Vapor–Liquid Phase Equilibrium Data of CO2 in Some Physical

Jan 31, 2014 - Additionally, Henry,s law constant increases with temperature increase to ... physical solvents with esters or ether bonds for CO2 capt...
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Vapor−Liquid Phase Equilibrium Data of CO2 in Some Physical Solvents from 285.19 K to 313.26 K Xia Gui,*,† Wei Wang,† ChenWei Wang,† Ling Zhang,† Zhi Yun,† and Zhg Tang*,‡ †

College of Chemistry and Chemical Engineering, Nanjing University of Technology, Nanjing, Jiangsu 210009, P. R. China State Key Laboratory of Chemical Engineering, Department of Chemical Engineering, Tsinghua University, Beijing 100084, P. R. China

‡

ABSTRACT: The solubility of CO2 in polyethylene glycol dimethyl ether (NHD), octamethyl cyclotetrasiloxane (D4), and diethyl succinate (DS) was determined at the temperature variations from 285.19 K to 313.26 K up to 6 MPa by the constant-volume method. Then, Henry’s law constant (H) based on mole fraction was obtained by linear fitting of the vapor−liquid phase equilibrium data, and some thermodynamic properties of solutions were also calculated from the correlation of H. The values of H in NHD, D4, and DS vary from 2.5 MPa to 8 MPa and increase in the following order: DS < D4 < NHD, which is identical to the order of the solvents ability to dissolve CO2. Additionally, Henry’s law constant increases with temperature increase to confirm the solubility of CO2 decrease in the corresponding solvents for the pressure range studied.

1. INTRODUCTION Global warming and climate change caused by greenhouse gases (GHGs) have become one of the most critical issues of global concern in recent years, due to a further deterioration of the natural environment, economic development, and even human survival.1,2 As one of the main contributors, carbon emission reduction has become a worldwide environmental issue at the current time. Integrated gasification combined cycle (IGCC) combined with carbon capture and storage (CCS) technology is one of the promising options for near-zero CO2 emission.3,4 Compared with other decarbonization methods, the traditional solvent-based process is still the most commonly used technology and expected to be an economically feasible and effective CO2 capture process.5 Unlike chemical solvent absorption, physical solvents such as methanol, propylene carbonate, and polyethylene glycol dimethyl ether (Selexol) can be treated at low temperature or high pressure in absorption process and then regenerated by the pressure or temperature change in the desorption process.6 Thus, an effective and lowcost physical absorbent for large-scale industrial applications should have the characteristics of low vapor pressure to prevent solvent loss, high CO2 selectivity, low viscosity, chemical stability, and noncorrosive behavior. Some studies have shown that the dissolving ability of different organic solvents on CO2 is closely related to their molecular structure and weight.7,8 Moreover, it is also found by contrast that a macromolecule solvent with esters or ether bonds in molecules has a greater solubility and higher selectivity.9 As a successive work, this study also pays special attention to physical solvents with esters or ether bonds for CO 2 capture.5,9,10 The vapor−liquid equilibrium (VLE) experiments were performed within the temperature range 290.15 K to 320.15 K at pressures from 0.1 MPa to 6 MPa. New experimental © 2014 American Chemical Society

data of CO2 solubility in NHD, D4, and DS were presented. However, it is noteworthy that NHD (developed by the Research Institute of Nanjin Chemical Industry Group) is a molecular mixture with a different structural formula (CH3O(CH2CH2O)nCH3), where n is the number of ethylene oxide. NHD has similar excellent properties to UOP Selexol solvent, such as negligible vapor pressure, chemical and thermal stability, and nontoxicity. D4 is a kind of medium molecular weight spherical crown ether, which can be used as an intermediate in preparing silicondioxide, siliconeoil and silicone by ring-opening polymerization. DS is commonly used as a kind of plasticizer, special lubricant, or organic synthetic intermediate, etc.

2. EXPERIMENTAL SECTION 2.1. Materials. CO2 with a volume fraction of 0.9999 was supplied by BeiWen Gas in Beijing. NHD (CH3O(CH2CH2O)nCH3, with a mass fraction of 0.999, made in China), D4 (C8H24O4Si4, with a mass fraction of 0.999, made in China), and DS (C8H14O4, with a mass fraction of 0.999, made in China) were obtained from Aladdin-Reagent Company in Shanghai. All components were used without further purification, and some properties of these substances from supplier are listed in Table 1. 2.2. Apparatus and Experimental Procedures. The vapor−liquid phase equilibrium data between CO2 and various solvents (NHD, D4, and DS) were determined by the constantvolume method. The apparatus mainly consists of a highpressure equilibrium vessel (250 mL/15 MPa) and a gas buffer tank (250 mL/25 MPa), both with precision pressure sensors (± 1 kPa) and resistance thermometer (Pt-100, ± 0.1 K). Received: November 14, 2013 Accepted: January 24, 2014 Published: January 31, 2014 844

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Table 1. Basic Properties of NHD, D4, and DS properties

NHD

D4

DS

molecular formula average molecular weight/g·mol−1 density at 298 K/g·mol−1 freezing point/K boiling point/K

CH3O(CH2CH2O)nCH3, n = 3 to 8 250 1.027 248 523

C8H24O4Si4 296.62 0.956 288 448

C8H14O4 174.2 1.04 253 490

equilibrium vessel step, (n1 − n2) is the total amount of CO2 gas entered equilibrium vessel 3, and ng is the amount of CO2 in gas phase at equilibrium state. The values of n1, n2, ng, and ni are calculated respectively by the SRK equation of state with some nonideality correction from PVT data. At last, assume that the solvent follows Raoult’s law, and then the equilibrium CO2 partial pressure PE can be calculated from:

The whole system temperature was controlled by a jacket heating mode. All of the sensors were connected by a digital indicator, which can transmit the pressure and temperature variations to the computer continuously. Details of the experimental apparatus are given in Figure 1. Experiments

P E = P − P S(1 − x) − P i

where P is the total equilibrium pressure inside the vessel 3, PS is the saturated vapor pressure of the solvent at the equilibrium temperature, and Pi is the inert gas pressure. The expanded uncertainties of the whole measurement comprise system errors for pressure, temperature, and volume. The measurement errors of temperature, pressure, and volume are u(T) = 0.1 K, u(P1) = u(P2) = 0.01 MPa, u(PE) = 0.001 MPa, and u(V) = 0.05 mL. According to the method of the estimation of uncertainties, the overall uncertainty for the measured solubility of CO2 can be calculated from:

Figure 1. Schematic diagram of the apparatus. 1, CO2 gas cylinder; 2, gas buffer tank; 3. equilibrium vessel; 4, waste container; 5, water bath; 6, digital temperature; 7, digital pressure transducer; 8, vacuum pump; 9, liquid injector; 10, computer.

u(x) = x

were performed respectively at 285.19 K, 291.43 K, 299.56 K, 304.37 K, and 313.26 K in the high-pressure equilibrium vessel. When the system reached equilibrium status, the pressure and temperature reading in the vessel were constant for a long time. Then, the vapor−liquid phase equilibrium data were calculated from material balance. The details of the experiment can be found in a previous report.5,9

=

nE nE + nl E

u(n1)2 + u(n2)2 + u(ng )2 (n E)2

+

u(n1)2 + u(n2)2 + u(ng )2 + u(n l)2 (n E + n l)2

(5) 2 ⎛ u(V ) ⎞2 ⎛ u(T ) ⎞2 u(n) 1 ⎛ u(P) ⎞ = ⎜ ⎟ +⎜ ⎟ +⎜ ⎟ ⎝ V ⎠ ⎝ T ⎠ n R ⎝ P ⎠

(6)

and u(nl) is estimated by: ρ u(n l) = u(Vl ) (7) M 3.2. Henry’s Constant and Thermodynamic Properties. Henry’s constant is often defined as:5,6,9

(1) l

where n is the gas amount absorbed and n is the solvent amount added. Then, the amount of solvent nl added to equilibrium vessel 3 is calculated from

Hx(T , P) = lim

xCO2 → 0

ρΔV (2) M where ρ is the density of the solvent, ΔV is the volume of the solventm and M is the mean molecular weight of the solvent. Because of the negligible vapor pressure of high boiling point solvents selected, the residual amount of gas ni after evacuating equilibrium vessel 4 can be considered to be inert, and the absorbed amount of CO2 nE in liquid phase at equilibrium state is considered to be: nl =

n E = (n1 − n2) − n i − ng

⎛ u(n E) ⎞2 ⎛ u(n E + n l) ⎞2 ⎟ ⎜ E ⎟ +⎜ E ⎝ n ⎠ ⎝ n + nl ⎠

in which u(n1), u(n2), and u(ng) can be estimated by:

3. RESULTS AND DISCUSSION 3.1. CO2 Solubility in Physical Solvents. The solubility of CO2 in various physical solvents is expressed in mole fraction: x=

(4)

≈

PE xCO2

L fCO (T , P ) 2

xCO2

= lim

xCO2 → 0

PϕCO (T , P) 2

xCO2 (8)

where Hx(T,P) is the Henry’s law constant based on the mole fraction, xCO2 is the mole fraction of CO2 in the liquid phase, f LCO2 is the fugacity of CO2, PϕCO2(T,P) is the fugacity coefficient, and PE is the equilibrium partial pressure of CO2. By convention, f LCO2 is considered to be approximately equal to PE at moderate pressure. Henry’s constant often represents the linear relationship well between gas concentration and pressure at finite dilution, which also means that Henry’s law constant can be obtained by calculating the linear slope of pressure and molar fraction.

(3)

where n1 is the initial amount of CO2 in buffer tank 2, n2 is the amount of CO2 in buffer tank 2 after the gas entering 845

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Table 2. Mole Fraction (xi), Equilibrium Partial Pressure of CO2 (PE), and Uncertainties (δi) for the Binary Mixture CO2 + NHD from 285.19 K to 313.26 K PE/MPa

xi

0.0786 0.1442 0.1688 0.1853 0.2275 0.2666 0.2993 0.3651 0.4254

0.0295 0.0541 0.0633 0.0732 0.0853 0.0999 0.1122 0.1294 0.1595

0.0752 0.1262 0.1733 0.2291 0.2677 0.3005 0.3443 0.3928 0.4090

0.0253 0.0424 0.0582 0.0702 0.0899 0.1009 0.1156 0.1305 0.1373

0.0810 0.1355 0.1969 0.2524 0.2666 0.3057 0.3502 0.4618 0.5215

0.0229 0.0383 0.0557 0.0629 0.0754 0.0865 0.0991 0.1165 0.1475

0.0666 0.1273 0.1598 0.2044 0.2599 0.2988 0.3371 0.3773 0.4422

0.0179 0.0315 0.0429 0.05484 0.0697 0.0775 0.0904 0.1012 0.1079

0.0803 0.1272 0.1791 0.1947 0.2533 0.2806 0.3869 0.4518 0.7795

0.0189 0.0299 0.0375 0.0459 0.0526 0.0661 0.0818 0.1065 0.1838

δi

PE/MPa

T = 285.19 K 0.0009 0.5765 0.0009 0.6511 0.0011 0.7222 0.0008 0.9531 0.0013 1.2423 0.0009 1.4776 0.0011 1.6003 0.0011 1.8319 0.0010 2.146 T = 291.43 K 0.0013 0.4269 0.0008 0.6938 0.0010 0.9143 0.0011 1.2621 0.0008 1.5374 0.0009 1.7135 0.0009 1.9969 0.0012 2.1847 0.0009 2.3985 T = 299.56 K 0.0010 0.7728 0.0010 0.9763 0.0008 1.2775 0.0009 1.5413 0.0009 1.7316 0.0011 1.9528 0.0010 2.2712 0.0011 2.5323 0.0012 2.8526 T = 304.37 K 0.0011 0.4605 0.0011 0.5011 0.0010 0.7968 0.0009 1.1239 0.0010 1.6962 0.0012 2.1464 0.0008 2.494 0.0008 2.8599 0.0010 3.1002 T = 313.26 K 0.0010 1.3327 0.0010 1.6616 0.0009 1.9492 0.0009 2.1644 0.0010 2.4309 0.0009 2.7007 0.0008 2.9355 0.0008 3.1526 0.0013 3.4303

Table 3. Mole Fraction (xi), Equilibrium Partial Pressure of CO2 (PE), and Uncertainties (δi) for the Binary Mixture CO2 + D4 from 285.19 K to 313.26 K

xi

δi

PE/MPa

xi

δi

0.2162 0.2366 0.2708 0.3574 0.4658 0.5540 0.6001 0.6869 0.7672

0.0010 0.0011 0.0012 0.0011 0.0009 0.0011 0.0010 0.0009 0.0010

0.0818 0.1324 0.1899 0.2102 0.2556 0.3269 0.3937 0.433

0.0275 0.0445 0.0605 0.0707 0.0859 0.1099 0.1257 0.1456

0.1433 0.2329 0.3069 0.4236 0.4993 0.5755 0.6703 0.7334 0.7850

0.0011 0.0009 0.0009 0.0012 0.0008 0.0009 0.0012 0.0011 0.0010

0.0916 0.1355 0.1882 0.2413 0.2712 0.3364 0.3998 0.4485 0.4992

0.0277 0.0411 0.0569 0.0732 0.0821 0.1018 0.1209 0.1357 0.1506

0.2186 0.2705 0.3614 0.4360 0.4898 0.5524 0.6425 0.7164 0.7956

0.0012 0.0011 0.0010 0.0009 0.0011 0.0009 0.0009 0.0009 0.0010

0.0891 0.1406 0.1887 0.2249 0.2865 0.4519 0.6043 0.7466 0.8538

0.0243 0.0383 0.0487 0.0613 0.0781 0.1149 0.1647 0.1953 0.2327

0.1236 0.1345 0.2084 0.3016 0.4551 0.5759 0.6692 0.7673 0.8049

0.0011 0.0010 0.0009 0.0011 0.0010 0.0011 0.0009 0.0012 0.0009

0.0773 0.1336 0.1699 0.2427 0.2738 0.3621 0.4449 0.5604 0.6941

0.0199 0.0319 0.0438 0.0601 0.0707 0.0883 0.1097 0.1446 0.1766

0.3142 0.3917 0.4454 0.5102 0.5730 0.6367 0.6920 0.7432 0.7851

0.0011 0.0009 0.0008 0.0010 0.0010 0.0009 0.0010 0.0009 0.0013

0.05833 0.1514 0.1876 0.2614 0.2957 0.3766 0.4431 0.6462 0.8561

0.0134 0.0301 0.0407 0.0529 0.0677 0.0862 0.0946 0.1479 0.1915

PE/MPa

T = 285.19 K 0.0012 0.5571 0.0010 0.6665 0.0012 0.7467 0.0009 0.8643 0.0008 1.1620 0.0009 1.4409 0.0011 1.7874 0.0009 2.2351 T = 291.43 K 0.0007 0.5646 0.0008 0.6006 0.0009 0.7742 0.0011 0.8822 0.0010 0.9623 0.0013 1.2869 0.0011 1.5535 0.0012 1.9985 0.0010 2.4634 T = 299.56 K 0.0006 0.9292 0.0008 1.1192 0.0010 1.3634 0.0011 1.6085 0.0007 1.7017 0.0006 1.9535 0.0011 2.1869 0.0004 2.4423 0.0007 2.7742 T = 304.37 K 0.0009 0.7537 0.0012 0.8934 0.0009 1.1279 0.0011 1.4663 0.0009 1.7285 0.0009 1.9701 0.0012 2.2535 0.0009 2.5382 0.0011 2.8362 T = 313.26 K 0.0009 1.1457 0.0010 1.4935 0.0009 1.6538 0.0011 1.8152 0.0009 2.1297 0.0012 2.4527 0.0011 2.7678 0.0012 3.1335 0.0012 3.4822

xi

δi

0.1873 0.2140 0.2511 0.2906 0.3907 0.4845 0.6010 0.7179

0.0010 0.0008 0.0009 0.0010 0.0011 0.0011 0.0013 0.0008

0.1648 0.1817 0.2342 0.2578 0.2911 0.3893 0.4699 0.5955 0.7148

0.0012 0.0013 0.0009 0.0009 0.0007 0.0012 0.0009 0.0007 0.0012

0.2533 0.2941 0.3716 0.4275 0.4638 0.5324 0.5960 0.6439 0.7288

0.0008 0.0010 0.0009 0.0008 0.0010 0.0006 0.0004 0.0007 0.0006

0.1945 0.2306 0.2911 0.3707 0.4358 0.5084 0.5816 0.6448 0.7061

0.0009 0.0011 0.0013 0.0008 0.0010 0.0008 0.0009 0.0011 0.0009

0.2624 0.3283 0.3787 0.4157 0.4877 0.5617 0.6339 0.7085 0.7746

0.0011 0.0007 0.0009 0.0010 0.0009 0.0011 0.0009 0.0008 0.0014

equilibrium at a given pressure and temperature, the value of the Gibbs free energy is minimized. P0 refers to 0.1 MPa.

Thermodynamic properties of CO2 dissolved in physical solvents can be deduced from the following equations:6,11,12

⎛ ∂ ln(H(T , P))/P 0 ⎞ Δsol H = R ⎜ ⎟ ∂(1/T ) ⎠P ⎝

RT ln(H(T , P)) Δsol G = (9) P0 where ΔsolG is the solution Gibbs free energy and also the chemical potential. When the binary mixture system reaches

(10)

where ΔsolH is the enthalpy, which also determines whether the absorption process is spontaneous. Furthermore, the value of 846

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Figure 2. Vapor−liquid equilibrium of the binary mixture CO2 + NHD. x is the mole fraction of CO2 in the liquid phase, and PE is the partial pressure of CO2 at equilibrium state: ●, 285.19 K; ■, 291.43 K; ▲, 299.56 K; ○, 304.37 K; △, 313.26 K.

Figure 3. Vapor−liquid equilibrium of the binary mixture CO2 + D4. x is the mole fraction of CO2 in the liquid phase, and PE is the partial pressure of CO2 at equilibrium state: ●, 285.19 K; ■, 291.43 K; ▲, 299.56 K; ○, 304.37 K; △, 313.26 K.

Figure 4. Vapor−liquid equilibrium of the binary mixture CO2 + DS. x is the mole fraction of CO2 in the liquid phase, and PE is the partial pressure of CO2 at equilibrium state: ●, 285.19 K; ■, 291.43 K; ▲, 299.56 K; ○, 304.37 K; △, 313.26 K.

ΔsolH also indicates the strength of interaction between solute and solvent in the liquid phase. Δsol S =

Δsol H − Δsol G T

decreasing pressure, which indicates that the absorption of CO2 in these solvents is the typical physical process. At a constant temperature, it is often known that the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of the gas in equilibrium with the liquid. Thus, the gas−liquid partitioning equilibrium constant, better known as Henry’s law constant, can be considered to be not evidently influenced by pressure at moderate pressure. Figures 2 to 4 just explain that the gas solubility in solvents follows Henry’s Law well at low pressure, but the deviation of linearity between P−x becomes larger while pressure increases. Henry’s constants (based on mole fraction, H) of CO2 in NHD, D4, and DS at different temperature are given in Table 5 and plotted in Figure 5.

(11)

where ΔsolS is the solution entropy to show the order of the amount of molecules in the whole system. 3.3. Results and Discussion. The operating temperature T, the CO2 partial pressure PE at the equilibrium state, CO2 mole fraction xi in the liquid phase, and the estimated uncertainties δi, for the binary systems CO2 + NHD, CO2 + D,4 and CO2 + DS are presented in Tables 2, 3, and 4 and plotted in Figure 2, 3, and 4. It can be seen from Tables 2 to 4 that the solubility of CO2 in NHD, D4, and DS decreases with increasing temperature and 847

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Table 4. Mole Fraction (xi), Equilibrium Partial Pressure of CO2 (PE), and Uncertainties (δi) for the Binary Mixture CO2 + DS from 285.19 K to 313.26 K PE/MPa

xi

0.0636 0.1336 0.1992 0.2732 0.5255 0.8287 0.9662 1.2609 1.4352

0.0143 0.0300 0.0389 0.0616 0.1067 0.1868 0.2178 0.2707 0.3236

0.1397 0.1762 0.2281 0.2722 0.4631 0.8078 1.0027 1.3376 1.6052

0.0273 0.0345 0.0407 0.0532 0.0906 0.1522 0.1962 0.2539 0.2945

0.1784 0.2584 0.3227 0.4851 0.5229 0.6367 0.7233 0.9547 1.4085

0.0292 0.0424 0.0529 0.0796 0.0858 0.1045 0.1187 0.1567 0.2180

0.1231 0.2557 0.3244 0.4711 0.6415 0.8289 1.0933 1.3964 1.7182

0.0187 0.0388 0.0492 0.0714 0.0972 0.1256 0.1657 0.2117 0.2604

0.1547 0.2544 0.4539 0.5074 0.7672 0.8851 1.2448 1.5831 1.7878

0.0201 0.0329 0.0587 0.0656 0.0863 0.1144 0.1609 0.2047 0.2311

δi T 0.0010 0.0012 0.0009 0.0007 0.0008 0.0009 0.0007 0.0008 0.0013 T 0.0011 0.0010 0.0010 0.0009 0.0008 0.0012 0.0011 0.0007 0.0011 T 0.0006 0.0005 0.0009 0.0009 0.0013 0.0010 0.0012 0.0011 0.0007 T 0.0012 0.0011 0.0011 0.0012 0.0012 0.0011 0.0007 0.0009 0.001 T 0.0008 0.0012 0.0011 0.0007 0.0011 0.0012 0.0013 0.001 0.0013

PE/MPa = 285.19 K 1.7246 1.8935 2.1579 2.4146 2.5962 2.7723 2.9798 3.3784 3.5653 = 291.43 K 1.8431 2.0235 2.3414 2.5619 2.8865 3.3142 3.595 3.8831 4.2124 = 299.56 K 1.7121 2.1197 2.3151 2.7334 2.9904 3.2797 3.5822 3.9619 4.2986 = 304.37 K 2.059 2.4713 2.6519 2.9577 3.3318 3.5792 3.7944 4.1568 4.6732 = 313.26 K 2.0433 2.3651 2.7457 3.2295 3.7326 4.2401 4.7611 5.4505 5.8058

xi

Table 5. Henry’s Constant (H) of the CO2 in NHD, D4, and DS from 285.19 K to 313.26 K H/MPa

δi

0.3888 0.4269 0.4865 0.5444 0.5853 0.6250 0.6718 0.7391 0.7812

0.0009 0.0012 0.0010 0.0009 0.0009 0.0013 0.0012 0.0011 0.0013

0.3607 0.3959 0.4581 0.5013 0.5648 0.6485 0.7035 0.7499 0.8047

0.0012 0.0013 0.0009 0.0008 0.0013 0.0012 0.0009 0.0009 0.0012

0.280985361 0.339673735 0.379948139 0.448598438 0.490776603 0.538255761 0.587901267 0.633804897 0.679216175

0.0009 0.0010 0.0009 0.0012 0.0010 0.0012 0.0007 0.0007 0.0007

0.3121 0.3746 0.4019 0.4483 0.5051 0.5425 0.5751 0.6164 0.6932

0.0009 0.0012 0.001 0.0009 0.0009 0.0013 0.001 0.0009 0.0009

0.2642 0.3058 0.3421 0.4175 0.4826 0.5353 0.6156 0.6918 0.7377

0.001 0.0012 0.0006 0.0013 0.0014 0.0011 0.001 0.0009 0.0012

T/K 285.19 291.43 299.56 304.37 313.26

NHD 2.6969 3.0011 3.5430 3.7568 4.2694

± ± ± ± ±

D4 0.08 0.11 0.17 0.14 0.26

3.0187 3.3604 3.7307 3.9289 4.4087

DS

± ± ± ± ±

0.10 0.15 0.19 0.22 0.33

4.4769 5.1483 6.1671 6.6445 7.8109

± ± ± ± ±

0.11 0.17 0.24 0.31 0.45

Figure 5. Henry’s constant (based on mole fraction) of CO2 in different solvents: ●, NHD, this study; ▲, D4, this study; ■, DS, this study; ○, Selexol, studied by Xu et al.;13 △, D4, studied by Wilcock and Mchale;14 □, DS, studied by Feng et al.15

Table 6. Thermodynamic Properties of Solutions for CO2 in NHD, D4, and DS at 313.26 K ΔsolG −1

ΔsolH −1

T/K

kJ·mol

kJ·mol

NHD D4 DS

9.7772 9.8608 11.3504

−10.2803 −10.0781 −12.4575

ΔsolS J·mol−1·K−1 −64.0283 −63.6497 −76.0004

of CO2 in NHD, D4, and DS obtained will be important for developing processes of CO2 capture. Moreover, these data are essential for the kinetic modeling of NHD, D4, DS, or their mixtures in gas purification process design.

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AUTHOR INFORMATION

Corresponding Authors

*E-mail: [email protected], [email protected]. Fax: +86-025-8358 7184. *E-mail: [email protected]. Funding

This research is supported by the National Natural Science Foundation of China (NSFC 21306088) and State Key Laboratory of Chemical Engineering (no. SKL-ChE-13A01, Tsinghua University, China). Notes

The authors declare no competing financial interest.

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REFERENCES

(1) Fisher, J. C.; Siriwardane, R. V.; Stevens, R. W. Process for CO2 Capture from High-Pressure and Moderate-Temperature Gas Streams. Ind. Eng. Chem. Res. 2012, 51, 5273−5281. (2) D’Alessandro, D. M.; Smit, B.; Long, J. R. Carbon dioxide capture: prospects for new materials. Angew. Chem., Int. Ed. 2010, 49, 6058−6082. (3) Cristina, B.; Randall, P. F.; Robert, D. B.; Howard, J. H.; Ahmed, F. G. Performance of an IGCC Plant with Carbon Capture and Coal-

The results illustrate that Henry’s constant varies from 2.5 MPa to 8 MPa and increases with the operating temperature increasing. Compared with the literature data, the deviations are in the allowable range, which show the same trend with temperature as that in literature.13−15 Additionally, the predicted values of ΔsolG, ΔsolH, and ΔsolS are listed in Table 6. Henry’s constants and the thermodynamic properties 848

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dx.doi.org/10.1021/je400985u | J. Chem. Eng. Data 2014, 59, 844−849