Next Article in Journal
Polymer Electrolyte Membranes Based on Nafion and a Superacidic Inorganic Additive for Fuel Cell Applications
Next Article in Special Issue
A Multilayer Emitter Close to Ideal Solar Reflectance for Efficient Daytime Radiative Cooling
Previous Article in Journal
Polymer Science and Engineering Using Deep Eutectic Solvents
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
Polymers
Volume 11
Issue 5
10.3390/polym11050913
polymers-logo
Submit to this Journal Review for this Journal Propose a Special Issue
► Article Menu

Article Menu

share Share announcement Help format_quote Cite question_answer Discuss in SciProfiles thumb_up
...
Endorse textsms
...
Comment
first_page
settings
Order Article Reprints
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:
Background:
Article

Effect of Triblock Copolymer on Carbon-Based Boron Nitride Whiskers for Efficient CO2 Adsorption

by
Urooj Kamran
1,
Kyong Yop Rhee
2,* and
Soo-Jin Park
1,*
1
Department of Chemistry, Inha University, 100 Inharo, Incheon 22212, Korea
2
Department of Mechanical Engineering, College of Engineering, Kyung Hee University, Yongin 17104, Korea
*
Authors to whom correspondence should be addressed.
Polymers 2019, 11(5), 913; https://doi.org/10.3390/polym11050913
Submission received: 19 April 2019 / Revised: 16 May 2019 / Accepted: 19 May 2019 / Published: 21 May 2019
(This article belongs to the Special Issue Polymers for Energy Storage and Conversion)
Browse Figures
Versions Notes

Abstract

:
Herein, we investigated novel carbon-containing P123 copolymer-activated boron nitride whiskers (P123-CBNW) fabricated via a structure directing approach followed by a single-step heat treatment under N2. The resulting materials were found to be highly micro- and mesoporous. The influence of the activating agent (P123 copolymer) on the CO2 adsorption efficiency was determined. The prepared samples possessed high specific surface areas (594–1732 m2/g) and micropore volumes (0.258–0.672 cm3/g). The maximum CO2 uptakes of the prepared adsorbents were in the range 136–308 mg/g (3.09–7.01 mmol/g) at 273 K and 1 bar and 97–114 mg/g (2.22–4.62 mmol/g) in the following order: CBNW < P123-CBNW3 < P123-CBNW2 < P123-CBNW1 < P123-CBNW0.5. The isosteric heat of adsorption values (∆Qst) were found to be 33.7–43.7 kJ/mol, demonstrating the physisorption nature of the CO2 adsorption. Extensive analysis revealed that the presence of carbon, the high specific surface area, the high microporosity, and the chemical structural defects within the adsorbents are responsible for raising the CO2 adsorption ability and the selectivity over N2 gas. The fabricated adsorbents show excellent regeneration ability after several repeated adsorption cycles, making the prepared adsorbents promising candidates for gas storage applications.

1. Introduction

Carbon dioxide (CO2) emission is an issue of major concern because CO2 is a primary anthropogenic cause of environment variation and global warming. The International Monetary Fund (IMF) reported that up to 36 billion tons, considered an unacceptable level, of CO2 are released all over the world, harshly influencing human health, the ecosystem, as well as gross domestic products [1]. The common sources of CO2 emissions are coal fired plants and the combustion of fossil fuels include petroleum and mineral-coal, and methane gas generated from factories and the transportation and energy sectors [2,3,4,5]. Fossil fuels have a major impact on the increased CO2 levels, up to 406.4 ppm, which is directly responsible for further exacerbating the greenhouse effect [6]. For this reason, carbon capture and storage (CSS) is considered to be a very efficient approach to lower the levels of environmental CO2. While various defensive and remedial approaches to handle CO2 emissions are available, such as cryogenic distillation, liquid scrubbing, membrane separation, and conventional temperature or pressure swing (TSA or PSA) [7], these techniques have some drawbacks such as high energy consumption, greater processing time, and high cost [8,9]. At the commercial scale, traditional methods, such as wet scrubbing, utilize liquid amine-based materials for CO2 storage. Such methods possess some demerits including greater energy and cost consumption, equipment rusting, the toxic nature of amines and their byproducts, and loss of liquid from instruments [10,11]. Therefore, CO2 uptake by adsorption on various porous adsorbents, like covalent and porous organic polymers (COPs and POPs) [12,13,14], hexagonal/porous boron nitride (h-BN) [15,16], silica [17,18], polymeric materials [19], nitrogen doped carbon compounds [20,21], metal–organic frameworks (MOFs) [22,23], and metal oxide based carbonaceous materials [24,25,26], have been introduced as alternatives.
Among these adsorbents, porous boron nitride compounds (BN) seem to be the most effective because of their identical physiochemical characteristics, including high thermal and chemical durability and conductivity, low density, tunable high specific surface area (almost identical to activated carbon), few morphological defects, and possession of higher ordered chemistry as compared to carbonaceous adsorbents due to the existence of polar B–N bonds [27,28,29,30,31,32]. These advantageous properties lend porous BN to be favorable for applications in various areas, such as for gas adsorption of H2 [33], removal of organic pollutants and dyes from water [34], and use as a catalytic support. For instance, a previously fabricated porous BN material capable of CO2 uptake of up to 0.6 mmol/g was reported by Sofia et al. while h-BN synthesized by Chen et al. showed CO2 capture of up to 3.74 mmol/g at 298 K. Furthermore, Xiao et al. demonstrated CO2 uptake of about 0.45 mmol/g at 298 K by layered h-BN sheets [29], while CO2 adsorption of approximately 1.1 mmol/g was exhibited by BN pellets at 298 K [35]. On the basis of previous reports, we can conclude that CO2 capture by porous BN materials is relatively low. Therefore, future research in this area should focus on the development of porous BN materials that show greater CO2 adsorption ability. An efficient way to synthesize porous BN materials involves the decomposition reaction of boron and nitrogen reagents in the presence of additives for the induction of porosity and for structure directing purposes (CTAB and P123 copolymer) [36,37].
The research presented herein focuses on the development of unique carbon containing highly porous activated BN whiskers (CBNW) that exhibit high CO2 uptake ability. The activated porous CBNW were fabricated in the presence of triblock copolymer P123 [polyethylene glycol)-block-polypropylene glycol)-block-poly(ethylene glycol)] as a structure directing agent via structure directing methodology. The influence of P123 copolymer on the specific surface area and porosity of the synthetic materials and the resulting effect on the CO2 adsorption capacity of the materials were evaluated. The results show that a specified concentration of P123 copolymer in CBNW proved very efficient in improving CO2 uptake by increasing the microporosity and specific surface area of the material.

2. Experimental

2.1. Materials

Boric acid (H3BO3) was purchased from Duksan pure chemicals, Ansan, South Korea. Melamine (C3N6H6) was bought from Sigma Aldrich, St. Louis, MO, USA. Triblock copolymer P123 [polyethylene glycol)-block-polypropylene glycol)-block-poly(ethylene glycol)] with an average molecular weight of approximately 5800 was purchased from Sigma Aldrich, Riedstr, Germany. HNO3 (60% purity) was purchased from DAEJUNG KOSDAQ, Siheung-si, South Korea. All these chemicals were used as received without further purification.

2.2. Synthesis of P123 Activated Porous Carbon Containing BN Whiskers (P123-CBNW)

A brief schematic layout of the adsorbent synthesis is shown in Figure 1. First, 3.73 g of H3BO3 was dissolved in 250 mL of distilled water, then melamine (3.78 g) was slowly added with vigorous stirring. The pH of the mixture was kept at approximately pH 6 with 0.1 M HNO3. Next, 5 g of P123 copolymer was added to the reaction mixture at 90 °C under continuous stirring to produce a uniform solution. This mixture was allowed to react at the same conditions for 6 h after which the mixture was cooled to ambient temperature and the white product was collected by vacuum filtration and washed with cold distilled water. After drying at 100 °C for 8 h, the prepared powder was activated by pyrolytic treatment; in this case the white precipitates were calcined at low temperature (900 °C) for 4 h under N2 atmosphere with a flow rate of 150 mL/min to control carbon incorporation. The prepared product was abbreviated as P123-CBNW1. Other samples were prepared under the same conditions with half (2.5 g), double (10 g), and triple (15 g) the amount of P123 copolymer, designated as P123-CBNW0.5, P123-CBNW2, and P123-CBNW3, respectively, while the product fabricated without P123 copolymer was denoted as CBNW.

2.3. Characterization

The size and morphological analysis of the prepared materials was performed by high resolution scanning electron microscopy (HR-SEM; Model-SU8010, Hitachi Co. Ltd., Tokyo, Japan) at 1 kV and by transmission electron microscopy (TEM, JEM-2100F, JEOL, Tokyo, Japan). The thermal stability was assessed by thermo-gravimetric analysis (TGA; Model TG-209F3, NETZSCH, Bavarian, Germany). The functional group predictions were confirmed by Fourier transform infrared vacuum spectrometry (FTIR, Vertex- 80 V, Bruker, Billerica, MA, USA) wherein the spectra were obtained in the scanning range of 4000–400 cm−1. The X-ray diffraction peaks were obtained in the range of 2 theta angle (8–80°) using powder X-ray diffractometry (XRD, D-2 Phaser, Bruker Co, Panalytical Incorporated, Netherland). Elemental analysis was performed by Elemental-analyzer EA1112 (ThermoFisher scientific, Seoul, Korea). The surface properties were investigated by X-ray photoelectron spectroscopy (XPS, K-α, VG Scientific Co., Waltham, MA, USA) with monochromatic Mg Kα X-rays running at 150 W. Furthermore, the specific surface area, pore size distribution, and diameter of materials was obtained by N2 gas adsorption/desorption analysis using the instrument Belsorp Max (BEL-Japan). The target gas (CO2) capturing ability of the materials at different temperatures (273 K, 283 K, and 298 K) were also assessed with the Belsorp Max system (BEL-Japan Inc.). Prior to gas adsorption experiments, residual moisture in all samples was removed by degassing at 200 °C under vacuum for 6 h.

3. Results and Discussions

3.1. Structural and Morphological Analysis

The morphology of the prepared adsorbents was studied using HR-SEM and TEM at different micrometer and nanometer magnifications. The HR-SEM images in Figure 2a–e shows that CBNW and P123-CBNW samples exhibit disordered whisker-like non-uniform structures [38]. The TEM micrograph in Figure 2f shows the CBNW sample possessed minimum porosity; however, Figure 2g–h shows the poor crystalline nature of the adsorbents which is congruent with the XRD results. The insets indicate the porosity in P123-CBNW adsorbents introduced with P123-copolymer. The minimum size of the prepared samples was 100 nm. This type of disordered structure contributes to the porosity of the P123-CBNW materials [16]. The inset images show a close view of the material surface (200 nm resolution) displaying the highly porous nature generated by the activating agent during heat treatment. This is expected to play a significant role in enhancing the CO2 adsorption ability of the material [39].
Additionally, TGA of prepared adsorbents was performed in an air atmosphere (rate = 10 °C/min) in order to determine the thermal stability and carbon content of the materials (Figure 3). The initial mass loss (5%) for all adsorbents below 106 °C is due to the elimination of residual solvent and moisture adsorbed on the material surface. It was noted that mass loss from 150–800 °C (for samples CBNW, P123-CBNW0.5, P123-CBNW1) and from 150–500 °C (for samples P123-CBNW2, P123-CBNW3) indicated the incorporation of carbon content within the samples, which undergoes combustion on raising the temperature. This weight loss can also be attributed to the removal of oxygen functionalities from the materials [40,41]. However, P123-CBNW2 and P123-CBNW3 undergoes stabilization above 500 °C.
The FTIR spectra in Figure 4a indicate the presence of functional groups and the nature of the bonds found within the prepared samples. The sharp shoulder at 1366 cm−1 and small peak at 794 cm−1 are attributed to two types of B–N stretching; the former value indicates in-plane B–N transverse stretching and the latter is indicative of above plane B–N–B bonds [42,43]. However, in P123 copolymer activated products the additional small shoulders at 983 and 692 cm−1 correspond to C–N, C–H, and B–N–O bonds, respectively [44,45,46]. The structure of the samples was further analyzed by XRD analysis. As mentioned in Figure 4b, an indiscernible peak appearing at 23° with low intensity shows plan phases of [002], indicating the existence of carbonaceous content in the prepared materials. Other peaks, at 43° with a phase index of [100] and at 61°, were attributed to poor crystallinity and defective structure, as confirmed by HR-SEM and TEM micrographs. These defects were due to the nanometer size of the whiskers [38] resulting in a turbostratic morphology, a type of shape found among hexagonal and amorphous materials [47,48].
The results of the elemental analysis are presented in Table 1. It was observed that carbon content increased from 14.99% (P123-CBNW0.5) to 25.12% (P123-CBNW3) due to the increasing amount of P123 copolymer.
The chemical environment of the atoms above the surface of the samples was characterized by XPS. In Figure 5a,d,g), the C1s deconvoluted scans of CBNW, P123-CBNW0.5, and P123-CBNW3 presented five binding energies. The high intensity peak at 283 eV in C1s is due to C–C bonds while the binding energies at around 285 and 286 eV correspond to the B–C–N2 and C–N3 bonds. The two remaining low intensity peaks in the region of 286–289 eV correspond to C–O species [49,50,51]. The scans of B1s (Figure 5b,e,h) demonstrated the deconvolution in to three main species; the first two relative peaks at 189 and 190 eV indicated B–N3 and O–B–N2 type binding. The other peak at approximately 192 eV corresponds to O2–B–N or O2–B–C species [52,53]. Furthermore, the N1s spectra of all adsorbents mentioned in Figure 5c,f,i exhibited a main peak at 397 eV corresponding to N–B3 type bonds. The remaining peak at 398 eV is attributed to N–C binding, while signals at 399 eV originate from N–H/N–O type bonding [54]. Therefore, the existence of C–C, C–N, and B–C–N bonds confirmed the presence of carbon in the boron nitride whiskers.

3.2. Textural Analysis

The textural analyses of CBNW and P123 copolymer activated adsorbents were obtained by nitrogen adsorption/desorption isotherms at 77 K. Prior to measurement, samples were degassed at 200 °C for 6 h under high vacuum conditions. Figure 6 illustrates the resulting isotherms and pore size distributions obtained by the non-local density functional theory equation (NLDFT). The shape of the isotherm indicated a IV type structure, which confirmed the existence of micro- and mesoporous structures that are linked via capillary condensation.
The calculated numerical parameters, including specific surface area, total pore volume, micropore volume, and mesopore volume, are summarized in Table 2. It was noted that a minimum concentration of P123 copolymer plays a vital role in increasing the specific surface area of the fabricated materials (CBNW = 594 m2/g, P123-CBNW0.5 = 1732 m2/g). However, it was observed that a greater increase in the ratio of P123 copolymer lead to a decrease in specific surface area from 1281 m2/g (P123-CBNW1) to 764 m2/g (P123-CBNW3); concurrently, pore volume also declined due to inaccessibility of the pores to N2 due to blockage by excess activating agent (P123 copolymer) [55].
The maximum recorded specific surface area is much higher than that of the previously synthesized porous BN material (817 m2/g) [56]. The highest microporosity (0.67 cm2/g) was seen for P123-CBNW0.5 and it decreased as the activating agent ratio increased (P123-CBNW3 = 0.33 cm2/g) [57,58]. The pore volumes of prepared specimens were calculated by the Dubinin Radushkevich equation (Equation 1).
W = W o exp   [ − B ( T β ) l o g 2 ( p p o ) ]
Therefore, it can be summarized that the introduction of a quantified amount of P123 copolymer during fabrication is invaluable to the attenuation of the porous morphology and specific surface area of the resulting materials [59].

3.3. Gas Capture Analysis

The fabricated CBNW and P123-CBNW materials possessed higher specific surface areas and different micro- and mesoporous structures with various pore sizes. These properties enable us to evaluate their efficiency of CO2 uptake. Figure 7a–c presents the CO2 adsorption/desorption isotherms of samples collected at 273, 283, and 298 K at 1 bar while whole adsorption values are summarized in Table 3. CBNW shows a CO2 adsorption capacity of 136.2 mg/g at 273 K which increased with the addition of P123 copolymer (308.7 mg/g for P123-CBNW0.5) due to the high specific surface area, greater total pore volume, and increased microporosity of the polymer modified sample. In contrast, CO2 capture ability dropped from 270.5 mg/g (P123-CBNW1) to 190.2 mg/g (P123-CBNW3) with the continued increase in P123 copolymer. This decline in gas storage capacity occurred because of the following reasons: (1) decrease in micropore volume, and (2) lower specific surface area [35]. When considering the influence of temperature on CO2 uptake, it was observed that at 298 K, a clear decline in gas uptake occurred plateauing at 97.6, 203.6, 155.8, 134.2, and 114.8 mg/g for CBNW, P123-CBNW0.5, P123-CBNW1, P123-CBNW2, and P123-CBNW3, respectively. This trend depicts an exothermic adsorption phenomenon, wherein the CO2 capturing ability is inversely related to the adsorption temperature [60,61].
It is well-known that the important challenge is to adsorb CO2 gas at low pressure, however the high porous nature and functionality above the adsorbents provide enough active gas capturing centers to take acidic CO2 at low pressure (1 bar). In order to clearly understand the mechanism and reasons by which P123-CBNW adsorbents shows higher adsorption ability, it can be noted that the following two features attributed to the above mentioned results; (1) the porous morphology possesses strong merits for higher capture of CO2 molecules, however mesoporosity provides little resistance for adsorption of CO2 molecules, on the other hand higher microporosity provides a greater number of active sites for capturing CO2 easily. (2) the dual functionality –NH2 (attached to carbon) and –OH (attached to boron) also able the CO2 adsorption ability to be enhanced. The physiosorption of CO2 in-plane sites (functional groups) of adsorbents extensively based on vander waal interaction, that existed on the top sites of boron or nitrogen atoms as well as onto the bridges sites of B–N linkage [62,63].
In order to further investigate the nature of the adsorption process and the interaction between CO2 and the adsorbent materials, the Clausius–Clapeyron equation (Equation (2)) was applied to gas adsorption/desorption isotherms obtained at 273 and 298 K to calculate their isosteric heat of adsorption (∆Hads/∆Qst) [64].
Q s t = R   [ ∂ l n P ∂ ( 1 T   ) ]   θ
While, P is pressure, R denotes real gas constant, T is adsorption temperature, and θ indicates the fraction of adsorbed sites. As presented in Figure 7d and Table 3, the calculated Qst values determined for CO2 were 43.7, 36.7, 40.4, 37.6, and 33.7 kJ/mol for 5 mg of CBNW, P123-CBNW0.5, P123-CBNW1, P123-CBNW2, and P123-CBNW3, respectively. These small values correspond to a physisorption type of CO2 capture for the aforementioned adsorbent materials. As the CO2 adsorption capacity increased, the heat of adsorption declined due to the heterogeneous nature of the adsorption sites [16].
While selecting effective adsorbents for maximum CO2 capturing capacity, we also considered the selectivity over other gases such as N2 and CH4. That is, if the adsorbents showed excellent capacity for the uptake of all tested gases simultaneously, they were considered unsuitable for CO2 capture. Herein, we also assessed the CO2/N2 selectivity of the prepared materials at 273 and 298 K (1 bar) as seen in Figure 8a–c. The N2 adsorption capacity was very low as compared to CO2 adsorption at both temperatures (at 1 bar). Both the ideal adsorbed solution theory (IAST) method and Henry’s law were applied to find the CO2/N2 selectivity by adsorbents. The equilibrium selectivity of CO2 gas (X) over N2 gas (Y) on the adsorbents was calculated by the ratio of the initial slopes obtained by Henry’s law as shown in following equation,
S x , y = K x K y
Kx and Ky represent the slope obtained from the single isotherm of CO2 and N2 gas. However, IAST calculations was performed by fitting the specific model; in this case one site and double site Langmuir Freundlich models has been applied to compare the pure-adsorbent equilibrium data and identify the adsorption of gas mixture. The calculated adsorption selectivities at 1 bar by Henry’s law were 44.89 (CBNW), 37.81 (P123-CBNW0.5), 40.43 (P123-CBNW1), 43.91 (P123-CBNW2), and 41.13 (P123-CBNW3) at 273 K and 52.82 (CBNW), 37.92 (P123-CBNW0.5), 46.42 (P123-CBNW1), 43.23 (P123-CBNW2), and 64.58 (P123-CBNW3) at 298 K for CO2 over N2. However, by the IAST method the investigated selectivities were 118.97, 65.07, 70.3, 76, 95.12 at 273 K (1 bar) and 117.03, 61.75, 98.69, 89.13, 224.97 at 298 K (1 bar) for samples CBNW, P123-CBNW0.5, P123-CBNW1, P123-CBNW2, and P123-CBNW3 respectively. The IAST plots are presented in Figure 9a–e. The higher CO2 gas selectivity of the carbon containing BN samples was due to the physisorption attraction of the polar B–N bond towards the acidic CO2 gas. This covalent polar bond and highly porous nature of the materials enhanced their affinity towards CO2; in contrast, other carbon-based materials did not exhibit the same abilities [65,66]. From an economical point of view, we also focused on the regenerative ability of the prepared adsorbents. In this study, we examined this aspect of the adsorbents by performing four repeated CO2 adsorption cycles at 298 K and 1 bar (Figure 8d). The results indicated that the prepared samples exhibited high potential for regeneration and recyclability, thus making the adsorbents promising candidates for gas storage applications.

4. Conclusions

In this work, we successfully fabricated highly microporous and mesoporous carbon containing P123-CBNW adsorbents. This was accomplished through a structure directed approach using boric acid and melamine as boron and nitrogen precursors along with a triblock copolymer as an activating agent followed by a single step pyrolytic heat treatment under a N2 atmosphere. The prepared P123-CBNW0.5 and P123-CBNW1 adsorbents exhibited high micro- and mesoporosity, structural chemical defects, and high specific surface areas (1732 and 1281 m2/g, respectively), which are responsible for the increase in CO2 adsorption ability (308 and 270 mg/g, respectively) as compared to CBNW (136 mg/g) at 273 K and 1 bar. All prepared materials exhibited high selectivity for CO2 over N2. The CO2 capture ability of the materials increased in the order of CBNW < P123-CBNW3 < P123-CBNW2 < P123-CBNW1 < P123-CBNw0.5 and the aforementioned samples possessed higher CO2 adsorption capacity than previously reported materials (Table 4). On the basis of our reported work, it was demonstrated that the adsorption ability can be increased by altering the microporosity and surface area of the adsorbents through the addition of a minor amount of activating agent. The adsorbents show excellent regeneration ability after several repeated adsorption cycles. Therefore, these reported materials prove to be very efficient for future gas storage applications.

Author Contributions

Funding acquisition, S.-J.P.; Investigation, U.K.; Methodology, U.K.; Software, U.K.; Supervision, S.-J.P.; Writing—original draft, U.K.; Writing—review & editing, U.K., K.Y.R. and S.-J.P.

Acknowledgments

This work was supported by the Technology Innovation Program (or Industrial Strategic Technology Development Program (10080293, Development of carbon-based non phenolic electrode materials with 3,000 m2/g grade surface area for energy storage device) funded by the Ministry of Trade, Industry & Energy (MOTIE, Korea) and the Commercialization Promotion Agency for R&D Outcomes (COMPA) funded by the Ministry of Science and ICT (MSIT) [2018_RND_002_0064, Development of 800 mA·h·g−1 pitch carbon coating materials].

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Miti’c, P.; Munitlak Ivanovi’c, O.; Zdravkovi’c, A. A cointegration analysis of real GDP and CO2 emissions in transitional countries. Sustainability 2017, 9, 568. [Google Scholar] [CrossRef]
  2. Raupach, M.R.; Marland, G.; Ciais, P.; Le Quéré, C.; Canadell, J.G.; Klepper, G.; Field, C.B. Global and regional drivers of accelerating CO2 emissions. Proc. Natl. Acad. Sci. USA 2007, 104, 10288–10293. [Google Scholar] [CrossRef]
  3. Samanta, A.; Zhao, A.; Shimizu, G.K.H.; Sarkar, P.; Gupta, R. Post-combustion CO2 capture using solid sorbents: A review. Ind. Eng. Chem. Res. 2012, 51, 1438–1463. [Google Scholar] [CrossRef]
  4. Bollini, P.; Didas, S.A.; Jones, C.W. Amine-oxide hybrid materials for acid gas separations. J. Mater. Chem. 2011, 21, 15100–15120. [Google Scholar] [CrossRef]
  5. Kuwahara, Y.; Kang, D.Y.; Copeland, J.R.; Brunelli, N.A.; Didas, S.A.; Bollini, P.; Sievers, C.; Kamegawa, T.; Yamashita, H.; Jones, C.W. Dramatic enhancement of CO2 uptake by poly(ethyleneimine) using zirconosilicate supports. J. Am. Chem. Soc. 2012, 134, 10757–10760. [Google Scholar] [CrossRef]
  6. McGee, M. Earth CO2 Homepage. Available online: https://www.CO2.earth/ (accessed on 20 January 2017).
  7. Zhou, X.; Yi, H.; Tang, X.; Deng, H.; Liu, H. Thermodynamics for the adsorption of SO2, NO and CO2 from flue gas on activated carbon fiber. Chem. Eng. J. 2012, 200, 399–404. [Google Scholar] [CrossRef]
  8. Olajire, A.A. CO2 capture and separation technologies for end-of-pipe applications—A review. Energy 2010, 35, 2610–2628. [Google Scholar] [CrossRef]
  9. Pires, J.C.M.; Martins, F.G.; Simões, M. Chemical engineering research and design recent developments on carbon capture and storage: An overview. Chem. Eng. Res. Des. 2011, 89, 1446–1460. [Google Scholar] [CrossRef]
  10. Gray, M.L.; Champagne, K.J.; Fauth, D.; Baltrus, J.P.; Pennline, H. Performance of immobilized tertiary amine solid sorbents for the capture of carbon dioxide. Int. J. Greenh. Gas Con. 2008, 2, 3–8. [Google Scholar] [CrossRef]
  11. Luis, P. Use of monoethanolamine (MEA) for CO2 capture in a global scenario: Consequences and alternatives. Desalination 2016, 380, 93–99. [Google Scholar] [CrossRef]
  12. Puthiaraj, P.; Lee, Y.R.; Ahn, W.S. Microporous amine-functionalized aromatic polymers and their carbonized products for CO2 adsorption. Chem. Eng. J. 2017, 319, 65–74. [Google Scholar] [CrossRef]
  13. Puthiaraj, P.; Ahn, W.S. Facile synthesis of microporous carbonaceous materials derived from a covalent triazine polymer for CO2 capture. J. Energy Chem. 2017, 26, 965–971. [Google Scholar] [CrossRef]
  14. Puthiaraj, P.; Ahn, W.S. CO2 Capture by porous hyper-cross-linked aromatic polymers synthesized using tetrahedral precursors. Ind. Eng. Chem. Res. 2015, 55, 7917–7923. [Google Scholar] [CrossRef]
  15. Marchesini, S.; Regoutz, A.; Payne, D.; Petit, C. Tunable porous boron nitride: Investigating its formation and its application for gas adsorption. Micropor. Mesopor. Mater. 2017, 243, 154–163. [Google Scholar] [CrossRef] [Green Version]
  16. Chen, S.; Li, P.; Xu, S.; Pan, X.; Fu, Q.; Bao, X. Carbon doping of hexagonal boron nitride porous materials toward CO2 capture. J. Mater. Chem. A 2018, 6, 1832–1839. [Google Scholar] [CrossRef]
  17. Ren, J.; Wu, L.; Li, B.G. Preparation and CO2 sorption/desorption of N-(3-aminopropyl) aminoethyl tributylphosphonium amino acid salt ionic liquids supported into porous silica particles. Ind. Eng. Chem. Res. 2012, 51, 7901–7909. [Google Scholar] [CrossRef]
  18. Heo, Y.J.; Le, M.U.T.; Park, S.J. Investigation of carbon dioxide adsorption by nitrogen-doped carbons synthesized from cubic MCM-48 mesoporous silica. Carbon Lett. 2016, 18, 62–66. [Google Scholar] [CrossRef] [Green Version]
  19. Rehman, A.; Park, S.J. Facile synthesis of nitrogen-enriched microporous carbons derived from imine and benzimidazole-linked polymeric framework for efficient CO2 adsorption. J. CO2 Util. 2017, 21, 503–512. [Google Scholar] [CrossRef]
  20. Heo, Y.J.; Park, S.J. A role of steam activation on CO2 capture and separation of narrow microporous carbons produced from cellulose fibers. Energy 2015, 91, 142–150. [Google Scholar] [CrossRef]
  21. Rehman, A.; Park, S.J. Comparative study of activation methods to design nitrogen-doped ultra-microporous carbons as efficient contenders for CO2 capture. Chem. Eng. J. 2018, 352, 539–548. [Google Scholar] [CrossRef]
  22. Yaghi, O.M.; Millward, A.R. Metal-organic frameworks with exceptionally high capacity for storage of carbon dioxide at room-temperature. JACS 2005, 127, 17998–17999. [Google Scholar]
  23. Trickett, C.A.; Helal, A.; Al-Maythalony, B.A.; Yamani, Z.H.; Cordova, K.E.; Yaghi, O.M. The chemistry of metal–organic frameworks for CO2 capture, regeneration and conversion. Nat. Rev. Mater. 2017, 2, 17045. [Google Scholar] [CrossRef]
  24. Wang, Q.; Tay, H.H.; Zhong, Z.; Luo, J.; Borgna, A. Synthesis of high-temperature CO2 adsorbents from organo-layered double hydroxides with markedly improved CO2 capture capacity. Energy Environ. Sci. 2012, 5, 7526–7530. [Google Scholar] [CrossRef]
  25. Ravi, S.; Puthiaraj, P.; Ahn, W.S. Hydroxylamine-anchored covalent aromatic polymer for CO2 adsorption and fixation into cyclic carbonates. ACS Sustain. Chem. Eng. 2018, 6, 9324–9332. [Google Scholar] [CrossRef]
  26. Heo, Y.J.; Park, S.J. Facile synthesis of MgO-modified carbon adsorbents with microwave-assisted methods: Effect of MgO particles and porosities on CO2 capture. Sci. Rep. 2017, 7, 5653. [Google Scholar] [CrossRef]
  27. Jiang, X.-F.; Weng, Q.; Wang, X.-B.; Li, X.; Zhang, J.; Golberg, D.; Bando, Y. Recent progress on fabrications and applications of boron nitride nanomaterials: A review. J. Mater. Sci. Technol. 2015, 31, 589–598. [Google Scholar] [CrossRef]
  28. Lin, Y.; Connell, J.W. Advances in 2D boron nitride nanostructures: Nanosheets, nanoribbons, nanomeshes, and hybrids with graphene. Nanoscale 2012, 4, 6908–6939. [Google Scholar] [CrossRef]
  29. Xiao, F.; Chen, Z.; Casillas, G.; Richardson, C.; Li, H.; Huang, Z. Controllable synthesis of few-layered and hierarchically porous boron nitride nanosheets. Chem. Commun. 2016, 52, 3911–3914. [Google Scholar] [CrossRef] [Green Version]
  30. Zhang, Y.; Choi, J.R.; Park, S.J. Thermal conductivity and thermo-physical properties of nanodiamond-attached exfoliated hexagonal boron nitride/epoxy nanocomposites for microelectronics. Compos. Part A Appl. Sci. Manuf. 2017, 101, 227–236. [Google Scholar] [CrossRef]
  31. Zhang, Y.; Choi, J.R.; Park, S.J. Enhancing the heat and load transfer efficiency by optimizing the interface of hexagonal boron nitride/elastomer nanocomposites for thermal management applications. Polymer 2018, 143, 1–9. [Google Scholar] [CrossRef]
  32. Zhi, C.Y.; Bando, Y.; Tang, C.C.; Kuwahara, H.; Golberg, D. Large-scale fabrication of boron nitride nanosheets and their utilization in polymeric composites with improved thermal and mechanical properties. Adv. Mater. 2009, 21, 2889–2893. [Google Scholar] [CrossRef]
  33. Li, J.; Lin, J.; Xu, X.; Zhang, X.; Xue, Y.; Mi, J.; Mo, Z.; Fan, Y.; Hu, L.; Yang, X. Porous boron nitride with a high surface area: Hydrogen storage and water treatment. Nanotechnology 2013, 24, 155603. [Google Scholar] [CrossRef]
  34. Li, J.; Huang, Y.; Liu, Z.; Zhang, J.; Liu, X.; Luo, H.; Ma, Y.; Xu, X.; Lu, Y.; Lin, J.; et al. Chemical activation of boron nitride fibers for improved cationic dye removal performance. J. Mater. Chem. A 2015, 3, 8185–8193. [Google Scholar] [CrossRef]
  35. Marchesini, S.; McGilvery, C.M.; Bailey, J.; Petit, C. Template-free synthesis of highly porous boron nitride: Insights into pore network design and impact on gas sorption. ACS Nano 2017, 11, 10003–10011. [Google Scholar] [CrossRef]
  36. Schlienger, S.; Alauzun, J.; Michaux, F.; Vidal, L.; Parmentier, J.; Gervais, C.; Babonneau, F.; Bernard, S.; Miele, P.; Parra, J. Micro,mesoporous boron nitride-based materials templated from zeolites. Chem. Mater. 2011, 24, 88–96. [Google Scholar] [CrossRef]
  37. Dibandjo, P.; Bois, L.; Chassagneux, F.; Miele, P. Thermal stability of mesoporous boron nitride templated with a cationic surfactant. J. Eur. Ceram. Soc. 2007, 27, 313–317. [Google Scholar] [CrossRef]
  38. Luo, W.; Yang, T.; Su, L.; Chou, K.C.; Hou, X. Preparation of hexagonal BN whiskers synthesized at low temperature and their application in fabricating an electrochemical nitrite sensor. RSC Adv. 2016, 6, 27767–27774. [Google Scholar] [CrossRef]
  39. Li, Q.; Yang, T.; Yang, Q.; Wang, F.; Chou, K.C.; Hou, X. Porous hexagonal boron nitride whiskers fabricated at low temperature for effective removal of organic pollutants from water. Ceram. Int. 2016, 42, 8754–8762. [Google Scholar] [CrossRef]
  40. Huang, C.; Chen, C.; Zhang, M.; Lin, L.; Ye, X.; Lin, S.; Antonietti, M.; Wang, X. Carbon-doped BN nanosheets for metal-free photoredox catalysis. Nat. Commun. 2015, 6, 7698. [Google Scholar] [CrossRef] [Green Version]
  41. Rushton, B.; Mokaya, R. Mesoporous boron nitride and boron-nitride-carbon materials from mesoporous silica templates. J. Mater. Sci. 2008, 18, 235–241. [Google Scholar] [CrossRef]
  42. Shankar, R.; Hankin, A.; Petit, C. Porous boron nitride for combined CO2 capture and photoreduction. ChemRxiv 2018. [Google Scholar] [CrossRef]
  43. Kumari, S.; Sharma, O.P.; Gusain, R.; Mungse, H.P.; Kukrety, A.; Kumar, N.; Sugimura, H.; Khatri, O.P. Alkyl-chain-grafted hexagonal boron nitride nanoplatelets as oil-dispersible additives for friction and wear reduction. ACS Appl. Mater. Interfaces 2015, 7, 3708–3716. [Google Scholar] [CrossRef]
  44. Goyal, R.; Sarkar, B.; Bag, A.; Lefebvre, F.; Sameer, S.; Pendem, C.; Bordoloi, A. Single-step synthesis of hierarchical Bx CN: A metal-free catalyst for low-temperature oxidative dehydrogenation of propane. J. Mater. Chem. A 2016, 4, 18559–18569. [Google Scholar] [CrossRef]
  45. Sudeep, P.M.; Vinod, S.; Ozden, S.; Sruthi, R.; Kukovecz, A.; Konya, Z.; Vajtai, R.; Anantharaman, M.R.; Ajayan, P.M.; Narayanan, T.N. Functionalized boron nitride porous solids. RSC Adv. 2015, 5, 93964–93968. [Google Scholar] [CrossRef]
  46. Li, J.; Xiao, X.; Xu, X.; Lin, J.; Huang, Y.; Xue, Y.; Jin, P.; Zou, J.; Tang, C. Activated boron nitride as an effective adsorbent for metal ions and organic pollutants. Sci. Rep. 2013, 3, 3208. [Google Scholar] [CrossRef]
  47. Park, H.; Kim, T.K.; Cho, S.W.; Jang, H.S.; Lee, S.I.; Choi, S.Y. Large-scale synthesis of uniform hexagonal boron nitride films by plasma-enhanced atomic layer deposition. Sci. Rep. 2017, 7, 40091. [Google Scholar] [CrossRef] [PubMed] [Green Version]
  48. Thomas, J.; Weston, N.; O’connor, T. Turbostratic1 boron nitride, thermal transformation to ordered-layer-lattice boron nitride. JACS 1962, 84, 4619–4622. [Google Scholar] [CrossRef]
  49. Dong, G.; Jacobs, D.L.; Zang, L.; Wang, C. Carbon vacancy regulated photoreduction of NO to N2 over ultrathin g-C3N4 nanosheets. Appl. Catal. B 2017, 218, 515–524. [Google Scholar] [CrossRef]
  50. Beniwal, S.; Hooper, J.; Miller, D.P.; Costa, P.S.; Chen, G.; Liu, S.-Y.; Dowben, P.A.; Sykes, E.C.H.; Zurek, E.; Enders, A. Graphene-like boron–carbon–nitrogen monolayers. ACS Nano 2017, 11, 2486–2493. [Google Scholar] [CrossRef]
  51. Li, D.; Chen, Y.; Zheng, M.; Zhao, H.; Zhao, Y.; Sun, Z. Hierarchically structured porous nitrogen-doped carbon for highly selective CO2 capture. Sustain. Chem. Eng. 2016, 4, 298–304. [Google Scholar] [CrossRef]
  52. Prakash, A.; Sundaram, K.B. Optical and XPS studies of BCN thin films by co-sputtering of B4C and BN targets. Appl. Surf. Sci. 2017, 396, 484–491. [Google Scholar] [CrossRef]
  53. Tabassum, H.; Zou, R.; Mahmood, A.; Liang, Z.; Guo, S. A catalyst-free synthesis of B, N co-doped graphene nanostructures with tunable dimensions as highly efficient metal free dual electrocatalysts. J. Mater. Chem. A 2016, 4, 16469–16475. [Google Scholar] [CrossRef]
  54. Xue, Y.; Dai, P.; Jiang, X.; Wang, X.; Zhang, C.; Tang, D.; Weng, Q.; Wang, X.; Pakdel, A.; Tang, C.; et al. Template-free synthesis of boron nitride foam-like porous monoliths and their high-end applications in water purification. J. Mater. Chem. A 2016, 4, 1469–1478. [Google Scholar] [CrossRef]
  55. Subagyono, D.J.N.; Marshall, M.; Knowles, G.P.; Chaffee, A.L. CO2 adsorption by amine modified siliceous mesostructured cellular foam (MCF) in humidified gas. Micropor. Mesopor. Mat. 2014, 186, 84–96. [Google Scholar] [CrossRef]
  56. Wang, J.; Hao, J.; Liu, D.; Qin, S.; Portehault, D.; Li, Y.; Chen, Y.; Lei, W. Porous boron carbon nitride nanosheets as efficient metal-free catalysts for the oxygen reduction reaction in both alkaline and acidic solutions. ACS Energy Lett. 2017, 2, 306–312. [Google Scholar] [CrossRef]
  57. Lee, M.S.; Lee, S.Y.; Park, S.J. Preparation and characterization of multi-walled carbon nanotubes impregnated with polyethyleneimine for carbon dioxide capture. Int. J. Hydrog. Energy 2015, 40, 3415–3421. [Google Scholar] [CrossRef]
  58. Puthiaraj, P.; Kim, S.S.; Ahn, W.S. Covalent triazine polymers using a cyanuric chloride precursor via Friedel–Crafts reaction for CO2 adsorption/separation. Chem. Eng. J. 2016, 283, 184–192. [Google Scholar] [CrossRef]
  59. Groen, J.C.; Peffer, L.A.A.; Pe’rez-Ramı’rez, J. Pore size determination in modified micro- and mesoporous materials. Pitfalls and limitations in gas adsorption data analysis. Micropor. Mesopor. Mater. 2003, 60, 1–17. [Google Scholar] [CrossRef]
  60. Hsu, S.C.; Lu, C.; Su, F.; Zeng, W.; Chen, W. Thermodynamics and regeneration studies of CO2 adsorption on multiwalled carbon nanotubes. Chem. Eng. Sci. 2010, 65, 1354–1361. [Google Scholar] [CrossRef]
  61. Weng, Q.; Wang, X.; Bando, Y.; Golberg, D. One-step template-free synthesis of highly porous boron nitride microsponges for hydrogen storage. Adv. Energy Mater. 2014, 4, 1301525. [Google Scholar] [CrossRef]
  62. Yang, C.; Wang, J.; Chen, Y.; Liu, D.; Huang, S.; Lei, W. One-step template-free synthesis of 3D functionalized flower-like boron nitride nanosheets for NH3 and CO2 adsorption. Nanoscale 2018, 10, 10979–10985. [Google Scholar] [CrossRef]
  63. Yang, C.; Liu, D.; Chen, Y.; Chen, C.; Wang, J.; Fan, Y.; Huang, S.; Lei, W. 3D Functionalized Boron Nitride Nanosheets/ZnO Superstructures for CO2 Capture. ACS Appl. Mater. Interfaces 2019, 11, 10276–10282. [Google Scholar] [CrossRef]
  64. Pan, H.; Ritter, J.A.; Balbuena, P.B. Examination of the approximations used in determining the isosteric heat of adsorption from the Clausius-Clapeyron equation. Langmuir 1998, 14, 6323–6327. [Google Scholar] [CrossRef]
  65. Song, L.; Ci, J.; Lu, H.; Sorokin, P.B.; Jin, C.H.; Ni, J.; Kvashnin, A.G.; vashnin, D.G.; Lou, J.; Yakobson, B.I.; et al. Large scale growth and characterization of atomic hexagonal boron nitride layers. Nano Lett. 2010, 10, 3209–3215. [Google Scholar] [CrossRef]
  66. Marom, N.; Bernstein, J.; Garel, J.; Tkatchenko, A.; Joselevich, E.; Kronik, L.; Hod, O. Stacking and registry effects in layered materials: The case of hexagonal boron nitride. Phys. Rev. Lett. 2010, 105, 046801. [Google Scholar] [CrossRef]
  67. Heo, Y.J.; Park, S.J. H2O2/steam activation as an eco-friendly and efficient top-down approach to enhancing porosity on carbonaceous materials: The effect of inevitable oxygen functionalities on CO2 capture. Green Chem. 2018, 20, 5224–5234. [Google Scholar] [CrossRef]
  68. Singh, M.G.; Lakhi, K.S.; Park, D.H.; Srivastava, P.; Naidu, R.; Vinu, A. Facile one-pot synthesis of activated porous biocarbons with a high nitrogen content for CO2 capture. ChemNanoMat 2018, 4, 281–290. [Google Scholar] [CrossRef]
  69. Shen, W.; Zhang, S.; He, Y.; Li, J.; Fan, W. Hierarchical porous polyacrylonitrile-based activated carbon fibers for CO2 capture. J. Mater. Chem. 2011, 21, 14036–14040. [Google Scholar] [CrossRef]
  70. Singh, G.; Lakhi, K.S.; Ramadass, K.; Kim, S.; Stockdale, D.; Vinu, A. Combined strategy of acid-assisted polymerization and solid state activation to synthesize functionalized nanoporous activated biocarbons from biomass for CO2 capture. Micropor. Mesopor. Mater. 2018, 271, 23–32. [Google Scholar] [CrossRef]
  71. Bing, X.; Wei, Y.; Wang, M.; Xu, S.; Long, D.; Wang, J.; Qiao, W.; Ling, L. Template-free synthesis of nitrogen-doped hierarchical porous carbons for CO2 adsorption and supercapacitor electrodes. J. Colloid Interface Sci. 2017, 488, 207–217. [Google Scholar] [CrossRef]
  72. Liu, F.-Q.; Wang, L.-L.; Li, G.-H.; Li, W.; Li, C.-Q. Hierarchically structured graphene coupled microporous organic polymers for superior CO2 capture. ACS Appl. Mater. Interfaces 2017, 9, 33997–34004. [Google Scholar] [CrossRef] [PubMed]
Polymers 11 00913 g001 550
Figure 1. Schematic illustration of fabrication of P123 activated carbon containing porous boron nitride (BN) whiskers.
Figure 1. Schematic illustration of fabrication of P123 activated carbon containing porous boron nitride (BN) whiskers.
Polymers 11 00913 g001
Polymers 11 00913 g002 550
Figure 2. HR-SEM micrographs of samples (a) CBNW, (b) P123-CBNW0.5, (c) P123-CBNW1, (d) P123-CBNW2, and (e) P123-CBNW3. TEM images of (f) CBNW, (g) P123-CBNW0.5, (h) P123-CBNW1, (i) P123-CBNW2, and (j) P123-CBNW3. Insets show the high resolution photographs of the adsorbent surface.
Figure 2. HR-SEM micrographs of samples (a) CBNW, (b) P123-CBNW0.5, (c) P123-CBNW1, (d) P123-CBNW2, and (e) P123-CBNW3. TEM images of (f) CBNW, (g) P123-CBNW0.5, (h) P123-CBNW1, (i) P123-CBNW2, and (j) P123-CBNW3. Insets show the high resolution photographs of the adsorbent surface.
Polymers 11 00913 g002
Polymers 11 00913 g003 550
Figure 3. TGA curves of prepared samples in an air atmosphere (10 °C/min).
Figure 3. TGA curves of prepared samples in an air atmosphere (10 °C/min).
Polymers 11 00913 g003
Polymers 11 00913 g004 550
Figure 4. (a) FTIR spectra and (b) XRD patterns of CBNW, P123-CBNW0.5, P123-CBNW1, P123-CBNW2 and P123-CBNW3 samples.
Figure 4. (a) FTIR spectra and (b) XRD patterns of CBNW, P123-CBNW0.5, P123-CBNW1, P123-CBNW2 and P123-CBNW3 samples.
Polymers 11 00913 g004
Polymers 11 00913 g005 550
Figure 5. XPS scan of C1s (a,d,g), B1s (b,e,h), and N1s (c,f,i) of CBNW, P123-CBNW0.5 and P123-CBNW3 respectively.
Figure 5. XPS scan of C1s (a,d,g), B1s (b,e,h), and N1s (c,f,i) of CBNW, P123-CBNW0.5 and P123-CBNW3 respectively.
Polymers 11 00913 g005
Polymers 11 00913 g006 550
Figure 6. (a) N2 adsorption-desorption isotherms of prepared samples at 77 K, (b–f) non-local density functional theory equation (NLDFT)-pore size distribution plots of respective samples.
Figure 6. (a) N2 adsorption-desorption isotherms of prepared samples at 77 K, (b–f) non-local density functional theory equation (NLDFT)-pore size distribution plots of respective samples.
Polymers 11 00913 g006
Polymers 11 00913 g007 550
Figure 7. Adsorption, desorption isotherm of CO2 on prepared adsorbent materials at 273 K (a), 283 K (b), 298 K (c) and heat of adsorption of all materials (d).
Figure 7. Adsorption, desorption isotherm of CO2 on prepared adsorbent materials at 273 K (a), 283 K (b), 298 K (c) and heat of adsorption of all materials (d).
Polymers 11 00913 g007
Polymers 11 00913 g008 550
Figure 8. CO2 and N2 adsorption isotherm plots of CBNW (a), P123-CBNW0.5 (b), P123-CBNW1 (c), P123-CBNW2 (d), P123-CBNW3 (e), at 273 and 298 K for selective adsorption analysis, and (f) adsorption–desorption cycles for adsorbents at 298 K.
Figure 8. CO2 and N2 adsorption isotherm plots of CBNW (a), P123-CBNW0.5 (b), P123-CBNW1 (c), P123-CBNW2 (d), P123-CBNW3 (e), at 273 and 298 K for selective adsorption analysis, and (f) adsorption–desorption cycles for adsorbents at 298 K.
Polymers 11 00913 g008
Polymers 11 00913 g009 550
Figure 9. CO2/N2 selectivity using ideal adsorbed solution theory (IAST) method of CBNW (a), P123-CBNW0.5 (b), P123-CBNW1 (c), P123-CBNW2 (d), and P123-CBNW3 (e) at 273 and 298 K.
Figure 9. CO2/N2 selectivity using ideal adsorbed solution theory (IAST) method of CBNW (a), P123-CBNW0.5 (b), P123-CBNW1 (c), P123-CBNW2 (d), and P123-CBNW3 (e) at 273 and 298 K.
Polymers 11 00913 g009
Table
Table 1. Elemental analyses of the adsorbents fabricated.
Table 1. Elemental analyses of the adsorbents fabricated.
SamplesWeight (%)
C aH bN c
CBNW12.592.6129.62
P123-CBNW0.514.992.4430.41
P123-CBNW116.452.8129.65
P123-CBNW221.342.9225.15
P123-CBNW325.123.0126.54
a Carbon contents. b Hydrogen contents. c Nitrogen contents.
Table
Table 2. Textural properties of prepared materials from N2 isotherms at 77 K.
Table 2. Textural properties of prepared materials from N2 isotherms at 77 K.
MaterialsSBETaVtotalbVmesocVmicrod
CBNW5940.38290.12490.2580
P123-CBNW0.517320.83510.16280.6723
P123-CBNW112810.7180.220.4960
P123-CBNW211280.56060.0850.4756
P123-CBNW37640.44880.11570.3331
a Specific surface area (m2/g) obtained by Brunauer–Emmett–Teller (BET) method. b Total pore volume (cm3/g) calculated at P/P0 = 0.99. c Mesopore volume (cm3/g) analyzed by Barrett-Joyner-Halenda (BJH) method. d Micropore volume (cm3/g) obtained by D-R equation.
Table
Table 3. CO2 and N2 gas uptake by the prepared samples at different temperatures at 1 bar pressure.
Table 3. CO2 and N2 gas uptake by the prepared samples at different temperatures at 1 bar pressure.
SamplesCO2 Uptakes (mg/g)Qst for CO2 (kJ/mol)N2 Uptakes (mg/g)
273 K283 K298 K 273 K298 K
CBNW136.2118.197.643.812.35.3
P123-CBNW0.5308.7265.7203.636.419.811.9
P123-CBNW1270.5193.5155.840.217.68.8
P123-CBNW2232.4165.1134.237.313.17.6
P123-CBNW3190.2154.3114.833.810.76.1
Table
Table 4. Comparative study of CO2 capture capacities of prepared sample with various adsorbents at 273 K and 1 bar.
Table 4. Comparative study of CO2 capture capacities of prepared sample with various adsorbents at 273 K and 1 bar.
AdsorbentsCO2 Uptakes (mmol/g)References
P123-CBNW0.57.01Present work
R-HAC 205.57[67]
BCN (2:1)5.50[16]
NEPB-3UK4.8[68]
CF-850-act4.41[20]
PAN-PK4.40[69]
APAB-34.1[70]
NHPC43.96[71]
PCTP-23.45[57]
SG–MOP-53.37[72]
PHAP-22.37[14]

Share and Cite

MDPI and ACS Style

Kamran, U.; Rhee, K.Y.; Park, S.-J. Effect of Triblock Copolymer on Carbon-Based Boron Nitride Whiskers for Efficient CO2 Adsorption. Polymers 2019, 11, 913. https://doi.org/10.3390/polym11050913

AMA Style

Kamran U, Rhee KY, Park S-J. Effect of Triblock Copolymer on Carbon-Based Boron Nitride Whiskers for Efficient CO2 Adsorption. Polymers. 2019; 11(5):913. https://doi.org/10.3390/polym11050913

Chicago/Turabian Style

Kamran, Urooj, Kyong Yop Rhee, and Soo-Jin Park. 2019. "Effect of Triblock Copolymer on Carbon-Based Boron Nitride Whiskers for Efficient CO2 Adsorption" Polymers 11, no. 5: 913. https://doi.org/10.3390/polym11050913

APA Style

Kamran, U., Rhee, K. Y., & Park, S. -J. (2019). Effect of Triblock Copolymer on Carbon-Based Boron Nitride Whiskers for Efficient CO2 Adsorption. Polymers, 11(5), 913. https://doi.org/10.3390/polym11050913

Note that from the first issue of 2016, this journal uses article numbers instead of page numbers. See further details here.

Article Metrics

Back to TopTop