Application of silver in microtubular solid oxide fuel cells
In this paper, the behaviour of silver as cathode conductive material, interconnect wire, and sealing for anode lead connection for microtubular solid oxide fuel cells (µSOFC) is reported. The changes in silver morphology are examined by scanning electron microscopy on cells that had been operated under reformed methane. It is found that using silver in an solid oxide fuel cell (SOFC) stack can improve the cell performance. However, it is also concluded that silver may be responsible for cell degradation. This report brings together and explains all the known problems with application of silver for SOFCs. The results show that silver is unstable in interconnect and in cathode environments. It is found that the process of cell passivation/activation promotes silver migration. The difference in thermal expansion of silver and sealant results in damage to the glass. It is concluded that when silver is exposed to a dual atmosphere condition, high levels of porosity formation is seen in the dense silver interconnect. The relevance of application of silver in SOFC stacks is discussed.
KeywordsSilver SOFC Microtubular SOFC SOFC stacks
Several configurations of solid oxide fuel cells (SOFC) are commercially available; however, the selection of suitable materials and development techniques is still the subject of current research. Within an SOFC cell, the cathode is a significant contributor to the cell overpotential caused by the slow oxygen reduction reaction , which occurs at the electrolyte–cathode–air boundary phase (triple-phase boundary). When the temperature of SOFC is low, the oxygen dissociative adsorption slows further because of the decrease in catalytic activity of the cathode oxygen reduction. Key requirements for cathode materials are that they have to be highly conductive for electrons and oxygen ions, and they should maintain thermal stability in SOFC operating temperature. The conductivity of modern cathode materials such as lanthanum strontium manganite (LSM) or lanthanum strontium cobalt ferrite (LSCF) decreases at lower operating temperature. High ohmic losses in the cathode result in reduced cell performance. This can be overcome by the addition of a metal-based current collection layer that enhances the electronic conductivity. The high-conductive layer ensures adhesion and connectivity between the cathode and the interconnect. This consequently reduces the contact resistance of the cathode/interconnect interface.
In planar cells, a silver mesh can be applied to reduce the contact resistance between the interconnect and the cathode . The presence of silver will also act as a catalyst for oxygen reduction . Silver has been proven as a cathode material showing good results at intermediate temperatures in SOFC [1, 4, 5, 6]. In these tests, the limiting feature was the length of the oxygen diffusion paths. Moreover, silver does not form a nonconductive oxide layer when exposed to air at elevated temperatures. The high resistance to oxidation at elevated temperatures is thus beneficial for SOFC application. Silver also has one of the highest electrical conductivities of metals (6.30 × 107 S m−1 at 20 °C), thus the addition of silver improves electron percolation. Silver is often used as a conductive material for the cathode in microtubular solid oxide fuel cells (µSOFC) [7, 8, 9, 10]. This has been implemented for planar  or honeycomb  cell designs, too. Silver in a µSOFC can also function as a sealant [13, 14]. Infiltration of silver into the porous cathode is an alternative method to improve current collection [1, 9]. Infiltration of silver or an alternative highly conductive material such as lanthanum strontium cobalt (LSC) can significantly improve current density of the standard LSM cathode [6, 10, 15]. Adding silver into the cathode system has shown to reduce the overpotential related to oxygen reduction . Porous silver can also function as a cathode for low-temperature SOFC  Inert properties and stability in the oxidising atmosphere can make silver a good candidate as a cathode interconnect material for intermediate-temperature SOFC.
However, silver tends to agglomerate during annealing in air or in ambient oxygen . Porous silver tends to become dense at elevated temperatures. For the mixed Ag/cathode systems of yttrium or erbium stabilized bismuth oxide, 1 h of sintering was shown to be enough to result in porosity reduction, separation of compounds, and increase in Ag phase . Silver is also known to be prone to migration at elevated temperature. Compson et al.  suggested to use silver as an interconnect for SOFC only at temperatures below 650 °C. Above this temperature, loss of silver caused by sublimation, evaporation, and diffusion transport may affect cell performance.
Using silver as a current collector can reduce cell performance since the low-temperature melting point of silver requires changes in cell preparation technique . Moreover, silver can evaporate even at low (300–350 °C) temperatures . Evaporation of silver increases with temperature and is similar in the air and in the reducing environment . Silver does not have high gas penetrability. However, silver has high oxygen solubility. The solubility allows application of silver as an anode for direct carbon SOFC . Silver tends to migrate when submitted to an electric field at high temperature with of oxygen [23, 24, 25]. Silver ions Ag+ can move under the influence of the electrical field . The presence of Cr can increase the Ag migration into the cathode. Formation of compounds such as AgCrO2 with higher evaporation rate than pure Ag increases Ag migration . Migration of silver and formation of conductive filaments can cause short-circuit failures . Singh et al.  observed that exposure to the dual oxidation–reduction environment can damage the silver microstructure. They observed the formation of pores and cracks on the fuel side of the solid silver barrier. They suggested that dissociation and dissolution of H and O into silver and formation of steam cause development of pores in solid silver barriers. Using silver in SOFC cells and stacks has many benefits and for that reason many researchers are trying to improve SOFC performance using silver compounds. However, the incorporation of silver will affect the cell durability. The aim of this work is to discuss the plausibility of Ag as an SOFC material and to highlight the problems that may occur for application of silver in SOFC. In this work, silver is utilised in the µSOFC systems, as an interconnect, as a cathode or as an additional cathode conductive layer and for the sealing of an anode/lead connection. The aim of this work is to examine the degradation mechanisms of a µSOFC cell.
The current interruption method was applied for internal resistance measurements. Electrochemical impedance spectra were performed using Solartron cell test system 1400A/1470E (Potentiostat/Galvanostat). The cell response was measured over a frequency range of 1 MHz to 0.1 Hz with AC voltage amplitude 10 mV at the open circuit voltage (OCV) condition. Electrochemical performance measurements were made using the Solartron in galvanostatic mode.
Long-term cell tests were conducted under potentiostatic mode at a set voltage of 0.7 V. Every 24 h the test was interrupted by I–V test and impedance scan.
Analysis of cell morphology: post-cell test the cells were fractured, cell surface and cell cross-section were characterised using a Hitachi TM3030Plus scanning electron microscope (SEM).
The cell temperature was maintained at the temperature of 650 or 700 °C in a tubular furnace (Vecstar HZ/split-tube) and monitored by thermocouples flanking the test chamber.
The cell exhaust was cemented (using high-temperature cement) to a manifold, and the gas feed was connected using a silicone tube so the cell was free to move in the axial direction. Cells were operated at 650 and 700 °C using either hydrogen or methane/air mixture. Inside the cell/tube, at the inlet, a partial oxidation catalyst (CPOX) (0.1 g) was inserted in the shape of a honeycomb structure. Hydrogen was introduced into the cell at 145 ml min−1, and after 1 h of OCV, a polarisation curve was recorded (galvanostatic mode) with 0.5 V as a lower safe limit. Then the voltage was set to 0.7 V (potentiostatic mode) and a short 1 h constant voltage test was performed. Afterwards, the fuel was changed to a mixture of CH4:air (dry air) with molar ratio CH4:air of 1:2.4 and a long-term durability test was conducted at 0.7 V (CH4 48 ml min−1). These conditions were chosen to simulate the realistic conditions of a µSOFC auxiliary power unit (APU) . The fuel gas connection was outside the hot zone, which eliminated problems with sealing. All tests were conducted under ambient air-condition on the cathode side. Details about the cell test system were described in previous papers [28, 29].
Results and discussion
Benefits from using silver
Usually, tubular cells have large cell voltage and ohmic losses since electrons have to be transported through the cathode along the cell. The addition of silver can reduce this problem. Thus, the surface of the cathode was covered with silver ink (SPI 5001) for these test cells. The primary role of the silver layer was to deliver and distribute the flux of electrons over the whole cathode area. This also helped to reduce the area-specific resistance (ASR) of the connection between the cathode and the interconnect (LSCF-Ag wire). An additional benefit of adding silver was to support oxygen reduction reaction. The silver ink formed a porous layer of 10–30 μm. The high porosity of the silver layer allowed free gas diffusion.
For cells tested without Ag coating on the cathode surface, cathode lead wires (0.71 mmAg) were coated with LSCF to improve contact interconnect/cathode. For cells with the Ag cathode coating layer, the wires were coated with Ag ink.
To confirm and compare how the various cathode coatings affect the cell performance, a selection of cells was coated with Pt ink, Ag ink and LSCF ink (to improve connection between already sintered LSCF cathode and Ag wires). These cells were tested at 700 °C. Increasing the cell-operating temperature from 650 to 700 °C reduced the cell overpotential, for the cell covered with Ag (Fig. 2a–b). The possible reason for this was the increased conductivity of the cathode and the electrolyte and higher catalytical activity of the cathode. Slightly larger impedance for Ag was obtained for the cell covered by Pt ink (Fig. 2b). In contrast, for the LSCF coating, the resistance of the cell increased at all frequencies. The cell ohmic resistance for Ag (0.03 Ω) was slightly lower than for Pt (0.04 Ω) and much lower than for LSCF (0.28 Ω). In addition, the size of both impedance arcs was slightly smaller for Ag than for Pt and much smaller than for LSCF. The cell performance depends on the used current collector. The low-frequency semicircle for Pt and Ag was slightly larger than the high-frequency. The characteristic frequency for high and low-frequency arcs was independent of the type of cathode coating.
The EIS spectra confirmed the positive aspect of introduction silver to the cathode structure. The data and results presented clearly show that SOFC with the Ag-coated cathode, operating in the temperature region of 650–700 °C, showed improved performance compared to similar cells without silver in the cathode system.
Anode Ag sealing interconnect
The whole area of the exposed anode was covered by silver paste to improve the electrical connection and to part-seal the anode. The silver was densified by sintering. However, as the thermal expansion coefficient of silver is higher than that of the ceramic cell, it is expected that the connection between the cell and the interconnect further improves through the silver expansion during heating. Silver is ductile and should easily deform under thermal stress avoiding delamination and keep the cell hermeticity. However, using only silver paste as a sealant resulted in poor sealing. Fuel leakage was seen, indicated by high temperatures detected by the thermocouples around the anode current connection. The cells with only silver as a sealant could operate for around 24–50 h. To investigate the reason for the weak sealing, the cell was tested at 700 °C with H2 (3% H2O) for 8 h under OCV. The H2 leak test conducted after silver sintering indicated gas tightness of the silver/anode joint at room temperature.
Singh et al.  suggested that pores and voids in silver are developed because of water vapour formation. Adsorption and dissolution of H and O gaseous molecules in silver interconnect is followed by diffusion and reaction of dissolved species and water vapour formation. The hydrogen and oxygen concentration in silver increases up to a critical pressure and bubbles are generated. The increase in the size of the pores in the silver layer can finally result in fuel leakage. According to Jackson et al. , 24 h of exposure to the dual atmosphere is enough to form pores across a 1-mm thick silver membrane. The high temperature of fuel combustion and possible anode oxidation at the middle of the anode can result in crack formation and damage to the cell.
The fact that porosity always began to form from the fuel side of the silver layer suggests faster solubility of oxygen than hydrogen. Also the ratio of O:H 1:2 in water promotes nucleation closer to the hydrogen source. The diffusivity and highest concentration in silver under dual atmosphere at 800 °C is, respectively : H2 2.9 × 10−4 cm2s−1; 6.1 × 10−7 mol cm−3, O2 1.1 × 10−5 cm2 s−1; 1.1 × 10−5 mol cm−3.
The rapid degradation of silver mechanical integrity and hermeticity after exposure to dual atmosphere affects the cell performance. Formation of pores in the silver also has an influence on the stability of the silver seal. Such degradation of the structure leads to fuel leakage. For this system of tubular cells with the anode connection at the middle of the cell, the silver seal would be exposed to the dual atmosphere. Therefore, if silver is applied as a sealant/current collector for a µSOFC, it has to be isolated to avoid exposure to the dual atmosphere. The additional sealing of the silver by glass was needed to extend the cell operation. This was achieved by coating the silver anode connection by a 10 µm layer of glass sealant. This extended the life of the µSOFC up to more than 800 h.
However, due to the difference in thermal expansion coefficient of silver and glass, there is a risk of damage to the glass coating. The components that have much lower thermal expansion coefficient than silver are YSZ 10.5, Ni/YSZ 12.5, SDC 12.8 and cathode 14.6, compared to silver 18.9 × 10−6 K−1. The glass sealant’s thermal expansion coefficient was selected to match the expansion of the cell components and was around 12 × 10−6 K−1. With this mismatch in thermal expansion, significant internal stress is created. After the glass sintering (at 850 °C for 8 h), there was no visible damage to the glass surface. However, the long-term cell operation at elevated temperature or thermo-cycling resulted in the crack formation in the glass structure (Fig. 1d). These studies suggest that the high silver coefficient of thermal expansion can create problems for application of silver as an anode interconnect (and sealant) for the µSOFCs even with a glass coating. For this specific application, the rapid start and cooling required by APU could favour crack formation within the glass sealant.
The glass surface showed visible pinhole formation, approximately 1 μm in diameter. Several effects, including the application/deposition technique, can cause this effect. In this case, it has been attributed to the irregular surface of silver to which it was applied. Due to the complex shape of wire/anode connection, it was difficult to obtain a smooth silver surface. Pinholes usually indicate localised microbubbles or dewetting that degassed during sintering. Contaminants like dust particles can cause a formation of localised microbubbles. This could come from insulation material. The glass coating thickness is in a micron range, and it is possible for the debris to be larger in diameter than the coating thickness. The electrostatic attraction is enough to hold small particulates on the surface. Some particulates could also have a high moisture level. In addition, if there are existing cracks on the glass surface, the heat generated by fuel combustion could be enough to melt the glass and produce pinholes. For future work, the glass coating technique has to be improved.
Pores formed across all surface areas of Ag wire. The silver wire at the anode connection became brittle. Surprisingly, the cell performance was stable for more than 850 h of operation under such gas leakage conditions. Formation of silver crystals damaged the glass sealing and increased the exposure of the wire to air. These results did not confirm Compson’s conclusion  that for silver interconnects 650 °C is a safe operating temperature. After 850 h of operation at 650 °C, all the interconnect wire and sealing paste was significantly deformed and damaged. It can be concluded that silver paste should not be used as a sealant for the anode connection for long-term cell operation.
At higher operating temperature (450 h at 700 °C) the structures formed were more intensive; all surfaces of the wire had changed; however, the structures were smaller (Fig. 5d). Wires at the anode side behaved differently. Some faceting was visible, but significant wire area became porous (Fig. 5c). This part of the wire was only 10 mm from the anode connection (presented in Fig. 4), and after damage to the glass the coating was exposed to the dual atmosphere. The damage to the silver wire microstructure was observed even 10 mm from the point of wire exposure to the dual air–fuel atmosphere after long operational time. After several hours of operation, silver wires became brittle. This affected the mechanical strength and integrity. Even low physical stress could break the wire. This is important if a stack with silver wires is considered for an APU unit in vehicles where the system must resist vibrational stresses and strains. A cell with such brittle wires would be prone to damage caused by vibration. The risk of breaking the wire connection is significant. All these problems with silver will lead to degradation of the cell structural stability and in long-term operation to the degradation of the cell/stack performance. Zhong et al.  using Ag mesh for cathode current collector did not observe this type of degradation. However, they used Pt paste to improve the strength of the connection, and the test time was short. Silver commercially available has the purity of 99.95%. Silver is rarely used by industry in pure form caused by its softness and susceptibility to damage. Also for SOFC application, silver alloys should be considered instead of pure silver. Where higher strength at elevated temperature is required, silver-palladium alloys are more suitable; however, that would increase the cost. Also the application of Ag(Al) alloys can enhance the thermal stability of silver . The addition of aluminium reduces silver agglomeration at elevated temperature and prevents diffusion of silver into the matrix of support material. Wires with high Ni, Fe or Cr content are less suitable because of formation of a nonconductive oxide layer and reduced conductivity between the cathode and the interconnect. The addition of other elements and alloy formation on the silver surface may be the solution for application of silver current collectors in SOFC. Silver wires coated with gold are slightly more expensive than pure silver.
Cathode conductive layer
The risk of vaporisation and sublimation of silver exposed to air increases at higher reaction and operating temperatures. The vaporisation rate depends on temperature and atmosphere, and is higher in air than in H2/H2O atmosphere. Meulenberg et al.  extrapolated that up to 2% of silver can evaporate after 40,000 h at 690 °C in air. The evaporation will increase with the increase in the silver surface area. The cathode silver layer used in presented experiments was porous. Considering high porosity of the silver layer and its thickness 10–30 μm, a significant part of the silver can evaporate after the cell’s lifetime. The glass sealant, which is applied to maintain gas tightness, also poses a problem as glass sealants usually require sintering at 850 °C for several hours—leading to evaporation of silver into and through the glass matrix. In our previous report , the cathode was coated with silver ink to receive good current collection before glass sintering. This exposed the porous silver to the high temperature of 850 °C for 8 h. The reverse fabrication, with sintering glass before coating the cathode with silver, reduced silver degradation. However, it increases the complexity of the cell mass production. The Ag current collection film can be applied after the glass sintering for a single cell, although this process is impractical for the stack manufacture.
It can be concluded that initial morphological structure of the porous silver current collector was destroyed as a reason of silver sintering and evaporation. The silver microstructure was unstable at intermediate cell operating temperature. Therefore, for a long-term application, silver is not suitable as a conductive material. Mixing silver with the ceramic phase or infiltration of silver with ceramic precursors could prevent silver densification. The ceramic shell can restrain densification of silver porous structure . Another method is to incorporate silver into a ceramic matrix of the cathode . The decrease in temperature operation of SOFC can increase the stability of silver. Zhu et al.  obtained high performance of the cathode with silver nanoparticles at 500 °C. The stability of Ag nanoparticles was increased by the strong metal-support (Ag–SNC) bonding interaction. Mixing silver with SSZ can reduce silver agglomeration on the cathode. Morphology of this cermet is stable at 500 °C . Application of silver ink with thinner can improve the wetting and impregnation of silver into the cathode matrix. However, from our experience, application of lower viscosity silver ink directly on the LSCF cathode can sometimes result in a cathode flaking.
Migration of silver and agglomeration at the electrolyte interface could also result in cathode peeling . Silver tends to agglomerate at elevated temperature, which can lead to cathode delamination. However, no silver was detected in the SDC layer for samples where cathode delamination or cracks in the SDC layer occurred. In addition, no silver was detected on the electrolyte for areas where the cathode exfoliation occurred. Therefore, silver penetration into SDC was not responsible for the cathode delamination.
The mechanism responsible for migration of silver and condensation across the SDC layer is unclear. It is unlikely that thermal effect alone is responsible for Ag migration to SDC. The temperature distribution along the cell was relatively uniform and silver deposited in the SDC layer was observed only at the cell inlet (the most active part of the cell). Silver migration could be a result of electromigration  or it can be associated with the formation of Ag (g) species and vapour transport to the cathode–electrolyte face followed by reduction to metal phase . Ag (g) has higher vapour pressure than Ag2O (g) at the SOFC operation temperature. Therefore, it is thought Ag (g) formation and penetration in SDC are possible for this mechanism. However, electromigration and evaporation/deposition of silver are too slow to be alone directly responsible for the observed rate of silver migration during the electrode polarisation . Mosialek et al.  observed silver migration on the YSZ electrolyte in the potential range − 0.2–0.5 V; no migration was observed without polarisation. In addition, no migration was observed without the electrolyte. They concluded that for the formation of silver dendrites, it is necessary to have a potential difference between the cathode (with Ag) and the oxygen ion conductor. Therefore, silver migration is not correlated directly with current density. Similar results were reported for the GDC electrolyte . The mechanism responsible for silver mass transport is difficult to distinguish. Silver migration is possibly related to electron transfer and oxygen flux. The flow of electrons can promote silver electromigration. This can explain the agglomeration of silver at the edge of electrolyte since electrolyte can conduct only ions. The short 1–2 h OCV break in the cell power generation affected the performance of tested cells. Rapid cell degradation was often seen directly after OCV. Since the OCV state is not conductive for thermal or electromigration of silver , the cathode polarisation must promote silver migration. Moving from one state (including OCV) of operation to another could affect cell performance. The process of cell passivation/activation resulted in the difference in temperature distribution along and across the cell and could result in some microcrack formation in the electrolyte. Also, the risk of coke deposition on the anode during OCV was significant because no steam was formed from fuel electrooxidation and only 60–70% of fuel was converted on the CPOX catalyst . Formed coke and temperature gradient may also result in microcracks formation in the electrolyte structure. However, SEM scans did not confirm electrolyte cracks. Simner et al.  observed that fresh cell was not affected by holding it under OCV. This confirms our result that short-circuit occurs directly after a short OCV break in the cell operation if the cell was in operation for several hours. Another possible explanation is that during OCV period (no current flow through electrodes), silver deposited in the SDC layer was saturated with oxygen. This oxygen was reduced after the cell returned to the operation mode with the flow of electrons. According to Simner et al. , during OCV, it is possible that the formation of oxygen-containing species can block the oxygen charge transport.
Silver metal diffusion through the electrolyte and ion migration can be a nanoscale phenomenon , which is impossible to be detected by SEM during post-mortem analyses. This can explain the detection of the short-circuit (at room temperature) without any visible cracks in the electrolyte, despite many SEM/EDX cross-section scans. However, this will require rigorous further investigation to validate the theory proposed.
Therefore, it is concluded that silver is a poor candidate for a contact material interconnect/cathode despite low and stable ASR. Gold is an alternative material for the current collector. In contrast to Pt and Ag, Au does not represent the tendency for migration into the SDC layer . However, the performance of the Au conductive layer may decrease with time of operation.
The application of silver as a cathode conductive material, interconnect wires, and sealing for anode lead connection for a µSOFC was studied. The addition of silver as a cathode conductive layer reduced the cell overpotential and increased the cell performance. However, the results showed that silver was also responsible for the cell degradation. Using silver in SOFC stacks reduces system durability. The silver thermal expansion did not match with the thermal expansion of the other cell materials, and therefore, caused damage to the glass sealant. Silver was also found unstable in the dual atmosphere. The results demonstrated that the microstructure of the silver anode lead connection wire changed after it had been exposed to the dual atmosphere, the solid silver wires and the seal became porous. The formation of striation structures and porosity affected the mechanical strength of the Ag interconnect wires.
The cathode polarisation process after OCV promotes silver migration what can lead to the cell short-circuit.
It can be concluded, that silver is not suitable as interconnect at the intermediate temperature in the long-term SOFC application if there is a risk of exposure to the dual atmosphere. Silver migration was also responsible for short-circuit formation.
The results are part of the outcome of the SAFARI project funded under Europe’s Fuel Cell and Hydrogen Joint Undertaking (FCH JU), Grant Agreement No.325323. The Consortium gratefully acknowledges the support of the FCH JU.
- 10.Heo, S., Hirano, A., Imanishi, N., Takeda, Y.: Improvement of SOFC’s cathode by silver and LSC infiltration. Meet. Abstr. MA2010-02(4), 240 (2010)Google Scholar
- 16.Mosiałek, M., Bielańska, E., Socha, R.P., Dudek, M., Mordarski, G., Nowak, P., Barbasz, J., Rapacz-Kmita, A.: Changes in the morphology and the composition of the Ag|YSZ and Ag|LSM interfaces caused by polarization. Solid State Ionics. 225, 755–759 (2012). https://doi.org/10.1016/j.ssi.2012.03.011 CrossRefGoogle Scholar
- 17.Asset, T., Roy, A., Sakamoto, T., Padilla, M., Matanovic, I., Artyushkova, K., Serov, A., Maillard, F., Chatenet, M., Asazawa, K., Tanaka, H., Atanassov, P.: Highly active and selective nickel molybdenum catalysts for direct hydrazine fuel cell. Electrochim. Acta. 215, 420–426 (2016). https://doi.org/10.1016/j.electacta.2016.08.106 CrossRefGoogle Scholar
- 18.Lee, W.H., Cho, B.S., Kang, B.J., Kim, J.Y., Lee, J.G., Jeong, C.O., Kim, Y.G.: Enhanced properties of Ag alloy films for advanced TFT-LCD’s. J. Korean Phys. Soc. 40(1), 110–114 (2002)Google Scholar
- 19.Compson, C., Choi, S., Abemathy, H., Choi, Y., Liu, M.: Stability and performance of silver in an SOFC interconnect environment. In: Advances in solid oxide fuel cells III: ceramic engineering science proceedings, vol. 28, pp. 301–312 (2009). https://doi.org/10.1002/9780470339534.ch28
- 25.Lavrenko, V.A., Malyshevskaya, A.I., Kuznetsova, L.I., Litvinenko, V.F., Pavlikov, V.N.: Features of high-temperature oxidation in air of silver and alloy Ag-Cu, and adsorption of oxygen on silver. Powder Metall. Met. Ceram. 45(9–10), 476–480 (2006). https://doi.org/10.1007/s11106-006-0108-8 CrossRefGoogle Scholar
- 33.Chen, Y., Wang, F., Chen, D., Dong, F., Park, H.J., Kwak, C., Shao, Z.: Role of silver current collector on the operational stability of selected cobalt-containing oxide electrodes for oxygen reduction reaction. J. Power Sources. 210, 146–153 (2012). https://doi.org/10.1016/j.jpowsour.2012.03.019 CrossRefGoogle Scholar
- 38.Kumar, A., Ciucci, F., Morozovska, A.N., Kalinin, S.V., Jesse, S.: Measuring oxygen reduction/evolution reactions on the nanoscale. Nat. Chem. 3(9), 707–713 (2011). doi:http://www.nature.com/nchem/journal/v3/n9/abs/nchem.1112.html#supplementary-information
Open AccessThis article is distributed under the terms of the Creative Commons Attribution 4.0 International License (http://creativecommons.org/licenses/by/4.0/), which permits unrestricted use, distribution, and reproduction in any medium, provided you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made.