J. Chem. Thermodynamics 43 (2011) 1389–1394

Contents lists available at ScienceDirect

J. Chem. Thermodynamics

journal homepage: www.elsevier .com/locate / jc t

Densities, viscosities, speed of sound, and IR spectroscopic studies of binarymixtures of tert-butyl acetate with benzene, methylbenzene, and ethylbenzeneat T = (298.15 and 308.15) K

Mehdi Hasan a,⇑, Arun B. Sawant a, Rajashri B. Sawant a,b, Pratibha G. Loke a,c

a P.G. Department of Physical Chemistry, M.S.G. College, Malegaon Camp 423 105, Indiab Department of Chemistry, S.P.H. Mahila College, Malegaon Camp 423 105, Indiac Department of Physics, G.M.D. Arts, B.W. Commerce and Science College, Sinnar, India

a r t i c l e i n f o

Article history:Received 13 January 2011Received in revised form 18 March 2011Accepted 8 April 2011Available online 16 April 2011

Keywords:Excess molar volumesDeviations in viscosityDeviations in isentropic compressibilityIRtert-Butyl acetateBenzenes

0021-9614/$ - see front matter � 2011 Elsevier Ltd. Adoi:10.1016/j.jct.2011.04.008

⇑ Corresponding author. Tel.: +91 2554 561544; faxE-mail address: mihasan@rediffmail.com (M. Hasa

a b s t r a c t

Densities, viscosities, speed of sound, and IR spectroscopy of binary mixtures of tert-butyl acetate (TBA)with benzene, methylbenzene, and ethylbenzene have been measured over the entire range of composi-tion, at (298.15 and 308.15) K and at atmospheric pressure. From the experimental values of density, vis-cosity, speed of sound, and IR spectroscopy; excess molar volumes VE, deviations in viscosity Dg,deviations in isentropic compressibility Djs and stretching frequency m have been calculated. The excessmolar volumes and deviations in isentropic compressibility are positive for the binaries studied over thewhole composition, while deviations in viscosities are negative for the binary mixtures. The excess molarvolumes, deviations in viscosity, and deviations in isentropic compressibility have been fitted to the Red-lich–Kister polynomial equation. The Jouyban–Acree model is used to correlate the experimental valuesof density, viscosity, and speed of sound.

� 2011 Elsevier Ltd. All rights reserved.

1. Introduction

The molecular shape and size play an important role in deter-mining the thermodynamic behavior of mixtures. Studies on ther-modynamic and transport properties of binary liquid mixturesprovide information on the nature of interactions in the constitu-ent binaries. Literature provides extensive data on the densityand viscosity of liquid mixtures but a combined study of density,viscosity, speed of sound, and IR study is quite scarce. The effectof molecular size, shape, chain length, and chain branching of alkylacetates on solute–solvent interaction were reported by Sakuraiet al. [1]. The interaction between esters and hydrocarbons werereported [2] for the binary mixtures of butyl acetate with aromatichydrocarbons. We now report the density, viscosity, and speed ofsound data for the binary mixtures of TBA with benzene, methyl-benzene, and ethylbenzene at (298.15 and 308.15) K.

The electron withdrawing groups increase IR absorption fre-quency while electron donating groups lower IR absorption fre-quency. We have attempted to study the physico-chemicalproperties of the mixtures indicated above, in order to explainthe strength and nature of the interactions between the compo-

ll rights reserved.

: +91 02554 251705.n).

nents by deriving various thermodynamic parameters from viscos-ity, density, speed of sound data, and spectroscopic study.

2. Experimental

Benzene and methylbenzene (Sisco Research Lab Pvt. Ltd., pur-ity > 0.997), ethyl benzene (Otto Kemi, purity > 0.99), and tert-bu-tyl acetate (TBA) (Spectrochem Pvt. Ltd., purity > 0.99) were usedafter single distillation. The purity of the solvents, after purifica-tion, was ascertained by comparing their densities, viscosities,and speed of sound with the corresponding literature values at(298.15 and 308.15) K (table 1). Binary mixtures were preparedby mass in air tight stoppered glass bottles. The masses were re-corded on an Adairdutt balance to an accuracy of ±1 � 10�4 g.

Care was taken to avoid evaporation and contamination duringmixing. The estimated uncertainty in mole fraction was <1 � 10�4.

Densities were determined by using a 15 cm3 bicapillary pyc-nometer as described earlier [3]. The pycnometer was calibratedusing conductivity water with 0.99705 g � cm�3 as its density [4]at 298.15 K. The estimated uncertainty of density measurementsof solvent and binary mixtures was 0.0001 g � cm�3. At least threeto four measurements were made which had an average deviationof ±0.0001 g � cm�3.

The dynamic viscosities were measured using an Ubbelohdesuspended level viscometer [3], calibrated with conductivity

TABLE 1Comparison of experimental density, viscosity, and sound speed of pure liquids with literature values at (298.15 and 308.15) K.

Liquid T/K q � 10�3/(kg �m�3) g/(mPa � s) u/(m � s�1)

This work Reference This work Reference This work Reference

tert-Butyl acetate 298.15 0.8611 0.86057a 0.683 1092 1092.8c

308.15 0.8494 0.84938a 0.596 1055 1049.7c

Benzene 298.15 0.8730 0.87278d 0.609 0.6080b 1296 1295.6e

308.15 0.8620 0.8628f 0.539 0.53951d 1260 1260g

Methylbenzene 298.15 0.8622 0.8622h 0.556 0.556h 1312 1310i

308.15 0.8525 0.8522j 0.500 0.4989 l 1270 1272 m

0.8527k

Ethylbenzene 298.15 0.8644 0.86433n 0.631 0.629o 1325 1319p

308.15 0.8554 0.8555f 0.569 0.5688q 1280 1278r

a Reference [1].b Reference [12].c Reference [18].d Reference [19].e Reference [20].f Reference [21].g Reference [22].h Reference [23].i Reference [24].j Reference [25].k Reference [26].l Reference [27].m Reference [28].n Reference [29].o Reference [30].p Reference [31].q Reference [32].r Reference [33].

1390 M. Hasan et al. / J. Chem. Thermodynamics 43 (2011) 1389–1394

water. At least three repetitions of each data reproducible to±0.05 s were obtained, and the results were averaged. The uncer-tainties in dynamic viscosities are of the order ±0.003 mPa � s.

The speed of sound (u) were measured at a frequency of 2 MHzin these solutions through interferometric method (using Mittal’sF-81 model) at (298.15 and 308.15) K (±0.05 K). The uncertaintyin speed measurements is ±0.1%. FTIR spectra of the above mix-tures were recorded on FTIR spectrometer model SHIMADZU8400S PC.

3. Results and discussion

Experimental values of densities q, viscosities g, and speed ofsound u of mixtures at (298.15 and 308.15) K are listed as a func-tion of mole fraction in table 2. The density values have been usedto calculate excess molar volumes VE using the following equation

VE=ðcm3 �mol�1Þ ¼ ðx1M1 þ x2M2Þ=q12 � ðx1M1=q1Þ�ðx2M2=q2Þ; ð1Þ

where q12 is the density of the mixture and x1, M1, q1, and x2, M2, q2

are the mole fraction, the molecular weight, and the density of purecomponents 1 and 2, respectively.

The viscosity deviations Dg were calculated using

Dg=ðmPa � sÞ ¼ g12 � x1g1 � x2g2; ð2Þ

where g12 is the viscosity of the mixture and x1, x2 and g1, g2 are themole fraction and the viscosity of pure components 1 and 2,respectively.

The isentropic compressibility, js was obtained using the La-place relation,

js ¼ ð1=u2qÞ ð3Þ

and the deviation from isentropic compressibility, (Djs), was ob-tained using the relation,

Djs ¼ js12 � x1js1 � x2js2; ð4Þ

where js12 is the experimental isentropic compressibility of themixture, x1, x2 and js1, js2 are the mole fraction and isentropic com-pressibility of pure components.

The excess molar volumes and deviations in viscosity and isen-tropic compressibility were fitted to Redlich Kister [5] equation ofthe type

Y ¼ x1x2

Xn

i¼0

aiðx1 � x2Þi; ð5Þ

where Y is either VE, or Dg , or Djs, and n is the degree of polyno-mial. Coefficients ai were obtained by fitting equation (5) to exper-imental results using a least-squares regression method. In eachcase, the optimum number of coefficients is ascertained from anexamination of the variation in standard deviation r.

r was calculated using the relation

rðYÞ ¼PðYexpt � YcalcÞ2

N � n

" #1=2

; ð6Þ

where N is the number of data points and n is the number of coef-ficients. The calculated values of the coefficients ai along with thestandard deviations r are given in table 3.

The variation of VE with the mole fraction x1 of TBA for benzene,methylbenzene, and ethylbenzene at 298.15 K is represented infigure 1. Literature [6] provides the VE values of butyl acetate(BA) with benzene and methylbenzene, but there are no reportsfor the VE values of TBA with benzene, methylbenzene, and ethyl-benzene, hence a comparison of our results with the literature val-ues can not be made. The VE of all the three binary mixtures arepositive over the whole composition range. It is explained [6] thatthe positive VE values result because of the breaking of dipole–di-pole interactions and also due to the formation of interactionsamong the polar acetate groups and electrons on the benzene ring.When a methyl group is introduced in the benzene ring the elec-tron cloud increases and these interactions become more strongwhich results in the decrease of VE, but this interaction again

TABLE 2Density (q), viscosity (g), speed of sound (u), excess molar volume (VE), deviation in viscosity (Dg), isentropic compressibility (js) and deviation in isentropic compressibility(Djs) for {tert-butyl acetate (1) + benzenes (2)} at (298.15 and 308.15) K.

x1 q � 10�3/(kg �m�3) VE � 106/(m3 �mol�1) g/(mPa � s) Dg/(mPa � s) u/(m � s�1) js/(TPa�1) Djs/(TPa�1)

CH3COOC(CH3)3 (1) + C6H6 (2)T = 298.15 K

0.0000 0.8730 0.000 0.609 0.000 1296 682 00.0987 0.8706 0.073 0.613 �0.003 1254 730 190.1999 0.8685 0.143 0.618 �0.006 1220 774 340.2990 0.8667 0.191 0.623 �0.008 1192 812 430.3982 0.8653 0.220 0.629 �0.010 1169 846 480.4980 0.8641 0.230 0.636 �0.010 1149 876 490.5995 0.8630 0.235 0.643 �0.010 1133 903 460.6996 0.8623 0.205 0.651 �0.009 1120 925 390.7999 0.8617 0.163 0.661 �0.008 1109 944 290.8993 0.8613 0.089 0.671 �0.005 1099 961 161.0000 0.8611 0.000 0.683 0.000 1092 974 0

CH3COOC(CH3)3 (1) + C6H6 (2)T = 308.15 K

0.0000 0.8620 0.000 0.539 0.000 1260 731 00.0987 0.8593 0.100 0.540 �0.008 1215 789 260.1999 0.8568 0.200 0.542 �0.005 1179 840 430.2990 0.8549 0.270 0.544 �0.011 1150 884 560.3982 0.8532 0.324 0.548 �0.013 1127 923 620.4980 0.8519 0.343 0.552 �0.015 1107 957 640.5995 0.8508 0.346 0.558 �0.015 1091 987 600.6996 0.8500 0.311 0.565 �0.014 1079 1011 520.7999 0.8495 0.250 0.574 �0.010 1068 1031 390.8993 0.8494 0.131 0.584 �0.006 1060 1048 231.0000 0.8494 0.000 0.596 0.000 1055 1058 0

CH3COOC(CH3)3 (1) + C6H5CH3 (2)T = 298.15 K

0.0000 0.8622 0.000 0.556 0.000 1312 674 00.0976 0.8619 0.021 0.567 �0.002 1275 713 100.1986 0.8616 0.050 0.577 �0.004 1242 752 190.2993 0.8612 0.087 0.588 �0.006 1213 790 260.3975 0.8608 0.124 0.599 �0.008 1187 824 310.4983 0.8605 0.153 0.611 �0.009 1165 857 330.5978 0.8603 0.172 0.623 �0.010 1145 887 330.6975 0.8602 0.173 0.636 �0.009 1128 914 310.7972 0.8603 0.148 0.650 �0.008 1113 938 250.8987 0.8606 0.093 0.666 �0.005 1101 958 151.0000 0.8611 0.000 0.683 0.000 1092 974 0

CH3COOC(CH3)3 (1) + C6H5CH3 (2)T = 308.15 K

0.0000 0.8525 0.000 0.494 0.000 1270 727 00.0976 0.8519 0.027 0.502 �0.002 1232 774 140.1986 0.8512 0.072 0.509 �0.005 1197 819 260.2993 0.8505 0.120 0.516 �0.008 1168 862 360.3975 0.8499 0.169 0.524 �0.010 1143 901 430.4983 0.8494 0.204 0.533 �0.011 1120 938 460.5978 0.8489 0.231 0.542 �0.012 1101 971 470.6975 0.8487 0.228 0.553 �0.012 1085 1001 440.7972 0.8487 0.194 0.565 �0.010 1072 1026 350.8987 0.8489 0.123 0.580 �0.006 1062 1045 201.0000 0.8494 0.000 0.596 0.000 1055 1058 0

CH3COOC(CH3)3 (1) + C6H5CH2CH3 (2)T = 298.15 K

0.0000 0.8644 0.000 0.631 0.000 1325 659 00.0979 0.8639 0.012 0.635 �0.001 1287 699 90.1974 0.8633 0.050 0.639 �0.003 1254 737 160.2989 0.8626 0.102 0.641 �0.006 1224 774 210.3983 0.8619 0.160 0.644 �0.008 1198 808 240.4976 0.8613 0.210 0.647 �0.010 1176 840 240.5986 0.8607 0.242 0.651 �0.011 1155 871 240.6977 0.8604 0.251 0.656 �0.011 1137 899 200.7979 0.8630 0.219 0.663 �0.010 1121 925 150.8978 0.8605 0.144 0.671 �0.007 1106 950 81.0000 0.8611 0.000 0.683 0.000 1092 974 0

CH3COOC(CH3)3 (1) + C6H5CH2CH3 (2)T = 308.15 K

0.0000 0.8554 0.000 0.569 0.000 1280 714 00.0979 0.8547 0.006 0.571 �0.001 1245 755 70.1974 0.8539 0.035 0.573 �0.002 1214 795 130.2989 0.8529 0.083 0.573 �0.004 1186 834 18

(continued on next page)

M. Hasan et al. / J. Chem. Thermodynamics 43 (2011) 1389–1394 1391

TABLE 2 (continued)

x1 q � 10�3/(kg �m�3) VE � 106/(m3 �mol�1) g/(mPa � s) Dg/(mPa � s) u/(m � s�1) js/(TPa�1) Djs/(TPa�1)

0.3983 0.8520 0.126 0.574 �0.005 1161 870 200.4976 0.8511 0.172 0.575 �0.007 1139 905 200.5986 0.8503 0.206 0.576 �0.009 1119 939 200.6977 0.8497 0.210 0.579 �0.009 1101 971 170.7979 0.8493 0.192 0.582 �0.008 1085 1001 130.8978 0.8492 0.126 0.588 �0.005 1069 1030 71.0000 0.8494 0.000 0.596 0.000 1055 1058 0

TABLE 3Parameters and standard deviation r of equations (5) and (6) for tert-butyl acetate(TBA) + benzene, +methylbenzene, +ethylbenzene.

T/K a0 a1 a2 r

CH3COOC(CH3)3 (1) + C6H6 (2)VE/(cm3 �mol�1) 298.15 0.9491 0.1008 �0.0504 0.004

308.15 1.4080 0.2243 �0.1466 0.006Dg /(mPa � s) 298.15 �0.0406 �0.0111 �0.0065 0.0004

308.15 �0.0584 �0.0096 �0.0023 0.0006Djs/(TPa�1) 298.15 195.98 �24.12 �0.6293 0.16

308.15 252.50 �23.02 27.07 0.60

CH3COOC(CH3)3 (1) + C6H5CH3 (2)VE/(cm3 �mol�1) 298.15 0.6150 0.4958 0.0217 0.001

308.15 0.8290 0.6415 0.0028 0.002Dg/(mPa � s) 298.15 �0.0363 �0.0199 �0.0036 0.0003

308.15 �0.0464 �0.0259 0.0018 0.0004Djs/(TPa�1) 298.15 133.23 30.45 9.96 0.31

308.15 187.63 41.05 4.38 0.48

CH3COOC(CH3)3 (1) + C6H5CH2CH3 (2)VE/(cm3 �mol�1) 298.15 0.8388 0.8844 0.0221 0.002

308.15 0.6915 0.8057 0.0504 0.002Dg/(mPa � s) 298.15 �0.0394 �0.0375 �0.0064 0.0005

308.15 �0.0291 �0.0291 �0.0064 0.0004Djs/(TPa�1) 298.15 97.77 �8.20 �4.27 0.22

308.15 83.22 �2.31 �7.36 0.38

0.00

0.10

0.20

0.30

0.0 0.2 0.4 0.6 0.8 1.0

x1

VE /(

cm3 .m

ol-1

)

FIGURE 1. Excess molar volumes (VE) at 298.15 K for x1 tert-butyl acetate + (1 � x1)benzenes: j benzene; d methylbenzene; N ethylbenzene.

-0.012

-0.007

-0.002

0.0 0.2 0.4 0.6 0.8 1.0

x1

Δη

/(mP

a.s)

FIGURE 2. Deviations in viscosity (Dg) at 298.15 K for x1 tert-butyl ace-tate + (1 � x1) benzenes: j benzene; d methylbenzene; N ethylbenzene.

TABLE 4Interaction parameters and standard deviations r of equations (7) and (8) for tert-butyl acetate + benzene, +methylbenzene, +ethylbenzene.

System T/K G12 r

tert-Butyl acetate + benzene 298.15 �0.0586 0.12308.15 �0.1023 0.06

tert-Butyl acetate + methylbenzene 298.15 �0.0360 0.22308.15 �0.0743 0.19

tert-Butyl acetate + ethylbenzene 298.15 �0.0591 0.44308.15 �0.0571 0.26

0

10

20

30

40

50

60

0.0 0.2 0.4 0.6 0.8 1.0

x1

ΔK

s/ (T

Pa-1

)

FIGURE 3. Deviation in isentropic compressibility (Djs) at 298.15 K for x1 tert-butyl acetate + (1 � x1) benzenes: j benzene; d methylbenzene; N ethylbenzene.

1392 M. Hasan et al. / J. Chem. Thermodynamics 43 (2011) 1389–1394

decreases when a bulkier ethyl group is substituted. Therefore theVE values follow the order TBA + benzene > TBA + ethylbenzene >TBA + methylbenzene.

The VE values for the binary mixture of TBA with benzene andmethylbenzene increase with an increase in temperature whereasthe VE values decrease with an increase in temperature for the bin-ary mixture of TBA with ethylbenzene.

Figure 2 depicts the variation of Dg with the mole fraction x1 ofTBA. The Dg values of many organic liquids with aromatic hydro-carbons are characterized by negative and very low (almost ideal

TABLE 5Parameters of Jouyban–Acree model and average percentage deviation for densities, viscosities, and speed of sound.

System Ao A1 A2 A3 A4 APD

Densitytert-Butyl acetate + benzene �5.4861 0.4606 0.0615 0.2623 0.02tert-Butyl acetate + methylbenzene �2.2554 �1.1937 0.0835 �0.1597 0.01tert-Butyl acetate + ethylbenzene �1.928 �1.8392 �0.0151 0.00

Viscositytert-Butyl acetate + benzene �2.2554 �1.1937 0.0835 �0.1597 0.01tert-Butyl acetate + methylbenzene �18.7724 �10.2031 �0.1268 �1.4133 2.0568 0.14tert-Butyl acetate + ethylbenzene �16.059 �16.524 �0.5149 0.03

Speed of soundtert-Butyl acetate + benzene �47.1654 12.4093 �6.4449 0.2663 0.11tert-Butyl acetate + methylbenzene �39.1336 0.4846 �2.1562 1.0579 0.10tert-Butyl acetate + ethylbenzene �25.6926 6.1568 �0.9600 0.0955 0.04

TABLE 6FTIR stretching frequency (cm�1) of tert-butyl acetate (TBA) (x1) and benzene,methylbenzene, ethylbenzene (1 � x1).

x1 mC@O mC–H mC@C mC–O

TBA (x1) + benzene (1 � x1)0.0 3057.27 (s) 1475.59 (m)

3039.91 (s)0.4 1730.21 (s) 2978.19 (m) 1465.95 (m) 1261.49 (s)

1166.97 (s)0.5 1732.13 (s) 2976.26 (m) 1464.02 (m) 1261.49 (s)

3061.13 (shoulder) 1168.90 (s)0.6 1730.21 (s) 2970.48 (m) 1462.09 (m) 1261.49 (s)

1168.90 (s)0.7 1734.06 (s) 2974.33 (m) 1462.09 (m) 1261.49 (s)

1168.90 (s)0.8 1734.06 (s) 2982.05 (m) 1464.02 (m) 1263.42 (s)

1168.90 (s)1.0 1732.13 (s) 2982.05 (m) 1261.49 (s)

1168.90 (s)

TBA (x1) + methylbenzene (1 � x1)0.0 2922.25 (m) 1460.16 (s)

2868.24 (shoulder)3026.41 (m)

0.4 1735.99 (w) 2924.18 (m) 1458.23 (m) 1033.88 (w)2868.24 (shoulder) 1168.90 (w)3028.34 (m)

0.5 1732.13 (s) 2978.19 (s) 1375.29 (m) 1261.49 (s)1168.90 (s)

0.6 1735.99 (s) 2978.19 (s) 1373.36 (m) 1261.49 (s)2929.97 (shoulder)

1170.83 (s)0.7 1735.99 (s) 2980.12 (m) 1373.36 (m) 1261.49 (s)

2929.97 (shoulder)1170.83 (s)

0.8 1734.06 (s) 2980.12 (m) 1373.36 (m) 1261.49 (s)1168.90 (s)

1.0 1732.13 (s) 2982.05 (m) 1261.49 (s)1168.90 (s)

TBA (x1) + ethylbenzene (1 � x1)0.0 2966.62 (s) and

Many peaks within 1454.38 (m)2872.10 to 3068.85

0.4 1730.21 (s) 2958.90 (s) 1465.95 (m) 1263.42 (s)1375.29 (m) 1168.90 (s)

1261.49 (s)0.5 1732.13 (s) 2972.40 (m) 1465.95 (m) 1168.90 (s)

3074.63 (shoulder) 1452.45 (m)1373.36 (m)

0.6 1732.13 (s) 2976.29 (m) 1454.38 (m) 1261.49 (s)3072.71 (shoulder) 1373.36 (m) 1170.83 (s)

0.7 1732.13 (s) 2966.62 (m) 1464.02 (m) 1261.49 (s)1454.38 (m) 1168.90 (s)1375.29 (m)

0.8 1734.06 (s) 2978.19 (m) 1460.16 (m) 1261.49 (s)1373.36 (m) 1170.83 (s)

1.0 1732.13 (s) 2982.05 (m) 1261.49 (s)1168.90 (s)

w – weak, m – medium, s – strong.

M. Hasan et al. / J. Chem. Thermodynamics 43 (2011) 1389–1394 1393

nature) values [7–12]. The Dg values are negative in all systemswith nearly the same magnitude. The negative Dg values showthat there are only weak interactions present in the binary mix-tures studied. The Dg values show little or no effect oftemperature.

The viscosities of the binary mixtures have been correlated withthe help of Grunberg and Nissan [13] viscosity model.

ln g ¼ x1 ln g1 þ x2 ln g2 þ x1x2G12; ð7Þ

where G12 is an interaction parameter which is a function of thecomponents 1 and 2 as well as temperature.The correlating abilityof equation (7), was tested by calculating the percentage standarddeviation r between the experimental and calculated viscosity as

r ¼X

gexpt � gcalc

� �.mexpt

� �2�ðn�mÞ

� �1=2

; ð8Þ

where n represents the number of experimental points and m rep-resents the number of coefficients.

Table 4 includes the parameters for Grunberg�Nissan and per-centage standard deviations. From table 4, it is seen that the valuesof G12 are negative for the binary mixtures of TBA with benzene,methylbenzene, and ethylbenzene.

The variation of Djs with mole fraction x1, of TBA is representedin figure 3.The Djs are positive in all systems. Kiyohara and Benson[14] suggested that, Djs is the resultant of several opposing effects.The positive values may be attributed to the size of these mole-cules that allow relative molecular interactions between acetatemolecules [15].

The Jouyban and Acree [16,17] proposed a model for correlatingthe density and viscosity of liquid mixtures at various tempera-tures. The proposed equation is

ln ym;T ¼ f1 ln y1;T þ f2 ln y2;T þ f1f2

XAjðf1 � f2Þj=Th i

; ð9Þ

where ym,T, y1,T and y2,T is density, or viscosity of the mixture andsolvents 1 and 2 at temperature, respectively, f1and f2 are the molefraction, and Aj are the model constants.

Jouyban–Acree model is applied to density, viscosity, and speedof sound data and the correlating ability of the model was tested bycalculating the average percentage deviation (APD) between theexperimental and calculated density, viscosity, and speed of soundvalues as

APD ¼ ð100=NÞX

ðjyexpt � ycalcjÞ=yexptÞ� �

; ð10Þ

where N is the number of data points in each set. The optimumnumbers of constants Aj, in each case, were determined from theexamination of the average percentage deviation value.

The constant Aj calculated from the least squares analysis, arepresented in table 5 along with the average percentage deviation

1394 M. Hasan et al. / J. Chem. Thermodynamics 43 (2011) 1389–1394

(APD). The proposed model provides reasonably accurate calcula-tions for the density, viscosity, and speed of sound of binary liquidmixtures at various temperatures and the model could be used indata modeling.

From table 6, for TBA + benzene, irregular trend in mC@O is ob-served. While mC–H decreased from x1 = 0.4 up to 0.6, it increasedfrom x1 = 0.7 onwards. Also mC@C decreased from x1 = 0.4 up to 0.7and increased at x1 = 0.8. The mC–O almost remains the same. It isconcluded that there is dipole-induced dipole interaction takingplace between p-electron cloud of aromatic ring and carbonylgroup of TBA due to steric hindrance created by methyl groups ofTBA.

mC@O of TBA + methylbenzene remains same in the regionx1 = 0.4 to 0.7 except at x1 = 0.5. It continuously decreased fromx1 = 0.8 onwards. mC–H remained same in the region x1 = 0.0 to0.4 and then increased from x1 = 0.5 onwards. mC@C did not changebetween x1 = 0.5 and 0.8, while mC–O remains same in all x1. Thisreveals that electron donating inductive effect of CH3 group of phe-nyl ring disturbs aromatic mC@C.

mC@O remains same in all x1 of TBA + ethylbenzene, while anirregular trend in alkyl mC–H is observed. mC@C showed maximaat x1 = 0.4 then almost remains same. mC–O variation is very smallin magnitude. From observations of system II and III, it is clear thatadditional CH2 group in ethylbenzene as compared to methylben-zene effects mC@C and mC–H as compared to methylbenzene andthe magnitude of interaction is small in ethylbenzene.

Acknowledgment

Authors thank Principal, Dr. D.F. Shirude, M.S.G. College, Male-gaon-Camp for the facilities provided.

References

[1] M. Sakurai, K. Nakamura, K. Nitta, J. Chem. Eng. Data 41 (1996) 1171–1175.[2] G. Chandrasekhar, P. Venkatesu, M.V. Prabhakara Rao, Phys. Chem. Liq. 40

(2002) 81–189.[3] U.B. Kadam, A.P. Hiray, A.B. Sawant, M. Hasan, J. Chem. Thermodyn. 38 (2006)

1675–1683.

[4] K.N. Marsh, Recommended Reference Materials for the Realisation ofPhysicochemico Properties, Blackwell Scientific Publication, Oxford, UK, 1987.

[5] O. Redlich, A.T. Kister, Ind. Eng. Chem. 40 (1948) 345–348.[6] S. Maken, A. Gaur, N. Verma, K.C. Singh, S. Lee, J.W. Park, J. Ind. Eng. Chem. 7

(2007) 1098–1102.[7] M.M. Palaiologou, J. Chem. Eng. Data 41 (1996) 1036–1039.[8] S. Viswanathan, M. Anand Rao, D.H.L. Prasad, J. Chem. Eng. Data 45 (2000)

764–770.[9] S. Singh, B.P.S. Sethi, R.C. Katyal, V.K. Rattan, J. Chem. Eng. Data 50 (2005) 12–

127.[10] S. Varshney, M. Singh, J. Chem. Eng. Data 51 (2006) 1136–1140.[11] K.J. Han, J.H. Oh, S.J. Park, J. Chem. Eng. Data 51 (2006) 1339–1344.[12] D. Agrawal, M. Singh, J. Chem .Eng. Data 49 (2004) 1218–1224.[13] L. Grunberg, A. Nissan, Nature 164 (1949) 799–800.[14] O. Kiyohara, G.C. Benson, J. Chem. Thermodyn. 11 (1979) 861–863.[15] J.M. Resa, C. Gonzalez, R.G. Concha, M. Iglesias, Phys. Chem. Liq. 42 (2004)

521–543.[16] A. Jouyban, M. Khoubnasabjafari, Z. Vaez-gharamaleki, Z. Fekari, W.E. Acree Jr.,

Chem. Pharm. Bull. 53 (2005) 519–523.[17] A. Jouyban, A. Fathi Azarbayjani, M. Khoubnasabjafari, W.E. Acree Jr., Indian J.

Chem. 44 (2005) 1553–1560.[18] M. Sakurai, K. Nakamura, K. Nitta, N. Takenaka, K. Mukae, J. Chem. Eng. Data 43

(1998) 249–254.[19] B.B. Gurung, A. Choudhary, M.N. Roy, J. Indian Chem. Soc. 81 (2004) 330–334.[20] V. Vyas, S.V. Krishna, J. Pure Appl. Ultrason. 19 (1997) 50–56.[21] N.C. Erarchos, M.T. Margari, I.N. Demtropoulos, J. Chem. Eng. Data 40 (1995)

567–571.[22] J. George, N.V. Sastry, J. Chem. Eng. Data 49 (2004) 1116–1126.[23] J.A. Al-Kandary, A.S. Al-Jimaz, A.H.M.A. Latif, J. Chem. Eng. Data 51 (2006)

2074–2082.[24] T.M. Aminabhavi, K. Banerjee, R.H. Balundgi, Indian J. Chem. 38 (1999) 768–

777.[25] S.L. Ostwal, A.G. Kotiya, M.V. Pandya, Indian J. Chem. 17 (1979) 605–607.[26] A.F.A. Asfour, M.H. Siddique, D.V. Traintafillos, J. Chem. Eng. Data 35 (1990)

192–198.[27] T.M. Aminabhavi, V.A. Aminabhavi, S.S. Joshi, R.H. Balundgi, Indian J. Technol.

29 (1991) 545–557.[28] P.S. Nikam, B.S. Jagdale, A.B. Sawant, M. Hasan, J. Pure Appl. Ultrason. 22 (2000)

115–122.[29] Y. Changsheng, Y. Wali, M. Peisheng, J. Chem. Eng. Data 50 (2005) 1197–1203.[30] T.M. Aminabhavi, S. Joshi, Indian J. Technol. 30 (1992) 197–208.[31] P. Venkatesu, M.V. Prabhakara Rao, Phys. Chem. Liq. 34 (1997) 213–219.[32] M. Fermeglia, R. Lapasin, G. Torriano, J. Chem. Eng .Data 35 (1990) 260–265.[33] P. Venkatesu, D. Venkatesu, M.V. Prabhakar Rao, Indian J. Pure Appl. Phys. 31

(1993) 818–822.

JCT 10-414