¹C.C.M.M., Departamento de Química e Bioquímica da Faculdade de Ciências da Universidade de Lisboa, Campo Grande, 1749-016 Lisboa, Portugal

²Laboratório Nacional de Energia e Geologia, Paço do Lumiar 22, Fuel Cells and Hydrogen Unit, 1649-038 Lisboa, Portugal

doi: 10.4152/pea.201105335

Abstract

In this work LaNiO₃ oxide was prepared by a self-combustion method using citric acid. The electrodes were obtained by coating a nickel foam support with the oxide suspension. Optical microscopy and cyclic voltammetry were used on the electrodes characterization. The evaluation of the electrodes electrocatalytic activity, towards the oxygen evolution reaction in alkaline medium, was performed by means of steady state measurements.

Keywords: LaNiO₃ electrode, nickel foam, oxygen evolution, electrocatalysis.

Introduction

Search for new or improved electrode materials is restless in the field of power sources, namely, of batteries and fuel cells. One of the challenging problems in the area is to find an effective electrode material that operates alternatively as anode and cathode and catalyses the oxygen electrochemical reactions (bifunctional oxygen electrode) [1, 2]. Perovskite type oxide materials are considered potential candidates since they can catalyse oxygen evolution and reduction, simultaneously. Several studies found in the literature suggest that Ni containing perovskites are among the most active [3-10]. Indeed LaNiO₃ is one of the best catalysts for the oxygen evolution reaction (OER), in alkaline medium, and it is also reported as a good catalyst for the oxygen reduction reaction (ORR) [11].

It is well known that the properties and behaviour of the LaNiO₃ electrode depend on the oxide preparation method, the experimental conditions, and in particular the support employed in the electrode construction [7,11,12]. Consequently, the kinetic parameters for oxygen evolution and reduction might vary.

The main goal of the work presented in this paper is the development of stable LaNiO₃ electrodes, with enhanced electrocatalytic activity towards the OER, using as support Ni foam.

To our knowledge this is the first report of construction of a LaNiO₃ electrode using Ni foam as support.

Experimental

The formation of the perovskite-type phase was confirmed by X-ray diffraction (XRD) using a Philips PW 1730 X-ray powder diffractometer, operating with Cu Kα radiation.

The films were prepared by coating (brush painting) nickel foam supports (Goodfellows), typically 1 cm × 1 cm, with a suspension of the oxide on TritonX-100 Fluke Chemie AG. After each application, the solvent was evaporated and the dried layer fired, in an oven, till the temperature reaches 673 K(≈4 h) followed by 3 h at 673 K. The oxide loading was around 89±5 mg cm^-2.

The samples were then mounted in a glass tube with Araldite epoxy resin, so that the electrolyte could only make contact with the oxide. Three specimens were prepared two for electrochemical experiments and one for morphological characterization.

The global aspect of the electrodes was observed by optical microscopy (Nikon SMZ 1500).

A conventional three-electrode glass cell was used. The measurements were carried out at room temperature, using Hg/HgO (+0.098V vs. SHE) and Ni foam as reference and counter electrodes, respectively. A Voltalab 10 (PGZ100) Radiometer apparatus controlled by a personal computer through the VoltaMaster 4 software has been used.

The potassium hydroxide 1 M solution (>90%, Sigma Aldrich) was prepared using Millipore Milli-Q ultrapure water (18 MΩ). Prior to each electrochemical measurement, the KOH 1 M solution was purged with high-purity N₂.

Steady state measurements were performed after stabilising the electrode at 0.720 V vs. Hg/HgO, for 10 min, in order to obtain a stable surface, prior to the measurements. Measurements were recorded from the higher to the lower potential value.

Results and discussion

The morphology of the LaNiO₃ coating was examined by optical microscopy, before and after being used as anode for the OER, in order to confirm that the Ni foam substrate was suitably covered with the oxide. For comparison, the images of the Ni foam were recorded. Fig. 1 shows the representative global aspect of the new (a), used (b) electrodes and the uncovered Ni foam support (c). The porosity of the nickel foam is evident from the image. Concerning the LaNiO₃ coating, the Ni foam support is almost fully covered by the oxide, although some uncovered Ni points are observed. The coating is characterized by an irregular surface, indicating high roughness. The electrode images, after and before being used for oxygen evolution, do not show significant variations.

Cyclic voltammetry

Fig. 2 shows a representative stabilized cyclic voltammogram recorded for a Ni/LaNiO₃ coated electrode in 1 M KOH at a sweep rate of 10 mVs^-1. For all the electrodes, an anodic and the corresponding cathodic peak are observed, prior oxygen evolution, usually assigned to the redox pair Ni³⁺/Ni²⁺ [7-10]. The estimated formal redox potential associated with this pair of peaks is within the range of those published, for the same oxide electrodes [7, 8]. In the negative potential range a cathodic peak is observed around -0.170 V vs. Hg/HgO attributed to the oxygen reduction [10]. The cyclic voltammograms run after and before the oxygen evolution showed similar features.

Oxygen evolution reaction

The study of the electrocatalytic activity of the prepared electrodes, towards the oxygen evolution reaction was studied in 1 M KOH solutions in the potential range of 0.500 - 0.720 V vs. Hg/HgO. Fig. 3 shows a representative Tafel plot, without Ohmic drop correction, for a freshly prepared Ni/LaNiO₃ coated electrode. As Fig, 3 shows, meaningful current intensities could be measured for potentials higher than 0.500 V vs. Hg/HgO. Once the standard potential of the oxygen electrode in basic solution is +0.300 V vs. Hg/HgO, it can be said that a minimum overpotential of ≈ 0.200 V is needed for oxygen evolution to occur. Linear plots for log i vs. E were obtained over less than 1 decade of current, in the potential range of 0.520-0.580 V (see Fig. 3 inset). Deviations at more anodic potentials can be due either to uncompensated Ohmic drops or to a second Tafel line + IR drops. The calculated Tafel slope has the value of 56 ± 4 mV. Values between 40 and 60 mV can be found in the literature, for this potential region, depending on the oxide preparation method, oxide support and electrode type [4, 7, 9, 13].

The most striking feature on the log i vs. E plots is the extremely narrow Tafel region. Similar behaviour has been observed by some of us for spinel type Fe - Co₃O₄ thin film [14] and Li - Co₃O₄ electrodes [15]. A detailed analysis of the data led us to conclude that the observed deviations, from Tafel behaviour, were a result of uncompensated Ohmic drops due to the electrode and electrolyte resistances as well as oxygen bubbles surface obstruction.

In order to distinguish between Ohmic drops or a second Tafel line, the Ohmic drops were estimated, following the methodology proposed by Boodts and Trasatti [16].

Fig. 4 shows the relationship of the potential difference ΔE, measured at constant current, between the experimental points and the extended Tafel line and the current density, in the potential range 0.560 - 0.710 V vs. Hg/HgO.

As in the presence of uncompensated Ohmic drops Tafel equation can be written as E = a + b lni + iR, it results dE/di = b/i + R [14, 17]. Fig. 5 shows the plot of ΔE/Δi vs. 1/i , being ΔE and Δi the difference of two consecutive experimental points and i the mean value between two consecutive values.

From the slope of the plot of ΔE/Δi vs. 1/i the corrected Tafel slope has been calculated and a value of 45±3 mV was obtained. This value is similar to the lowest values found in the literature for LaNiO₃ oxide electrodes, in the forms of pellets [4] and thin films on platinum [7], at low potentials.

The reaction order with respect to OH^-was obtained from E vs. log i curves recorded at varying concentrations of KOH at constant ionic strengths, using KNO₃ as the inert electrolyte. An order of 1.0 was estimated from the slope of the plot, log i vs. log [OH^-] at 683 mV vs. Hg/HgO (Fig. 6).

The reaction order and the Tafel slope observed indicate a mechanism similar to that already given by Bockris and Otagawa [18].

To get a better insight on the OER kinetics, the apparent exchange current density (i_0a) has been evaluated. In order to eliminate geometric effects and discriminate the geometric and electronic effects, the value of the true exchange current density i_0t (= i_0a/R_f), has been calculated by normalising i_0a to unit real surface area, taking into account the oxide roughness factor (R_f) [19], estimated from voltammetric curves, recorded in a narrow range of potential, near the open circuit potential [20].

Table 1 presents the estimated kinetic parameters for the OER on Ni/ LaNiO₃ electrodes. For the purpose of comparison, data for LaNiO₃ electrodes prepared by different methods, and presenting Tafel slopes of the same order, are shown.

The enhanced activity, towards the oxygen evolution reaction, of the electrodes prepared in this work, has been confirmed by the comparison between the potential values measured at 100 mA cm^-2 of apparent current density for LaNiO₃ films prepared by thermal decomposition and sequential coating, on Ni plates, under varying conditions [8]. A value of 0.760 V vs. Hg/HgO is reported for the most active electrode, while a lower value of 0.715 V vs. Hg/HgO was obtained in this work. Similarly higher values, 0.728 V vs. Hg/HgO, are quoted for LaNiO₃ films prepared by oxide-slurry painting, from powders prepared by the hydroxide solution precursor method [9].

Conclusions

In our exploration of new supports for the LaNiO₃ oxide we have successfully made use of Ni foam. It was found that the oxide preparation procedure by the self-combustion method, using citric acid, in combination with the use of Ni foam as support, enhanced the electrode surface properties. Consequently its electrocatalytic activity, towards the OER, is higher when compared with the reported in the literature for the same oxide electrode prepared by other methods. The better performance exhibited is due to the electrochemical properties of foam-oxide films originated from their highly porous morphologies. Synergetic effects between the Ni foam and the perovskite oxide cannot be discarded.

References