Page 280 - Characterization and Properties of Petroleum Fractions - M.R. Riazi

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AT029-06
260 CHARACTERIZATION AND PROPERTIES OF PETROLEUM FRACTIONS
TABLE 6.10—(Continued)
3 1/2
3
Compound
Formula
M
No. AT029-Manual AT029-Manual-v7.cls June 22, 2007 20:46 T M ,K H f /RT M at T M V 25 ,cm /mol δ 25 , (J/cm )
N C
62 n-Hexadecylbenzene C 22 H 38 22 302.55 300.15 22.1207 356.160 16.39
63 n-Heptadecylbenzene C 23 H 40 23 316.55 305.15 22.9782 373.731 16.30
64 n-Octadecylbenzene C 24 H 42 24 330.58 309.00 23.7040 390.634 16.24
1-n-Alkylnaphthalenes (aromatics)
65 Naphthalene C 10 H 8 10 128.16 353.43 6.4588 123.000 19.49
66 1-Methylnaphthalene C 11 H 10 11 142.19 242.67 3.4420 139.899 19.89
67 1-Ethylnaphthalene C 12 H 12 12 156.22 259.34 7.5592 155.579 19.85
68 1-n-Propylnaphthalene C 13 H 14 13 170.24 264.55 7.9943 172.533 19.09
69 1-n-Butylnaphthalene C 14 H 16 14 184.27 253.43 11.9117 189.358 19.10
70 1-n-Pentylnaphthalene C 15 H 18 15 198.29 248.79 11.3121 205.950 18.85
71 1-n-Hexylnaphthalene C 16 H 20 16 212.32 255.15 . . . 224.155 18.72
72 1-n-Nonylnaphthalene C 19 H 26 19 254.40 284.15 . . . 272.495 17.41
73 1-n-Decylnaphthalene C 20 H 28 20 268.42 288.15 . . . 289.211 17.20
Other organic compounds
74 Benzoic acid C 7 H 6 O 2 7 122.12 395.52 5.4952 112.442 24.59
75 Diphenylmethane C 13 H 12 13 168.24 298.39 7.3363 167.908 19.52
76 Antheracene C 14 H 10 14 190.32 488.93 7.7150 182.900 17.75
Nonhydrocarbons
77 Water H 2 O . . . 18.02 273.15 2.6428 18.0691 47.81
78 Methanol CH 3 OH 1 32.04 −97.68 0.2204 40.58 29.59
79 Ethanol C 2 H 5 OH 2 46.07 −114.1 0.3729 58.62 26.13
80 Isobutanol C 4 H 9 OH 4 74.12 −108.0 0.4634 . . . 22.92
81 Carbon dioxide CO 2 1 44.01 216.58 5.0088 37.2744 14.56
82 Hydrogen sulfide H 2 S . . . 34.08 187.68 1.5134 35.8600 18.00
83 Nitrogen N 2 . . . 28.01 63.15 1.3712 34.6723 9.082
84 Hydrogen H 2 . . . 2.02 13.95 1.0097 28.5681 6.648
85 Oxygen O 2 . . . 32.00 54.36 0.9824 28.0225 8.182
86 Ammonia NH 3 . . . 17.03 195.41 3.4819 24.9800 29.22
87 Carbon monoxide CO 1 28.01 68.15 1.4842 35.4400 6.402
a API-TDB [11] gives different values for V 25 of light hydrocarbons. These values are given in parentheses and seem more accurate, as also given in Table 6.11.
Values in this table are obtained from a program in Ref. [13].
2
L
should be noted that the polynomial correlation given for n- Laar theory since by replacing A 12 = (V /RT)(δ 1 − δ 2 ) and
1
2
L
alkylbenzenes cannot be used for compounds heavier than A 21 = (V /RT)(δ 1 − δ 2 ) into Eq. (6.144), it becomes identical
2
C 24 . The other two equations may be extrapolated to heavier to Eq. (6.145). However, the main advantage of Eq. (6.145)
compounds. Equations (6.148) and (6.149) may be used to- over Eq. (6.144) is that parameters V i L and δ i are calcula-
gether with the pseudocomponent method described in Chap- ble from thermodynamic relations. Riazi and Vera [23] have
ter 3 to estimate V 25 and δ for petroleum fractions whose shown that predicted values of solubility are sensitive to the
molecular weights are in the range of application of these values of V and δ i and they have recommended some specific
L
i
L
equations. Values of V and δ given in Table 6.10 are taken values for δ i of various light gases in petroleum fractions.
i
from Ref. [13] at temperature of 25 C. It seems that for some Other commonly used activity coefficient models include
◦
light gases (i.e., CH 4 ), there are some discrepancies with re- Wilson and NRTL (nonrandom two-liquid) models, which
ported values in other references. Values of these properties are applicable to systems of heavy hydrocarbons, water, and
for some compounds as recommended by Pruasnitz et al. [21]
are given in Table 6.11. Obviously at 25 C, for light gases such
◦
as CH 4 or N 2 values of liquid properties represent extrapo- TABLE 6.11—Values of liquid molar volume and solubility
parameters for some pure compounds at 90 and 298 K.
lated values and for this reason they vary from one source to Compound V , (cm /mol) δ i , (J/cm )
3
L
3 1/2
another. It seems that values given in Table 6.10 for light gases N 2 (at 90 K) i 38.1 10.84
correspond to temperatures lower than 25 C. For this reason N 2 (at 298 K) 32.4 5.28
◦
for compounds such as C 1 ,C 2 ,H 2 S, CO 2 ,N 2 , and O 2 values CO (at 90 K) 37.1 11.66
L
of V and δ at 25 C as given in Table 6.11 are recommended CO (at 298 K) 32.1 6.40
◦
i
to be used. O 2 (at 90 K) 28.0 14.73
33.0
8.18
O 2 (at 298 K)
For multicomponent solutions, Eqs. (6.145) and (6.146) are CO 2 (at 298 K) 55.0 12.27
replaced by the following relation: CH 4 (at 90 K) 35.3 15.14
CH 4 (at 298 K) 52.0 11.62
L
V (δ i − δ mix) 2 C 2 H 6 (at 90 K) 45.7 19.43
i
ln γ i =
RT C 2 H 6 (at 298 K) 70.0 13.50
Taken from Ref. [21]. Components N 2 , CO, O 2 ,CO 2 ,CH 4 ,andC 2 H 6 at
(6.150) δ mix = j δ j 298 K are in gaseous phase (T c < 298 K) and values of V and δ i are
L
i
j hypothetical liquid values which are recommended to be used. Values
x j V L j given at 90 K are for real liquids. All other components are in liquid form
j = x k V L at 298 K. Values reported for hydrocarbons heavier than C 5 are similar
k k to the values given in Table 6.10. For example, for n-C 16 it provides
L
where the summation applies to all components in the mix- values of 294 and 16.34 for V and δ i , respectively. Similarly for benzene
i
values of 89 and 18.8 were provided in comparison with 89.48 and 18.7
ture. Regular solution theory is in fact equivalent to van given in Table 6.10.
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