Oxidation of chlorinated ethenes by potassium permanganate: a kinetics study

Huang, Kun-Chang; Hoag, George E.; Chheda, Pradeep; Woody, Bernard A.; Dobbs, Gregory M.

doi:10.1016/s0304-3894(01)00241-2

Cited by 76 publications

(46 citation statements)

References 18 publications

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“…(8) After linear regression analysis (R 2 =0.9550), a value of 43.07 kJ/mol (10.25 kcal/mol) was calculated for E a . This activation energy value is a little higher than that measured for other organic compounds during permanganate oxidation, such as cyanotoxins MC-RR (28.8 kJ/mol) [17] and chloroethylene (24.36−39.1 kJ/mol) [32,33].…”

Section: Effect Of Temperaturementioning

confidence: 59%

Oxidation of estrone by permanganate: Reaction kinetics and estrogenicity removal

2010

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Permanganate was used as an oxidant to control estrone in the present study. Kinetics was determined at pH 2.5−9.4 and temperature 15-40°C for the reaction of estrone with potassium permanganate. It was found that the reaction is second-order overall and first-order with respect to both estrone and permanganate. The second-order rate constant for the reaction at pH 5.8 and 25°C is 44.45 L mol −1 s −1 . The reaction rate first decreased with the increase of pH in the range of 2.5−6.6 and then increased greatly with the increase of pH in the range of 6.6−9.4. In addition, the rate constant exponentially increased with the increase of reaction temperature. Removal of estrogenicity was also investigated during the degradation of estrone using yeast estrogen screen (YES). Results show that the estrogenicity increased in the initial 15 min of reaction and then decreased fast, with a removal rate of 73.8% within the 30 min of reaction. Results also demonstrate that the reaction rate between estrone and permanganate is faster in natural water background than in the ultra-pure water system. Permanganate oxidation is therefore a feasible option for removal of estrone in drinking water treatment processes. However, the contact time must be enough in order to remove estrone without causing the increase of estrogenicity. estrone, permanganate, rate constants, estrogenicity Citation: Shao X L, Ma J, Wen G, et al. Oxidation of estrone by permanganate: Reaction kinetics and estrogenicity removal.

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Section: Effect Of Temperaturementioning

confidence: 59%

Oxidation of estrone by permanganate: Reaction kinetics and estrogenicity removal

2010

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“…While the oxidation rates of organic contaminants achieved with permanganate is less than other oxidants, it is advantageous in that it is more persistent in the subsurface and can react over a wide pH range. Permanganate reactivity with chlorinated ethenes has been reported (Huang et al 2001;Hood et al 2000). But few data are available for the oxidation of chlorophenols by permanganate.…”

Section: Introductionmentioning

confidence: 99%

Oxidation of Chlorophenols in Aqueous Solution by Excess Potassium Permanganate

Hossain

McLaughlan

2011

Water Air Soil Pollut

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A simple spectrophotometric method was developed to quantify chlorophenol (CP) concentrations after reaction with potassium permanganate and quenching with sodium sulfite. Other quenching agents (peroxide, sodium thiosulfate and hydroxylamine hydrochloride) were found to create absorbance in the spectral range required for CP quantification. Analysis at pH 12 gave greater absorption and sensitivity for the method compared with pH 5.6. The calibration curves of the proposed methods were linear in the concentration ranges 0.0061-0.61 and 0.0078-0.78 mM with detection limit of 0.0006 and 0.0008 mM for dichlorophenols and monochlorophenols, respectively. The oxidation kinetics of five chlorophenols in aqueous solution with excess potassium permanganate were evaluated using the analytical method. The pseudo-first-order reaction rates were found to be relatively rapid 1.42× 10 −3 to 0.024 s −1 and followed the sequence 2-chlorophenol (2-CP) > 2,6-dichlorophenol (2,6-DCP)> 4-chlorophenol (4-CP) > 2,4-dichlorophenol (2, 4-DCP)>3-chlorophenol (3-CP). The apparent second-order rate constant was calculated from the measured pseudo-first-order rate constant with respect to CP with initial KMnO 4 concentration (1.5 mM) and follows the same sequence of pseudofirst-order rate constant. This shows that chlorine atoms in the structure of chlorophenol had a significant influence on the oxidation of chlorophenols by potassium permanganate. Permanganate can be used for the treatment of chlorophenolcontaminated soil and groundwater.

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“…They found that the kinetic rate of degradation decreased in the order of PCE, TCE, trans-DCE, and cis-DCE. It is interesting to note that this is nearly the opposite order found for chloroethene degradation by Huang et al (2001b) for permanganate oxidation. Waldemer et al (2007) generally found chloride production to be nearly quantitative, with about 80-90% recovered, but did identify several organic byproducts from chloroethene degradation.…”

Section: Chloroethenesmentioning

confidence: 85%

Fundamentals of ISCO Using Persulfate

Petri

Watts

Tsitonaki³

et al. 2010

SERDP/ESTCP Environmental Remediation Technology

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ScopeChemistry and use of persulfate for in situ chemical oxidation of subsurface contaminants, including free radical and other reaction mechanisms, catalysts, subsurface transport, and contaminant treatability. Key ConceptsPersulfate reaction chemistry is complex. Persulfate can react through direct electron transfer or free radical reactions. Electron transfer reactions are relatively slow and selective. Upon activation, the free radicals generated have nonspecific reactivity that allows for the degradation of a wide range of organic contaminants. The radicals that are presently understood to play a major role in reactions are the sulfate radical and the hydroxyl radical. However, there is emerging evidence that the superoxide anion and the perhydroxyl radical also may be important. Persulfate activation may be achieved by heat, chelated or non-chelated transition metals (especially iron), hydrogen peroxide, and alkaline pH conditions. The efficiency, effectiveness, and reaction products may vary between contaminants, activation methods, and the porous media to be treated. Carbonate, bicarbonate, or chloride ions can act as free radical scavengers and reduce reaction efficiency and effectiveness. The kinetics of reaction between persulfate and target compounds is complex. To simplify, pseudo first-order kinetics are often assumed. However, these usually require laboratory estimation because extrapolating between systems is difficult. The interaction of aquifer solids and persulfate is not well understood; persulfate does react with aquifer solids resulting in oxidant consumption, but the rate and magnitude of this process are not well characterized. Persistence varies from days to months, depending on conditions. The impact of persulfate on metal mobility is not well understood. Conceivably, persulfate could impact metal concentrations in groundwater through modification of pH, oxidation of metals, injection of activation amendments, and other mechanisms.

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Oxidation of chlorinated ethenes by potassium permanganate: a kinetics study

Cited by 76 publications

References 18 publications

Oxidation of estrone by permanganate: Reaction kinetics and estrogenicity removal

Oxidation of estrone by permanganate: Reaction kinetics and estrogenicity removal

Oxidation of Chlorophenols in Aqueous Solution by Excess Potassium Permanganate

Fundamentals of ISCO Using Persulfate

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