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: 9 June 2025

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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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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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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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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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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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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.<br>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.<br>Master of Science
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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.<br>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.<br>Ph.D.<br>Department of Civil and Environmental Engineering<br>Engineering and Computer Science<br>Environmental Engineering PhD
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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., та Z. N. Soroko. "17-Chlorine". У 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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Spiegel, M., and H. J. Grabke. "Chlorine Induced Corrosion of Steels in Fossil Fuel Power Plants." In CORROSION 1998, 1–19. NACE International, 1998. https://doi.org/10.5006/c1998-98178.

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Abstract The corrosion of steels in power plants (coal combustion, waste incineration) is mainly due to condensed chlorides in the ash deposited on the boiler tubes. These chlorides are stabilized by HCl in the combustion gas. In the case of coal as a fuel, chlorine is present as chloride minerals in the raw material which is converted to HCl during the combustion process. Corrosion of steels in chlorine containing environments occurs by the ‘active oxidation’ mechanism, which is a self - sustaining accelerated oxidation process, catalysed by chlorine. This study shows that solid chlorides react with the oxide scale of the steels to form chlorine, which initiates ‘active oxidation’. In order to prevent chlorine induced corrosion, the deposition of chlorides on the tubes within the coal ash must be avoided. This is possible by the presence of SO2, which is present in the combustion gas, converting the chlorides to sulfates in the gas phase. The paper presents an example of a failure case in a coal fired plant in Germany. In this plant, chlorine induced corrosion was observed after effective removal of SO2 by additions of CaO. From thermodynamic calculations it can be shown that a certain amount of SO2 is necessary in order to avoid deposition of chlorides and to prevent corrosion.
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McNallan, M. J., and Y. S. Park. "High Temperature Corrosion of Alloys and Ceramics by Alkali Chlorides." In CORROSION 1996, 1–10. NACE International, 1996. https://doi.org/10.5006/c1996-96441.

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Abstract Alkali chlorides are well known to cause accelerated corrosion. At elevated temperatures, the presence of alkali chlorides as vapors or molten deposits can cause accelerated attack of either high temperature metal alloys or ceramics. The mechanism of attack is different in the two cases, however, with the chlorine component being most aggressive for corrosion of metals and the alkali being most aggressive for corrosion of ceramics. The reaction of the alkali chloride with the oxide scale on metals releases chlorine which causes accelerated corrosion. The corrosion rate can be reduced by absorbing this chlorine. For ceramics, the alkali oxide species produced by such reactions is most damaging and the rate of corrosion can be reduced by adding chlorine to the system.
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McNallan, Michael. "High Temperature Corrosion of Silicon Based Ceramics in Environments Containing Halogens and Alkali Halides." In CORROSION 1999, 1–14. NACE International, 1999. https://doi.org/10.5006/c1999-99275.

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Abstract Silicon carbide and other silicon-based ceramics obtain their oxidation resistance by the formation of protective silica films in oxygen containing environments. In the presence of chlorine or alkali chlorides, this film may not form, or may be unprotective, so that accelerated oxidation occurs. Chlorine and alkali halides may contribute to accelerated oxidation via three possible mechanisms. Active oxidation occurs at relatively low temperatures and high ratios of chlorine to oxygen, and is characterized by simultaneous formation of silicon chlorides and non-protective oxides. Silica film disruption occurs at higher temperatures when volatile chlorides form at the interface between SiC and the SiO2 scale, and cause bubbles to form in the film. Alkali fluxing occurs in the presence of alkali chloride vapors. In alkali fluxing, a low melting glass is formed by the reaction between the alkali vapor species and silica rather than by reactions with chlorine itself.
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Forsén, Olof, Jari Aromaa, and Markku Tavi. "The Effect of Oxygen and Chlorine Evolution on the Corrosion of Ruthenium Oxide Anodes." In CORROSION 1996, 1–15. NACE International, 1996. https://doi.org/10.5006/c1996-96564.

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Abstract The electrochemical behaviour of RuO2-based anodes has been investigated in 0.5 M Na2SO4 and 6-300 g/l NaCl solutions with galvanostatic polarization curves. Chlorine gas is the primary reaction product when electrolyzing chloride solutions but the corrosion of the anodes depends on the amount of oxygen evolution. The solution conditions, where oxygen evolution is significant were estimated from polarization curves. The decrease of solution pH had a stronger effect on the suppressing of oxygen evolution than the increase of NaCl concentration. Oxygen evolution was significant at pH&amp;gt;2 in sodium chloride solutions 0-300 g/l NaCl. At pH=2 no significant oxygen evolution was found in 35-300 g/l NaCl solutions. Below pH=5 chlorine evolution is the main reaction. Otherwise the current density has to be high enough to increase the anode potential to a level, where chlorine evolution may begin. In 6-35 g/l NaCl solutions with pH=5-6 at potentials E≤ 1050 mV the only reaction was oxygen evolution. At potentials E ≥ 1150 mV chlorine evolution was again the main reaction. When reactions proceed simultaneously, chlorine evolution will dominate if chloride ion concentration is high enough.
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Havn, Torfinn. "Corrosion of Engineering Materials in Seawater, Freshwater and 3.5% NaCl Solution with Additions of Chlorine and Chlorite." In CORROSION 2007, 1–15. NACE International, 2007. https://doi.org/10.5006/c2007-07260.

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Abstract Sea water systems on many offshore platforms are treated with small amounts of chlorine to prevent marine growth inside piping and equipment. It is well known that small additions of chlorine increase the oxidation strength (corrosion potential) of Ti and stainless steels in sea water. Regarding Al, CuNi and carbon steel, it is difficult to find the effect of chlorine on these materials described in the literature. Therefore, during laboratory tests the corrosion potentials of engineering materials under influence of additions of chlorine and chlorite were measured. The investigated engineering materials were an Al-alloy, 316L stainless steel, 6Mo stainless steel, 3 grades of duplex stainless steels, CuNi, Ti and carbon steel. A systematic test program for these engineering materials was carried out with chlorine and chlorite rest levels of 0.5 ppm, 5 ppm, 50 ppm and 500 ppm. The motivation for the tests with chlorite, originated from a project on an offshore platform containing produced water with high amounts of H2S. The H2S was decided to be removed by adding sodium-chlorite to the water. The sodium-chlorite dissolves to sodium and chlorite prior to the H2S removal reaction. The H2S removal reaction is based on chlorite and water reacting with H2S and forming sulfate and H-ions. After treating the water with sodium-chlorite, the water was found to be free of H2S. However, it turned out that the water became very corrosive, probably due to high rest levels of chlorite. Pumps and equipment suffered from heavy corrosion, especially an Al-alloy. The literature is very limited with respect to data on corrosivity due to chlorite additions in sea water. Based on available data on critical pitting and crevice potentials for the passive materials, and overvoltage curves for the active materials, it is possible to predict how the “chlorination” will influence on the resistance against corrosion.
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Krause, H. H. "Chlorine Corrosion in Waste Incineration." In CORROSION 1987, 1–11. NACE International, 1987. https://doi.org/10.5006/c1987-87401.

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Abstract Incineration of municipal or industrial wastes can result in severe corrosion of boiler tubes in waste-to-energy systems as a result of the chlorine in the waste. Corrosion probe studies conducted in such boilers showed that for carbon and low alloy steels the wastage rates are functions of chlorine concentration, metal temperature, and flue gas temperature. Breakaway corrosion occurred at a metal temperature of 800 F (427 C) when the flue gas temperature exceeded 1500 F (843 C). Corrosion rates of stainless steels and alloy 825 proved to be an order of magnitude lower than that of carbon steel and independent of chlorine concentration at low levels. The chlorine content of municipal refuse was found to be a more important factor in corrosion than the refuse processing. Industrial wastes of low ash content were less corrosive than comparable municipal refuse of high ash content. Metal chlorides were identified that can form eutectic mixtures having low melting points. Such mixtures are a source of molten salt corrosion that can be more severe than attack by HCl and chlorine gases.
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Otsuka, N., Y. Nishiyama, and T. Hosoda. "Thermodynamic Equilibrium Calculations of Deposits on Superheater Tubes in Waste Incinerators." In CORROSION 2000, 1–14. NACE International, 2000. https://doi.org/10.5006/c2000-00229.

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Abstract Thermodynamic equilibrium calculations were conducted to obtain flue-gas composition and molar amount of volatile condensate deposits on superheater tubes upon combustion of municipal solid waste. Effects of sodium, potassium, chlorine, and sulfur involved in municipal solid waste on deposit chemistry were examined. Possible influence of flue-gas temperature and metal temperature on corrosion were investigated as well. Calculated flue-gas composition agreed relatively well with the flue gas composition in real incinerators. Equilibrium calculation showed that vapor condensate deposits on the 550°C tube surface from 650 and 750°C flue gases consisted predominantly of sodium and potassium chlorides. Sulfate precipitation from hot gases was slight. The amount of molecular chloride precipitates was greater for flue gas of 750°C than of 650°C. For the same gas and metal temperature, 0.1-0.5wt.% chlorine in municipal solid waste did not affect the tube deposit chemistry drastically. It is suggested that high chlorine, low sulfur, moderate amount of sodium/potassium, and trace inclusion of heavy metals such as lead and zinc in waste are the principal factors in the fuel chemistry which cause severe corrosion attack of superheater tubes in waste incinerators.
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Kamaraj, Abinaya, Johann Wilhelm Erning, Stefan Reimann, and Alfons Ahrens. "Susceptibility of 304 Stainless Steel to Crevice Corrosion in Electrochemically Active Fluids." In CORROSION 2019, 1–13. NACE International, 2019. https://doi.org/10.5006/c2019-12868.

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Abstract The generation of active disinfectants by electrochemical processes gains market share due to the lack of need for transportation and storage of dangerous goods as well as the ease of operation. Usually, the process involves the use of specific electrodes for electrolysis of water to produce active chlorine species, sometimes supported by the addition of chlorides to the process water. Thus, the influence on the corrosion behavior can vary widely. The susceptibility of AISI 304 stainless steel to crevice corrosion on the effect of contact with electrochemically active fluids was investigated using exposure and stepwise potentiostatic polarisation. Crevice materials made up of 304 SS and Polyether ether ketone (PEEK) forming two kinds of crevices including 304 SS-to-PEEK and 304 SS-to-304 SS were tested, and results indicate that 304 SS specimen is strongly susceptible to crevice corrosion in 304 SS crevice former assembly. The combination of the influence of oxidant and chloride concentration were examined in detail, and results indicate a strong influence of free chlorine and chloride concentration to crevice corrosion. The corroded surface morphology was investigated using scanning electron microscope(SEM), Energy Dispersive X-ray (EDX) and Confocal microscope.
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Thongtem, S., M. J. McNallan, and G. Y. Lai. "Corrosion of Superalloys by Volatilization and Internal Penetration in High Temperature Chlorine Contaminated Environments." In CORROSION 1986, 1–11. NACE International, 1986. https://doi.org/10.5006/c1986-86372.

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Chlorine contamination has been encountered in more high temperature environments as increasing energy costs have led to the use of lower quality fuels and the application of waste heat recuperation technology to a wider variety of industrial and metallurgical processes1. The presence of chlorine generally accelerates the corrosion rates of materials, and many materials which are usually considered to be corrosion resistant can be attacked very rapidly in chlorine containing atmospheres. 2-5 Chlorine can accelerate corrosion by promoting the formation of a liquid salt deposit, but can also produce substantial increases in the corrosion rate even when it is present only in the gas phase.6 Depending on the system in which the chlorine is encountered, it may be in the form of HCl, Cl2, or the vapors of chloride salts. The form of the chlorine and the partial pressure of oxygen prevailing in the corrosive atmosphere have significant effects on the corrosion behavior. In this study, the effect of a small amount of Cl2 in an oxidizing environment on the corrosion behavior of superalloys has been investigated over the temperature range 700°C to 850°C.
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Hasan, S. Khalid, and M. Mobin. "Hot Corrosion Behaviour of Protective Oxide Scales with Sodium Chloride in Chlorine Gas Environment." In CORROSION 2013, 1–17. NACE International, 2013. https://doi.org/10.5006/c2013-02125.

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Abstract Sodium chloride (NaCl) is one of the prominent hot corrosion inducing constituents of salt deposits that accumulate on the alloy surface in the field. In a marine environment NaCl is ingested into a gas turbine as an aerosol of sea salt along with intake air. At high temperatures, conventional alloys are severely attacked by NaCl and protective oxide scales like Cr2O3, Al2O3 and NiO invariably deteriorate. This paper deals with the high temperature reaction kinetics of such metal oxides with NaCl in a Cl2 gas environment at atmospheric pressure. The kinetics of the reactions between NaCl and metal oxides were studied by monitoring them by thermo-gravimetric analysis. Reaction products were identified by XRD analysis and SEM studies. Water soluble metal species in the mixture were estimated with the help of atomic absorption spectroscopy and pH of aqueous solution was taken into account to establish the reaction mechanism. The result showed that the mixed oxide of the type (Na2O.M2Ox) and metal chlorides were the usual reaction products. Water soluble reaction products indicated the presence of metal oxy anions (CrO2-; AlO2-; and NiO2-;) in the mixture. The aqueous solution of NaCl and Al2O3 in the system was found basic whereas for NiO and Cr2O3 it was acidic.
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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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