Solubility and thermodynamic properties of SO 2  in three low volatile urea derivatives

Jiang, Yaotai; Liu, Xiaobang; Deng, Dongshun

doi:10.1016/j.jct.2016.05.004

Cited by 18 publications

(7 citation statements)

References 31 publications

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“…The physical absorption and chemical absorption part were described, respectively, by Henry's law (Equation ()) and the reaction equilibrium (Equation ()):

P goodbreak= H_{m} γ {SO}_{2} ((), \frac{m_{{SO}_{2}}}{m})

K^{0} goodbreak= \frac{γ {SO}_{2} IL ((), \frac{m_{{SO}_{2} IL}}{m})}{\frac{P}{P^{0}} γ IL ((), \frac{m_{IL}}{m})}

The relationship equation between the total solubility of SO 2 in PIL and the partial pressure of SO 2 is similar to that reported in the literature 40,44 . Henry's constant ( H m ) and reaction equilibrium constant ( K 0 ) were obtained by fitting Equation () to Figure 5 for the two absorbents at different temperatures, and the fitted correlation coefficient R 2 > 0.99.

normalm t goodbreak= m {IL}_{0} \frac{K^{0} P}{K^{0} P + 1} goodbreak+ \frac{P}{Hm}

m {IL}_{0} goodbreak= \frac{10^{3}}{M_{IL}}

Table 3 summarizes the absorption thermodynamic parameters K 0 and H m for SO 2 absorption in TMEA and [TMEA][Im].…”

Section: Resultssupporting

confidence: 63%

“…Thermodynamic properties can contribute to the understanding of the dissolution process of SO 2 in absorbents. Fitting the adsorption isotherm in Figure 5 with the reaction equilibrium thermodynamic model, the Henry's constant and the reaction equilibrium constant of SO 2 absorption at different temperatures can be fitted 38,44 . From the above conclusion, the absorption of SO 2 was divided into a physical absorption part and a chemical absorption part, which can be expressed by the following Equations () and ():

{SO}_{2} ((), g) \to {SO}_{2} ((), L)

{SO}_{2} ((), g) goodbreak+ IL ((), L) \to {SO}_{2} IL ((), L)

…”

Section: Resultsmentioning

confidence: 98%

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Effective absorption of SO₂ by imidazole‐based protic ionic liquids with multiple active sites: Thermodynamic and mechanical studies

et al. 2022

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In view of the environmental hazards caused by SO2, the development of efficient SO2 capture technology has important practical significance. In this work, a low‐viscosity protic ionic liquids containing imidazole (Im), ether linkage, and tertiary amine structure was synthesized by acid–base neutralization of tris(3,6‐dioxaheptyl)amine (TMEA) and Im for SO2 absorption. The results showed that the solubility of SO2 in [TMEA][Im] reached 12.754 mol kg−1 at 298.2 K and 1 bar and the ideal selectivity of SO2/CO2 (1/1) is 141.7 at 1 bar. Furthermore, [TMEA][Im] can be reused and the SO2 absorption performance was not significantly reduced after five cycles. In addition, the absorption of low‐concentration SO2 (2000 ppm) in [TMEA][Im] was also tested. Further spectroscopic research and thermodynamic analysis suggested that the high SO2 uptake by [TMEA][Im] was caused by the synergistic effect of physical and chemical absorption.

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“…The physical absorption and chemical absorption part were described, respectively, by Henry's law (Equation ()) and the reaction equilibrium (Equation ()):

P goodbreak= H_{m} γ {SO}_{2} ((), \frac{m_{{SO}_{2}}}{m})

K^{0} goodbreak= \frac{γ {SO}_{2} IL ((), \frac{m_{{SO}_{2} IL}}{m})}{\frac{P}{P^{0}} γ IL ((), \frac{m_{IL}}{m})}

normalm t goodbreak= m {IL}_{0} \frac{K^{0} P}{K^{0} P + 1} goodbreak+ \frac{P}{Hm}

m {IL}_{0} goodbreak= \frac{10^{3}}{M_{IL}}

Table 3 summarizes the absorption thermodynamic parameters K 0 and H m for SO 2 absorption in TMEA and [TMEA][Im].…”

Section: Resultssupporting

confidence: 63%

{SO}_{2} ((), g) \to {SO}_{2} ((), L)

{SO}_{2} ((), g) goodbreak+ IL ((), L) \to {SO}_{2} IL ((), L)

…”

Section: Resultsmentioning

confidence: 98%

Effective absorption of SO₂ by imidazole‐based protic ionic liquids with multiple active sites: Thermodynamic and mechanical studies

et al. 2022

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“…Therefore, the activity coefficient γ is regarded as 1. Part of the derivation process is similar to Huang and Deng et al Finally, a simple derivation yields eq , in which the Henry constant of absorption and the reaction equilibrium constant can be obtained by fitting the isotherm. The fitted results are recorded in Table . On the basis of the calculated results, the equilibrium constant K 0 of SO 2 in [TMEA][MOAc] is larger than those of the remaining three PILs, while the Henry constant H m of [TMEA][MOAc] is the smallest, indicating that [TMEA][MOAc] is the strongest for both chemical and physical affinities of SO 2 .…”

Section: Results and Discussionmentioning

confidence: 99%

“…Here, Δ phy H m can be obtained by fitting ln H m and 1/ T according to eq , , and the fitted curves are shown in Figure S6. Δ chem H m was calculated according to eq As shown in Table , the negative values of Δ phy H m mean that the physical absorption of SO 2 in PILs is also an exothermic process. Particularly, in [TMEA][MOAC], Δ phy H m and Δ chem H m are −37.434 and −17.191 kJ·mol –1 , respectively, which more clearly indicates that physical absorption captures SO 2 better than chemical absorption.…”

Section: Results and Discussionmentioning

confidence: 99%

Rich Ether-Based Protic Ionic Liquids with Low Viscosity for Selective Absorption of SO₂ through Multisite Interaction

Liu

Cai

Zhang

et al. 2022

Ind. Eng. Chem. Res.

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Four low-viscosity protic ionic liquids (PILs) with the tertiary amine and rich ether skeletons are designed for selective absorption of SO2. To evaluate the selective absorption of SO2 by these PILs, the solubilities of SO2, CO2, and H2S are measured in the temperature range of 303.2–333.2 K and pressures up to 120 kPa by a volumetric method, respectively. The absorption of SO2 by [TMEA][MOAc] at 303.2 K and 101.3 kPa was found to be 10.424 mol·kg–1 (4.310 mol·mol–1), and the ideal selectivity of SO2/CO2 was 86.83. In addition, the solubility data are fitted using a reaction equilibrium thermodynamic model to obtain thermodynamics parameters including Gibbs free energy change (Δr G m), enthalpy change (Δr H m, Δphy H m, Δchem H m), and entropy change (Δr S m). The mechanism of SO2 absorption by [TMEA][MOAc] is also investigated by FTIR and NMR analyses. Mechanistic and thermodynamic studies suggest that the high SO2 absorption is attributed to the O–SO2 multisite physical interaction. These ether-rich PILs are considered as a promising absorber because of their high SO2 solubility, good cycling performance, and low viscosity before and after absorption.

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“…Nowadays, many new substances and materials have been studied to capture SO 2 from flue gas such as organic solvents, − deep eutectic solvents (DESs), metal–organic frameworks (MOFs), supported ionic liquid phase materials, , etc. However, the practical utilization of these are subject to secondary pollution, high cost of the operation processes, unknown toxicity, loss of structural integrity, limited reusability of the absorbents, and so on.…”

Section: Introductionmentioning

confidence: 99%

Absorption of SO₂ in Furoate Ionic Liquids/PEG200 Mixtures and Thermodynamic Analysis

2018

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Carboxylate ionic liquid (IL) and polyethylene glycol 200 (PEG200) mixtures are suitable for the absorption of acidic SO2 because of their unique properties. In the present work, tetraethylammonium furoate ([N2222][FA]) and choline furoate ([Ch][FA]) were blended with PEG200 to form 40 wt % ILs/PEG200 mixtures as SO2 absorbents. The solubilities of SO2 in these two ILs/PEG200 mixtures were measured at T = (303.15, 313.15, 323.15, and 333.15) K and pressure up to 1.2 bar. [N2222][FA]/PEG200 demonstrated the high SO2 absorption capacity of 7.224 mol per kg absorbent at 303.15 K and 1.0 bar. The chemisorption mechanism of SO2 by mixture was studied by Fourier transform infrared and nuclear magnetic resonance spectra, and the influence of cations on the SO2 absorption capacity was analyzed. Furthermore, the reaction equilibrium thermodynamic model was used to correlate the experimental data, and Henry’s law constant (H), reaction equilibrium constant (K 0), and thermodynamic properties (Δr G m 0, Δr H m 0, and Δr S m 0) were derived. The absorption enthalpies of the two binary mixtures are −46.39 and −23.07 kJ·mol–1 for the two mixtures, respectively. Considering the low cost, biodegradability of the materials, high capacity, and low absorption enthalpy, the [N2222][FA]/PEG200 mixture was regarded to be an attractive and promising alternative to pure ILs and ordinary solvent as a desulfurizer.

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Solubility and thermodynamic properties of SO 2 in three low volatile urea derivatives

Cited by 18 publications

References 31 publications

Effective absorption of SO₂ by imidazole‐based protic ionic liquids with multiple active sites: Thermodynamic and mechanical studies

Effective absorption of SO₂ by imidazole‐based protic ionic liquids with multiple active sites: Thermodynamic and mechanical studies

Rich Ether-Based Protic Ionic Liquids with Low Viscosity for Selective Absorption of SO₂ through Multisite Interaction

Absorption of SO₂ in Furoate Ionic Liquids/PEG200 Mixtures and Thermodynamic Analysis

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Solubility and thermodynamic properties of SO 2 in three low volatile urea derivatives

Cited by 18 publications

References 31 publications

Effective absorption of SO2 by imidazole‐based protic ionic liquids with multiple active sites: Thermodynamic and mechanical studies

Effective absorption of SO2 by imidazole‐based protic ionic liquids with multiple active sites: Thermodynamic and mechanical studies

Rich Ether-Based Protic Ionic Liquids with Low Viscosity for Selective Absorption of SO2 through Multisite Interaction

Absorption of SO2 in Furoate Ionic Liquids/PEG200 Mixtures and Thermodynamic Analysis

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Resources

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Effective absorption of SO₂ by imidazole‐based protic ionic liquids with multiple active sites: Thermodynamic and mechanical studies

Effective absorption of SO₂ by imidazole‐based protic ionic liquids with multiple active sites: Thermodynamic and mechanical studies

Rich Ether-Based Protic Ionic Liquids with Low Viscosity for Selective Absorption of SO₂ through Multisite Interaction

Absorption of SO₂ in Furoate Ionic Liquids/PEG200 Mixtures and Thermodynamic Analysis