. Eng. J., 15, 147–157.
Konno, M., Terabyashi, M. & Takako, Y. (1995). Adsorption equilibria of hydrocarbon gaseous mixture containing polar components, J. Chem. Eng. Jpn., 18, 398–408.
Zhou, C. (1994). Modeling and Prediction of Pure and Multicomponent Gas Adsorption, Oklahoma State University, Stillwater.
Zheng, Y. & GU, T. (1998). Modified Van der Waals equation for the prediction of gas multicomponent isotherm, J. Colloid Interface Sci., 206, 457–463.
Pan, Z. (2004). Modeling of gas adsorption using TwoDimensional equation of state, Oklahoma State University, Stillwater, 2004.
Fitzgerald, J.E., Pan, Z., Sudibandriyoa, M., Robinson, R.L., Gasem, K.A.M. & Reevesb, S. (2005). Adsorption of methane, nitrogen, carbon dioxide and their mixtures on wet Tiffany coal, Fuel, 84, 2351–2363.
De Boer, J. H. (1953). Dynamical Character of Adsorption. Clarendon Press: London.
Ross, S., & Olivier, J. P. (1964). On Physical Adsorption. Interscience Publishers, New York.
Hyun, S. H. & Danner, R.O. (1989). Equilibrium Adsorption of Ethane, Ethylene, Isobutane, Carbon Dioxide, and Their Binary Mixtures on 13X Molecular Sieves, J. Chem. Eng. Data, 27, 196–200.
Loughlin, K.F, Hasanian, M.A. & AbdulRehman, H.B (1990). Ternary, Binary, and Pure Component Sorption on Zeolites. 2. Light Alkanes on Linde 5A and 13X Zeolite at Moderate to High Pressures., J. Ind. Eng. Chem. Res., 29, 1535–1546.
Siperstein, F.R. & Myesr, A.L. (2001). MixedGas Adsorption, AICHE J., 47, 1141–1159.
Grande, C.A., Gigola, C. & Rodrigues, A.E. (2003). PropanePropylene Binary Adsorption on Zeolite 4A, Adsorption, 9, 321–329.
Nolan, T. J, Mckeehan, W. & Danner, P.R. (1981). Equilibrium Adsorption of Oxygen. Nitrogen, Carbon Monoxide, and Binary Mixture on Molecular Sieve Type 10X , J. Chem. Eng. Data, 26, 112–115.
StatisticsArticle View: 160PDF Download: 169