Relevant bibliographies by topics / Chlorine

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  1. Journal articles
  2. Dissertations / Theses
  3. Books
  4. Book chapters
  5. Conference papers
  6. Reports

Academic literature on the topic 'Chlorine'

Author: Grafiati
Published: 4 June 2021
Last updated: 14 September 2024

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Journal articles on the topic "Chlorine"

1

Svenson, Doug R., Hou-min Chang, Hasan Jameel, and John F. Kadla. "The role of non-phenolic lignin in chlorate-forming reactions during chlorine dioxide bleaching of softwood kraft pulp." Holzforschung 59, no. 2 (February 1, 2005): 110–15. http://dx.doi.org/10.1515/hf.2005.017.

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Abstract The affect of phenolic hydroxyl groups on the reaction efficiency during chlorine dioxide pre-bleaching of a softwood kraft pulp was investigated. The removal of phenolic hydroxyl groups via pulp methylation did not adversely affect the chlorine dioxide bleaching efficiency or the amount of chlorate formed during exposure to chlorine dioxide. Ion analysis of the reaction systems revealed that the formation of chloride and chlorite ions during the bleaching process were very similar between the kraft and methylated kraft pulps. These results indicate that the kinetic rates of lignin oxidation by chlorine dioxide and its reduction products, chlorite and hypochlorous acid, are much faster than the rate of inorganic reactions leading to chlorate formation.
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MOKIIЕNKO, Andrii, Larysa SPASONOVA, and Oleksandr BONDARCНUK. "ANALYSIS OF METHODS FOR DETERMINATION OF CHLORINE DIOXIDE, CHLORITE AND CHLORATE ANIONS IN DRINKING WATER." Herald of Khmelnytskyi National University. Technical sciences 317, no. 1 (February 23, 2023): 294–99. http://dx.doi.org/10.31891/2307-5732-2023-317-1-294-299.

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The analysis shows that the primary measure for the purification of drinking water is its reliable disinfection with oxidants, which are chlorine and its compounds, chlorine dioxide, ozone. The aim of the article is to analyze the existing methods for determination of chlorine dioxide, chlorite, hypochlorite and chlorate anions in drinking water. To analyze the chlorine dioxide strength solutions (to control the generator performance) the iodometric method (determination of chlorine dioxide concentration, concentration of free chlorine, chlorite and chlorate anions; relative error ≤ 5%) and the method of direct absorption at 445 nm (determination of chlorine dioxide concentration in the range of concentrations of 100-700 mg / l; relative error ≤ 2%) were used. To analyze the residual concentrations of chlorine dioxide, chlorite and hypochlorite anions in their joint presence the titrimetric and photometric methods with N,N-діетил-1,4-фенилендіамінсульфатом (DFD) (error of determination is of 0.05 mg/l) were used as well as iodometric method with photometric determination of iodine at 350 nm in the concentration range 0.01-0.5 mg/l. To analyze the residual concentrations of chlorine dioxide (selective methods), such methods were used: the photometric method with chlorophenol red in the concentration range of 0.02-0.7 mg/l; relative error ≤ 5%; photometric method with chromic violet acid in the concentration range of 0.1-1.5 mg/l. The method of ion chromatography was used to analyze the residual concentrations of chlorite and chlorate anions. Given the necessity for harmonization of domestic regulatory and guidance documentation with European one, it should be considered as necessary to control chlorites and chlorates in drinking water by method of ion chromatography. It is appropriate to conduct research on the approbation of ion chromatography method for the simultaneous determination of chlorites and chlorates in samples of water after its disinfection by various oxidants (sodium hypochlorite, ozone, chlorine dioxide).
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Paun, Iuliana, Florentina Laura Chiriac, Vasile Ion Iancu, Florinela Pirvu, Marcela Niculescu, and Nicoleta Vasilache. "Disinfection by-products in drinking water distribution system of Bucharest City." Romanian Journal of Ecology & Environmental Chemistry 3, no. 1 (June 25, 2021): 10–18. http://dx.doi.org/10.21698/rjeec.2021.102.

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Chlorine is widely used in Romania and all over the world as a disinfectant of drinking water. During the chlorination process, the natural organic matter and inorganic ions react with chlorine forming disinfection by-products (DBPs). The predominant organic disinfection by-products are trihalomethanes (THMs) while the main inorganic disinfection by-products are chlorate and chlorite ions. THMs were detected in all investigated drinking water samples from Bucharest distribution system with values from 27.8 µg/L up to 75.1 µg/L, which are below the maximum concentration value admitted by Romanian drinking water legislation of 100 µg/L. Chloroform constitutes the major component in total THMs concentration found in all tested drinking water. Chlorate and chlorite anions were not detected in any of the investigated drinking water samples. THMs concentration was correlated with total organic carbon (TOC), residual chlorine and chloride.
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Lapina, E. A., S. A. Zverev, S. V. Andreev, and K. A. Sakharov. "Determination of chlorine-containing compounds in disinfectants using ion-exchange chromatography." Fine Chemical Technologies 18, no. 3 (August 2, 2023): 254–64. http://dx.doi.org/10.32362/2410-6593-2023-18-3-254-264.

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Objectives. To develop a method for the determination of hypochlorite, chloride, chlorite, chlorate, and perchlorate ions in solution; to determine the limits of detection and quantitation for ClO−, Cl−, ClO2−, ClO3−, and ClO4− ions; to evaluate the applicability of the developed method and its suitability for disinfectant analysis.Methods. Ionic chromatography using a conductometric detection system in isocratic elution mode.Results. The method developed for chromatographic determination of chlorine-containing ions can be used to quantify the content of hypochlorite, chloride, chlorite, chlorate, and perchlorate ions. In isocratic elution mode at 7.5 mM NaOH and a flow rate of 0.4 mL/min, the content of chlorine-containing ions can be determined with high sensitivity. The presented method does not require the use of expensive equipment for the ultrasensitive analysis of the studied compounds.Conclusions. A novel method for the simultaneous determination of hypochlorite, chloride, chlorite, chlorate, and perchlorate ions in case of their combined presence is proposed. The technique can be used to carry out routine control of the content of these disinfectant components during use, increasing their effectiveness at the same time as managing associated toxicological risks.
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Gambardella, Mario, Santad Kongpricha, James J. Pitts, and Albert W. Jache. "Disproportionation of chlorine in hydrogen fluoride and related media." Canadian Journal of Chemistry 67, no. 11 (November 1, 1989): 1828–31. http://dx.doi.org/10.1139/v89-283.

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Chlorine can be made to disproportionate to chlorine monofluoride and chloride, taking advantage of Le Chatelier's principle in several different ways. It will disproportionate to form insoluble silver chloride and chlorine monofluoride when silver fluoride is present. It will disproportionate in a melt of alkali metal fluorides to form alkali metal chlorides and chlorine monofluoride. The alkali metal chlorides will react with hydrogen fluoride to regenerate the metal fluorides and hydrogen chloride. Chlorine will also disproportionate in hydrogen fluoride containing antimony pentafluoride to yield antimony pentafluoride adducts of chlorine monofluoride and of hydrogen chloride. These adducts are readily decomposed to yield the disproportionation products and the original antimony pentafluoride. Keywords: hydrogen fluoride, disproportionation, chlorine, waterlike, solvent system.
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Xu, Cuisheng, Ningke Hao, Lei Zhan, Shiwei Wang, Shuangquan Yao, Shuangxi Nie, and Shuangfei Wang. "High Purity Chlorine Dioxide Generation Based on the Mixed Reductant: From the Laboratory to Industry." Journal of Biobased Materials and Bioenergy 13, no. 4 (August 1, 2019): 517–22. http://dx.doi.org/10.1166/jbmb.2019.1885.

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Methanol was used as reducing agent in the chlorine dioxide generation technology, and sodium chlorate was reduced to form chlorine dioxide under acidic conditions. The side reaction during the preparation process would produce chlorine, which results in a high content of chlorine in the product and leads to an increase in the amount of AOX formation during pulp bleaching. In this work, the chlorine dioxide generation technology based on the mixed reductant was developed. On the basis system based on the methanol method, a high-purity chlorine dioxide for pulp bleaching was successfully produced using a vertical generator by adding a mixed reducing agent that contain hydrogen peroxide and sodium chloride. This invention can not only solve the problems of low conversion rate of sodium chlorate and high content of chlorine in the traditional methanol reduction method, but also reduces the production cost. The chlorine content in the chlorine dioxide solution is reduced to less than 0.2 g/L.
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Moore, Nathan, Shelir Ebrahimi, Yanping Zhu, Chengjin Wang, Ron Hofmann, and Susan Andrews. "A comparison of sodium sulfite, ammonium chloride, and ascorbic acid for quenching chlorine prior to disinfection byproduct analysis." Water Supply 21, no. 5 (March 2, 2021): 2313–23. http://dx.doi.org/10.2166/ws.2021.059.

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Abstract This study compared 3 commonly used quenching agents for dechlorinating samples prior to disinfection byproduct (DBP) analysis under typical drinking water sampling conditions for a representative suite of chlorination byproducts. Ascorbic acid and sodium sulfite quenched the residual free chlorine to below detection within 5 seconds. Ammonium chloride did not quench the chlorine to below detection with up to a 70% molar excess, which agrees with published ammonium chloride-chlorine chemistry. With respect to the DBPs, ascorbic acid worked well for the trihalomethanes and haloacetic acids, except for dibromoiodomethane, which exhibited 2.6–28% error when using ascorbic acid compared to non-quenched control samples. Sodium sulfite also worked well for the trihalomethanes (and performed similarly to ascorbic acid for dibromoiodomethane) and was the best performing quenching agent for MX and the inorganic DBPs, but contributed to the decay of several emerging DBPs, including several halonitromethanes and haloacetamides. Ammonium chloride led to considerable errors for many DBPs, including 27–31% errors in chloroform concentrations after 24 hours of storage. This work shows that ascorbic acid is suitable for many of the organic DBPs analyzed by gas chromatography-electron capture detection and that sodium sulfite may be used for simultaneous chlorite, chlorate, and bromate analysis.
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Wu, Ming Song, Xun Xu, Xin Yang Xu, Shu Juan Chen, Zi Wei Huang, Deng Biao, and Ya Jie Hu. "High-Purity Chlorine Dioxide Generation Process from Sodium Chlorate by Using Waste Molasses." Advanced Materials Research 955-959 (June 2014): 3924–27. http://dx.doi.org/10.4028/www.scientific.net/amr.955-959.3924.

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A new chlorate-based chlorine dioxide generation process was developed by using waste molasses as reductant in the presence of sulfuric acid catalyst. The optimum technological condition was determined as 80 oC, 50% sulfuric acid, molasses and sodium chlorite weight ratio of 1:4. The best conversion rate and purity of chlorine dioxide was 73.8% and 95.1%, respectively. Chlorite was found in the reacting mixtures, and major reactions of in process were inferred. The results obtained provides a new way for waste molasses comprehensive utilization and chlorine dioxide generation.
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Monteiro, Mayra K. S., Ángela Moratalla, Cristina Sáez, Elisama V. Dos Santos, and Manuel A. Rodrigo. "Production of Chlorine Dioxide Using Hydrogen Peroxide and Chlorates." Catalysts 11, no. 12 (December 2, 2021): 1478. http://dx.doi.org/10.3390/catal11121478.

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Chlorine dioxide was produced by the reduction of chlorate with hydrogen peroxide in strongly acidic media. To avoid reaction interference during measuring procedures, UV spectra were acquired to monitor the chlorate reduction. This reduction led to the formation of chlorine dioxide and notable concentrations of chlorite and hypochlorous acid/chlorine, suggesting that the hydrogen peroxide:chlorate ratio is important. Once chlorates are transformed to chlorine dioxide, the surplus hydrogen peroxide promoted the further reaction of the chlorinated species down to less-important species. Moreover, chlorine dioxide was stripped with the outlet gas flow. A linear relationship was established between the amount of limiting reagent consumed and the maximum height of the absorption peak at 360 nm after testing with different ratios of hydrogen peroxide and chlorate, allowing calculations of the maximum amount of chlorine dioxide formed. To verify the reproducibility of the method, a test with four replicates was conducted in a hydrogen peroxide/chlorate solution where chlorine dioxide reduction was not promoted due to the presence of surplus chlorate in the reaction medium after the test. Results confirmed the efficient formation of this oxidant, with maximum concentrations of 8.0 ± 0.33 mmol L−1 in 400–450 min and a conversion percentage of 97.6%. Standard deviations of 0.14–0.49 mmol L−1 were obtained during oxidation (3.6–6.5% of the average), indicating good reproducibility.
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Mikkelsen, Marie K., Jesper B. Liisberg, Maarten M. J. W. van Herpen, Kurt V. Mikkelsen, and Matthew S. Johnson. "Photocatalytic chloride-to-chlorine conversion by ionic iron in aqueous aerosols: a combined experimental, quantum chemical, and chemical equilibrium model study." Aerosol Research 2, no. 1 (March 19, 2024): 31–47. http://dx.doi.org/10.5194/ar-2-31-2024.

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Abstract. Prior aerosol chamber experiments show that the ligand-to-metal charge transfer absorption in iron(III) chlorides can lead to the production of chlorine (Cl2/Cl). Based on this mechanism, the photocatalytic oxidation of chloride (Cl−) in mineral dust–sea spray aerosols was recently shown to be the largest source of chlorine over the North Atlantic. However, there has not been a detailed analysis of the mechanism that includes the aqueous formation equilibria and the absorption spectra of the iron chlorides nor has there been an analysis of which iron chloride is the main chromophore. Here we present the results of experiments measuring the photolysis of FeCl3 ⋅ 6H2O in specific wavelength bands, an analysis of the absorption spectra of FeCln3-n (n=1 … 4) made using density functional theory, and the results of an aqueous-phase model that predicts the abundance of the iron chlorides with changes in pH and iron concentrations. Transition state analysis is used to determine the energy thresholds of the dissociations of the species. Based on a speciation model with conditions extending from dilute water droplets and acidic seawater droplets to brine and salty crust, as well as the absorption rates and dissociation thresholds, we find that FeCl2+ is the most important species for chlorine production for a wide range of conditions. The mechanism was found to be active in the range of 400 to 530 nm, with a maximum around 440 nm. We conclude that iron chlorides will form in atmospheric aerosols from the combination of iron(III) cations with chloride and that they will be activated by sunlight, generating chlorine (Cl2/Cl) from chloride (Cl−) in a process that is catalytic in both chlorine and iron.
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Dissertations / Theses on the topic "Chlorine"

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Desai, Unmesh Jeetendra. "Comparative Analytical Methods for the Measurment of Chlorine Dioxide." Thesis, Virginia Tech, 2002. http://hdl.handle.net/10919/34134.

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Four commercially available methods used for the analysis of low-level Chlorine Dioxide (ClO2) concentrations in drinking water were evaluated for accuracy and precision and ranked according to cost, efficiency and ease of the methods under several conditions that might be encountered at water treatment plants. The different analytical methods included: 1.The DPD (N, N-diethyl-p-phenylenediamine) method 2.Lissamine Green B (LGB) wet-chemical method 3.Palintest® kit LGB 4.Amperometric titration All these tests were performed with standard 1.0 mg/L ClO2 either alone or in the presence of different chlorine species, including chlorite ion (ClO2-, 0.5 mg/L), chlorate ion (ClO3-, 0.5 mg/L) and chlorine (Cl2, 1.0 mg/L). The tests were performed with four different matrices, with different concentrations of 0.1 mg/L ClO2, 0.5 mg/L ClO2 and 1.0 mg/L ClO2 at a constant temperature of 20oC and at different temperatures of 0oC, 10oC and 20oC at a fixed ClO2 concentration of 1.0 mg/L. None of the four methods produced the desired level of either accuracy or precision. For all four methods, interference to the measured ClO2 concentration from the addition of ClO2-, ClO3-, and Cl2 was minimal when the methods were performed according to specifications. The Palintest® was the best all-round method because it was easy to perform, performed well at all concentrations tested, and its colored product was stable. The HACH® DPD method was also easy to perform and gave the best results when measuring concentrations of 1.0 mg/L ClO2. The DPD method was less accurate than the Palintest® at lower concentrations. The DPD colored product that formed upon reaction of ClO2 and DPD was unstable, making it necessary to measure the intensity of the colored product at exactly 1 minute. The amperometric titration and lissamine green methods were more cumbersome and time-consuming to perform than either the DPD or Palintest® methods; for this reason they are less desirable for routine use.
Master of Science
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Johansson, Emma. "Organic chlorine and chloride in soil /." Linköping : Univ, 2000. http://www.bibl.liu.se/liupubl/disp/disp2000/arts210s.htm.

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Ellenberger, Christine Spada. "Water Quality Impacts of Pure Chlorine Dioxide Pretreatment at the Roanoke County (Virginia) Water Treatment Plant." Thesis, Virginia Tech, 1999. http://hdl.handle.net/10919/30807.

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Chlorine dioxide (ClO₂) was included in the Spring Hollow Water Treatment Plant (Roanoke County, Virginia) to oxidize manganese and iron, prevent tastes and odors, and avoid the formation of excessive halogenated disinfection by-products. A state-of-the-art, gas:solid ClO₂ generation system manufactured by CDG Technology, Inc. was installed at the plant and is the first full-scale use of this technology in the world. The ClO₂ generator produces a feed stream free of chlorine, chlorite ion (ClO₂⁻), and chlorate ion (ClO₃⁻), resulting in lower by-product concentrations in the treatment system The objectives of this project were to study ClO₂ persistence and by-product concentrations throughout the treatment plant and distribution system and to evaluate granular activated carbon (GAC) columns for removing ClO₂⁻ from the finished water. The ClO₂ dosages applied during this study were relatively low (<0.75 mg/L), and, as a result, ClO₂⁻ concentrations never approached the maximum contaminant level (MCL) (1.0 mg/L). Likewise, the plant effluent ClO₂ concentration never approached the maximum residual disinfectant level (MRDL) (0.80 mg/L), but concentrations as high as 0.15 mg/L reformed in the distribution system by ClO₂⁻ reaction with chlorine. Chlorate ion was monitored despite the fact that no ClO₃⁻ MCL has been proposed, and concentrations were quite low (never greater than 0.10 mg/L) throughout the treatment plant and in the distribution system. The reasons for the low concentrations are that ClO₃⁻ is not produced by the gas-solid generator used at the facility and ClO₂⁻ concentrations in the clearwell prior to chlorination were uniformly low. The average ClO₂⁻ reduction upon passage of treated water through the GAC contactor was approximately 64 percent, but the GAC effectiveness was declining over the six-month study period. Apparently, GAC effectiveness, as shown by others, is short-lived, and if higher ClO₂ dosages are ever applied at the Roanoke County facility, the ClO₂⁻ concentrations will have to be reduced by either ferrous coagulants or reduced-sulfur compounds. Regenerated ClO₂ concentrations in the distribution system were below 0.2 mg/L, but concentrations as low as 0.03 mg/L were found at homes of customers who complained of odors. During this study, twelve complaints were received from eight customers, and each complainant had recently installed new carpeting, which has been shown to contribute volatile organics that react with ClO₂ to produce odors similar to kerosene and cat urine. While meeting the Cl₂ MCL likely will be no problem if the ClO₂ dose at the plant remains below 1.0 mg/L, the problem of offensive odors in the distribution system will likely continue as long as any ClO₂ is in the finished water when chlorine is present.
Master of Science
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4

Nguyen, Caroline Kimmy. "Interactions Between Copper and Chlorine Disinfectants: Chlorine Decay, Chloramine Decay and Copper Pitting." Thesis, Virginia Tech, 2005. http://hdl.handle.net/10919/35674.

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Interactions between copper and chlorine disinfectants were examined from the perspective of disinfectant decay and copper pitting corrosion. Sparingly soluble cupric hydroxide catalyzed the rapid decay of free chlorine, which in turn, led to production of less soluble and more crystalline phases of cupric hydroxide. The catalytic activity of the cupric hydroxide was retained over multiple cycles of chlorine dosing. Experiments with chloramine revealed that copper species could also trigger rapid loss of chloramine disinfectant. In copper pipes, loss of free chlorine and chloramine were both rapid during stagnation. Reactivity of the copper to the disinfectants was retained for weeks. Phosphate tended to decrease the reactivity between the copper pipe and chlorine disinfectants. A novel, inexpensive and real-time test to monitor copper pitting corrosion was developed. In a normal pipe, it is not possible to measure the electron flow or pitting current from the pit anode to the cathode. But a new method was developed that can form an active pit on the tip of a copper wire, which in turn, allows the pitting current to be measured. Preliminary experiments presented herein have proven that this technique has promise in at least one water condition known to cause pitting. The method also quickly predicted that high levels of orthophosphate could stop pitting attack in this water, whereas low levels would tend to worsen pitting. Future research should be conducted to examine this technique in greater detail.
Master of Science
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Arevalo, Jorge Miguel. "MODELING FREE CHLORINE AND CHLORAMINE DECAY IN A PILOT DISTRIBUTION SYSTEM." Doctoral diss., University of Central Florida, 2007. http://digital.library.ucf.edu/cdm/ref/collection/ETD/id/3815.

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The purpose of this study was to identify the effect that water quality, pipe material, pipe size, flow conditions and the use of corrosion inhibitors would have on the rate of free chlorine and chloramine decay in distribution systems. Empirical models were developed to predict the disinfectant residual concentration with time based on the parameters that affected it. Different water treatment processes were used to treat groundwater and surface water to obtain 7 types of finished waters with a wide range of water quality characteristics. The groundwater was treated either by conventional treatment by aeration (G1) or softening (G2) or high pressure reverse osmosis (RO) and the surface water was treated either by enhanced coagulation, ozonation and GAC filtration (CSF-O3-GAC or S1) or an integrated membrane system (CSF-NF or S2). The remaining two water types were obtained by treating a blend of G1, S1 and RO by softening (S2) and nanofiltration (G4). A pilot distribution systems (PDS) consisting of eighteen (18) lines was built using old pipes obtained from existing distribution system. The pipe materials used were polyvinyl chloride (PVC), lined cast iron (LCI), unlined cast iron (UCI) and galvanized steel (G). During the first stage of the study, the 7 types of water were blended and fed to the PDS to study the effect of feed water quality changes on PDS effluent water quality, and specifically disinfectant residual. Both free chlorine and chloramines were used as disinfectant and the PDSs were operated at hydraulic retention times (HRT) of 2 and 5 days. The PDSs were periodically tested for free and combined chlorine, organic content, temperature, pH, turbidity and color. The data obtained were used to develop separate models for free chlorine and chloramines. The best fit model was a first-order kinetic model with respect to initial disinfectant concentration that is dependent on the pipe material, pipe diameter and the organic content and temperature of the water. Turbidity, color and pH were found to be not significant for the range of values observed. The models contain two decay constants, the first constant (KB) accounts for the decay due to reaction in the bulk liquid and is affected by the organics and temperature while the second constant, KW, represents the reactions at the pipe wall and is affected by the temperature of the water and the pipe material and diameter. The rate of free chlorine and chloramine decay was found to be highly affected by the pipe material, the decay was faster in unlined metallic pipes (UCI and G) and slower in the synthetic (PVC) and lined pipes (LCI). The models showed that the rate of disinfectant residual loss increases with the increase of temperature or the organics in the water irrespective of pipe material. During the second part of the study, corrosion control inhibitors were added to a blend of S1, G1 and RO that fed all the hybrid PDSs. The inhibitors used were: orthophosphate, blended ortho-polyphosphate, zinc orthophosphate and sodium silicate. Three PDSs were used for each inhibitor type, for a total of 12 PDSs, to study the effect of low, medium and high dose on water quality. Two PDSs were used as control, fed with the blend without any inhibitor addition. The control PDSs were used to observe the effect of pH control on water quality and compare to the inhibitor use. One of the control PDSs (called PDS 13) had the pH adjusted to be equal to the saturation pH in relation to calcium carbonate precipitation (pHs) while the pH of the other control PDS (PDS 14) was adjusted to be 0.3 pH units above the pHs. The disinfectant used for this part of the study was chloramine and the flow rates were set to obtain a HRT of 2 days. The chloramine demand was the same for PDS 14 and all the PDSs receiving inhibitors. PDS 13 had a chloramine demand greater than any other PDS. The lowest chloramine demand was observed in PDS 12, which received silicate inhibitor at a dose of 12 mg/L, and presented the highest pH. The elevation of pH of the water seems to reduce the rate of decay of chloramines while the use of corrosion inhibitors did not have any effect. on the rate of chloramine decay. The PDS were monitored for chloramine residual, temperature, pH, phosphate, reactive silica, and organic content. Empirical models were developed for the dissipation of chloramine in the pilot distribution systems as a function of time, pipe material, pipe diameter and water quality. Terms accounting for the effect of pH and the type and dose of corrosion inhibitor were included in the model. The use of phosphate-based or silica-based corrosion inhibitors was found to have no effect on the rate of chloramine dissipation in any of the pipe materials. Only the increase of pH was found to decrease the rate of chloramine decay. The model to best describe the decay of chloramine in the pilot distribution systems was a first-order kinetic model containing separate rate constants for the bulk reactions, pH effect and the pipe wall reactions. The rate of chloramine decay was dependent on the material and diameter of the pipe, and the temperature, pH and organic content of the water. The rate of chloramine decay was low for PVC and LCI, and more elevated in UCI and G pipes. Small diameter pipes and higher temperatures increase the rate of chlorine decay irrespective of pipe material. Additional experiments were conducted to evaluate the effect of flow velocity on chloramine decay in a pilot distribution system (PDS) for different pipe materials and water qualities. The experiments were done using the single material lines and the flow velocity of the water was varied to obtain Reynolds' numbers from 50 to 8000. A subset of experiments included the addition of blended orthophosphate corrosion inhibitor (BOP) at a dose of 1.0 mg/L as P to evaluate the effect of the inhibitor on chloramine decay. The effect of Reynolds' number on the overall chloramine decay rate (K) and the wall decay rate constant (W) was assessed for PVC, LCI, UCI, and G pipes. PVC and LCI showed no change on the rate of chloramine decay at any flow velocity. UCI and G pipes showed a rapid increase on the wall decay rate under laminar conditions (Re < 500) followed by a more gradual increase under fully turbulent flow conditions (Re > 2000). The use of the BOP inhibitor did not have an effect on the rate of chloramine decay for any of the pipe materials studied. Linear correlations were developed to adjust the rate of chloramine decay at the pipe wall for UCI and G depending on the Reynolds' number.
Ph.D.
Department of Civil and Environmental Engineering
Engineering and Computer Science
Environmental Engineering PhD
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6

Simper, Jessica Mary. "Electrochemical characterization of aqueous chlorine and inorganic chloramine species." Thesis, Imperial College London, 2000. http://ethos.bl.uk/OrderDetails.do?uin=uk.bl.ethos.311946.

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Johnson, Jessica Mary. "Chlorine production from anhydrous hydrogen chloride in a molten salt electrolyte membrane cell." Diss., Georgia Institute of Technology, 2001. http://hdl.handle.net/1853/11246.

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Leahy, Joseph Gerard. "Inactivation of Giardia muris cysts by chlorine and chlorine dioxide." The Ohio State University, 1985. http://rave.ohiolink.edu/etdc/view?acc_num=osu1345744018.

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Burke, Michael A. "Kinetics of the chlorate-hydrogen peroxide reaction in the formation of chlorine dioxide." Thesis, Georgia Institute of Technology, 1993. http://hdl.handle.net/1853/11817.

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Courtis, Benjamin John. "Water quality chlorine management." Thesis, University of Birmingham, 2003. http://ethos.bl.uk/OrderDetails.do?uin=uk.bl.ethos.289743.

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Books on the topic "Chlorine"

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United States. Agency for Toxic Substances and Disease Registry. Division of Toxicology. Chlorine dioxide and chlorite. Atlanta, Ga.]: U.S. Dept. of Health and Human Services, Agency for Toxic Substances and Disease Registry, 2004.

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Institute, Chlorine, ed. The chlorine manual: Chlorine. 6th ed. Washington, D.C. (2001 L St., N.W., Suite 506, Washington 20036): Chlorine Institute, 1997.

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Tocci, Salvatore. Chlorine. New York: Children's Press, 2005.

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Blashfield, Jean F. Chlorine. Austin, Tex: Raintree Steck-Vaughn, 2002.

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United States. Agency for Toxic Substances and Disease Registry. and Syracuse Research Corporation, eds. Toxicological profile for chlorine dioxide and chlorite. [Atlanta, GA]: U.S. Dept. of Health and Human Services, Public Health Service, Agency for Toxic Substances and Disease Registry, 2004.

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B, Taylor Jessilynn, Wohlers David, Amata Richard, United States. Agency for Toxic Substances and Disease Registry., and Syracuse Research Corporation, eds. Draft toxicological profile for chlorine dioxide and chlorite. [Atlanta, Ga.]: Agency for Toxic Substances and Disease Registry, 2002.

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executive, Health and safety. Chlorine vaporisers. London: H.M.S.O., 1985.

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Tundo, Pietro, Liang-Nian He, Ekaterina Lokteva, and Claudio Mota, eds. Chemistry Beyond Chlorine. Cham: Springer International Publishing, 2016. http://dx.doi.org/10.1007/978-3-319-30073-3.

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S, Dobson, Cary R, World Health Organization, International Labour Organisation, United Nations Environment Programme, International Program on Chemical Safety., and Inter-Organization Programme for the Sound Management of Chemicals., eds. Chlorine dioxide (gas). Geneva: World Health Organization, 2002.

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San Francisco (Calif.). Board of Supervisors. Budget Analyst. Cost of chlorine versus sodium hypo-chlorite in sewage treatment. San Francisco, CA: Budget Analyst, 1994.

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Book chapters on the topic "Chlorine"

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Kendrick, Mark A. "Chlorine." In Encyclopedia of Earth Sciences Series, 1–3. Cham: Springer International Publishing, 2016. http://dx.doi.org/10.1007/978-3-319-39193-9_89-1.

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Kendrick, Mark A. "Chlorine." In Encyclopedia of Earth Sciences Series, 241–44. Cham: Springer International Publishing, 2018. http://dx.doi.org/10.1007/978-3-319-39312-4_89.

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Chaidez, Cristóbal, Nohelia Castro-del Campo, J. Basilio Heredia, Laura Contreras-Angulo, Gustavo González-Aguilar, and J. Fernando Ayala-Zavala. "Chlorine." In Decontamination of Fresh and Minimally Processed Produce, 121–33. Oxford, UK: Wiley-Blackwell, 2012. http://dx.doi.org/10.1002/9781118229187.ch7.

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Eggenkamp, Hans. "Chlorine." In The Geochemistry of Stable Chlorine and Bromine Isotopes, 15–19. Berlin, Heidelberg: Springer Berlin Heidelberg, 2014. http://dx.doi.org/10.1007/978-3-642-28506-6_2.

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de Mello Prado, Renato. "Chlorine." In Mineral nutrition of tropical plants, 243–50. Cham: Springer International Publishing, 2021. http://dx.doi.org/10.1007/978-3-030-71262-4_16.

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Lück, Erich, and Martin Jager. "Chlorine." In Antimicrobial Food Additives, 116–19. Berlin, Heidelberg: Springer Berlin Heidelberg, 1997. http://dx.doi.org/10.1007/978-3-642-59202-7_13.

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Bonifacie, Magali. "Chlorine Isotopes." In Encyclopedia of Earth Sciences Series, 1–5. Cham: Springer International Publishing, 2016. http://dx.doi.org/10.1007/978-3-319-39193-9_90-1.

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Bonifacie, Magali. "Chlorine Isotopes." In Encyclopedia of Earth Sciences Series, 244–48. Cham: Springer International Publishing, 2018. http://dx.doi.org/10.1007/978-3-319-39312-4_90.

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Sukhoruchkin, S. I., and Z. N. Soroko. "17-Chlorine." In Tables of Proton and α-Particle Resonance Parameters. Part 1, 534–84. Berlin, Heidelberg: Springer Berlin Heidelberg, 2004. http://dx.doi.org/10.1007/10730526_17.

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Gooch, Jan W. "Chlorine Retention." In Encyclopedic Dictionary of Polymers, 140–41. New York, NY: Springer New York, 2011. http://dx.doi.org/10.1007/978-1-4419-6247-8_2319.

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Conference papers on the topic "Chlorine"

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Melwani Daswani, Mohit, and Edwin S. Kite. "CHLORIDE DEPOSITS ON MARS: CHLORINE FROM THE SKY, OR CHLORINE FROM THE ROCKS?" In GSA Annual Meeting in Denver, Colorado, USA - 2016. Geological Society of America, 2016. http://dx.doi.org/10.1130/abs/2016am-285235.

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Themelis, Nickolas J. "Chlorine Sources, Sinks, and Impacts in WTE Power Plants." In 18th Annual North American Waste-to-Energy Conference. ASMEDC, 2010. http://dx.doi.org/10.1115/nawtec18-3577.

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The principal sources of chlorine in the MSW feed to WTE power plants are food wastes (e.g., wheat, green vegetables, melon, pineapple), yard wastes (leaves, grass, etc.), salt (NaCl), and chlorinated plastics (mostly polyvinyl chloride). Chlorine has important impacts on the WTE operation in terms of higher corrosion rate than in coal-fired power plants, formation of hydrochloric gas that must be controlled in the stack gas to less than the U.S. EPA standard (29 ppm by volume), and potential for formation of dioxins and furans. Past Columbia studies have shown that the chlorine content in MSW is in the order of 0.5%. In comparison, chlorine concentration in coal is about 0.1%; this results in much lower HCl concentration in the combustion gases and allows coal-fired power plants to be operated at higher superheater tube temperatures and thus higher thermal efficiencies. Most of the chlorine output from a WTE is in the fly ash collected in the fabric filter baghouse of the Air Pollution Control system. This study examined in detail the sources and sinks of chlorine in a WTE unit. It is concluded that on the average MSW contains about 0.5% chlorine, which results in hydrogen chloride concentration in the WTE combustion gases of up to 600 parts per million by volume. About 45% of the chlorine content in MSW derives from chlorinated plastics, mainly polyvinyl chloride (PVC), and 55% from salt (NaCl) and chlorine-containing food and yard wastes. An estimated 97–98% of the chlorine input is converted to calcium chloride in the dry scrubber of the Air Pollution Control (APC) system and captured in the fly ash collected in the baghouse; the remainder is in the stack gas at a concentration that is one half of the U.S. EPA standard. Reducing the input of PVC in the MSW stream would have no effect on dioxin formation but would reduce the corrosion rate in the WTE boiler.
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Marshall, Mark, Joseph Messinger, and Helen Leung. "CHLORINE NUCLEAR QUADRUPOLE HYPERFINE STRUCTURE IN THE VINYL CHLORIDE-HYDROGEN CHLORIDE COMPLEX." In 70th International Symposium on Molecular Spectroscopy. Urbana, Illinois: University of Illinois at Urbana-Champaign, 2015. http://dx.doi.org/10.15278/isms.2015.wj06.

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Uusitalo, M., P. Vuoristo, T. Mäntylä, L.-M. Berger, and R. Backman. "The Effect of Chlorine on Degradation Mechanisms of Thermal Sprayed Coatings at Elevated Temperatures." In ITSC2003, edited by Basil R. Marple and Christian Moreau. ASM International, 2003. http://dx.doi.org/10.31399/asm.cp.itsc2003p0485.

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Abstract The significance of biofuels and the other chlorine-containing fuels in energy production is in strong increase. Serious erosion-corrosion problems in boilers combusting fuels with high chlorine-content have been detected frequently. A series of erosion-corrosion and corrosion tests were performed on thermal sprayed coatings and coating precursors in chlorine-containing environments in order to evaluate possibilities to utilize thermal sprayed coatings for erosion-corrosion protection in boilers combusting chlorine-containing fuels. A series of hot erosion and erosion-corrosion tests were performed on thermal sprayed coatings at elevated temperatures with and without chlorine. Carbide-containing HVOF coatings performed well in hot erosion tests, but they were completely destroyed in the presence of chlorine due to rapid oxidation of carbides. Metallic HVOF coatings with high chromium content performed well in both conditions. Iron-based arc-sprayed coatings with unhomogeneous microstructure suffered more hot erosion and erosion-corrosion damages than metallic HVOF coatings. The E-C (erosion-corrosion) resistance of carbide-containing coatings in the presence of chlorides was worse than expected. A series of oxidation tests were performed on various carbides in order to elucidate the effect of chlorine on high temperature oxidation behavior of carbides. TGA and isothermal oxidation tests proved that gaseous chlorine-containing species and also solid chlorides have a detrimental effect on oxidation resistance of tested carbides.
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Chapman, K., K. Kirollos, F. Saunders, and M. Stryker. "237. Monitoring Chlorine Dioxide Without a Chlorine Interference." In AIHce 2003. AIHA, 2003. http://dx.doi.org/10.3320/1.2758009.

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Chang, Kui, Jinliang Gao, Yixing Yuan, and Wenyan Wu. "Water Distribution Network Residual Chlorine Modeling Based on the Synergy of Chlorine and Chlorine Dioxide." In 12th Annual Conference on Water Distribution Systems Analysis (WDSA). Reston, VA: American Society of Civil Engineers, 2011. http://dx.doi.org/10.1061/41203(425)64.

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Rahmani, B., T. Smaili, B. Saghi, S. Bhosle, and G. Zissis. "Effect of chlorine on irradiance of excilamp kypton chlorine." In 2010 IEEE 37th International Conference on Plasma Sciences (ICOPS). IEEE, 2010. http://dx.doi.org/10.1109/plasma.2010.5533947.

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Liu, Xi, Hai-Zhen Wei, Shao-Yong Jiang, Anthony E. Williams-Jones, and Jian-Jun Lu. "Pressure-Induced Chlorine Isotope Fractionation Among Chlorine- Bearing Minerals." In Goldschmidt2020. Geochemical Society, 2020. http://dx.doi.org/10.46427/gold2020.1610.

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Agrinier, Pierre, Magali Bonifacie, Gerard Bardoux, Thomas Giunta, Francis Lucazeau, and Magali Ader. "Chlorine isotopes from chlorides in sedimentary fluids of the ocean crust and the Cl budget of Earth surface Chlorine." In Goldschmidt2021. France: European Association of Geochemistry, 2021. http://dx.doi.org/10.7185/gold2021.4214.

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Wei, Hai-Zhen, Anthony Williams-Jones, Shao-Yong Jiang, Xi Liu, and Jianjun Lu. "Chlorine isotope fractionation during metal-chloride complexation: Implications for metallogenic processes." In Goldschmidt2022. France: European Association of Geochemistry, 2022. http://dx.doi.org/10.46427/gold2022.10685.

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Reports on the topic "Chlorine"

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Shul, R. J., R. D. Briggs, S. J. Pearton, C. B. Vartuli, C. R. Abernathy, J. W. Lee, C. Constantine, and C. Baratt. Chlorine-based plasma etching of GaN. Office of Scientific and Technical Information (OSTI), February 1997. http://dx.doi.org/10.2172/432987.

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Wilde, E. W. Chlorine demand of Savannah River water. Office of Scientific and Technical Information (OSTI), January 1989. http://dx.doi.org/10.2172/5695222.

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Ludowise, P. D. Ultrafast measurements of chlorine dioxide photochemistry. Office of Scientific and Technical Information (OSTI), August 1997. http://dx.doi.org/10.2172/658167.

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Istas, Laurence. Chlorine Distribution in the Idaho Batholith. Portland State University Library, January 2000. http://dx.doi.org/10.15760/etd.2607.

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Huber, Zachary, Michael Powell, Tyler Schlieder, Juan Cervantes, James Davis, Parker Okabe, Riane Stene, Tatiana Levitskaia, and Bruce McNamara. Chlorine Isotope Separations using Thermal Diffusion. Office of Scientific and Technical Information (OSTI), January 2024. http://dx.doi.org/10.2172/2339481.

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Haas, P. A., D. D. Lee, and J. C. Mailen. Reaction of uranium oxides with chlorine and carbon or carbon monoxide to prepare uranium chlorides. Office of Scientific and Technical Information (OSTI), November 1991. http://dx.doi.org/10.2172/10155443.

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STEVENS, G. M. Chlorine Containment System Natural Phenomena Hazards Analysis. Office of Scientific and Technical Information (OSTI), February 2001. http://dx.doi.org/10.2172/806025.

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McNallan, M., S. Danyluk, and J. E. Indacochea. High temperature corrosion during use of chlorine. Office of Scientific and Technical Information (OSTI), January 1992. http://dx.doi.org/10.2172/6970166.

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Ahuja, Amrita, Douglas B. Marshall, Celine Gratadour, Vivian Hoffmann, Pamela Jakiela, Renaud Lapeyre, Clair Null, Olga Rostapshova, and Ryan Sheely. Chlorine Dispensers in Kenya: Scaling for Results. International Initiative for Impact Evaluation, 2015. http://dx.doi.org/10.23846/ow1029.

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Muchmore, C. B. Thermal treatment for chlorine removal from coal. Office of Scientific and Technical Information (OSTI), January 1991. http://dx.doi.org/10.2172/5877887.

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