Yu Shua,
Jun Maruyama
b,
Satoshi Iwasakib,
Shohei Maruyamab,
Yehua Shenc and
Hiroshi Uyama*ac
aDepartment of Applied Chemistry, Graduate School of Engineering, Osaka University, Suita, Osaka 565-0871, Japan. E-mail: uyama@chem.eng.osaka-u.ac.jp
bResearch Division of Environmental Technology, Osaka Research Institute of Industrial Science and Technology, 1-6-50 Morinomiya, Joto-ku, Osaka 536-8553, Japan
cKey Laboratory of Synthetic and Natural Functional Molecule Chemistry of Ministry of Education, College of Chemistry and Materials Science, Northwest University, Xi'an, Shaanxi Province 710127, PR China
First published on 5th September 2017
N-doped porous monolithic carbons (PMC) have been developed from polyacrylonitrile (PAN) via a template-free thermally induced phase separation (TIPS) approach followed by an easy pyrolysis process. Three-dimensional (3D) PAN monolith (PM) was firstly fabricated as the starting material. The shape of the 3D PM was designed during the phase separation step, revealing that the product carbons had the potential advantages of desired porosity and controllable shape. Two typical activation methods were employed and compared to prepare PMC. KOH-activated PMC showed a larger surface area of 1600 m2 g−1 and higher nitrogen content of 5.6% in comparison to that being activated in a carbon dioxide atmosphere (CD-PMC). The electrochemical measurements revealed that PMC possessed a high capacitance of 270 F g−1 at 0.2 A g−1 and 195 F g−1 even at 100 A g−1, ultra-high rate capability with 72% capacitance retention from 0.2 to 100 A g−1 and outstanding cycling stability with 100% capacitance retention at 20 A g−1 after 5000 cycles. These results demonstrate that the present facile and efficient synthetic strategy for PMC from PAN can benefit the promotion of its application in energy storage devices and it is highly likely to be extended to other polymer sources.
Recently, the modifications of surface functionalities with heteroatoms, such as N, O, B, S, or P, have been discovered effectively to adjust the electron donor/acceptor properties of carbon materials giving rise to additional pseudo-capacitance and maintain the excellent rate capability and cycling stability.17–19 More and more heteroatom-doped carbon materials have been synthesized and N-doping is evidenced to be positive in improving the capacity by enhancing the electronic conductivity and surface wettability.20–23 Traditional N-doped carbons are usually prepared by introducing a certain amount of N into carbon frameworks through a post-treatment process, such as treat with ammonia, urea, amines, etc.; however, it often results in a lower content of nitrogen.24 Compared to the post-treatment process, pyrolysis directly of N-containing polymer precursors such as polypyrrole,25 polyaniline,26 and polyacrylonitrile (PAN)27 seems to be more effective to get carbons with higher N content. Among the polymers mentioned above, PAN, a widely used precursor for synthesizing carbon materials, possesses a nitrogen atom per monomeric unit and forms an infusible stable ladder structure after a cyclization reaction to withstand the further high temperature. However, PAN was mainly employed to prepare carbon fibers.28–33 Limited reports were related to activated carbons or monolithic carbons from PAN through an easy pyrolysis process. In our previous study, 3D monoliths with uniform meso/macro-porosity have been fabricated by a template-free thermally induced phase separation (TIPS) approach. The shapes of the monolith can be freely designed, which are advantageous for large-scale industrial applications.34 Moreover, the derived activated carbons kept a microstructure even after heating at a high temperature and interestingly possessed high adsorption capacity for carbon dioxide.35 Considering these merits of PAN and TIPS, it is highly promising to develop novel porous carbons with large surface area, nitrogen self-doped, and controllable shape to high performance SCs.
In this study, N-doped porous monolithic carbons (PMC) were obtained from PAN by the low-cost and facile template-free TIPS approach followed by a pyrolysis process. The fabricated PAN monolith (PM), as the precursor to prepare carbons, showed a three-dimensional (3D) porous structure. The shape of PM can be designed during the phase separation process, which will be beneficial to give the further product carbons a controllable shape. Subsequently, two typical pyrolysis methods including carbon dioxide and potassium hydroxide activation were employed and compared to obtain PMC with desired properties. The specific surface areas and porosity parameters were systematically investigated and the electrochemical performances were fully evaluated on both three- and two-electrode systems. In comparison with PMC prepared by carbon dioxide activation (CD-PMC), KOH-activated PMC possessed a large surface area, suitable pore size distribution, and high N content, resulting in a high specific capacitance, excellent cycle stability, and long cycle life. These results demonstrated that the PAN-based monolithic carbons presented herein are highly promising electrode candidate for energy storage devices.
Firstly, a three-electrode system was assembled by using 1 M H2SO4 as the aqueous electrolyte, platinum wire as the counter electrode, Ag/AgCl as the reference electrode, and glassy carbon (4 mm diameter) as the working electrode. The working electrode was prepared as follows: 20.0 mg active samples (powder size < 45 μm) were mixed with 1 mL 0.8 wt% Nafion solution (diluted by isopropanol from 5% Nafion®) and sonicated for 30 min to form a well-dispersed ink, 3.5 μL of which was casted into the surface of the glassy carbon electrode. CV measurements were performed in a potential range of 0 V to 0.8 V vs. Ag/AgCl by varying scan rates from 1 to 500 mV s−1. GCD measurements were carried out at current density at 0.2–100 A g−1. The cycling life was evaluated by the GCD measurement at a constant current density of 20 A g−1 for 5000 and 10000 cycles. The specific capacitance (C, F g−1) obtained from CV was calculated by the following equation:
C = (qa + qc)/(2mΔV) | (1) |
The specific capacitance (C, F g−1) calculated from the discharge process of the GCD curves was obtained by the equation:
C = IΔt/(mΔV) | (2) |
Electrochemical impedance spectroscopy (EIS) was measured in the frequency range from 10−2 Hz to 104 Hz at 0 V with voltage amplitude of 10 mV in 1 M H2SO4 electrolyte. The PMC-based working electrodes were prepared as follows. A homogenized slurry consisting of 85 wt% PMC (powder size < 45 μm), 10 wt% acetylene black, and 5 wt% polytetrafluoroethylene (PTFE) binder was rolled into a thin film. Then, the film was dried at 120 °C for one day and punched into a circular sheet (6 mm diameter). The PMC-based carbon sheet was pressed on the surface of SUS mesh as the working electrode. A platinum wire and an Ag/AgCl electrode were used as the counter electrode and the reference electrode, respectively.
The practical electrochemical performance was fully evaluated in a two-electrode system. Before the electrochemical tests, the PMC-based carbon sheet (6 mm diameter) and separator were sufficiently vacuum-impregnated with 1 M H2SO4 aqueous solution overnight. The two-electrode symmetrical system was assembled in a 2E-CELL-SUS cell (Eager Corporation, Japan) by using two nearly identical (weight and size) and fully impregnated carbon sheets as electrodes and polypropylene non-woven cloth as a separator (Fig. S1†). The average weight of each electrode was around 2 mg. For comparison, commercial activated carbon (YP-50F, Kuraray Chemical Co.) was also tested in the same condition. The CV and GCD measurements were carried out in the potential window of 0–1.0 V. The specific capacitance of the total symmetrical SC cell (Ct, F g−1) was obtained based on the GCD measurements from the equation:
Ct = IΔt/(2mΔV) | (3) |
The energy density (Et, Wh kg−1) and power density (Pt, W kg−1) of the symmetric SC were calculated according to the following equations:
Et = (CtΔV2)/(2 × 3.6) | (4) |
Pt = Et/Δt | (5) |
![]() | ||
Fig. 1 TG curves of the used PAN powder and the fabricated PM (a), nitrogen adsorption/desorption isotherms with the inset of pore size distribution calculated by DFT model of PM (b). |
Sample | From N2 adsorption at 77 K | From EDX (wt%) or a CHN Corder (%) | |||||
---|---|---|---|---|---|---|---|
SBETa (m2 g−1) | Vtotalb (cm3 g−1) | Davec (nm) | C (wt%) | N (wt%) | O (wt%) | H (%) | |
a SBET calculated by BET method.b Total pore volume (Vtotal) calculated at P/P0 ≈ 0.99.c Average pore diameter (Dave). | |||||||
Raw PAN | — | — | — | 67 | 28 | 5.2 | — |
PM | 188 | 0.710 | 15.1 | 67 | 27 | 5.9 | — |
SPM | — | — | — | 66 | 27 | 6.9 | — |
PSPM | 8.95 | 0.017 | 7.57 | 71 (71%) | 26 (19%) | 3.5 | 2.1 |
CD-PMC | 722 | 0.493 | 2.73 | 86 (72%) | 7.8 (3.2%) | 5.3 | 1.7 |
PMC | 1600 | 0.862 | 2.16 | 83 (80%) | 10 (5.6%) | 6.0 | 0.5 |
After the stabilization process, two methods were chosen to prepare porous monolithic carbons, one was that stabilized PM was directly activated under the existence of carbon dioxide to obtain CD-PMC; another was that SPM was first carbonized in the argon gas and then activated with an equal weight of KOH to get PMC. The micromorphology and microstructure of all samples were studied by SEM images (Fig. 2). No significant differences can be observed in the external shape of the four samples and the interconnected 3D porous structures still remained even after activation process.
The nitrogen adsorption/desorption isotherms and pore size distributions were illustrated to analyze the pore structure of PMC and CD-PMC. As shown in Fig. 3a, they both exhibited a type-I isotherm, while PMC possessed a higher adsorbed volume. The pore size was mostly smaller than 4 nm from DFT method and microporous size from the HK model was mainly distributed between 0.8 nm to 2 nm with a peak around 1.2 nm (Fig. 3b). The specific surface areas of PMC and CD-PMC measured by BET method were 1600 and 700 m2 g−1, which were much higher than that of PM. The detailed summary of the specific surface area, pore volume, average pore size, and chemical composition of all samples was presented in Table 1. It can be seen that approximately 27 wt% of nitrogen was detected for PM and SPM from EDX spectrum, while 3.2% and 5.6% were obtained for CD-PMC and PMC from a CHN Corder. The nitrogen content decreased and carbon content increased after carbonization and activation process. Fig. 3c showed XRD patterns of CD-PMC and PMC. There were two characteristic peaks observed at around 24° and 43°, corresponding to the (002) and (10) diffractions, respectively. The XRD pattern of PMC showed weaker peak intensities than those of CD-PMC, corresponding to more disordered and smaller crystallites, which suggested the formation of the developed pore structure and relatively low graphitization degree.
XPS measurements were employed to analyze the components and chemical bondings at the surface of the carbon materials. The peaks of C 1s, N 1s, and O 1s were detected from the wide XPS survey spectrum. The high-resolution XPS spectra of C 1s, N 1s, and O 1s were collected to analyze the detailed information (Fig. 3d–f and S4†). The C 1s spectrum of PMC can be deconvoluted into five peaks located at 284.6, 285.9, 286.5, 287.6, and 288.8 eV (Fig. 3d), corresponding to aromatic and aliphatic carbon (C–C), hydroxyl and phenol groups (COR), carbon in keto–enol equilibria (CKE), keto and quinone groups (CO), and carboxylic groups (COOR), respectively. In the region of the N 1s core-level spectrum (Fig. 3e), the chemical states of the N atom, with binding energies of 398.3, 399.9 and 401.6 eV, can be identified as the pyridinic-N (N-6, ∼34%), the pyrrolic-N (N-5, ∼49%), and graphitic-N (N-G, ∼17%), respectively.40,41 Among them, N-5 and N-6 contribute to the pseudo-capacitance, while N-G promotes electron transport and effectively enhances the conductivity of carbon materials. Four characteristic peaks in the O 1s spectrum were centered at 531.5 eV, 532.4 eV, 533.3 eV, and 534.2 eV (Fig. 3f).42,43 These peaks were assigned to C
O groups (group 1), carbonyl oxygen atoms in esters, amides, anhydrides and carbonyl oxygen atoms in hydroxyls or ethers (group 2), the ether oxygen atoms in esters and anhydrides (group 3), and the oxygen atoms in carboxyl groups (group 4). The atomic contents of C, N and O species of PMC were calculated quantitatively as 86, 2.6, and 11 at%, respectively. The high-resolution XPS spectra of the carbonized composite sample (CD-PMC) were also plotted in Fig. S4.† The C, N and O species were calculated quantitatively as 90, 2.8, and 7.0 at%, respectively. As shown in Fig. S4b,† three types of N-functionality were N-6 (∼50%), N-5 (∼39%), and N-G (∼11%). The synergy of N-6, N-5 and N-G would contribute to the capacitance behavior greatly with pseudo-capacitance.
The GCD curves of CD-PMC and PMC measured in 1 M H2SO4 at a current density of 5 A g−1 were depicted in Fig. 4d. They both displayed a triangular shape which presented reversibility, an ideal electric double layer capacitive characteristic and high charge/discharge efficiency.49 Theoretically, the longer charge/discharge time is, the more electrolyte ions would participate in the charge/discharge process, resulting in a higher specific capacitance.50 In comparison with CD-PMC, PMC revealed a longer charge/discharge time and thus a higher specific capacitance. The GCD curves of PMC retained linearity and symmetry very well at current densities varying from 0.2 to 5 A g−1 (Fig. 4e). The typical isosceles triangular shape without obvious voltage drop represented an indication of excellent capacitive behavior of PMC. Even at high current densities ranging from 10 to 100 A g−1, the triangular shapes were maintained and a small voltage drop occurred (Fig. 4f). The charge/discharge time significantly decreased with an increase of current densities because the electrolyte ions had sufficient time to enter and diffuse into the pores at low current densities.51
The gravimetric specific capacitances at various current densities ranging from 0.2 to 100 A g−1 were calculated by eqn (2) and plotted in Fig. 5a. The specific capacitances of CD-PMC and PMC almost remained unchanged after 10 A g−1, indicating their superior rate capability. Obviously, PMC displayed higher specific capacitances than CD-PMC within the all range of current densities. The specific capacitances of PMC were 270 F g−1 at 0.2 A g−1, and 195 F g−1 even at a very high current density of 100 A g−1, resulting in a high capacitance retention rate of 72%. Cycling stability is another crucial factor in practical applications of the SCs. Therefore, the cycle life of PMC-based electrode was measured by GCD tests for 5000 charge/discharge cycles at a current density of 20 A g−1 within the potential window of 0–0.8 V (Fig. 5b). Remarkably, PMC possessed the outstanding cycle durability with the high retention rate of nearly 100% after 5000 cycles. The gradually increased capacitance between 2500 to 5000 cycles could be possibly attributed to the improved wettability and activing process of this electrode, that is, the continuous diffusion of the electrolyte ions into the porosity would lead to the gradual increase in the effective charge storage sites of PMC-based electrode and thus the specific capacitance.52 The GCD curves of the first and last five cycles were almost identical isosceles triangles, demonstrating an excellent long-term cycle stability of PMC (Fig. 5b, inset). Furthermore, there was almost no capacitance decay after 10000 cycles for PMC-based electrode (Fig. S5†). And the GCD curves of the 5000th cycle and 10000th cycle remained unchanged. EIS measurements were performed at room temperature in the 1 M H2SO4 electrolyte to explore the frequency response characteristics of PMC (Fig. 5c). The Nyquist plots of PMC-based electrode displayed a small semicircle and nearly vertical line, indicative of a low contact resistance and good capacitive response.
In order to further investigate the electrochemical capacitive practical performances for the PAN-based carbon electrodes, a symmetric SC was assembled with two nearly identical (weight and size) carbon films as the electrodes and 1 M H2SO4 aqueous solution as the electrolyte. For comparison, the commercial activated carbon (YP-50F) was also tested. Fig. 6a showed that the CV curves of the three kinds of electrodes were tested at scan rate of 5 mV s−1 under the potential window of 0–1 V. It was clearly observed that all CV curves exhibited a relatively rectangular shape and PMC-based SC possessed the largest integrated CV area, which was consistent with the above results of that tested in the three-electrode system. In this as-assembled practical SC, carbon-based electrodes were sufficiently impregnated in the aqueous electrolyte solution and then directly used without the addition of electrolyte (Fig. S1†). Therefore, the electrochemical performance of the SC was strongly determined by the capability of electrodes. The surface morphology of the carbon films were observed by SEM images (Fig. S6†). The electrodes from CD-PMC and PMC showed a similar surface appearance. In addition, the capacitive behaviors of electrodes were also dependent on the wettability of the inner pores for the electrolyte.53 Contact angle (CA) measurement was also carried out to study the surface wettability of all electrodes for 1 M H2SO4 aqueous electrolyte, which was used to preliminary evaluate the performance of the electrodes for SCs (Fig. S6,† inset).54 PMC-based electrode gave a smaller CA value, which was in agreement with the larger CV integrated area, and thus a higher specific capacitance. The CV curves of PMC-based SC remained a relatively rectangular shape at various scan rates from 5 to 500 mV s−1, indicating a near-ideal capacitive behavior with good rate performance (Fig. 6b). The GCD curves of three kinds of electrodes at a constant current density of 0.5 A g−1 exhibited typical triangle shapes without obvious voltage drops, indicating excellent coulombic efficiency together with good double-layer capacitive performance (Fig. 6c). PMC-based SC showed the longest charge/discharge time, meaning the highest specific capacitance. The GCD curves of PMC at current densities ranging from 0.1 to 1 A g−1 were shown in Fig. 6d. All GCD curves exhibited good triangle-shapes and excellent coulomb efficient.
The relationships between the specific capacitance of the total symmetrical SC calculated by eqn (3) and the current densities were summarized in Fig. 7a. The specific capacitances of PMC-based SC were as high as 63 F g−1 at 0.1 A g−1, and 40 F g−1 even at the high current density of 20 A g−1 (about 63% capacitance retention), which was obviously higher than the values of commercial AC-based SC. The energy density and power density of the PMC-based SC were calculated by eqn (4) and (5), respectively. And the Ragone plot was drawn in Fig. 7b. The energy density of the PMC-assembled SC decreased from 8.8 to 2.9 Wh kg−1 with increasing of current density from 0.1 to 20 A g−1, while the power density reached to 3666 from 25 W kg−1. PMC-based SC possessed higher energy/power densities than the commercial AC. Finally, the cycling performance of PMC-based SC was also evaluated using the GCD measurement and plotted in Fig. 7c. The specific capacitance displayed 47 F g−1 for the first cycle and remained at 45 F g−1 for the 3000th cycle with the retention of 96%, indicating that the charge/discharge process of PMC-assembled SC was highly reversible. The almost similar GCD curves of the first and the last five cycles revealed the good cycling and stability behaviors of the as-assembled SC (Fig. 7c, inset). Comparison with other reported carbons derived from PAN or its composites, as shown in Table 2, PMC herein demonstrated the desired specific capacitance, excellent rate capacitance and cycle stability not only in the three-electrode system but also in the symmetrical SC.
Precursor | SBET (m2 g−1) | Electrolyte | Capacitance (F g−1) | Rate capacitance | Cycle stability | Cellc | Ref. |
---|---|---|---|---|---|---|---|
a 1 M LiPF6 in EC/DMC: 1 M of LiPF6 in a mixture of ethylene carbonate (EC) and dimethyl carbonate (DMC) (3![]() ![]() |
|||||||
PAN | 722 | 1 M H2SO4 | 108 at 0.05 A g−1 | 50% from 0.05 to 20 A g−1 | — | 3E | 55 |
PAN/APEG | 753 | 6 M KOH | 302 at 0.2 A g−1 | 56% from 0.2 to 40 A g−1 | 95% | 2E | 56 |
PAN-b-PMMA | 403 | 2 M KOH | 314 at 0.5 A g−1 | 68% from 0.5 to 20 A g−1 | 90% | 3E | 57 |
210 at 0.5 A g−1 | 58% from 0.5 to 10 A g−1 | — | 2E | ||||
PAN | 1165 | 6 M KOH | 167 at 30 mV s−1 | 67% from 0.75 to 6 A g−1 | 78% | 3E | 58 |
PAN | 3550 | Organica | 216 at 0.05 A g−1 | 56% from 0.05 to 10 A g−1 | 100% | 2E | 59 |
PAN/CNT | 613.8 | 1 M H2SO4 | 216 at 10 mV s−1 | 63% from 10 to 200 mV s−1 | 100% | 3E | 60 |
PAN/PANI | 410 | 1 M H2SO4 | 335 at 0.5 A g−1 | 52% from 0.5 to 32 A g−1 | — | 3E | 61 |
— | — | 86% | 2E | ||||
PAN | 3130 | Organicb | 181 at 1 A g−1 | 77% from 1 to 10 A g−1 | 96% | 2E | 43 |
PMMA/PAN | 2085 | 6 M KOH | 314 at 0.5 A g−1 | 83% from 1 to 20 A g−1 | 96% | 3E | 27 |
PAN | 1600 | 1 M H2SO4 | 270 at 0.2 A g−1 | 72% from 0.2 to 100 A g−1 | 100% | 3E | This work |
253 at 0.1 A g−1 | 62% from 0.1 to 20 A g−1 | 96% | 2E |
Footnote |
† Electronic supplementary information (ESI) available: Supplementary figures. See DOI: 10.1039/c7ra07003a |
This journal is © The Royal Society of Chemistry 2017 |