Densities, Viscosities, and Refractive Indices of Dimethyl Carbonate +

Article pubs.acs.org/jced

Densities, Viscosities, and Refractive Indices of Dimethyl Carbonate + 1-Hexanol/1-Octanol Binary Mixtures at Different Temperatures Mehrdad Moosavi,† Ahmad Motahari,*,‡ Amir Vahid,§ Vahideh Akbar,§ Abbas Ali Rostami,† and Abdollah Omrani† †

Faculty of Chemistry, University of Mazandaran, Babolsar 47416-13534, Iran Young Researchers and Elite Club, Jahrom Branch, Islamic Azad University, Jahrom 74147-85318, Iran § Research Institute of Petroleum Industry, Tehran 14857-33111, Iran ‡

S Supporting Information *

ABSTRACT: The densities, viscosities, and refractive indices for the binary mixtures of dimethyl carbonate (DMC) + 1-hexanol/1octanol were measured at atmospheric pressure and temperature of 293.15, 298.15, 303.15, 308.15, 313.15, 318.15, and 323.15 K over the whole concentration range. Different thermodynamic, transport, and optical properties, such as excess molar volume, partial molar volume, thermal expansion coefficient, isothermal coefficient of pressure excess molar enthalpy, activation energy of flow, excess refractive index, and electronic polarizability were obtained from the experimental data. The results were analyzed in terms of specific molecular interactions and mixing behavior between mixture components with taking into considerations the effect of temperature. Moreover, the thermophysical properties were examined with predictive and correlative equations. The quality of the predictions for the studied systems was evaluated by measuring the deviations and drawing the comparison plots.

1. INTRODUCTION Dimethyl carbonate (DMC) is an environmentally benign chemical that is used in the replacement of hazardous chemicals and belongs to organic carbonate family. An increased use of DMC as a safe substitute for hazardous chemicals can be predicted; principally, as methylating agent in place of dimethyl sulfate and methyl halides and as a carbonylation agent in place of phosgene for the production of polycarbonates and polyurethanes.1−3 Furthermore, due to its high oxygen content, it can be considered as an option for meeting the oxygenated specifications on gasoline and as a means of converting natural gas to a liquid transportation fuel.4,5 Investigation on the properties of alkyl carbonate and alcohol liquid mixtures, in addition to application in crucial synthesis in chemical industries,4,6 is interested for chemists that intend to examine how the number and position of hydroxyl functional groups as well as variation in the carbon chain length of alcohols can be of influence on the thermophysical properties of DMC mixtures. For instance, Trenzado et al.7 reported the density, viscosity, and excess thermodynamic properties of diethyl carbonate with ethanol, 1-propanol, 1-pentanol, and 1octanol within the temperature range of (288.15 to 313.15) K. Francesconi and co-workers8 investigated the densities, refractive indices, and related excess parameters of diethyl carbonate with methanol, ethanol, 1-propanol, 1-butanol, 1hexanol, and 1-octanol. Li et al.9 measured excess molar © XXXX American Chemical Society

enthalpies of dimethyl carbonate with methanol, ethanol, 1propanol, and 2-propanol at different temperatures and pressures. Oh et al.10 studied the vapor−liquid equilibria at 333.15 K and excess molar volumes at 298.15 K for dimethyl carbonate + 1-propanol/1-butanol. The temperature dependence of density, refractive index and speed of sound on the binary mixtures of dimethyl carbonate + methanol, ethanol, 1propanol, 2-propanol, 1-butanol, 2-butanol, and 1-pentanol were studied by Rodriguez et al.11 In addition, Francesconi et al.12 measured the excess molar enthalpies and excess molar volumes of the binary mixtures containing dimethyl carbonate + four butanol isomers at (288.15, 298.15, and 313.15) K. Also, Romano et al.13 studied the thermophysical properties of four binary mixtures of dimethyl carbonate + 1-alcohol at temperature range of 288.15 to 313.15 K. The analysis of the reliable themophysical data and deviation from the ideality of the properties of liquid represents some important information about the solution behavior and their interactions that is essential for the industrial design and attaining acceptable chemical theories. The industry of carbonates and alcohols is very important, and therefore, it is Received: September 27, 2015 Accepted: May 4, 2016

A

DOI: 10.1021/acs.jced.5b00830 J. Chem. Eng. Data XXXX, XXX, XXX−XXX

Journal of Chemical & Engineering Data

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where t is the flow time and k is the capillary constant of viscometer. The viscosities were averaged from three measurements. The accuracy of viscosity measurements was estimated to be ±0.01 mPa s. Refractive index measurements were carried out using a digital Abbe refractometer (AR2008, Kruss-Germany). The apparatus measures refractive indices in the range of 1.3000 to 1.7200 for the temperature range of 273.15 to 372.15 K with 0.01 K resolutions. The accuracy of refractive index instrument was estimated to be less than ±0.0002 units. The experimental densities, ρ, viscosities, η, and refractive indices, nD, of pure liquids were compared with the available literature values at all studied temperatures and given in Table 2. As can be seen from Table 2, there is a good agreement between the experimental and literature values. Also, relative deviations against temperature between the experimental densities, viscosities, and refractive indices reported by different authors at atmospheric pressure for the studied pure liquids are shown graphically in Figures S1, S2, and S3. These deviations are discussed in the first section of Supporting Information.

necessary to study the thermodynamic and transport properties for these systems. This paper reports the experimental densities, viscosities, and refractive indices of DMC + 1-hexanol/1-octanol binary mixtures at temperatures of 293.15, 298.15, 303.15, 308.15, 313.15, 318.15, and 323.15 K and atmospheric pressure. Various thermophysical properties were obtained from the experimental data. The values of excess molar volume, excess refractive index, and viscosity deviation were correlated with Redlich−Kister polynomial equation. Moreover, the values of viscosity and refractive index were predicted with Grunberg− Nissan and Lorentz−Lorenz models, respectively.

2. EXPERIMENTAL SECTION 2.1. Chemicals. Dimethyl carbonate (DMC) was supplied from Sigma-Aldrich. 1-Hexanol and 1-octanol were purchased from Fluka. The purity of these chemicals was higher than 99% and their water content was less than 0.1%. All these chemicals were used without further purification and the purities were verified by measuring the normal boiling points of pure chemicals. The water content of the chemicals was measured with Kyoto mks-210 Karl Fischer instrument in order to be aware of the effect of water on temperature control. Table 1 shows the specifications of the used chemicals in detail.

3. RESULTS AND DISCUSSION Measurements of the density of DMC (x1) + 1-hexanol/1octanol (x2) as a function of temperature and concentration at constant pressure were performed at temperatures between (293.15 and 323.15) K with 5 K interval over the whole concentration range. The experimental values of densities, viscosities, and refractive indices for DMC + 1-hexanol/1octanol binary mixtures at different temperatures are presented in Table 3. Here, it should be noted that Romano et al.13 also measured the density and viscosity of DMC + 1-octanol binary mixture at temperatures of 293.15 and 303.15 K, which is common to the present study. However, our results differ from their obtained results, which may be because of the experimental protocols or of the apparatus. Graphical comparison will be shown below. The calculated thermodynamic, transport, and optical properties are given in Tables S1, S2, S3, and S4 in the Supporting Information. Figure 1 shows the temperature dependence of density (ρ − T) for DMC + 1-alkanol binaries at different temperatures. According to Figure 1, the experimental values can be fitted linearly (R2 = 0.999) as follows

Table 1. Specifications of the Used Chemicals compound DMC

a

CAS number 616-38-6

1-hexanol

111-27-3

1-octanol

111-87-5

supplier SIGMAAldrich (517127) Fluka (73117) Fluka (95446)

purity (supplier)

water content (supplier)

water content (K. F.)b

≥99%

1-hexanol >1-pentanol >1-butanol >1-propanol > ethanol > methanol. From methanol to 1-octanol, with increasing the number of −CH 2 − group in alcohol, the volume showed more expansibility and positive deviation to ideality. As Romano et al.13 discussed in their work, the positive values of excess molar volume, along with the positive values of excess molar enthalpy, indicated a preponderance of the expansive and endothermic effects associated with the rupture of the homomolecular interactions, which can finally suggest weak heteromolecular interactions. Since in all 1-alkanols the hydroxyl functional group is the same, the variation of thermophysical properties with carbon chain length can be ascribed to the structural contribution. From the above information, it can be concluded that the variation of carbon chain length (molecular size) and accommodation of molecules significantly affects the excess molar volume values. The same temperature and composition behavior was also observed for DMC + 2-alkanol and diethyl carbonate (DEC) + 1-alkanol binary systems.7,8 In the DEC + 1-alkanol binary mixtures, similar to DMC + 1-alkanol systems, the excess molar volume shifted to more positive values by increasing the carbon chain length of alcohol. Partial molar quantities are important in the study of the dependence of an extensive property on the phase composition

at constant pressure and temperature. The partial molar volume of component i in the binary mixtures, V̅ i, is defined as ⎛ ∂V ⎞ Vi̅ = ⎜ ⎟ ⎝ ∂ni ⎠T , P , n

(9)

j

where ni is the number of moles of the ith component added into the system and nj is the number of moles of the other components of the mixture. Here, with the use of excess molar volume and molar volume of the pure components, the partial molar volume of components 1 and 2, V̅ 1 and V̅ 2, in the binary mixtures were calculated using the following equations: ⎛ ∂V E ⎞ V1̅ = VmE + V1* + (1 − x1)⎜ m ⎟ ⎝ ∂x1 ⎠T , P

(10)

⎛ ∂V E ⎞ V2̅ = VmE + V 2* − x1⎜ m ⎟ ⎝ ∂x1 ⎠T , P

(11)

where V*1 and V*2 are the molar volume of pure components 1 and 2, respectively. The

∂VmE ∂x1

( )

value was calculated by the

T ,P

differentiation of the polynomial fitting of VEm equation with respect to x1. The obtained values of the partial molar volume for the studied mixtures at different temperatures are listed in Tables S1 and S2. Figure 4 shows the partial molar volumes as a function of DMC mole fraction at 298.15 K. Accordingly, with increasing the DMC concentration the partial molar volume of E



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Figure 1. Density, ρ, as a function of temperature, T, for the binary mixtures of (a) DMC + 1-hexanol and (b) DMC + 1-octanol at different DMC mole fractions, x.

entire composition range. Moreover, according to eq 12 and Figure S5, the variation of the mixture volume to temperature was negligible in comparison to the total molar volume of the mixtures. Therefore, high temperatures are required for a considerable change in the volume of the liquid. Figure S6 shows the variation of isothermal coefficient of pressure excess molar enthalpy for the binary mixtures of DMC + 1-hexanol/1-

DMC increased and inversely the partial molar volume of alcohol decreased. On the basis of Gibbs−Duhem equation, this is general for the binaries in their partial properties that with raising the partial properties of one component the partial properties of the other one decreases. The variation of entropy to pressure at constant temperature,

( ∂∂PS )T ,x, and isothermal coefficient of pressure excess molar enthalpy,

∂HmE ∂P

( )

, give useful information about the

intermolecular forces with pressure change. They can be calculated by the following relations: (12)

⎛ ∂H E ⎞ ⎛ ∂V E ⎞ ⎜ m ⎟ = VmE − T ⎜ m ⎟ ⎝ ∂P ⎠T , x ⎝ ∂T ⎠ P , x

(13)

The computed values of

∂VmE ∂T

( ∂∂PS )T ,x

T ,x

E P

P ,x

Refractive index is a property that expresses the ratio of the speed of light in vacuum relative to that in the considered medium. It is one of the important properties having many applications, such as checking the purity of materials and measuring the concentration of solutes in solutions. The experimental data for the refractive indices of DMC + 1hexanol/1-octanol binary mixtures at different temperatures are listed in Table 3. Accordingly, for both studied mixtures, the refractive index decreased when DMC mole fraction increased. The refractive index is informative about the behavior of the molecules in solution as well as forces between the molecules

( ∂∂PS )T ,x, using the densities and eq

12, for binary mixtures of DMC + 1-hexanol/1-octanol are indicated in Figure S5 in the Supporting Information. The values of

T ,x

∂HmE ∂P

T ,x

⎛ ∂S ⎞ ⎛ ∂V ⎞ ⎜ ⎟ =−⎜ ⎟ ⎝ ∂P ⎠T , x ⎝ ∂T ⎠ P , x

∂HmE ∂P

( ) for both studied systems were negative. The values of ( ) had opposite sign as those of ( ) and α for these mixtures. octanol at 298.15 K. The values of

were negative for both mixtures over the F



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Excess refractive index can be obtained by the following equation:17 * )2 + φ (nD2 * )2 ]1/2 nDE = nD − [φ1(nD1 2

(15)

where φ1 and φ2 are the volume fractions of pure components, nD is the refractive index of binary mixture, and n*D1 and n*D2 are the refractive indices of pure components at a given temperature. The values of excess refractive index, with the standard uncertainty of 0.0005, are reported in Tables S3 and S4. Figure 5 shows the composition dependence of excess refractive indices for the DMC + 1-hexanol/1-octanol binary mixtures. The excess refractive indices were correlated with Redlich−Kister eq 7 as shown in Figure 5, and the calculated values of Ai along with their standard deviations are listed in Table 4. The values of excess refractive index for both studied mixtures were negative and shifted to zero when temperature increased. Coordination between size and sign of nED and VEm is predictable. In fact, the positive excess molar volume demonstrates the week interaction between the mixture components leading to an increase in the volume of the mixture (packing effect). Hence, in the real mixtures, the free volume is more available than in the ideal state and the light travels at higher speed, so the excess refractive indices of the mixture become negative. Prediction of refractive index can be carried out by different models, such as, Arago−Biot, Gladston−Dale, Newton, Eyring−John, Edwards, Lorentz−Lorenz, Weiners, Eykman, and Hellers.18 Here, the refractive index prediction was done by Lorentz−Lorenz equation:19 ⎡ n2 − 1 ⎤ ⎡ n2 − 1 ⎤ ⎡ n2 − 1 ⎤ ⎥ ⎢ D2 ⎥ ⎥ = φ1⎢ D1 ⎢ D2 + φ 2 2 2 + 2⎦ + 2⎦ ⎣ nD2 ⎣ nD1 ⎣ nD + 2 ⎦

Figure 2. Excess molar volumes, VEm, as a function of DMC mole fraction, x1, for (a) DMC + 1-hexanol and (b) DMC + 1-octanol binary mixtures at different temperatures. The solid lines represent the corresponding correlations by the Redlich−Kister equation.

where φ1 and φ2 are the volume fractions of pure components, nD is the refractive index of binary mixture, and nD1 and nD2 are the refractive indices of pure components. Figure 6 shows this prediction at 298.15 K. Accordingly, the used mixing rule predicted the experimental refractive index data satisfactorily with the absolute average deviation of 0.119% and 0.102% for DMC + 1-hexanol or 1-octanol, respectively. Therefore, the proposed prediction equation was effective and gave a reliable estimation method for predicting the refractive index of the binaries. The absolute average deviation (AAD) was calculated as follows:

using its relation with the electronic polarizability of the molecule. Generally, an imposed electric field, F, displaces the electrons in an atom somewhat to produce a dipole moment, μ. The induced dipole moment is proportional to the electric field, μ = αeF.15 The proportionality constant is electronic polarizability, and its usual value is about actual atomic volumes. The electronic polarizability is obtained by strong correlation between density and refractive index according to the following equation:16 αe =

3ε0Vm ⎛ nD2 − 1 ⎞ ⎜ ⎟ NA ⎝ nD2 + 2 ⎠

(16)

N

ΔAAD% =

Aiexp − Aical ⎛ 100 ⎞ ⎜ ⎟ ∑ ⎝ N ⎠ Aiexp i=1

(17)

where N is the number of the experimental data points. The subscripts “exp” and “calc” represent the values of the experimental and the calculated property, respectively. The experimental data for dynamic viscosities, η, of pure components and their mixtures at different studied temperatures and compositions are reported in Table 3. The viscosities of the mixtures decreased nonlinearly with increasing DMC concentration, which is a reflection of strength of selfassociation of the molecules in the pure alcohols (Figure 7). The viscosity is one of the best criteria for determination of association of components in the mixture and pure state. On the basis of the dependency of viscosity to temperature and composition, several semiempirical relations have been proposed to estimate the viscosity of liquid mixtures. It is well known that there is no universally accepted method of

(14)

where nD, NA, and ε0 are refractive index, Avogadro’s number, and the permittivity of free space, respectively. The calculated values of electronic polarizability are reported in Tables S3 and S4 for the studied systems at all temperatures. Accordingly, the electronic polarizability decreased when DMC concentration increased. Generally, the electronic polarizability increases as volume occupied by electrons increases. The alkanols used in this study, in comparison to DMC, are larger and have less electronegative atoms (the sp2 carbon in DMC is more electronegative than a sp3 carbon). Therefore, charge distribution takes place easier, and that is why the electronic polarizability of the mixtures increased by increasing 1-hexanol or 1-octanol concentration. G



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Table 4. Coefficients of Redlich−Kister Equation for Excess Molar Volume, VEm, Excess Refractive Index, nED, and Viscosity Deviation, Δη, of DMC + 1-Hexanol/1-Octanol Binary Mixtures at Different Temperatures along with Their Standard Deviations, σ DMC + 1-hexanol T/K

A0

A1

A2

A3

DMC + 1-octanol σ

A4

293.15 298.15 303.15 308.15 313.15 318.15 323.15

3.567 3.818 4.085 4.271 4.468 4.836 4.951

1.251 1.362 1.472 1.543 1.574 1.706 1.658

−0.326 −0.513 −0.235 −0.429 −0.247 −0.196 −0.344

0.004 −0.080 −0.214 −0.269 −0.222 −0.075 −0.154

1.307 1.746 1.258 1.716 1.423 1.409 1.470

293.15 298.15 303.15 308.15 313.15 318.15 323.15

−0.013 −0.012 −0.041 −0.011 −0.011 −0.010 −0.009

−0.002 −0.002 −0.002 −0.002 −0.002 −0.002 −0.002

−0.002 −0.003 −0.004 −0.004 −0.003 −0.002 −0.001

0.006 0.007 0.006 0.007 0.007 0.007 0.007

0.009 0.010 0.012 0.013 0.012 0.012 0.010

293.15 298.15 303.15 308.15 313.15 318.15 323.15

−7.086 −5.581 −4.714 −3.976 −3.288 −3.109 4.951

4.289 3.847 3.204 2.756 2.272 1.620 1.658

−5.029 −3.886 −3.278 −2.624 −2.219 −2.006 −0.344

3.143 0.721 1.426 0.869 0.477 0.176 −0.154

0.646 0.904 0.588 0.925 0.703 0.730 1.470

VEm 0.007 0.008 0.006 0.011 0.014 0.041 0.024 nED 0.00003 0.00003 0.00007 0.00005 0.00008 0.00006 0.00007 Δη 0.029 0.014 0.010 0.012 0.005 0.103 1.911

A0

A1

4.180 4.458 4.816 5.108 5.392 5.709 5.996

σ

A2

A3

A4

0.696 0.797 0.966 1.073 1.190 1.440 1.480

−0.170 −0.650 −1.036 −1.318 −1.650 −1.241 −1.324

1.680 1.338 1.351 1.155 0.864 0.402 0.306

3.032 3.809 4.112 4.728 5.478 4.853 5.198

0.007 0.006 0.009 0.005 0.004 0.012 0.014

−0.011 −0.010 −0.010 −0.009 −0.008 −0.008 −0.008

−0.004 −0.004 −0.004 −0.004 −0.003 −0.004 −0.003

−0.011 −0.011 −0.010 −0.011 −0.011 −0.011 −0.010

0.001 0.002 0.001 0.0006 0.0009 0.0009 0.0008

0.009 0.010 0.009 0.011 0.013 0.013 0.014

0.00003 0.00004 0.00005 0.00005 0.00006 0.00003 0.00005

−12.289 −9.977 −7.831 −6.448 −5.405 −4.488 −3.697

6.873 5.435 3.991 3.325 2.639 2.244 1.861

−4.117 −2.802 −0.805 −1.299 −0.363 −0.928 −0.601

3.511 1.718 0.487 0.469 0.251 0.283 0.271

−3.341 −2.197 −1.812 −0.678 −1.458 −0.436 −0.287

0.015 0.008 0.024 0.003 0.013 0.012 0.009

Figure 3. Excess molar volumes, VEm, as a function of DMC mole fraction, x1, for different DMC + alcohols binary mixtures at 303.15 K.

ln η = x1ln η1 + x 2 ln η2 + x1x 2D12

predicting the viscosity of liquid mixtures. Almost all methods assume that values of the viscosities of the pure components are available and depend on the temperatures, mole fractions or volume fractions of components. Some of these semiempirical equations include Kendall−Monroe, Arrhenius, Grunberg− Nissan, Hind−Ubbelohde, and Frenkle.20 Here, GrunbergNissan21 was used, which has the following form:

(18)

where D12 is a parameter proportional to the interchange energy. This equation predicted the experimental viscosity values satisfactorily with the absolute average deviation of 0.855% and 2.233% for DMC + 1-hexanol or 1-octanol, respectively (Figure 8). H



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Figure 4. Partial molar volume, V̅ i, as a function of DMC mole fraction, x1, for the binary mixtures of DMC + 1-hexanol/1-octanol at 298.15 K. The solid lines are a guide to the eye.

Figure 6. Comparison of the experimental and theoretical refractive index values as a function of DMC mole fraction, x1, for (a) DMC + 1hexanol and (b) DMC + 1-octanol binary mixtures at 298.15 K.

systems, the plot of ln η against 1/T showed a linear fit with reasonable standard deviation and, therefore, was acceptable to calculate the activation energy of flow. Figure S7 reveals the activation energy of flow for DMC + 1-hexanol/1-octanol binary mixtures at 298.15 K. The values of Ea decreased with DMC concentration. The activation energies of flow for DMC + 1-octanol systems were higher than those of DMC + 1hexanol systems, which can be explained by the difference in the solvent viscosity. Although doubts have been cast on the legitimacy of applying the thermodynamic concepts of ideal and excess quantities to the viscosity which is a transport property,17 the viscosity deviation eq (eq 19) has been used in many literatures and gives favorable information about the interaction and association in solution22,23

Figure 5. Excess refractive index, nED, as a function of DMC mole fraction, x1, for (a) DMC + 1-hexanol and (b) DMC + 1-octanol binary mixtures at different temperatures. The solid lines represent the corresponding correlations by the Redlich−Kister equation.

Δη = ηmix − x1η1 − x 2η2

The values of viscosity deviation, with the standard uncertainty of 0.04 mPa s, are reported in Tables S3 and S4. The graphical presentation of viscosity deviation is given in Figure S8 and the calculated values of Redlich−Kister coefficients along with their standard deviations are listed in Table 4. The values of Δη were negative over the whole composition and temperature range, showing a minimum at the DMC mole fraction equals to 0.3 for both studied mixtures.

A classical way to analyze viscosity−temperature dependence Ea RT

( ), where A

is to use Arrhenius approach, η = A 0exp

0

(19)

is a

system-dependent constant equals to viscosity at high temperature limit (T → ∞), Ea is the activation energy of flow, and R is the universal gas constant. The activation energy is calculated from the slope of the liner approximation of each set of data at each DMC mole fraction. For DMC + 1-hexanol/1-octanol I



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Figure 7. Viscosity, η, as a function of DMC mole fraction, x1, for (a) DMC + 1-hexanol and (b) DMC + 1-octanol binary mixtures at different temperatures. The solid lines are a guide to the eye.

Figure 8. Comparison of the experimental and theoretical viscosity values as a function of DMC mole fraction, x1, for (a) DMC + 1hexanol and (b) DMC + 1-octanol binary mixtures at 298.15 K.

Moreover, the viscosity deviations became less negative by increasing temperature. Generally, the positive values of the excess molar volume and negative values of the excess refractive index and viscosity deviation is quite usual for this kind of mixture, which has weak interaction between unlike molecules.

electronegative atoms than DMC. The activation energy of flow, determined from viscosity values, decreased with increasing DMC concentration in the binary mixtures. The experimental values of the refractive index and viscosity were well predicted with the Lorentz−Lorenz and Grunberg−Nissan models, respectively.

4. CONCLUSIONS The thermophysical properties were determined by measuring the experimental densities, viscosities and refractive indices of dimethyl carbonate (DMC) + 1-hexanol/1-octanol at temperature range of 293.15 to 323.15 K over the whole concentration range and atmospheric pressure. The excess molar volume, obtained from density, was positive for both the studied binaries and increased with temperature rising. The positive excess molar volume ascribed to the weak interactions between unlike molecules. It was found that by increasing the carbon chain length of alcohols the excess molar volume shifted to values that were more positive. Moreover, the obtained positive values of excess thermal expansion coefficient were in agreement with the variation of excess molar volume against temperature. The excess quantities of molar volume and refractive index were well correlated by the Redlich−Kister equation. The calculated negative values of excess refractive index and viscosity deviation represented no specific interaction between components. The electronic polarizability of the mixtures increased by increasing 1-hexanol or 1-octanol concentration because these alcohols are larger and have less

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ASSOCIATED CONTENT

S Supporting Information *

The Supporting Information is available free of charge on the ACS Publications website at DOI: 10.1021/acs.jced.5b00830. Comparison of the experimental properties of the pure liquids between this work and the available literature data. Thermal expansion coefficient, excess thermal expansion coefficient, excess molar volume, partial molar volume, excess refractive index, electronic polarizability, and viscosity deviation for the binary mixtures of DMC + 1-hexanol/1-octanol at different temperatures. Relative deviations against temperature between the experimental densities, viscosities, and refractive indices reported by different authors at atmospheric pressure for DMC, 1-hexanol, and 1-octanol. Dependence of density, pressure dependence of entropy, isothermal coefficient of pressure excess molar enthalpy, activation energy of flow, and viscosity deviation as a function of DMC mole J



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fraction for the binary mixtures of DMC + 1-hexanol/1octanol (PDF)

AUTHOR INFORMATION

Corresponding Author

*Tel.: +989171920300. E-mail: [email protected] or [email protected]. Notes

The authors declare no competing financial interest.

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ACKNOWLEDGMENTS The instrumental support from Iran’s Research Institute of Petroleum Industry is gratefully acknowledged. REFERENCES

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Densities, Viscosities, and Refractive Indices of Dimethyl Carbonate +

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