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Synthesis of Carbon-Supported MnO2 Nanocomposites for Supercapacitors Application

Jolita Jablonskiene
Dijana Simkunaite
Jurate Vaiciuniene
Giedrius Stalnionis
Audrius Drabavicius
Vitalija Jasulaitiene
Vidas Pakstas
Loreta Tamasauskaite-Tamasiunaite
* and
Eugenijus Norkus
Center for Physical Sciences and Technology, Sauletekio Ave. 3, LT-10257 Vilnius, Lithuania
Authors to whom correspondence should be addressed.
Crystals 2021, 11(7), 784;
Submission received: 11 May 2021 / Revised: 30 June 2021 / Accepted: 1 July 2021 / Published: 5 July 2021


In this study, carbon-supported MnO2 nanocomposites have been prepared using the microwave-assisted heating method followed by two different approaches. The MnO2/C nanocomposite, labeled as sample S1, was prepared directly by the microwave-assisted synthesis of mixed KMnO4 and carbon powder components. Meanwhile, the other MnO2/C nanocomposite sample labeled as S2 was prepared indirectly via a two-step procedure that involves the microwave-assisted synthesis of mixed KMnO4 and MnSO4 components to generate MnO2 and subsequent secondary microwave heating of synthesized MnO2 species coupled with graphite powder. Field emission scanning electron microscopy (FE-SEM), transmission electron microscopy (TEM), X-ray photoelectron spectroscopy (XPS), and inductively coupled plasma optical emission spectroscopy have been used for characterization of MnO2/C nanocomposites morphology, structure, and composition. The electrochemical performance of nanocomposites has been investigated using cyclic voltammetry and galvanostatic charge/discharge measurements in a 1 M Na2SO4 solution. The MnO2/C nanocomposite, prepared indirectly via a two-step procedure, displays substantially enhanced electrochemical characteristics. The high specific capacitance of 980.7 F g−1 has been achieved from cyclic voltammetry measurements, whereas specific capacitance of 949.3 F g−1 at 1 A g−1 has been obtained from galvanostatic charge/discharge test for sample S2. In addition, the specific capacitance retention was 93% after 100 cycles at 20 A g−1, indicating good electrochemical stability.

1. Introduction

The development of high-performance, environmentally friendly, flexible, light and inexpensive energy storage devices has become one of the most significant worldwide concerns over the past few decades [1,2,3,4]. In this regard, supercapacitors (SCs) are widely viewed as potential candidates for next-generation energy storage devices [5,6]. They are of particular interest for high power capability, cyclic stability, safe and simple operation principle, and speedy charge dynamics compared to the other storage devices [7,8].
The decisive role in the fabrication of efficient SCs is directly related to the intrinsic properties of the electrode material used [2,9]. Various new advanced nanostructured materials or their hybrid combinations of two or more components are being looked at. Currently, transition metal oxides (TMOs) coupled mainly with high-surface-area carbon-based materials have been allowed to achieve various hybrid SCs systems, which have superior characteristics of power and energy densities compared to those values obtained at each system separately [10,11]. Among the preferential TMO materials for SCs, a series of manganese oxide-based hybrids were developed recently [12,13,14,15,16]. Exceptional attention has been focused on MnO2 for its relatively low cost, environmental friendliness, natural abundance, multiple oxidation states of Mn, wide operating voltage range (0–1.00 V vs. NHE in the neutral electrolyte), and high theoretical specific capacitance (Cs) close to 1370 F g−1 [17,18].
However, regardless of the above-mentioned superb characteristics, the main drawback for MnO2 widespread application is relatively poor electronic (10−5–10−6 S cm−1) and ionic (10−13 S cm−1) conductivity [8,15]. The experimentally achieved actual capacitance value is far below the theoretically predicted value and depends strongly on the mass loading of MnO2. Typically it decreases rapidly with the increase in the MnO2 mass [19]. To improve the capacitive performance of MnO2, several strategies have been proposed. Nanostructured MnO2-based electrodes with various morphologies have a high specific surface area and a large surface-to-volume ratio for more effective contact with electrolyte ions, such as mesoporous MnO2 nanotubes/nanosheets [20], nanowires [21], or flowerlike, urchinlike, and nano rodlike structures that have been developed. Multiple-phase heterostructures for high-capacitance electrodes have been created as well [22]. Two high-capacitance crystal phases of MnO2, namely α-MnO2 nanowires and δ-MnO2 ultrathin nanoflakes, have been combined and generated a self-branch heterostructure with a high Cs value of 178 F g−1 at 5 mV s−1 [22].
To enhance the electric conductivity of MnO2, the incorporation of conductive metals including Au, Al, Cu, Fe, Mg, Co [23,24,25,26,27,28,29,30,31] able to act as electron donors have been applied. Changes in electron structure by foreign heteroatoms resulted in the improved capacitive performance of MnO2 and revealed that, for example, Cu-doped δ -MnO2 film delivered the maximum Cs value as high as 296 F g−1 at 1 A g−1 [26]; for Fe-doped MnO2 nanostructures, this value was of 267.0 F g−1 even under a high mass loading of 5 mg cm−2 [28]. In the presence of Co, the achieved Cs value was of 350 F g−1 at a current density of 0.1 A g−1 [29]. The Al-doped MnO2 demonstrated a high mass and areal specific capacitance of 213 F g−1 and 146 F cm−2, respectively, at 0.1 A g−1 [25]. Meanwhile, Au-doped MnO2 showed a high Cs value of 626 F g−1 at 5 mV s−1 [24].
However, the most effective and currently most widely used way to improve Cs of MnO2-based electrodes is the deposition of thin films of latter materials on highly conductive and large surface areas containing materials, such as carbon-based substrates, including activated carbon, carbon nanotubes (CNTs), graphene, carbon fiber, or graphitic carbon. Carbon-based materials are the most widely used because of their physical and chemical properties, including low cost, variety of forms, low effort of processing, relatively inert electrochemistry, controllable porosity, and numerous electrocatalytic active sites for a variety of redox reactions [32,33,34] However, the performance of carbon-based substrates has some limitations related to the insufficient penetration of ions on the inert surface. Therefore, nanohybrids from two or more materials have been developed to overcome such limitations and gained special attention due to synergetic effects in enhancing the surface and electron donor properties. S.V. Prabhakar Vattikuti et al. reported 1D/2Dcarbon-CuO-graphitic carbon nitride (C/CuO@g-C3N4) ternary heterostructure that showed a better specific capacitance of 247.2 F g−1 compared with the pristine g-C3N4 of 83.7 F g−1, at the same time possessing good stability, with 92.1% of the initial capacitance remaining even after 6000 cycles [35]. Newly designed nanohybrids with Bi2S3 nanorod core@ amorphous carbon shell heterostructure C@Bi2S3 displayed a high specific capacity of 333.43 F g−1 at a current density of 1 A g−1 and outperformed that of pristine Bi2S3 of 124.24 F g−1, due to well-defined cross linkages between the Bi2S3 core and carbon shell [36]. The carbon layer was supposed to bind efficiently with Bi2S3 nanorods, and thus improve electrical contact with the current collector, confirming the more active carbon participation in the charge/discharge reaction process. These highly porous structures allow the free permeation of electrolyte ensuring rapid movement of ions. Further on, a novel Na2Ti3O7/single-walled carbon nanotubes SWCNTs nanostructure electrode material due to high surface area, enriched interfacial conductivity, abundant active edge sites, and mesoporous nature demonstrated a capacity of 576.01 F g−1, at 0.8 A g−1, with cycling stability featuring 91.43% retaining of capacitance after 5000 cycles [37].
Recently, a synergy of such carbon-based materials, featuring excellent conductivity and ultrastability, with MnO2 substances having less lower conductivity but larger electrochemical capacitance, has allowed overcoming limitations of each material separately by making full use of their advantages due to the synergistic effects between those two types of SCs materials [38,39,40,41,42,43,44]. Y. Ping et al. produced the hierarchically porous CJE/MnO2 composite with a large specific capacitance of 283 F g−1 at 1 A g−1, which was on account of high specific surface area (1283 m2 g−1) and abundant active sites for pseudocapacitance, that particularly resulted from the introduction of MnO2 [38]. Meanwhile, highly loaded MnOx of 7.02 mg cm−2, electrodeposited on conductive carbon cloth allowed achieving excellent rate capability due to the dual-tuning effect and showed specific capacitance of 161.2 F g−1 (1.13 F cm−2) at a high current density of 20 mA cm−2 [39]. Recently, an MnO2 nanowires/graphenated CNTs composite was grown in situ on 316 L stainless steel and exhibited a high capacitance of 495.2 mF cm−2 (615.6 F g−1) at a current density of 0.5 mA cm−2 and 95% capacity retention after 5000 cycles due to the synergistic effects of the high conductivity of graphenated CNTs and high pseudocapacitance of MnO2 nanowires [42].
Bearing in mind that the structure of the electrode material directly affects the electrochemical properties of the electrode and simultaneously determines the performance of SCs, different methods have been tested to develop high capacitive MnO2-based electrode materials. Among them are such methods as hydrothermal synthesis [20,45,46], electrochemical deposition [42,47,48], electrochemical exfoliation [48], electrospinning [49], chemical coprecipitation [50], or even those, using templates [40]. Particular attention has been focused on the simple, fast, cost-effective, and reliable microwave-assisted approach. This method has several advantages that count the possibility to get great gain in energy savings and enhanced fabrication of homogeneous materials since they do not need expensive equipment or complicated procedures; microwave reactions take less time compared to conventional methods and overtake all the substance uniformly, providing uniform particle-size distribution in the sample. Recently, this approach was successfully introduced to synthesize MnO2 materials that proved themselves for possible use in high-performance supercapacitor applications [51,52,53,54,55,56,57].
In this study, the carbon-supported MnO2 nanocomposites (MnO2/C) were prepared by the rapid and simple microwave-assisted heating method by employing manganese(II) sulfate (MnSO4) or potassium permanganate (KMnO4) and carbon powder as the microwave absorbing material. The electrochemical properties of the prepared MnO2/C nanocomposites have been studied to evaluate the possibility of using these nanocomposites as potential supercapacitor electrode materials.

2. Materials and Methods

Graphite powder, KMnO4, MnSO4∙H2O, Na2SO4, polyvinylidene fluoride (2%, PVDF), N-methyl-2-pyrrolydone (NMP) were obtained from a Sigma-Aldrich supplier (Taufkirchen, Germany). All reagents were of analytical grade and used as received without further purification. Aqueous solutions were prepared using Milli-Q water with a resistivity of 18.2 MΩ cm−1.
MnO2/C nanocomposite labeled as sample S1 was prepared by the following steps: 2 g of KMnO4 was mixed with 0.1 g of graphite powder and 20 mL of deionized water in an ultrasound bath for 30 min. Then, the reaction mixture was put into a microwave reactor Monowave 300 (Anton Paar, Graz, Austria). The synthesis of MnO2/C was carried out at a temperature of 150 °C for 5 min. After that, the precipitate was filtered out, washed with deionized water, and dried in a vacuum oven at a temperature of 80 °C for 2 h. Equation (1) describes the formation of MnO2 [18]:
4KMnO4 + 3C + H2O → 4MnO2 + K2CO3 + 2KHCO3
Another MnO2/C nanocomposite labeled as sample S2 was prepared by the following procedure: at first, the pure MnO2 was prepared. In a typical experiment, 0.063 g of KMnO4 and 0.1 g of MnSO4∙H2O was dispersed in 20 mL of deionized water and mixed in an ultrasound bath for 30 min. Then, the reaction mixture was put into a microwave reactor, and the synthesis was carried out at a temperature of 150 °C for 5 min. The precipitate was filtered out, washed with deionized water, and dried in a vacuum oven at 80 °C for two h. Equation (2) shows the formation process of pure MnO2 [58]:
2KMnO4 + 3MnSO4 + 2H2O → 5MnO2 + 2H2SO4 + K2SO4
Then, 0.01 g of the prepared MnO2 was mixed with 0.1 g of graphite powder and 20 mL of deionized water in an ultrasound bath for 30 min. The synthesis of MnO2/C was carried out under the same conditions as for the sample S1.
The prepared nanocomposites’ morphology, structure and composition were characterized using an SEM-focused ion beam facility (Helios Nanolab 650, FEI, Eindhoven, The Netherlands) equipped with an EDX spectrometer (INCA Energy 350 X-Max 20, Oxford Instruments, Oxford, UK). The amount of active material was determined using an ICP optical emission spectrometer Optima700DV (Perkin Elmer, Waltham, MA, USA).
The shape and size of catalyst particles were examined using a Transmission Electron Microscope Tecnai G2 F20 X-TWIN (FEI, Eindhoven, The Netherlands) equipped with an EDAX spectrometer with an r-TEM detector. For microscopic examinations, 10 mg of sample was first sonicated in 1 mL of ethanol for 1 h and then deposited on the Cu grid covered with a continuous carbon film.
XPS measurements were carried out to obtain information about the elemental chemical states and surface composition of powders on the upgraded Vacuum Generator (VG) ESCALAB MKII spectrometer (VG Scientific, UK) fitted with a new XR4 twin anode. The non-monochromatized Al Kα X-ray source was operated at hν = 1486.6 eV with 300 W power (20 mA/15 kV), and the pressure in the analysis chamber was lower than 5 × 10−7 Pa during spectral acquisition. The analyzer work function was determined, assuming the binding energy of the Au4f7/2 peak to be 84.0 eV. The spectra were acquired with an electron analyzer pass energy of 20 eV for narrow scans and resolution of 0.05 eV and with a pass energy of 100 eV for survey spectra. All spectra were recorded at a 90° take-off angle. The spectra calibration, processing, and fitting routines were done using Avantage software (v5.962) provided by Thermo VG Scientific (Waltham, MA, USA). Core level peaks of Mn 2p, Mn 3s, O 1s, and C 1s were recorded and analyzed using a nonlinear Shirley-type background. The calculation of the elemental composition was performed on the basis of Scofield’s relative sensitivity factors.
XRD patterns of studied powders were measured using an X-ray diffractometer SmartLab (Rigaku, Japan) equipped with a 9 kW rotating Cu anode X-ray tube. The measurements were performed using Bragg–Brentano geometry with a graphite monochromator on the diffracted beam and a step scan mode with the step size of 0.02° (in 2θ scale) and counting time of 1s per step. The measurements were conducted in the 2θ range 10–75°. Phase identification was performed using software package PDXL (Rigaku, Japan) and ICDD powder diffraction database PDF-4+ (2020 release).
All electrochemical measurements were performed with a three-electrode cell using cyclic voltammetry (CV) and galvanostatic charge/discharge (GCD). The prepared MnO2/C nanocomposites coated on the glassy carbon electrode (GCE) were employed as the working electrode; a Pt sheet as a counter electrode and an Ag/AgCl/KCl electrode were used as a reference. The working electrodes were prepared as follows: the required amount of the active material (MnO2/C) was dispersed ultrasonically in 2% of PVDF in an NMP solution for 1 h. Then, the obtained slurry was pipetted onto the polished surface of GCE and dried in an oven at a temperature of 80 °C for 2 h.
All electrochemical measurements were performed with a Zennium electrochemical workstation (ZAHNER-Elektrik GmbH & Co.KG, Kronach, Germany). Cyclic voltammograms (CVs) were recorded in a 1 M Na2SO4 solution at different scan rates between 10 and 200 mV s−1. All solutions were de-aerated by argon for 15 min before measurements. The specific capacitance Cs (F g−1) of the electrode material was calculated from the CV test according to the following equation (Equation (3)) [43]:
C s = 1 m · v · Δ V   i d v ,
where Cs, is the specific capacitance (F g−1), m—the mass of the active material (g), v—the scan rate of potential (V s−1), ΔV—the range of scan potential (V), and i—the current (A).
Further, galvanostatic charge/discharge cycling was carried out within a potential range between 0 and 1 V at a current density of 1, 2, 5, 10, and 20 A g−1. The Cs was calculated using the following equation (Equation (4)) [55]:
C s = I Δ t m · Δ V ,
where I is the discharge current (A), Δt is the time for a full discharge (s), and ΔV represents the voltage change during the discharge process (V).

3. Results

The carbon-supported MnO2 nanocomposites were prepared using the microwave-assisted heating method and two different approaches. The MnO2/C nanocomposite, labeled as sample S1, was prepared directly by the microwave-assisted synthesis of mixed KMnO4 and carbon powder components. Another MnO2/C nanocomposite, labeled as sample S2, was prepared in another way: at first, pure MnO2 was obtained by synthesizing KMnO4 and MnSO4. Then, the mixture of the obtained MnO2 and carbon powder was affected by microwave-assisted heating.
SEM images of the prepared MnO2/C samples S1 (a, b) and S2 (c, d) under different magnifications are presented in Figure 1.
As evident, both samples are composed of spherical manganese nanograins located on the carbon surface, but they differ significantly in particle number, size and density. In the case of sample S1, a sparse population of almost separate particles under a low MnO2 aggregation level is arranged (Figure 1a,b). The size of particles in this sample is close to 20 nm. In the case of sample S2, a nanograins’ aggregate forms a large porous network structure with carbon embedded inside (Figure 1c,d). The aggregation level of MnO2 develops to a large extent without any clear interparticle boundaries.
The samples S1 and S2 were further characterized by TEM analysis. TEM images of the samples S1 and S2 confirm the fibrous morphologies of both samples with the more expressed one for sample S2 (Figure 2). It was found that in the prepared sample S1, the MnO2 nanoparticles are spherical and are ca. 13–18 nm in size (Figure 2a,b). Furthermore, no large MnO2 nanoparticles are present within the prepared sample, indicating their negligible aggregation. In the case of sample S2, thin flakelike morphology is observed (Figure 2c,d).
The chemical composition and the surface electronic state of the prepared MnO2/C nanocomposites were analyzed using XPS. The C 1s signal and Mn 2p and O 1s peaks were observed in the XPS survey spectra of both samples S1 and S2 (Figure 3a). It indicates the successful synthesis of MnO2/C, while K content in the samples S1 and S2 was ca. 3.5 and 0.88 at.%, respectively. In both cases, the deconvoluted spectra of Mn show a spin-orbit doublet of the main Mn 2p3/2 and Mn 2p1/2 peaks located at binding energies (Eb) of 642.2 eV and 654.0 eV, respectively, with a spin-energy separation of 11.8 eV (not shown). This value confirms the presence of MnO2 in the prepared nanocomposites [59,60,61,62].
XPS spectra of Mn2p3/2 and C 1s for MnO2/C samples S1 and S2 are shown in Figure 3b–e. As evident, for both samples, the Mn 2p3/2 peaks were deconvoluted into four peaks at binding energies of 640.6 ± 0.3, 642.2, 643.5, and 644.7 and 646.6 eV, indicating the mixed-valence of manganese oxide phases (Figure 3b,c). Following the data reported in [59,60,61,62,63,64], the position of deconvoluted Mn 2p3/2 peaks are generally assigned to Mn (IV) or Mn (II) oxidation state at Eb ranging between 641.85–643.0 eV or 640.10–641.12 eV, respectively. Therefore, peaks determined at 640.6 ± 0.3 and 642.2 eV confirm the presence of Mn(II) and Mn(IV) species in the samples S1 and S2 (Figure 3b,c). Moreover, the additional peak at 644.7 eV close to that obtained at 644.9 eV in [65,66] could similarly be assigned to a satellite shake-up peak located at higher Eb values than the main component and is a characteristic feature of the MnO phase Mn 2p core peak maximum at 640.6 ± 0.3 eV [67]. Meanwhile, peaks at 643.5 eV and 644.7 eV based on data in [66] could be related to Mn (VI and VII) species in the samples. There is no Mn 2p3/2 signal (647 eV) from permanganate ions, suggesting permanganate ions have been reduced to MnO2 [68]. It should be noted that the dominating fraction in the prepared samples S1 and S2 is the MnO2 phase and is equal to ~59 and 53%, respectively. At the same time, the MnO (Mn (II)) phase remains significantly lower compared to that determined for the MnO2 (Mn (IV)) phase.
The high-resolution C 1s spectrum for sample S1 can be deconvoluted into three peaks centered at Eb of 284.1, 285.1 and 286.1 eV (Figure 3d). The first one value could be assigned to carbon atoms C–C; meanwhile, other peaks could be assigned to oxygen functionalized carbon atoms, such as C–O, or C–OH and C=O [60,69].
In the case of the sample S2, the C 1s XPS spectrum could be fitted into three peaks at 284.6, 285.8, and 288.4 eV (Figure 3e), which corresponded to C–C/C=C, C–O, and O–C=O bonds, respectively [70]. The strong peak of C–C/C=C bonds shows that carbon contained high graphitization.
The obtained XRD patterns for both MnO2/C samples are shown in Figure 4. The presence of broad peaks implied that the synthesized samples S1 and S2 are essentially a mixture of amorphous and nanocrystalline phases. The prominent peaks from both samples (Figure 4) locate at 26°, which can be assigned to the (002) crystal plane of graphitic carbon (ICDD card no. 00-056-0159). The diffraction peaks of α-MnO2 are indexed according to ICDD card no. 04-005-4884, indicating a tetragonal unit cell with lattice parameters of a = b = 9.82 Å and c = 2.85 Å. The synthesized powders are composed of small crystallites with an average size of about 3.2 ± 0.3 nm.
The electrochemical performance of samples S1 and S2 was evaluated from the cyclic voltammetry and galvanostatic charge/discharge measurements using a three-electrode system in a 1 M Na2SO4 solution. Figure 5 shows the CV curves of the sample S1 (a), sample S2 (b), and pure carbon (c) at the scan rates of 10, 50, 100, and 200 mV s−1. No obvious peaks are observed in all the CV curves. This indicates that the electrodes are charged and discharge at a constant rate over the complete cycle.
Both sample S1 and carbon show symmetrical rectangular shapes, which indicates the ideal capacitive behavior of those samples (Figure 5a,c). In the case of sample S2, deviations in the rectangularity of CV curves occur (Figure 5b). It can be seen that the current response of sample S2 is significantly higher as compared with that of sample S1 and carbon (Figure 5a–c). It is clearly seen that the sample S2 shows a significantly higher capacitive behavior as compared with that of sample S1 (Figure 5d).
The calculated Cs values for the sample S2 were 980.7, 743.2, 641.0, and 536.6 F g−1 at scan rates of 10, 50, 100, and 200 mV s−1, respectively (Figure 6). Meanwhile, for the sample S1, Cs values were 535.8, 349.6, 275.2, and 209.7 F g−1 at scan rates of 10, 50, 100, and 200 mV s−1. Those values were found to be ca. 1.8–2.6 times lower than those obtained for sample S2.
Comparisons of the supercapacitive behavior of various MnO2-based electrode materials reported in the literature and the present work are listed in Table 1, exhibiting the high specific capacitance of our prepared electrode materials.
Galvanostatic charge/discharge curves for the sample S2 measured at different current densities of 1, 2, 5, 10, and 20 A g−1 are shown in Figure 7a. The shapes of the curves show a typical triangular symmetrical distribution with a slight curvature. This result indicates a combination of electric double-layer and pseudocapacitive contributions. Specific capacitance values were calculated from the discharge test. It was found that the sample S2 can deliver high Cs values of 949.3, 719.3, 480.8, 406.7, and 371.5 F g−1 at a current density of 1, 2, 5, 10, and 20 A g−1 (Figure 7b). The long-term stability of the charge/discharge process was also performed on this sample S2 at a high current density of 20 A g−1 up to 100 cycles (Figure 7c). As evident, this electrode showed excellent long-term stability with 93% retention of its initial capacitance value during 100 cycles.

4. Conclusions

We have successfully fabricated carbon-supported MnO2 nanocomposites via a simple microwave-assisted heating method. Different architecture containing MnO2 nanocomposites demonstrates improved conductivity, which is a key limitation in pseudocapacitors. The electrochemical measurements revealed that (due to this conductivity) MnO2/C nanocomposites, especially those prepared via a two-step procedure, exhibit excellent electrochemical performance, including a high specific capacitance of 980.7 F g−1. Moreover, the specific capacitance retention was 93% after 100 cycles at 20 A g−1, indicating good electrochemical stability. The obtained results demonstrate that the prepared MnO2/C nanocomposites should be a promising electrode material for supercapacitor applications and could be further extended to fabricate other materials for supercapacitors.

Author Contributions

This study was conducted through the contributions of all authors. Conceptualization, J.J.; L.T.-T. and E.N.; methodology, G.S., A.D., V.P. and V.J.; investigation, J.V., G.S. and A.D.; writing—original draft preparation, J.J. and D.S.; writing—review and editing, L.T.-T. and E.N.; visualization, D.S., J.V., V.P. and V.J. All authors have read and agreed to the published version of the manuscript.


This research was funded by the European Social Fund under the No 09.3.3-LMT-K-712-02-0142 “Development of Competencies of Scientists, other Researchers, and Students through Practical Research Activities” measure.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Conflicts of Interest

The authors declare no conflict of interest.


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Figure 1. SEM images of MnO2/C: (a,b) sample S1; (c,d) sample S2 under different magnifications.
Figure 1. SEM images of MnO2/C: (a,b) sample S1; (c,d) sample S2 under different magnifications.
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Figure 2. TEM images of MnO2/C: (a,b) sample S1; (c,d) sample S2 under different magnifications.
Figure 2. TEM images of MnO2/C: (a,b) sample S1; (c,d) sample S2 under different magnifications.
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Figure 3. Survey spectra for samples S1 and S2 (a). XPS spectra of Mn 2p and C 1s for MnO2/C: (b,c) sample S1; (d,e) sample S2.
Figure 3. Survey spectra for samples S1 and S2 (a). XPS spectra of Mn 2p and C 1s for MnO2/C: (b,c) sample S1; (d,e) sample S2.
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Figure 4. XRD patterns of samples S1 (1 pattern) and sample S2 (2 pattern).
Figure 4. XRD patterns of samples S1 (1 pattern) and sample S2 (2 pattern).
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Figure 5. CVs of: (a) sample S1; (b) sample S2; (c) carbon were recorded in 1 M Na2SO4 at different scan rates. (d) CVs of samples S1 and S2 at 10 mV s−1.
Figure 5. CVs of: (a) sample S1; (b) sample S2; (c) carbon were recorded in 1 M Na2SO4 at different scan rates. (d) CVs of samples S1 and S2 at 10 mV s−1.
Crystals 11 00784 g005aCrystals 11 00784 g005b
Figure 6. Specific capacitances of the sample S1, sample S2, and carbon obtained from CV curves.
Figure 6. Specific capacitances of the sample S1, sample S2, and carbon obtained from CV curves.
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Figure 7. (a) Galvanostatic charge/discharge curves of the sample S2 measured at different constant current densities of 1–20 A g−1; (b) Specific capacitance obtained from galvanostatic charge/discharge curves with different current densities.
Figure 7. (a) Galvanostatic charge/discharge curves of the sample S2 measured at different constant current densities of 1–20 A g−1; (b) Specific capacitance obtained from galvanostatic charge/discharge curves with different current densities.
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Table 1. Comparisons of specific capacitance for various MnO2-based electrode materials.
Table 1. Comparisons of specific capacitance for various MnO2-based electrode materials.
MaterialsScan Rate,
mV s−1
F g−1
MnO2/C (S2)10980.7This work
MnO2/C (S1)10535.8This work
Self-branched α-MnO2/δ-MnO2 heterojunction nanowires10152.0[22]
Ultra-long MnO2 nanowires2495.0[69]
MnO2 NPs/Ni foam5549.0[71]
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Jablonskiene, J.; Simkunaite, D.; Vaiciuniene, J.; Stalnionis, G.; Drabavicius, A.; Jasulaitiene, V.; Pakstas, V.; Tamasauskaite-Tamasiunaite, L.; Norkus, E. Synthesis of Carbon-Supported MnO2 Nanocomposites for Supercapacitors Application. Crystals 2021, 11, 784.

AMA Style

Jablonskiene J, Simkunaite D, Vaiciuniene J, Stalnionis G, Drabavicius A, Jasulaitiene V, Pakstas V, Tamasauskaite-Tamasiunaite L, Norkus E. Synthesis of Carbon-Supported MnO2 Nanocomposites for Supercapacitors Application. Crystals. 2021; 11(7):784.

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Jablonskiene, Jolita, Dijana Simkunaite, Jurate Vaiciuniene, Giedrius Stalnionis, Audrius Drabavicius, Vitalija Jasulaitiene, Vidas Pakstas, Loreta Tamasauskaite-Tamasiunaite, and Eugenijus Norkus. 2021. "Synthesis of Carbon-Supported MnO2 Nanocomposites for Supercapacitors Application" Crystals 11, no. 7: 784.

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