Thermophysical Properties of Acetophenone with Ethylchloroacetate at Temperatures of 303.15, 313.15 and 323.15 K

Journal of the Korean Chemical Society.
2012.
Aug,
56(4):
424-430

- Received : August 12, 2011
- Accepted : July 03, 2012
- Published : August 20, 2012

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Densities, viscosities, refractive indices and speed of sounds of the binary mixtures of Acetophenone with Ethylchloroacetate were measured over the entire mole fractions at (303.15, 313.15 and 323.15) K. From these experimental results, excess molar volume
V^{E}
, viscosity deviation Δη, refractive index deviation Δ
n_{D}
, deviations in speed of sound Δ
u
, deviations in isentropic compressibility Δ
k_{s}
and excess intermolecular free length Δ
L_{f}
were calculated. The viscosity data have been correlated with the equations of Grunberg and Nissan, Hind et al., Tamura and Kurata, Katti and Chaudri, Sedgwick, Krishnan-Laddha and McAllister. The thermo physical properties under study were fit to the Jouyban-Acree model. The excess values were correlated using Redlich-Kister polynomial equation to obtain their coefficients and standard deviations. It was found that in all cases, the data obtained fitted with the values correlated by the corresponding models very well. The results are interpreted in terms of molecular interactions occurring in the solution.
n_{D}
) and ultrasonic velocity (
u
) of pure acetophenone and ethylchloroacetate as well as for the binary system constituted by these two chemicals at temperatures of 303.15, 313.15 and 323.15 K. The viscosity values have been fitted to Grunberg and Nissan,
6
Hind et al.,
7
Tamura and Kurata,
8
Katti and Chaudhari,
9
Sedgwick,
10
McAllister
11
and Krishnan and Laddha model.
12
The Jouyban-Acree model
13
has also been extended to density, viscosity, refractive index and ultrasonic velocity of binary mixture. The deviation values have been fitted to Redlich-Kister type
14
equation. Literature survey showed that no measurements have been previously reported for the mixture studied in this paper.
T
=303.15 K in
1
.
Comparison of experimental and literature values of acetophenone and ethylchloroacetate at 303.15 K
^{3}
and a capillary of an internal diameter of about 1 mm is used to measure the densities (ρ) of pure liquids and binary mixtures. The pycnometer is calibrated by using conductivity water (having specific conductance less than 1×10
^{-6}
ohm
^{-1}
) with 0.9970 and 0.9940 g·cm
^{-3}
as its densities at T=(298.15 and 308.15) K, respectively. The pycnometer filled with air bubbles free liquids is kept in a thermostat with a thermal stability of ±0.01 K for over 30 min to attain thermal equilibrium. The precision of the density measurements was estimated to be ±0.0002 g·cm
^{-3}
.
where the two constants
a
and
b
were obtained by measuring the flow time
t
of benzene.
^{-1}
. The isentropic compressibility was calculated by the equation
where ρ is the density of the mixture and u is the ultrasonic velocity of the mixture. The intermolecular free length (
L_{f}
) was calculated by the equation
where K = ((91.368 + 0.3565T)×10
^{-8}
) is temperature dependent Jacobson’s constant.
_{D}
) and ultra sonic velocities (u) of acetophenone with ethylchloroacetate mixtures at various temperatures are listed in
2
. Excess molar volumes
V^{E}
are calculated from the measured densities (ρ) by using equation
where ρ
_{m}
is the density of the mixture and M
_{1}
, ρ
_{1}
,
x
_{1}
and M
_{2}
, ρ
_{2}
,
x
_{2}
are molecular mass, density and mole fractions of pure acetophenone (1) and ethylchloroacetate (2), respectively. The uncertainty in the measurement of
V^{E}
was found to be ±0.0003 cm
^{3}
mol
^{-1}
. The deviations in viscosities, Δη, are computed using the relationship
where η is the dynamic viscosity of the mixture and η
_{1}
,
x
_{1}
and η
_{2}
,
x
_{2}
are the viscosity and mole fractions of pure acetophenone (1) and ethylchloroacetate (2), respectively. The uncertainty in the measurement of Δη was found to be ±0.0001. The deviations of refractive index (Δ
n_{D}
) over the entire mole fraction range are obtained by
The isentropic compressibility deviation (Δ
k_{s}
) over the entire composition range are obtained by
k_{s}
_{1}
,
k_{s}
_{2}
, and
k_{s}
refer to the isentropic compressibility of components 1 and 2 and the mixture, respectively.
Densities ρ, viscosities η, refractive indices n_{D} and ultrasonic velocity u for the Acetophenone (1) + Ethylchloroacetate (2) mixture at T = (303.15, 313.15, and 323.15) K
The change of intermolecular free length (Δ
L_{f}
) on mixing are calculated by the equation
where
L_{f}
_{1}
and
L_{f}
_{2}
refer to the intermolecular free length of component 1 and 2.
The excess molar volumes, deviations of viscosity, deviations of refractive index, isentropic compressibility deviation and change of intermolecular free length were fitted to a Redlich-Kister
14
equation of the type
where Y is either
V^{E}
, Δη, Δ
n_{D}
, Δ
u
, Δ
k_{s}
or Δ
L_{f}
and
n
is the degree of polynomial. Coefficients Ai were obtained by fitting equation (9) to experimental results using a leastsquares regression method. In each case, the optimum number of coefficients was ascertained from an examination of the variation in standard deviation (S). S was calculated using the relation
where
N
is the number of data points and
n
is the number of coefficients. The calculated values of coefficients along with the standard deviation (
S
) are given in
3
. Interaction parameters and standard deviations of the McAllister model and Krishnan and Laddha model for the viscosity of acetophenone and ethylchloroacetate mixtures at (303.15, 313.15, and 323.15) K are presented in
4
and
5
. Interaction parameters and standard deviations of the Grunberg and Nissan, Hind, Tamura and Kurata, Katti and Chaudri, and Sedgwick models are presented in
6
. Constants and standard deviations of the Jouban-Acree model of the acetophenone and n-alkyl acetate at (303.15, 313.15, and 323.15) K are presented in
7
.
Parameters and standard deviations (S ) of Redlich-Kister equation for Acetophenone (1) + Ethylchloroacetate (2) mixture at T = (303.15, 313.15, and 323.15) K
Parameters of the McAllister and standard deviation for the kinematic viscosity Acetophenone (1) + Ethylchloroacetate (2) mixtures at T = (303.15, 313.15, and 323.15) K
Parameters of the Krishnan - Laddha and standard deviation for the kinematic viscosity Acetophenone (1) + Ethylchloroacetate (2) mixtures at T = (303.15, 313.15, and 323.15) K
Interaction parameters (G_{12}), (T_{12}), (H_{12}), (C) and (K_{12}) for Acetophenone and Ethylchloroacetate mixtures at 303.15, 313.15 and 323.15 K
The excess molar volumes with the mole fraction (
x
_{1}
) of acetophenone and ethylchloroacetate at (303.15, 313.15 and 323.15) K are represented in
. 1
. This shows that the excess molar volumes are always positive for all the studied temperatures. The sign of excess volume of a system depends on the relative magnitude of expansion/contraction on mixing of two liquids. If the factors causing expansion dominate the factors causing contraction, then
V^{E}
becomes positive.
17
,
26
The factors that are responsible for expansion in volume are as follows. (1) Loss of dipolar association (2) the geometry of molecules structure, which does not allow fitting of one component in to other component. (3) Steric hindrance, which opposes the proximity of the constituent molecules. The experiment in present investigation indicates that the factors which are responsible for expansion in volume are dominant over the entire composition range in all the studied temperatures of acetophenone with ethylchloroacetate.
Parameters and standard deviations of Jouyban-Acree model for Acetophenone (1) + Ethylchloroacetate (2) mixture at T = (303.15, 313.15, and 323.15) K
Excess molar volume (V^{E} ) for acetophenone (1) + ethylchloroacetate (2) at ◆, 303.15 K; ■, 313.15 K; ▲, 323.15 K.
Viscosity Deviation (η) for acetophenone (1) + ethylchloroacetate (2) at ◆, 303.15 K; ■, 313.15 K; ▲, 323.15 K.
Viscosity deviations are positive over the entire range of composition for the binary mixture of acetophenone + ethylchloroacetate, which indicates that the interaction between binary mixtures is strong.
27
Experimental values of mixture viscosities and the viscosities of their components are used to evaluate the interaction parameters of various models like
G
_{12}
,
T
_{12}
,
H
_{12}
,
K
_{12}
and
C
values for the studied system are recorded in
6
. The results of refractive index deviations versus
x
_{1}
at (303.15, 313.15 and 323.15) K for the system of acetophenone and ethylchloroacetate are shown in
. 3
. In
. 3
, the positive values are observed for the system of acetophenone with ethylchloroacetate.
Refractive index deviation (Δn_{D}) for acetophenone (1) + ethylchloroacetate (2) at ◆, 303.15 K; ■, 313.15 K; ▲, 323.15 K.
Excess ultrasonic velocity deviation (Δu) for acetophenone (1) + ethylchloroacetate (2) at ◆, 303.15 K; ■, 313.15 K; ▲, 323.15 K.
The system of acetophenone and ethylchloroacetate shows negative deviations through Δ
k_{s}
isotherms over the entire range of mole fractions (
. 5
) and exhibiting a clear minima at the mole fraction around
x
_{1}
=0.45, indicating that the maximum interactions are at that mole fraction range in every system. From
. 4
, it is observed that Δ
u
values are positive while values are negative. Such a trend of positive deviation in speed of sound and negative deviation in isentropic compressibility is quite common. The excess free length is negative over the whole mole fraction range for binary mixtures at different temperatures,
. 6
. This indicates that due to intermolecular interaction, the structural readjustment occurs in the liquid mixtures towards the less compressible phase of fluid.
23
,
24
Excess isentropic compressibility (Δk_{s} ) for acetophenone (1) + ethylchloroacetate (2) at ◆, 303.15 K; ■, 313.15 K; ▲, 323.15 K.
Excess inter molecular free length (ΔL_{f} ) for acetophenone (1) + ethylchloroacetate (2) at ◆, 303.15 K; ■, 313.15 K; ▲, 323.15 K.
k_{s}
and Δ
L_{f}
. The positive deviations were observed for
V^{E}
, Δη, Δ
n_{D}
and Δ
u
. The results are analyzed in the sight of molecular interactions between the components. It may be concluded that the interactions resulting in the interstitial accommodation of ethylchloroacetate into acetophenone are the predominant factor over dipole-dipole interaction. The intermolecular interactions between acetophenone and ethylchloroacetate mixture lead to weak dispersive type. The viscosity data are correlated with the Grunberg and Nissan, Hind, Tamura and Kurata, Katti and Chaudri, Sedgwick, Krishnan- Laddha and McAllister. It has been concluded that the Jouyban Acree model is very well suited for correlating the thermo physical properties of the studied binary mixture.

INTRODUCTION

The thermodynamic and transport properties of liquids and liquid mixtures
1
are used to study the molecular interactions between the various components of the mixture and also to understand engineering applications concerning heat transfer, mass transfer, and fluid flow. In chemical process industries, materials are normally handled in fluid form, and as a consequence, the physical, chemical, and transport properties of fluids assume importance. Thus, data on some of the properties associated with the liquids and liquid mixtures like density, viscosity, refractive index and ultrasonic velocity find extensive application in solution theory and molecular dynamics.
2
Such results are necessary for interpretation of data obtained from thermo chemical, electrochemical, biochemical and kinetic studies.
3
Acetophenone is an important industrial chemical widely used as an ingredient of flavor and fragrance in soaps, detergents, cosmetics and perfumes. Ethylchloroacetate are used as a solvent in preparation of drugs, perfumes, cosmetics and pesticides. The acetophenone and ethylchloroacetate mixture is used as cosmetics, intermediates of drugs, perfumes, and pesticides. In our earlier paper, we had studied the transport properties of binary liquid mixtures.
4
,
5
In continuation of this research, we have reported density (ρ), viscosity (η), refractive index (
EXPERIMENTAL SECTION

- Materials

Acetophenone and ethylchloroacetate (Lobo Chemicals, India, and Mass fraction 0.998) were purified by using the methods described in the literature
15
,
16
and only middle fractions were used in the experiment. Binary mixtures are prepared by mixing appropriate volumes of the liquid components in the specially designed glass bottles with air tight Teflon coated caps and mass measurements performed on a Shimadzu Corporation Japan type BL 2205 electronic balance, with a precision of ±0.01 mg. The required properties are measured on the same day immediately after preparing each composition. The uncertainty of the mole fraction is ±0.0001. The experimental values of density, viscosity, refractive indices and ultrasonic velocity for the pure liquids are compared, with the available literature values at
Comparison of experimental and literature values of acetophenone and ethylchloroacetate at 303.15 K

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- Density

A double-arm pycnometer with a bulb of 25 cm
- Kinematic Viscosity

The kinematic viscosity of pure liquids and liquid mixtures were measured using Ostwald viscometer previously calibrated using water.
4
,
5
The time was measured with a precision of 0.01 s, and the uncertainty in the viscosity was estimated to be less than 0.0002 mPa·s. The kinematic viscosity was obtained from the working equation
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- Refractive Index

Refractive indices were measured using thermostatically controlled Abbe refractometer with accuracy less than 0.0001 units. Water was circulated into the prism of the refractometer by a circulation pump connected to an external thermo stated water bath. Calibration was performed by measuring the refractive indices of doubly distilled water and propyl alcohol at defined temperatures. The sample mixture was directly injected in to the prism assembly of the instrument using a syringe. The solutions were pre thermo stated at the temperature of the experience before the experiments to achieve a quick thermal equilibrium.
- Ultrasonic Velocity

The Speed of sound was measured by using a variable path, single crystal interferometer. (Mittal Enterprises, New Delhi) operating at a frequency of 2MHz, which was calibrated with water and benzene. The interferometer cell was filled with the test liquid, and the temperature of the solution was maintained constant within ±0.01 K by circulation of water from a thermostatically regulated water bath through the water jacketed cell. The uncertainty was estimated to be 0.1 ms
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RESULTS AND DISCUSSION

The experimental values of densities (ρ), viscosities (η), refractive indices (n
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Densities ρ, viscosities η, refractive indicesnDand ultrasonic velocity u for the Acetophenone (1) + Ethylchloroacetate (2) mixture atT= (303.15, 313.15, and 323.15) K

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Parameters and standard deviations (S) of Redlich-Kister equation for Acetophenone (1) + Ethylchloroacetate (2) mixture atT= (303.15, 313.15, and 323.15) K

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Parameters of the McAllister and standard deviation for the kinematic viscosity Acetophenone (1) + Ethylchloroacetate (2) mixtures atT= (303.15, 313.15, and 323.15) K

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Parameters of the Krishnan - Laddha and standard deviation for the kinematic viscosity Acetophenone (1) + Ethylchloroacetate (2) mixtures atT= (303.15, 313.15, and 323.15) K

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Interaction parameters (G12), (T12), (H12), (C) and (K12) for Acetophenone and Ethylchloroacetate mixtures at 303.15, 313.15 and 323.15 K

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Parameters and standard deviations of Jouyban-Acree model for Acetophenone (1) + Ethylchloroacetate (2) mixture atT= (303.15, 313.15, and 323.15) K

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CONCLUSIONS

Experimental data of the density, viscosity, refractive index and ultrasonic velocity of acetophenone and ethylchloroacetate mixture have been measured at 303.15, 313.15 and 323.15 K. These data have used to compute the excess molar volumes, viscosity deviations, refractive index deviations, compressibility deviation and change in intermolecular free length for mixtures of acetophenone and ethylchloroacetate. Negative deviations were observed for Δ
Acknowledgements

The authors thank the University authorities for providing the necessary facilities to carry out the work.

Kim E. S.
,
Marsh K. N.
1988
J. Chem. Eng. Data
33
288 -
** DOI : 10.1021/je00053a020**

Mchaweh A.
,
A. Alsaygh A.
,
Mosh-Feghian M. A.
2004
Fluid Phase Equilib.
224
157 -
** DOI : 10.1016/j.fluid.2004.06.054**

Kenart C. M.
,
Kenart W.
2000
Phys. Chem. Liq.
38
155 -
** DOI : 10.1080/00319100008030266**

Baskaran R.
,
Kubendran T. R.
2008
J. Chem. Eng. Data
53
978 -
** DOI : 10.1021/je700714m**

Baskaran R.
,
Kubendran T. R.
2008
J. Chem. Eng. Data
53
1956 -
** DOI : 10.1021/je8002699**

Grunberg L.
,
Nissan A.
1949
Nature
164
799 -
** DOI : 10.1038/164799b0**

Hind R. K.
,
Mclaughlin E.
,
Ubbelohde A. R.
1960
Trans. Faraday Soc.
56
328 -
** DOI : 10.1039/tf9605600328**

Tamura M.
,
Kurata M.
1952
Bull. Chem. Soc. Jpn.
25
32 -
** DOI : 10.1246/bcsj.25.32**

Katti P. K.
,
Chaudhari M. M.
1964
J. Chem. Eng. Data
9
442 -
** DOI : 10.1021/je60022a047**

Sedgwick T. O.
,
Ph.D Thesis
1962
The viscosity and thermal conductivity of liquid mixtures.
Brooklyn Polytechnic Institute
Ph.D Thesis

McAllister R. A.
1960
AIChE Journal
6
427 -
** DOI : 10.1002/aic.690060316**

Krishnan M. R. V.
,
Laddha G. S.
1963
Indian Chemical Engineer, Trans.
57 -

Jouyban A.
,
Khoubnasabjafari M.
,
Vaezgharamaleki Z.
,
Fekari Z.
,
Jr. Acree W. E.
2005
Chem. Pharm. Bull.
53
519 -
** DOI : 10.1248/cpb.53.519**

Redlich O.
,
Kister A. T.
1948
Ind. Eng. Chem.
40
345 -
** DOI : 10.1021/ie50458a036**

Perrin D. D.
,
Armerego W. L. F.
1988
Purification of Laboratory Chemistry
3rd ed.
Pergamon press
Oxford

Riddick J. A.
,
Bunger W. B.
,
Sakano T. K.
1986
Orgarnic Solvent
4th ed.
Wiley-Interscience
New York

Treszczanowicz A. J.
,
Kiyohara O.
,
Benson G. C.
1981
J. Chem. Thermodyn.
13
253 -
** DOI : 10.1016/0021-9614(81)90125-7**

Syamala V.
,
Venkateshwarlu P.
,
Sivakumar K.
2006
J. Chem. Eng. Data
51
928 -
** DOI : 10.1021/je050413l**

Manapragada V. R.
,
Sudhir M.
,
Manapragada S. K.
2010
J. Chem. Eng. Data
55
5946 -
** DOI : 10.1021/je100715x**

Surendranath K. N.
,
K. Ramanjaneyulu K.
,
Krishnaiah A.
1990
Fluid Phase Equilb.
59
225 -
** DOI : 10.1016/0378-3812(90)85037-B**

Syeda A. B.
,
Ranjith K. B.
,
Koppula A. J.
,
Sathyanarayana B.
,
Sathyanarayana N.
2010
J. Chem. Eng. Data
55
1067 -
** DOI : 10.1021/je900525f**

Sathyanarayana N.
,
Sathyanarayana B.
,
Savitha J. T.
2007
J. Chem. Eng. Data
52
405 -
** DOI : 10.1021/je060343y**

Oswal S. L.
,
Patel N. B.
2000
J. Chem. Eng. Data
45
225 -
** DOI : 10.1021/je980305h**

Rama R. G. V.
,
Viswanatha S. A.
,
Rambabu C.
2004
Indian J. Pure & Appl. Phys.
42
820 -

Jyoti N. N.
,
Mrityunjaya I. A.
,
Aminabhavi T. M.
2007
J. Chem. Eng. Data
47
964 -

Roux A.
,
Desnoyers J.
1978
Indian Acad. Proc., Chem. Soc.
78
435 -

Fort R. J.
,
Moore W. R.
1966
Trans. Faraday Soc.
62
1112 -
** DOI : 10.1039/tf9666201112**

Iloukhani H.
,
Rostami Z.
2007
J. Chem. Eng. Data
52
921 -
** DOI : 10.1021/je600519p**

Citing 'Thermophysical Properties of Acetophenone with Ethylchloroacetate at Temperatures of 303.15, 313.15 and 323.15 K
'

@article{ JCGMDC_2012_v56n4_424}
,title={Thermophysical Properties of Acetophenone with Ethylchloroacetate at Temperatures of 303.15, 313.15 and 323.15 K}
,volume={4}
, url={http://dx.doi.org/10.5012/jkcs.2012.56.4.424}, DOI={10.5012/jkcs.2012.56.4.424}
, number= {4}
, journal={Journal of the Korean Chemical Society}
, publisher={Korean Chemical Society}
, author={Saravanakumar, K.
and
Baskaran, R.
and
Kubendran, T. R.}
, year={2012}
, month={Aug}