Preparation of Nanoporous Carbonaceous Promoters for Enhanced CO2 Absorption in Tertiary Amines

Aqueous solutions of tertiary amines are promising absorbents for CO2 capture, as they are typically characterized by a high absorption capacity, low heat of reaction, and low corrosivity. However, tertiary amines also exhibit very low kinetics of CO2 absorption, which has made them unattractive options for large-scale utilization. Here, a series of novel nanoporous carbonaceous promoters (NCPs) with different properties were synthesized, characterized, and used as rate promoters for CO2 absorption in aqueous N, N-diethylethanolamine (DEEA) solutions. To prepare a DEEA–NCP nanofluid, NCPs were dispersed into aqueous 3 mol∙L 1 DEEA solution using ultrasonication. The results revealed that among microporous (GC) and mesoporous (GS) carbonaceous structures functionalized with ethylenediamine (EDA) and polyethyleneimine (PEI) molecules, the GC–EDA promoter exhibited the best performance. A comparison between DEEA–GC–EDA nanofluid and typical aqueous DEEA solutions highlighted that the GC-EDA promoter enhances the rate of CO2 absorption at 40 C by 38.6% (36.8–50.7 kPa min ) and improves the equilibrium CO2 absorption capacity (15 kPa; 40 C) by 13.2% (0.69–0.78 mol of CO2 per mole of DEEA). Moreover, the recyclability of DEEA–GC–EDA nanofluid was determined and a promotion mechanism is suggested. The outcomes demonstrate that NCP–GC–EDA in tertiary amines is a promising strategy to enhance the rate of CO2 absorption and facilitate their large-scale deployment. 2020 THE AUTHORS. Published by Elsevier LTD on behalf of Chinese Academy of Engineering and Higher Education Press Limited Company. This is an open access article under the CC BY license (http://creativecommons.org/licenses/by/4.0/).


Introduction
Rising carbon dioxide (CO 2 ) emissions from global industrial sources have strengthened international concerns and scientific endeavors to reduce the impact of anthropogenic climate change [1,2]. The Paris Agreement in 2016 focused attention on reducing the growth in CO 2 emissions over the coming decades through a variety of mechanisms [3,4]. One viable approach is carbon capture and storage (CCS), which is strongly reliant on feasible CO 2 capture technologies. CCS will enable international governments to meet their Paris Agreement targets-especially in the industrial sector, including important industries such as ammonia and fertilizer production, cement kilns, as well as iron and steel manufacturing. Among the different CO 2 absorption techniques that are currently available (e.g., absorption [5][6][7], adsorption [8][9][10], membrane separation [11,12], and condensation [13,14]), chemical absorption using aqueous amine solutions has been the most commercially successful technology for CO 2 capture from flue gas (postcombustion carbon capture) and natural gas sweetening [15,16].
Monoethanolamine (MEA), diethanolamine (DEA), and methyldiethanolamine (MDEA) are commonly used primary, secondary, and tertiary amines for large-scale CO 2 absorption applications. Both primary and secondary amines are able to directly react with CO 2 molecules and produce carbamate, which is considered a fast reaction and can significantly increase the kinetics of CO 2 absorption during continuous operation. Nonetheless, the carbamate formation mechanism in primary and secondary amine solutions causes a relatively low CO 2 absorption capacity (1:2 stoichiometry up to 0.5 mol CO 2 per mole amine) in which one molecule of CO 2 reacts with two molecules of amine. Thus, both MEA and DEA benefit from fast kinetics of CO 2 absorption, which differentiates them from the tertiary amine candidates. However, these compounds suffer from a high heat of regeneration, corrosion, and oxidation problems [17,18]. On the other hand, in tertiary amine solutions, one molecule of CO 2 reacts with one molecule of amine and forms bicarbonate, which provides a high absorption capacity (1:1 stoichiometry up to 1 mole CO 2 per mole amine). Therefore, the tertiary amine MDEA has a high CO 2 absorption capacity, low heat of regeneration, and considerable resistance against chemical oxidation [19,20]. However, the slow kinetics of CO 2 absorption in aqueous MDEA solution-or in tertiary amine solutions in general-has substantially inhibited its commercial development.
In 2007, Vaidya and Kenig [21] introduced N,N-diethylethanolamine (DEEA) as a substitute for MDEA with a higher CO 2 absorption rate. Afterward, Chowdhury et al. [22,23] evaluated the absorption properties of 26 different tertiary amines and demonstrated that DEEA has a higher CO 2 absorption rate, higher cyclic CO 2 absorption capacity, and lower heat of absorption compared with conventional MDEA. Nevertheless, the study supported the conclusion that the kinetics of CO 2 absorption in both MDEA and DEEA are not comparable with primary or secondary amines.
To take advantage of the properties of tertiary amines, research endeavors have focused on overcoming their low CO 2 absorption rate by adding primary and secondary amines. Hafizi et al. [19] investigated the efficiency of different polyamines as active promoters for MDEA solutions. Similarly, Gao et al. [6] studied the effect of different amine activators on the CO 2 absorption rate of aqueous DEEA solutions. The results revealed that, although amine promoters can effectively increase the kinetics of CO 2 absorption, they can also considerably increase the required heat of regeneration, corrosion activity, and chemical oxidation. Recently, it was established that using metal oxide nanoparticles and carbonbased nanomaterials in an aqueous solution of tertiary amines can promote the CO 2 absorption capacity and kinetics of CO 2 absorption without introducing the drawbacks of amine promoters.
Rahmatmand et al. [24] displayed that the addition of only 0.02 wt% carbon nanotube (CNT) enhanced the CO 2 absorption capacity of MDEA solution up to 23%. Komati and Suresh [25] showed that the presence of Fe 3 O 4 nanoparticles in MDEA solutions is capable of decreasing the mass transfer resistance at the liquid-gas interface and enhancing mass transfer. Irani et al [20] and Maleki et al [26] investigated the CO 2 and H 2 S absorption using aqueous MDEA solution in the presence of pristine graphene oxide (GO) and amine-functionalized graphene oxide (GO-NH 2 ). They pointed out that the CO 2 absorption enhancement of pristine GO-promoted MDEA solution is governed by a physical promotion mechanism that takes advantage of the nanofluids. On the other hand, GO-NH 2 -promoted MDEA solution not only benefits from the physical absorption improvement mechanism of the nanofluids, but also takes advantage of chemical absorption promotion. Tavasoli et al. [26] showed that the primary amine functional groups located on the surface of GO can actively react with CO 2 molecules, enhance CO 2 absorption capacity, and promote CO 2 absorption rate in aqueous MDEA solvent.
However, due to the low surface area and porosity of GO, the number of active primary amine groups is limited, which negatively affects its chemical promotion efficiency. Importantly, the present research highlights the potential of amine-functionalized nanoporous nanoparticles to act as a promoter for the DEEA system. Accordingly, this investigation focuses on the synthesis of nanoporous carbonaceous promoters (NCPs) derived from commercial activated carbon samples with high surface area and different surface functionalities, which make them unique candidates for the preparation of amine-based nanofluids. The synthesized NCPs were post-functionalized by two different polyaminesethylenediamine (EDA) and polyethylenimine (PEI)-both of which have the primary amine moiety that is needed to act as a promoter. This study therefore investigated the active primary/secondary amine groups on the accessible surface area of nanoporous carbon structure; and determined the improvement to CO 2 absorption capacity as well as increase in the rate of CO 2 absorption in the aqueous DEEA solution.

Synthesis of oxidized NCPs (NCP-COOH)
To synthesize the oxidized NCPs from commercial granular activated carbon (GAC), 2 g of GAC was washed several times with deionized (DI) water, dried at 60°C in a vacuum oven overnight, and completely crushed by a grinder into a fine powder. The resultant fine activated carbon powder was placed in a round flask and mixed with 100 mL of concentrated HNO 3 . Due to the exothermic oxidation reaction between HNO 3 and the high-surface-area activated carbon, HNO 3 was gradually added into the flask at room temperature. To improve the oxidation ability of HNO 3 , 40 mL of H 2 SO 4 was slowly added as a strong oxidation promoter to the mixture under vigorous stirring provided by an external magnetic stirrer. Activated carbon powder was further dispersed in the HNO 3 /H 2 SO 4 mixture by ultrasonication for 2 h. The obtained mixture was heated to 85°C and refluxed at this temperature for 12 h. Following this, the product was diluted by 1000 mL of water; the supernatant liquid was then separated and filtered using a sintered glass funnel and washed with a copious amount of boiling water until a neutral pH was obtained. The residue was separated and dried using a vacuum oven at 60°C overnight. It was labeled as NCP-GC-COOH for the microporous structure and NCP-GS-COOH for the mesoporous structure.

Synthesis of amine-functionalized NCPs (NCP-NH 2 )
Amine functionalization of the NCP-COOH samples was carried out in two consecutive steps using the EDC-NHS cross-linking method to couple the amine groups of polyamines onto the carboxylic groups of NCP-COOH. Briefly, 1.5 g of NCP-COOH was dispersed in 1000 mL of MES buffer (0.1 molÁL À1 and pH 5.5) and ultrasonicated for 15 min to obtain a uniform solution. Next, 3.3 g of EDC and 2 g of NHS were slowly added to the mixture and gently stirred for 18 h at room temperature in the absence of light. The resultant mixture was subsequently filtered using a sintered glass funnel and washed with DI water to completely remove unreacted EDC/NHS molecules on the porous structure. In the second step, the filtered NCP sample with amine-reactive NHS ester groups (NCP-NHS) was suspended in 500 mL MOPS buffer (0.1 molÁL À1 and pH 7.5) and ultrasonicated for 15 min to make a homogeneous solution. Afterward, 500 mL of aqueous EDA or PEI solution (10 mgÁmL À1 ) was mixed with the solution and stirred for an additional 12 h at room temperature to graft aminereactive NHS ester groups onto the surface of the NCPs. At the end, after the conjunction of the polyamines to the aminereactive NHS ester groups of NCP-NHS, the reaction mixture was filtered, washed with DI water to remove unreacted amines, dried at 60°C overnight, and labeled as NCP-X-Y, where X represents the porosity type of the sample (GC or GS) and Y indicates the grafted polyamine on the surface (EDA or PEI). For example, NCP-GC-EDA refers to a microporous carbon-based promoter with grafted EDA molecules on the surface. The reaction pathway for the conjunction of the polyamines on the surface of NCP is schematically illustrated in Fig. 1.

Characterization
Fourier-transform infrared spectroscopy (FT-IR) spectra in the range of 400-4000 cm À1 were collected using a Bruker Tensor II (Bruker Corporation, USA) in attenuated total reflection (ATR) mode to detect chemical bonding and functional groups. The elemental composition of the samples was determined by a LECO TruMac CNS analyzer (LECO, USA). To indirectly measure the amount of functional groups, thermogravimetric analysis (TGA) and differential thermogravimetry (DTG) were undertaken using a NETZSCH TG 209 F1 Libra analyzer (NETZSCH Holding, Germany) heated from 30 to 850°C with a heating rate of 10°CÁmin À1 in N 2 stream. X-ray photoelectron spectroscopy (XPS) was carried out on a VG ESCALAB 220i-XL spectrometer (Thermo Fisher Scientific, USA) under severe vacuum pressure (10 À7 Pa) with A1 Ka radiation and a fixed photon energy of 1486.6 eV. In addition to a broad survey scan in the 0-1400 eV range with 1.0 eV resolution, high-resolution scans for C 1s (282-294 eV), N 1s (396-408 eV), and O 1s (528-538 eV) were conducted with 0.05 eV resolution. Raman spectra were obtained with a Renishaw inVia Qontor confocal Raman microscope system (Renishaw, India) with a laser excitation wavelength of 532 nm, spectral resolution of 1 cm À1 , and over 800-3200 cm À1 range. To effectively immobilize the carbon powder during the operation of the Raman instrument, the samples were dispersed in ethanol, coated on a silicon wafer, and dried under vacuum at ambient temperature for 2 h. Scanning electron microscopy (SEM) images were taken by an FEI Quanta 200 ESEM FEG instrument (USA), with 20 and 30 kV operation voltages. Zeta potential and dynamic light scattering (DLS) measurements were performed by a Malvern Zetasizer Nano ZS (Malvern Panalytical Ltd., UK) equipped with a He-Ne ion laser (k = 633 nm). The species formed during CO 2 absorption in the amine solution were identified by NMR spectroscopy analysis (Agilent 500 MHz; Agilent Technologies, Inc., USA). The delay time and number of scans were set at 20 s and 128, respectively, for 13 C NMR, and at 2 s and 32, respectively, for 1 H NMR measurement. Each NMR tube contained 600 lL D 2 O (as a solvent), 100 lL sample, and 10 lL acetonitrile (as an internal reference). The surface area and pore volume were measured by a Micrometrics 3Flex instrument (MicroMetrics, USA) using the N 2 adsorption technique at 77 K. A BS/IP/RF U-tube reverse-flow capillary viscometer (ASTM D445-06) was employed to measure the viscosity of the amine solutions and the prepared nanofluids.

Preparation of DEEA-NCP nanofluid
The concentration of aqueous DEEA solution was kept constant at 3 molÁL À1 for all experiments. 350 g of DEEA was dissolved in DI water and diluted until a 1 L volume of solution was obtained. To prepare the DEEA-NCP nanofluid, typically 0.1 g of NCP sample was weighed, dispersed in 100 mL of aqueous 3 molÁL À1 DEEA solution and ultrasonicated for 30 min. The obtained nanofluids were labeled as DEEA-X-Y, where X defines the porosity type of NCP (i.e., GC or GS), and Y defines the surface functionalities of NCP (i.e., COOH, EDA, or PEI).

Measurement of CO 2 absorption
In order to quantitatively monitor the absorption of CO 2 into the prepared nanofluids, an in-house vapor-liquid equilibrium (VLE) apparatus was used. The details of operation and measurement accuracy have been presented in our previous works [5,27]. A simple schematic diagram of the CO 2 absorption apparatus is presented in Fig. 2. In a typical CO 2 absorption experiment, 100 mL of nanofluid was weighed and loaded in the stainless-steel reactor with 325 mL available volume. Afterward, the reactor was completely sealed, put into a water bath, and connected to the gas injection system. Before starting the CO 2 absorption experiments, the system was purged with pure N 2 at 70°C for 15 min to remove dissolved air and other unwelcome gas molecules from the loaded DEEA-NCP nanofluid. The reactor was then pressurized with pure N 2 to 175 kPa, and the water bath temperature was set at a desired operational temperature (typically 40°C) for CO 2 absorption. When the reactor temperature set-point was reached and its pressure was stabilized, the buffer tank (500 mL) was pressurized with pure CO 2 gas and the final pressure was recorded (P 1 ). After that, the pressurized CO 2 was injected from the buffer tank to the reactor and the new pressure of the buffer tank was again recorded (P 2 ).
To dynamically monitor and record the pressure of the apparatus, two micro silicon pressure sensor transducers with high accuracy (0.08% of full-scale) were installed on each of the CO 2 buffer tank (Omega, PX409-150 GUSBH, 0-1030 kPa) and the reactor (OMEGA, PX409-100 GUSBH, 0-690 kPa; OMEGA Engineering Inc., UK). The water bath was equipped with a digital immersion heater circulator (Ratek, TH7000; Ratek Instruments, Australia) with high accuracy to control the temperature of the water bath, and a thermocouple (Omega, TJ-USB-K1; OMEGA Engineering Inc., UK) with ±0.1°C accuracy was used to monitor the reactor temperature.
The total number of moles of CO 2 injected into the VLE reactor can be directly calculated by Eq. (1): where P 1 and P 2 are the pressure of the CO 2 buffer tank before and after CO 2 injection; V BT is the available volume of the buffer tank; T a is the ambient temperature; R is the ideal gas constant; and Z 1 and Z 2 are the compressibility factor of CO 2 corresponding to the P 1 and P 2 pressures. To calculate the compressibility factor at different CO 2 partial pressures, the Soave-Redlich-Kwong (SRK) equation of state was employed (Eq. (2)) [1]: where P is the pressure; T is the temperature; Z is the compressibility factor. All necessary coefficients can be obtained by Eqs. (3)- (5): where T c is the critical temperature, T r is the reduced temperature, P c is the critical pressure, and x is the acentric factor.
The partial pressure of CO 2 in the VLE reactor (P CO 2 ) can be calculated by Eq. (6): where P R is the reactor pressure and P I is the initial N 2 pressure injected in the VLE reactor. Accordingly, the total number of moles of CO 2 in the gas (n g CO 2 , Eq. (7)) and liquid (n l CO 2 , Eq. (8)) phases is obtained by the following: where V g is the gas volume in the reactor, T R is the adjusted reactor temperature, and Z CO 2 is the compressibility factor corresponding to the P CO 2 . The total amount of absorbed CO 2 into the loaded DEEA-NCP nanofluid during each CO 2 injection cycle is computed by Eqs. (9) and (10): where m CO 2 is the molality of CO 2 (mole of CO 2 per kilogram of amine solution); a CO 2 is the CO 2 loading (mole of CO 2 per mole of amine); w sol is the weight of the solution (kg); and n amine is the total number of moles of amine in the solution.
To measure the rate of CO 2 absorption and CO 2 absorption rate enhancement after adding nanoporous carbonaceous promoters, Eqs. (11) and (12) were employed, respectively.
where R CO 2 is the rate of CO 2 absorption (kPaÁmin À1 ); P is the operating pressure (kPa); t is the time (min); and DP (i.e., 50, 100, 150, 200, 250, and 300 kPa) is the pressure drop after starting the gas absorption experiment (kPa). For cyclic CO 2 absorption-desorption experiments, the CO 2saturated DEEA-NCP nanofluid was poured into a round flask and heated at 95°C for 3 h under reflux conditions. Next, the regenerated DEEA-NCP nanofluid was naturally cooled down to room temperature and used again for CO 2 absorption experiments. The regeneration efficiency was defined as follows: where i is the number of each cycle.

Characterization of NCPs
The FT-IR spectra of all commercial activated carbons and synthesized NCPs are illustrated in Figs. 3(a) and (b). In brief, the absorbance bands centered on 1750 and 1150 cm À1 were ascribed to the vibration of C=O and C-O bonds, respectively [28,29]. In addition, the prominent absorbance at around 1570 and 1380 cm À1 corresponded to the N-O and C-N stretching vibrations [29,30]. Compared with commercial activated carbons (i.e., AC-GC and AC-GS), the spectra of NCP-GC-COOH and NCP-GS-COOH had stronger absorbance bands for all four C=O, C-O, N-O, and C-N vibrations. To be specific, the intensification of the C=O/C-O and N-O/C-N characteristic peaks implies the successful implantation of carboxylic (-COOH) and nitrous (-NO 2 ) functional groups on the surface of nanoporous carbon as the direct result of HNO 3 oxidation/nitration [30,31]. After EDA and PEI functionalization using EDC-NHS cross-linking agents, the intensity of the absorption band related to the carbonyl bond (C=O) was significantly reduced. Similarly, the intensity of the C-O vibrational bands located at 1150 cm À1 decreased after the conjunction of polyamines on the previously implanted carboxylic groups. These observations confirm the polyamine immobilization on the surface of the nanoporous carbon through the successful conversion of carboxylic groups to amide groups using EDC-NHS cross-linker [32][33][34][35].
To gain additional information on the attached functional groups on the surface of the synthesized NCPs, we report on the combination of TGA/DTG and elemental analysis. According to the TGA (Fig. S1 in Appendix A) and DTG (Fig. S2 in Appendix A) curves of the commercial activated carbons and functionalized NCPs, the weight loss can be categorized into three different regions. The first weight-loss region was observed around 90-110°C and was due to moisture evaporation [10]. The decomposition of oxygencontaining functional groups (i.e., -COOH and -OH) started at 180°C and continued to higher temperatures. In addition to the decomposition of oxygen groups at 300-330°C, another peak was observed in the EDA-and PEI-grafted NCP samples (see Fig. S1 and Fig. S2) and continued until 600°C; this was mainly due to the decomposition of amine groups [30]. Hence, the weight loss between 180 and 600°C was considered to be an indicator of the amount of functional groups. The results are presented in Figs. 3(c) and (d). Pristine AC-GC and AC-GS exhibited 4.9% and 2.1% weight reduction, respectively, which can be ascribed to their inherent carboxyl (-COOH) and carbonyl (-OH) functional groups. Nevertheless, the weight reduction of HNO 3 -oxidized NCP-GS-COOH (20.0 wt%) was considerably higher than that of NCP-GC-COOH (12.7 wt%). Interestingly, after polyamine grafting, the microporous NCP-GC-EDA displayed greater weight reduction (18.1 wt%) than the NCP-GC-PEI (17.4 wt%), while the polyamine-functionalized mesoporous NCP-GS showed a contrary behavior. The weight reduction of mesoporous EDA-grafted NCP-GS-EDA (20.2 wt%) was 27.7% less than that of PEI-grafted NCP-GS-PEI (25.8 wt%). It seems that the PEI molecules failed to effectively enter the micropores of the NCP-GC structure due to their high molecular weight and large radius of gyration, while the EDA molecules successfully loaded the micropores with high grafting conversion. Similarly, the results of the elemental analysis for different NCP samples (Table 1) proved the presence of inherent oxygen functional groups on the surface of commercial AC-GS carbon, remarkable enrichment of oxygen content after HNO 3 oxidation (i.e., NCP-GC-COOH and NCP-GS-COOH), and nitrogen content after polyamine conjunction (i.e., NCP-GC-EDA, NCP-GC-PEI, NCP-GS-EDA, and NCP-GS-PEI) on the surface, all of which are compatible with the previously presented interpretations. Table 1 shows the textural properties of ACs (i.e., AC-GC and AC-GS) and the prepared NCP promoters. As can be seen, although the coal-based AC-GS sample possessed a greater specific surface area (SSA) (1425.17 m 2 Ág À1 ) and pore volume (0.93 cm 3 Ág À1 ) than the coconut-based AC-GC (1137.41 m 2 Ág À1 and 0.46 cm 3 Ág À1 ), its pore volume and SSA were remarkably affected by surface oxidation and decreased to 263.75 m 2 Ág À1 and 0.16 cm 3 Ág À1 in NCP-GS-COOH. In comparison, the NCP-GC-COOH promoter displayed a highly accessible SSA (860.82 m 2 Ág À1 ) and pore volume (0.47 cm 3 Ág À1 ), making it a better porous base for amine grafting. Hence, NCP-GC-EDA (227.28 m 2 Ág À1 and 0.13 cm 3 Ág À1 ) and NCP-GS-PEI (9.78 m 2 Ág À1 and 0.01 cm 3 Ág À1 ) respectively exhibited the best and worst textural properties among the four polyamine grafted promoters.
To further explore the structure of ACs and NCP samples, Raman spectroscopy was employed (Figs. 4(a) and (b)). All samples exhibited two peaks around 1350 cm À1 (D band) and 1590 cm À1 (G band), which were both characteristic indicators of the carbon structure. The D band shows the sp 3 disordered/amorphous mode and the G band corresponds to the sp 2 bond stretching of the carbon structure [29,30,36]. Therefore, the intensity ratio of the D band to the G band (I D /I G ) can representatively indicate structural disorder in carbon-based nanomaterials (see Table S1 in Appendix A). Both AC-GC (1.12) and AC-GS (1.14) displayed high I D /I G values, indicating a high degree of defect in the structure of commercial microporous and mesoporous activated carbons. After surface oxidation with HNO 3 , the I D /I G value decreased in the NCP-GC-COOH (1.04) and NCP-GS-COOH (0.96) samples, which can be ascribed to the partial graphitization of the porous carbon structure under the harsh oxidation conditions [37]. However, the reduced I D /I G values of NCP-GC-COOH and NCP-GS-COOH are still comparable with those previously reported in the literature [8,[28][29][30]. On the other hand, the I D /I G ratio increased from NCP-GC-COOH (1.04) to NCP-GC-EDA (1.06) and NCP-GC-PEI (1.07) when polyamines were immobilized through the structure of the nanoporous carbon. In a similar trend, both polyamine-functionalized NCP-GS-EDA (1.05) and NCP-GS-PEI (0.98) exhibited a higher I D /I G ratio than that of NCP-GS-COOH (0.96), indicating that new defects were created by grafted polyamines on the surface.
In addition to the FT-IR, TGA, and elemental analysis, XPS was utilized as a quantitative surface analysis technique to measure the amount of different functional groups on the surface of the NCPs. The XPS survey spectra and the amount of oxygen/nitrogen species on the surface of NCP-GC-COOH and NCP-GC-EDA, as the representative NCPs, are depicted in Fig. 4(c). In the XPS survey spectra (Fig. 4(c)), three major peaks were recorded at around 285, 397, and 532 eV, which represent C 1s, N 1s, and O 1s [38]. As the total atomic analysis (Fig. 4(d)) of the surface shows, the oxygen content decreased from 14.55 at% in NCP-GC-COOH to 12.46 at%  in NCP-GC-EDA, whereas the nitrogen content increased from 1.83 at% in NCP-GC-COOH to 6.44 at% in NCP-GC-EDA; these results superficially ratify amine conjunction on the surface through amide formation. To scrutinize the amine functionalization mechanism, high-resolution spectra of different moieties were recorded (Figs. 4(e)-(h) and Fig. S3 in Appendix A). According to Fig. 4(e), the NCP-GC-COOH sample possessed two C-O-H (8.22 at%; 533.2 eV) and C=O (5.88%; 531.6 eV) peaks, which were both the main constituents of carboxylic groups. In addition, the presence of both -NO 2 (0.77 at%; 405.6 eV) and C-N (1.06 at%; 399.3 eV) peaks in the high-resolution N 1s spectrum of NCP-GC-COOH ( Fig. 4(g)) reconfirms the nitrification of the carbon structure during surface oxidation by HNO 3 [39]. Similarly, the high-resolution O 1s (Fig. 4(f)) spectrum of NCP-GC-EDA shows that the C-O-H content dropped to 4.97 at% (from 8.22 at% in NCP-GC-COOH) and, contrarily, the C=O content increased to 7.09 at% (from 5.88 at% in NCP-GC-COOH). Moreover, two new amide/-NH 2 (5.28 at%, 399.8 eV) and -NH 2 (0.8 at%, 402.2 eV) peaks appeared in the high-resolution N 1s spectra of NCP-GC-EDA (Fig. 4(h)). These changes signal the formation of amide groups on the surface of NCP-GC-EDA after the crosslinking of polyamines on the carboxylic groups. SEM images of the commercial activated carbons, oxidized carbon structures, and amine-functionalized NCPs are shown in Figs. 5 (a)-(p). The images show that the particle size of the carbon slightly decreased after HNO 3 /H 2 SO 4 treatment, which confirms that the carbon structure was broken down into smaller units after the harsh oxidation. However, the morphology remains nearly the same for all samples (either GC or GS structure) before and after the conjunction of different functional groups. Therefore, nitric acid oxidation does not affect the structural morphology of the NCP and no aggregation was observed after amine conjunction. Fig. S4 in Appendix A shows the average particle size distribution of different NCPs obtained by DLS measurement. The results clearly confirm that all prepared NCP samples possessed an average diameter of less than 400 nm, which is much smaller than those displayed by SEM micrographs (1-2 lm). This discrepancy can be generally attributed to the differences in the operating mechanism of DLS and SEM characterizations. In SEM microscopy, characterization is performed in the solid state, which can strikingly accelerate the agglomeration of particles and increase the size of clusters. On the other hand, in the DLS technique, the particles are fully dispersed in solution using ultrasonication before starting the measurement, making DLS a better characterization method for determining the average particle size of similar systems.

Stability of NCP samples
To assess the stability of the synthesized NCPs, one of the most crucial characteristic factors of nanofluids, a zeta potential investi-gation was carried out. Figs. 6(a)-(h) shows the zeta potential values of all prepared DEEA-NCP nanofluids with different functionalities on the surface of the nanoporous promoters, along with photographs of their stability at different time intervals. In general, the zeta potential indicates the electrostatic charge (either attractive or repulsive) of solid particles/clusters suspended in a liquid phase. Therefore, the zeta potential value can indirectly represent the stability of suspended nanomaterials in nanofluids. Specifically, both very high (greater than 10 mV) and very low (less than À10 mV) zeta potential values can show that the suspended nanomaterials are thoroughly stable in solution. In contrast, values that fall between these extremes typically display nanomaterial instability and a tendency to agglomerate/precipitate. According to Figs. 6(a) and (b), as-prepared microporous NCP-GC-COOH (À33.42 mV) and mesoporous NCP-GS-COOH (À11.98 mV) exhibited high negative zeta potential values, which were attributed to the acidic functional groups (-COOH and -OH). Moreover, the zeta potential value of NCP-GC-COOH was about two times higher than that of the NCP-GS-COOH sample, which clearly shows that coconut-derived carbon is a better candidate for surface functionalization and NCP preparation than coal-derived carbon. As anticipated, the NCP-GC-COOH and NCP-GS-COOH promoters remained stable in suspension over a five-day period. After the conjunction of polyamines on the carboxylic groups through amide formation reaction, the zeta potential values increased due to the positive charges of the deprotonated amine groups. The strong positive charge of the polyamine groups on the surface of NCP-GC-PEI (À8.26 mV) and NCP-GS-EDA (À5.62 mV) elevated the particles' zeta potential to greater than À10 mV, resulting in unstable suspensions (Figs. 6(g) and (h)). Conversely, the NCP-GC-EDA (À26.08 mV) and NCP-GS-PEI (À10.02 mV) promoters remained stable in the solution over a five-day period, due to optimum functional group distribution on the surface.

Kinetics of CO 2 absorption in DEEA-NCP nanofluids
As a tertiary amine, DEEA is unable to directly react with CO 2 molecules and generate carbamate. The reaction of tertiary amines with CO 2 is governed by an indirect hydrolysis reaction producing bicarbonate and protonated amine. As a result, most tertiary amines have a low rate of CO 2 absorption, which has hindered their prevalent utilization despite their considerable advantages (e.g., high absorption capacity and low heat of desorption). In this study, in order to quantify the role of different NCPs in the rate of CO 2 absorption in aqueous DEEA solutions, the pressure drop of CO 2 versus time for different DEEA-NCP nanofluids is provided in Figs. 7(a) and (b) Table S2 in Appendix A. Since PEI molecules contain many primary and secondary amine groups, it was expected that PEI-grafted NCP-GC-PEI and NCP-GS-PEI nanoporous promoters would exhibit a higher rate of CO 2 absorption compared with those containing EDA-grafted promoters with only one primary and one secondary amine site. Despite these expectations, DEEA-NCP nanofluids containing PEI-grafted NCPs exhibited a poorer CO 2 rate enhancement than those with EDA-grafted NCPs under similar conditions. According to Fig. 7(b), the CO 2 absorption curve of DEEA-GS-PEI nanofluid had a considerable overlap with the typical DEEA solution across the whole absorption time period, confirming the poor performance of NCP-GS-PEI as a promoter. The low efficiency of PEI-grafted mesoporous DEEA-GS-PEI nanofluid demonstrated that the PEI molecules blocked the porous structure; as a result, most of the primary and secondary amine sites of the polyamine were nearly inaccessible in the DEEA-GS-PEI nanofluid, leading to insignificant reaction enhancement.
In contrast, nanofluids containing microporous promoters displayed superior performance compared with those containing mesoporous promoters, as demonstrated in Figs. 7(c) and (d) (also see Figs. S5 and S6 in Appendix A). Among all the prepared DEEA-NCP nanofluids, DEEA-GC-EDA nanofluid showed the best performance and succeeded in increasing the rate of CO 2 absorption to 50.7 kPaÁmin À1 , which is 38.6% greater than that of commercial DEEA solution (36.8 kPaÁmin À1 ). Following this, in decreasing order were DEEA-GC-PEI (47.8 kPaÁmin À1 ), DEEA-GS-EDA (46.6 kPaÁmin À1 ), and DEEA-GS-PEI (37.8 kPaÁmin À1 ), all of which improved the CO 2 absorption rate (by 28.2%, 27.8%, and 3.1%, respectively), in comparison with aqueous DEEA. Hence, the NCP-GC-EDA promoter with an EDA-grafted microporous structure was chosen as the best candidate among all synthesized NCPs with different properties. Therefore, it can be anticipated that using NCP-GC-EDA as a promotor for tertiary amine solutions can not only reduce the required residence time in the absorption column in order to reach a constant absorption capacity, but also decrease the solvent circulation rate and subsequently the amount of required energy for thermal regeneration.

Effect of NCP-GC-EDA concentration
As NCP-GC-EDA presented the best performance in CO 2 absorption rate enhancement among all screened microporous and mesoporous NCPs with different polyamine functionalities, the nanoporous NCP-GC-EDA promoter was selected to assess the role of carbonaceous promoter concentration on the rate of CO 2 absorption. To achieve this objective, DEEA-GC-EDA nanofluid with four different mass fractions of NCP-GC-EDA promoter (0.05 wt%, 0.1 wt%, 0.2 wt%, and 0.5 wt%) was analyzed for the concentration-dependent promotion of CO 2 absorption. Both the CO 2 absorption rate and the rate enhancement are presented in Figs  absorption. However, increasing the concentration of NCP-GC-EDA promoter to 0.1 wt% markedly increased the rate of CO 2 absorption in the nanofluid up to 50.7 kPaÁmin À1 , which was 38.6% more than that of aqueous DEEA solution without any promoter. Interestingly, the CO 2 absorption rate of both DEEA-GC-EDA nanofluids with 0.2 wt% (42.4 kPaÁmin À1 ) and 0.5 wt% (36.8 kPaÁmin À1 ) promoter was much less than that of DEEA-GC-EDA nanofluids with 0.1 wt% (50.7 kPaÁmin À1 ). This adverse effect of NCP-GC-EDA promoter on the kinetics of CO 2 absorption can be related to the high viscosity of nanofluids at a high concentration of nanomaterials (see also Fig. S8 in Appendix A). This interpretation is consistent with the findings of Dharmalingam et al. [40], who reported the great influence of nanoparticles on the viscosity of nanofluids and their corresponding CO 2 absorption performance. According to Dharmalingam et al., the high concentration of nanomaterials in the aqueous solution can greatly increase the viscosity of the nanofluids, diminish the mass transfer coefficients at the gas-liquid interface, and suppress the positive effect of the promoter on the CO 2 absorption rate. Overall, this part of the study clearly suggested that adding nanoporous NCP-GC-EDA promoter with 0.1 wt% concentration as the optimum amount of promoter can substantially enhance the CO 2 absorption rate of aqueous DEEA solution, and indicated that using greater concentrations of GC-EDA should be avoided.

Absorption isotherms of CO 2 in DEEA-GC-EDA nanofluid
The CO 2 absorption capacity of both conventional aqueous 3 molÁL À1 DEEA solution and DEEA-GC-EDA nanofluid (3 molÁL À1 , 0.1 wt%) at different CO 2 partial pressures and 40°C is provided in Fig. 8(a) (see also Table S3 and Table S4 in Appendix A). It can be seen that the trend of CO 2 absorption in both liquid absorbers was essentially identical and the solubility of CO 2 was raised by increasing the CO 2 partial pressure. Compared with conventional aqueous 3 molÁL À1 DEEA solution, the DEEA-GC-EDA nanofluid showed noticeably higher CO 2 absorption capacity over the range of CO 2 partial pressures (0.1-90 kPa), particularly at low CO 2 partial pressures. A simple comparison at a CO 2 partial pressure of 15 kPa (Fig. 8(b)) revealed that only the presence of 0.1 wt% NCP-GC-EDA promoter increased the CO 2 absorption capacity by 13.1% from 0.69 mol in aqueous DEEA solution to 0.78 mol CO 2 per mole DEEA in DEEA-GC-EDA nanofluid. In other words, DEEA-GC-EDA nanofluid has a CO 2 absorption capacity that is 13.1% higher than that of commercial aqueous DEEA solution for CO 2 from flue gas streams (at 15 kPa and 40°C). With respect to the outcomes, the positive effect of NCP-GC-EDA promoter on the CO 2 absorption capacity is based on two factors. First, the porous structure of NCP-GC-EDA, which has a high surface area and pore volume, can physically adsorb a considerable amount of dissolved CO 2 molecules, CO 2 -containing species, and protonated amines in the solvent, shift the bicarbonate formation reaction to the right side, and increase the equilibrium CO 2 absorption capacity in the whole system. Second, through the porous structure of NCP-GC-EDA, primary/secondary amine groups can effectively react with CO 2 molecules through carbamate formation reactions, facilitate the diffusion of CO 2 molecules into the nanoporous structure, and improve the final CO 2 absorption capacity of the solution. Although the DEEA-GC-EDA nanofluid maintained its CO 2 loading superiority over commercial aqueous DEEA solution, the CO 2 loading enhancement ratio gradually dropped from 13.1% at 15 kPa to 9.1% and 4.8% at 30 and 60 kPa, respectively. The better performance of NCP-GC-EDA promoter at low CO 2 partial pressures may be related to the fact that the effect of physical adsorption by the GC structure and the chemical promotion reaction by pri- Fig. 8. Comparing (a) the CO 2 absorption isotherm, (b) equilibrium CO 2 loading and enhancement ratio of typical aqueous DEEA solution (grey) and DEEA-GC-EDA nanofluid (yellow). mary/secondary amine sites inside the micropores is more significant at low CO 2 partial pressures.
To evaluate the stability of nanoporous NCP-GC-EDA as a newly introduced CO 2 promoter, the CO 2 absorption rate, CO 2 rate enhancement compared with aqueous DEEA solution, and regeneration efficiency of DEEA-GC-EDA nanofluid during three consecutive absorption-desorption cycles were measured ( Fig. 9(a)). As shown in Fig. 9(a), the regeneration efficiency dropped to 96.19% during the first cycle, resulting in a CO 2 absorption rate reduction from 50.70 kPaÁmin À1 (38.6% enhancement) to 48.77 kPaÁmin À1 (32.88% enhancement). This reduction can be attributed to the partial distortion (or saturation) of amine sites and blockage of the GC structure due to the irreversible physical absorption and chemical reaction between CO 2 and primary amine groups on the surface. In a similar trend, the rate of CO 2 absorption and regeneration efficiency gradually declined to 47.89 kPaÁmin À1 and 94.46% during the second cycle, and reached 48.06 kPaÁmin À1 and 94.79% in the third cycle. Due to the similar regeneration efficiency values in the second and third cycles, it was assumed that the cyclic CO 2 absorption rate of DEEA-GC-EDA nanofluid stabilized after three successive cycles. Analyzing the data revealed that the cyclic CO 2 absorption rate of DEEA-GC-EDA nanofluid was only 5.2% (50.7 to 48.06 kPaÁmin À1 ) less than its initial CO 2 absorption rate, which shows the high performance of nanoporous NCP-GC-EDA during cyclic CO 2 absorption-desorption operation. Thus, NCP-GC-EDA promoter can be easily used for large-scale CO 2 absorption from flue gas using aqueous tertiary amine solutions.
To investigate the promotion mechanism of microporous NCP-GC-EDA in aqueous DEEA solution during CO 2 absorption, CO 2saturated DEEA-GC-EDA nanofluid was centrifuged (10 000, 15 min) and the remaining brownish supernatant was characterized by FT-IR and NMR spectroscopy. FT-IR, 13 C NMR, and 1 H NMR spectra of CO 2 -saturated DEEA-GC-EDA nanofluid, CO 2saturated DEEA solution without using any promoter, and fresh aqueous DEEA solution (before CO 2 absorption) are depicted in Figs. 9(b) and (c) and Fig. S7(b) in Appendix A. A comparison between the FT-IR spectra of different samples disclosed that both the aqueous DEEA solution and the DEEA-GC-EDA nanofluid contained similar species. The increase in the intensity of the absorption bands in the 1350-1360 and 1560-1625 cm À1 regions is related to the formation of bicarbonate and protonated amine during CO 2 absorption [41]. Also, the 1 H NMR and 13 C NMR spectra of different samples displayed similar results to those of FT-IR and confirmed the presence of bicarbonate as the only CO 2containing species in the solution. It is worth noting that both characterization methods emphasized that no carbamate formed in the solution during CO 2 absorption. This finding implies that using carbonaceous NCP-GC-EDA promoter does not influence the CO 2 absorption mechanism in tertiary amine solutions, and that the reaction is governed by direct bicarbonate formation reaction. Hereupon, it can be deduced that nanoporous NCP-GC-EDA can promote the rate of CO 2 absorption and equilibrium CO 2 absorption capacity of tertiary amines through a direct carbamate formation reaction between physically absorbed CO 2 molecules and the primary/secondary amine groups of grafted polyamines in the nanoporous structure of NCPs.

Conclusions
In summary, a novel nanoporous rate promoter with polyamine functional groups was introduced to enhance the rate of CO 2 absorption in aqueous tertiary amines. To assess the roles of textural porosity and amine functional groups, both GC and GS carbon structures were employed and post-functionalized by EDA and PEI molecules as typical polyamines with low and high molecular weight, respectively. All synthesized NCPs were fully characterized by FT-IR, XPS, TGA, Raman, SEM, and elemental analysis to evaluate the structure of the promoters. The results of CO 2 absorption in aqueous DEEA-NCP nanofluids confirmed that DEEA-GC-EDA nanofluid containing EDA-grafted GC structures displayed the most promising performance among all prepared nanofluids. To be specific, the use of only 0.1 wt% of NCP-GC-EDA promoter in a typical aqueous DEEA solution succeeded in improving the rate of CO 2 absorption from 36.8 to 50.7 kPaÁmin À1 (38.6%) and the equilibrium CO 2 absorption capacity from 0.69 to 0.78 mol CO 2 per mole DEEA (13.2%). Moreover, the effect of NCP-GC-EDA concentration on the kinetics of CO 2 absorption was studied, and it was demonstrated that 0.1 wt% is the optimum amount of NCP in the aqueous DEEA solution. To assess the recyclability of NCP-GC-EDA, the cyclic CO 2 absorption rate of DEEA-GC-EDA nanofluid was measured, which only displayed 5.2% (50.7-48.06 kPaÁmin À1 ) reduction over three successive CO 2 absorption-desorption cycles. In addition, an enhancement mechanism was suggested for the NCP-GC-EDA rate promoter based on the FT-IR and NMR spectroscopy before and after CO 2 absorption in DEEA-GC-EDA nanofluid. Overall, the microporous NCP-GC-EDA structure can be proposed as a viable promoter to effectively overcome the drawbacks of tertiary amine solutions, in order to enhance the rate of CO 2 absorption and facilitate their large-scale utilization.