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Chapter 5. Aspects of Metal-YSZ Electrode Kinetics 166 TPB sites is about 10 μm [82]. From these values, a simple calculation can be done to estimate the LSRP in a porous electrode and compare it to the point electrode measurements. This gives a LSRP value in the range of 20-60 kΩ cm for the porous cermet (of course this would be on average, since there is a gradient in the porous electrode with more reactions occurring at the TPB regions closer to the electrolyte). In the present work, LSRP values of approximately 6 and 30 kΩ cm were measured on the point electrode (with a TPB presumably blocked by impurities) at 850 °C in 50% H2O/H2 and 3% H2O/H2 respectively. Since the activating effect of H2O is much less significant in a fine cermet, presumably the 3% H2O/H2 value can be compared. That the order of magnitude agrees so well is remarkable, and if such a simple calculation is correct, it suggests that perhaps equal concentrations of impurities are segregated to the TPB in the cermet electrode. In that case, the fine microstructure itself would be solely responsible for the different electrochemical properties of coarse and fine microstructured electrodes (such as the different activation energies). 5.5. Conclusions Metal wires contacting YSZ were systematically characterized as model electrodes for solid oxide cells. A number of important observations about the electrode kinetics of metal-YSZ interfaces were made: Widely different impedance responses of the different metals to the same parameter changes (such as gas composition and applied potential) were observed, which provides evidence that the different metals do not generally share the same reaction mechanisms, contrary to some recent studies that tried to correlate electrocatalytic activity of metals for H2 oxidation with a single other property of the metals. Trends in the responses were observed, indicating that some metals do share the same reaction mechanism in some conditions. The relative performance of the metals was Ni > Pd > Pt > Cu for H2 oxidation, Pd > Ni > Pt > Cu for H2O reduction, Ni > Pd > Cu > Pt for CO oxidation, and Pd > Ni > Pt > Cu for CO2 reduction. Pd was especially more active for the reduction reactions than for the oxidation reactions whereas Cu and Ni behaved oppositely. Pt was more active for oxidation of H2 than reduction of H2O, but in CO/CO2 it was more active for CO2 reduction than CO oxidation. Oxidation of Ni electrodes followed by re-reduction apparently induced formation of a fine microstructure of the Ni electrode and improved the electrode performance by an order of magnitude, but at high temperature (>850 °C) the effect was subsequently undone, most likely due to coarsening back to a smooth TPB.PDF Image | Electrolysis of CO2 and H2O
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