Science Journal of Pure and Applied Chemistry
ISSN: 2276-6308
Published By
Science Journal Publication
http://www.sjpub.org
© Author(s) 2013. CC Attribution 3.0 License.
International Open Access Publisher
doi: 10.7237/sjpac/196
Research Article
Density and Viscosity Study of Binary Mixtures of Ethanol -Water at Different
Temperatures
Arun Nikumbh ¹ and Ganesh Kulkarni *¹
1 P.g.department of Chemistry,
S.s.g.m.college, Kopargaon.-423601.
(M.s.) India.
Email: Ganeshkulkarni.1841@rediffmail.com
Accepted 23 March, 2013
Abstract- Density and viscosity of ethyl alcohol with its binary mixtures
have been measured as a function of composition over the temperature
range of 298.15, 303.15, 308.15, 310.15 and 313.15 K. The excess molar
volume, excess viscosity, excess free energy of activation of viscous flow and
interaction parameters of Grunberg and Nissan’s have been calculated from
the experimental data as a function of composition. All the excess functions
are found to be either positive or negative over the entire range of
composition depending on the molecular interaction and the nature of liquid
mixtures. Further the density and viscosity data have been theoretically
analyzed for the validity of several viscosity models. The main thrust of the
study is to co-relate the excess properties and the relevant interaction
parameters with the nature of molecular interactions between the mixing
components.
In this paper we report experimental data of densities (d), η, ΔG #E, H12, d12,
A12, T12 parameters of binary mixtures of ethanol - water at different
temperatures.
Keywords: density, viscosity, relative viscosities, interaction parameters.
Introduction
Experimental
A.R.grade ethanol was distilled in quick fit glass assembly.
Water was triply distilled to get it in pure form in presence of
permanganate. The purities for the samples were tested by
their physical properties (density and viscosity). These
physical properties were compared with reported data1.
Binary mixtures were prepared by weight percent. The
measurement of weights are performed on a single pan
analytical balance (Dona 100 India) with a precision of 0.01 x
10 -6 kg. The required properties of the mixture are measured
on the same day. The uncertainty is estimated to be less than
± 1 x 10 -4. The density of pure liquids and their mixtures are
determined by using a double arm pycnometer 2. Ubbelohde
viscometer has been used to measure the flow time of pure
liquids and liquid mixtures. It is calibrated with benzene,
acetone, aniline, carbon tetra chloride and nitrobenzene and
tripled distilled water.
The viscosities of both the pure liquids and liquid mixtures
were measured at 298.15, 303.15, 308.15, 310.15 and 313.15
K at atmospheric pressure with an Ubblohde viscometer.
Result and Discussion
The excess molar volume VE of binary liquid mixtures was
evaluated using the following equation.
VE =
(X1M1  X2M2) (X1M1) (X2M2)

d12
d1
d2
…….1
Where X1 and X2 are the mole fraction of components
1(ethanol) and 2(water) respectively. M1 and M2 are the
molar mass of components 1 and 2 respectively.d12 is density
of the binary liquid mixtures, d1 and d2 are density of
component 1 and component 2 respectively.
Science Journal of Pure and Applied Chemistry
Fig: 1. Plot of VE verses mole fraction of ethanol at 310.15 K.
Since the values of VE are near about same at five selected
temperatures the plot of VE verses mole fraction of ethanol at
310.15K is shown in fig.1.It is seen from Table. 1 and Fig. 1
the values of VE are negative for ethanol – water mixtures
over the whole composition range studied at specified
temperatures. The VE values decrease with increase in
composition (mole fraction) of ethanol. The negative value of
VE may be ascribed to the intestinal accommodation of
alcohol molecules in to the H- bonded aggregates of water.
The VE values increase with mole fraction of alcohol.
The deviation in viscosity were calculated from the following
equation
Δη = η12 – (X1 η1 + X2 η2)
P a g e |2
………2
Where η1 and η2 are viscosities of component 1 and
component 2 respectively. X1 and X2 are the mole fraction of
component 1 and component 2 respectively. A perusal of
Table 2 and Fig. 2 show that the values of Δη are positive over
the selected range of composition at the specified
temperatures. The Δη values decrease with increase in
temperature over the selected composition range. Blanco et al
3 have reported positive Δη values for ester + hydrocarbon
mixtures at various temperatures.
How to Cite this Article: Arun Nikumbh and Ganesh Kulkarni “Density and Viscosity Study of Binary Mixtures of Ethanol -Water at Different Temperatures”
Science Journal of Pure and Applied Chemistry, Volume 2013, Article ID sjpac-196, 13 Pages, 2012. doi: 10.7237/sjpac/196
Science Journal of Pure and Applied Chemistry
The variation of VE and Δη with mole fraction of alcohol for
ethanol-water mixtures at various temperatures are depicted
in Table.1 and Table.2 respectively. The negative values of V E
can be explained by considering the chemical or specific
interactions which have resulted from difference in molecular
volumes and free volumes10, possible association by
hydrogen bonds and/or dipole-dipole interactions leading to
weak complex formation. The large negative values of VE arise
due to increased interactions13 between unlike molecules14, 15
or very large differences in the molar volume of pure
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components at low temperatures. The VE becomes less
negative with increasing mole fractions. The VE values are
near about constant over temperature range studied. The
negative VE arise several contributions involving specific
interactions, interstitial accommodation and change of free
volume which seem to be probably absent in the present
investigation. Negative VE and positive Δη suggest that the
dispersion forces prevail between ethyl alcohol- water
molecules. Excess volumes are possibly influenced by 1) loss
of dipolar association and difference in size and shape11 2)
dipole-dipole, dipole induced dipole interactions and charge
transfer
Fig: 2. Plot of deviation in viscosities verses mole fraction of Ethanol at 310.05 K.
How to Cite this Article: Arun Nikumbh and Ganesh Kulkarni “Density and Viscosity Study of Binary Mixtures of Ethanol -Water at Different Temperatures”
Science Journal of Pure and Applied Chemistry, Volume 2013, Article ID sjpac-196, 13 Pages, 2012. doi: 10.7237/sjpac/196
Science Journal of Pure and Applied Chemistry
complexation between unlike molecules8. The former effect
leads to expansion in volume while the latter effect
contributes to contraction in volume .The experimental
results suggest that the latter effect is dominant in all
mixtures over selected range of composition at five selected
temperatures.The excess Gibb’s free energy of activation of
flow ΔG#E for the binary liquid mixtures were calculated from
the equation
ΔG#E = RT [{ln (η V) – X1 ln (η1 V1) - X2 ln (η2 V2)
………3.
Where V1, V2 and V are the molar volumes of the component
1, component 2 and mixture respectively. η1 η2 and η are the
viscosities of component1, component 2 and mixture
respectively. R and T have their usual meaning. It can be
observed from Table 3 and Fig.3 that the ΔG #E values are
negative for all mixtures over entire composite on range at all
temperatures. The ΔG#E values increase with increase of
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temperatures and composition of the binary mixtures. It can
be seen that the values of ΔG#E are negative, which indicate
the dominance of 16 dispersion forces between the mixing
components 17.The densities and viscosities of mixtures of
various composition are listed in Table 4 and Table.5 It is
observed that the density decreases with increase of mole
fraction of ethanol and temperature. The Wvis values are
listed in Table.6. The G parameter is proportional to Wvis /
RT where Wvis is the interchange energy and may be
regarded as an approximate measure of interaction
parameter. It is observed that the Wvis values are decreasing
with increasing mole fraction of ethanol. The Wvis values
decrease with temperature. It can be seen from Table: 7, 8, 9
and 10 that the interaction parameters d12, A12 H12and T12 are
positive for ethanol- water mixtures at five different
temperatures. The G parameter increases with increase of
composition while decreases with increase of temperature.
Fig: 3. Plot of excess Gibb’s free energy verses mole fraction of ethanol at 310.15
How to Cite this Article: Arun Nikumbh and Ganesh Kulkarni “Density and Viscosity Study of Binary Mixtures of Ethanol -Water at Different Temperatures”
Science Journal of Pure and Applied Chemistry, Volume 2013, Article ID sjpac-196, 13 Pages, 2012. doi: 10.7237/sjpac/196
P a g e |5
Science Journal of Pure and Applied Chemistry
The H12 and T12 parameters are positive. Positive H12 and T12
support the existence of weak interactions and dispersion
forces. The d12 and H12 parameters are positive and
increasing with composition suggests that the interaction
parameters though weak are increasing with composition 8-9,
20.According to Reed 18and Mayer19excess Gibb’s free energy
of activation ΔG#E may be considered as a reliable tool to
detect the presence of interaction between molecules.
Negative values of ΔG#E can be seen in present binary
mixtures where specific interactions between molecules take
place.
G, T12 and H12 are positive for ethanol-water mixtures at
298.15, 303.15, 308.15, 310.15 and 313.15 K over the
selected composition range. This is in good agreement with
the view put forward by Jain and Singh 7 in regard the nature
of parameter d12 and T12.The positive value of H12 and T12
support the existence of weak interactions and dispersion
forces.7, 8
The several models(equations ) have been put forward from
time to time for correlating the viscosity of binary liquid
mixtures with those of the components of liquids with a view
to interpret the molecular interaction parameters of the
viscosity models Grunberg and Nissan 4 have suggested the
following logarithmic equation/ relation between the
viscosity of the binary liquid mixture and pure components
References
Viscosity Models and Interaction Parameters
ln η = X1ln η1 + X1ln η1 + X1X2 d12
…….4.
Where d12 is a constant, proportional to interchange energy,
X1 andX2 are the mole fraction ofcomponent1and
component2 respectively. η1, η2
and η12 are the dynamic
viscosities of component 1 component 2 and binary mixtures
respectively.
Tamura and Kurata have developed the following equation
for the viscosity of binary liquid mixtures.
5
η = X1Φ1 η1 + X2Φ2 η2 + 2X1 X2Φ1 Φ2) 0.5T12
….5.
Where T12 is the interaction parameter which depends on
temperature and composition of the mixture. X1 and X2 are
the mole fractions of
component 1 and component 2
respectively. η and η2 are the viscosity of the component 1
and component 2 respectively. Φ1andΦ2 volume fractions of
component 1 component 2respectively.
Hind et al have suggested the following equation for the
viscosity of binary liquid mixtures.
6
η1 = X12 η1 + X22 η2 + 2X1X2 H12
……… 6.
where H12 is Hind interaction parameter and attributed to
unlike pair interactions. X1 and X2 are the mole fraction of
component 1 and component respectively. η 1 and η 2 are
the viscosity of component 1 and component 2 respectively. It
can be seen from table.5, 9and 10 that interaction parameters
In conclusion, it may be said that observed variation of
properties of mixtures support the view that some specific
interactions occur between ethanol and water molecules
where the extent of interaction depends upon the amount of
water or ethanol molecule in the mixture.
1.
Physical constants of organic compounds , J.F.Timermann.
3.
Blanco A.M.,Ortega J,. Garcia B and Leal J.M,.Thermochima Acta.
202(1993)127.
2.
4.
5.
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8.
9.
Satyanarayana.B,. Ranjith Kumar. B,. Savita Jyostna,T and Satyanarayana
M. J.Chem.Thermodyn., 39 (2007)16.
Grunberg Land,. Nissan A.H. Nature 164(1949)799.
Tamura M and Kurata M.Bull.Chem.Soc.Jpn25 (1952)32.
HindR.K.M
C
Laughlin
R.Trans.Farady.Soc.56(1960)328.
E
and
Ubelohde
A.
Jain Pand SingM.J.Indian Chem. Soc. 82(2005)225.
Katyl R.C.,Sethi Bps and Raju K.S.N.,Indian J. Technol.,29(1999)20.
Gupta P.C.and Sing M.J. Indian Chemical Society,78(2001) 133.
10. Prolongo M.C.Masegosa R.M.Fuentes
J.Phys.Chem.88(1984) 2163.
H.I.
and
Horta
A.P.
11. Krishnaiah A,. Rao D.N.and Naidu P.R., Polish J.Chem,55(1981)2633.
12. Sangita sharma, Pragnesh Patel Rignesh Patel and Vora J.J.,
J.Ind.Council.Chem.25 (2008) 46-50.
13. A.Pal.;P.N.Haldar and W.Singh.; Indian J.Chem.Sec.A.33(1994) 154.
14. A.N.Kannappan.;S.Vanaja.; N.Palanivelu
J.Chem.Technol.,1(1994) 124.
15. P.S.Nikam.;L.N.Shirsath
and
Chem.Soc.;77(2000)244-248.
and
Mehedi
V.Rajendra.;
Hasan.;
Indian
J.Indian
16. Oswal.S.L and Rao A.V.; Indian J. Chem. 24A(1985) 1026.
17. Surabhi Singh and Mukhtar Singh.;Indian J.Of Chem. 41A(2002) 15881592.
18. Reed.T.M and TaylorT.E.; J.Phy.Chem.;63(1959)58.
19. Mayer R,;Meyor M,; Mertzer J and Paneloux J.Chem.Phy. 62(1971)405.
20. A.B. Sawant .; Ph.D. Thesis,. University of Pune ,January 1996.
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Science Journal of Pure and Applied Chemistry, Volume 2013, Article ID sjpac-196, 13 Pages, 2012. doi: 10.7237/sjpac/196
P a g e |6
Science Journal of Pure and Applied Chemistry
Table: 1. Excess volume VE for the System ethanol- water
mixtures at different temperatures. Cm3mol-1
Ethanol
Wt %
Mole
fraction
Temperature
298.15 K
303.15 K
308.15 K
310.15 K
313.15 K
1
0.0039
-80.62
-80.50
-80.48
-80.47
-80.45
2
0.0079
-79.14
-79.27
-79.20
-79.01
-79.07
3
0.0119
-77.63
-77.60
-77.58
-77.56
-797.54
4
0.016
-76.14
-76.11
-76.08
-76.07
-76.05
5
0.0201
-74.66
-74.63
-74.59
-74.59
-74.57
6
0.0243
-73.16
-73.13
-73.11
-73.09
-73.08
7
0.0285
-71.90
-71.87
-71.84
-71.83
-71.68
8
0.0328
-70.27
-70.24
-70.19
-70.13
-70.49
9
0.0372
-68.86
-68.84
-68.79
-68.78
-68.63
10
0.0416
-67.46
-67.43
-67.40
-67.39
-67.36
How to Cite this Article: Arun Nikumbh and Ganesh Kulkarni “Density and Viscosity Study of Binary Mixtures of Ethanol -Water at Different Temperatures”
Science Journal of Pure and Applied Chemistry, Volume 2013, Article ID sjpac-196, 13 Pages, 2012. doi: 10.7237/sjpac/196
P a g e |7
Science Journal of Pure and Applied Chemistry
Table:2.. Deviation in viscosity Δη for the System ethanol- water mixtures at different temperatures. η kg/m3
Ethanol
Wt %
Mole
fraction
Temperature
298.15 K
303.15 K
0.0236
0.0188
308.15 K
310.15 K
313.15 K
2
0.0079
0.3161
0.0238
0.0163
0.0140
0.0137
3
0.0119
0.0704
0.0597
0.0563
0.0339
0.0332
4
0.016
0.1059
0.0766
0.0612
0.0568
0.0521
5
0.0201
0.1374
0.1150
0.1089
0.0978
0.0744
6
0.0243
0.1731
0.1392
0.1117
0.1023
0.0938
7
0.0285
0.2125
0.1913
0.1395
0.1268
0.1103
8
0.0328
0.2491
0.2102
0.1718
0.1519
0.1377
9
0.0372
0.3127
0.2304
0.1882
0.1736
0.1564
10
0.0416
0.3597
0.2226
0.2243
0.2312
0.1803
1
0.0039
0.0033
0.0025
0.0017
How to Cite this Article: Arun Nikumbh and Ganesh Kulkarni “Density and Viscosity Study of Binary Mixtures of Ethanol -Water at Different Temperatures”
Science Journal of Pure and Applied Chemistry, Volume 2013, Article ID sjpac-196, 13 Pages, 2012. doi: 10.7237/sjpac/196
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Science Journal of Pure and Applied Chemistry
Table: 3. Excess Gibb’s free energy ΔG#E for ethanol- water mixtures at various temperatures kJ.mole-1
313.15
310.15
308.15
303.15
298.15
Temperature K
Ethanol
Wt %
Mole fraction
1
0.0039
-4.2086
-4.1988
-4.1785
-4.1779
-4.1298
2
0.0079
-4.1820
-4.1706
-4.1772
-4.1650
-4.1299
3
0.0119
-3.8655
-3.8599
-3.8874
-3.8470
-3.8415
4
0.0160
-3.7691
-3.7553
-3.7323
-3.7243
-3.7099
5
0.0201
-3.5531
-3.5456
-3.5413
-3.5109
-3.5011
6
0.0243
-3.4842
-3.4626
-3.4552
-3.4397
-3.3938
7
0.0285
-3.4377
-3.3998
-3.3638
-3.3416
-3.2924
8
0.0328
-3.2907
-3.2362
-3.1900
-3.1798
-3.1555
9
0.0372
-2.2053
-3.1937
-3.1636
-3.1626
-3.1157
10
0.0416
-2.1862
-2.1838
-2.1551
-2.1523
-2.1088
How to Cite this Article: Arun Nikumbh and Ganesh Kulkarni “Density and Viscosity Study of Binary Mixtures of Ethanol -Water at Different Temperatures”
Science Journal of Pure and Applied Chemistry, Volume 2013, Article ID sjpac-196, 13 Pages, 2012. doi: 10.7237/sjpac/196
P a g e |9
Science Journal of Pure and Applied Chemistry
Table: 4. Experimental density d0 for the ethanol- water mixtures at different temperatures. η kg/m3
2
0.0079
3
313.15 K
995.08
310.15 K
0.0039
kg/m3
308.15 K
1
303.15 K
Mole
fraction
298.15 K
Ethanol
Wt %
Temperature
993.80
992.29
991.88
990.44
993.09
991.66
988.33
987.56
987.33
0.0119
991.55
990.18
988.64
987.99
986.89
4
0.0160
999.81
988.44
986.86
986.14
985.18
5
0.0201
988.28
986.82
984.82
984.57
983.41
6
0.0243
985.31
983.75
982.62
981.73
980.87
7
0.0285
985.00
983.57
981.86
981.10
979.94
8
0.0328
982.40
980.97
979.14
978.34
977.51
9
0.0372
982.05
980.67
978.85
978.08
977.69
10
0.0416
979.31
978.09
976.56
975.96
974.56
How to Cite this Article: Arun Nikumbh and Ganesh Kulkarni “Density and Viscosity Study of Binary Mixtures of Ethanol -Water at Different Temperatures”
Science Journal of Pure and Applied Chemistry, Volume 2013, Article ID sjpac-196, 13 Pages, 2012. doi: 10.7237/sjpac/196
P a g e | 10
Science Journal of Pure and Applied Chemistry
Table: 5. Experimental viscosity η0 for the ethanol- water mixtures at different temperatures. η N.s.m-2
313.15 K
310.15 K
308.15 K
Temperature
303.15 K
Mole
fraction
298.15 K
Ethanol
Wt %
1
0.0039
0.8942
0.8032
0.7265
0.6981
0.6613
2
0.0079
0.9268
0.8260
0.7402
0.7101
0.6711
3
0.0119
0.9547
0.8520
0.7332
0.7306
0.6912
4
0.0160
1.0024
0.8801
0.7864
0.7541
0.7190
5
0.0201
1.0334
0.9193
0.8319
0.7919
0.7338
6
0.0243
1.0709
0.9442
0.8383
0.8011
0.7540
7
0.0285
1.1112
0.9401
0.8662
0.8262
0.7772
8
0.0328
1.1485
1.0111
0.8968
0.8521
0.7993
9
0.0372
1.2091
1.0413
0.9172
0.8745
0.8187
10
0.0416
1.2606
1.0743
1.0140
0.9383
0.8434
How to Cite this Article: Arun Nikumbh and Ganesh Kulkarni “Density and Viscosity Study of Binary Mixtures of Ethanol -Water at Different Temperatures”
Science Journal of Pure and Applied Chemistry, Volume 2013, Article ID sjpac-196, 13 Pages, 2012. doi: 10.7237/sjpac/196
P a g e | 11
Science Journal of Pure and Applied Chemistry
Ethanol
Wt %
Table: 6 Wvis for ethanol- water system at various temperatures.
1
Mole
fraction
0.0039
3
0.0119
2
0.0079
4
0.016
5
0.0201
6
0.0243
7
0.0285
8
0.0328
9
0.0372
10
0.0416
Temperature
298.15 K
303.15 K
308.15 K
310.15 K
313.15 K
0.8665
0.8354
0.8293
0.8146
1.7479
1.6933
0.5314
0.5233
0.3939
0.291
0.2253
0.1897
0.1581
0.1365
0.1184
0.8387
0.377
0.2892
0.2301
0.1892
0.1548
0.1341
0.1178
1.6835
0.5151
0.3766
0.2852
0.2289
0.189
0.1539
0.1335
0.1166
1.6681
0.5132
0.3689
0.2793
0.2284
0.1882
0.1534
0.1326
0.1165
1.6331
0.5041
0.303
0.2753
0.2246
0.1863
0.1531
0.1304
0.111
Table: 7 Gruenberg and Nissan’s parameters for ethanol- water system at various temperatures
Ethanol
Wt %
1
2
3
4
5
6
7
8
9
10
Temperature K
298.15 303.15
308.15
310.15
313.15
0.0039
1.1793
0.3938
0.9020
0.0737
0.2416
0.016
3.8576
3.2394
2.7004
2.5370
2.5318
Mole
fraction
0.0079
0.0119
0.0201
0.0243
0.0285
0.0328
0.0372
0.0416
3.0769
3.1508
4.1576
4.2582
4.4123
4.4763
4.8101
4.6231
2.6283
3.0051
3.5987
3.6799
3.9982
3.8433
3.8672
3.8547
2.1507
2.4967
3.4870
2.9352
3.2184
3.1829
3.1147
3.0681
1.9787
2.2801
2.6355
2.7590
2.8423
3.0494
2.9019
2.8639
2.4511
2.5789
2.7419
2.7575
2.9018
2.9345
2.9904
3.1350
How to Cite this Article: Arun Nikumbh and Ganesh Kulkarni “Density and Viscosity Study of Binary Mixtures of Ethanol -Water at Different Temperatures”
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P a g e | 12
Science Journal of Pure and Applied Chemistry
Ethanol
Wt %
1
2
3
4
5
6
7
8
9
10
Table: 8. A12 parameters for ethanol- Water system various temperatures.
Mole fraction
0.0039
0.0079
0.0119
0.0160
0.0201
0.0243
0.0285
0.0328
0.0372
0.0416
Temperature K
298.15
303.15
0.7558
0.7930
0.3974
0.5082
0.2687
0.2684
0.2039
0.2608
0.1651
0.1636
0.1395
0.1389
0.1231
0.1209
0.1071
0.1063
0.0964
0.0955
0.0862
0.0832
308.15
0.7859
0.3997
0.2653
0.2020
0.1633
0.1381
0.1197
0.1060
0.0951
0.0871
310.15
0.7761
0.3934
0.2631
0.2015
0.1631
0.1377
0.1194
0.1058
0.0952
0.0869
313.15
0.7729
0.3908
0.2622
0.2005
0.1624
0.1371
0.1189
0.1033
0.0948
0.0865
Table: 9. H12 parameters for ethanol- Water system at various temperatures.
Ethanol
Wt %
1
2
3
4
5
6
7
8
9
10
Mole fraction
0.0039
0.0079
0.0119
0.0160
0.0201
0.0243
0.0285
0.0328
0.0372
0.0416
Temperature K
298.15
303.15
0.5927
0.3430
2.5653
2.1377
3.5014
2.9981
4.0560
2.9037
4.4565
3.7589
4.6125
3.7514
4.8300
4.2418
4.9367
4.0137
5.3620
4.0131
5.1727
4.0102
308.15
0.3790
1.9700
2.3417
2.3516
3.4334
3.0802
3.2225
3.3607
3.2945
3.2540
310.15
0.0204
1.4691
2.1979
2.1717
3.0111
2.8498
2.9578
3.2610
3.2594
3.2249
313.015
0.0779
2.1012
2.6170
2.3941
2.8549
2.8753
3.1834
3.1979
3.2179
3.4040
Table: 10. T12 parameters for ethanol- Water system at various temperatures.
Ethanol
Wt %
1
2
3
4
5
6
7
8
9
10
Mole fraction
0.0039
0.0079
0.0119
0.0160
0.0201
0.0243
0.0285
0.0328
0.0372
0.0416
Temperature K
298.15
303.15
1.1793
0.3938
3.07692
2.6283
3.1508
3.0051
3.8576
3.2394
4.1576
3.5987
4.2582
3.6799
4.4123
3.9982
4.4763
3.8433
4.8101
3.8672
4.6231
3.8547
308.15
0.09025
2.1507
2.4967
2.7004
3.4870
2.9732
3.0784
3.1829
3.1147
3.0681
310.15
0.07369
1.9787
2.2800
2.5370
2.6355
2.7590
2.8423
3.0494
2.9019
2.8639
313.015
0.2416
2.4511
2.5789
2.5378
2.7419
2.7475
2.9018
2.9345
2.9904
3.1350
How to Cite this Article: Arun Nikumbh and Ganesh Kulkarni “Density and Viscosity Study of Binary Mixtures of Ethanol -Water at Different Temperatures”
Science Journal of Pure and Applied Chemistry, Volume 2013, Article ID sjpac-196, 13 Pages, 2012. doi: 10.7237/sjpac/196
P a g e | 13
Science Journal of Pure and Applied Chemistry
Table: 11. Change in free energy of activation for Ethanol- Water mixtures at various temperatures (Δμ*)
Ethanol
Wt %
1
2
3
4
5
6
7
8
9
10
Mole fraction
0.0039
0.0079
0.0119
0.0160
0.0201
0.0243
0.0285
0.0328
0.0372
0.0416
Temperature K
298.15
303.15
54.8437
55.4262
54.9596
55.6003
55.0055
55.7022
55.1756
55.8044
55.2952
55.9339
55.4031
56.0251
55.5150
56.1788
55.6191
56.2505
55.7676
56.3279
55.8371
56.4198
308.15
56.1437
56.2419
56.3616
56.4383
56.5985
56.6453
56.7495
56.8595
56.9944
57.0151
310.15
56.4040
56.5020
56.5945
56.6974
56.8334
56.8971
56.9946
56.0979
56.1821
57.2650
313.015
56.8467
56.9468
57.0440
57.1372
57.2398
57.3322
57.4553
57.5568
57.6665
57.8052
How to Cite this Article: Arun Nikumbh and Ganesh Kulkarni “Density and Viscosity Study of Binary Mixtures of Ethanol -Water at Different Temperatures”
Science Journal of Pure and Applied Chemistry, Volume 2013, Article ID sjpac-196, 13 Pages, 2012. doi: 10.7237/sjpac/196