Heat capacities near room temperature of ten solid alkane-α, ω-diols HO-(CH2)n-OH where n = 6 and 8 ≤ n ≤ 16

Article abstract of DOI:10.1006/jcht.1998.0470

The molar heat capacities at constant pressure Cp,m of a homologous series of alkane-α, ω-diols HO-(CH₂)_n-OH, where n has values of 6 and (8 to 16), were determined by using differential scanning calorimetry over the temperature range (280 to 310) K, in flowing gas. The measured values of C_p,m showed a very good linear dependence on temperature, except 1,9-nonanediol and 1,13-tridecanediol. The heat capacities at T = 298.15 K were obtained by interpolating the smoothed fitting equations as a function of temperature. The contribution to the heat capacity at T = 298.15 K of the CH₂ group was derived from the slope of the C_p,m values of diols as a function of the number of carbon atoms in their molecules, and compared with the values obtained from a comprehensive collection of literature data for homologous alkyl organic compounds in the solid state. 1999 Academic Press.

Full text of DOI:10.1006/jcht.1998.0470

J. Chem. Thermodynamics 1999, 31, 537–546
Article No. jcht.1998.0470
Available online at http://www.idealibrary.com on
Heat capacities near room temperature of ten
solid alkane-α, ω-diols HO–(CH2)n–OH where
n = 6 and 8 6 n 6 16
Giuseppe Della Gatta,a
Dipartimento di Chimica IFM, Universita` di Torino, Via P. Giuria 9, 10125
Turin, Italy
Maꢀlgorzata Jo´z´wiak,
Katedra Chemii Fizycznej, Uniwersytet Lꢀ o´dz´ki, Pomorska 165, 91-236 Lꢀ o´dz´,
Poland
and Paolo Ferloni
Dipartimento di Chimica Fisica/CSTE-CNR, Universita` di Pavia, Viale
Taramelli 16, 27100 Pavia, Italy
The molar heat capacities at constant pressure C
of a homologous series of alkane-α, ω-
p,m
diols HO–(CH ) –OH, where n has values of 6 and (8 to 16), were determined by using
2
n
differential scanning calorimetry over the temperature range (280 to 310) K, in flowing
gas. The measured values of C showed a very good linear dependence on temperature,
p,m
except 1,9-nonanediol and 1,13-tridecanediol. The heat capacities at T = 298.15 K were
obtained by interpolating the smoothed fitting equations as a function of temperature. The
contribution to the heat capacity at T = 298.15 K of the CH group was derived from
2
the slope of the C
values of diols as a function of the number of carbon atoms in their
p,m
molecules, and compared with the values obtained from a comprehensive collection of
literature data for homologous alkyl organic compounds in the solid state.
c
ꢀ1999 Academic Press
KEYWORDS: alkane-α, ω-diols; methylene group; heat capacity; differential scanning
calorimetry
1. Introduction
Simple organic compounds, including alkanediols,(1) are useful model systems for solute–
solventinteractionsindilutesolution. However, ofthedataneededtoobtainacomprehensive
thermodynamic description of the process, molar heat capacities Cp,m of pure solutes are
often missing from the literature. These quantities are employed to convert to T = 298.15 K,
a
To whom correspondence should be addressed (E-mail: dellagatta@ch.unito.it).
c
0021–9614/99/040537 + 10 $30.00/0
ꢀ 1999 Academic Press

538
G. Della Gatta, M. Jo´z´wiak, and P. Ferloni
both enthalpies of vaporization or sublimation measured at other temperatures for liquid or
solid solutes, and hence derive their standard enthalpies of solvation(2) by using enthalpies of
solution at infinite dilution. They can also be employed to obtain partial molar heat capacities
ofsolutesthroughadditiontothechangesofheatcapacityduetosolutionprocessesatinfinite
dilution.(3)
As a part of our study on the thermodynamic properties of a number of series of organic
compounds,(4–15) this work reports the molar heat capacities measured by using differential
scanning calorimetry (d.s.c.) near room temperature of ten solid alkane-α, ω-diols, with
the general formula HO–(CH2)n–OH, namely 1,6-hexanediol, and 1,8-octanediol to 1,16-
hexadecanediol. To our knowledge, no previous heat capacities of solid terminal diols
at T = 298.15 K are available in the literature, except for 1,6-hexanediol(16) and 1,10-
decanediol.(17) Furthermore, these results contribute to an evaluation of the contribution to
the heat capacity of the CH2 group in solid alkyl compounds.
2. Experimental
The alkane-α, ω-diols investigated were analytical grade reagents from various suppliers.
Original mass fraction purities (when indicated) ranged from 0.98 to 0.99, and are listed
in table 1. Only those terminal diols that are solid at room temperature were considered
in this work, from N(C) = 6 to N(C) = 16, where N(C) denotes the number of C
atoms in the molecule, but 1,7-heptanediol N(C) = 7 was omitted because it melts at
T ≈ 290 K. All commercial products were purified by successive crystallizations from
(water + ethanol) or absolute ethanol solutions, except 1,14-tetradecanediol, which was
used as received. Since 1,13-tridecanediol is not commercially available, we prepared this
compound in our laboratory by reduction of 1,11-undecandicarboxylic acid (Pfaltz & Bauer)
by LiAlH4 (Aldrich, powder, mass fraction 0.95) in a tetrahydrofuran (Aldrich, anhydrous,
mass fraction 0.999) solution. The precipitated compound was then purified by up to seven
crystallizations from absolute ethanol and repeated sublimations.
All the samples were subjected to prolonged drying in a vacuum oven and in most cases
the final purification of the samples also included sublimation under vacuum. Purities were
determined by the d.s.c. peak profile method(18, 19) and are reported in the last column of
table 1. The procedures adopted significantly increased the purity despite the well-known
difficulty of purifying this class of compound. The final mass fraction of our samples was
sometimes better than 0.995, but did not reach the excellent values we have obtained in
other cases, e.g. for N-alkylureas.(13)
In the heat flow calibration procedure, high purity benzoic acid from NPL (SRM M16-06,
mass fraction 0.9999) was used as reference material.
Heat capacities were measured by using d.s.c. in the temperature range (280 to 310) K
with a Perkin–Elmer DSC-2 apparatus calibrated for temperature and enthalpy at both
superambient and subambient temperatures.(20, 21) However, this calibration procedure has
been recently improved as described in reference 13. In particular: benzoic acid in the
form of pressed pellets was used as a calorimetric standard over the whole experimental
temperature range; a (0.10He + 0.90Ne) mixture (He mass fraction 0.999995 and Ne mass
fraction > 0.9998) supplied by SIAD (Dalmine, Bergamo, Italy) was employed as a more

Heat capacities of solid alkane-α, ω-diols
539
TABLE 1. List of the alkane-α, ω-diols, molar mass M, commercial
b
origin, mass fraction w , and final mass fraction w determined in this
f
(18, 19)
work by the d.s.c. peak profile method
a
−1
b
Compound
M/(g·mol
)
Origin
w
w
f
1,6-Hexanediol
118.176
146.230
160.257
174.283
188.310
202.337
216.364
230.391
244.418
258.445
Aldrich
Aldrich
>0.99
0.98
0.98
0.98
0.994
0.985
0.996
0.998
0.996
0.995
0.993
0.988
0.996
0.991
1,8-Octanediol
1,9-Nonanediol
Aldrich
1,10-Decanediol
1,11-Undecanediol
1,12-Dodecanediol
1,13-Tridecanediol
1,14-Tetradecanediol
1,15-Pentadecanediol
Aldrich
Pfaltz & Bauer
Aldrich
0.99
this work
Aldrich
c
Pfaltz & Bauer
Aldrich
1,16-Hexadecanediol
0.98
a
Based on the 1991 IUPAC Table of Standard Atomic Weights of the El-
b
ements. w was not indicated by the supplier for 1,11-undecanediol, 1,14-
tetradecanediol, and 1,15-pentadecanediol, whereas 1,13-tridecanediol was
c
prepared in this work. Used as received.
appropriate gaseous thermal exchanger near room temperature; the samples were prepared
in the form of pellets about 1 mm thick and 4 mm in diameter, and mass in the range (10 to
25)·10−3 g, stored over P2O5 in a vacuum desiccator at room temperature and then sealed
in Al volatile-sample pans, in order to prevent any contact with moisture. A compromise
was achieved between scanning rate, sample mass, and instrumental sensitivity range to
obtain a sufficiently large signal-to-noise ratio.
The ordinate-displacement method was adopted and covered the temperature range (30 to
40) K. Two different reference samples and the empty sample holder were usually scanned
before and after recording the series of runs necessary to explore the full temperature range
for each sample of the studied compounds. The average value of the ordinate displacements
in two or three subsequent runs was determined for each sample at the selected temperatures.
For the reference samples and empty holder, the average of all the recorded values was taken
into account.
The accuracy of the measurements was estimated to be within 2 per cent over the whole
temperature range considered. The uncertainty of the temperature at the scanning rate of
0.167 K·s−1 selected was within ±0.2 K. More details concerning the calibration and ex-
perimental procedures adopted for measurements with our Perkin-Elmer DSC-2 equipment
are reported in an earlier paper.(13)
No solid-to-solid transitions were found in the temperature range of the measurements.
A complete investigation concerning solid-to-liquid and solid-to-solid transitions from
T = 298 K for this series of terminal diols is being prepared for publication.

540
G. Della Gatta, M. Jo´z´wiak, and P. Ferloni
f
e
400
300
200
d
c
b
a
280
290
300
310
320
T/K
FIGURE 1. Molar heat capacities C
of alkane-α, ω-diols as a function of temperature T . a, 1,6-
p,m
hexanediol; b, 1,8-octanediol; c, 1,10-decanediol; d, 1,12-dodecanediol; e, 1,14-tetradecanediol; f,
1,16-hexadecanediol.
3. Results and discussion
The results of the measurements are reported in table 2, where Cp,m values are averaged
over two or more experimental runs. They are also presented in figures 1 and 2 to illustrate
their substantial linearity as a function of temperature, though for 1,13-tridecanediol, and
partially for 1,9-nonanediol, a slight progressive increase of the slope was observed. No
other determinations of heat capacities of terminal diols that are solid at room temperature
are available in the literature, except for 1,6-hexanediol(16) and 1,10-decanediol.(17)
The linear equations Cp,m/(J·K−1 ·mol−1) = A + B{(T/K) − 298.15)} were obtained
by a least-squares analysis of all the data, except that for 1,13-tridecanediol the values at

Heat capacities of solid alkane-α, ω-diols
541
c
d
400
300
200
b
a
280
290
300
T/K
310
FIGURE 2. Molar heat capacities C
of alkane-α, ω-diols as a function of temperature T . a, 1,9-
p,m
nonanediol; b, 1,11-undecanediol; c, 1,13-tridecanediol; d, 1,15-pentadecanediol.
just the first four temperatures were extrapolated to T = 298.15 K. The results are shown
in table 3, where columns 2, 3, and 4 give the intercepts at T = 298.15 K (A), slopes (B),
and product-moment correlation coefficients (r), respectively. The only two values in the
literature(16, 17) are in agreement with those obtained in the present work.
Figure 3 shows the heat capacities at T = 298.15 K (table 3, column 2) as a func-
tion of the number of carbon atoms of the ten alkane-α, ω-diols. Its slope represents the
average contribution of the CH2 group to the total heat capacity of various diols and
gave a value of (23.05 ± 0.98) J·K−1 ·mol−1. Furthermore, if the heat capacity at T =
298.15 K for 1,6-hexanediol(16) and that extrapolated to the same temperature from the solid
1,2-ethanediol(22) arealsoconsidered, theinterceptatn = 0gives(58.4 ± 6.6)J·K−1 ·mol−1

542
G. Della Gatta, M. Jo´z´wiak, and P. Ferloni
−1
−1
TABLE 2. Experimental molar heat capacities C
/(J·K ·mol ) of the alkane-α, ω-diols
p,m
HO–(CH ) –OH at selected temperatures
2
n
n
T
K
6
8
9
10
11
12
13
14
15
16
280
285
290
295
300
305
310
176.79
181.38
184.44
187.86
191.48
195.58
201.31
220.57
224.94
229.22
233.58
238.21
242.48
247.67
236.75
242.64
247.95
253.00
259.24
266.64
276.36
261.93
267.17
272.19
276.41
281.16
286.10
291.66
276.74
282.35
287.82
294.06
300.28
307.13
314.09
307.46
312.99
319.54
326.45
332.75
339.77
347.62
334.27
341.02
351.23
360.98
370.82
383.38
399.87
354.16
361.26
368.23
375.97
382.04
391.17
399.00
352.36
359.13
366.86
372.72
380.61
388.17
396.86
396.62
405.15
413.14
421.16
429.53
437.70
446.96
TABLE 3. Molar heat capacities of the alkane-α, ω-
diols as a function of temperature from the equation
−1
−1
C
/(J·K ·mol ) = A + B{(T/K) − 298.15} in the
p,m
interval T = (280 to 310) K
a
a
b
Compound
A
B
r
c
1,6-Hexanediol
190.7 ± 0.3
0.779 ± 0.031
0.99598
0.99966
0.99331
0.99949
0.99896
0.99909
0.99632
0.99908
0.99897
0.99981
1,8-Octanediol
236.5 ± 0.1 0.896 ± 0.010
1,9-Nonanediol
258.7 ± 0.7 1.272 ± 0.066
d
1,10-Decanediol
1,11-Undecanediol
1,12-Dodecanediol
1,13-Tridecanediol
1,14-Tetradecanediol
1,15-Pentadecanediol
279.6 ± 0.1
0.972 ± 0.014
298.4 ± 0.3 1.243 ± 0.025
330.7 ± 0.3 1.338 ± 0.026
365.8 ± 1.3 1.807 ± 0.110
380.4 ± 0.3 1.487 ± 0.029
378.2 ± 0.3 1.467 ± 0.030
426.4 ± 0.2 1.661 ± 0.014
1,16-Hexadecanediol
a
Uncertainties are twice the standard deviation of the mean.
Product-moment correlation coefficient. A = 203.60.
b
c
(16) d
A =
(17)
270.10.
corresponding to the molar heat capacity at T = 298.15 K of solid HO–OH, in excellent
agreement with the value of (58.7 ± 0.1) J·K−1 ·mol−1 for H2O2(cr) at the same temper-
ature, as extrapolated by a least-squares analysis from the data of Gigue`re et al.(23) in the
subambient temperature interval (130 to 240) K.
In table 4, the two molar heat capacity contributions of the CH2 group for our ten solid
alkane-α, ω-diols derived (first line), or also including references 16 and 22 (second line) are
compared with those obtained from a comprehensive collection of literature data embracing
many homologous series of solid organic alkyl compounds. The values in column 4 (third
line and following) were derived from the slopes of the plots of the smoothed Cp,m values
at T = 298.15 K as a function of the total number of carbon atoms in the molecules of each
homologous series. All these values were recalculated from original data, and in many cases

Heat capacities of solid alkane-α, ω-diols
543
450
400
350
300
250
200
150
100
50
0
2
4
6
8
10
12
14
16
N (C)
FIGURE 3. Molar heat capacities C
number of C atoms N(C).
of alkane-α, ω-diols at T = 298.15 K as a function of the
p,m
the temperature interval considered was restricted to obtain a sufficiently representative set
of values near room temperature, which can be satisfactorily interpolated by a linear plot.
Furthermore, the Cp,m values of those compounds that are liquid at room temperature were
obtained for solids at T = 298.15 K by extrapolating the original subambient temperature
data by a least-squares analysis. The number N of compounds considered for each series,
and the lowest and highest total carbon atoms in their molecular backbone N(C) are set out
in columns 2 and 3. Differences between these two columns can originate either from the
presence of isomers in a complete, or almost complete, series of homologous compounds
(positive differences), or from the absence of reliable literature values at T = 298.15 K for
some terms of the series (negative differences).
The contribution to the molar heat capacities calculated in this work for the CH2 group
in solids ranges from 20.6 J·K−1 ·mol−1 for alkanoic acids to 26.8 J·K−1 ·mol−1 for both
N-alkylureas and N-acetylamino acid amides. The data reported in table 4 can be related to
the type of crystal structures in which alkyl chains are packed in the series of solid organic
homologous compounds considered.
In n-alkanes, dispersion forces alone are present, whereas in all the other series H-bond
networks play a more or less significant role in building up crystal structures. The influence
of the shared H-bonds depends on the nature and size of the functional groups, so that alkyl

544
G. Della Gatta, M. Jo´z´wiak, and P. Ferloni
TABLE 4. Heat capacity at T = 298.15 K of the CH group contribution to C
of solid
p,m
2
alkane-α, ω-diols compared with the values derived from various series of homologous alkyl
compounds in the literature; N denotes the number of compounds in the series, and N(C)
the number of C atoms in the compounds at the extremities of the series
−1
−1
)
Compounds
N
N(C)
C
/(J·K ·mol
References
p,m
Alkane-α, ω-diols
Alkane-α, ω-diols
n-Alkanes
10
12
22
13
12
5
6 to 16
2 to 16
4 to 33
1 to 16
7 to 20
2 to 6
23.05 ± 0.98
22.5 ± 0.6
22.5 ± 0.4
22.9 ± 0.6
20.6 ± 0.7
25.1 ± 1.0
25.1 ± 1.3
26.8 ± 0.4
26.7 ± 1.5
this work
this work, 16, 22
24–26
27–32
33, 34
35, 36
12
n-Alkan-1-ols
n-Alkanoic acids
Amino acids
N-acetyl-N-methylamino acid amides
N-acetylamino acid amides
2,5-diketopiperazines
N-alkylureas (mono-, di-, tri-,
and tetra-substituted)
N-alkylthioureas
8
5 to 9
5
4 to 8
14
4
4 to 6
14
20
7
1 to 9
1 to 5
27.3 ± 1.7
26.8 ± 0.7
26.3 ± 1.8
24.4 ± 0.5
23.6 ± 0.4
13, 37
15
Li-alkanoates
7
1 to 7
38–41
42–45
46–48
Na-alkanoates
5
1 to 16
7 to 12
Tl-alkanoates
3
chains can be differently packed and be allowed to give a progressively higher contribution
to the total heat capacity. Therefore, in amino acids and their various derivatives, as well as
in N-alkylureas and N-alkylthioureas, the increasing role of H-bond networks may account
for the higher heat capacity contribution of the CH2 group.
On the other hand, the increasing effect of the H-bond network can be observed by com-
paring the melting temperatures of compounds with the same N(C) belonging to different
series, e.g. C5H12 (n-pentane), Tfus = 143.4 K; C5H12O (n-pentan-1-ol), Tfus = 195.6 K;
C5H10O2 (n-pentanoic acid), Tfus = 239.2 K; and C5H12N2O2 (N-acetyl-L-alaninamide),
Tfus = 436.4 K; C5H10O (1,3-diethyl-2-urea), Tfus = 386.5 K; and C5H10S (1,3-diethyl-
2-thiourea), Tfus = 350.0 K.
The three families of metal alkanoates, which show a progressive slight decrease of the
contribution to Cp,m of their CH2 group as a function of the increasing size of the metal
ion, should not be included in this interpretation scheme and require data from other series
to be better understood.
In conclusion, the value of (23.05 ± 0.98) J·K−1 ·mol−1 derived in this work for the
contribution of the CH2 group to the Cp,m of alkane-α, ω-diols is closer to the weighted
mean of (22.1 ± 0.5) J·K−1 ·mol−1 for n-alkanes, n-alkanol-1-ols, and n-alkanoic acids
than to the corresponding value of (26.6 ± 0.9) J·K−1 ·mol−1 for the N-containing sub-
stances.

Heat capacities of solid alkane-α, ω-diols
545
Lastly, it is worth noting that the value of 21.92 J·K−1 ·mol−1 for the heat capacity of the
CH2 group contribution in solid organic compounds recently suggested by Domalski and
Hearing(49) on the basis of a group additivity scheme is decidedly closer to the weighted
mean for n-alkanes, n-alkan-1-ols, and n-alkanoic acids than to that obtained from the other
series of solid organic compounds reported in table 4, or e−ve1n to the weighted mean for all
the compounds reported therein, (24.3 ± 0.9) J·K−1 ·mol
.
This research was funded by the Ministero dell’Universita` e della Ricerca Scientifica e
Tecnologica (MURST) through the project Cofin. MURST 97 CFSIB. G. Della Gatta also
acknowledges financial support from the Consiglio Nazionale delle Ricerche through its
Committee 03. Participation of Maꢀlgorzata Jo´z´wiak in this work was made possible through
a research grant from the Universita` di Torino as a part of its cooperation agreement with
the Uniwersytet Lꢀ o´dzki.
References
1. }Nichols, N.; Sko¨ld, R.; Spink, C.; Wadso¨, I. J. Chem. Thermodynamics 1976, 8, 993–999.
2. }Della Gatta, G.; Barone, G.; Elia, V. J. Solution Chem. 1986, 15, 157–167.
3. }Bastos, M.; Briggner, L.-E.; Shehatta, I.; Wadso¨, I. J. Chem. Thermodynamics 1990, 22, 1181–
1190.
4. }Della Gatta, G.; Ferro, D. Thermochim. Acta 1987, 122, 143–152.
5. }Ferro, D.; Della Gatta, G. Thermochim. Acta 1987, 122, 189–195.
6. }Ferro, D.; Barone, G.; Della Gatta, G.; Piacente, V. J. Chem. Thermodynamics 1987, 19, 915–923.
7. }Ferro, D.; Della Gatta, G.; Barone, G. J. Therm. Anal. 1988, 34, 835–841.
8. }Piacente, V.; Ferro, D.; Della Gatta, G. Thermochim. Acta 1990, 158, 79–85.
9. }Barone, G.; Della Gatta, G.; Ferro, D.; Piacente, V. J. Chem. Soc. Faraday Trans. 1990, 86,
75–79.
10. }Piacente, V.; Ferro, D.; Della Gatta, G. Thermochim. Acta 1993, 223, 65–73; 1994, 232, 317–321.
11. }Ferro, D.; Martino, R.; Della Gatta, G. J. Chem. Thermodynamics 1994, 26, 183–190.
12. }Abate, L.; Della Gatta, G.; Somsen, G. Thermochim. Acta 1994, 239, 7–16.
13. }Ferloni, P.; Della Gatta, G. Thermochim. Acta 1995, 266, 203–212.
14. }Abate, L.; Palecz, B.; Giancola, C.; Della Gatta, G. J. Chem. Thermodynamics 1997, 29, 359–368.
15. }Abate, L.; Jozwiak, M.; Della Gatta, G. Thermochim. Acta 1997, 303, 63–68.
16. }Steele, W. V.; Chirico, R. D.; Nguyen, A.; Hossenlopp, I. A.; Smith, N. K. DIPPR Data Series
1991, 1, 103–134.
17. }Steele, W. V.; Chirico, R. D.; Hossenlopp, I. A.; Knipmeyer, S. E.; Nguyen, A.; Smith, N. K.
DIPPR Data Series 1994, 2, 188–215.
18. }Plato, C. Anal. Chem. 1972, 44, 1531–1534.
19. }Sondack, D. L. Anal. Chem. 1972, 44, 888 and 2089.
20. }Ferloni, P.; Franzosini, P. Gazz. Chim. Ital. 1975, 105, 391–401.
21. }Zabinska, G.; Ferloni, P.; Sanesi, M. Thermochim. Acta 1987, 122, 87–94.
22. }Parks, G. S.; Kelley, K. K. J. Am. Chem. Soc. 1925, 47, 2089–2097.
23. }Gigue`re, P. A.; Liu, I. D.; Dugdale, J. S.; Morrison, J. A. Can. J. Chem. 1954, 32, 117–127.
24. }Parks, G. S.; Huffman, H. M.; Thomas, S. B. J. Am. Chem. Soc. 1930, 52, 1032–1041.
25. }Huffman, H. M.; Parks, G. S.; Barmore, M. J. Am. Chem. Soc. 1931, 53, 3876–3888.
26. }Finke, H. L.; Gross, M. E.; Waddington, G.; Huffman, H. M. J. Am. Chem. Soc. 1954, 76,
333–341.
27. }Parks, G. S. J. Am. Chem. Soc. 1925, 47, 338–345.
28. }Kelley, K. K. J. Am. Chem. Soc. 1929, 51, 779–786.
29. }Cline, J. K.; Andrews, D. H. J. Am. Chem. Soc. 1931, 53, 3668–3673.

546
G. Della Gatta, M. Jo´z´wiak, and P. Ferloni
30. }Parks, G. S.; Kennedy, W. D.; Gates, R. R.; Mosley J. R.; Moore, G. E.; Renquist, M. L. J. Am.
Chem. Soc. 1956, 78, 56–59.
31. }Counsell, J. F.; Lees, E. B.; Martin, J. F. J. Chem. Soc. A 1968, 1819–1823.
32. }Mosselman, C.; Mourik, J.; Dekker, H. J. Chem. Thermodynamics 1974, 6, 477–487.
33. }Schaake, R. C. F.; van Miltenburg, J. C.; de Kruif, C. G. J. Chem. Thermodynamics 1982, 14,
771–778.
34. }Schaake, R. C. F.; van Miltenburg, J. C.; de Kruif, C. G. J. Chem. Thermodynamics 1982, 14,
763–769.
35. }Spink, C. H.; Wadso¨, I. J. Chem. Thermodynamics 1975, 7, 561–572.
36. }Hutchens, J. O.; Cole, A. G.; Stout, J. W. J. Am. Chem. Soc. 1960, 82, 4813–4815.
37. }Kabo, G. J.; Kozyro, A. A.; Diky, V. V.; Simirsky, V. V. J. Chem. Eng. Data 1995, 40, 371–393.
38. }Ferloni, P.; Kenesey, C.; Westrum, Jr., E. F. J. Chem. Thermodynamics 1994, 26, 1349–1363.
39. }Franzosini, P.; Westrum, Jr., E. F., J. Chem. Thermodynamics 1984, 16, 81–90.
40. }Ngeyi, S. P.; Westrum, Jr., E. F.; Franzosini, P. J. Chem. Thermodynamics 1986, 18, 609–618.
41. }Franzosini, P.; Ngeyi, S. P.; Westrum, Jr., E. F. J. Chem. Thermodynamics 1986, 18, 1169–1181.
42. }Westrum, Jr., E. F.; Chang, S. S.; Levitin, N. E. J. Phys. Chem. 1960, 64, 1553–1554.
43. }Franzosini, P.; Plautz, W. A.; Westrum, Jr., E. F. J. Chem. Thermodynamics 1983, 15, 445–456.
44. }Franzosini, P.; Westrum, Jr., E. F.; Plautz, W. A. J. Chem. Thermodynamics 1983, 15, 609–618.
45. }Wirth, H. E.; Droege, J. W.; Wood, J. H. J. Phys. Chem. 1959, 63, 152–153.
46. }Labban, A. K.; Lopez de la Fuente, F. L.; Cheda, J. A. R.; Westrum, Jr., E. F.; Ferna´ndez-Mart´ın,
F. J. Chem. Thermodynamics 1989, 21, 375–384.
47. }Lopez de la Fuente, F. L.; Cheda, J. A. R.; Ferna´ndez-Mart´ın, F.; Westrum, Jr., E. F. J. Chem.
Thermodynamics 1988, 20, 1137–1148.
48. }Lopez de la Fuente, F. L.; Westrum, Jr., E. F.; Cheda, J. A. R.; Ferna´ndez-Mart´ın, F. J. Chem.
Thermodynamics 1987, 19, 1261–1270.
49. }Domalski, E. S.; Hearing, E. D. J. Phys. Chem. Ref. Data 1993, 22, 805–1177.
(Received 15 December 1997; in final form 1 December 1998)
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