# Direct Synthesis of MnO2 Nanorods on Carbon Cloth as Flexible Supercapacitor Electrode

Authors: Shuang Xi; Yinlong Zhu; Yutu Yang; Ying Liu
Journal: Journal of Nanomaterials
 (2017)

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## Abstract

MnO2 nanorod/carbon cloth (MnO2/CC) composites were prepared through in situ redox deposition as freestanding electrodes for flexible supercapacitors. The CC substrates possessing porous and interconnecting structures enable the uniform decoration of MnO2 nanorods on each fiber, thus forming conformal coaxial micro/nanocomposites. Three-dimensional CC can provide considerable specific surface area for high mass loading of MnO2, and the direct deposition process without using polymeric binders enables reliable electrical connection of MnO2 with CC. The effect of MnO2 decoration on the electrochemical performances was further investigated, indicating that the electrode prepared with 40 min deposition time shows high specific capacitance (220 F/g at a scan rate of 5 mV/s) and good cycling property (90% of the initial specific capacitance was maintained after 2500 cycles) in 1 M Na2SO4 aqueous solution. This enhanced electrochemical performance is ascribed to the synergistic effect of good conductivity of carbon substrates as well as outstanding pseudocapacitance of MnO2 nanorods. The obtained MnO2/CC compositing electrode with the advantages of low cost and easy fabrication is promising in applications of flexible supercapacitors.


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## Body

## 1. Introduction

Manganese oxide, as one of the most promising electrode materials for supercapacitors, has attracted significant attention with its excellent electrochemical properties such as high theoretical pseudocapacitance (~1370 F/g), low cost, and environmental friendliness [1, 2]. However, in practice such high theoretical capacitance has never been reached which is mainly caused by its inherent poor electrical conductivity and dense morphology of the oxide [3, 4]. Particularly, when the mass loading of MnO2 on the electrode is high (which is essential for obtaining high energy density), densely packed MnO2 enormously reduce the available surface area participating in the electrochemical process and increase the difficulty for electrolyte penetrating into the bulk MnO2 and thus raise the contact resistance of the electrode [5–7]. All these phenomena remarkably limit kinetics of charge transfer reaction and finally hinder the improvement of specific capacitance. Therefore, a reasonable-structured MnO2 coating with good electrical connection becomes essential in designing high-performance electrodes for MnO2-based supercapacitors [8, 9].To handle these issues, one powerful and straightforward approach is to transfer bulk MnO2 to nanoscale structures, that is, nanometer-thick thin films, nanosheets, nanorods, and nanotubes [10, 11], and also grow nano-MnO2 onto highly conductive cores [12–14]. The nanostructured MnO2 possessing large surface area could significantly enhance the efficiency in utilizing the electrode material, while the conductive backbone on which MnO2 dispersed can provide electrical pathway through the backbone to MnO2 to accomplish the charge storage reaction.Various conductive substrates could be supporting backbones for MnO2, including the carbon-based materials [15, 16] and various high-conductivity metal oxides [17, 18]. Among them, carbon cloths (CCs) are considered as promising conductive substrates due to their reasonable cost, excellent chemical stability, and 3D porous network texture. The 3D porous architecture not only allows high mass loading of MnO2 but also facilitates the diffusion of active species and transport of electrons, leading to good electrochemical performance [7, 19]. Additionally, the flexible nature of carbon cloths is advantageous for the fabrication of flexible supercapacitors from the design and packaging perspectives. In fact, in many subjects of functional materials research the utilization of 3D conductive backbones clearly indicates nano-MnO2 shell grown on micron-size conductive carbon fibers can be an effective solution for constructing outstanding supercapacitors [12, 20].In this work, we reported the binder-free integration of large-area MnO2 nanorods on CCs through a simple electrodeposition method. The one-step synthesized MnO2/CC electrodes with the advantages of low cost and being easily scalable exhibit considerable electrochemical properties with high specific capacitance and good cycling property, indicating their broad applications in flexible energy storage device.


## 2. Experimental

### 2.1. Materials

CC with hydrophilic surfaces was purchased from CeTech Co. Ltd (W0S 1002, Taiwan, China). All chemicals were of analytical grade. Acetone (AR,⩾99.5%), ethanol (AR, ⩾99.7%), MnSO4·H2O (AR, ⩾99.0%), and Na2SO4 (AR, ⩾99.0%) were purchased from Sinopharm Chemical Reagent Co. Ltd (SCR, Shanghai, China) and used as received without any further purification. Deionized (DI) water (18.2 MU cm) from Milli Q was used throughout the entire experiment, and all aqueous solutions were prepared with ultrapure water.


### 2.2. Synthesis of MnO2 on Carbon Cloth

The CC substrates were firstly cleaned by sonication sequentially in acetone, ethanol, and DI water for 30 min each. After being dried, an electrochemical deposition process was then conducted to decorate MnO2 nanostructures onto pristine CC using Autolab electrochemical workstation (PGSTAT-302 N, Eco Chemie B.V. Company, Utrecht, Netherlands) with a three-electrode system. The process was carried out under galvanostatic conditions at the constant current density of 1 mA/cm2. A precursor solution with equal volume of 0.1 M MnSO4·H2O and 0.1 M Na2SO4 was used as the electrolyte. The cleaned CC was used as working electrode, a platinum wire was used as counter electrode, and KCl-saturated Ag/AgCl was used as reference electrode. The formation of MnO2 in the electrochemical deposition process occurs via the following reactions [21]:(1)Mn2++2H2O⟶Mn3+Δ+1+Δe-⟶MnO2+4H++2e-Briefly, Mn(II) ion is firstly oxidized to the intermediate species of Mn(III) ion, which is thermodynamically unstable, and then disproportionation reaction of Mn(III) ion occurs to generate MnO2 before Mn(III) ion is reduced to be Mn(II) ion.By varying the depositing time from 10 min to 50 min, different morphologies of MnO2 films were obtained. After deposition, these samples were washed with distilled water to eliminate any loosely attached chemical substance and dried naturally, and then the flexible MnO2/CC electrodes were fabricated. The overall process is scalable.


### 2.3. Characterization

The morphologies of the samples were characterized by field emission scanning electron microscopy (FESEM, Hitachi, S-4800, Japan) equipped with energy-dispersive X-ray (EDX). The structures of the samples were examined by X-ray diffraction (XRD, Bruker D8 Advance) with Cu-Ka radiation (1.5418 Å) operating at 40 kV, 100 mA. X-ray photoelectron spectroscopy (XPS) was carried out at room temperature in ESCALAB 250 system. Cyclic voltammetry (CV) and electrochemical impedance spectroscopy (EIS) tests were conducted on an Autolab work station in 1 M Na2SO4 aqueous solution. Galvanostatic charging/discharging and cycling tests were conducted using a battery measurement system (LAND CT2001A, Wuhan LAND Electronics, Wuhan, China). All the electrochemical experiments were conducted at room temperature.


## 2.1. Materials

CC with hydrophilic surfaces was purchased from CeTech Co. Ltd (W0S 1002, Taiwan, China). All chemicals were of analytical grade. Acetone (AR,⩾99.5%), ethanol (AR, ⩾99.7%), MnSO4·H2O (AR, ⩾99.0%), and Na2SO4 (AR, ⩾99.0%) were purchased from Sinopharm Chemical Reagent Co. Ltd (SCR, Shanghai, China) and used as received without any further purification. Deionized (DI) water (18.2 MU cm) from Milli Q was used throughout the entire experiment, and all aqueous solutions were prepared with ultrapure water.


## 2.2. Synthesis of MnO2 on Carbon Cloth

The CC substrates were firstly cleaned by sonication sequentially in acetone, ethanol, and DI water for 30 min each. After being dried, an electrochemical deposition process was then conducted to decorate MnO2 nanostructures onto pristine CC using Autolab electrochemical workstation (PGSTAT-302 N, Eco Chemie B.V. Company, Utrecht, Netherlands) with a three-electrode system. The process was carried out under galvanostatic conditions at the constant current density of 1 mA/cm2. A precursor solution with equal volume of 0.1 M MnSO4·H2O and 0.1 M Na2SO4 was used as the electrolyte. The cleaned CC was used as working electrode, a platinum wire was used as counter electrode, and KCl-saturated Ag/AgCl was used as reference electrode. The formation of MnO2 in the electrochemical deposition process occurs via the following reactions [21]:(1)Mn2++2H2O⟶Mn3+Δ+1+Δe-⟶MnO2+4H++2e-Briefly, Mn(II) ion is firstly oxidized to the intermediate species of Mn(III) ion, which is thermodynamically unstable, and then disproportionation reaction of Mn(III) ion occurs to generate MnO2 before Mn(III) ion is reduced to be Mn(II) ion.By varying the depositing time from 10 min to 50 min, different morphologies of MnO2 films were obtained. After deposition, these samples were washed with distilled water to eliminate any loosely attached chemical substance and dried naturally, and then the flexible MnO2/CC electrodes were fabricated. The overall process is scalable.


## 2.3. Characterization

The morphologies of the samples were characterized by field emission scanning electron microscopy (FESEM, Hitachi, S-4800, Japan) equipped with energy-dispersive X-ray (EDX). The structures of the samples were examined by X-ray diffraction (XRD, Bruker D8 Advance) with Cu-Ka radiation (1.5418 Å) operating at 40 kV, 100 mA. X-ray photoelectron spectroscopy (XPS) was carried out at room temperature in ESCALAB 250 system. Cyclic voltammetry (CV) and electrochemical impedance spectroscopy (EIS) tests were conducted on an Autolab work station in 1 M Na2SO4 aqueous solution. Galvanostatic charging/discharging and cycling tests were conducted using a battery measurement system (LAND CT2001A, Wuhan LAND Electronics, Wuhan, China). All the electrochemical experiments were conducted at room temperature.


## 3. Results and Discussions

### 3.1. Structural Characterizations

After electrochemical deposition, MnO2 was successfully decorated onto the surface of CC. Different depositing durations were preset to investigate the morphology variation of the heterostructures. Typical SEM images of the MnO2/CC with different depositing time are shown in Figure 1, which clearly demonstrate that the well-established nano-MnO2 has been grown on CC. Figures 1(a), 1(c), 1(e), 1(g), and 1(i) show the carbon fiber after electrochemical deposition of MnO2 for 10, 20, 30, 40, and 50 min, respectively, while the enlarged SEM images of the corresponding local area are presented in Figures 1(b), 1(d), 1(f), 1(h), and 1(j), respectively. From the magnified SEM images, it can be found that MnO2 film consists of large quantities of nanorods, which appears to have a rough, uniform, and worm-like shape. With the relatively short electrochemical depositing duration such as 10 min, the CC surface is covered mostly by the MnO2 particle islands with some carbon fiber surface exposed to the environment (Figures 1(a) and 1(b)). When the depositing duration is prolonged, the MnO2 particle islands on the surface of the carbon fibers evolve into more compact film. With the depositing time more than 40 min, the carbon fiber is fully covered by dense MnO2 nanorods as shown in Figures 1(g)–1(j). These results indicate that the morphology of the product can be readily controlled by simply varying the depositing time of MnO2.Figure 1
SEM images of MnO2/CC integrated structures with the left side are low-magnitude views and with the right side are corresponding enlarged views of the left side.
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(j)EDX, XRD, and XPS analysis were employed to determine the composition and crystallinity of MnO2 deposits, as shown in Figure 2, where the typical MnO2/CC with depositing time of 40 min was chosen as the testing sample. The EDX analysis is conducted to study the chemical composition of the sample, as shown in Figure 2(a), in which C, Mn, and O elements can be detected. Considering that the C element is coming from the CC substrate, the nanostructure obtained by electrochemical deposition is manganese oxide. To explore the chemical structure and phase purity of the as-prepared deposit, XRD was employed as shown in Figure 2(b). Figure 2(b) shows the XRD patterns of the pristine CC and MnO2/CC composites. Compared with CC, two additional characteristic peaks at 36.9° and 66.3° (marked by black arrows) appear in the pattern of MnO2/CC composites, which endorse the presence of amorphous birnessite-type MnO2 (JCPDS, Card number 18-0802). It can be seen that these MnO2 peaks are broad and unclear, indicating the poor crystallinity and fine grain size of the deposition. No extra diffraction peaks other than MnO2 and carbon were detectable, implying the high purity of the product. From XRD data, the crystallite size of MnO2 nanoparticles is estimated to be 18.1 nm according to Scherrer’s equation.Figure 2
(a) EDX spectrums of MnO2/CC. (b) XRD patterns of MnO2/CC composites and CC. (c) XPS spectrums of MnO2/CC with the inset showing the Mn 2p spectrums.
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(c)The sample was further characterized by XPS to investigate the state of Mn within the composites, as shown in Figure2(c), which exhibits only signals from Mn, C, and O elements, corresponding to the result of EDX. The presence of manganese oxide is evidenced by Mn 3s and Mn 2p peaks along with O 1s and O 2s peaks. As shown in the inset of Figure 2(c), the Mn 2p region consists of a spin-orbit doublet of Mn 2p3/2 and Mn 2p1/2 located at 642.7 and 654.3 eV, respectively, with a spin-energy difference of 11.6 eV. These peak values are in good agreement with those reported for MnO2 [15, 22].


### 3.2. Electrochemical Evaluations

In order to examine the electrochemical characteristics of the obtained electrodes, samples with size of 1 cm2 were tested by CV measurements. The specific CV curves of the electrodes are shown in Figure 3(a) with MnO2 deposition of 0 min (pure CC), 10 min, 20 min, 30 min, 40 min, and 50 min at the scan rate of 50 mV/s in 1 M Na2SO4 electrolyte. The CV curves show a near symmetric rectangular shape and exhibit near mirror-image current response on voltage reversal, suggesting a fast, reversible reaction as well as excellent capacitive performance of the hybrid electrode. The specific geometric capacitance of pure CC, due to limited electroactive sites, is as low as 0.0168 mF/cm2 at the scan rate of 50 mV/s, and the specific geometric capacitance of CC is three magnitudes lower than that of MnO2/CC. Moreover, after deposition, carbon material underneath is blocked to participate in the charge storage process, considering the process is mainly conducted at or near the surface of the active materials. Hence, the capacitance contribution from carbon core can be negligible to the MnO2/CC composites.Figure 3
(a) CV of the pure CC and MnO2/CC composites at a scan rate of 50 mV/s in 1 M Na2SO4 electrolyte. (b) Gravimetric and geometric capacitance as a function of depositing time. (c) CV of the MnO2/CC-40 min at various scan rates. (d) Gravimetric capacitance of the MnO2/CC-40 min as a function of scan rate.
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(d)In Figure3(a), with short deposition time the CV curves are closer to rectangular shape, while with the deposition time extending CV curves deform gradually. This result is due to the fact that more MnO2 loading on the carbon surface participating in reactions and thus pseudocapacitance become the main electrochemical mechanism replacing double-capacitance. Moreover, for the depositing time from 10 min to 40 min, the geometric capacitance of MnO2/CC increases with the depositing time prolonged, while when the depositing duration continues to extend to 50 min, the geometric capacitance decreases (as shown in Figure 3(b)).As the corresponding mass uptake of MnO2 increases from 0.146 mg/cm2 to 0.715 mg/cm2, the specific gravimetric capacitance depending on the depositing time is plotted in Figure 3(b), in which the same tendency could also be found. That is to say, the specific capacitance of MnO2/CC rises from 91 F/g (10 min) to 177 F/g (40 min) and then drops to 122 F/g (50 min). This phenomenon can be explained as follows: when the depositing time is less than 40 min, the MnO2 film could not fully cover the carbon fiber and as the depositing time increases, the coverage ratio increases apparently (as shown in Figures 1(a)–1(f)); MnO2 film totally overlays carbon fiber at the depositing time of 40 min (as shown in Figures 1(g)–1(h)), and in this condition, its utilization is most sufficient; when the duration extends to 50 min, MnO2 loading continues to increase leading the film to be more compacting, which reduces the active site exposing to the electrolyte and thus limits the electrochemical performance of the hybrid electrode. These phenomena reveal that too thick MnO2 film may limit its optimal electrochemical performance as mentioned earlier. Thus, the employ of MnO2 film with appropriate thickness and surface morphology is critical to improving the performance of the hybrid electrode, which can be easily controlled by the fabrication process.The CV curves of the electrodes with 40 min deposition at different scan rates are shown in Figure3(c). It can be found that the CV shape remains nearly rectangular at a high scan rate of 100 mV/s, indicating a small polarization resistance. As the mass loading of MnO2 is 0.6428 mg/cm2 for 40 min depositing process, the calculated specific capacitance is 220 F/g at 5 mV/s and keeps 144 F/g at 100 mV/s scan rate, showing a good rate capability. The dependence of gravimetric capacitance on different scan rate is plotted in Figure 3(d). It is obvious that with the scan rate increasing the specific capacitance decreases substantially. The decline of specific capacitance can be explained as follows: at a low scan rate, the ions in the electrolyte can diffuse sufficiently into the MnO2 coatings for more charge storage, while at a higher scan rate, the diffusion time is reduced for insertion/extraction of protons or Na+, leading to a lower capacitance.The electrochemical performance of MnO2/CC-40 min electrode was further investigated by galvanostatic charging/discharging technique. Figure 4(a) shows the charging/discharging curves at various current densities from 0.5 to 15 mA/cm2. It could be observed that the discharge curves are symmetric with their corresponding charge counterparts, indicating superior reversibility and good Coulombic efficiency. These discharge curves are approximately straight line after a small voltage drop (IR drop), which reflects the equivalent series resistance of electrodes, that is, ionic resistance of electrolyte, intrinsic resistance of the hybrid electrode, and interfacial contact resistance between electrode and electrolyte. The specific capacitance obtained from the discharging curves is calculated according to the following equation [9]:(2)C=I×ΔtΔV×m,where I (mA) is the applied current, Δt (s) is the discharge time, ΔV (V) is the sweep potential range, and m (g) is the mass of active material, respectively.Figure 4
(a) Galvanostatic charging/discharging curves of MnO2/CC-40 min electrode at different current density. (b) Changing tendency of the specific capacitance depending on current densities.
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(b)As shown in Figure4(b), the specific capacitance of MnO2/CC-40 min decreases distinctly as the current density increases for low current density from 0.5 mA/cm2 (~193 F/g) to 4 mA/cm2 (~149 F/g). As the current density continues to increase to 15 mA/cm2, the areal capacitance drops very little and finally keeps stable (~149 F/g). It is noteworthy that the electrode maintained 77.2% retention of its initial specific capacitance measured at a high rate of 15 mA/cm2 (23.3 A/g), which is superior to the previously reported values of other MnO2/carbon-based electrodes including MnO2/CNT@carbon microelectrode (gravimetric capacitance remains less than 50% with the increase of current density from 0.5 mA/cm2 to 3 mA/cm2 [21]), MnO2/CFP (75% retention from 1 A/g to 10 A/g [23]), and PPy/MnO2@carbon cloth (capacitance retention of 70% from 0.2 A/g to 5 A/g [24]). Moreover, the specific capacitance of MnO2/CC-40 min electrode is substantially higher than the value reported for MnO2 nanosheets/carbon nanofibers (151.1 F/g at the current density of 1 A/g [15]). This suggests that our electrode with its prior feature for fast charge/discharge under a large current density might have huge potential in supercapacitor applications.Besides high specific capacitance, good cycling performance is also an important property for high-performance supercapacitors. The long-term stability of the MnO2/CC-40 min electrode was examined through galvanostatic charge/discharge cycling at a current density of 2 mA/cm2 in 1 M Na2SO4 electrolyte. Figure 5 displays the specific capacitance retention and Coulombic efficiency of the hybrid electrode as a function of charge/discharge cycling number. From this figure, the Coulombic efficiency keeps >95% from the 40th cycle and finally reaches to 99%. The capacitance retention decreases about 10% of the initial value over the first 300 cycles, while, then, remaining quite stable for the last 2200 cycles. The inset of Figure 5 shows the last several cycles of charging/discharging curves between −0.1 V and 0.7 V, which exhibit almost the same shape, revealing excellent long-term cyclability of the hybrid array electrode. The excellent cycling performance for MnO2/CC reveals the good structural stability as well as close contact between MnO2 nanorods and carbon fibers.Figure 5
Cycling performance and Coulombic efficiency of the electrode up to 2500 cycles at the current density of 2 mA/cm2. The inset showing the charging/discharging curves after 2000 cycles.To further understand the fundamental behavior of the prepared supercapacitor electrodes, EIS measurements for MnO2/CC electrodes with depositing time from 10 min to 50 min have been carried out and the corresponding Nyquist plots are shown in Figure 6. The EIS data can be fitted by an equivalent circuit consisting of internal resistance (Rs), charge transfer resistance (Rct), double-layer capacitance (Cdl), pseudocapacitance (Cps), and Warburg impedance (Zw), as presented in the inset of Figure 6. At high-frequency region, the Nyquist plots of MnO2/CC-10 min, MnO2/CC-20 min, MnO2/CC-30 min, and MnO2/CC-40 min show similar Rs of 1.68 Ω, 1.70 Ω, 1.77 Ω, and 1.77 Ω, respectively, while MnO2/CC-50 min has much higher Rs of 2.942 Ω, indicating the MnO2/CC electrodes with depositing time from 10 min to 40 min possess superior charge transport properties compared with MnO2/CC-50 min electrode. At low frequency region, the plots of MnO2/CC electrodes with deposition time from 10 min to 40 min demonstrate steeper Warburg tail, indicating their lower diffusion-resistance. Moreover, Cps for the five electrodes is calculated to be 0.00989 F, 0.01198 F, 0.01239 F, 0.01531 F, and 0.01221 F, respectively, representing the fact that the MnO2/CC-40 min electrode has the best capacitive property, which could be due to the optimized loading mass of electrochemical active material (MnO2), and thus providing reasonable active area for electrochemical reactions. All the results suggest that the MnO2/CC-40 min electrode has very small resistance with good ion response, indicating that the obtained structure could indeed act as a good supercapacitor electrode.Figure 6
Nyquist plots of the MnO2/CC electrode. The insets are the equivalent circuit and the magnification of Nyquist plots at high frequency.


## 3.1. Structural Characterizations

After electrochemical deposition, MnO2 was successfully decorated onto the surface of CC. Different depositing durations were preset to investigate the morphology variation of the heterostructures. Typical SEM images of the MnO2/CC with different depositing time are shown in Figure 1, which clearly demonstrate that the well-established nano-MnO2 has been grown on CC. Figures 1(a), 1(c), 1(e), 1(g), and 1(i) show the carbon fiber after electrochemical deposition of MnO2 for 10, 20, 30, 40, and 50 min, respectively, while the enlarged SEM images of the corresponding local area are presented in Figures 1(b), 1(d), 1(f), 1(h), and 1(j), respectively. From the magnified SEM images, it can be found that MnO2 film consists of large quantities of nanorods, which appears to have a rough, uniform, and worm-like shape. With the relatively short electrochemical depositing duration such as 10 min, the CC surface is covered mostly by the MnO2 particle islands with some carbon fiber surface exposed to the environment (Figures 1(a) and 1(b)). When the depositing duration is prolonged, the MnO2 particle islands on the surface of the carbon fibers evolve into more compact film. With the depositing time more than 40 min, the carbon fiber is fully covered by dense MnO2 nanorods as shown in Figures 1(g)–1(j). These results indicate that the morphology of the product can be readily controlled by simply varying the depositing time of MnO2.Figure 1
SEM images of MnO2/CC integrated structures with the left side are low-magnitude views and with the right side are corresponding enlarged views of the left side.
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(j)EDX, XRD, and XPS analysis were employed to determine the composition and crystallinity of MnO2 deposits, as shown in Figure 2, where the typical MnO2/CC with depositing time of 40 min was chosen as the testing sample. The EDX analysis is conducted to study the chemical composition of the sample, as shown in Figure 2(a), in which C, Mn, and O elements can be detected. Considering that the C element is coming from the CC substrate, the nanostructure obtained by electrochemical deposition is manganese oxide. To explore the chemical structure and phase purity of the as-prepared deposit, XRD was employed as shown in Figure 2(b). Figure 2(b) shows the XRD patterns of the pristine CC and MnO2/CC composites. Compared with CC, two additional characteristic peaks at 36.9° and 66.3° (marked by black arrows) appear in the pattern of MnO2/CC composites, which endorse the presence of amorphous birnessite-type MnO2 (JCPDS, Card number 18-0802). It can be seen that these MnO2 peaks are broad and unclear, indicating the poor crystallinity and fine grain size of the deposition. No extra diffraction peaks other than MnO2 and carbon were detectable, implying the high purity of the product. From XRD data, the crystallite size of MnO2 nanoparticles is estimated to be 18.1 nm according to Scherrer’s equation.Figure 2
(a) EDX spectrums of MnO2/CC. (b) XRD patterns of MnO2/CC composites and CC. (c) XPS spectrums of MnO2/CC with the inset showing the Mn 2p spectrums.
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(c)The sample was further characterized by XPS to investigate the state of Mn within the composites, as shown in Figure2(c), which exhibits only signals from Mn, C, and O elements, corresponding to the result of EDX. The presence of manganese oxide is evidenced by Mn 3s and Mn 2p peaks along with O 1s and O 2s peaks. As shown in the inset of Figure 2(c), the Mn 2p region consists of a spin-orbit doublet of Mn 2p3/2 and Mn 2p1/2 located at 642.7 and 654.3 eV, respectively, with a spin-energy difference of 11.6 eV. These peak values are in good agreement with those reported for MnO2 [15, 22].


## 3.2. Electrochemical Evaluations

In order to examine the electrochemical characteristics of the obtained electrodes, samples with size of 1 cm2 were tested by CV measurements. The specific CV curves of the electrodes are shown in Figure 3(a) with MnO2 deposition of 0 min (pure CC), 10 min, 20 min, 30 min, 40 min, and 50 min at the scan rate of 50 mV/s in 1 M Na2SO4 electrolyte. The CV curves show a near symmetric rectangular shape and exhibit near mirror-image current response on voltage reversal, suggesting a fast, reversible reaction as well as excellent capacitive performance of the hybrid electrode. The specific geometric capacitance of pure CC, due to limited electroactive sites, is as low as 0.0168 mF/cm2 at the scan rate of 50 mV/s, and the specific geometric capacitance of CC is three magnitudes lower than that of MnO2/CC. Moreover, after deposition, carbon material underneath is blocked to participate in the charge storage process, considering the process is mainly conducted at or near the surface of the active materials. Hence, the capacitance contribution from carbon core can be negligible to the MnO2/CC composites.Figure 3
(a) CV of the pure CC and MnO2/CC composites at a scan rate of 50 mV/s in 1 M Na2SO4 electrolyte. (b) Gravimetric and geometric capacitance as a function of depositing time. (c) CV of the MnO2/CC-40 min at various scan rates. (d) Gravimetric capacitance of the MnO2/CC-40 min as a function of scan rate.
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(d)In Figure3(a), with short deposition time the CV curves are closer to rectangular shape, while with the deposition time extending CV curves deform gradually. This result is due to the fact that more MnO2 loading on the carbon surface participating in reactions and thus pseudocapacitance become the main electrochemical mechanism replacing double-capacitance. Moreover, for the depositing time from 10 min to 40 min, the geometric capacitance of MnO2/CC increases with the depositing time prolonged, while when the depositing duration continues to extend to 50 min, the geometric capacitance decreases (as shown in Figure 3(b)).As the corresponding mass uptake of MnO2 increases from 0.146 mg/cm2 to 0.715 mg/cm2, the specific gravimetric capacitance depending on the depositing time is plotted in Figure 3(b), in which the same tendency could also be found. That is to say, the specific capacitance of MnO2/CC rises from 91 F/g (10 min) to 177 F/g (40 min) and then drops to 122 F/g (50 min). This phenomenon can be explained as follows: when the depositing time is less than 40 min, the MnO2 film could not fully cover the carbon fiber and as the depositing time increases, the coverage ratio increases apparently (as shown in Figures 1(a)–1(f)); MnO2 film totally overlays carbon fiber at the depositing time of 40 min (as shown in Figures 1(g)–1(h)), and in this condition, its utilization is most sufficient; when the duration extends to 50 min, MnO2 loading continues to increase leading the film to be more compacting, which reduces the active site exposing to the electrolyte and thus limits the electrochemical performance of the hybrid electrode. These phenomena reveal that too thick MnO2 film may limit its optimal electrochemical performance as mentioned earlier. Thus, the employ of MnO2 film with appropriate thickness and surface morphology is critical to improving the performance of the hybrid electrode, which can be easily controlled by the fabrication process.The CV curves of the electrodes with 40 min deposition at different scan rates are shown in Figure3(c). It can be found that the CV shape remains nearly rectangular at a high scan rate of 100 mV/s, indicating a small polarization resistance. As the mass loading of MnO2 is 0.6428 mg/cm2 for 40 min depositing process, the calculated specific capacitance is 220 F/g at 5 mV/s and keeps 144 F/g at 100 mV/s scan rate, showing a good rate capability. The dependence of gravimetric capacitance on different scan rate is plotted in Figure 3(d). It is obvious that with the scan rate increasing the specific capacitance decreases substantially. The decline of specific capacitance can be explained as follows: at a low scan rate, the ions in the electrolyte can diffuse sufficiently into the MnO2 coatings for more charge storage, while at a higher scan rate, the diffusion time is reduced for insertion/extraction of protons or Na+, leading to a lower capacitance.The electrochemical performance of MnO2/CC-40 min electrode was further investigated by galvanostatic charging/discharging technique. Figure 4(a) shows the charging/discharging curves at various current densities from 0.5 to 15 mA/cm2. It could be observed that the discharge curves are symmetric with their corresponding charge counterparts, indicating superior reversibility and good Coulombic efficiency. These discharge curves are approximately straight line after a small voltage drop (IR drop), which reflects the equivalent series resistance of electrodes, that is, ionic resistance of electrolyte, intrinsic resistance of the hybrid electrode, and interfacial contact resistance between electrode and electrolyte. The specific capacitance obtained from the discharging curves is calculated according to the following equation [9]:(2)C=I×ΔtΔV×m,where I (mA) is the applied current, Δt (s) is the discharge time, ΔV (V) is the sweep potential range, and m (g) is the mass of active material, respectively.Figure 4
(a) Galvanostatic charging/discharging curves of MnO2/CC-40 min electrode at different current density. (b) Changing tendency of the specific capacitance depending on current densities.
(a)
(b)As shown in Figure4(b), the specific capacitance of MnO2/CC-40 min decreases distinctly as the current density increases for low current density from 0.5 mA/cm2 (~193 F/g) to 4 mA/cm2 (~149 F/g). As the current density continues to increase to 15 mA/cm2, the areal capacitance drops very little and finally keeps stable (~149 F/g). It is noteworthy that the electrode maintained 77.2% retention of its initial specific capacitance measured at a high rate of 15 mA/cm2 (23.3 A/g), which is superior to the previously reported values of other MnO2/carbon-based electrodes including MnO2/CNT@carbon microelectrode (gravimetric capacitance remains less than 50% with the increase of current density from 0.5 mA/cm2 to 3 mA/cm2 [21]), MnO2/CFP (75% retention from 1 A/g to 10 A/g [23]), and PPy/MnO2@carbon cloth (capacitance retention of 70% from 0.2 A/g to 5 A/g [24]). Moreover, the specific capacitance of MnO2/CC-40 min electrode is substantially higher than the value reported for MnO2 nanosheets/carbon nanofibers (151.1 F/g at the current density of 1 A/g [15]). This suggests that our electrode with its prior feature for fast charge/discharge under a large current density might have huge potential in supercapacitor applications.Besides high specific capacitance, good cycling performance is also an important property for high-performance supercapacitors. The long-term stability of the MnO2/CC-40 min electrode was examined through galvanostatic charge/discharge cycling at a current density of 2 mA/cm2 in 1 M Na2SO4 electrolyte. Figure 5 displays the specific capacitance retention and Coulombic efficiency of the hybrid electrode as a function of charge/discharge cycling number. From this figure, the Coulombic efficiency keeps >95% from the 40th cycle and finally reaches to 99%. The capacitance retention decreases about 10% of the initial value over the first 300 cycles, while, then, remaining quite stable for the last 2200 cycles. The inset of Figure 5 shows the last several cycles of charging/discharging curves between −0.1 V and 0.7 V, which exhibit almost the same shape, revealing excellent long-term cyclability of the hybrid array electrode. The excellent cycling performance for MnO2/CC reveals the good structural stability as well as close contact between MnO2 nanorods and carbon fibers.Figure 5
Cycling performance and Coulombic efficiency of the electrode up to 2500 cycles at the current density of 2 mA/cm2. The inset showing the charging/discharging curves after 2000 cycles.To further understand the fundamental behavior of the prepared supercapacitor electrodes, EIS measurements for MnO2/CC electrodes with depositing time from 10 min to 50 min have been carried out and the corresponding Nyquist plots are shown in Figure 6. The EIS data can be fitted by an equivalent circuit consisting of internal resistance (Rs), charge transfer resistance (Rct), double-layer capacitance (Cdl), pseudocapacitance (Cps), and Warburg impedance (Zw), as presented in the inset of Figure 6. At high-frequency region, the Nyquist plots of MnO2/CC-10 min, MnO2/CC-20 min, MnO2/CC-30 min, and MnO2/CC-40 min show similar Rs of 1.68 Ω, 1.70 Ω, 1.77 Ω, and 1.77 Ω, respectively, while MnO2/CC-50 min has much higher Rs of 2.942 Ω, indicating the MnO2/CC electrodes with depositing time from 10 min to 40 min possess superior charge transport properties compared with MnO2/CC-50 min electrode. At low frequency region, the plots of MnO2/CC electrodes with deposition time from 10 min to 40 min demonstrate steeper Warburg tail, indicating their lower diffusion-resistance. Moreover, Cps for the five electrodes is calculated to be 0.00989 F, 0.01198 F, 0.01239 F, 0.01531 F, and 0.01221 F, respectively, representing the fact that the MnO2/CC-40 min electrode has the best capacitive property, which could be due to the optimized loading mass of electrochemical active material (MnO2), and thus providing reasonable active area for electrochemical reactions. All the results suggest that the MnO2/CC-40 min electrode has very small resistance with good ion response, indicating that the obtained structure could indeed act as a good supercapacitor electrode.Figure 6
Nyquist plots of the MnO2/CC electrode. The insets are the equivalent circuit and the magnification of Nyquist plots at high frequency.


## 4. Conclusion

In summary, MnO2 nanorods were successfully synthesized on flexible CC substrates through a facile electrodepositing method. The effect of depositing time on the morphology and electrochemical properties of the composites has been investigated, verifying that the MnO2/CC electrode with 40 min depositing time demonstrates optimal specific capacitance, good rate capability, and good cyclic stability. Such excellent electrochemical properties are attributed to the synergetic effect of nanostructured MnO2 and interconnected porous CC acting as a conductive backbone. The prepared electrode may have promising potential as the high-performance flexible supercapacitor.



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*Source: 7340961-2017-04-06.xml*