Synthesis of Hydrogen Peroxide in a Proton Exchange Membrane Electrochemical Reactor

Tatapudi, Pallav; Fenton, James M.

doi:10.1149/1.2056245

Cited by 27 publications

(12 citation statements)

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“…Examining ORR kinetics on oxide thin films allows a more accurate measure of the specific activity of solely the oxide surface , in comparison to ORR studies of composite electrodes that consist of oxide and carbon particles. As carbon is very active for the two-electron pathway of the ORR forming hydroperoxide, , its presence in composite electrodes can greatly influence the measured number of electrons transferred and ORR activity of catalysts with low activities. ,,− In addition, these thin-film oxide samples allow for the study of the role of surface termination on ORR kinetics. ,, Moreover, studying pure catalysts without the incorporation of conductive carbon enables the measure of charge transfer kinetics on the oxide surface using kinetically facile redox couples such as [Fe(CN) 6 ] 3–/4– in solution, independent from ORR kinetics measurements . Having relatively thin oxide films on conductive substrates (Nb-doped SrTiO 3 or Pt) to facilitate charge transfer kinetics at the oxide surface is critical, as most manganese oxides are poor electronic conductors.…”

Section: Measuring and Quantifying Orr Kinetics: Specific And Mass Ac...mentioning

confidence: 99%

“…35 Examining ORR kinetics on oxide thin films allows a more accurate measure of the specific activity of solely the oxide surface 34,36 in comparison to ORR studies of composite electrodes that consist of oxide and carbon particles. As carbon is very active for the two-electron pathway of the ORR forming hydroperoxide, 37,38 its presence in composite electrodes can greatly influence the measured number of electrons transferred and ORR activity of catalysts with low activities. 35,37,39−42 In addition, these thin-film oxide samples allow for the study of the role of surface termination on ORR kinetics.…”

Section: Measuring and Quantifying Orr Kineticsmentioning

confidence: 99%

“…Thus, studies of both binary and ternary manganese oxides point to Mn 3+ , possibly including some Mn 4+ (but not Mn 2+ ) as key to catalyzing the four-electron process. We caution, however, that common support materials such as carbon 37,38 and gold 91 are active for oxygen reduction to hydroperoxide (2e − ) at large overpotentials and may influence the observed number of electrons transferred.…”

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confidence: 97%

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Recent Insights into Manganese Oxides in Catalyzing Oxygen Reduction Kinetics

et al. 2015

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The sluggish kinetics of the oxygen reduction reaction (ORR) limit the efficiency of numerous oxygen-based energy conversion devices such as fuel cells and metal-air batteries. Among earth abundant catalysts, manganese-based oxides have the highest activities approaching that of precious metals. In this Review, we summarize and analyze literature findings to highlight key parameters that influence the catalysis of the ORR on manganese-based oxides, including the number of electrons transferred, specific and mass activities. These insights can help develop design guides for highly active ORR catalysts, and shape future fundamental research to gain new knowledge regarding the molecular mechanism of ORR catalysis.2

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Section: Measuring and Quantifying Orr Kinetics: Specific And Mass Ac...mentioning

confidence: 99%

Section: Measuring and Quantifying Orr Kineticsmentioning

confidence: 99%

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confidence: 97%

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Recent Insights into Manganese Oxides in Catalyzing Oxygen Reduction Kinetics

et al. 2015

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“…In general, there are two main pathways to degrade organic pollutants in an electrochemical reactor. One is direct oxidation of the anode, and the other is indirect oxidation of electro-generated H 2 O 2 from the two-electron reduction of oxygen on cathode, as described by eq . − …”

Section: Resultsmentioning

confidence: 99%

Potential of Sludge Carbon as New Granular Electrodes for Degradation of Acid Orange 7

Sun

Chen

Kong

et al. 2015

Ind. Eng. Chem. Res.

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Powdered sludge carbons were prepared by pyrolysis at 800 °C and used for the first time as microparticle electrodes of a three-dimensional electrode reactor. It was found that acid orange 7 (AO7) could be efficiently removed by adsorption and electro-oxidation. The electrochemical oxidation could degrade both AO7 in aqueous solution and AO7 adsorbed on the microparticle electrodes. The degradation efficiency of the former reached 80.2%, and that of the latter is estimated to be 13.6% of the adsorption amount under the conditions of 20 V cell voltage, 300 mL min–1 airflow, and 60 min reaction time. This degradation is a result of not only the electrocatalytic activity of the carbon component but also the electro-Fenton-like effect of Fe3O4 and the co-Fenton-like effect of SiO2 and Al2O3 in the sludge carbon.

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“…The PbQ/gold, carbon, and graphite M&Es were prepared using the procedure in Ref. 3 gold. This catalyst mixture was then deposited onto the CFP with a loading of 6.2 mg/cm 2.…”

Section: Methodsmentioning

confidence: 99%

Simultaneous Synthesis of Ozone and Hydrogen Peroxide in a Proton‐Exchange‐Membrane Electrochemical Reactor

Tatapudi

Fenton

1994

J. Electrochem. Soc.

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Deionized water was oxidized to form ozone at the anode while oxygen was reduced to hydrogen peroxide at the cathode in a proton-exchange-membrane electrochemical flow reactor. The conditions for simultaneous generation of these oxidants were determined as a function of the applied voltage, electrode materials (lead dioxide for ozone evolution; gold, carbon, or graphite for peroxide evolution), and electrode configurations. Measured and calculated quantities included cell current, liquid-and gas-phase ozone concentrations, hydrogen peroxide concentrations, current efficiency for ozone and peroxide evolution, and ozone and peroxide production rates. An applied potential of 4.5 V resulted in a current density of 2 A/cm z, yielding maximum gas-and liquid-phase ozone concentrations of 60 and 3.1 mg/liter at the anode (4.5% current efficiency) and hydrogen peroxide concentrations between 3 and 5 mg/liter at the cathode (0.8% current efficiency).The simultaneous synthesis of ozone and hydrogen peroxide in a proton-exchange-membrane (PEM) electrochemical flow reactor was explored. The research methodology for the paired synthesis was split into four reaction systems: 1, oxygen evolution at the anode and hydrogen evolution at the cathode (water electrolysis); 2, ozone + oxygen evolution at the anode and hydrogen evolution at the cathode; 3, oxygen reduction at the cathode (hydrogen peroxide synthesis) and oxygen evolution at the anode; and 4, simultaneous synthesis of ozone and hydrogen peroxide.Preliminary studies on the first two reaction systems I and detailed studies on reaction systems 2 ~ and 33 have been conducted. This paper describes the simultaneous oxidation of water at the anode to form ozone while reducing humidified oxygen at the cathode to form hydrogen peroxide (reaction system 4).Although there have been investigations on the individual electrochemical synthesis of ozone and hydrogen peroxide in aqueous electrolytes (acidic electrolytes for ozone, 4 and acidic and basic electrolytes for hydrogen peroxide), 5-~ very little information exists on the generation of ozone in pure water. 9'I° Also, other than the authors' own work, ~ no information exists on the generation of hydrogen peroxide using oxygen as the reactant and a proton exchange membrane as the electrolyte. Furthermore, no study has been performed to date on the design and development of a process to synthesize simultaneously ozone and hydrogen peroxide electrochemically.Ozone evolution occurs at E ° = 1.51 V vs. NHE, while hydrogen peroxide is produced at a much lower potential, E ° = 0.682 V vs. NHE. This large difference in the standard potentials suggests that high current efficiencies for hydrogen peroxide will not be obtained at potentials at which ozone is formed (due to the reduction of oxygen and hydrogen peroxide to water and possible hydrogen evolution at higher potentials). Although this large difference exists, the paired synthesis of these oxidants will eliminate the use of two separate cells where ozone is an anodic product (with ...

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Synthesis of Hydrogen Peroxide in a Proton Exchange Membrane Electrochemical Reactor

Cited by 27 publications

References 0 publications

Recent Insights into Manganese Oxides in Catalyzing Oxygen Reduction Kinetics

Recent Insights into Manganese Oxides in Catalyzing Oxygen Reduction Kinetics

Potential of Sludge Carbon as New Granular Electrodes for Degradation of Acid Orange 7

Simultaneous Synthesis of Ozone and Hydrogen Peroxide in a Proton‐Exchange‐Membrane Electrochemical Reactor

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