Silver-Functionalized Ionic Liquid@MCM-41 Adsorbents for C₂H₄/C₂H₆ Separation

Abstract

Ionic liquids (ILs) have attracted considerable attention for light olefin separation owing to their negligible vapor pressure, excellent thermal stability, and tunable molecular structures. However, their intrinsically high viscosity severely restricts gas diffusion, leading to poor mass-transfer efficiency and limited separation performance in bulk form. Herein, we report the develop a high-performance adsorbent by immobilizing a silver-functionalized ionic liquid within ordered mesoporous MCM-41 to overcome the diffusion limitations of bulk ILs. The IL@MCM-41 composites were prepared via an impregnation–evaporation strategy, and their mesostructural integrity and textural evolution were confirmed by XRD and N₂ sorption analyses. Their C₂H₄/C₂H₆ separation performance was subsequently evaluated. The composite with a 70 wt% IL loading achieves a high C₂H₄ uptake of 25.68 mg/g and a C₂H₄/C₂H₆ selectivity of 15.59 in breakthrough experiments (298 K, 100 kPa). X-ray photoelectron spectroscopy results are consistent with the presence of reversible Ag⁺–π interactions, which governs the selective adsorption of C₂H₄. Additionally, the composite exhibits excellent thermal stability (up to 570 K) and maintains stable separation performance over 10 adsorption–desorption cycles. These IL@MCM-41 composites have significant potential for designing sorbent materials for efficient olefin/paraffin separation applications.

1. Introduction

The separation of C₂H₄ and C₂H₆ is critically important in the petrochemical industry. C₂H₄ serves as a key feedstock for producing polyethylene, ethanol, ethylbenzene, dichloroethane, and ethylene oxide, and various other essential industrial chemicals [1,2]. C₂H₆, in addition to being a crucial precursor for ethylene cracking, is also used in the synthesis of acetic acid, halogenated hydrocarbons, and other high-value chemicals, thereby playing a pivotal role in modern petrochemical value chains [3,4]. However, separating C₂H₄ from C₂H₆ remains inherently challenging due to their remarkably similar molecular sizes, polarities, and boiling points [5]. Conventional separation techniques, including cryogenic distillation, membrane separation, and adsorption, each present significant limitations [6,7,8,9]. Cryogenic distillation is highly energy-intensive and requires substantial capital investment, which considerably restricts its industrial applicability [10,11]. Membrane-based methods often suffer from insufficient selectivity, a trade-off between flux and purity, and stability issues, making it difficult to obtain high-purity C₂H₄.

Compared with distillation and membrane-based processes, adsorption provides several distinct advantages for C₂H₄/C₂H₆ separation, including mild operating conditions, lower energy consumption, and tunable host–guest interactions. These features make adsorption a promising alternative for efficiently separating molecules with similar physical properties. As a result, the development of high-performance adsorbent materials capable of selectively distinguishing between C₂H₄ and C₂H₆ has become an active research focus in recent years. Wang et al. constructed a series of π-conjugated microporous polyaminal networks (PAN-P, PAN-NA and PAN-AN), where strengthened C–H···π interactions with C₂H₆ in ultramicropores (∼0.55–1.1 nm) led to a C₂H₆ uptake of 2.38 mmol/g and a C₂H₆/C₂H₄ IAST selectivity of 1.68 at 298 K and 1 bar, as well as a breakthrough selectivity of 2.70 for a C₂H₆/C₂H₄ = 5/95 mixture at 298 K [12]. Min et al. developed Ag-exchanged ZK-5 zeolites [Ag-ZK-5(II), Si/Al = 3.7], in which Ag⁺–π complexation with C₂H₄ inside KFI cages yielded an equilibrium C₂H₄/C₂H₆ selectivity of 2.54 at 298 K under vacuum-swing adsorption conditions and effective separation of a C₂H₄/C₂H₆/Ar (25:25:50 v/v/v) stream in breakthrough experiments at 298 K [13]. Chen et al. reported an Fe-based MOF MIL-142A, where stronger van der Waals interactions and higher adsorption heat for C₂H₆ over C₂H₄ enabled a C₂H₆ uptake of 3.8 mmol/g and a C₂H₆/C₂H₄ IAST selectivity of 1.5 at 298 K and 100 kPa, together with a dynamic selectivity of 1.8 for an equimolar C₂H₆/C₂H₄ mixture at 298 K and 1 atm [14]. Wang et al. synthesized a Ag-decorated Hf MOF NUS-6(Hf)-Ag, where Ag⁺ sites anchored by sulfonic acid groups form π*–d complexes with C₂H₄, giving a C₂H₄ uptake of 2.02 mmol/g at 298 K and 105.8 kPa and an IAST C₂H₄/C₂H₆ selectivity of 6.0 at 298 K and 100 kPa (106 at 1 kPa), as well as a co-adsorption selectivity of 4.4 for an equimolar C₂H₄/C₂H₆ mixture in breakthrough tests at 298 K and 1 atm with excellent cycling stability [15]. However, despite substantial progress in adsorbent design, the majority of reported materials continue to exhibit insufficient C₂H₄/C₂H₆ selectivity.

Ionic liquids (ILs) have attracted substantial attention for light olefin separations owing to their near-zero vapor pressure, excellent thermal stability, and highly tunable cation–anion structures [16,17,18]. ILs exhibit high gas solubility, and their affinity toward C₂H₄ can be finely tuned through the rational selection of cations and anions [19,20]. Silver-ion-mediated olefin/paraffin separation has also been demonstrated in liquid-phase-facilitated transport configurations. For example, aqueous AgNO₃ solutions were employed in gas–liquid membrane contactors for C₂H₄/C₂H₆ separation, where the separation performance was strongly dependent on the Ag⁺ concentration and operating flow conditions, highlighting the effectiveness of reversible Ag⁺–olefin complexation [21]. Several IL-based systems have demonstrated substantial potential for C₂H₄/C₂H₆ separation. Ren et al. synthesized a silver salt-containing IL, where synergistic interactions between Ag⁺–π coordination and strong hydrogen bonding between ethylene glycol and BF₄⁻ significantly enhanced C₂H₄ uptake and selectivity, achieving a C₂H₄ solubility of 6.0 mol L⁻¹ and a selectivity of 8.57 at 298.15 K and 1.0 bar [22]. Cheng et al. developed an Er³⁺-containing IL mixture ([Bmim][TFO]/Er(TFO)₃ + DMF), where selective coordination between C₂H₄ and the 4f/5d vacant orbitals of Er³⁺ resulted in a selectivity of 10 and excellent cycling stability [23]. Xing et al. introduced dual-nitrile groups symmetrically on an imidazolium cation to obtain a dual-CN-functionalized IL, [(CP)₂im][NTf₂], where dipole–quadrupole interactions suppressed C₂H₆ solubility. Upon the addition of AgNTf₂, the C₂H₄ selectivity increased to 10.7 [24]. Wu et al. prepared a protic imidazolium IL containing Ag⁺, [Bim]_1.5[Ag(NTf₂)_2.5], where reversible π-complexation between Ag⁺ and C₂H₄ contributed to exceptional selectivity (41.2 at 303 K and 0.2 MPa) and high C₂H₄ solubility (1.86 mol C₂H₄ mol⁻¹ Ag⁺) [25]. Despite these advantages, bulk ILs inherently suffer from high viscosity, which leads to the formation of thick liquid films, reduced gas–liquid interfacial area, and restricted molecular diffusion [26]. These factors collectively suppress mass-transfer efficiency and severely limit the practical separation performance of IL-based systems [27,28].

To overcome the mass-transfer limitations inherent to bulk ILs, researchers have increasingly explored immobilizing ILs onto porous solid matrices. Such porous supports—with high surface areas and well-defined pore architectures—can effectively disperse ILs, enlarge the gas–liquid interfacial area, and facilitate molecular diffusion. Previous studies have demonstrated that IL-modified mesoporous materials can generate highly polar microenvironments that significantly enhance gas adsorption capacity and selectivity [29]. Ionogel systems with low IL loadings have also shown rapid adsorption kinetics and excellent cyclic stability [30]. Recent computational and experimental studies have demonstrated that incorporating ionic liquids into porous frameworks (e.g., IL@MOFs) can effectively tune gas affinities and separation performance by combining the selective interactions of ILs with the transport advantages of porous materials [31]. From a theoretical standpoint, first-principles calculations have been extensively employed to elucidate gas–surface interactions in silica-based materials and to clarify how variations in local coordination environments and heteroatom incorporation influence adsorption energetics and electronic structures. For instance, density functional theory investigations on undoped and doped silica surfaces have demonstrated that gas adsorption and dopant incorporation can markedly modify adsorption strengths and the electronic density of states, thereby providing fundamental molecular-level insight into host–guest interactions [32]. Despite these promising advances, most reported systems remain focused on CO₂ capture, whereas systematic investigations of IL-modified porous adsorbents for C₂H₄/C₂H₆ separation have not yet been reported. Moreover, direct mechanistic evidence—particularly regarding Ag⁺–π interactions under confined mesoporous environments—has yet to be comprehensively elucidated. MCM-41, a well-established mesoporous molecular sieve with a highly ordered two-dimensional hexagonal channel system and a large surface area [33,34], serves as an ideal host for IL immobilization.

Herein, we design and synthesize a series of silver-functionalized ionic liquid composites by immobilizing [Emim][BF₄]/AgBF₄ within the ordered mesoporous channels of MCM-41. The structural integrity, pore evolution, thermal stability, and chemical environments of the resulting IL@MCM-41 materials were systematically characterized using XRD, FTIR, N₂ sorption, TGA, SEM/EDS, elemental analysis, and XPS. Furthermore, the influences of IL loading, temperature, pressure, and cycling on C₂H₄ and C₂H₆ adsorption were comprehensively investigated to elucidate the confined Ag⁺–π interaction mechanisms governing selectivity. This work demonstrates how mesoporous confinement and Ag⁺–π complexation synergistically improve ethylene capture, offering design principles for advanced ionic-liquid-based adsorbents for efficient C₂H₄/C₂H₆ separation.

2. Materials and Methods

2.1. Chemicals and Reagents

MCM-41 molecular sieves were purchased from Tianjin Yuanli Chemical Co., Ltd. (Tianjin, China). 1-Ethyl-3-methylimidazolium tetrafluoroborate ([Emim][BF₄], 99%) was obtained from the Lanzhou Institute of Chemical Physics, Chinese Academy of Sciences (Lanzhou, China). Silver tetrafluoroborate (AgBF₄, 99%) and acetonitrile (analytical grade) were supplied by Macklin Biochemical Technology Co., Ltd. (Shanghai, China). All gas samples were provided by Huizhou Southern Huayan Chemical Products Co., Ltd. (Huizhou, China).

2.2. Preparation of IL@MCM-41 Composites

Silver-functionalized ionic liquid-loaded MCM-41 composites were prepared using an impregnation–evaporation method, as schematically illustrated in Figure 1. [Emim][BF₄] was first dried under vacuum at 333.15 K for 12 h. The dried ionic liquid was then mixed with AgBF₄ at a molar ratio of 4:1 and stirred at 298.15 K for 12 h to obtain the Ag⁺-containing ionic liquid [22,25]. The resulting ionic liquid was dissolved in 200 mL of anhydrous acetonitrile and magnetically stirred until a homogeneous solution was formed.

Separately, MCM-41 was dried at 120 °C to constant weight and subsequently added to the ionic-liquid solution to achieve IL loadings of 30–70 wt%. The suspension was stirred using a rotary evaporator (Zhengzhou Greatwall Scientific Industrial and Trade Co., Ltd., Zhengzhou, China) at 80 rpm for 12 h to facilitate infiltration of the ionic liquid into the mesoporous channels. After impregnation, acetonitrile was removed under reduced pressure at 358.15 K, followed by vacuum drying at 378.15 K for 24 h. The resulting samples were denoted as x wt% IL@MCM-41 (x = 30, 40, 50, 60, 70).

2.3. Characterization Methods of IL@MCM-41 Composites

All IL@MCM-41 samples were vacuum-dried at 333 K for 48 h prior to characterization. Small-angle X-ray diffraction (XRD) measurements were performed using a Rigaku SmartLab diffractometer (Rigaku Corporation, Akishima, Tokyo, Japan) over a 0.5–10° (2θ) range to evaluate pore ordering and mesostructural integrity. N₂ adsorption–desorption isotherms were measured using an Autosorb-iQ-XR analyzer (Anton Paar QuantaTec Inc., Boynton Beach, FL, USA), and the Brunauer–Emmett–Teller (BET) method and density functional theory (DFT) were used to determine specific surface areas and pore-size distributions. Fourier-transform infrared (FTIR) spectra were recorded on a Thermo Nicolet iS50 spectrometer (Thermo Fisher Scientific Inc., Waltham, MA, USA) in the range of 4000–400 cm⁻¹ to identify functional groups and confirm IL incorporation. Thermogravimetric analysis (TGA, Mettler-Toledo AG, Greifensee, Zurich, Switzerland) was carried out under a N₂ atmosphere at a heating rate of 10 K min⁻¹ from room temperature to 1273 K to evaluate the thermal stability of the composites. Scanning electron microscopy (SEM, Carl Zeiss Microscopy GmbH, Oberkochen, Germany) and energy-dispersive X-ray spectroscopy (EDS, Oxford Instruments plc, Abingdon, Oxfordshire, UK) were used to examine particle morphology and elemental distributions. X-ray photoelectron spectroscopy (XPS, Thermo Fisher Scientific Inc., Waltham, MA, USA) was performed to analyze chemical states and surface composition. Elemental analysis was conducted to determine the nitrogen content, enabling the calculation of actual IL loadings in the composites.

2.4. Determining Adsorption of Ethylene and Ethane on IL@MCM-41

Static adsorption isotherms of C₂H₄ and C₂H₆ were measured using an Autosorb-iQ-XR analyzer. Pure-component adsorption isotherms were measured volumetrically by stepwise dosing of gas to the desired pressure. The effect of temperature on C₂H₄ adsorption was investigated by varying the measurement temperature. High-pressure static adsorption measurements were performed using a quadrupole magnetic suspension balance over a pressure range of 1.0 × 10²–1.9 × 10³ kPa to investigate the pressure-dependent adsorption behavior.

Dynamic breakthrough experiments were conducted using a custom-built fixed-bed setup (schematic shown in Figure 2). IL@MCM-41 samples were packed into a stainless-steel adsorption column with an inner diameter of 7 mm and a length of 200 mm, and tested at 298 K and ambient pressure. The feed gas mixture consisted of C₂H₄/C₂H₆ = 1.02/0.98 (v/v) and was introduced at a total flow rate of 1.0 mL/min. We first measured the system dead volume using blank breakthrough experiments with He as a non-adsorbing tracer (≈7.2–7.3 mL). We then used this value to correct the residence time in all breakthrough curves. This correction was applied before capacity calculations. The corresponding residence time was subtracted from all breakthrough curves prior to data analysis to ensure accurate evaluation of the adsorption capacity. Prior to each adsorption experiment, both the adsorption column and the dummy column were thoroughly purged with He until a stable baseline was obtained. Breakthrough curves were recorded upon switching the inlet gas from He to the C₂H₄/C₂H₆ mixture, and the outlet gas composition was continuously monitored using an Agilent 8890 gas chromatograph (Agilent Technologies, Inc., Santa Clara, CA, USA) equipped with a TCD detector.

The breakthrough time was defined as the point at which the outlet gas concentration reached 5% of the inlet concentration, while the saturation point was defined as 95% of the inlet concentration. After each run, the adsorbent was regenerated by purging with He. Five adsorption–desorption cycles were conducted for each sample to evaluate cyclic stability. In addition, the optimal 70 wt% IL@MCM-41 sample was further subjected to ten consecutive cycles. Adsorption capacities and selectivities were calculated from material balance relationships using the inlet and outlet gas compositions and flow rates, as expressed in Equations (1) and (2) [35]:

$$n_i={\int }_0^t{\displaystyle \frac{p_1·V_{in}·y_i^0}{\mathrm{R}T}}dt-{\int }_0^t{\displaystyle \frac{p_2·V_{out}·y_i}{\mathrm{R}T}}dt-{\displaystyle \frac{p{V}_0{y}_i^0}{\mathrm{R}T}}$$

(1)

$$S_{a/b}={\displaystyle \frac{n_a}{n_b}}$$

(2)

where n_i is the equilibrium adsorption amount (mol); p₁ and p₂ are the inlet and outlet pressures (Pa); V_in and V_out are volumetric flow rates (m³/s); y_i⁰ and y_i are inlet and outlet volume fractions; V₀ is the system dead volume (m³); R is the gas constant (8.314 J/mol/K⁻); and T is the temperature (K).

3. Results and Discussion

3.1. Characterization and Properties of IL@MCM-41 Composites

Small-angle XRD patterns of pristine MCM-41 and IL@MCM-41 composites are shown in Figure 3. The parent MCM-41 exhibits a distinct (100) diffraction peak at 2θ ≈ 2.3°. This peak is a hallmark of a highly ordered 2D hexagonal mesostructure [33]. Upon incorporation of the ionic liquid, the intensity of the (100) reflection progressively decreases and the peak shifts slightly toward higher angles. Consequently, both the interplanar spacing (d₁₀₀) and lattice parameter (a₀) decrease with increasing IL loading. The shift in the (100) peak toward higher angles suggests partial penetration of the ionic liquid into the mesoporous channels, resulting in slight pore contraction. In the 40 wt% sample, a weak feature appears near 1°. We attribute it to a slight change in mesostructural ordering at intermediate IL loading. It is not due to crystalline impurities or phase separation [34,36,37]. Notably, the incorporation of ILs does not disrupt the periodicity of the mesoporous framework, indicating that the robust Si–O–Si network of MCM-41 effectively resists structural distortion even at high IL loadings [30,38].

Nitrogen adsorption–desorption isotherms and pore-size distributions (Figure 4) reveal substantial changes in the textural properties of the materials upon IL loading, with the corresponding quantitative parameters summarized in

Table 1. BET surface area and pore volume of pristine MCM-41 and IL@MCM-41 composites.

Sample	BET Surface Area (m2/g)	Pore Volume (cm3/g)
MCM-41	1027.43	0.78
30 wt%IL@MCM-41	299.15	0.26
40 wt%IL@MCM-41	34.70	0.07
50 wt%IL@MCM-41	34.34	0.04
60 wt%IL@MCM-41	31.27	0.03
70 wt%IL@MCM-41	31.21	0.03

. Pristine MCM-41 exhibits a high BET surface area (1027.43 m²/g) and a large pore volume (0.78 cm³/g), consistent with typical mesoporous MCM-41 [39]. Its adsorption isotherm displays combined type I/IV features with a pronounced H1 hysteresis loop, indicative of a uniform mesoporous structure [40]. As the IL loading increases, both the BET surface area and pore volume decrease sharply—dropping to 299.15 m²/g at 30 wt% IL loading and further to approximately 33 m²/g at loadings ≥ 70 wt%. Correspondingly, the hysteresis loop nearly disappears and the pore-size distributions become significantly flattened, indicating that the IL progressively occupies the mesoporous channels. The BET surface area and pore volume decrease sharply with increasing IL loading. This trend suggests that the IL progressively occupies the mesopores and limits N₂ access. The absence of a separate phase also implies good IL dispersion within the framework [41]. The progressive reduction in accessible pore volume indicates that a larger fraction of Ag⁺ sites becomes confined within narrower pore spaces, thereby increasing their effective accessibility to C₂H₄ molecules and contributing to the enhanced adsorption capacity.

Elemental analysis was employed to quantify the actual IL loadings in the IL@MCM-41 composites. Since pristine MCM-41 contains no nitrogen, whereas [Emim][BF₄] contains nitrogen within the imidazolium cation, the nitrogen content detected in each composite directly reflects the amount of ionic liquid incorporated. Based on the measured nitrogen contents, the mass fractions of IL in the IL@MCM-41 composites were calculated, and the results are summarized in

Table 2. Elemental analysis results of pristine MCM-41 and IL@MCM-41 composites.

Sample	N (wt%)		IL (wt%)
	Theoretical	Measured	Theoretical	Measured
MCM-41	0.00	0.00	0.00	0.00
30 wt%IL@MCM-41	3.41	3.27	30	28.76
40 wt%IL@MCM-41	4.54	4.03	40	35.50
50 wt%IL@MCM-41	5.68	5.41	50	47.62
60 wt%IL@MCM-41	6.81	6.61	60	58.24
70 wt%IL@MCM-41	7.95	7.36	70	64.79

. For all samples, the experimentally determined IL loadings agreed well with the theoretical values, with deviations within 15%. This discrepancy is mainly attributed to a portion of the ionic liquid remaining adhered to the container walls.

Figure 5 shows the FTIR spectra of pristine MCM-41 and IL@MCM-41 composites. The IL@MCM-41 samples exhibit several characteristic absorption bands that are absent in pristine MCM-41, including B–F stretching vibrations at 698, 645, and 622 cm⁻¹, as well as imidazolium ring C–H and C=N vibrations at 3123 and 1570 cm⁻¹. Meanwhile, the Si–O–Si asymmetric and symmetric stretching vibrations at approximately 1040 and 800 cm⁻¹ remain essentially unchanged, indicating that IL incorporation does not disrupt the silica framework [42]. No new peaks or significant peak shifts are observed, suggesting the absence of new chemical bonds between the ionic liquid and MCM-41; thus, the ionic liquid is primarily immobilized through physical loading rather than chemical interaction.

SEM images and EDS elemental mapping (Figure 6) reveal a homogeneous distribution of C, N, and F throughout the IL@MCM-41 composite. Compared with pristine MCM-41, the intensities of these elements are significantly enhanced after IL incorporation. The weak C, N, and F signals observed in pristine MCM-41 are mainly attributed to background contamination and instrumental noise inherent to EDS analysis of light elements. The uniform elemental distribution suggests that the ionic liquid is well dispersed within the mesoporous framework without obvious aggregation, which is beneficial for maintaining open diffusion pathways and enabling rapid access of C₂H₄ molecules to the active sites.

TGA curves (Figure 7) show that pristine MCM-41 undergoes minimal mass loss (~2.82%) from room temperature to 1273 K, which is primarily attributed to the desorption of physisorbed moisture. The IL@MCM-41 composites exhibit no significant mass loss below approximately 570 K, indicating that the silver-based ionic liquid is thermally stable within this temperature range and does not undergo noticeable decomposition or volatilization. Therefore, the composites meet the thermal requirements for adsorption–desorption cycling and are suitable for regenerable operation in practical gas-separation processes.

3.2. Effect of IL Loading and Partial Pressure on Adsorption Performance

Adsorption performance of C₂H₄ and C₂H₆ on pristine MCM-41 and IL@MCM-41 composites is shown in Figure 8. The C₂H₄ uptake increases substantially with increasing IL loading. At 100 kPa, the C₂H₄ adsorption capacity rises from 14.45 mg/g at 30.16 wt% IL loading to 30 mg/g at 70 wt%. In sharp contrast, C₂H₆ adsorption remains extremely low (1–2 mg/g), showing minimal dependence on IL loading and even falling below that of pristine MCM-41. This pronounced uptake disparity confirms a strong preferential adsorption of C₂H₄ relative to C₂H₆ in the IL-modified composites.

3.3. Effect of Temperature on Adsorption

Adsorption temperature strongly influences practical separation performance. Therefore, the C₂H₄ adsorption performance of the 70 wt% IL@MCM-41 composite was evaluated at different temperatures, as shown in Figure 9. The adsorption capacity increases as the temperature decreases; when the temperature is reduced from 328.15 K to 298.15 K, the C₂H₄ uptake rises from 17.55 mg/g to 30.16 mg/g. This trend indicates that lower temperatures are more favorable for ethylene adsorption, consistent with the typical behavior of exothermic adsorption processes.

3.4. Effect of Pressure on Adsorption

Pressure is another important parameter governing gas adsorption behavior. As shown in Figure 10, the 70 wt% IL@MCM-41 composite was examined for C₂H₄ and C₂H₆ adsorption over a pressure range of 1–19 bar. The C₂H₄ uptake increases progressively with rising pressure, from 27.72 mg/g at 100 kPa to 36.87 mg/g at 1.9 × 10³ kPa, without reaching a clear saturation limit. This monotonic increase indicates that additional adsorption sites remain available under elevated pressures. In contrast, C₂H₆ uptake remains consistently low across the entire pressure range, reflecting its weak interaction with the composite. Consequently, the disparity between C₂H₄ and C₂H₆ uptakes widens with increasing pressure, clearly showing that higher pressures further reinforce the preferential adsorption of C₂H₄.

3.5. Adsorption Mechanism of IL@MCM-41 Composites

The XPS spectra were employed to probe the chemical states of the adsorbent and to evaluate whether the Ag⁺–π interaction with C₂H₄ remains operative after repeated adsorption–desorption cycling.

Compared with pristine MCM-41, the fresh IL@MCM-41 composite (before cycling) exhibits clear N 1s, F 1s, and Ag 3d signals, along with an intensified C 1s peak originating from the ionic liquid [43]. After adsorption–desorption cycles, the regenerated IL@MCM-41 sample was intentionally re-exposed to C₂H₄ prior to XPS analysis in order to examine whether the Ag⁺–π interaction remains active after cycling. As shown in Figure 11, the C 1s spectrum of the cycled and re-adsorbed sample exhibits a distinct shoulder at 285.14 eV, which can be assigned to C=C (sp²) species, confirming that C₂H₄ can still be effectively adsorbed after prolonged cyclic operation [44]. Meanwhile, the C–N-related peaks shift positively by approximately +0.3 eV, indicating a reduction in local electron density due to interaction with Ag⁺ centers; the N⁺ feature at 401.4 eV also exhibits a slight positive shift of +0.07 eV, consistent with cation–π interactions. In addition, the Ag 3d_5/2 peak shifts from 368.52 eV (fresh IL@MCM-41) to 368.81 eV after re-adsorption of C₂H₄ on the cycled sample, providing direct evidence that Ag⁺–π coordination remains reversible and chemically stable even after repeated cycling. No signal attributable to metallic Ag⁰ is detected, demonstrating that Ag⁺ remains unreduced throughout both the synthesis and adsorption processes [45].

These XPS results conclusively confirm that reversible π-complexation between Ag⁺ and C₂H₄ is the dominant interaction governing the high C₂H₄/C₂H₆ selectivity of the IL@MCM-41 composites, while also verifying the chemical stability of Ag⁺ under adsorption–desorption cycling conditions. The strengthened Ag⁺–π interaction can be partly attributed to the confinement of the ionic liquid within the mesoporous channels of MCM-41, which promotes IL dispersion, enhances the accessibility of Ag⁺ sites, and brings ethylene molecules into closer proximity with the active centers. Such confinement-induced enhancement of metal–guest interactions has been widely observed in porous host–ionic liquid systems, supporting the view that the ordered mesopores cooperatively contribute to the improved ethylene affinity [46,47]. The presence of C=C-related signals in the cycled sample arises from deliberate re-adsorption of C₂H₄ prior to XPS measurement, rather than from incomplete regeneration, indicating preserved adsorption functionality and excellent reversibility of the Ag⁺ sites.

3.6. Breakthrough Dynamics and Mass-Transfer Characteristics

Dynamic breakthrough curves (Figure 12) clearly highlight the stark contrast between pristine MCM-41 and the 70 wt% IL@MCM-41 composite. Pristine MCM-41 shows nearly overlapping breakthrough profiles for C₂H₄ and C₂H₆, indicating negligible separation capability. In contrast, the 70 wt% IL@MCM-41 composite exhibits a pronounced C₂H₄ breakthrough delay exceeding 60 min, whereas C₂H₆ breaks through rapidly. We attribute this behavior to three factors. First, Ag⁺ forms π-complexes with C₂H₄. Second, the composite shows minimal affinity for C₂H₆. Third, confining the IL in mesopores improves mass transfer and reduces diffusion resistance [25].

The breakthrough behaviors of C₂H₄ over pristine MCM-41, the bulk ionic liquid, and the 70 wt% IL@MCM-41 composite are presented in Figure 13. Pristine MCM-41 shows an early breakthrough and a very sharp adsorption front, indicative of rapid intraparticle diffusion but weak physisorption interactions, which together result in a low equilibrium uptake. In contrast, the column packed with the bulk [Emim][BF₄]/AgBF₄ ionic liquid exhibits a markedly broader mass-transfer zone and a gradual increase in C_t/C₀. This broadening reflects the strong Ag⁺–π interactions toward C₂H₄ as well as the substantial diffusional resistance imposed by the high viscosity of the liquid phase and the limited gas–liquid interfacial area.

Notably, the 70 wt% IL@MCM-41 composite displays a delayed breakthrough compared with pristine MCM-41 but a significantly steeper breakthrough front than the bulk ionic liquid. This behavior demonstrates that confining the Ag⁺-functionalized ionic liquid within the mesoporous channels appreciably enhances overall mass-transfer efficiency while preserving high-affinity adsorption sites for C₂H₄. The much narrower mass-transfer zone relative to the bulk IL confirms that the mesoporous framework provides shortened diffusion pathways and an enlarged accessible interfacial area, thereby enabling faster transport of C₂H₄ molecules toward Ag⁺ active centers.

To further clarify the mass-transfer behavior observed in the breakthrough experiments, the normalized breakthrough curves of bulk ionic liquid, pristine MCM-41, and IL@MCM-41 composites with different ionic-liquid loadings were analyzed using the Clark model (Figure S1). The corresponding kinetic parameters are summarized in Table S1. This normalized analysis reduces the influence of absolute uptake capacity and allows a clearer comparison of mass-transfer efficiency. The results show that the mass-transfer efficiency of IL@MCM-41 composites first increases and then decreases as the ionic-liquid loading increases. This trend reflects enhanced gas–sorbent interactions at low loadings and increased diffusion resistance caused by partial pore blocking at higher loadings. It should be noted that the Clark model is mainly applicable to adsorption-dominated systems. Therefore, the comparison involving bulk ionic liquid is discussed only in a qualitative manner.

3.7. Effect of IL Loading on Mixed-Gas Adsorption Performance

Figure 14 shows the C₂H₄ and C₂H₆ capacities, together with the corresponding selectivities, of the adsorbents at various IL loadings. As illustrated, increasing the IL content markedly enhances the C₂H₄ uptake—from 6.47 mg/g at 0 wt% to 25.68 mg/g at 70 wt%—whereas the C₂H₆ uptake decreases slightly. As a result, the C₂H₄/C₂H₆ selectivity rises sharply from 1.10 to 15.59. Notably, the 70 wt% IL@MCM-41 composite exhibits a markedly enhanced dynamic separation performance compared with the bulk ionic liquid, as evidenced by its steeper breakthrough front, narrower mass-transfer zone, and substantially higher C₂H₄/C₂H₆ selectivity under identical breakthrough conditions. This result highlights the critical role of mesoporous confinement in improving mass-transfer efficiency while preserving strong Ag⁺–C₂H₄ interactions [22].

3.8. Comparison of Adsorption Performance

Comparison with previously reported adsorbents (

Table 3. Comparison of the C₂H₄/C₂H₆ separation performance of the 70 wt% IL@MCM-41 composite with previously reported adsorbents.

Adsorbents	T (K)	P (bar)	mmol C2H4/ g-Adsorbent	mmol C2H6/ g-Adsorbent	Selectivity (C2H4/C2H6)	Ref.
CuCl2/CSC	313	1	0.84	0.11	7.60	[48]
MIL-142A	298	1	1.8	3.3	0.56	[14]
NUS-6(Hf)-Ag	298	1	0.72	0.16	4.40	[15]
AC-F-20	298	1	0.5	1.96	0.26	[49]
70 wt%IL@MCM-41	298	1	0.92	0.059	15.59	This work

) further highlights the superior separation performance of the IL@MCM-41 composites. Most conventional adsorbents exhibit selectivities below 7.6 under comparable conditions, whereas the 70 wt% IL@MCM-41 composite achieves a substantially higher selectivity of 15.59. This performance advantage demonstrates the effectiveness of integrating Ag⁺-functionalized ionic liquids with ordered mesoporous supports, providing a more efficient separation strategy than conventional physisorbents.

3.9. Cyclic Stability

Cyclic adsorption–desorption measurements (Figure 15) demonstrate that the IL@MCM-41 composite possesses excellent operational stability. After ten consecutive cycles, the material retains essentially unchanged adsorption performance, maintaining a C₂H₄ uptake of 25.47 mg/g, a C₂H₆ uptake of 1.77 mg/g, and a C₂H₄/C₂H₆ selectivity of approximately 15.43. The negligible variation across cycles confirms the robustness of the Ag⁺ active sites, the stable distribution of the ionic liquid within the mesoporous channels, and the outstanding regenerability of the composite under repeated adsorption–desorption operation.

4. Conclusions

In this study, a series of silver-based ionic liquid-modified MCM-41 composites were synthesized using [Emim][BF₄]/AgBF₄ as the functional phase, and their structural evolution, adsorption properties, and C₂H₄/C₂H₆ separation performance were systematically investigated. At an IL loading of 70 wt%, the composite exhibited outstanding performance at 298 K and 100 kPa, achieving a C₂H₄ uptake of 25.68 mg/g and a C₂H₄/C₂H₆ selectivity of 15.59, significantly surpassing most reported adsorbents. Compared with the bulk ionic liquid, the IL@MCM-41 composites exhibit markedly higher mass-transfer efficiency and separation selectivity. This high selectivity arises from the synergistic contributions of strong Ag⁺–π complexation and the confined mesoporous environment of MCM-41, which together promote preferential C₂H₄ binding while effectively suppressing C₂H₆ adsorption. Comprehensive characterizations confirmed that the ordered mesoporous structure of MCM-41 remained intact after IL incorporation, with the ionic liquid uniformly dispersed throughout the pore channels. The composites exhibited thermal stability up to 570 K and showed excellent regenerability, with the 70 wt% IL@MCM-41 retaining nearly all of its initial adsorption capacity and selectivity over ten adsorption–desorption cycles.

Overall, these silver-based IL-modified MCM-41 composites combine high selectivity, high uptake capacity, and strong cycling durability, offering promising potential for low-energy, high-efficiency C₂H₄/C₂H₆ separation under mild conditions. These results provide meaningful guidance for the design of next-generation ionic liquid-based adsorbents for olefin/paraffin separations.