Electrochemical oxidation of hydrogen peroxide at platinum electrodes. Part II: effect of potential

Hall, Simon B.; Khudaish, Emad A.; Hart, A. L.

doi:10.1016/s0013-4686(97)10116-5

Cited by 122 publications

(87 citation statements)

References 23 publications

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“…These experiments were performed in OER (green triangles), hydrogen peroxide oxidation (red squares, forming oxygen), and formic acid oxidation (blue circles, forming carbon dioxide, Figure 7). [40][41][42][43][44][45] These tests produced gas bubbles of various sizes on the electrode surface. At high gas generation rates, bubbles as large as 10 μl could periodically form and cover the electrode surface before diffusing away from the electrode.…”

Section: Resultsmentioning

confidence: 99%

Activity and Durability of Iridium Nanoparticles in the Oxygen Evolution Reaction

Alia

Rasimick

Ngo

et al. 2016

J. Electrochem. Soc.

169

223

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Unsupported iridium (Ir) nanoparticles, that serve as standard oxygen evolution reaction (OER) catalysts in acidic electrolyzers, were investigated for electrochemical performance and durability in rotating disk electrode (RDE) half-cells. Fixed potential holds and potential cycling were applied to probe the durability of Ir nanoparticles, and performance losses were found to be driven by particle growth (coarsening) at moderate potential (1.4 to 1.6 V) and Ir dissolution at higher potential (≥1.8 V Hydrogen is a major commodity chemical with approximately 2% of U. S. used energy going through a hydrogen pathway, primarily for ammonia production (agriculture) and the upgrading of crude oil (transportation). The majority of hydrogen in the US is produced from natural gas by steam methane reformation.1 While electrochemical water splitting currently represents a small percentage of hydrogen production, it is expected to have a growing role as costs decrease. 2Although the commercial competitiveness of electrolysis is currently limited by feedstock costs, catalyst cost and durability will become increasingly important as electrolyzers move toward low cost, intermittent, renewable sources of electricity such as wind and solar. 3,4 Acidic electrolyzers typically use iridium (Ir) in the oxygen evolution reaction (OER) as this material exhibits both reasonable activity and stability.5 Platinum and ruthenium have also been investigated as alternatives. Platinum, however, requires a higher overpotential (lower efficiency) and ruthenium has durability (dissolution) concerns. [6][7][8] Efforts to develop improved OER catalysts for acidic electrolyzers typically focus on supporting Ir oxide on titania 9-13 or alloying Ir with platinum, ruthenium, or other transition metal oxides [14][15][16][17][18][19][20][21][22][23] to improve durability and performance. Density functional theory studies have correlated trends in the OER activity of metal oxides to the adsorption energies of surface oxygen species, suggesting future directions for improving OER catalysts.24 Strasser et al. also examined the intrinsic activity of Ir, platinum, and ruthenium polycrystalline metals and nanoparticles in rotating disk electrode (RDE) half-cells, using carbon monoxide to determine catalyst surface areas.6 Efforts exploring OER catalysts, however, pale in comparison to the efforts expended in the pursuit of fuel cell catalysts for the oxygen reduction reaction (ORR). Specifically, the fuel cell community has established baselines and protocols for the performance and durability of ORR catalysts. [25][26][27][28] No such protocols or baselines currently exist for OER catalysts.This study presents data from several different commercial suppliers of unsupported and supported Ir and Ir oxide catalysts, and investigates the intrinsic activity of Ir in RDE half-cells, evaluating both performance and durability while presenting the data under standardized conditions. The modes of losses for Ir nanoparticles under specific testing protocols are present...

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Section: Resultsmentioning

confidence: 99%

Activity and Durability of Iridium Nanoparticles in the Oxygen Evolution Reaction

Alia

Rasimick

Ngo

et al. 2016

J. Electrochem. Soc.

169

223

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“…The oxidation of H 2 O 2 at metal electrodes has been studied in great detail by Hall et al 50,68 . It is also found to depend on surface oxide films.…”

Section: Acknowledgmentsmentioning

confidence: 99%

Nonlinear, electrocatalytic swimming in the presence of salt

Sabass

Seifert

2012

The Journal of Chemical Physics

112

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A small, bimetallic particle in a hydrogen peroxide solution can propel itself by means of an electrocatalytic reaction. The swimming is driven by a flux of ions around the particle. We model this process for the presence of a monovalent salt, where reaction-driven proton currents induce salt ion currents. A theory for thin diffuse layers is employed, which yields nonlinear, coupled transport equations. The boundary conditions include a compact Stern layer of adsorbed ions. Electrochemical processes on the particle surface are modeled with a first order reaction of the Butler-Volmer type. The equations are solved numerically for the swimming speed. An analytical approximation is derived under the assumption that the decomposition of hydrogen peroxide occurs mainly without inducing an electric current. We find that the swimming speed increases linearly with hydrogen peroxide concentration for small concentrations. The influence of ion diffusion on the reaction rate can lead to a concave shape of the function of speed vs. hydrogen peroxide concentration. The compact layer of ions on the particle diminishes the reaction rate and consequently reduces the speed. Our results are consistent with published experimental data.

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“…Moreover, the detection of H2O2 on conventional metal or carbon fiber electrodes is hindered by slow kinetics [10], [20] and relatively high overpotential [21], which allows also the oxidation of interfering species, such as ascorbic acid and uric acid [10]. Thus, new materials that facilitate fast and interference-free detection of H2O2 as well as resist biofouling are in demand.…”

Section: Introductionmentioning

confidence: 99%

Electrochemical detection of hydrogen peroxide on platinum-containing tetrahedral amorphous carbon sensors and evaluation of their biofouling properties

Tujunen

Kaivosoja

Protopopova

et al. 2015

Materials Science and Engineering: C

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Hydrogen peroxide is the product of various enzymatic reactions, and is thus typically utilized as the analyte in biosensors. However, its detection with conventional materials, such as noble metals or glassy carbon, is often hindered by slow kinetics and biofouling of the electrode. In this study electrochemical properties and suitability to peroxide detection as well as ability to resist biofouling of Pt-doped ta-C samples were evaluated. Pure ta-C and pure Pt were used as references. According to the results presented here it is proposed that combining ta-C with Pt results in good electrocatalytic activity towards H2O2 oxidation with better tolerance towards aqueous environment mimicking physiological conditions compared to pure Pt. In biofouling experiments, however, both the hybrid material and Pt were almost completely blocked after immersion in protein-containing solutions and did not produce any peaks for ferrocenemethanol oxidation or reduction. On the contrary, it was still possible to obtain clear peaks for H2O2 oxidation with them after similar treatment. Moreover, quartz crystal microbalance experiment showed less protein adsorption on the hybrid sample compared to Pt which is also supported by the electrochemical biofouling experiments for H2O2 detection.

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Electrochemical oxidation of hydrogen peroxide at platinum electrodes. Part II: effect of potential

Cited by 122 publications

References 23 publications

Activity and Durability of Iridium Nanoparticles in the Oxygen Evolution Reaction

Activity and Durability of Iridium Nanoparticles in the Oxygen Evolution Reaction

Nonlinear, electrocatalytic swimming in the presence of salt

Electrochemical detection of hydrogen peroxide on platinum-containing tetrahedral amorphous carbon sensors and evaluation of their biofouling properties

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