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Cite This: J. Chem. Eng. Data 2019, 64, 2542−2549
Hydrate Dissociation Data for the Systems (CO2/CH4/Ar) + Water with (TBAF/TBAA/TBPB/TBANO3 and Cyclopentane) Poorandokht Ilani-Kashkouli, Hamed Hashemi,* Anneline Basdeo, Paramespri Naidoo, and Deresh Ramjugernath
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Thermodynamics Research Unit, School of Engineering, University of KwaZulu-Natal, Howard College Campus, King George V Avenue, Durban 4041, South Africa ABSTRACT: Hydrate dissociation conditions are reported for the following systems: CO2 + tetra-n-butyl ammonium acetate (TBAA) + water, CO2 + tetra-n-butyl ammonium fluoride (TBAF) + water, CO2 + tetra-n-butyl ammonium bromide (TBAB) + cyclopentane + water, Ar + tetrabutylphosphonium bromide (TBPB) + water, Ar + tetrabutyl ammonium nitrate (TBANO3) + water, and methane + TBAB + cyclopentane + water. The measurements were performed using an isochoric pressure-search method in the temperature range of (276.1−302.7) K and the pressure range of (0.31− 9.90) MPa. The results show that TBAF and TBAA have a promotion effect on CO2 hydrates, and TBPB and TBANO3 promote Ar hydrate formation. Furthermore, the addition of cyclopentane to 0.05 mass fraction TBAB aqueous solution results in a significant promotion effect.
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desalination,20 refrigeration,21,22 separation processes,23 natural gas recovery from natural hydrate formations24−26 and fire extinction27 are examples of positive applications of hydrate formation. Carbon dioxide (CO2) is regarded as the main greenhouse gas which results from anthropogenic activities causing global warming and climate change.28 The increasing level of carbon dioxide in the atmosphere is one of the most concerning environmental issues of era because of the industrial revolution.29 In order to limit CO2 emissions and mitigate its effects on climate change, carbon capture and storage technologies from industrial and natural sources are required.30 There are several known technologies available for CO2 capture such as absorption,31−33 adsorption,34−36 membrane,37,38 cryogenic separation,28,39 and so forth. A novel approach that has been recently proposed is separation of CO2 through utilization of the gas hydrate formation (crystallization) technique.40−43 Submarine gas hydrate reservoirs (SUGAR)44 is the name of a project running in Germany, in which CO2 is being injected into the submarine methane hydrate reservoirs to replace methane molecules with CO2 molecules in the hydrate cavities, resulting in the vast production of methane gas in a win−win situation. Knowledge of hydrate-phase equilibria is necessary to design and optimize hydrate-based processes.
INTRODUCTION Gas hydrates (or clathrate hydrates) are nonstoichiometric, crystalline inclusion compounds composed of water (the host) and small molecules of a suitable size (the guest), formed under conditions of low temperatures and high pressures.1 Within the clathrate lattice, water molecules form a network of hydrogen-bonded cavity structures that enclose the guests.1 Compounds having a molecular size less than 0.9 nm may form clathrate hydrates which, depending on the size of the entrapped molecule(s), commonly occur as structures I (sI), II (sII), and H (sH), composed of various types of cavities.2 It is known that van der Waals forces between the guest and the host molecules ensure the stability of the hydrate structure.3 Clathrate hydrates generally form under conditions of high pressures and low temperatures, as mentioned earlier.3 Semi-clathrate hydrates have unusual hydrate structures which are formed by quaternary ammonium salts (QAS) such as tetra-n-butyl ammonium chloride (TBAC), tetra-n-butyl ammonium fluoride (TBAF), tetrabutylphosphonium bromide (TBPB), and tetrabutyl ammonium nitrate (TBANO3) with water molecules.4 In QAS semi-clathrate hydrates, the water molecules and anions (such as Cl-, F-) build a polyhedral host framework of the cages, and the cations (TBA+) occupy cages as guest molecules.5 Several studies on semi-clathrate hydrates have been reported.6−12 It has been shown over the past half century that hydrate formation, although undesirable during oil and gas production and transportation,13 can be advantageously exploited in various processes. Gas storage and transportation,14−17 carbon dioxide capture and sequestration,18,19 water treatment and © 2019 American Chemical Society
Received: January 18, 2019 Accepted: April 12, 2019 Published: May 24, 2019 2542
DOI: 10.1021/acs.jced.8b01195 J. Chem. Eng. Data 2019, 64, 2542−2549
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Table 1. Purities and Suppliers of Chemicalsa,b chemical
CAS number
purity (mass fraction)
supplier
N,N,N-tributyl-1-butanaminium acetate N,N,N-tributyl-1-butanaminium fluoride tetrabutyl phosphonium bromide TBANO3 N,N,N-tributyl-1-butanaminium bromide cyclopentane carbon dioxide methane argon
10534-59-5 429-41-4 3115-68-2 1941-27-1 1643-19-2 287-92-3 124-38-9 74-82-8 7440-37-1
≥0.97 ≥0.97 ≥0.98 ≥0.97 ≥0.97 ≥0.995 ≥0.999 ≥0.999 ≥0.999
Capital Lab Suppliers DLD Suppliers Sigma-Aldrich Sigma-Aldrich Sigma-Aldrich Sigma-Aldrich AFROX Ltd AFROX Ltd AFROX Ltd
a
Ultrapure Millipore Q water; conductivity = 18 MΩ·cm. bMole fraction purity stated by the manufacturer.
bath for temperature control. Because of the low freezing point of ethylene glycol, it provides an ideal medium for the thermostat bath. Platinum (Pt) temperature resistors are inserted into the cell to monitor the temperature of the bulk and fluid phase. The Pt100 probes measure over a range of (73.15−1073.15) K and temperature measurement uncertainties are estimated to be 0.1 K. Pressure transducers measure the cell pressure. The transducer has a pressure range of 1−10 MPa and pressure measurement uncertainties are estimated to be 0.005 MPa. The guidelines prepared by the National Institute of Standards and Technology53 were used in estimating the expanded uncertainties for the measured pressure and temperature. These combined uncertainties (for each variable, temperature or pressure) were calculated by taking into account the maximum error in the calibration polynomial and the manufacturer uncertainty inherent to the reference value (temperature or pressure transmitter). Experimental Procedure. The hydrate dissociation conditions were measured using an isochoric pressure-search method.54−56 The cell was immersed into the temperaturecontrolled bath. It was then evacuated using an Edwards vacuum pump to 0.01 kPa for approximately 30 min, after which the solution/liquid was introduced. Gas was then supplied from a gas cylinder through a pressure-regulating valve into the evacuated cell until the pressure inside the cell was increased to the desired level. After temperature and pressure recordings had stabilized, the valve in the line connecting the cell and cylinder was closed. Subsequently, the stirrer was initiated, and the temperature was slowly decreased to form hydrates. During cooling, a steady decrease of pressure was observed. Initial hydrate formation was detected by a rapid decrease in pressure because of encapsulation of the hydrate former. Because hydrate formation is an exothermic process, an abrupt increase in pressure was also observed. Once crystallization stopped, the temperature returned to the operative temperature. Throughout the process, pressure and temperature changes were monitored and recorded by a data acquisition system. After the completion of hydrate formation, the system was slowly heated to dissociate the hydrates. An abrupt increase in pressure marked the start of the dissociation process. The system was then allowed to reach equilibrium. Pressure and temperature changes were monitored and recorded by a data acquisition system. The complete decomposition of hydrates (equilibrium point) was noted by a decrease in the pressuretemperature gradient. For accurate equilibrium data, the dissociation process should be performed at a slow heating rate (∼0.1 K/h) to allow the system to reach equilibrium and prevent metastability. Figure 1 shows a typical pressure−
There are various studies in the literature considering the phase equilibrium of methane and carbon dioxide hydrate formation. Deschamps and Dalmazzone45 reported dissociation enthalpies and phase equilibrium for TBAB semi-clathrate hydrates of pure gases: N2 and CO2 and mixtures: N2 + CO2 and CH4 + CO2. Mayoufi et al.46 obtained phase equilibrium data for the CO2 hydrate in the presence of different ammonium/phosphonium salts including TBACl, TBANO3, and TBPB. Fukumoto et al. (2014, 2015)47,48 developed a thermodynamic model based on the model approach of Paricaud49 for predicting the hydrate dissociation conditions of CO2 and CO2 + H2 in the presence of TBAB, TBAF, TBAC, and TBPB TBNO3. In this study, we report phase equilibrium data (dissociation conditions) for the CO2 + tetra-n-butyl ammonium acetate (TBAA) + water, CO2 + TBAF + water, Ar + TBPB + water, Ar + TBANO3 + water, and CO2/CH4 + tetra-n-butyl ammonium bromide (TBAB) + cyclopentane (CP) + water systems. One of the objectives is to evaluate the effects of the aforementioned salts on hydrate stability conditions of CO2 and argon as well as the effect of an insoluble promoter such as CP on hydrate dissociation conditions for the system of CO2/CH4 + TBAB aqueous solution. We therefore report hydrate dissociation data for the systems of methane + TBAB + CP + water. Methane was included in this study because it is a well-known help gas for large hydrate formers.50 Gas separation using clathrate hydrate formation has been considered lately by many researchers, especially for the close boiling point gases. The purification of Xe from a mixture of noble gases such as Ar, Kr, and Xe using the gas hydrate process requires hydrate dissociation conditions. Furthermore, it is desirable to operate at low pressures because argon forms hydrate at comparatively high pressures. Hence, the generation of accurate hydrate-phase equilibrium data of gaseous mixtures in the presence of promoters becomes essential.
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EXPERIMENTAL SECTION Chemicals. Table 1 presents the purities and supplier details of the chemicals used in this work. Ultrapure Millipore Q water was obtained from the laboratory using Elga OptionR15 PURELAB Water Purification System at the University of KwaZulu-Natal (UKZN), and an electrical resistivity of 18 MΩ·cm was measured. Apparatus. A detailed description of the apparatus used in this study are reported in previous studies.51,52 Briefly, the apparatus contains a cylindrical equilibrium cell made of corrosion-resistant 316 stainless steel. A magnetic stirrer is installed in the cell to agitate the fluid and hydrate crystals inside it. The cell is immersed in an ethylene glycol and water 2543
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temperature diagram used for estimating hydrate dissociation conditions.
Figure 2. Hydrate dissociation conditions for the (CO2 + H2O) system: ◆, this work; ◇, ref 57; (CO2 + TBAA + H2O) systems: ■, 0.10 mass fraction, this work; ▲, 0.20 mass fraction, this work; ×, 0.30 mass fraction, this work.
Figure 1. Determination of hydrate dissociation point for semiclathrate hydrate of argon + 0.20 mass fraction TBPB aqueous solution.
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RESULTS AND DISCUSSION The hydrate dissociation conditions of CO2 in water were first measured and compared with the experimental data reported in the literature for checking the experimental procedure adapted in this work. Table 2 shows the measured dissociation Table 2. Measured Hydrate Dissociation Conditions for CO2 + H2Oa T/K
P/MPa
276.1 278.2 280.2 282.4
1.79 2.33 3.06 4.06
Figure 3. Hydrate dissociation conditions for: (CO2 + H2O system): ◆, this work; ◇, ref 57; (CO2 + TBAF + H2O) systems: ●, 0.041 mass fraction, this work; ○, 0.067 mass fraction, this work; ▲, 0.02 mass fraction, ref 58; □, 0.041 mass fraction, ref 57; -, 0.05 mass fraction, ref 58; ×, 0.15 mass fraction, ref 58; ■, 0.083 mass fraction, ref 57; +, 0.1 mass fraction, ref 59.*, 0.049 mass fraction, ref 59; △, 0.105 mass fraction, ref 60.
a
u(T) = 0.1 K, u(P) = 0.005 MPa.
CO2 are shifted to lower pressures or higher temperatures because of the presence of TBAF in the system (in the concentration ranges studied in the present work) when compared with the pure CO2 hydrate. It is found in Figures 2 and 3 that the hydrate stability zone is enlarged with TBAA and TBAF concentrations, respectively. An increase in TBAA and TBAF concentration results in an improved promotion effect of the equilibrium pressure. When comparing the two promoters, TBAA and TBAF, TBAF displays a greater promotion effect, as evident in the data presented in Figure 3, with TBAF mass fraction (of 0.02− 0.15), as compared to the TBAA mass fraction of 0.1−0.3 as presented in Figure 2. The agreement between the experimental data reported in the literature and this study is generally acceptable. The phase equilibrium data of semi-clathrate hydrates of argon + TPBP + water and argon + TBANO3 + water systems are reported in Tables 5 and 6 and Figures 4 and 5, respectively. It can be seen in Figure 4 that TBPB has a strong promotion effect on argon hydrate. The addition of TBPB salt causes the phase equilibrium curve of Ar + TBPB + water to shift to
data for the hydrate (H) of CO2 (V) in water (Lw) and the comparison with the literature data is plotted in Figures 2 and 3. Although extensive CO2 hydrate dissociation data can be found in the literature,1 these new measurements were undertaken in order to validate the experimental procedure, as mentioned earlier. Furthermore, this served as a means to assess the accuracy of the experimental set up. As observed in Figures 2 and 3, the newly reported CO2 hydrate dissociation data are consistent with those reported in the literature, confirming the reliability of dissociation points reported herein. Experimental hydrate dissociation conditions for CO2 + aqueous solutions of TBAA and TBAF in the phase boundary of hydrate−liquid water−vapor (H−Lw−V) are reported in Tables 3 and 4, respectively. The reported experimental data are also plotted in Figures 2 and 3 and are compared with the literature data. Few sets of experimental data are available in the literature for the CO2 + TBAF + water system. TBAF acts as the semi-clathrate hydrate former which would have lower dissociation pressures than of the pure CO2 hydrate. The hydrate dissociation conditions of 2544
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Table 3. Semi-Clathrate Hydrate Dissociation Conditions (H−Lw−V) for the CO2 + TBAA + Water Systema
Table 5. Semi-Clathrate Hydrate Dissociation Conditions (H−Lw−V) for the (Ar + TBPB + H2O) Systema
mass fraction of TBAA
T/K
P/MPa
mass fraction of TBPB
T/K
P/MPa
0.10
283.6 283.1 282.4 281.4 280.4 279.3 287.0 286.6 286.4 286.2 285.9 285.6 285.2 288.9 288.6 288.4 288.3 288.1 287.9
4.00 3.45 2.84 2.22 1.70 1.25 4.55 3.87 3.38 2.84 2.28 1.74 1.17 3.33 2.87 2.35 2.02 1.68 1.24
0.1
290.2 289.3 288.1 286.8 285.3 283.4 292.5 291.8 290.8 289.9 288.7 286.8 284.6 293.1 292.5 291.5 290.8 289.3 287.9 285.8
9.26 7.42 5.71 4.04 2.78 1.64 9.78 8.42 6.78 5.43 3.98 2.39 1.07 9.90 8.27 6.73 5.50 3.96 2.62 1.30
0.20
0.30
0.2
0.3
a
u(T) = 0.1 K, u(P) = 0.005 MPa. a
Table 4. Semi-Clathrate Hydrate Dissociation Conditions (H−Lw−V) for the CO2 + TBAF + Water Systemsa mass fraction of TBAF
T/K
P/MPa
0.041
285.8 286.7 287.5 287.9 288.3 288.8 289.3 289.7 291.6 292.2 292.9 293.3
0.68 1.15 1.80 2.11 2.40 3.05 3.53 4.05 2.48 3.12 4.04 4.93
0.067
u(T) = 0.1 K, u(P) = 0.005 MPa.
Table 6. Semi-Clathrate Hydrate Dissociation Conditions (H−Lw−V) for the (Ar + TBANO3 + H2O) Systema mass fraction of TBANO3
T/K
P/MPa
0.05
282.1 281.2 280.1 278.9 277.6 285.3 283.9 282.0 280.2 283.3 286.3 285.3 284.6 283.4 282.0 280.0 278.4
9.56 8.10 6.56 5.13 3.75 9.50 7.34 5.16 3.79 6.77 9.20 7.74 7.03 5.38 3.89 2.35 1.22
0.1
0.2
a
u(T) = 0.1 K, u(P) = 0.005 MPa.
moderate conditions (low pressures and high temperatures) when compared with the pure Ar hydrate. It can be observed that, by increasing the concentration of TBPB, the promotion effect of TBPB on argon hydrate increases dramatically. The presence of TBANO3 leads to the dissociation conditions of the Ar + TBANO3 + water system shift to low pressure and high temperature (Figure 5). The phase equilibrium curves of Ar + TBANO3 + water have a same trend with the phase equilibrium curve of Ar + TBPB + water but the semi-clathrate hydrates of Ar + TBANO3 + water form at the lower temperature. As can be seen in Figure 5, by increasing the concentration of TBANO3, the promotion effect of TBANO3 increases and the phase equilibrium curve shifts to the low pressure and high temperature. The experimental and literature phase equilibrium data for systems of Ar + TBPB + water, Ar + TBANO3 + water, Ar + TBAB + water, and Ar + TBAC + water are plotted and compared in Figure 6. To the best of the author’s knowledge, no data exist in the literature for Ar + TBPB + water at TBPB concentrations greater than 0.2 mass fraction. It is observed
a
u(T) = 0.1 K, u(P) = 0.005 MPa.
that the effect of TBPB on argon hydrate is the same as the effect of TBAB (as shown in both plots a and b). According to Figure 6, TBANO3 has a reduced promotion effect on argon hydrate in comparison with other salts. TBAC shows a strong promotion effect on argon hydrate by increasing the equilibrium temperature and decreasing the hydrate equilibrium pressure. As can be seen in Figure 6b, the isobaric dissociation temperatures of the Ar + TBANO3 (a), Ar + TBPB (b), Ar + TBAB (c), and Ar + TBAC (d) hydrates increase as Td > Tc = Tb > Ta. The results obtained in this study indicate that TBPB has a greater promotion effect on Ar hydrate than methane and CO2 hydrates. In the present study, the effect of addition of CP on hydrate dissociation condition of methane/CO2 + TBAB aqueous 2545
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Figure 4. Hydrate dissociation conditions for the (Ar + TBPB + H2O) system: *, pure Ar hydrate, ref 61; ■, 0.10 mass fraction, this work; ●, 0.20 mass fraction, this work; ▲, 0.30 mass fraction, this work.
Figure 6. Comparison of semi-clathrate hydrate dissociation conditions of the argon in the presence of different salts at specified concentration. Symbols represent experimental data: (a); ■, argon + TBANO3 (0.10 mass fraction), this work; ●, argon + TBPB (0.10 mass fraction), this work; ▲, argon + TBAB (0.10 mass fraction), ref 61. (b); ■, argon + TBANO3 (0.20 mass fraction), this work; ●, argon + TBPB (0.20 mass fraction), this work; ▲, argon + TBAB (0.20 mass fraction), ref 61; ⧫, argon + TBAC (0.20 mass fraction), ref 62.
Figure 5. Hydrate dissociation conditions for the (Ar + TBANO3 + H2O) system: *, pure Ar hydrate, ref 61; ■, 0.05 mass fraction, this work; ●, 0.10 mass fraction, this work; ▲, 0.20 mass fraction, this work.
Table 7. Semi-Clathrate Hydrate Dissociation Conditions (H−Lw−LCP−V) for the (CO2 + TBAB + 5 mL CP + H2O) Systema
solution with two different concentrations of 0.05 and 0.30 mass fractions of TBAB was also investigated. The results are depicted in Tables 7 and 8 as well as Figures 7 and 8. It is observed that the addition of CP to 0.05 mass fraction of TBAB aqueous solution promotes the hydrate dissociation condition for CO2 and CH4 significantly. However, as observed in Figures 7 and 8 for CO2 hydrate in the presence of CP, increasing TBAB mass fraction from 0.05 to 0.3 results in a slight shift of the phase equilibrium curve to the left. In the case of CH4 hydrate, in the presence of 0.3 mass fraction of TBAB, a significant shift of the phase equilibrium to the left was observed. As depicted in Figure 8 for CO2 hydrate, comparing the data for 0.25 mass fraction of TBAB and 0.3 mass fraction of TBAB + CP, no significant change in the hydrate-phase equilibrium conditions was observed which can be explained by the fact that CP molecules most likely did not participate in hydrate formation. In order to compare the promotion effect of the promoters investigated in this study and those in the literature, hydrate dissociation data of methane in the presence of TBPB and TBAF are also depicted in Figure 7. One can observe in Figure 8 that the effect of TBAB concentration on CO2 hydrate-phase equilibrium is
b
mass fraction of TBAB
T/K
P/MPa
0.05
282.73 285.46 287.55 289.34 290.51 291.22 291.64 290.30 289.68 288.94 287.87 286.14 290.88 285.50 290.30
0.307 0.659 1.112 1.649 2.198 2.689 2.959 2.515 2.105 1.699 1.225 0.682 3.062 0.379 2.515
0.30
a
u(T) = 0.1 K, u(P) = 0.005 MPa. bCP free mass fraction basis.
similar for the concentrations of 0.05 and 0.5 mass fractions of TBAB. 2546
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CONCLUSIONS Experimental hydrate dissociation conditions for the semiclathrate hydrates of carbon dioxide + aqueous solutions of TBAA and TBAF, argon + aqueous solutions of TBPB and TBANO3, carbon dioxide + aqueous solutions of TBAB + CP, and methane + aqueous solutions of TBAB + CP are reported herein. An isochoric pressure-search method was used to perform the measurements.56 There is satisfactory agreement between our experimental data and the literature data. The comparison of the hydrate dissociation data for the aforementioned systems with the CO2/Ar + water system shows that TBAA, TBAF, TBPB, and TBANO3 can enlarge the hydrate stability zone for the studied gases. For CO2 and CH4, the addition of CP to 0.05 mass fraction of TBAB aqueous solution promotes the hydrate dissociation condition significantly. For 0.25 and 0.30 mass fraction of TBAB aqueous solutions, different behaviors can be observed: In the case of CO2 hydrate (0.25 TBAB mass fraction), no change in the hydrate dissociation conditions was observed, while for the CH4 hydrate (0.3 TBAB mass fraction), the addition of CP results in a slight shift of the phase equilibrium curve to the right.
Table 8. Semi-Clathrate Hydrate Dissociation Conditions (H−Lw−LCP−V) for the (CH4 + TBAB +5 mL CP + H2O) systema b
Mass fraction of TBAB
T (K)
P (MPa)
0.05
286.93 290.34 293.65 296.79 298.26 299.68 300.72 301.59 302.27 303.07 291.81 297.90 299.28 300.06
0.559 1.057 1.937 3.111 4.014 5.083 5.954 6.779 7.722 8.063 2.620 6.336 7.809 8.956
0.30
Article
a
u(T) = 0.1 K, u(P) = 0.005 MPa. bCP-based free mass fractions.
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AUTHOR INFORMATION
Corresponding Author
*E-mail:
[email protected]. ORCID
Hamed Hashemi: 0000-0003-1986-6923 Deresh Ramjugernath: 0000-0003-3447-7846 Funding
This work is based upon the research supported by the South African Research Chairs Initiative (SARChI) of the Department of Science and Technology and National Research Foundation (grant number: 64817). The authors would also like to thank the National Research Foundation of South Africa (NRF) for financial assistance.
Figure 7. Hydrate dissociation conditions for: ▲ and ◊, pure CH4 hydrate, refs 63,64, (CH4 + TBAB/TBPB/TBAF + H2O): ■, 0.05 mass fraction TBAB ref 63; ×, 0.05 mass fraction TBPB ref 65; ―, 0.05 mass fraction TBAF ref 58; •, 0.3 mass fraction TBAB ref 66; (CH4 + TBAB + CP + H2O) ○, 0.05 TBAB mass fraction + 5 mL CP, this work; *, 0.30 TBAB mass fraction + 5 mL CP this work.
Notes
The authors declare no competing financial interest.
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REFERENCES
(1) Sloan, E. D., Jr. Fundamental principles and applications of natural gas hydrates. Nature 2003, 426, 353−359. (2) Sloan, E. D. Clathrate Hydrates of Natural Gases, 3rd ed.; Marcel Dekker: 2008. (3) Sloan, E. D. Clathrate Hydrates of Natural Gases, 3rd ed.; CRC Press: Florida, USA, 2008 (4) Fowler, D. L.; Loebenstein, W. V.; Pall, D. B.; Kraus, C. A. Some Unusual Hydrates of Quaternary Ammonium Salts. J. Am. Chem. Soc. 1940, 62, 1140−1142. (5) Jeffrey, G. A. Hydrate inclusion compounds. J. Inclusion Phenom. 1984, 1, 211−222. (6) Li, X.-S.; Xu, C.-G.; Chen, Z.-Y.; Wu, H.-J. Tetra-n-butyl ammonium bromide semi-clathrate hydrate process for postcombustion capture of carbon dioxide in the presence of dodecyl trimethyl ammonium chloride. Energy 2010, 35, 3902−3908. (7) Sun, Z.-G.; Liu, C.-G.; Zhou, B.; Xu, L.-Z. Phase Equilibrium and Latent Heat of Tetra-n-butylammonium Chloride Semi-Clathrate Hydrate. J. Chem. Eng. Data 2011, 56, 3416−3418. (8) Sun, Z.-G.; Liu, C.-G. Equilibrium Conditions of Methane in Semiclathrate Hydrates of Tetra-n-butylammonium Chloride. J. Chem. Eng. Data 2012, 57, 978−981. (9) Chapoy, A.; Anderson, R.; Tohidi, B. Low-pressure molecular hydrogen storage in semi-clathrate hydrates of quaternary ammonium compounds. J. Am. Chem. Soc. 2007, 129, 746−747.
Figure 8. Hydrate dissociation conditions for: ⧫, CO2 in pure water, ref 67; (CO2 + TBAB + H2O): *, 0.05 mass fraction ref 68; -, 0.5 mass fraction ref 68; ▲, 0.0701 mass fraction ref 69; □, 0.25 mass fraction ref 68; (CO2 + TBAB + CP + H2O): ●, 0.05 TBAB mass fraction + 5 mL CP, this work; +, 0.30 TBAB mass fraction + 5 mL CP, this work. 2547
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DOI: 10.1021/acs.jced.8b01195 J. Chem. Eng. Data 2019, 64, 2542−2549
