Electrochemical advanced oxidation process for water treatment using DiaChem® electrodes

Tröster, I.; Fryda, M.; Herrmann, D.; Schäfer, Lothar; Hänni, W.; Perret, André; Blaschke, M.; Kraft, Alexander; Stadelmann, Manuela

doi:10.1016/s0925-9635(01)00706-3

Cited by 129 publications

(61 citation statements)

References 17 publications

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“…These include the possibility that oxidizing agents (e.g., hydroxyl radicals, active chlorine) are electrochemically produced at the anode without the need, in many cases, to add further reagents. 14,15 Additionally, the unselective nature of the produced oxidizing agents makes the method applicable for a large range of pollutants.…”

Section: Introductionmentioning

confidence: 99%

Electrochemical degradation of the dye reactive orange 16 using electrochemical flow-cell

Gomes¹,

Miwa²,

Malpass³

et al. 2011

J. Braz. Chem. Soc.

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As remoções eletroquímicas de cor e do conteúdo orgânico de soluções do corante laranja reativo 16 (RO16) foram efetuadas usando uma célula em fluxo e um eletrodo de trabalho de Pt. As influências das variáveis do sistema, tais como fluxo, concentração de NaCl, potencial aplicado e pH da solução, foram estudadas. A melhor remoção de cor foi de 93% (l = 493 nm) após 60 min de eletrólise potentiostática a 2,2 V vs. ERH, usando 1,00 g L -1 NaCl como eletrólito suporte. Os aumentos na concentração de NaCl e do potencial aumentam a velocidade de remoção de cor. A melhor remoção de carbono orgânico total (57%) foi obtida com a aplicação de 1,8 V, sem membrana de separação, indicando que as melhores condições para remoção de cor não são necessariamente as melhores para remover conteúdo orgânico. A eficiência de degradação diminui com a diminuição do pH da solução.Electrochemical removals of color and organic load from solutions containing the dye reactive orange 16 (RO16) were performed in an electrochemical flow-cell, using a platinum working electrode. The influence of the process variables flow-rate, such as NaCl concentration, applied potential and solution pH, were studied. The best color removal achieved was 93% (l = 493 nm) after 60 min at 2.2 V vs. RHE electrolysis, using 1.00 g L -1 NaCl as supporting electrolyte. The rises in the concentration of NaCl and applied potential increased the color removal rate. The best total organic carbon removal (57%) was obtained at 1.8 V, without the separating membrane, indicating that the ideal conditions for the color removal are not necessarily the same as those to remove the total organic carbon. The degradation efficiency decreased with the solution pH decrease.Keywords: decolorization, textile effluent, electrochemical degradation, reactive dye, Pt electrode IntroductionWhen untreated textile effluents are discharged into receiving water bodies many environmental problems can occur. The principal problems are that the presence of dyes (even at concentrations of < 1 ppm) that can cause considerable coloration in water courses, affect transparency to natural light (reducing photosynthesis), reduce gas solubility and may also present carcinogenic and mutagenic properties. 1,2Wide varieties of dyes are used in the textile industry and can be classified according to the manner in which they are fixed to the textile fiber (e.g., direct, reactive) or by their chemical structure (e.g., azo, anthraquinone). In the textile industry, reactive dyes are widely used due to their relatively easy application in the dyeing process and stability during wear. As a result of this stability, reactive dyes may require more complicated systems to achieve their removal from effluent flows. A number of methods presented in the literature are traditionally used to treat textile effluent and they are generally based on physical, chemical and biological treatments.3-5 Physical treatment methods tend to simply transfer the pollutant to a different phase and biological methods can be prolonged and ...

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Section: Introductionmentioning

confidence: 99%

Electrochemical degradation of the dye reactive orange 16 using electrochemical flow-cell

Gomes¹,

Miwa²,

Malpass³

et al. 2011

J. Braz. Chem. Soc.

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“…The ammonium persulfate solution was used as a modifier. The persulfate ions are characterised by a high redox potential E ⦵ = 2.01 V similar to ozone (E ⦵ = 2.07 V), which indicates great oxidation reactivity [27,28]. Kinetics of the modification process and the changes of the carbon surface were also investigated.…”

Section: Introductionmentioning

confidence: 99%

Persulfate treatment as a method of modifying carbon electrode material for aqueous electrochemical capacitors

Kopczyński

Pęziak-Kowalska

Lota

et al. 2016

J Solid State Electrochem

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The activated carbon was modified by the wet method with a solution of ammonium persulfate at room temperature with different times. Kinetics studies showed that the modification took place mostly during the first 60 min of the process. The physicochemical properties of the obtained carbon were evaluated by thermogravimetric studies, Raman and FTIR spectroscopy, elementary and BET analyses. Furthermore, the fabricated material was applied in symmetric capacitors operated on the three aqueous electrolytes (1 M H 2 SO 4 , 6 M KOH and 1 M Na 2 SO 4 ). Mild conditions of the modification process are optimal to obtain electroactive groups on the carbon surface, which make this material useful in a supercapacitor application. In our studies, we noticed that this type of functional groups mainly appears on the surface of the activated carbon, in the first oxidation stage. With prolonged oxidation, they may transform into undesirable groups. The results show that this kind of modification improves the capacity of all the tested supercapacitors. It was connected mainly with an increase of the carbon material's wettability and in the case of capacitor operated in acid and base electrolytes due to a redox reaction of oxygen functional groups.

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“…The formation of sulfur may come with a significant solids handling problem and can lead to problems in cell operation. 8 In many applications, for example, in the chemical process industries, sulfuric acid is a desirable product as it can be used in chemical manufacture and is readily transported.…”

mentioning

confidence: 99%

Remove Sulfur Dioxide from Flue Gases to Obtain Sulfuric Acid through Electrodialysis Enrichment

NingPing

et al. 2015

J. Electrochem. Soc.

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This article illustrates the experimental research which disposes low concentration SO 2 flue gases through liquid absorption and electrodialysis enrichment. It introduces the technology and devices to produce sulfuric acid by liquid absorption and oxidation of low concentration SO 2 in aqueous solutions as well as electrodialysis enrichment in the same reactor. Numerous experiments have been carried out in order to observe the performance of the reactor under the operating conditions: the current density, temperature, volume flow rate of the electrolyte, the sulfuric acid concentration, volume flow rate of the gas, the components of gas mixture, and initial SO 2 concentration. When the removal rate of SO 2 reaches 83.64%, we eventually get sulfuric acid with the concentration of 28.56%. Sulfur dioxide in flue gas generated from the combustion of fossil fuel, such as metal smelting factory, thermal power plants, etc. It is the main cause of air pollution and acid rain. Many countries have therefore adopted strict regulations to SO 2 emissions from coal and oil-fired boilers, which are one of the primary sources of SO 2 emissions. The increasing importance of sulfur dioxide pollution control stimulated the improvement of technology for the removal of sulfur dioxide from flue and waste gases.The electrochemical processes which do not require the continuous use of chemical reagents, possess advantages and bring a helpful contribution in the proposal or development of depollution processes. 1 Sulfur dioxide can be oxidized electrochemically to species such as sulfuric acid and dithionite, the electrochemical oxidation of SO 2 has been investigated both as a pollution control method and as part of recycling and utilization of resources.2,3 The electrochemical oxidation of sulfur dioxide can be achieved either through a direct process at an anode surface or using a redox mediator through a chemical process, which has to be regenerated at the electrode. 4 In the electrolysis of the sulfur dioxide absorbed in aqueous solution, the process involves a chemical oxidation of SO 2 by adsorbed oxygen species.5 It is also possible that SO 2 is oxidized at the anode while hydrogen is produced at the cathode.6 Furthermore, the removal of SO 2 from the copper ions containing wastes provides electrowinning of copper simultaneously. 7The main products of electrochemical oxidation and reduction of SO 2 in acid solution are sulfuric acid and sulfur, respectively. The formation of sulfur may come with a significant solids handling problem and can lead to problems in cell operation.8 In many applications, for example, in the chemical process industries, sulfuric acid is a desirable product as it can be used in chemical manufacture and is readily transported.The overall reaction for the oxidation of SO 2 can be written as:Where hydrogen is formed at the cathode. Dissolved sulfur dioxide is converted to sulfuric acid at the anode and hydrogen is formed at the cathode. 9 The mechanism of SO 2 oxidation in water is complex, the absorption ...

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Electrochemical advanced oxidation process for water treatment using DiaChem® electrodes

Cited by 129 publications

References 17 publications

Electrochemical degradation of the dye reactive orange 16 using electrochemical flow-cell

Electrochemical degradation of the dye reactive orange 16 using electrochemical flow-cell

Persulfate treatment as a method of modifying carbon electrode material for aqueous electrochemical capacitors

Remove Sulfur Dioxide from Flue Gases to Obtain Sulfuric Acid through Electrodialysis Enrichment

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