Kinetics and energy efficiency for the degradation of 1,4-dioxane by electro-peroxone process

Bakheet, Belal; Yuan, Shi; Li, Xiang; Yu, Gang; Murayama, Seiichi; Wang, Huijiao

doi:10.1016/j.jhazmat.2015.03.058

Cited by 91 publications

(34 citation statements)

References 35 publications

Supporting

Mentioning

Contrasting

Unclassified

Order By: Relevance

“…Mixing hydrogen peroxide with Fe 2+ or UV has been shown to be effective in removing dioxane (Kiker et al, 2010; Vescovi et al, 2010). Bench scale experiments have also demonstrated the effective removal of 1,4-dioxane using ozone, ozone plus hydrogen peroxide, persulfate, sono-activated persulfate, permanganate, and UV based oxidation technologies (Eberle et al, 2016; Ikehata et al, 2016; Li and Zhu, 2016; Wang et al, 2015; Félix-Navarro et al, 2007; Waldemer and Tratnyek, 2006; Vescovi et al, 2010; Mohr et al, 2010; Schreier et al, 2006). …”

Section: Introductionmentioning

confidence: 99%

Remediating 1,4-dioxane-contaminated water with slow-release persulfate and zerovalent iron

et al. 2017

View full text Add to dashboard Cite

1,4-dioxane is an emerging contaminant that was used as a corrosion inhibitor with chlorinated solvents. Metal-activated persulfate can degrade dioxane but reaction kinetics have typically been characterized by a rapid decrease during the first 30 min followed by either a slower decrease or no further change (i.e., plateau). Our objective was to identify the factors responsible for this plateau and then determine if slow-release formulations of sodium persulfate and Fe0 could provide a more sustainable degradation treatment. We accomplished this by conducting batch experiments where Fe0-activated persulfate was used to treat dioxane. Treatment variables included the timing at which the dioxane was added to the Fe0-persulfate reaction (T = 0 and 30 min) and including various products of the Fe0-persulfate reaction at T=0 min (Fe2+, Fe3+, and SO42−). Results showed that when dioxane was spiked into the reaction at 30 min, no degradation occurred; this is in stark contrast to the 60% decrease observed when added at T = 0 min. Adding Fe2+ at the onset (T= 0 min) also severely halted the reaction and caused a plateau. This indicates that excess ferrous iron produced from the Fe0-persulfate reaction scavenges sulfate radicals and prevents further dioxane degradation. By limiting the release of Fe0 in a slow-release wax formulation, degradation plateaus were avoided and 100% removal of dioxane observed. By using 14C-labeled dioxane, we show that ~40% of the dioxane carbon is mineralized within 6 d. These data support the use of slow-release persulfate and zerovalent iron to treat dioxane-contaminated water.

show abstract

Section: Introductionmentioning

confidence: 99%

Remediating 1,4-dioxane-contaminated water with slow-release persulfate and zerovalent iron

et al. 2017

View full text Add to dashboard Cite

show abstract

“…Wang vd. [28] çalışmalarında; ozon, elektrooksidasyon ve E-perokson prosesleri ile 1,4-dioksan giderimini karşılaştırmışlardır. Eperokson reaksiyon hızı konvansiyonel ozonlama prosesinden 16 kat daha yüksek elde edilmiştir.…”

Section: Elektroperokson Ozonlama Ve Elektrooksidasyonunclassified

Tannic acid oxidation by electroperoxone

Türkay

2019

Gazi Üniversitesi Mühendislik Mimarlık Fakültesi Dergisi

View full text Add to dashboard Cite

Highlights:Graphical/Tabular Abstract  Electroperoxone as a combination of ozone and electrooxidation processes has been tested for tannic acid oxidation.  Hydroxyl radical is generated by the reaction of ozone with in-situ produced H2O2.  Molecular ozone and hydroxyl radical have been involved together in tannic acid oxidation.Electoperoxone (E-peroxone) process enabling in-situ H2O2 production can supersede the conventional peroxone process that is required external addition of H2O2 into ozone to produce hydroxyl radicals (OH•). Eperoxone process provides electrochemically H2O2 production using the sparged oxygen during ozone generation by an ozone generator. This environment is achieved by placing an electrooxidation apparatus into an ozonation system. A highly oxidative medium rises in the E-peroxone system including the produced H2O2, dissolved ozone, and OH• radicals produced via both ozone self-decomposition and the reaction of ozone with H2O2. Tannic acid oxidation has been tested in this medium and potentially responsible oxidant species have been evaluated. The effect of ozone concentration and applied current change has also investigated in this study. Figure A. The produced oxidant species in the E-peroxone system and the comparison of oxidation processes through tannic acid degradation against timePurpose: This paper examines the combined use of ozone and electrooxidation (i.e. E-peroxone) to oxidize tannic acid. Theory and Methods:Two carbon-PTFE cathodes and Ti/IrO2-Ta2O5 anode were placed in an 800 ml circular ozone reactor. Ozonation and electrooxidation processes were operated both individually and in combination. The comparison of the oxidation efficiencies of the processes has been indicated as the normalized value of the tannic concentration and the dissolved organic carbon. The oxidation species produced were also observed as well as the removal efficiency. Results:Tannic acid oxidation by E-peroxone provided 10% more removal efficiency than that of ozonation. The oxidation of tannic acid is dominated by molecular ozone in the early stage of the reaction, and then the OH• radicals are abundantly produced in the aqueous medium, causing further oxidation of tannic acid. However, OH• radicals depleted after a while due to a decrease in pH value corresponding to carboxylic acid formation. According to observation on the effect of operating conditions on the removal efficiency, the amount of ozone that releases to the bulk solution should be increased and the applied current should be adjusted so as not to produce excess H2O2 to avoid the possible inhibitory effect of H2O2 on OH• radicals. Conclusion:The E-peroxone process has some advantages, such as in-situ H2O2 production using excess oxygen released from the ozone generator. Hydroxyl radicals can be effectively produced in this way, however, the role of the OH• radicals in oxidation may vary depending on the reactivity of the target substance against ozone and the pH of the aqueous medium. In the case of tannic acid, molecular ozone was do...

show abstract

“…This result indicates that E-peroxone is a superior process to mineralize venlafaxine and its transformation products than the two individual processes. This enhancement can be explained by the significant production of aqueous • OH from multiple sources during the E-peroxone process [23,[28][29][30], which enables non-selective mineralization of venlafaxine and its transformation products from the solution. In comparison, pollutant mineralization kinetics is limited by the selective oxidation of O 3 in ozonation process, and mass transfer of pollutants to the anode in electrolysis process [31,38,39].…”

Section: Degradation Of Venlafaxine By Ozonation Electrolysis and Ementioning

confidence: 99%

“…2 inset). This change can be mainly attributed to the formation and subsequent removal of carboxylic acid intermediates during the degradation of venlafaxine by the E-peroxone treatment (see discussion below and refer to [29,39]). To evaluate the effects of solution pH on the degradation of venlafaxine and TOC, the solution pH was controlled at three constant values (3.5, 7.5 and 10.5) throughout the whole reaction time by adding small amounts of 0.05 M NaOH or H 2 SO 4 .…”

Section: Effects Of Operational Parameters On Venlafaxine Degradationmentioning

confidence: 99%

Electro-peroxone treatment of the antidepressant venlafaxine: Operational parameters and mechanism

Wang

Zhao

et al. 2015

Journal of Hazardous Materials

Self Cite

View full text Add to dashboard Cite

Kinetics and energy efficiency for the degradation of 1,4-dioxane by electro-peroxone process

Cited by 91 publications

References 35 publications

Remediating 1,4-dioxane-contaminated water with slow-release persulfate and zerovalent iron

Remediating 1,4-dioxane-contaminated water with slow-release persulfate and zerovalent iron

Tannic acid oxidation by electroperoxone

Electro-peroxone treatment of the antidepressant venlafaxine: Operational parameters and mechanism

Contact Info

Product

Resources

About