ACES  Vol.6 No.4 , October 2016
Morphological and Electrochemical Characterization of Ti/MxTiySnzO2 (M = Ir or Ru) Electrodes Prepared by the Polymeric Precursor Method
This paper describes the effect of the composition of the oxide films on the properties of electrodes Ti/MxTiySnzO2 (M = Ir or Ru) prepared by the polymeric precursor method. XRD studies showed that the anodes are formed by solid solutions. The electrodes containing IrO2 exhibit lower activity for the oxygen evolution reaction. The doping of the electrode surface with SnO2 improves the catalytic properties of the anodes. However, it should be held in appropriate compositions, because the change in the atomic ratio of this element shows a marked effect on the stability of the oxides. Electrode Ti/Ir0.2Ti0.3Sn0.5O2 has lower lifetime, i.e. 6 hours. The 20% decrease in the stoichiometric amount of SnO2 increases the time to a value above 70 hours, as observed for Ti/Ir0.3Ti0.4Sn0.3O2. Electrode Ti/Ru0.3Ti0.4Sn0.3O2 shows lifetime of 11 hours; therefore IrO2 is more stable than RuO2 under the conditions investigated. These results suggest that electrode Ti/Ir0.3Ti0.4Sn0.3O2 is promising for different applications, such as water electrolysis, capacitors and organic electrosynthesis.

1. Introduction

Oxide electrodes have been technologically important since the discovery of dimensionally stable anodes (DSA®) by Beer [1] and their applications in chlor-alkali industries. These electrodes constitute a mixture of oxides frequently prepared by standard thermal decomposition (SD) of metallic precursor salts in aqueous or alcohol solution, supported by metallic titanium [2] .

The electro-catalytic properties of metal oxides are associated with electronic and geometric factors [3] . The electronic factor is related to the chemical composition of the film, hence the physico-chemical properties of the constituent oxides, affecting the adhesion strength surface/intermediate. The geometric factor is directly related to the morphology of the film.

Research has been conducted to find new materials and procedures to improve the performance of DSA, for example, thermal decompositon of iridium and/or ruthenium precursor salts [4] [5] , thermal decomposition of hydroxo-aceto-chloro-based precursors [6] , Ti/TiO2 nanotubes prepared by anodization method [7] spin coating deposition technique [8] . The total or partial deactivation of thin films prepared by SD can be observed when they operate under drastic conditions and in a short period of time [4] [9] [10] . Electrodes as Ti/RuO2 and Ti/IrO2, prepared by the decomposition of polymeric precursors (Pechini method) [11] , have shown better electrochemical activity, i.e. longer life and higher active area than those prepared by the method of chlorides [12] - [14] . Moreover, the chemical or mechanical stability of oxide electrodes can be enhanced by incorporating/doping other metal ions into the films [3] .

The polymeric precursor method consists in the formation of chelates between metal cations and carboxylic acid and subsequent polymerization by a polyesterification reaction with polyalcohol [15] . The central idea is to distribute the cations throughout the polymeric structure. Heat treatment causes the release of organic matter and the formation of crystallites duly ordained [16] . This result is particularly interesting when the aims are to obtain materials with high crystallinity and controlled distribution of the constituents in the crystalline lattice.

This study investigates the morphological and electrochemical properties of oxide electrodes Ti/Ir0.3Ti0.4Sn0.3O2; Ti/Ir0.2Ti0.3Sn0.5O2 and Ti/Ru0.3Ti0.4Sn0.3O2 prepared by the thermal decomposition of polymeric precursors.

2. Experimental

2.1. Preparation of Electrodes

Thin film electrodes of nominal compositions Ir0.3Ti0.4Sn0.3O2, Ir0.2Ti0.3Sn0.5O2 and Ru0.3Ti0.4Sn0.3O2 were prepared by the thermal decomposition of a polymeric precursor solution (DPP) [11] . This method consists in synthesizing resins of metallic precursors by mixing citric acid (CA) in ethylene glycol (EG). The Ru, Ir, Sn, and Ti resins were prepared separately. First, 8 g of citric acid (Merk) were dissolved in 9 mL ethylene glycol (Merk) at 60˚C - 65˚C. After the dissolution of the acid, a solution of the precursor metal in isopropanol with 0.1 mol∙L−1 concentration (RuCl3∙xH2O, IrCl3∙xH2O, TiCl2∙6H2O all purchased from Aldrich and C6H5O7Sn2 synthesized from SnCl2 (Aldrich), as described in [17] ), was added to the CA/EG solution. The temperature was then raised up to 85˚C - 90˚C and the solution under was kept under rigorous stirring (300 rpm) for 1 - 2 hours for esterification and total isopropanol evaporation.

The precursor solutions were deposited on both sides of the pretreated metallic titanium (2.5 × 2.5 cm) by brushing, as described in the literature [12] . After the application of the coating, the electrodes were dried at 130˚C for 5 minutes and then calcined at 450˚C for 5 minutes. This procedure was repeated until the desired mass (125 mg∙cm−2) had been achieved. The layers were finally annealed at 450˚C for 1 hour under air flow.

2.2. Morphological and Electrochemical Characterizations

This measurement and others are deliberate, using specifications that anticipate your paper as one part of the entire journals, and not as an independent document. Please do not revise any of the current designations. The crystalline structures were physically characterized by X-ray diffraction (XRD) using an XRD-6000 diffractometer (Shimadzu) with a CuKα radiation source (λ = 1.5406 Å) operating in the continuous scan mode (4˚ min−1) from 10˚ to 90˚.

The surface morphology and microstructure of the deposited oxide films were analyzed through optical microscopy and scanning electron microscopy (SEM). Photomicrographs were obtained by a Zeiss LEO model 440 SEM coupled to an OXFORD operating with electron beam of 15 kV. The average composition was analyzed by PGT PRISM energy dispersive X-ray spectrometer (EDX) coupled to the SEM instrument.

2.3. Electrochemical Measurements

Electrochemical experiments were conducted with AUTOLAB model PGSTAT30 instrumentation. Voltammetric curves were recorded at scan rate of 50 mV∙s−1 using 0.5 mol∙dm−3 of H2SO4 as the supporting electrolyte. A platinum foil served as the auxiliary electrode and the KCl saturated calomel electrode (SCE) was used as the reference. The cell was thermostated at 25˚C.

Impedance spectra were recorded at constant potential between 0.3 and 1.4 V vs Ag/ AgCl. Electrochemical impedance spectroscopy (EIS) measurements were obtained in the 5 mHz - 10 kHz frequency interval using the “single sine” method and a sine wave amplitude of 5 mV (p/p). An AUTOLAB software program (FRA analyzer) was used for the analysis of the impedance data.

The stability of the electrodes was assessed based on their lifetime (LT) under galvanostatic conditions at a high current density (400 mA∙cm−2) in 0.5 mol∙dm−3 of H2SO4. The electrode lifetime was considered the time necessary for the electrode potential to achieve a value of 8.0 V.

3. Results and Discussion

3.1. Morphological and Chemical Characterizations

Figure 1 shows the XRD patterns for different compositions of electrodes prepared at 450˚C. In the electrodes containing iridium, characteristic diffraction peaks were

Figure 1. XRD patterns obtained for the oxide electrodes with different nominal compositions (a) Ti/Ir0.3Ti0.4Sn0.3O2; (b) Ti/Ir0.2Ti0.3Sn0.5O2; (c) Ti/Ru0.3Ti0.4Sn0.3O2.

observed and attributed to IrO2, according to JCPDS PDF #15-0870. Ti/Ru0.3Ti0.4Sn0.3O2 showed two peaks, one at 2θ = 43.7˚ and another at 2θ = 53.6˚, which correspond to RuO2 JCPDS PDF #40-1290. However, by comparing the positions of the peaks in the XRD obtained with the respective pure oxide, it is possible to observe that Sn-rich electrode composition displays peaks shifted toward the pure SnO2 pattern JCPDS PDF #46-1088, indicating that Ir and/or Ti atoms may be incorporated into the SnO2 crystalline reticule. The opposite trend is observed for Ru-electrode composition, which have their peaks shifted toward the pure RuO2 pattern due to the incorporation of Sn and/or Ti atoms into the RuO2 crystalline reticule. All samples displayed typical crystalline characteristics of tetragonal, with space group P42/nm. All those evidences suggesting the formation of a saturated solid solution for all the compositions investigated, one for Ir/Ti/Sn and other for Ru/Ti/Sn compositions. The XRD patterns show that all materials synthesized contained the Ti phase attributed to the Ti metallic subtract.

The average crystallite sizes of the oxide particles were estimated by the Debye- Scherrer equation [18] at crystalline planes ((210): 2θ = 43.7˚) for Ti/Ru0.3Ti0.4Sn0.3O2, and ((101): 2θ = 34.5˚) for Ti/Ir0.2Ti0.3Sn0.5O2 and Ti/Ir0.3Ti0.4Sn0.3O2. The values obtained were approximately 4 and 5 nm, respectively.

The roughness of the oxides Table 1 was estimated from the optical microscopy analyses Figure 2 performed in random areas of the film (average of five analyses). The electrode with nominal composition of Ti/Ru0.3Ti0.4Sn0.3O2 showed the lowest roughness, which suggests that the morphology of the oxide layers is highly dependent on the physicochemical properties of the oxides and the nature of the precursors.

Figure 3 shows some representative SEM images of the oxide films. Films containing

Table 1. Roughness estimated for the oxide films prepared by the polymeric precursor method.

Figure 2. Optical microscopy of the oxide electrodes, original magnification 350× (a) Ti/Ir0.3Ti0.4Sn0.3O2; (b) Ti/Ir0.2Ti0.3Sn0.5O2; (c) Ti/Ru0.3Ti0.4Sn0.3O2. Beside each picture is displayed the scale in μm.

Figure 3. SEM surface image of the oxide electrodes, original magnification 4000× (a) Ti/Ir0.3Ti0.4Sn0.3O2; (b) Ti/Ir0.2Ti0.3Sn0.5O2; (c) Ti/Ru0.3Ti0.4Sn0.3O2.

IrO2 (a, b) show uniform and continuous structures with cracks, i.e., mud-cracked-type morphology which are typical of thermally prepared oxide layers [10] [12] . Moreover, one observe that due to the increase in the amount of SnO2 in the electrode composition, cracks become larger (b), however the surface becomes less rough (see Table 1). However, the SEM image of the films containing RuO2 (c) indicate a distinct morphology, and in this case, the morphology change severally where the amount of fissures and cracks increase. The oxide surface morphology shows a clear relationship with the coating compositions investigated.

Table 2 shows the EDX analyses of the micrographs Figure 3. The EDX analysis of the electrodes indicated a good correlation between experimental and nominal compositions. The control of the composition of the films can be explained by the method used, since this polymer is formed before the calcination and the metal atoms are trapped in the matrix, which hinders its evaporation and consequent loss. All electrodes exhibited a homogenous distribution of particles on the electrode surface.

3.2. Electrochemical Characterizations

Figure 4 shows the j/E curve obtained in the cyclic voltammetric experiments. This profile is typical of thermally prepared oxide layer electrodes [19] [20] and characteristic of DSA® electrodes [21] . The figure also shows a blurred peak at around 0.5 V associated with the Ru (III)/Ru(IV) redox transition [22] for the Ti/Ru0.3Ti0.4Sn0.3O2 electrode. The voltammograms of the electrodes containing IrO2 showed a peak typical of the Ir(III)/Ir (IV) transition in the region between 0.4 and 0.8 V [6] .

The oxygen evolution reaction occurs at a more positive potential for the electrode containing the largest amount of SnO2. According to Fukunaga et al. [23] , the doping of the electrode surface with SnO2 is an effective strategy to improve performance even in

Table 2. Atomic ratios (%) of the oxide films with different nominal compositions.

Figure 4. Cyclic voltammograms at 50 mV・s−1 in 0.5 mol・dm−3 of H2SO4 of the oxide electrodes vs. SCE (a) Ti/Ir0.3Ti0.4Sn0.3O2; (b) Ti/Ir0.2Ti0.3Sn0.5O2; (c) Ti/Ru0.3Ti0.4Sn0.3O2.

the treatment of degradation of organic compounds thus our results are in agreement with previous report.

The comparison between the electrode containing IrO2 and those containing RuO2 shows the IrO2 exhibits lower activity for the oxygen evolution reaction.

The impedance behavior of the electrodes was investigated to further characterize the different Ti/Ir0.3Ti0.4Sn0.3O2; Ti/Ir0.2Ti0.3Sn0.5O2 and Ti/Ru0.3Ti0.4Sn0.3O2 systems. The Nyquist diagram (Z' vs Z") of the electrodes obtained between 0.3 and 1.4 V vs Ag/AgCl is shown in Figure 5. In the low frequency domain, electrodes Ti/Ir0.3Ti0.4Sn0.3O2 and Ti/Ir0.2Ti0.3Sn0.5O2 formed a straight line parallel to Z", characteristic of an ideally polarizable electrode, and a slight deviation from the straight line along Z", suggesting a non-ideally polarizable electrode [24] [25] . The shift from the ideal capacitor behavior is a consequence of the material’s porosity [24] [26] . In the low-frequency domain region a decrease in impedance was found when the applied potentials were positively shifted. This result suggests that the EIS responses in this domain region indicate a faradaic process of the bulk redox transitions of the oxide material. The difference observed between the Ir-based electrodes and Ru-based electrodes maybe could be explained due to the higher electronic conductivity in the Ru-Ti-Sn/solution than in the Ir-Ti-Sn/solution interfaces.

The Bode plot (θ vs. log f) obtained at 0.3 V vs Ag/AgCl for electrodes is shown in Figure 6. An analysis of this figure indicates that the main feature of these electrodes is the appearance of a well-defined time constant (τ) for the Ti/Ru0.3Ti0.4Sn0.3O2 electrode, which is characterized by a maximum phase angle ranging from 1 to 100 Hz. This behavior can be ascribed to the large number of RuO2 transition states contributing to the charging system [27] . This results corroborated with the Nyquist plot interpretation above because the Ru-based electrode shows more pseudo capacitive behavior than the Ir-based electrode [10] [24] .

The stability of the electrodes was assessed based on their lifetime, considering the time necessary for the electrode potential to reach 8.0 V. The electrode containing larger amounts of SnO2 (Ti/Ir0.2Ti0.3Sn0.5O2) has a shorter lifetime. The 20% decrease in the stoichiometric amount of this oxide as well as the high amount (10%) of IrO2 (Ti/ Ir0.3Ti0.4Sn0.3O2) increase the time to a value above 70 hours. Comparing the electrode Ti/Ir0.3Ti0.4Sn0.3O2 with Ti/Ru0.3Ti0.4Sn0.3O2, IrO2 has higher stability under drastic conditions of electrolysis than RuO2 (Table 3).

The lifetime of oxide electrodes is directly correlated with two factors: passivation and dissolution of the coating [21] . The first factor is due to the penetration of the electrolyte through the pores or cracks towards the substrate, resulting in the oxidation of the metallic support and forming a non-conductive layer between the substrate and the oxide coating [28] - [30] . The second factor involves the loss of electroactive material (erosion or dissolution), resulting in a gradual reduction of the voltammetric charge. This may occur due to the pores in the layer and the rapid evolution of gas on the surface, inducing the separation of weakly bound parts of the active layer [28] [31] [32] .

Morphological changes of the electrode surface after the lifetime test can be observed

Figure 5. Nyquist diagrams of the oxide electrodes as a function of the applied potential (0.3, 0.7, 1.0 and 1.4 V) vs. Ag/AgCl (a) Ti/Ir0.3Ti0.4Sn0.3O2; (b) Ti/Ir0.2Ti0.3Sn0.5O2; (c) Ti/Ru0.3Ti0.4Sn0.3O2.

Figure 6. Bode plot at 0.3 V vs. Ag/AgCl as a function of the oxide electrodes. (-○-) Ti/Ir0.2Ti0.3Sn0.5O2; (-■-) Ti/Ir0.3Ti0.4Sn0.3O2 (-Ø-) Ti/Ru0.3Ti0.4Sn0.3O2.

Table 3. Lifetime values obtained for the oxide electrodes under galvanostatic conditions at a high current density (400 mA・cm−2) in 0.5 mol・dm−3 of H2SO4.

through microstructural analysis (Figure 7), which shows worn structures with erosion of the active layer. The EDX analysis revealed a decrease in the quantity of Ir and Ru, confirming the loss of the electroactive material, well as a decrease of Sn (Table 4).

The curves obtained for the lifetime showed a slow increase in the potential followed by an abrupt increase at the end of the experiment for all compositions investigated. This behavior indicates a rise in the electrode structure resistance. Such an increase may have resulted from the loss of Ir or Ru in the top layers of the electrode and/or the formation and growth of a non-conductive oxide film between the metallic substrate and the conductive oxide [9] [31] .

EDX analysis after lifetime revealed a considerable increase in the titanium signal. These results suggest that besides the process of erosion, there is also a process of anodic passivation of the metallic base due to the formation of an insulating film composed primarily of TiOx.

Figure 7. SEM surface image of the oxide electrodes after the lifetime test, original magnification 4000×. (a) Ti/Ir0.3Ti0.4Sn0.3O2; (b) Ti/Ir0.2Ti0.3Sn0.5O2; (c) Ti/Ru0.3Ti0.4Sn0.3O2.

Table 4. Variation in the atomic ratios (%) of the oxide films after the lifetime test.

4. Conclusion

This study has demonstrated the effect of the composition of oxide films on the properties of DSA prepared by the thermal decomposition of polymeric precursors. IrO2- based electrodes are more stable than RuO2-based electrode under the conditions investigated and show lower activity for the oxygen evolution reaction, which makes it attractive in the oxidation of organic substances. The introduction of tin oxide in the composition film enhances the catalytic properties of the anodes. However, it should be held in appropriate compositions, because the change in the atomic ratio of this element produces marked effects on the stability of the oxides. The thin films formed are composed of a solid solution among the various oxides constituents of the film. The procedure employed for the preparation of the anodes is a good alternative to SD, minimizing the volatilization of the metal.


The authors would like to acknowledge the Conselho Nacional de Desenvolvimento Científico e Tecnológico-CNPq, the Fundação de Amparo à Pesquisa do Estado de São Paulo-Fapesp (2013/02762-5) and Fundação de Amparo à Pesquisa do Estado do Espírito Santo-FAPES for the financial support provided to this research.

Cite this paper
Carneiro, J. , Silva, J. , Rocha, R. , Ribeiro, J. and Lanza, M. (2016) Morphological and Electrochemical Characterization of Ti/MxTiySnzO2 (M = Ir or Ru) Electrodes Prepared by the Polymeric Precursor Method. Advances in Chemical Engineering and Science, 6, 364-378. doi: 10.4236/aces.2016.64037.
[1]   Beer, H.B. (1980) The Invention and Industrial Development of Metal Anodes. Journal of the Electrochemical Society, 127, 303-307.

[2]   Varela, H., Camara Júnior, G.A.H.S. and Gonzalez, E.R. (2000) Oxygen Evolution Reaction on Mn2O3 Electrodes Supported on Stainless Steel. Quimica Nova, 23, 721-726.

[3]   Klink, M.J., Makgae, M.E. and Crouch, A.M. (2010) Physico-Chemical and Electrochemical Characterization of Ti/RhOx-IrO2 Electrodes Using Sol-Gel Technology. Materials Chemistry and Physics, 124, 73-77.

[4]   Trasatti, S. (1991) Physical Electrochemistry of Ceramic Oxides. Electrochimicam Acta, 36, 225-228.

[5]   Lipkowski, J. and Ross, P.N. (1994) The Electrochemistry of Novel Materials. VCH, University of Michigan.

[6]   Ferro, S., Rosestolato, D., Martínez-Huitle, C.A. and DeBattisti, A. (2014) Charge-Storage Process in IrO2-SnO2 Mixed-Oxide Electrodes. Role of Coating Composition, Solution pH and Temperature. Electrochimican Acta, 148, 85-90.

[7]   Kruthika, N.L., Karthika, S., Raju, G.B. and Prabhakar, S. (2013) Efficacy of Electrocoagulation and Electrooxidation for the Purification of Wastewater Generated from Gelatin Production Plant. Journal of Environmental Chemical Engineering, 1, 183-188.

[8]   Fierro, C. and Comninellis, C. (2010) Kinetic Study of Formic Acid Oxidation on Ti/IrO2 Electrodes Prepared Using the Spin Coating Deposition Technique. Electrochimica Acta, 55, 7067-7071.

[9]   Ribeiro, J. and de Andrade, A.R. (2004) Characterization of RuO2-Ta2O5 Coated Titanium Electrode Microstructure, Morphology, and Electrochemical Investigation. Journal of the Electrochemical Society, 151, D106-D111.

[10]   Tilak, B.V., Birss, V.I., Wang, J., Chen, C.P. and Rangarajan, S.K. (2001) Deactivation of Thermally Formed Ru/Ti Oxide Electrodes: An AC Impedance Characterization Study. Journal of the Electrochemical Society, 148, 112-116.

[11]   Pechini, M.P. (1967) Method of Preparing Lead and Alkaline Earth Titanates and Niobates and Coating Method Using the Same to Form a Capacitor. US Patent No. 3330697.

[12]   Forti, J.C., Olivi, P. and de Andrade, A.R. (2001) Characterisation of DSA-Type Coatings with Nominal Composition Ti/Ru0.3Ti(0.7﹣x)SnxO2 Prepared via a Polymeric Precursor. Electrochimica Acta, 47, 913-917.

[13]   Terezo, A.J. and Pereira, E.C. (1999) Preparation and Characterization of Ti/RuO2-Nb2O5 Electrodes Obtained by Polymeric Precursor Method. Electrochimica Acta, 44, 4507-4511.

[14]   Lassali, T.A.F., Boodts, J.F.C. and Bulhoes, L.O.S. (2000) Effect of Sn-Precursor on the Morphology and Composition of Ir0.3Sn0.7O2 Oxide Films Prepared by Sol-Gel Process. Journal of Non-Crystalline Solids, 273, 129-133.

[15]   Marciel, A.P., Longo, E. and Leite, E.R. (2003) Nanostructured Tin Dioxide: Synthesis and Growth of Nanocrystals and Nanoribbons. Quimica Nova, 26, 855-861.

[16]   Mourao, H.A.J.L., de Mendonca, V.R., Malagutti, A.R. and Ribeiro, C. (2009) Nanostructures in Photocatalysis: A Review about Synthesis Strategies of Photocatalysts in Nanometric Size. Química Nova, 32, 2181-2186.

[17]   Besso, M.M. (1965) Tin Salts of Citric Acid and Method of Preparation. US Patent No. 3213120.

[18]   Klung, H.P. and Alexander, L.E. (1975) X-Ray Diffraction Procedures for Polycrystalline and Amorphous Materials. Journal of Applied Crystallography, 8, 573-580.

[19]   Malpass, G.R.P., Miwa, D.W., Machado, S.A.S., Olivi, P. and Motheo, A.J. (2006) Oxidation of the Pesticide Atrazine at DSA Electrodes. Journal of Hazardous Materials, 137, 565-572.

[20]   Motheo, A.J., Gonzalez, E.R., Tremiliosi, G., Olivi, P., de Andrade, A.R., Kokoh, B., Leger, J.M., Belgsir, E.M. and Lamy, C. (2000) The Oxidation of Formaldehyde on High Overvoltage DSA Type Electrodes. Journal of the Brazilian Chemical Society, 11, 16-21.

[21]   Forti, J. F., Ribeiro, J., Lanza M.R.V., de Andrade, A.R. and Bertazzoli, R. (2010) Electrochemical Characterization of DSA-Type Electrodes Using Niobium Substrate. Electro-catalysis, 1, 129-138.

[22]   Ardizzone, S., Fregonara, G. and Trasatti, S. (1990) “Inner” and “Outer” Active Surface of RuO2 Electrodes. Electrochimica Acta, 35, 263-267.

[23]   Fukunaga, M.T., Guimaraes, J.R. and Bertazzoli, R. (2008) Kinetics of the Oxidation of Formaldehyde in a Flow Electrochemical Reactor with TiO2/RuO2 Anode. Chemical Engineering Journal, 136, 236-241.

[24]   Sugimoto, W., Iwata, H., Yokoshima, K., Murakami, Y. and Takasu, Y. (2005) Proton and Electron Conductivity in Hydrous Ruthenium Oxides Evaluated by Electrochemical Impedance Spectroscopy: the Origin of Large Capacitance. The Journal of Physical Chemistry B, 109, 7330-7338.

[25]   De Carvalho, L.A., de Andrade A.R. and Bueno, P.R. (2006) Electrochemical Impedance Spectroscopy Applied in the Study of Heterogeneous Reactions at Dimensionally Stable Anodes. Química Nova, 29, 796-804.

[26]   Terezo, A.J., Bisquert, J., Pereira, E.C. and Garcia-Belmonte, G. (2001) Separation of Transport, Charge Storage and Reaction Processes of Porous Electrocatalytic IrO2 and IrO2/Nb2O5 Electrodes. Journal of Electroanalytical Chemistry, 508, 59-69.

[27]   Horvat-Radosevic, V., Kvastek, K., Vukovic, M. and Marijan, D. (1999) Impedance of Ruthenium Electrodes in Sulphuric Acid Solution. Journal of Electroanalytical Chemistry, 463, 29-44.

[28]   Martelli, G.N., Ornelas, R. and Faita, G. (1994) Deactivation Mechanisms of Oxygen Evolving Anodes at High Current Densities. Electrochimica Acta, 39, 1551-1558.

[29]   Jovanovic, V.M., Dekanski, A., Despotov, P., Nikolic, B. and Atanasoski, R.T. (1992) The Roles of the Ruthenium Concentration Profile, the Stabilizing Component and the Substrate on the Stability of Oxide Coatings. Journal of Electroanalytical Chemistry, 339, 147-165.

[30]   Panic, V.V., Dekanski, A., Milonjic, S.K., Atanasoski, R.T. and Nilolic, B.Z. (1999) RuO2-TiO2 Coated Titanium Anodes Obtained by the Sol-Gel Procedure and Their Electrochemical Behaviour in the Chlorine Evolution Reaction. Colloids and Surfaces A: Physicochemical and Engineering Aspects, 157, 269-274.

[31]   Loucka, T. (1977) The Reason for the Loss of Activity of Titanium Anodes Coated with a Layer of RuO2 and TiO2. Journal of Applied Electrochemistry, 7, 211-214.

[32]   Iwakura, C. and Sakamoto, K. (1985) Effect of Active Layer Composition on the Service Life of (SnO2and RuO2)-Coated Ti Electrodes in Sulfuric Acid Solution. Journal of the Electrochemical Society, 132, 2420-2423.