- About this Journal ·
- Abstracting and Indexing ·
- Aims and Scope ·
- Article Processing Charges ·
- Articles in Press ·
- Author Guidelines ·
- Bibliographic Information ·
- Citations to this Journal ·
- Contact Information ·
- Editorial Board ·
- Editorial Workflow ·
- Free eTOC Alerts ·
- Publication Ethics ·
- Reviewers Acknowledgment ·
- Submit a Manuscript ·
- Subscription Information ·
- Table of Contents
Volume 2014 (2014), Article ID 826832, 7 pages
Reduced Graphene Oxide Supported Antimony Species for High-Performance Supercapacitor Electrodes
1Department of Inorganic, Analytical Chemistry and Electrochemistry, Faculty of Chemistry, Silesian University of Technology, Krzywoustego 6, 44-100 Gliwice, Poland
2Department of Biomaterials, Faculty of Materials Science and Ceramics, AGH University of Science and Technology, Mickiewicza 30, 30-059 Krakow, Poland
Received 15 January 2014; Accepted 11 February 2014; Published 5 March 2014
Academic Editors: D. Pavlov and E. Vallès
Copyright © 2014 Mateusz Ciszewski et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.
Antimony species was chemically anchored on graphene oxide using antimony (III) chloride precursor and then converted to the reduced graphene oxide-antimony species composite by a well-established polyol method. The resultant composite was successfully used as supercapacitor electrodes in a two-electrode symmetric system with aqueous electrolyte. The specific capacitance calculated from the galvanostatic charge/discharge curves obtained for this composite was 289 F/g. The enhanced capacitance results were confirmed by the electrochemical impedance spectroscopy and cyclic voltammetry. The high capacitance of the reduced graphene oxide-antimony species composite arises from the combination of double-layer charging and pseudocapacitance caused by the Faradaic reactions of the intercalated antimony species and residual surface-bonded functional groups.
Antimony is widely used in semiconductors, antifriction alloys, small arms and tracer bullets, and cable sheathing and in large quantities as a flame retarding additive . It has been widely used in the past to enhance the hardness and the mechanical stability of lead alloys in batteries . However, its usage was gradually limited because of toxicity, mostly of the trivalent species. In the lead batteries, antimony is generally known to be able to pass on a negative electrode through corrosion of current leads and decrease in the battery service life . The detailed description of antimony reactions in lead batteries was given by Pavlov et al. , who suggested that the influence of the antimony on the lead battery work depends on antimony species used in battery preparation. In case of the lead electrodes immersed in the antimony solution, formation of ions is observed that passivates the lead and decreases the capacitance. While for Pb-Sb alloys in sulfuric acid solution formation of antimony complexes of the type is observed that have a beneficial effect on the capacitance of electrodes. It is well known that antimony corrodes easily but results  suggest that the antimony-containing corrosion layer discharges with difficulty, and thus the active material discharges more readily than the corrosion layer and a passivation layer does not form at the grid/active material interface. So it appears that addition of antimony to the active material of electrode effectively retards capacitance loss. These opinions seem to be true because antimony has been thoroughly examined as an additive in newer energy sources, that is, lithium-ion batteries, liquid metal batteries, and fuel cells.
In the lithium-ion batteries, antimony is thought to play two roles. First, it acts as a spacer to prevent large volume changing of electrode during charging/discharging cycles; second, it can accommodate about 3 lithium atoms and give an additional capacitance. Problem of anode pulverization during electrode working was examined mainly by Besenhard [6, 7] who suggested that improvement of cycling performance of the lithium-ion batteries can be achieved by replacing large metallic particles with smaller micro- and nanoscale multiphase. Billaud [8–10] studied methods of antimony-based graphite composites preparation by reduction of antimony (V) chloride with sodium hydride and alloying antimony with alkali metals. Except for antimony-graphite composites, there have been proposed many other combinations of antimony with metals and metal oxides [11, 12]. In tin oxide, additional atoms like antimony or indium may increase the electrical conductivity, mechanical stability, and the free electron concentration [13–15].
These researches indicate that antimony chemistry may play a crucial role in the new energy storage systems. As far as we know, application of graphene oxide-antimony species composites as a supercapacitor electrode was never reported before, though we have found some preliminary trials to synthesize peroxoantimonates on graphene oxide , simulate antimony (V) chloride intercalations into graphene sheets , and remove of antimony (III) from aqueous solution using graphene . Electrochemical supercapacitors are promising energy storage systems due to low cost, long cycle life, and high power density that may be applied in many areas: video recorders, back-up memories, traffic warning signals, roadway display devices, and as the short time energy storage devices in electric vehicles and hybrid electric vehicles. Their high specific power can be used in engine starting and acceleration, loads lifting, and keeping the electric trains moving. Electrochemical supercapacitors, briefly, store electric energy in an electrochemical double-layer, so-called Helmholtz layer, forming the solid electrolyte interface. As their capacitance is proportional to the surface area of the electrode material, highly porous, chemically and electrochemically inert carbons are considered as good candidates for supercapacitor matrices. Activated carbon that can be easily prepared from the various natural or synthetic precursors and can possess well-defined pore structure is still the main supercapacitors material because of very high surface area, low price, and light weight . This situation may change using graphene, the parent of all graphitic forms, which emerges as a material of great interest due to its remarkable physical, chemical, and electrical properties.
It has high theoretical surface area up to 2630 m2/g, Young’s modulus as high as 1 TPa, and thermal conductivity of 5000 W/(mK) [20, 21], which are beneficial for the capacitance performance. The prominent feature of graphene and graphene oxide is that they can form composites easily. In this case, naturally occurring electric double-layer effect can be enhanced by pseudocapacitance. Metals and metal oxides are most often suggested as graphene and graphene oxide additives that can be used in supercapacitor electrodes because of additional redox reactions that improve capacitance. Scientific interest is mainly focused on transition metals and tin composites with graphene oxide or reduced graphene oxide [22–24]. As antimony exhibited the advantageous effects in the lead acid batteries and lithium-ion batteries, it has been tried to embed antimony species into graphene oxide and examine this composite as the electrode for supercapacitor.
2.1. Preparation of Antimony Composites
Graphite oxide (GO) was synthesized by a modified Staudenmaier method  from the synthetic graphite (SGL Company). The polyol method  was used to prepare reduced graphene oxide-antimony oxide hydroxide composite. Briefly, 300 mg GO was ultrasonicated in 1 : 3 deionized water : ethylene glycol (Chempur) solution for 1 h, resulting in graphene oxide suspension. Then, 0.337 g SbCl3 (Acros) was added, pH was adjusted above 11 by 1 M NaOH, and solution was magnetically mixed for 3 h at 600 rpm. Mixture was refluxed at 120°C for 3 h to reduce graphene oxide. Product was diluted with demineralized water, vacuum-filtrated on a fritted-glass funnel using filter paper with narrow pores (Munktel, Grade 390), and washed with water until neutral pH. Solid product was dried at 110°C in an oven for 2 h and reduced graphene oxide-antimony species composite was labeled as RGOSb.
Materials were characterized with powder X-ray diffraction (XRD, X’Pert Pro, Philips) with a step size 0.02° and Cu Kα radiation to evaluate reduction progress and identify antimony species. The crystallite height () has been examined from XRD signals based on the Scherrer equation ( = 0.9λ/B cos ), where is the wavelength of X-ray, is the Bragg’s diffraction angle, and B is a full width at half maximum (FWHM). The morphology of the products was characterized by scanning electron microscopy (SEM, Hitachi TM-3000). Raman spectroscopy was performed by using a Renishaw InVia with 514 nm laser excitation. The infrared spectra were measured on a Nicolet 6700 Fourier-transformed infrared spectrophotometer (FT-IR) with attenuated total reflectance (ATR method).
2.3. Electrochemical Measurements
All electrochemical experiments were performed with Autolab PGSTAT 30 workstation using the two-electrode symmetric system. The working electrode and counter/reference electrode, composed of 15 mg of active material and 2.5 mg polytetrafluoroethylene (PTFE) binder (Sigma Aldrich, 35 μm), were pasted on two electrochemical nickel current collectors and separated with PTFE membrane (Whatman, 90 μm thickness) soaked with 6 M KOH. Weight of the electrodes was accurately determined by a high precision balance (Mettler Toledo AT 261 DeltaRange). The cells were tested by the cyclic voltammetry (CV) at scan rates 5 mV/s, 20 mV/s, and 500 mV/s, galvanostatic charge/discharge (GD), and electrochemical impedance spectroscopy (EIS) in frequency range from 100 kHz to 100 mHz. The impedance measurements were performed at an open circuit voltage with a 10 mV voltage amplitude. The specific capacitance values were obtained from the galvanostatic charge/discharge curves using = it/(mdU), where is the current, t is the discharge time, m is the mass of active material of the one electrode, and dU is the range of voltage. Capacitance was also obtained from the CV curves using the following formula: where , , , and are the initial potential, final potential, scan rate, and mass of the active material of one electrode, respectively. Using EIS method, capacitance was obtained from , where is the signal frequency and is the imaginary resistance.
As mentioned previously, the polyol process using mixture of ethylene glycol and water was used to prepare reduced graphene oxide-antimony species composite. In comparison to the traditional reduction method using hydrazine or metal hydrides, the polyol process demonstrates an enhanced control of uniform metal dispersion and deposition as well as homogenous in situ generation of reducing species . Antimony (III) chloride was used as a metal precursor. It is thought that this compound converts into antimony (III) oxide in basic pH ; however, at lower temperature more probably trivalent antimony hydroxide is formed . Filella et al.  suggest that in the broad pH range from 2 up to 10 probably Sb(OH)3 or SbO(OH), called meta-antimonious acid (HSbO2), is formed.
The exact formula of the antimony species after hydrolysis at high pH is precisely not known.
It was not possible to univocally identify the obtained XRD pattern. Except for typical and characteristic broad graphitic signal located near 25 degrees satisfying GO reduction, there were sharp signals belonging to antimony species recognized as the antimony oxide hydroxide of the form Sb3O6OH and antimony oxide hydrated Sb2O5*4H2O. Figure 1 shows the powder XRD patterns of the parent graphite, GO, and RGOSb composite.
RGOSb composite was prepared in ethylene glycol that satisfied complete and uniform reduction of graphene oxide. Consequently, the broad signal in the graphitic region with the interlayer distance similar to that of parent graphite was observed. The XRD pattern of the RGOSb composite revealed also well-developed reflections of antimony species. This finding implies that the antimony salt truly cannot simply convert into antimony oxide but the oxide hydroxide or hydrated forms are preferred. Presence of antimony (III) and (V) in the composite may suggest partial oxidation of antimony by GO.
SEM micrographs show the morphology of graphite, graphite oxide, and reduced graphene oxide-antimony species. Graphite intercalated by the oxygen-containing groups after oxidation has a rose-like, corrugated structure that can be observed in a Figure 2(b). As it was calculated from the XRD data, the crystallite height decreased significantly from 19.8 nm for graphite to 0.9 nm for GO. SEM micrograph of the RGOSb (Figure 2(c)) showed GO structure reduced in ethylene glycol with the antimony species intercalated between graphene layers. In RGOSb, an increase of the to 3.3 nm (calculated for reduced graphene oxide) caused by stacking of some of the graphene layers after reduction was observed.
Raman spectroscopy is a useful method to investigate hybridization of carbon atoms and defects and crystal disorder of graphene composites. Figure 3 presents Raman spectra recorded for the graphite, GO, and RGOSb. There are observed two vibration bands the D around 1,355 cm−1 and the G around 1,580 cm−1. The D band, corresponding to material disorder, is very small in highly ordered graphite structure, which is composed of equally distant, flat graphene layers consisting of sp2-hybridized carbon atoms; however, after oxidation, the D band intensity increases because of an increase in disorder caused by the oxygen-containing functional groups. In RGOSb, the D band intensity is higher than the G band because corrugated graphene layers of GO are partially separated by the reducing agent and smaller crystallites are formed. Additionally, the higher D band intensity in the RGOSb can be attributed to the formation of more defects in GO sheets during metal intercalation.
The G band that corresponds to sp2 carbons is broadened after oxidation and its intensity with respect to the D band diminishes due to change of the carbon atoms hybridization from sp2 to sp3. This effect is more marked in the RGOSb, where most of the residual sp2 carbon atoms are converted to sp3 and bonded to the intercalating molecules.
The intensity ratio is a convenient measure of disordered carbon that corresponds to amount of sp3 and sp2 carbon atoms. Graphite, possessing ordered and layered structure with high crystallite size, has the ratio of 0.34 and of GO 0.89 due to the increase in disorder of turbostratically aligned graphene layers and diminishing of randomly located crystallite size, while for RGOSb this ratio is 1.24 that is higher than for GO.
Qualitative analysis of composite and its precursor was performed using infrared spectroscopy. Figure 4 shows FTIR spectra recorded for GO and graphene oxide-antimony composite. GO spectrum shows a broad signal located at 3,700–2,800 cm−1 attributed to the stretching vibration in hydroxyl groups and water molecules, signal at 1,700 cm−1 belonging to the carboxylic groups, signal at 1,600 cm−1 belonging to OH groups, 1,350 cm−1 due to deformation vibration in C–OH, 1,024 cm−1 represented by C–O groups, and finally peak around 940 cm−1 from epoxy groups.
After reduction of the composite in ethylene glycol, most of the signals disappeared, only one signal of the residual OH groups (higher magnification) located around 1,350 cm−1 was observed. This may indicate very efficient graphene oxide reduction in ethylene glycol; however, difficulties in removal of the OH groups from graphene oxide by chemical reduction were confirmed .
Electrodes were characterized in the two-electrode cell by the cyclic voltammetry, galvanostatic charge/discharge, and electrochemical impedance spectroscopy. The CV curves show the reversible charge/discharge characteristics of the composite electrode. Experiments were carried out at scan rate 5 mV/s, 20 mV/s, and 500 mV/s in two potential windows from 0 to 1 V and from −0.5 to +0.5 V. The potential window 0-1 V is more often used in aqueous electrolyte supercapacitors experiments ; therefore, it was mainly used, while −0.5 to +0.5 V window was used comparatively. Figure 5 compares the CV curves in the potential windows from 0 to 1 V and from −0.5 to +0.5 V obtained for parent graphite (gray), graphite oxide (red), and reduced graphene oxide-antimony species composite (blue) at the scan rate 20 mV/s.
The well-developed supercapacitor has to satisfy two conditions, namely, operate in a possibly high current and have a box-like rectangular shape. Based on a Figure 5, it can be noticed that the most rectangular shape was recorded for the reduced graphene oxide-antimony species composite. It should be pointed out that better shape was obtained in −0.5 to +0.5 V. Although shape of the graphite and graphite oxide CV curves was acceptable, the average charging/discharging current was very low. The lowest average charging current and consequently the lowest specific capacitance was obtained for GO 0.00001 A and less than 1 F/g after 100 cycles. Amazingly high electrical resistivity cannot be balanced by the additional redox reactions of the oxygen-containing groups. Even for graphite, the average charging current was 50 times higher, that is, 0.0005 A with specific capacitance as high as 3 F/g. For RGOSb, the recorded charging current was 0.002 A and specific capacitance calculated from the CV curves was 13 F/g after 100 cycles. Cyclability of RGOSb in comparison with graphite and graphite oxide was checked at scan rate 500 mV/s and 1000 cycles in a potential range 0-1 V; the resulting CV curves were presented in Figure 6(a).
After 1000 cycles the specific capacitance of graphite dropped to 50% of the initial with a charging current of 0.0015 A, while for GO difference between the first and the last step was quite small with the average charging current of 0.0004 A. In RGOSb, once again the highest average charging current of 0.009 A and more rectangular shape were recorded; however, the specific capacitance dropped to 80% of the initial value. Additionally, Figure 6(b) presents shape difference of the CV curves recorded for RGOSb at 5 mV/s and 100 cycles in potential ranges 0-1 V and −0.5 to +0.5 V. This experiment showed that more ideal behavior was obtained for −0.5 to +0.5 V; however, higher current and higher specific capacitance may be obtained for voltage range 0-1 V.
These results show univocally that antimony species in oxide hydroxide or hydrated form is able to enhance the specific capacitance of graphite oxide many times. This is mainly attributed to the additional Faradaic reactions of the active antimony species with the electrolyte. Although it has been demonstrated in literature that the oxygen-containing functional groups of graphite oxide can enhance the total capacitance through Faradaic reactions and may improve the wettability of porous carbon with electrolytes , it was not observed here; however, the enhanced capacitance was obtained for GO modified with antimony species.
The galvanostatic charge/discharge is the most credible method to calculate the specific capacitance. It is used to show real capacitance value and charge/discharge characteristics of energy storing materials. Figure 7 shows the galvanostatic charge/discharge curves obtained for RGOSb at different charge and discharge times.
RGOSb was galvanostatically charged at 0.004 A for 100 s (light blue) and 200 s (dark blue) and discharged for 700 s and 1000 s, respectively. The specific capacitance obtained from these measurements was 244 F/g at shorter discharge time and 289 F/g after 1000 s. In both cases, quite unsymmetrical galvanostatic curves with quick charging and very long discharge time were obtained preceded by iR drop. The specific capacitance for RGOSb was much higher than that obtained for graphite and graphite oxide, 12 F/g and 4 F/g, respectively.
Figure 8 shows the Nyquist plots of the impedance measured at an equilibrium open circuit potential (0 V) in the frequency range from 100 kHz to 100 mHz. EIS plots present the quasireversible behavior of the reduced graphene oxide-antimony species composite.
Generally, in the RGOSb composite, two regions can be distinguished including the semicircle corresponding to the Faradaic charge transfer resistance  and straight line in the low-frequency region indicating a pure capacitive behavior and representing the ion diffusion in the electrode structure. Steeper curve in the low-frequency region is attributed to the better Warburg diffusion. It is caused by an improved effective mass transfer from the electrolyte to the electrode interface in the composite. Neither in graphite nor in graphite oxide the semicircle was observed; however, graphite had steeper line in the low-frequency region. The maximum values of real resistance obtained for graphite, GO, and RGOSb were 100 Ω, 880 Ω, and 19 Ω, respectively. Consequently, the specific capacitance obtained for RGOSb using the EIS method was about 75 times higher than that obtained for GO and about 10 times higher than that obtained for graphite.
In this work, the new reduced graphene oxide-antimony species composite has been prepared and characterized for supercapacitor electrodes. The polyol process was used to prepare dispersion of antimony active species in reduced graphene oxide. This method did not require thermal annealing of the active species into antimony oxides. It showed the enhanced specific capacitance, as high as 289 F/g, resulting from the pseudocapacitance and very good cyclability with respect to the parent graphite and graphite oxide.
Conflict of Interests
The authors declare that there is no conflict of interests regarding the publication of this paper.
- M. Filella, N. Belzile, and Y.-W. Chen, “Antimony in the environment: a review focused on natural waters I. Occurence,” Earth-Science Reviews, vol. 57, no. 1-2, pp. 125–176, 2002.
- M. Kentner, M. Leinemann, K.-H. Schaller, D. Weltle, and G. Lehnert, “External and internal antimony exposure in starter battery production,” International Archives of Occupational and Environmental Health, vol. 67, no. 2, pp. 119–123, 1995.
- Y. B. Kamenev, A. V. Kiselevich, E. I. Ostapenko, and Y. V. Skachkov, “Antimony-free alloys for unattended (sealed) lead batteries,” Russian Journal of Applied Chemistry, vol. 75, no. 4, pp. 548–551, 2002.
- D. Pavlov, A. Dakhouche, and T. Rogachev, “Influence of antimony ions and PbSO4 content in the corrosion layer on the properties of the grid/active mass interface in positive lead-acid battery plates,” Journal of Applied Electrochemistry, vol. 27, no. 6, pp. 720–730, 1997.
- M. Kosai, S. Yasukawa, S. Osumi, and M. Tsubota, “Effect of antimony on premature capacity loss of lead/acid batteries,” Journal of Power Sources, vol. 67, no. 1-2, pp. 43–48, 1997.
- J. Yang, M. Winter, and J. O. Besenhard, “Small particle size multiphase Li-alloy anodes for lithium-ion-batteries,” Solid State Ionics, vol. 90, no. 1–4, pp. 281–287, 1996.
- A. Trifonova, M. Wachtler, M. Winter, and J. O. Besenhard, “Sn-Sb and Sn-Bi alloys as anode materials for lithium-ion batteries,” Ionics, vol. 8, no. 5-6, pp. 321–328, 2002.
- A. Dailly, P. Willmann, and D. Billaud, “Synthesis, characterization and electrochemical performances of new antimony-containing graphite compounds used as anodes for lithium-ion batteries,” Electrochimica Acta, vol. 48, no. 3, pp. 271–278, 2002.
- A. Dailly, R. Schneider, D. Billaud, Y. Fort, and P. Willmann, “New graphite-antimony composites as anodic materials for lithium-ion batteries. Preparation, characterisation and electrochemical performance,” Electrochimica Acta, vol. 47, no. 26, pp. 4207–4212, 2002.
- A. Dailly, R. Schneider, D. Billaud, Y. Fort, and J. Ghanbaja, “Nanometric antimony powder synthesis by activated alkaline hydride reduction of antimony pentachloride,” Journal of Nanoparticle Research, vol. 5, no. 3-4, pp. 389–393, 2003.
- S. Saadat, Y. Y. Tay, J. Zhu et al., “Template-free electrochemical deposition of interconnected ZnSb nanoflakes for Li-Ion battery anodes,” Chemistry of Materials, vol. 23, no. 4, pp. 1032–1038, 2011.
- J. M. Mosby and A. L. Prieto, “Direct electrodeposition of Cu2Sb for lithium-ion battery anodes,” Journal of the American Chemical Society, vol. 130, no. 32, pp. 10656–10661, 2008.
- F. D. Wu, M. Wu, and Y. Wang, “Antimony-doped tin oxide nanotubes for high capacity lithium storage,” Electrochemistry Communications, vol. 13, no. 5, pp. 433–436, 2011.
- F. Montilla, E. Morallón, A. de Battisti, A. Benedetti, H. Yamashita, and J. L. Vázquez, “Preparation and characterization of antimony-doped tin dioxide electrodes. Part 2. XRD and EXAFS characterization,” Journal of Physical Chemistry B, vol. 108, no. 16, pp. 5044–5050, 2004.
- Y. Wang, I. Djerdj, B. Smarsly, and M. Antonietti, “Antimony-doped SnO2 nanopowders with high crystallinity for lithium-ion battery electrode,” Chemistry of Materials, vol. 21, no. 14, pp. 3202–3209, 2009.
- S. Sladkevich, J. Gun, P. V. Prikhodchenko et al., “The formation of a peroxoantimonate thin film coating on graphene oxide (GO) and the influence of the GO on its transformation to antimony oxides and elemental antimony,” Carbon, vol. 50, no. 15, pp. 5463–5471, 2012.
- R. A. Nistor, D. M. Newns, and G. J. Martyna, “The role of chemistry in graphene doping for carbon-based electronics,” ACS Nano, vol. 5, no. 4, pp. 3096–3103, 2011.
- Y. Leng, W. Guo, S. Su, C. Yi, and L. Xing, “Removal of antimony(III) from aqueous solution by graphene as an adsorbent,” Chemical Engineering Journal, vol. 211-212, pp. 406–411, 2012.
- M. Zhu, C. J. Weber, Y. Yang et al., “Chemical and electrochemical ageing of carbon materials used in supercapacitor electrodes,” Carbon, vol. 46, no. 14, pp. 1829–1840, 2008.
- C. Lee, X. Wei, J. W. Kysar, and J. Hone, “Measurement of the elastic properties and intrinsic strength of monolayer graphene,” Science, vol. 321, no. 5887, pp. 385–388, 2008.
- A. A. Balandin, S. Ghosh, W. Bao et al., “Superior thermal conductivity of single-layer graphene,” Nano Letters, vol. 8, no. 3, pp. 902–907, 2008.
- X. Zhu, H. Dai, J. Hu, L. Ding, and L. Jiang, “Reduced graphene oxide-nickel oxide composite as high performance electrode materials for supercapacitors,” Journal of Power Sources, vol. 203, pp. 243–249, 2012.
- L. Wang, D. Wang, J. Zhu, and X. Liang, “Preparation of Co3O4 nanoplate/graphene sheet composites and their synergistic electrochemical performance,” Ionics, vol. 19, no. 2, pp. 215–220, 2013.
- Y. Wang, T. Brezesinski, M. Antonietti, and B. Smarsly, “Ordered mesoporous Sb-, Nb-, and Ta-doped SnO2 thin films with adjustable doping levels and high electrical conductivity,” ACS Nano, vol. 3, no. 6, pp. 1373–1378, 2009.
- L. Staudenmaier, “Verfahren zur Darstellung der Graphitsaure,” Berichte der Deutschen Chemischen Gesellschaft, vol. 31, no. 2, pp. 1481–1487, 1898.
- Z. Liu, J. Y. Lee, W. Chen, M. Han, and L. M. Gan, “Physical and electrochemical characterizations of microwave-assisted polyol preparation of carbon-supported PtRu nanoparticles,” Langmuir, vol. 20, no. 1, pp. 181–187, 2004.
- H.-W. Ha, I. Y. Kim, S.-J. Hwang, and R. S. Ruoff, “One-pot synthesis of platinum nanoparticles embedded on reduced graphene oxide for oxygen reduction in methanol fuel cells,” Electrochemical and Solid-State Letters, vol. 14, no. 7, pp. B70–B73, 2011.
- L. A. Zemnukhova and A. E. Panasenko, “A novel composite material based on antimony(III) oxide,” Journal of Solid State Chemistry, vol. 201, pp. 9–12, 2013.
- K. Oorts, E. Smolders, F. Degryse et al., “Solubility and toxicity of antimony trioxide (Sb2O3) in soil,” Environmental Science & Technology, vol. 42, no. 12, pp. 4378–4383, 2008.
- M. Filella, N. Belzile, and Y.-W. Chen, “Antimony in the environment: a review focused on natural waters II. Relevant solution chemistry,” Earth-Science Reviews, vol. 59, no. 1–4, pp. 265–285, 2002.
- S. Pei and H. M. Cheng, “The reduction of graphene oxide,” Carbon, vol. 50, no. 9, pp. 3210–3228, 2012.
- M. D. Stoller and R. S. Ruoff, “Best practice methods for determining an electrode material's performance for ultracapacitors,” Energy & Environmental Science, vol. 3, no. 9, pp. 1294–1301, 2010.
- B. Xu, S. Yue, Z. Sui et al., “What is the choice for supercapacitors: graphene or graphene oxide?” Energy & Environmental Science, vol. 4, no. 8, pp. 2826–2830, 2011.
- Y. Chen, X. Zhang, D. Zhang, P. Yu, and Y. Ma, “High performance supercapacitors based on reduced graphene oxide in aqueous and ionic liquid electrolytes,” Carbon, vol. 49, no. 2, pp. 573–580, 2011.