Influence of Temperature and Carbon Chain on Thermophysical

Jul 25, 2017 - Department of Chemistry, Ahvaz Branch, Islamic Azad University, Ahvaz, Iran. J. Chem. Eng. Data , 2017, 62 (8), pp 2406–2412...
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Influence of Temperature and Carbon Chain on Thermophysical Properties of Benzaldehyde/Alkan-2-ol Binary Mixtures Simin Shafaati and Mohammad Almasi* Department of Chemistry, Ahvaz Branch, Islamic Azad University, Ahvaz, Iran S Supporting Information *

ABSTRACT: In present paper, density, and viscosity values for binary systems of benzaldehyde + 2-propanol or 2-butanol or 2-pentanol have been measured over the entire range of composition and within the temperature range of 293.15−323.15 K. From these data, thermal expansion coefficient, excess thermal expansion coefficient, the pressure dependence of the excess molar enthalpy, partial molar volume, excess molar volume, and viscosity deviation were calculated. VEm is positive and decreases with rise of temperature and Δη is negative and increases with increasing temperature. Effect of temperature and carbon chain of alcohols on thermodynamic behavior of mixtures was discussed. The density values were used to test the applicability of the PC-SAFT model and the calculated density by this theory compared well with the corresponding experimental data.

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INTRODUCTION The thermophysical properties of mixtures such as density and viscosity would be of great importance in processing engineering designs and also helpful in getting information about molecular structure, understanding of the interactions between molecules and intermolecular forces in liquid mixture, which can be very helpful in making the choice of solvent in various applications.1 Benzaldehyde is an important compound in pharmaceuticals, fragrance, dye industries, and a precursor to certain acridine dyes. Short chain alcohols are polar organic molecules and have gained practical applications in broad areas and interest for investigating complicated molecular interactions because of their molecular structure, increasing hydrophobic character with increasing chain length, and high solubility in polar solvents.2 Hence, the thermodynamic and transport properties of benzaldehyde with alcohols are helpful for industrial applications as no density and viscosity data for these binary systems at different temperatures have been studied yet. In our earlier papers, thermodynamic and transport properties of binary mixtures containing alcohols were studied.3,4 In a continuation, we tend to report here thermal expansion coefficient, excess thermal expansion coefficient, the pressure dependence of the excess molar enthalpy, partial molar volume, excess molar volume, and viscosity deviation for binary liquid mixtures of benzaldehyde (1) + 2-propanol (2), benzaldehyde (1) + 2-butanol (2), and benzaldehyde (1) + 2-pentanol (2) at seven temperatures from T = 293.15 to 323.15 K and atmospheric pressure. These results are useful to interpretation of the nature of interactions occur among the components of mixtures. Also, this work provides a test of PC-SAFT model to correlate the density data of binary mixtures. © 2017 American Chemical Society

EXPRIMENTAL SECTION The chemicals used (benzaldehyde, 2-propanol, 2-butanol, and 2-pentanol) were of analytical grade obtained from Merck with stated label of purity grater than 99% of mass fraction. In Table 1, the purity of the components was supported by comparing their measured densities and viscosities with corresponding literature values.5−10 The agreement between the experimental and literature data is reasonable. The differences among the densities and viscosities of our pure chemicals and literature values are due to different sources of materials such as Fluka and Sigma (for our data and refs 7, 9, and 10), amount and sort of impurity (refs 6 and 7), and different techniques of measurements (refs 5 and 8). Density and viscosity were measured with a totally automated SVM 3000 Anton-Paar Stabinger viscometer that operates based on a modified Couette principle with a rapidly rotating outer tube and an inner measuring bob that rotates more slowly. Reproducibility of SVM 3000 for viscosity measurements is 0.35% and for density is 0.0005 g·cm−3. Repeatability of apparatus is 1% for viscosity and 0.0002 g·cm−3 for density measuring. Both density and viscosity are highly sensitive to temperature and therefore they were controlled by a built-in thermoelectric heating and cooling thermostat. Prior to each series of measurements, the apparatus was calibrated using doubly distilled degassed water and dry air at the atmospheric pressure. The SVM 3000 is an oscillating U-tube densimeter that measures highest accuracy in wide viscosity and temperature ranges and automatically corrects viscosity related Received: April 10, 2017 Accepted: July 12, 2017 Published: July 25, 2017 2406

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Table 1. Densities, ρ, and Viscosities, η, of Pure Components at Various Temperatures and P = 0.1 MPaa ρ(g·cm−3) chemical name

source

benzaldehyde

Merck

2-propanol

Merck

2-butanol

2-pentanol

Merck

Merck

mass fraction purity (as stated by the supplier) >0.99

T/K 293.15 298.15 303.15 308.15 313.15 318.15 323.15 293.15 298.15 303.15 308.15 313.15 318.15 323.15 293.15 298.15 303.15 308.15 313.15 318.15 323.15 293.15 298.15 303.15 308.15 313.15 318.15 323.15

0.997

0.995

>0.99

expt. 1.0463 1.0417 1.0371 1.0324 1.0279 1.0234 1.0191 0.7854 0.7811 0.7768 0.7724 0.7680 0.7634 0.7588 0.8067 0.8027 0.7984 0.7941 0.7898 0.7852 0.7806 0.8093 0.8053 0.8012 0.7970 0.7927 0.7884 0.7840

η (mPa·s) lit. b

1.04555 1.04104b 1.03653b 1.03201b 1.02749b 1.02297b 0.78496d 0.78075d 0.77654d 0.77232d 0.76811d 0.76390d

0.8023f 0.7939f 0.7851f

0.8047g 0.7966g 0.7881g

expt.

lit.

1.52 1.41 1.31 1.22 1.15 1.09 1.03 2.42 2.08 1.80 1.56 1.36 1.19 1.05 3.67 3.04 2.54 2.13 1.80 1.54 1.33 3.97 3.32 2.81 2.37 1.99 1.66 1.39

1.558c 1.427c 1.315c 1.222c 1.130c

2.386e 2.069e 1.763e 1.325e 1.002e 3.120f 2.171f 1.563f

3.38g 2.33g 1.674g

a Standard uncertainties are u(T) = 0.02 K, u(x) = 0.001, u(p) = 10 kPa, expanded uncertainty for density is U(ρ) = 0.001 g·cm−3 and relative expanded uncertainty for viscosity is Ur(η) = 0.04 (0.95 level of confidence). bReference 5. cReference 6. dReference 7. eReference 8. fReference 9. g Reference 10.

The variations in excess molar volume, VEm at T = 298.15 K for the binary mixtures of benzaldehyde (1) + 2-alkanol (2) are displayed in Figure 1. The excess molar volume results from molecular structure, specific forces, and physical intermolecular forces of liquids. VEm values are positive for all studied mixtures. The positive contribution arises from the breaking of intermolecular hydrogen bonding in self-associated pure components, physical dipole−dipole interactions between monomers and multimers, and also due to disruption in favorable orientation order of pure alcohols.1 This behavior suggests that the component molecules are closer together in the pure liquids than the mixture, indicating the weak attractive interactions between the mixture molecules. The alkyl chain of alcohols plays an important role on VEm. The rise of the excess molar volume with the molecular size of the alcohol molecule is closely associated with the spatial interference caused by a bulkier alkyl group. The results also can be viewed in terms of geometrical fit of the benzaldehyde molecules in an ordered structure of alcohol. It is difficult to accommodate benzaldehyde in an ordered solvent environment like alcohols. A similar trend12 was observed for binary mixtures benzaldehyde + 1butanol and benzaldehyde + 1-pentanol. Values of VEm for mentioned systems are positive and decrease with increasing temperature. VEm for benzaldehyde + 1-pentanol system are higher than those of benzaldehyde + 1-butanol. The main reason for positive VEm is reported due to the breaking up of Hbonding in alcohols by benzaldehyde and also the size of the

errors in the density by measuring the damping of the U-tubes oscillation caused by the viscosity of the filled-in sample. For measurement of densities and viscosities, the mixtures were prepared just prior to use and all properties were simultaneously and automatically measured. The liquid mixtures were prepared by mass on an analytical balance (Mettler AE 163, Switzerland) with the precision of ±0.01 mg. Cautions were taken to prevent evaporation of the samples after preparation. A set of 10 compositions were prepared for each mixture and their physical properties were measured at various compositions in the mole fraction range. The expanded uncertainty is 1 × 10−2 g·cm−3 for density measurements and relative expanded uncertainty for viscosity measurements is 0.04. The estimated uncertainty in the mole fraction was ±1 × 10−3. The effects of impurities were included in the uncertainties.11

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RESULTS AND DISCUSSION Densities and viscosities for pure compounds and binary mixtures at various temperatures are reported in Table 2. The excess molar volume, VEm was calculated using N

VmE =

∑ xiMi(ρ−1 − ρi−1) i=1

(1)

where xi is the mole fraction, Mi is the molar mass, ρ is the density of the mixture, ρi is the density of pure component i, and N stands for the number of components in the mixture. 2407

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Table 2. Densities ρ and Viscosities η for the Binary Mixtures as a Function of the Mole Fraction x1 of Benzaldehyde at Pressure P = 0.1 MPaa x1

T/K = 293.15

T/K = 298.15

T/K = 303.15

T/K = 308.15

T/K = 313.15

T/K = 318.15

T/K = 323.15

0.768 0.7910 0.813 0.8348 0.8644 0.8883 0.9226 0.944 0.967 0.9941 1.0146 1.0279

0.7634 0.7867 0.8086 0.8303 0.8598 0.8837 0.9180 0.9394 0.9632 0.9897 1.0108 1.0234

0.7588 0.7820 0.8037 0.8256 0.8551 0.8791 0.9134 0.9349 0.9589 0.9850 1.0060 1.0191

1.36 1.23 1.14 1.08 1.03 1.011 1.018 1.032 1.051 1.093 1.124 1.15

1.19 1.08 1.00 0.95 0.918 0.909 0.916 0.933 0.967 1.015 1.058 1.09

1.05 0.97 0.913 0.873 0.848 0.84 0.844 0.863 0.892 0.943 0.991 1.03

Benzaldehyde (1) + 2-Propanol (2) 0 0.0809 0.1596 0.2400 0.3492 0.4399 0.5693 0.6495 0.7399 0.8498 0.9399 1

0.7854 0.8096 0.8307 0.8525 0.8823 0.9064 0.9408 0.9622 0.9862 1.0128 1.0333 1.0463

0.7811 0.8043 0.8264 0.8482 0.8779 0.9019 0.9362 0.9576 0.9817 1.0080 1.0290 1.0417

0 0.0809 0.1596 0.2400 0.3492 0.4399 0.5693 0.6495 0.7399 0.8498 0.9399 1

2.42 2.11 1.86 1.675 1.499 1.42 1.402 1.414 1.434 1.47 1.502 1.52

2.08 1.82 1.63 1.47 1.342 1.296 1.284 1.298 1.318 1.354 1.385 1.41

ρ/(g·cm−3) 0.7724 0.7956 0.8176 0.8392 0.8688 0.8929 0.9272 0.9486 0.9726 0.9993 1.0197 1.0324 η/(mPa·s) 1.80 1.56 1.59 1.41 1.43 1.29 1.33 1.20 1.233 1.126 1.197 1.10 1.187 1.098 1.196 1.109 1.216 1.131 1.252 1.163 1.286 1.197 1.31 1.22 Benzaldehyde (1) + 2-Butanol (2) 0.7768 0.7999 0.8218 0.8437 0.8734 0.8974 0.9317 0.9531 0.9767 1.0041 1.0241 1.0371

ρ/(g·cm−3) 0 0.0813 0.1623 0.2401 0.3517 0.4404 0.5612 0.6519 0.7423 0.8511 0.9400 1

0.8067 0.8247 0.8428 0.8609 0.8869 0.9084 0.9381 0.9610 0.9844 1.0121 1.0325 1.0463

0.8027 0.8212 0.8395 0.8573 0.8832 0.9053 0.9346 0.9576 0.9802 1.0073 1.0286 1.0417

0 0.0813 0.1623 0.2401 0.3517 0.4404 0.5612 0.6519 0.7423 0.8511 0.9400 1

3.67 3.08 2.62 2.30 1.97 1.791 1.648 1.576 1.528 1.506 1.511 1.52

3.04 2.65 2.31 2.027 1.75 1.61 1.487 1.426 1.39 1.38 1.39 1.41

0.7984 0.8163 0.8341 0.8524 0.8781 0.8997 0.9292 0.9521 0.9757 1.0021 1.0232 1.0371

0.7941 0.8123 0.8299 0.8481 0.8739 0.8953 0.9247 0.9476 0.9711 0.997 1.019 1.0324

η/(mPa·s) 2.54 2.13 2.23 1.897 1.984 1.70 1.78 1.55 1.561 1.383 1.438 1.284 1.322 1.194 1.279 1.156 1.255 1.139 1.255 1.149 1.277 1.182 1.31 1.22 Benzaldehyde (1) + 2-Pentanol (2)

0.7898 0.8078 0.8255 0.8437 0.8693 0.8908 0.9203 0.9444 0.9667 0.9934 1.0141 1.0279

0.7852 0.8030 0.8208 0.8390 0.8646 0.8861 0.9157 0.9400 0.9621 0.9877 1.0093 1.0234

0.7806 0.7989 0.8164 0.8346 0.8600 0.8815 0.9110 0.9339 0.956 0.9821 1.0039 1.0191

1.80 1.636 1.49 1.366 1.23 1.146 1.079 1.05 1.038 1.057 1.10 1.15

1.54 1.388 1.265 1.172 1.068 1.01 0.966 0.95 0.948 0.979 1.026 1.09

1.33 1.215 1.128 1.056 0.977 0.932 0.895 0.882 0.887 0.913 0.962 1.03

0.7927 0.8086 0.8244

0.7884 0.8042 0.8200

0.7840 0.7997 0.8156

ρ/(g·cm−3) 0 0.0809 0.1662

0.8093 0.8252 0.8414

0.8053 0.8211 0.8372

0.8012 0.8170 0.8330

0.7970 0.8129 0.8288 2408

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Table 2. continued Benzaldehyde (1) + 2-Pentanol (2) 0.2441 0.3552 0.4418 0.5664 0.6565 0.7447 0.8528 0.9419 1

0.8583 0.8825 0.9030 0.9332 0.9564 0.9800 1.0085 1.0318 1.0463

0.8540 0.8782 0.8980 0.9282 0.9512 0.9754 1.0041 1.0274 1.0417

0.8497 0.8739 0.8944 0.9238 0.9469 0.9710 1.0000 1.0231 1.0371

0 0.0809 0.1662 0.2441 0.3552 0.4418 0.5664 0.6565 0.7447 0.8528 0.9419 1

3.97 3.30 2.75 2.36 1.95 1.757 1.62 1.568 1.537 1.516 1.51 1.52

3.32 2.775 2.35 2.05 1.731 1.584 1.458 1.416 1.395 1.39 1.395 1.41

2.81 2.40 2.06 1.809 1.55 1.411 1.301 1.259 1.25 1.259 1.28 1.31

0.8455 0.8696 0.8903 0.9193 0.9423 0.9665 0.9955 1.0180 1.0324

0.8411 0.8652 0.8852 0.9148 0.9378 0.9620 0.9911 1.0139 1.0279

0.8367 0.8608 0.8814 0.9104 0.9334 0.9574 0.9866 1.0091 1.0234

0.8322 0.8563 0.8769 0.9067 0.9289 0.9529 0.9816 1.0045 1.0191

2.37 2.035 1.78 1.584 1.369 1.25 1.159 1.128 1.117 1.138 1.175 1.22

1.99 1.746 1.537 1.37 1.185 1.088 1.021 0.999 0.999 1.035 1.088 1.15

1.66 1.46 1.291 1.167 1.032 0.963 0.90 0.881 0.884 0.932 1.011 1.09

1.39 1.206 1.068 0.984 0.887 0.831 0.789 0.782 0.799 0.85 0.941 1.03

η/(mPa·s)

a

x1 is the mole fraction of benzaldehyde in the (benzaldehyde + 2-alkanol) solutions. Standard uncertainties are u(T) = 0.02 K, u(x) = 0.001, u(p) = 10 kPa, expanded uncertainty for density is U(ρ) = 0.001 g·cm−3 and relative expanded uncertainty for viscosity is Ur(η) = 0.04 (0.95 level of confidence).

intermolecular bonds and molecular size and indicating the interaction of different molecules is reduced when the number of carbon atom increased. The Δη values for all studied systems at T = 298.15 K are presented as a function of mole fraction in Figure 2.

Figure 1. Excess molar volume VmE versus mole fraction of benzaldehyde with (▲) 2-propanol, (●) 2-butanol, (■) 2-pentanol at T = 298.15 K. () Redlich−Kister equation.

alkanol affects the excess molar volume. By contrast, VEm for benzaldehyde + 2-alkanol (our data) is greater than those of benzaldehyde + 1-alkanol which may be because branching alkanols (from 1-alkanol to 2-alkanol) creates steric hindrance which inhibit benzaldehyde molecules to suitable interactions with alcohols, so the weaker bonds are formed (comparing by 1-alkanol) and excess molar volume increases. Comparisons are reported in SI, Figures S1−S4. Deviation in the viscosity, Δη can be calculated by

Δη = η − x1η1 − x 2η2

Figure 2. Viscosity deviation Δη versus mole fraction of benzaldehyde with (▲) 2-propanol, (●) 2-butanol, (■) 2-pentanol at T = 298.15 K. () Redlich−Kister equation.

Excess molar volume and deviation in the viscosity have been fitted to the Redlich−Kister13 equation to derive the binary interaction parameter, Ak

(2)

η is the mixture viscosity and η1 and η2 are viscosity of the pure state. Δη for binary system benzaldehyde (1) + 2-alkanol (2) is negative over the whole range of composition and at all temperatures. The absolute values of Δη follow the order: 2pentanol > 2-butanol > 2-propanol. The negative value of Δη can be interpreted qualitatively by considering the strength of

N

YmE = x1(1 − x1) ∑ Ak (1 − 2x1)k k=0

(3)

where x1 is the mole fraction of benzaldehyde. Standard deviation was calculated using 2409

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E E 2 ⎤1/2 ⎡ − Ycal (Yexp ) ⎢ ⎥ σ= ∑ ⎢⎣ (n − p) ⎥⎦

YEexp

(4)

YEcal

where and are the experimental and calculated data, respectively. Values of VEm and Δη are reported in SI, Table S1. Adjustable parameters, Ak, and standard deviation are presented in SI, Table S2. Because the changes in the solution structure are very sensitive to temperature changes, the thermal expansion coefficient αp defined as below is a sensitive criterion for the detection of solute−solvent interactions14 ⎛ ∂ρ ⎞ ⎛ ∂V ⎞ αp = V −1⎜ ⎟ = −ρ⎜ ⎟ ⎝ ∂T ⎠ p ⎝ ∂T ⎠ p

Figure 4. Excess thermal expansion coefficient αEp versus mole fraction of benzaldehyde for benzaldehyde (1) + 2-propanol (2) at (○) 293.15 K, (Δ) 303.15 K, (▲) 313.15 K, (●) 323.15 K.

(5)

Excess thermal expansion coefficient αEp was obtained from the following equation: 2

αpE = αp,mix −

∑ φα i p, i

(6)

i=1

where αp,mix and φi are the mixture thermal expansion coefficient and volume fraction, respectively. The pressure dependence of the excess molar enthalpy at fixed composition and temperature was obtained by application of the expression ⎛ ∂H E ⎞ ⎛ ∂V E ⎞ ⎜ m ⎟ = VmE − T ⎜ m ⎟ ⎝ ∂P ⎠T,X ⎝ ∂T ⎠P,X

The calculated values αp, αpE, and

(7) ∂HmE ∂P

( )

at various

T,X

temperatures for binary mixture benzaldehyde (1) + 2-propanol (2) are graphically represented in Figures 3−5. αp values are

Figure 5. Pressure dependence of the excess molar enthalpy,

estimated errors on the thermal expansion coefficient, excess thermal expansion coefficient and pressure dependence of excess molar enthalpy are 5 × 10−6 K−1, 1 × 10−5 K−1, and 0.5 × 10−6 J·Pa−1·mol−1 respectively. Also the partial molar volume V̅ m,i was calculated15 over the whole range of composition for studied mixtures. Increasing temperature contributes to weakening of benzaldehyde-alcohol binding, so the partial molar volume of the benzaldehyde increases significantly. Values of V̅ m,1 for binary mixtures of benzaldehyde (1) + 2-alkanol (2) at T = 298.15 K are presented graphically in Figure 6. The errors in the partial molar volume is estimated to be 2 × 10−2 cm3·mol−1.The objective of this work in the next step is to model the density of binary mixtures. The density calculation has been carried out by applying the PC-SAFT model.16,17 The general expression for the Helmholtz energy in this model is explained by

increased with increasing temperature. Hydrogen bond rupture is the main microscopic reason for this phenomenon. The positive αEp values suggest that the expansivity of the solution is greater than that of pure liquid. This means a larger expansion of the solutions with increasing temperature and increase in the average intermolecular distance compared to the pure liquid. Therefore, the solution structure breaks easier than the pure state. As the temperature of the mixture increased, cavities are produced in the ordered solvent environment, resulting in the better fit of the benzaldehyde in the alcohols structure, so VEm, αEp , and

( ) ∂P

T,X

versys mole fraction of benzaldehyde for benzaldehyde (1) + 2propanol (2) at (□) 293.15 K, (●) 298 K, (■) 303.15 K, (▲) 308 K, (Δ) 313.15 K, (◆) 318, (○) 323.15 K.

Figure 3. Thermal expansion coefficient αp versus mole fraction of benzaldehyde for benzaldehyde (1) + 2-propanol (2) at (●) 293.15 K, (▲) 303.15 K, (Δ) 313.15 K, (○) 323.15 K.

∂HmE

∂HmE ∂P

( )

a res = achain + adisp + aassoc

Chain formation contribution a a

chain

= −∑ xi(mi − 1)ln

(8) chain

is calculated by

giihs

(9)

i

ghs ii

where m is the number of segment and is the hard sphere radial distribution function. The dispersion contribution to the Helmholtz energy, adis is

decrease with increasing temperature. The

T,x

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experimental data matches with this model with a high degree of precision.

■

ASSOCIATED CONTENT

S Supporting Information *

The Supporting Information is available free of charge on the ACS Publications website at DOI: 10.1021/acs.jced.7b00335. Excess molar volumes, viscosity deviations, coefficients of Redlich−Kister equation, parameters of pure materials for PC-SAFT, and binary interaction parameter kij for PC-SAFT model (PDF)

■

Figure 6. Partial molar volume V̅ m,1 versus mole fraction of benzaldehyde with (◆) 2-propanol, (Δ) 2-butanol, (●) 2-pentanol at T = 298.15 K.

adis

Corresponding Author

*E-mail: [email protected]. Tel.: + 98-611- 4431018. ORCID

Mohammad Almasi: 0000-0001-9771-8702

⎛ ∂ρ ⎞ ⎛ ε ⎞ ⎛ ε ⎞2 = −2I1πmρ2 ⎜ ⎟σ 3 − πmI2kT ⎜ ⎟ m2⎜ ⎟ σ 3 ⎝ kT ⎠ ⎝ ∂P ⎠hc ⎝ kT ⎠

Notes

The authors declare no competing financial interest.

■ ■

(10)

where ρ is the number density of fluids. Coefficients I1 and I2 are perturbation integral and can be solved for any intermolecular potential. The association term can be calculated as a

assoc

⎡ XA ⎤ = ∑ ⎢ln X A − ⎥ + 0.5S 2 ⎦ ⎣ A

ACKNOWLEDGMENTS The authors thank Islamic Azad University (Ahvaz Branch, Ahvaz) for providing the necessary facilities of this work.

100 n

∑

(11)

Xexp − Xcal Xcal

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where S is the number of association sites and the fraction XA is unbounded monomers of single site A.18 For correlation of mixtures density by PC-SAFT, van der Waals one fluid model was applied. Determined parameters for pure materials are reported in SI, Table S3. This model contains one adjustable interaction parameter kij, which is used to correct the dispersion energy in the mixtures and usually is independent of temperature. Values of this parameter are reported in SI, Table S4. Results of density calculations for binary systems show that the modeling of density has been accomplished with a very good accuracy. Average absolute deviation (AAD) was calculated by AAD% =

AUTHOR INFORMATION

(12)

where n is the number of data points, Xexp and Xcal are the experimental data and calculated values, respectively. ADD for benzaldehyde (1) + 2-propanol (2) was 1.1%, for benzaldehyde + 2-butanol was 1.2%, and for benzaldehyde + 2-pentanol was 1.4%.

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CONCLUSIONS New experimental values of density and viscosity for the binary liquid mixtures of benzaldehyde + 2-alkanol from 293.15 to 313.15 K were measured. Thermal behavior solutions were investigated by calculating thermodynamic parameters such as thermal expansion coefficient, excess thermal expansion coefficient and partial molar volumes and used to predict the intermolecular interactions in the mixtures. The excess molar volume and excess thermal expansion for all mixtures are positive and viscosity deviation is negative. PC-SAFT was used to correlate the density of the systems and in all cases the 2411

DOI: 10.1021/acs.jced.7b00335 J. Chem. Eng. Data 2017, 62, 2406−2412

Journal of Chemical & Engineering Data

Article

implementation, and online support. J. Chem. Eng. Data 2013, 58, 2699−2716. (12) Indraswati, N.; Mudjijati; Wicaksana, F.; Hindarso, H.; Ismadji, S. Measurements of Density and Viscosity of Binary Mixtures of Several Flavor Compounds with 1-Butanol and 1-Pentanol at 293.15 K, 303.15 K, 313.15 K, and 323.15 K. J. Chem. Eng. Data 2001, 46, 696−702. (13) Redlich, O. J.; Kister, A. T. Thermodynamic of nonelectrolyte solutions: algebraic representation of thermodynamic properties and the classification of solutions. Ind. Eng. Chem. 1948, 40, 345−348. (14) Lide, R. D. Handbook of chemistry and physics; CRC Press: Boca Raton, FL; 2000; p8 180−184, Section 6. (15) Davis, I. M. An analytic model for the excess properties of binary liquid mixtures. Thermochim. Acta 1983, 63, 67−82. (16) Gross, J.; Sadowski, G. Perturbed-Chain SAFT. An equation of state based on a perturbation theory for chain molecules. Ind. Eng. Chem. Res. 2001, 40, 1244−1260. (17) Gross, J.; Sadowski, G. Application of the perturbed-chain SAFT equation of state to associating systems. Ind. Eng. Chem. Res. 2002, 41, 5510−5515. (18) Chen, Y.; Mutelet, F.; Jaubert, J. N. Modeling the Solubility of Carbon Dioxide in Imidazolium-Based Ionic Liquids with the PCSAFT Equation of State. J. Phys. Chem. B 2012, 116, 14375−14388.

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DOI: 10.1021/acs.jced.7b00335 J. Chem. Eng. Data 2017, 62, 2406−2412