Article pubs.acs.org/jced
Solubility of N2O in and Density and Viscosity of Aqueous Solutions of 1,4-Butanediamine, 2‑(Diethylamino)-ethanol, and Their Mixtures from (298.15 to 333.15) K Zhicheng Xu, Shujuan Wang,* and Changhe Chen Key Laboratory for Thermal Science and Power Engineering of Ministry of Education, Beijing Key Laboratory for CO2 Utilization and Reduction Technology, Department of Thermal Engineering, Tsinghua University, Beijing 100084, China ABSTRACT: Densities of and N2O solubilities in aqueous solutions of 1,4-butanediamine (BDA), 2-(diethylamino)ethanol (DEEA), and their aqueous mixtures were measured at (298.15, 313.15, and 333.15) K, and viscosities were measured at (298.15, 303.15, 313.15, 323.15, and 333.15) K. The experiments cover the mole fraction ranges (1.95−14.3 mol %) BDA, (2.01−19.3 mol %) DEEA, and (3.63−16.7 mol %) BDA + (2.62−22.2 mol %) DEEA in the blended solutions. The results were compared with available data in the literature. The experimental density and viscosity data were correlated using two semi empirical correlations in the literature as functions of temperature and concentration of BDA and DEEA.
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INTRODUCTION Absorption of CO2 with amine-based absorbents is an established and proven technology.1 Many solvents, such as monoethanolamine (MEA), methyldiethanolamine (MDEA), diethanolamine (DEA), and piperazine (PZ), have been applied to capture CO2.2−4 However, this process always requires lots of energy during solvent regeneration. Recent years, the novel process of biphasic system DMX and lipophilic solvents were proposed with the energy consumption of DMX system being estimated to be 2.3 GJ/t CO2.5,6 Dimethylcyclohexylamine (DMCA), dipropylamine (DPA), and DPA and DMCA blend, 3(methylamino)propylamine (MAPA) and DEEA blend and some other unspecified amines in the literatures were studied for the biphasic system.7−11 The previous researches have investigated CO2 absorption by some potential biphasic solvents. The mixture of 8.75 mol % BDA and 17.5 mol % DEEA (2 M BDA+4 M DEEA) was found to be a potential biphasic solvent and has 46 % higher cyclic loading, 48 % higher cyclic capacity, and 11 % higher cyclic efficiency than 30 mass % MEA. The phase separation of the solution after CO2 absorption was due to the fast reaction rate of CO2 with BDA and the limited solubility of DEEA in the reaction products of BDA and CO2.12−14 As one of the most important issues in evaluating a solvent, kinetics parameters are typically derived from the experiments based on mass transfer process, and the data of physical diffusivity and solubility of CO2 in aqueous solvents solutions are required. However, due to the chemical reactions between CO2 and amine, these properties are not possible to be measured directly.15 It is suggested that using “N2O analogy” to estimate the aforementioned physicochemical properties, since N2O resembles CO2 in molecular volume, configuration and electronic structure, and it is a nonreactive gas in amine conditions,16−18 as © 2013 American Chemical Society
shown in eq 1. Moreover, density and viscosity of aqueous solvents are also essential for the calculation of other physicochemical properties such as diffusivity, gas solubility, and reaction rate constants. ⎛ HCO ‐ H O ⎞ 2 2 ⎟⎟HN O ‐ Am HCO2 ‐ Am = ⎜⎜ 2 ⎝ HN2O ‐ H2O ⎠
(1)
BDA has been widely investigated by evaluating the effect of chain length on the absorption and desorption capacity of biamine and by measuring the vapor liquid equilibrium of pure BDA.19−22 However, so far as we know, there is still no literature reporting the solubility of N2O in and density and viscosity of BDA aqueous solution. DEEA is usually blended with other activators (for example, piperazine) to absorb CO2 because of its low reaction rate. The densities of aqueous DEEA solutions were presented by Barbas et al. and Lebrette et al.,23,24 which did not include the concentrations needed in our kinetics study. The viscosities of aqueous DEEA solutions were measured by Maham et al. and Littel et al.25,26 The N2O or CO2 physical solubility in aqueous DEEA solution was obtained by Littel et al., Vaidya, and Li et al.,26−29 which just covered limited concentrations around 4.54 mol %. The solubility of N2O in and density and viscosity of BDA/DEEA mixtures have not been presented until now. In the present work, N2O solubilities in and densities of aqueous solutions of (1.95−14.3 mol %) BDA, (2.01−19.3 mol %) DEEA, and their aqueous mixtures were measured at (298.15, 313.15, and 333.15) K, with viscosities measured at (298.15, 303.15, 313.15, Received: December 27, 2012 Accepted: May 15, 2013 Published: May 24, 2013 1633
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323.15, and 333.15) K. The results were compared with available data in the literatures. The experimental data on density and viscosity were correlated using two semi empirical correlations in the literature as functions of temperature and concentrations of BDA and DEEA.
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EXPERIMENTAL SECTION BDA (≥ 98 wt % pure) and DEEA (≥ 99 wt % pure) were from Aladdin Reagent Company. The BDA and DEEA structures are shown below.
Distilled water was used for preparing experimental solutions. The BDA and DEEA concentrations were determined by titration against 2 N H2SO4 using a Metrohm 809 Titrando auto titrator. The N2O gas (99 vol % pure) was supplied by Beijing Huayuan Gas Company. Density and Viscosity. In this work, the densities of aqueous solutions were measured by National Institute of Metrology (NIM) of China, strictly following the JJG 1058-2010 verification regulation of laboratory oscillation-type liquid density meters issued by General Administration of Quality Supervision, Inspection and Quarantine of China (AQSIQ), using a DMA5000 density meter. NIM is China’s highest research center of metrology and the national technical center of legal metrology. The result of every point was the average value of six repeated trials. The viscosities of aqueous solutions were measured by a A&D SV-10 viscometer, with a measurement range of 0.3−1000 mPa·s. The total accuracy of viscosity given by the manufacturer is ± 1 %. Calibration of viscometer was done by measuring the viscosity of Standard Liquid GBW13601 (1203) and GBW13603 (1203) produced by NIM and approved by AQSIQ. The data for the calibration are given in Table 1.
Figure 1. Experimental setup of N2O solubility.
The amount of solvent added (around half of reactor) into the reactor was calculated by measuring the weight of solvent before and after the transference. After the solution reached vapor liquid equilibrium at set temperature, the pressure inside of the reactor, P1,N2O, was recorded. The temperature of the reactor was controlled by the circulating oil bath with an uncertainty of ± 0.1 K. Then N2O gas was added to the reactor by shortly opening valve No. 5 linking the reactor and the vessel. Considering that the open period for the reactor after the solution added was very short and the good airtightness of the reactor, the vapored amount of the solvent should be very small and can be neglected. Equilibrium was then established after 6−15 h (depending on temperature) with an agitation speed of 450 r/min. The reactor and vessel pressure were recorded by two pressure transducers (Druck PTX 7515 with uncertainty 0.2 % of full scale (200 kPa)). Two K-type thermocouples recorded temperatures in the reactor and in the vessel, respectively, with an uncertainty of ± 0.1 K. The amount added of N2O, nNadded , mol, was calculated from the 2O pressure difference of the gas supply vessel before and after feeding N2O as
Table 1. Viscosities of Standard Solutions for Calibration, 293.15 K, 1 atm (1.01325·105 Pa)
n Nadded = 2O
viscosity μ (mPa·s) standard
measurement
ref
deviation
GBW13601(1203) GBW13603(1203)
1.84 8.80
1.8388 8.793
−0.07 % 0.03 %
VV ⎛ PV1 PV2 ⎞ ⎟ ⎜ ‐ R ⎜⎝ TV1z1 TV2z 2 ⎟⎠
(2)
where PV1 and PV2 are the pressure of the vessel before and after feeding, Pa; TV1 and TV2 are the temperature of the vessel before and after feeding, K; z1, z2 represent the compressibility factor of gas before and after the feeding; R is universal gas constant, 8.3145 J·(mol·K)−1. The compressibility factor was calculated using the Peng−Robinson equation of state. The amount of N2O in the gas phase of the reactor ngN2O can be calculated by
It can be seen that viscosities from the measurements agree very well with the reference values for the standard liquid. Solubility of N2O. The N2O solubility apparatus consists of a jacketed stirred glass reactor and a stainless steel gas holding vessel, as shown in Figure 1. Before experiment, the volume of the gas holding vessel was measured by filling it up with water and calculating the water volume. Then the total volume of the reactor and the auxiliary pipe linking the reactor and valves no. 3−6 were measured by adding into it a known amount of N2O from the holding vessel. The added N2O amount was calculated by the amount difference in the gas holding vessel before and after adding N2O into reactor. The results show that the volume of vessel, VV, was 2.186·10−3 m3, while that of the reactor and the auxiliary, VR, was 5.628·10−4 m3. The reactor was first vacuumed until the pressure was less than 1 kPa, and then the solution was sucked into it through valve no. 3.
n Ng 2O =
PN2O(VR − VS) z N2ORTR
(3)
where TR is the reactor temperature after reaching equilibrium, K, and z is the compressibility factor of N2O after reaching equilibrium. VS is the volume of added solvent, which is the quotient of added solution amount and density, m3. PN2O is the N2O partial pressure and calculated by eq 4, Pa. PN2O = P1,N2O − P2,N2O (4) 1634
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Table 2. Measured N2O Solubilities (Mass Fraction w, kg/kg) in Water and 30 Mass % MEA, 293.15 to 333.15 K in This Work T (K)
293.15
water
PN2O (kPa)
MEA
w (%) PN2O (kPa)
111.0 0.1338
w (%) a
298.15
303.15
150.9
123.6
0.1677 141.7
0.1219
0.1402
313.15 150.3 0.1180 155.5 0.1195
323.15 142.7 0.0952
333.15 181.7 0.0829 142.0 0.0736
The standard uncertainty of w measurement is ± 2 %.
where P2,N2O is the total pressure of reactor after reaching equilibrium, Pa. The N2O amount in the liquid phase, nNlN2O, can then be expressed as the amount difference between added N2O and N2O in the gas phase by n Nl 2O = n Nadded − n Ng 2O 2O
(5)
The N2O concentration in the liquid phase, CN2O, can be calculated by C N2O =
n Nl 2O VS
(6)
The solubility of N2O at different pressures and temperatures have been expressed as mass fraction w (kg/kg) in this paper. Then the N2O solubility was expressed by a Henry’s law constant HN2O according to eq 7 in this paper. PN2O = HN2OC Nl 2O
Figure 3. N2O solubility HN2O in 30 mass % MEA: this work comparing with literature data.35−37
(7)
The units of CN2O and HN2O are mol·m−3 and kPa·m3·kmol−1. All operating conditions, including temperature and pressure, were recorded using Kingview (6.5.2 version) software. Calibrations were done by measuring the solubility of N2O in water and in 30 mass % MEA at different temperatures from (293.15 to 333.15) K and comparing the data with the literature. The data of N2O pressure in gas phase and concentration in liquid phase are shown in Table 2, whereas the comparisons of Henry’s law constant HN2O with several literature references are shown in Figures 2 and 3.15,30,33−37
It can be seen that the solubility of N2O in water and in 30 mass % MEA measured by this work agree very well with the literature data. The uncertainty is within 3 % when less than 313.15 K, whereas the differences were about 7 % at (323.15 and 333.15) K when compared with the data of Versteeg and van Swaaij.30
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RESULTS AND DISCUSSION Density. The measured densities for the aqueous solutions of BDA, DEEA, and BDA/DEEA blends are presented in Table 3 and Figures 4 and 5.
Figure 2. N2O solubility HN2O in water: this work comparing with literature data.15,30,33,34
Figure 4. Densities of aqueous BDA solutions measured and calculated by this work. 1635
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Table 3. Densities of Aqueous BDA (x1), DEEA (x2), and BDA/DEEA Blended Solutions at (298.15, 313.15, and 333.15) K and 1 atm (1.01325·105 Pa) density, ρa·10−3 (kg/m3) 10x1 (mol/mol)
a
T/K
032
0.1952
0.4244
298.15 313.15 333.15
0.99704 0.99222 0.98320
0.992346 0.986497 0.976433
0.988532 0.981237 0.969713
T/K
032
0.2012
0.4547
298.15 313.15 333.15
0.99704 0.99222 0.98320
0.993744 0.987552 0.976860
0.6965 0.985772 0.976817 0.963518 10x2 (mol/mol) 0.7875
0.990151 0.983322 0.981577 0.972648 0.968366 0.957191 10x1/10x2(mol/mol)
1.0253
1.4336
0.982813 0.972197 0.957323
0.978544 0.966791 0.950667
1.2520
1.9329
0.971858 0.959656 0.942334
0.961569 0.948632 0.930379
T/K
0.3629/1.4516
0.8749/1.7499
1.6703/2.2270
0.6799/1.0198
0.5618/0.5618
0.8712/0.9376
298.15 313.15 333.15
0.962903 0.950135 0.932259
0.948513 0.935423 0.917224
0.930513 0.917399 0.899304
0.967362 0.954889 0.937515
0.979531 0.968135 0.952165
0.973321 0.961226 0.944402
The standard uncertainty of ρ measurement is ± 0.01 %.
Figure 5. Densities of aqueous DEEA solutions measured and calculated by this work and compared with literature data.23,24
Table 4. Correlation Parameters, AADs, SSE, and R2 for Densities of BDA, DEEA, and BDA/DEEA Blended Solutions k1 BDA DEEA BDA+DEEA a
0.5635 0.5260 0.9686
k2 64.004 −2920.0 −142.11
k3
k4
k5
0.8865 −0.01838 4.9035
−1.4958·10 −1.5151·104 1.9634·105 4
273.87 307.54 −346.75
AADa
k6 −0.65421 37.2233 0.11514
−3
1.46·10 1.56·10−3 1.77·10−3
SSEb
R2c −5
4.59·10 6.76·10−5 6.58·10−5
0.9829 0.9889 0.9917
AAD = (1/N)Σi N= 1((|ρcal,i − ρexp,i|)/ρexp,i). bSSE = Σi N= 1(ρcal,i − ρexp,i)2. cThe squared correlation coefficients.
Optimization method in the 1STOPT software produced by 7D-Soft High Technology Inc.
For DEEA solutions, the deviations are less than 0.3 % when compared with Barbas et al. and Lebrette et al. under the same conditions,23,24 as shown in Figure 5. The densities of the binary and ternary mixtures decrease with increasing mole fractions of BDA and DEEA and temperature in the mixture. The experimental density data for the binary and ternary mixtures were fitted as a function of temperature and concentration of amine using the equation proposed by Liu et al.,31 as shown in eq 8. The correlation parameters were fitted for lowest average absolute deviation (AAD) using Levenberg−Marquardt and Universal Global
ρBDA + DEEA ( ·10−3(kg·m−3) ⎛ k ⎞ k = ⎜k1 + 2 (x BDA + k 3x DEEA ) + 42 ⎟ ⎝ T T ⎠ ⎛ k5 ⎞ × exp⎜ + k6(x BDA + k 3x DEEA )⎟ ⎝T ⎠
(8)
where ρ is the density of the mixture, T is the temperature, and x is the mole fraction of BDA or DEEA. k1 to k6 are the correlation 1636
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Table 5. Viscosities of Aqueous BDA (x1), DEEA (x2), and BDA/DEEA Blended Solutions from (298.15 to 333.15) K and 1 atm (1.01325·105 Pa) viscosity μa (mPa·s) 10x1 (mol/mol) T/K
032
0.1952
0.4244
0.6965
1.0253
1.4336
298.15 303.15 313.15 323.15 333.15
0.89 0.80 0.65 0.55 0.48
1.86 1.23 0.98 0.80 0.63
2.64 1.83 1.39 1.10 0.90
3.50 2.51 1.85 1.40 1.06
5.53 3.65 2.57 1.86 1.37
7.92 4.87 3.29 2.29 1.62
T/K
32
0.7875
1.2520
1.9329
5.57 3.61 2.42 1.72 1.24
8.00 5.75 3.76 2.60 1.87
11.61 8.05 5.27 3.69 2.53
10x2 (mol/mol) 0
298.15 303.15 313.15 323.15 333.15
a
0.2012
0.4547
0.89 0.80 0.65 0.55 0.48
2.16 1.40 1.12 0.94 0.75
3.62 2.34 1.66 1.32 1.03 10x1/10x2(mol/mol)
T/K
0.3629/1.4516
0.8749/1.7499
1.6703/2.2270
0.6799/1.0198
0.5618/0.5618
0.8712/0.9376
298.15 303.15 313.15 323.15 333.15
13.50 8.42 5.42 3.67 2.47
16.48 9.86 6.13 3.99 2.61
15.28 9.10 6.00 3.93 2.54
11.97 7.97 5.18 3.53 2.43
9.12 5.26 3.70 2.64 1.89
10.05 6.76 4.54 3.21 2.30
The standard uncertainty of μ measurement is ±6 %
Figure 6. Viscosities of aqueous DEEA solutions measured and calculated by this work and compared with literature data.25
Table 6. Correlation Parameters, AADs, SSE, and R2 for Viscosities of BDA, DEEA, and BDA/DEEA Blended Solutions BDA DEEA BDA+DEEA a
k1
k2
k3
k4
k5
k6
AADa
SSEb
R2c
1290 4486 −975.1
0.7115 2.4061 −0.9854
2.0806·107 1.6338·106 3.3713·107
−4011.71 −4324.48 −4032.22
1.238·106 1.31·106 1.40·106
−17.178 −1.1926 −119.26
0.1091 0.08617 0.09759
1.8350 1.4616 13.424
0.9748 0.9919 0.9726
AAD = (1/N)Σi N= 1((|μcal,i − μexp,i|)/μexp,i). bSSE = Σi N= 1(μcal,i − μexp,i)2. cThe squared correlation coefficients.
parameters. k3 is especially used to describe the interaction between the BDA and DEEA in the mixed solution. The calculated parameters k, the average absolute deviations (AADs), the residual sum of squares (SSEs) and the squared correlation coefficients (R2) are listed in Table 4.
As shown in Figures 4 and 5, the calculated densities from the correlation eq 8 are in good agreement with the experimental data of this work and the data in literature. The R2 of the correlation for BDA, DEEA, and BDA/DEEA blended solutions are 0.9829, 0.9889, and 0.9917, respectively. 1637
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where μ is the mixture viscosity, T is the temperature, x is the mole fraction of BDA or DEEA, and k1 to k6 are the correlation parameters. k2 is especially used to describe the interaction between BDA and DEEA. The calculated parameters and the average absolute deviations (AADs), the residual sum of squares (SSEs) and the squared correlation coefficients (R2) are listed in Table 6. As shown in Figures 6 and 7, the calculated viscosities from correlation eq 9 agree well with the experimental data in this paper and in the literature. The R2 of the correlation for BDA, DEEA, and BDA/DEEA blended solutions are 0.9748, 0.9919, and 0.9726, respectively. Solubility of N2O. The solubility of N2O defined by eq 7, HN2O, in BDA, DEEA, and BDA/DEEA solutions were presented in Figures 8 and 9, and the N2O solubility (mass fraction w, kg/kg) were listed in Table 7. Figure 10 compares the CO2 solubility data of DEEA calculated by N2O solubility data using eq 1 in this work and the data in the literatures26−29 under the same conditions. Also,
Viscosity. The measurements of viscosities in this work also comprise the aqueous solutions of BDA, DEEA, and the BDA/ DEEA blends. The experimental data are presented in Table 5 and Figures 6 and 7. For the DEEA solutions, the experimental data of this work are compared with literature data25 in Figure 6 for the same conditions. The viscosities of the binary and ternary mixtures increase with increasing mole fraction of BDA or DEEA and decreasing temperature. The experimental viscosity data for the binary and ternary mixtures were also fitted by Liu’s equation as a function of temperature and concentrations of BDA and DEEA,31 shown as eq 9. The correlation method was the same as for the density data. μBDA + DEEA (mPa ·s) ⎛ (x (x + k 2x DEEA ) + k 2x DEEA)2 ⎞ ⎟ = ⎜1 + k1 BDA + k 3 BDA T T2 ⎠ ⎝ ⎛k ⎞ k × exp⎜ 4 + 52 + k6(x BDA + k 2x DEEA )2 ⎟ ⎝T ⎠ T
(9)
Figure 7. Viscosities of aqueous BDA solutions measured and calculated by this work. Figure 9. N2O solubility HN2O in aqueous BDA/DEEA blended solutions at (298.15, 313.15, and 333.15) K.
Figure 10. CO2 physical solubility HCO2 in aqueous DEEA solutions at (298.15, 313.15, and 333.15) K in this work and compared with literature.27−29
Figure 8. N2O solubility HN2O in aqueous BDA and DEEA solutions at (298.15, 313.15, and 333.15) K. 1638
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Table 7. Solubility of N2O (Mass Fraction w, kg/kg) in Aqueous BDA (x1), DEEA (x2), and BDA/DEEA Blended Solutions at (298.15, 313.15, and 333.15) K 10x1 (mol/mol) 0
0.1952
T/K
PN2O/kPa
w/%
PN2O/kPa
w/%
PN2O/kPa
298.15 313.15 333.15
150.90 150.30 181.70
0.1677 0.1180 0.0829
129.80 152.98 146.43
0.1468 0.1111 0.0882
133.50 145.50 146.50
0
0.2012
0.6965 w/%
PN2O/kPa
0.1358 143.20 0.1009 166.02 0.0868 145.00 10x2 (mol/mol)
0.4547
T/K
PN2O/kPa
w/%
PN2O/kPa
w/%
PN2O/kPa
298.15 313.15 333.15
150.90 150.30 181.70
0.1677 0.1180 0.0829
133.10 156.60 170.19
0.1281 0.1130 0.1104
158.10 154.39 142.15
0.3629/1.4516
a
0.4244
0.8749/1.7499
1.0253 w/%
PN2O/kPa
w/%
PN2O/kPa
w/%
0.1143 0.1001 0.0863
143.20 166.02 145.00
0.1030 0.1053 0.0791
155.40 138.81 158.00
0.1039 0.0831 0.0827
0.7875 w/%
PN2O/kPa
0.1566 131.70 0.1196 140.97 0.1025 141.63 10x1/10x2(mol/mol)
1.6703/2.2270
1.4336
1.2520
1.9329
w/%
PN2O/kPa
w/%
PN2O/kPa
w/%
0.1385 0.1273 0.1141
128.80 130.94 139.49
0.1638 0.1513 0.1501
125.40 124.68 114.77
0.1962 0.1797 0.1457
0.6799/1.0198
0.5618/0.5618
0.8712/0.9376
T/K
PN2O/kPa
w/%
PN2O/kPa
w/%
PN2O/kPa
w/%
PN2O/kPa
w/%
PN2O/kPa
w/%
PN2O/kPa
w/%
298.15 313.15 333.15
126.30 107.40 135.00
0.1798 0.1343 0.1513
122.10 117.50 127.80
0.2022 0.1748 0.1765
115.90 107.40 119.70
0.2628 0.2077 0.1993
140.40 151.10 132.40
0.1548 0.1572 0.1282
141.20 150.30 135.20
0.1281 0.1255 0.1065
152.40 145.90 142.00
0.1788 0.1530 0.1360
The standard uncertainty of w measurement is ± 2 %.
Notes
the solubility data of 2.01 mol % DEEA at (313.15 and 333.15) K were repeated in Figure 10, to further verifies the good accuracy and repeatability of the experiment system. Figures 8 and 9 indicate that the N2O solubility of BDA is higher than DEEA at all of the measured concentrations. The N2O solubility in BDA solution increases with the increasing BDA concentration, while that in DEEA solution decreases with the increasing DEEA concentration. The N2O solubility in BDA/DEEA mixture decreases with the increasing DEEA concentration in the mixtures.
The authors declare no competing financial interest.
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CONCLUSION Densities, viscosities, and solubilities of N2O in BDA, DEEA, and BDA/DEEA aqueous solutions were measured with the amine concentration of (1.95−14.3 mol %) BDA, (2.01−19.3 mol %) DEEA, and (3.63−16.7 mol %) BDA + (2.62−22.2 mol %) DEEA. The densities and N2O solubilities were measured at (298.15, 313.15, and 333.15) K, whereas the viscosities were obtained at (298.15, 303.15, 313.15, 323.15, and 333.15) K. The measurement results agreed well with the literature data. The densities and viscosities of the binary and ternary mixtures were correlated by two semiempirical correlations in the literature. The correlated results are in good agreement with the experimental and literature data within the range of temperature and amine concentration in this work. The N2O solubility in BDA solution increases with the increasing BDA concentration, whereas that in DEEA solution decreases with the increasing DEEA concentration. The N2O solubility in BDA/DEEA mixture decreases with the increasing DEEA concentration in the mixture.
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REFERENCES
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Financial support from Chinese MOST project “Key Technology Research and Development on Advanced Coal Conversion and Power Generation” (2010DFA72730) is greatly appreciated. 1639
dx.doi.org/10.1021/je301371p | J. Chem. Eng. Data 2013, 58, 1633−1640
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