densities, viscosities and refractive indexes
TRANSCRIPT
Densities, viscosities, and refractive indexes
for {C2H5CO2(CH2)2CH3+C6H13OH+C6H6}
at T ¼ 308:15K
Herminio Casas, Sandra Garc�ııa-Garabal, Luisa Segade,Oscar Cabeza *, Carlos Franjo, Eulogio Jim�eenez
Departamento de F�ıısica, Facultade de Ciencias, Universidade da Coru~nna, Campus da Zapateira,
15071 A Coru~nna, Spain
Received 22 November 2002; accepted 10 March 2003
Abstract
In this work we present densities, kinematic viscosities, and refractive indexes of the ternary
system {C2H5CO2ðCH2Þ2CH3 þ C6H13OHþ C6H6} and the corresponding binary mixtures
{C2H5CO2ðCH2Þ2CH3þC6H6}, {C2H5CO2ðCH2Þ2CH3þC6H13OH}, and {C6H13OHþC6H6}.
All data have beenmeasured at T ¼ 308:15K and atmospheric pressure over the whole composi-
tion range. The excess molar volumes, dynamic viscosity deviations, and changes of the refractive
index onmixingwere calculated fromexperimentalmeasurements.The results for binarymixtures
were fitted to a polynomial relationship to estimate the coefficients and standard deviations. The
Cibulka equation has been used to correlate the experimental values of ternarymixtures.Also, the
experimental values obtained for the ternary mixture were used to test the empirical methods of
Kohler, Jacob and Fitzner, Colinet, Tsao and Smith, Toop, Scatchard et al., and Hillert. These
methods predict excess properties of the ternary mixtures from those of the involved binary mix-
tures.The results obtained fordynamicviscosities of thebinarymixtureswereused to test the semi-
empirical relations of Grunberg–Nissan, McAllister, Ausl€aander, and Teja–Rice. Finally, the
experimental refractive indexes were comparedwith the predicted results for the Lorentz–Lorenz,
Gladstone–Dale, Wiener, Heller, and Arago–Biot equations. In all cases, we give the standard
deviation between the experimental data and that calculated with the above named relations.
Ó 2003 Elsevier Science Ltd. All rights reserved.
Keywords: Density; Refractive index; Viscosity; Excess properties; Ternary mixture
J. Chem. Thermodynamics 35 (2003) 1129–1137
www.elsevier.com/locate/jct
*Corresponding author. Fax: +34-981-167065.
E-mail address: [email protected] (O. Cabeza).
0021-9614/03/$ - see front matter Ó 2003 Elsevier Science Ltd. All rights reserved.
doi:10.1016/S0021-9614(03)00081-8
1. Introduction
In a previous paper [1], we have reported experimental excess molar volumes,
dynamic viscosity deviations, and changes of refractive index on mixing of
{C2H5CO2ðCH2Þ2CH3 þ C6H13OHþ C6H6}, and of their corresponding binary
mixtures at T ¼ 298:15K. In the present paper, we continue with the investigation
of this ternary system but at T ¼ 308:15K. This paper and the previous one com-
plete the study of excess volumes of nonelectrolyte ternary mixtures with six car-
bon atoms started previously [2–4]. CibulkaÕs equation [5] has been used to
correlate the experimental values of ternary mixtures. Those experimental values
were used to test the empirical methods of Kohler [6], Jacob and Fitzner [7], Col-
inet [8], Tsao and Smith [9], Toop [10], Scatchard et al. [11], and Hillert [12]. These
methods predict excess properties of the ternary mixtures from those of the in-
volved binary mixtures. The results obtained for dynamic viscosities of the binary
mixtures were used to test the semiempirical relations of Grunberg–Nissan [13],
McAllister [14], Ausl€aander [15], and Teja–Rice [16]. Finally, the experimental re-
fractive indexes were compared with the predicted results for the Lorentz–Lorenz,
Gladstone–Dale, Wiener, Heller, and Arago–Biot equations, which were compiled
by Tasic et al. [17].
2. Experimental
The chemicals employed were supplied by Fluka. Their mole-fraction purities
were C2H5CO2ðCH2Þ2CH3 > 0:99, C6H13OH > 0:99, and C6H6 > 0:995. The sub-
stances were degassed by ultrasound and dried over molecular sieves (Sigma Union
Carbide, type 0.4 nm).
Excess molar volumes were determined from the densities of the pure liquids and
mixtures. Densities were measured with an Anton–Paar DMA 60/602 densimeter
thermostated at T ¼ ð308:15� 0:01ÞK in a Haake F3 circulating-water bath. The ac-
curacy of the measured densities is around 10ÿ2 kg �mÿ3. Immediately prior to each
series of measurements, distilled water and heptane were used to calibrate the densi-
meter. Kinematic viscosities were measured by means of Schott–Ger€aate automatic
viscometer with an accuracy of �5 � 10ÿ10m2 � sÿ1. The refractive indexes were mea-
sured with a thermostated automatic refractometer Atago RX-1000 with reproduc-
ibility in the refractive index data of 10ÿ4. Finally, mixtures were prepared in all cases
by mass using a Mettler AT 201 balance. The precision of the mole fraction is esti-
mated to be better than 10ÿ4.
3. Results and discussion
The measured densities, dynamic viscosities (obtained from the measured kine-
matic viscosities and densities), and refractive indexes of the pure liquids at
T ¼ 298:15K are listed in reference [1] together with published values when available.
1130 H. Casas et al. / J. Chem. Thermodynamics 35 (2003) 1129–1137
The agreement between both sets of data indicates that the compounds used were
pure and that our experimental equipment has a good accuracy.
The excess molar volumes V Em , dynamic viscosity deviations Dg, and changes
in the refractive index on mixing Dn were computed using equations (1) to (3),
respectively,
V Em ¼
X
N
i¼1
xiMiðqÿ1 ÿ q
ÿ1i Þ; ð1Þ
Dg ¼ gÿX
N
i¼1
xigi; ð2Þ
Dn ¼ gÿX
N
i¼1
xini: ð3Þ
In these equations q, g, and n are, respectively, the density, dynamic viscosity, and
refractive index in the mixture. The qi, gi, and ni are the properties of the pure
components, and N is the number of the components in the mixture (so N ¼ 2 in the
case of a binary mixture and N ¼ 3 for a ternary one). The derived excess functions
of the binary systems can be represented by a Redlich–Kister type equation [18],
QEij ¼ xixj
X
m
K¼0
AKðxi ÿ xjÞK; ð4Þ
TABLE 1
Coefficients AK and BK of equations (4) and (6) and standard deviations, s
A0 A1 A2 A3 A4 A5 A6 s
fx C2H5CO2ðCH2Þ2CH3 þ ð1ÿ xÞ C6H13OHg10ÿ6 � V E
m =ðm3 �molÿ1Þ 0.933 )0.052 0.153 0.0011
10ÿ3 � Dg=ðPa � sÞ )3.858 2.221 )1.776 0.9349 0.004
10ÿ3 � Dn )4.00 )0.58 0.23 0.03
fx C2H5CO2ðCH2Þ2CH3 þ ð1ÿ xÞ C6H6g
10ÿ6 � V Em =ðm3 �molÿ1Þ )0.217 )0.064 0.061 0.0012
10ÿ3 � Dg=ðPa � sÞ )0.0792 0.0209 )0.0429 0.0004
10ÿ3 � Dn )45.9 11.8 4.6 )16.7 )14.4 36.7 0.11
fx C6H13OHþ ð1ÿ xÞ C6H6g
10ÿ6 � V Em =ðm3 �molÿ1Þ 1.358 )0.669 0.186 0.132 )0.338 )0.474 0.865 0.0012
10ÿ3 � Dg=ðPa � sÞ )3.265 )0.7560 )0.1051 0.007
10ÿ3 � Dn )36.3 10.3 )2.7 0.15
B1 B2 B3 s
fx1 C2H5CO2ðCH2Þ2CH3 þ x2C6H13OHþ ð1ÿ x1 ÿ x2Þ C6H6g10ÿ6 � V E
m;123=ðm3 �molÿ1Þ )0.545 2.392 )2.642 0.005
10ÿ3 � Dg123=ðPa � sÞ 1.849 0.6731 2.113 0.011
10ÿ3 � Dn123 18.1 8.7 )13.5 0.15
H. Casas et al. / J. Chem. Thermodynamics 35 (2003) 1129–1137 1131
where QEij represents any of the following properties, V E
m , or Dg, or Dn; xi and xj are
the mole fractions of components i and j, respectively; and AK denotes the polyno-
mial coefficients. The degree of the polynomial Redlich–Kister equation was opti-
mised by applying the F test [19]. In table 1, we give the fitted coefficients AK for
equation (4) and the standard deviation, s, defined by,
s ¼X
M
i¼1
Ycalÿ
(
ÿ Yexp�2.
M ÿ 1
)1=2
; ð5Þ
where M is the number of data points, Ycal is the calculated value, and Yexp is the
experimental value.
Figures 1(a) to (c) show, respectively, the experimental V Em , Dg, and Dn plotted
against x together with the fitted curves. The V Em is negative for {propylpropanoate +
FIGURE 1. (a) Excess molar volumes V Em , (b) dynamic viscosity deviations Dg, and (c) changes in the
refractive index on mixing Dn at T ¼ 308:15K plotted against mole fraction x of: s, {xC2H5CO2ðCH2Þ2CH3 þ ð1ÿ xÞ C6H6}; �, {xC2H5CO2ðCH2Þ2CH3 þ ð1ÿ xÞ C6H13OH}; D, {xC6H13OHþ ð1ÿ xÞ C6H6}.
1132 H. Casas et al. / J. Chem. Thermodynamics 35 (2003) 1129–1137
benzene} and positive for the other systems, similar in shape and amplitude than for
T ¼ 298:15K [1]. The slightly negative value observed may be interpreted as proof of
some weak intermolecular interactions established between the carbonyl group of
propyl propanoate and the hydrogen atoms of the benzenic ring. This kind of inter-
action cannot be created between the OH group of 1-hexanol and benzene due to the
steric effect of the long hexanyl chain, which results in positive V Em . In a previous
work [20], there are reported V Em for {C6H6 þ C6H13OH} at T ¼ 298:15K and
T ¼ 308:15K. Their results are very similar to ours both in shape and absolute value.
Results for Dg, given in figure 1(b), show negative curves for the three binary mix-
tures. The absolute value of Dg is lower in around a 30% respecting those presented
before at T ¼ 298:15K for all binary mixtures [1]. Respecting Dn, presented in figure
1(c), the data present the same shape and nearly the same amplitude for all three bi-
nary mixtures than at T ¼ 298:15K. In conclusion, the effect of temperature is only
important for Dg, and not for Dn and V Em .
Table 2 shows the parameters calculated and the standard deviations between ex-
perimental values obtained for dynamic viscosity and the predicted results using the
semi-empirical relations of Grunberg–Nissan [13], McAllister [14], Ausl€aander [15],
and Teja–Rice [16]. The values of critical temperature and critical volume for pure
components, needed for the Teja–Rice relationship, were obtained from reference
[21]. As observed, the best accuracy is given for the Ausl€aander relationship.
Table 3 compares the experimental refractive indexes for binary mixtures with the
predicted results for the Lorentz–Lorenz, Gladstone–Dale, Arago–Biot, Heller, and
Wiener equations, which were compiled by Tasic et al. [17]. As in that paper, the
Lorentz–Lorenz relationship is the most suitable for our data.
TABLE 2
Parameters for the semiempirical relations of Grunberg–Nissan [13], McAllister [14], Ausl€aander [15], and
Teja–Rice [16] and standard deviations, s
System s=ðmPa � sÞ
fx C2H5CO2ðCH2Þ2CH3 þ ð1ÿ xÞ C6H13OHg
Grunberg–Nissan dw ¼ ÿ1:3855 0.03
McAllister g12 ¼ 0:7235 g21 ¼ 1:0903 0.018
Ausl€aander B12 ¼ 3:1844 B21 ¼ 0:0820 A21 ¼ 0:7186 0.012
Teja–Rice a12 ¼ ÿ0:0474 0.05
fx C2H5CO2ðCH2Þ2CH3 þ ð1ÿ xÞ C6H6g
Grunberg–Nissan dw ¼ ÿ0:1520 0.017
McAllister g12 ¼ 0:5659 g21 ¼ 0:4818 0.016
Ausl€aander B12 ¼ ÿ1:1414 B21 ¼ 7:1632 A21 ¼ 0:1835 0.016
Teja–Rice a12 ¼ 0:8482 0.017
fx C6H13OHþ ð1ÿ xÞ C6H6g
Grunberg–Nissan dw ¼ ÿ0:5121 0.05
McAllister g12 ¼ 1:7373 g21 ¼ 0:6530 0.012
Ausl€aander B12 ¼ 0:1523 B21 ¼ 1:4048 A21 ¼ 1:7648 0.009
Teja–Rice a12 ¼ 0:5029 0.04
H. Casas et al. / J. Chem. Thermodynamics 35 (2003) 1129–1137 1133
The experimental excess molar volumes V Em;123, dynamic viscosity deviations Dg123,
and changes of refractive index on mixing Dn123 for ternary mixtures were obtained
using equations (1) to (3), respectively. The Cibulka equation [5] has been used to
correlate the experimental properties of the ternary mixtures.
QE123 ¼ QE
bin þ x1x2ð1ÿ x1 ÿ x2ÞðB1 þ B2x1 þ B3x2Þ; ð6Þ
FIGURE 2. Curves of constant (a) 10ÿ6 � V Em;123=ðm
3 �molÿ1), (b) 10ÿ3 � Dg123=ðPa � sÞ, and (c) Dn123, for
{x1 C2H5CO2ðCH2Þ2CH3 þ x2 C6H13OHþ ð1ÿ x1 ÿ x2Þ C6H6} at T ¼ 308:15K.
TABLE 3
Standard deviations of the experimental refractive index results from the predicted for the Lorentz–Lorenz
(L–L), Gladstone–Dale (G–D), Arago–Biot (A–B), Heller (H), and Wiener (W) equations
System L–L G–D A–B H W
fx C2H5CO2ðCH2Þ2CH3 þ ð1ÿ xÞ C6H13OHg 0.0002 0.0001 0.0014 0.0004 0.0004
fx C2H5CO2ðCH2Þ2CH3 þ ð1ÿ xÞ C6H6g 0.0003 0.0010 0.0013 0.0003 0.0006
fx C6H13OHþ ð1ÿ xÞ C6H6g 0.0003 0.0009 0.0017 0.0016 0.0018
1134 H. Casas et al. / J. Chem. Thermodynamics 35 (2003) 1129–1137
where
QEbin ¼ QE
12 þ QE13 þ QE
23: ð7Þ
The symbol QE123 represents V
Em;123, Dg123 or Dn123, and QE
ij is given by equation (4).
The parameters BK for equation (6) and the corresponding standard deviations, s,
defined by equation (5), are given in table 1. The lines of constant ternary excess
properties, calculated by equations (6) and (7), are shown in figures 2(a) to (c) for
V Em;123, Dg123, or Dn123, respectively. Figures 3(a)–(c) shows lines of constant ‘‘ternary
contribution’’, which represent the difference between the experimental value and
that predicted from the binary mixtures (QE123 ÿ QE
bin). Inside the triangular diagrams
exist maxima and/or minima, whose coordinates are presented in table 4.
FIGURE 3. Curves of ternary contribution (a) 10ÿ6 � ðV Em;123 ÿ V E
m;binÞ=ðm3 �molÿ1), (b) 10ÿ3 � ðDg123 ÿ
Dgbin=ðPa � sÞ, and (c) (Dn123 ÿ Dnbin) for {x1 C2H5CO2ðCH2Þ2CH3 þ x2 C6H13OHþ ð1ÿ x1 ÿ x2Þ C6H6}
at T ¼ 308:15K.
H. Casas et al. / J. Chem. Thermodynamics 35 (2003) 1129–1137 1135
Finally, values of V Em;123, Dg123, and Dn123 have been also calculated using the em-
pirical equations proposed by Kohler [6], Jacob and Fitzner [7], Colinet [8], Tsao–
Smith [9], Toop [10], Scatchard et al. [11], and Hillert [12], which take only the binary
contribution into account. For the asymmetric methods (Tsao–Smith, Toop, Scat-
chard, and Hillert), we must indicate the order of components in the mixtures. Table
5 shows the standard deviations, s, between experimental and predicted values. The
most accurate predictions correspond to those of Toop, Scatchard, and Hillert.
TABLE 5
Standard deviations s of different models for: (a) {x1 C2H5CO2(CH2)2CH3 + x2 C6H13OH+(1)x1 ) x2)
C6H6}; (b) {x1 C6H13OH+ x2 C6H6 + (1) x1 ) x2) C2H5CO2(CH2)2CH3}; (c) {x1 C6H6 + x2 C2H5CO2
(CH2)2CH3 + (1)x1 ) x2) C6H13OH}
a b c
10ÿ6 � V Em;123, s=ðm
3 �molÿ1ÞJacob and Fitzner 0.012
Kohler 0.018
Colinet 0.015
Tsao and Smith 0.057 0.024 0.033
Toop 0.021 0.028 0.007
Scatchard 0.016 0.027 0.008
Hillert 0.017 0.027 0.007
10ÿ3 � Dg123, s=ðPa � sÞ
Jacob and Fitzner 0.0620
Kohler 0.0790
Colinet 0.0758
Tsao and Smith 0.2484 0.0159 0.2432
Toop 0.1342 0.0158 0.0924
Scatchard 0.1339 0.0157 0.0782
Hillert 0.1339 0.0157 0.0916
Dn123, s
Jacob and Fitzner 0.0004
Kohler 0.0005
Colinet 0.0004
Tsao and Smith 0.0017 0.0020 0.0002
Toop 0.0007 0.0006 0.0002
Scatchard 0.0006 0.0005 0.0002
Hillert 0.0006 0.0006 0.0002
TABLE 4
Maxima and minima for ternary contributions of the mixture: {x1 C2H5CO2(CH2)2CH3 + x2
C6H13OH+(1)x1 ) x2) C6H6}
Value Coordinates
10ÿ6 � ðV Em;123 ÿ VE
binÞ=ðm3 �molÿ1Þ Maximum 0.0125 x1 ¼ 0:67 x2 ¼ 0:12
Minimum )0.0420 x1 ¼ 0:19 x2 ¼ 0:5310ÿ3 � ðDg123 ÿ DgbinÞ=ðPa � sÞ Maximum 0.105 x1 ¼ 0:32 x2 ¼ 0:38
Dn123 ÿ Dnbin Maximum 0.0006 x1 ¼ 0:40 x2 ¼ 0:27
1136 H. Casas et al. / J. Chem. Thermodynamics 35 (2003) 1129–1137
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