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Journal articles on the topic 'Sulphur Dioxide Oxidation Reaction'

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Published: 4 June 2021

Last updated: 1 February 2022

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1

Pyshyev, Serhiy, Michael Bratychak, Vasyl Hayvanovych, Pavlo Paniv, and Witold Wacławek. "Water Effect on Oxidative Desulphurization Process of Straight-Run Kerosene Fraction / Wpływ Wody Na Utleniający Proces Odsiarczania Frakcji Nafty." Ecological Chemistry and Engineering S 20, no. 1 (March 1, 2013): 55–68. http://dx.doi.org/10.2478/eces-2013-0004.

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Abstract Sulphur dioxide obtained during fuels burning in combustion engines is one of the main pollutants. In diesel oils and gasolines the sulphur content must be 5-10 ppm and in jet fuels - 300-3000 ppm. However the production of hydrofined jet fuel is problematic. The reason is deterioration of fuel stability and antioxygenic properties. The oxidative desulphurization of straight-run kerosene was investigated. This method combines oxidation by atmospheric oxygen of sulphur compounds under increased temperature and pressure in the presence of water in the reaction medium, and removal of oxidized sulphur compounds from the oxidation-treated fuel via rectification. It was showed that water partially extracts from the hydrocarbon medium acidic compounds, formed in the beginning stage of oxidation, dissociation of which leads to the formation in water acidic medium. As a result, a pathway of the hydroperoxides decomposition partially changes from the formation of carbonic acids and oxyacids to the formation of alcohols, phenols and alkylphenols, which displayed an inhibitory effect in hydrocarbon oxidation. It was assumed that an inhibitory effect of water, in addition to the creation reverse micelles with peroxides and complexes with free radicals, caused by oxidation products created in the beginning stage of oxidation. The effect of water/kerosene ratio on the oxidative desulphurization of straight-run kerosene fraction has been examined. It was found that water improves process selectivity with insignificant influence on the degree of sulphur recovery. The optimum value of water/kerosene ratio for the fuel containing 0.15% mass of sulphuric compounds has been determined.

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2

Rakitskaya, Tatyana L., Tatyana A. Kiose, E. V. Kameneva, and V. Ya Volkova. "Natural Clinoptilolite Based Solid-State Compositions for Low-Temperature Air Purification from Sulphur Dioxide." Solid State Phenomena 230 (June 2015): 291–96. http://dx.doi.org/10.4028/www.scientific.net/ssp.230.291.

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Natural clinoptilolite (N-CLI) and N-CLI based solid-state compositions containing copper(II) chloride and halide ions (X- = Cl-, Br- or I-) were investigated by X‑ray diffraction phase analysis, IR spectroscopy, thermogravimetry, water vapour adsorption, and pH‑metry. After that, they were tested in the reaction of low-temperature sulphur dioxide oxidation with air oxygen. It has been found that N-CLI has no protective properties in respect of sulphur dioxide whereas CuCl2‑KX/N-CLI compositions have the significant protective activity in the process of air purification from sulphur dioxide increasing in the order Cl- < Br- < I-.

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3

Zaker, Mohammad Reza, Clémence Fauteux-Lefebvre, and Jules Thibault. "Modelling and Multi-Objective Optimization of the Sulphur Dioxide Oxidation Process." Processes 9, no. 6 (June 20, 2021): 1072. http://dx.doi.org/10.3390/pr9061072.

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Sulphuric acid (H2SO4) is one of the most produced chemicals in the world. The critical step of the sulphuric acid production is the oxidation of sulphur dioxide (SO2) to sulphur trioxide (SO3) which takes place in a multi catalytic bed reactor. In this study, a representative kinetic rate equation was rigorously selected to develop a mathematical model to perform the multi-objective optimization (MOO) of the reactor. The objectives of the MOO were the SO2 conversion, SO3 productivity, and catalyst weight, whereas the decisions variables were the inlet temperature and the length of each catalytic bed. MOO studies were performed for various design scenarios involving a variable number of catalytic beds and different reactor configurations. The MOO process was mainly comprised of two steps: (1) the determination of Pareto domain via the determination a large number of non-dominated solutions, and (2) the ranking of the Pareto-optimal solutions based on preferences of a decision maker. Results show that a reactor comprised of four catalytic beds with an intermediate absorption column provides higher SO2 conversion, marginally superior to four catalytic beds without an intermediate SO3 absorption column. Both scenarios are close to the ideal optimum, where the reactor temperature would be adjusted to always be at the maximum reaction rate. Results clearly highlight the compromise existing between conversion, productivity and catalyst weight.

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4

Klauson, Deniss, Jana Pilnik-Sudareva, Natalja Pronina, Olga Budarnaja, Marina Krichevskaya, Aleksandr Käkinen, Katre Juganson, and Sergei Preis. "Aqueous photocatalytic oxidation of prednisolone." Open Chemistry 11, no. 10 (October 1, 2013): 1620–33. http://dx.doi.org/10.2478/s11532-013-0290-8.

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AbstractThe research into the aqueous photocatalytic oxidation of the anti-inflammatory drug prednisolone was undertaken with P25 titanium dioxide (Evonik) and visible light-sensitive sol-gel synthesized titania-based photocatalysts containing carbon, sulphur, and iron. Possible prednisolone photocatalytic oxidation reaction pathways were proposed based on a number of oxidation by-products determined in the present study. The prednisolone adsorption properties, effects of initial prednisolone concentration, pH, usual wastewater matrix admixtures, like carbamide and sucrose, were studied. The nontoxicity of doped catalysts towards Tetrahymena thermophila, a ciliate protozoa present in the activated sludge, indicated their lower oxidative ability compared to P25, but also implied their potential application in pre-treatment of toxic hazardous materials under VIS or solar radiation before the biological degradation stage.

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5

Hoyle, C. R., C. Fuchs, E. Järvinen, H. Saathoff, A. Dias, I. El Haddad, M. Gysel, et al. "Aqueous phase oxidation of sulphur dioxide by ozone in cloud droplets." Atmospheric Chemistry and Physics Discussions 15, no. 23 (December 1, 2015): 33843–96. http://dx.doi.org/10.5194/acpd-15-33843-2015.

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Abstract. The growth of aerosol due to the aqueous phase oxidation of SO2 by O3 was measured in laboratory generated clouds created in the CLOUD chamber at CERN. Experiments were performed at 10 and −10 °C, on acidic (sulphuric acid) and on partially to fully neutralised (ammonium sulphate) seed aerosol. Clouds were generated by performing an adiabatic expansion – pressurising the chamber to 220 hPa above atmospheric pressure, and then rapidly releasing the excess pressure, resulting in a cooling, condensation of water on the aerosol and a cloud lifetime of approximately 6 min. A model was developed to compare the observed aerosol growth with that predicted by oxidation rates previously measured in bulk solutions. The model captured the measured aerosol growth very well for experiments performed at 10 and −10 °C, indicating that, in contrast to some previous studies, the oxidation rates of SO2 in a dispersed aqueous system are well represented by accepted rates, based on bulk measurements. To the best of our knowledge, these are the first laboratory based measurements of aqueous phase oxidation in a dispersed, super-cooled population of droplets. The measurements are therefore important in confirming that the extrapolation of currently accepted reaction rates to temperatures below 0 °C is correct.

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6

Kotzias, D., K. Fytianos, and F. Geiss. "Reaction of monoterpenes with ozone, sulphur dioxide and nitrogen dioxide—gas-phase oxidation of SO2 and formation of sulphuric acid." Atmospheric Environment. Part A. General Topics 24, no. 8 (January 1990): 2127–32. http://dx.doi.org/10.1016/0960-1686(90)90246-j.

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7

Hoyle, C. R., C. Fuchs, E. Järvinen, H. Saathoff, A. Dias, I. El Haddad, M. Gysel, et al. "Aqueous phase oxidation of sulphur dioxide by ozone in cloud droplets." Atmospheric Chemistry and Physics 16, no. 3 (February 12, 2016): 1693–712. http://dx.doi.org/10.5194/acp-16-1693-2016.

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Abstract. The growth of aerosol due to the aqueous phase oxidation of sulfur dioxide by ozone was measured in laboratory-generated clouds created in the Cosmics Leaving OUtdoor Droplets (CLOUD) chamber at the European Organization for Nuclear Research (CERN). Experiments were performed at 10 and −10 °C, on acidic (sulfuric acid) and on partially to fully neutralised (ammonium sulfate) seed aerosol. Clouds were generated by performing an adiabatic expansion – pressurising the chamber to 220 hPa above atmospheric pressure, and then rapidly releasing the excess pressure, resulting in a cooling, condensation of water on the aerosol and a cloud lifetime of approximately 6 min. A model was developed to compare the observed aerosol growth with that predicted using oxidation rate constants previously measured in bulk solutions. The model captured the measured aerosol growth very well for experiments performed at 10 and −10 °C, indicating that, in contrast to some previous studies, the oxidation rates of SO2 in a dispersed aqueous system can be well represented by using accepted rate constants, based on bulk measurements. To the best of our knowledge, these are the first laboratory-based measurements of aqueous phase oxidation in a dispersed, super-cooled population of droplets. The measurements are therefore important in confirming that the extrapolation of currently accepted reaction rate constants to temperatures below 0 °C is correct.

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8

Yemelyanova, V. S., T. V. Shakieva, Zh K. Kairbekov, E. M. Shakiev, and B. B. Baizhomartov. "Low-Temperature Catalytic Clearing of Gases of Thermal Power Station from Harmful Impurity in the Presence of the Cobalt Complexes Fixed on a Polymeric Matrix." Advanced Materials Research 807-809 (September 2013): 1586–92. http://dx.doi.org/10.4028/www.scientific.net/amr.807-809.1586.

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The results of optimization of catalysts for gases clearing from sulfur dioxide using processes of oxidation are presented in this work. The researches carried out with the help of modern methods: kinetic, IR-, UV-spectrophotometric, viscometry, LG-chromatography, redox-potentiometric. It is shown, that developed complexes of transitive metals immobilized on a polymeric matrix are highly effective and stable catalysts for the sulphur dioxide oxidation processes. By the example of cobalt compounds the reactions kinetic investigated in details, the kinetic equation is received, allowing to optimize process of gases clearing from sulfur dioxide, kinetic and thermodynamic parameters of process are calculated.

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9

Lelieveld, J., G. –J Roelofs, L. Ganzeveld, J. Feichter, and H. Rodhe. "Terrestrial sources and distribution of atmospheric sulphur." Philosophical Transactions of the Royal Society of London. Series B: Biological Sciences 352, no. 1350 (February 28, 1997): 149–58. http://dx.doi.org/10.1098/rstb.1997.0010.

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The general circulation model ECHAM has been coupled to a chemistry and sulphur cycle model to study the impact of terrestrial, i.e. mostly anthropogenic sulphur dioxide (SO 2 ), sources on global distributions of sulphur species in the atmosphere. We briefly address currently available source inventories. It appears that global estimates of natural emissions are associated with uncertainties up to a factor of 2, while anthropogenic emissions have uncertainty ranges of about +/− 30 per cent. Further, some recent improvements in the model descriptions of multiphase chemistry and deposition processes are presented. Dry deposition is modelled consistently with meteorological processes and surface properties. The results indicate that surface removal of SO 2 is less efficient than previously assumed, and that the SO 2 lifetime is thus longer. Coupling of the photochemistry and sulphur chemistry schemes in the model improves the treatment of multiphase processes such as oxidant (hydrogen peroxide) supply in aqueous phase SO 2 oxidation. The results suggest that SO 2 oxidation by ozone (O 3 ) in the aqueous phase is more important than indicated in earlier work. However, it appears that we still overestimate atmospheric SO 2 concentrations near the surface in the relatively polluted Northern Hemisphere. On the other hand, we somewhat underestimate sulphate levels in these regions, which suggests that additional heterogeneous reaction mechanisms, e.g. on aerosols, enhance SO 2 oxidation.

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10

Yemelyanova, V. S., H. Kurokawa, B. T. Dossumova, Zh K. Kairbekov, T. V. Shakiyeva, Zh K. Myltykbaeva, U. N. Dzhatkambayeva, E. M. Shakiyev, and E. Zh Aybasov. "Using of Microspheres of Power Ashes for Gases Cleaning from Sulphur Dioxide." Advanced Materials Research 1079-1080 (December 2014): 110–17. http://dx.doi.org/10.4028/www.scientific.net/amr.1079-1080.110.

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The composition and structure of the microspheric aluminosilicates of Combined Heating and Power Plants (CHРP) ashes is studied with the help of modern physical-chemical methods (XRD, scanning electron microscopy, BET, elemental and chemical analysis). The activity of microsphere-based catalysts for the reaction of Na2SO3 oxidation by oxygen is also studied by kinetic and potentiometric methods. By means of EPR and Möessbauer spectroscopy it is concluded that iron ions into the composition of cenospheres exist in two states – Fe3+ and Fe2+, thus, the iron (III) is in the form of solitary ions in an aluminosilicate matrix in the range of the iron content 3-4 mass %.

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11

Hewitt, C. Nicholas, and Brian Davison. "Field measurements of dimethyl sulphide and its oxidation products in the atmosphere." Philosophical Transactions of the Royal Society of London. Series B: Biological Sciences 352, no. 1350 (February 28, 1997): 183–89. http://dx.doi.org/10.1098/rstb.1997.0013.

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Dimethyl sulphide (DMS) is released into ocean waters by phytoplankton and may then cross the water–air interface into the atmosphere. Various models have been formulated to describe its behaviour in the atmosphere. Here, measurements of its concentrations and those of its major oxidation products, methane sulphonate, sulphur dioxide, non sea–salt sulphate and demethyl sulphoxide, in both the gas and aerosol phases, in Atlandtic air, are used to validate these qualitative descriptions of its oxidation. Behaviour consistent with day–time oxidation by the hydroxyl radical, with the yield of methane sulphonic acid being both temperature dependent and under the influence of the nitrogen dioxide mixing ratio, is seen. The rapid production of new particles also seems likely under certain conditions but it is not clear whether or not they enhance the concentrations of cloud condensation nuclei in the maritime troposphere. In maritime air a substantial fraction of the sulphate formed appears to be neutralized by reaction with ammonia to form ammonium aerosol.

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12

Bian, Jun Jie, Xin Min, Shu Zhang, and Chun Hu Li. "Supported Manganese Dioxide Catalyst for Seawater Flue Gas Desulfurization Application." Advanced Materials Research 236-238 (May 2011): 964–67. http://dx.doi.org/10.4028/www.scientific.net/amr.236-238.964.

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Ceramic-supported manganese dioxide catalyst, MnO2-ceramic, prepared by impregnation- precipitation method and calcined at 350 degree C, was exposed to flue gases to investigate the catalytic oxidation of sulphur dioxide in flue gas at seawater buffering system. The results showed that compared with acid treated ceramic, MnO2-ceramic gained 2%-46% higher Desulfurization efficiency in temperature range of 15-75 degree C. MnO2-ceramic exhibited 57% desulfurization efficiency at its favorable temperature (60 degree C) while ceramic showed 11% Desulfurization efficiency at 60 degree C. MnO2-ceramic was found to catalyze S(IV)oxidation even at low pH (pH<4) while the reaction rate of noncatalytic S(IV) oxidation is negligible under the identical conditions. No catalytic activity decay was observed after 40 hours’ run. XPS reveals that the Mn was in the oxidation state of +4 for the MnOx-ceramic. SEM-EDS and XRD indicated that the good catalytic activity of MnO2-ceramic at low temperature could be attributed to high dispersion of MnO2 on ceramic support. The high performance of MnO2-ceramic on the SO2 removal appeared to be promising in the seawater flue gas desulfurization industrial application when high sulfur coals were burned.

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13

Sapundzhiev, Christo, Georgi Grozev, and Dimiter Elenkov. "Influence of geometric and thermophysical properties of reaction layer on sulphur dioxide oxidation in transient conditions." Chemical Engineering & Technology - CET 13, no. 1 (1990): 131–35. http://dx.doi.org/10.1002/ceat.270130118.

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14

Cocic, Mira, Mihovil Logar, Sasa Cocic, Dragana Zivkovic, Branko Matovic, and Snezana Devic. "Determination of sulphide concentrates of ore copper by XRPD and chemical analysis." Chemical Industry 63, no. 4 (2009): 319–24. http://dx.doi.org/10.2298/hemind0904319c.

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Roasting process of sulphide copper concentrates in fluo-solid reactor is an oxidation process, and presents the first stage of copper concentrate processing in Copper Mining and Smelting Complex Bor, RTB Bor. Therefore, the importance of accurate and up to date process control is an apparent precondition for the correct treatment in the following stages and also for of high grade cathode copper. As concentrate is fed into the roaster, it is heated by a stream of hot air to about 590?C. The process takes place between solid and gaseous phases without the appearance of a liquid phase. The heat generated by the exothermic oxidation reaction of sulphur from cooper and iron minerals (chalcopyrite and pyrite) is sufficient to carry out the entire process autogenously at temperature from 620 to 670?C. The temperature of sulphur firing which defines the start of roasting depends on physical traits, particle size of sulfides and characteristic product of oxidation. The obtained products of the roasting process are: calcine, ready for smelting in the furnace and gas-rich sulphure dioxide (SO2), well suited for the production of sulfuric acid. The relationship between the quantitative mineral composition of the charge and of the calcine directly points out to the efficiency of the roasting process in fluo-solid reactor. The amount of bornite and magnetite, resulting from the sulfide oxidation is the most important parameter. Hence, quantitative determination of mineral composition is of great interest. In this work, the results of the determination of quantitative mineral composition of the copper sulphide concentrate (charge) and products of their roasting (calcine and overflow) in fluo-solid reactor in the RTB Bor are presented. The aim was to compare the results of the iron, copper, sulfur and oxygen contents determined by two independent techniques, the chemical (HA) and X-ray powder diffraction analysis (XRPD) that is based on the quantitative mineral composition. Differences in the obtained results are evident, but small enough to confirm the reliability of measurement.

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15

Barnes, I., V. Bastian, K. H. Becker, E. H. Fink, and W. Nelsen. "Oxidation of sulphur compounds in the atmosphere: I. Rate constants of OH radical reactions with sulphur dioxide, hydrogen sulphide, aliphatic thiols and thiophenol." Journal of Atmospheric Chemistry 4, no. 4 (December 1986): 445–66. http://dx.doi.org/10.1007/bf00053845.

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16

Meena, Vimlesh Kumar, Yogpal Dhayal, Deepak Singh Rathore, C. P. Singh Chandel, and K. S. Gupta. "Inhibition of Atmospheric Aqueous Phase Autoxidation of Sulphur Dioxide by Volatile Organic Compounds: Mono-, di- and Tri-Substituted Benzenes and Benzoic Acids." Progress in Reaction Kinetics and Mechanism 42, no. 2 (May 2017): 111–25. http://dx.doi.org/10.3184/146867817x14806858832108.

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Like many other volatile organic compounds (VOCs), the methoxy derivatives of benzene and benzoic acid are found in the atmosphere and, therefore, looking to their possible intervention in aqueous phase atmospheric oxidation of the major acid rain precursor, SO2, by oxygen, the kinetics of SO2 [hereafter referred to as S(IV)] autoxidation have been studied in the presence of methoxybenzene (anisole) and disubstituted 1,2-dimethoxybenzene, 1,3-dimethoxybenzene and 1,4-dimethoxybenzene. The effects of benzoic acid and its 2,6-dimethoxy, 3,4-dimethoxy, 2,3,4-trimethoxy and 2,4,5-trimethoxy derivatives have also been examined, as have the influences of 4-hydroxybenzoic acid, benzanilide and o-sulfobenzimide. As the methoxy group is known to influence the reaction SO4–· + organics [Formula: see text] SO42– + non-chain products, to understand the degree of influence of the methoxy group on the inhibition of this reaction, this series of methoxy compounds was selected. The kinetics were first-order in S(IV). Most of the VOCs inhibited S(IV) autoxidation, except benzanilide and o-sulfobenzimide, in accordance with kobs = k0/(1 + B [Inh]), where kobs and k0 are the first-order rate constants in the presence and absence of VOCs respectively and B is the inhibition parameter. The most interesting feature of this work is that, despite the high kinh values, the B values are unexpectedly quite low and benzanilide and o-sulfobenzimide showed no effect. The B values appear to be independent of kinh, which is opposite to that found in the case of a series of hydroxyl compounds. It appears probable that additional steps involving peroxy intermediates are involved.

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17

Beagley, Brian, David G. Kelly, Philomena P. Mac Rory, Charles A. McAuliffe, and Robin G. Pritchard. "Reaction of [FeL4X2][FeX4](L = OPPh3 or OAsPh3, X = Cl or Br) with sulphur dioxide to yield some rare examples of iron(III) complexes of sulphur dioxide, [FeL4{OS(O)X}2][FeX4]. The oxidation of sulphur dioxide by the iron(III) complexes and the isolation of the sulphuric acid derivatives (PPh3O)(PPh3OH)(HSO4) and (AsPh3OH)(HSO4). Crystal structure of the latter." Journal of the Chemical Society, Dalton Transactions, no. 9 (1990): 2657. http://dx.doi.org/10.1039/dt9900002657.

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18

Al-Farhan, K., Brian Beagley, Oraib El-Sayrafi, George A. Gott, Charles A. McAuliffe, Philomena P. Mac Rory, and Robin G. Pritchard. "Preparation, properties, and reactions with sulphur dioxide of triphenylphosphine oxide complexes of manganese(II) thiocyanate. Crystal structures of [{Mn(OPPh3)2(NCS)(µ-NCS)}2], [Mn(OPPh3)4(NCS)2], and (PPh3O)(PPh3OH)(HSO4), a derivative of sulphuric acid formed under ambient air oxidation of sulphur dioxide." J. Chem. Soc., Dalton Trans., no. 4 (1990): 1243–50. http://dx.doi.org/10.1039/dt9900001243.

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19

Li, X. Z., P. T. Yue, and C. L. Mak. "Photooxidation of wool dye and TCP in aqueous solution using an innovative TiO2 mesh electrode." Water Science and Technology 42, no. 12 (December 1, 2000): 181–88. http://dx.doi.org/10.2166/wst.2000.0267.

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An innovative titanium dioxide (TiO2) mesh electrode was prepared by anodisation, in which 0.5 M sulphuric acid was used as electrolyte and titanium (Ti) metal mesh was anodised in a two stage anodic process. The innovated mesh electrode was examined using Raman spectroscopy to determine the formation of TiO2 layer when different potentials of 120 V, 140 V, 160 V, and 180 V were applied in anodisation. Microporous surface of the electrode was also examined using scanning electron microscopy. The photocatalytic (PC) oxidation and photoelectrocatalytic (PEC) oxidation were studied using the new electrode for treating synthetic wastewater solutions of dye and trichlorophenol (TCP) respectively. The colour removal efficiency of 68% was achieved using the 160V-mesh electrode for treating wool dye solution after 80 minutes reaction time. However, it was found that a significant substrate adsorption on the surface of the mesh electrode could not be avoided when pH was below pHIEP of TiO2=6.3. In this condition, electrostatic adsorption occurred between the anionic substrate molecules and positively charged TiO2 surface. The adsorbed substrate anion occupied most active sites of TiO2 on the mesh electrode surface and significantly reduced the performance efficiency of photo-oxidation, when the TiO2 mesh electrode was reused. The experiment demonstrated that TCP adsorption on the mesh electrode could be significantly eliminated, when pH of TCP solution was adjusted to above 7. When raising pH in TCP photodegradation eliminated substrate adsorption, it was confirmed that PC oxidation with application of a potential bias could enhance the photo-oxidation rate and a repeatable photo-oxidation rate could be maintained when the same mesh electrode was reused in its following tests.

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20

Aiuppa, A., A. Franco, R. von Glasow, A. G. Allen, W. D'Alessandro, T. A. Mather, D. M. Pyle, and M. Valenza. "The tropospheric processing of acidic gases and hydrogen sulphide in volcanic gas plumes as inferred from field and model investigations." Atmospheric Chemistry and Physics 7, no. 5 (March 13, 2007): 1441–50. http://dx.doi.org/10.5194/acp-7-1441-2007.

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Abstract. Improving the constraints on the atmospheric fate and depletion rates of acidic compounds persistently emitted by non-erupting (quiescent) volcanoes is important for quantitatively predicting the environmental impact of volcanic gas plumes. Here, we present new experimental data coupled with modelling studies to investigate the chemical processing of acidic volcanogenic species during tropospheric dispersion. Diffusive tube samplers were deployed at Mount Etna, a very active open-conduit basaltic volcano in eastern Sicily, and Vulcano Island, a closed-conduit quiescent volcano in the Aeolian Islands (northern Sicily). Sulphur dioxide (SO2), hydrogen sulphide (H2S), hydrogen chloride (HCl) and hydrogen fluoride (HF) concentrations in the volcanic plumes (typically several minutes to a few hours old) were repeatedly determined at distances from the summit vents ranging from 0.1 to ~10 km, and under different environmental conditions. At both volcanoes, acidic gas concentrations were found to decrease exponentially with distance from the summit vents (e.g., SO2 decreases from ~10 000 μg/m3at 0.1 km from Etna's vents down to ~7 μg/m3 at ~10 km distance), reflecting the atmospheric dilution of the plume within the acid gas-free background troposphere. Conversely, SO2/HCl, SO2/HF, and SO2/H2S ratios in the plume showed no systematic changes with plume aging, and fit source compositions within analytical error. Assuming that SO2 losses by reaction are small during short-range atmospheric transport within quiescent (ash-free) volcanic plumes, our observations suggest that, for these short transport distances, atmospheric reactions for H2S and halogens are also negligible. The one-dimensional model MISTRA was used to simulate quantitatively the evolution of halogen and sulphur compounds in the plume of Mt. Etna. Model predictions support the hypothesis of minor HCl chemical processing during plume transport, at least in cloud-free conditions. Larger variations in the modelled SO2/HCl ratios were predicted under cloudy conditions, due to heterogeneous chlorine cycling in the aerosol phase. The modelled evolution of the SO2/H2S ratios is found to be substantially dependent on whether or not the interactions of H2S with halogens are included in the model. In the former case, H2S is assumed to be oxidized in the atmosphere mainly by OH, which results in minor chemical loss for H2S during plume aging and produces a fair match between modelled and measured SO2/H2S ratios. In the latter case, fast oxidation of H2S by Cl leads to H2S chemical lifetimes in the early plume of a few seconds, and thus SO2 to H2S ratios that increase sharply during plume transport. This disagreement between modelled and observed plume compositions suggests that more in-detail kinetic investigations are required for a proper evaluation of H2S chemical processing in volcanic plumes.

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21

Aiuppa, A., A. Franco, R. von Glasow, A. G. Allen, W. D’Alessandro, T. A. Mather, D. M. Pyle, and M. Valenza. "The tropospheric processing of acidic gases and hydrogen sulphide in volcanic gas plumes as inferred from field and model investigations." Atmospheric Chemistry and Physics Discussions 6, no. 6 (November 21, 2006): 11653–80. http://dx.doi.org/10.5194/acpd-6-11653-2006.

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Abstract. Improving the constraints on the atmospheric fate and depletion rates of acidic compounds persistently emitted by non-erupting (quiescent) volcanoes is important for quantitatively predicting the environmental impact of volcanic gas plumes. Here, we present new experimental data coupled with modelling studies to investigate the chemical processing of acidic volcanogenic species during tropospheric dispersion. Diffusive tube samplers were deployed at Mount Etna, a very active open-conduit basaltic volcano in eastern Sicily, and Vulcano Island, a closed-conduit quiescent volcano in the Aeolian Islands (northern Sicily). Sulphur dioxide (SO2), hydrogen sulphide (H2S), hydrogen chloride (HCl) and hydrogen fluoride (HF) concentrations in the volcanic plumes (typically several minutes to a few hours old) were repeatedly determined at distances from the summit vents ranging from 0.1 to ~10 km, and under different environmental conditions. At both volcanoes, acidic gas concentrations were found to decrease exponentially with distance from the summit vents (e.g., SO2 decreases from ~10 000 μg/m3 at 0.1 km from Etna's vents down to ~7 μg/m3 at ~10 km distance), reflecting the atmospheric dilution of the plume within the acid gas-free background troposphere. Conversely, SO2/HCl, SO2/HF, and SO2/H2S ratios in the plume showed no systematic changes with plume aging, and fit source compositions within analytical error. Assuming that SO2 losses by reaction are small during short-range atmospheric transport within quiescent (ash-free) volcanic plumes, our observations suggest that, for these short transport distances, atmospheric reactions for H2S and halogens are also negligible. The one-dimensional model MISTRA was used to simulate quantitatively the evolution of halogen and sulphur compounds in the plume of Mt. Etna. Model predictions support the hypothesis of minor HCl chemical processing during plume transport, at least in cloud-free conditions. Larger variations in the modelled SO2/HCl ratios were predicted under cloudy conditions, due to heterogeneous chlorine cycling in the aerosol phase. The modelled evolution of the SO2/H2S ratios is found to be substantially dependent on whether or not the interactions of H2S with halogens are included in the model. In the former case, H2S is assumed to be oxidized in the atmosphere mainly by OH, which results in minor chemical loss for H2S during plume aging and produces a fair match between modelled and measured SO2/H2S ratios. In the latter case, fast oxidation of H2S by Cl leads to H2S chemical lifetimes in the early plume of a few seconds, and thus SO2 to H2S ratios that increase sharply during plume transport. This disagreement between modelled and observed plume compositions suggests that more in-detail kinetic investigations are required for a proper evaluation of H2S chemical processing in volcanic plumes.

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22

Golodov, V. A., and L. V. Kashnikova. "Oxidation of Sulphur Dioxide in Aqueous Solutions." Russian Chemical Reviews 57, no. 11 (November 30, 1988): 1029–40. http://dx.doi.org/10.1070/rc1988v057n11abeh003409.

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23

Méndez, Manuel A., Alberto Cano, and Marco F. Suárez. "Sonophotocatalytic oxidation of elemental sulphur on titanium dioxide." Ultrasonics Sonochemistry 14, no. 3 (March 2007): 337–42. http://dx.doi.org/10.1016/j.ultsonch.2006.07.002.

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24

Napier, D. H., and M. H. Stone. "Catalytic oxidation of sulphur dioxide at low concentrations." Journal of Applied Chemistry 8, no. 12 (May 4, 2007): 781–86. http://dx.doi.org/10.1002/jctb.5010081202.

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25

WEDZICHA, B. L., and M. T. KAPUTO. "Reaction of melanoidins with sulphur dioxide: stoichiometry of the reaction." International Journal of Food Science & Technology 22, no. 6 (June 28, 2007): 643–51. http://dx.doi.org/10.1111/j.1365-2621.1987.tb00532.x.

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26

Balzhinimaev, Bair S., Alexei A. Ivanov, Olga B. Lapina, Vyacheslav M. Mastikhin, and Kirill I. Zamaraev. "Mechanism of sulphur dioxide oxidation over supported vanadium catalysts." Faraday Discussions of the Chemical Society 87 (1989): 133. http://dx.doi.org/10.1039/dc9898700133.

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27

Shin, Koo, and Harold M. Goff. "Iron(III) porphyrin promoted aerobic oxidation of sulphur dioxide." Journal of the Chemical Society, Chemical Communications, no. 6 (1990): 461. http://dx.doi.org/10.1039/c39900000461.

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28

Cerru, F. G., A. Kronenburg, and R. P. Lindstedt. "A systematically reduced reaction mechanism for sulphur oxidation." Proceedings of the Combustion Institute 30, no. 1 (January 2005): 1227–35. http://dx.doi.org/10.1016/j.proci.2004.08.083.

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29

Galwey, Andrew K. "The low-temperature reaction of ferrous sulphide with sulphur dioxide." Thermochimica Acta 291, no. 1-2 (April 1997): 155–69. http://dx.doi.org/10.1016/s0040-6031(96)03113-9.

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30

Leyshon, L. J., and C. Holstead. "Reaction of Sulphur Dioxide with Image Transfer Azo-Naphthol Dyes." Journal of Photographic Science 36, no. 3 (May 1988): 107–14. http://dx.doi.org/10.1080/00223638.1988.11736979.

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31

Hartman, M., K. Svoboda, O. Trnka, and V. Veselý. "Reaction of sulphur dioxide with magnesia in a fluidised bed." Chemical Engineering Science 43, no. 8 (1988): 2045–50. http://dx.doi.org/10.1016/0009-2509(88)87082-9.

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32

Sakurai, Yasuhiro, Yoshiaki Takahashi, and Tomoyuki Makino. "Laboratory measurement of absorption and oxidation of sulphur dioxide by zeolite." Journal of Geochemical Exploration 64, no. 1-3 (November 1998): 315–19. http://dx.doi.org/10.1016/s0375-6742(98)00041-7.

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33

Hjuler, Klaus, and Kim Dam-Johansen. "Wet oxidation of residual product from spray absorption of sulphur dioxide." Chemical Engineering Science 49, no. 24 (1994): 4515–21. http://dx.doi.org/10.1016/s0009-2509(05)80037-5.

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34

Lagrange, J., C. Pallares, and P. Lagrange. "Electrolyte effects on aqueous atmospheric oxidation of sulphur dioxide by ozone." Journal of Geophysical Research 99, no. D7 (1994): 14595. http://dx.doi.org/10.1029/94jd00573.

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35

Iliev, P., I. Nikolov, T. Vitanov, and E. Budevski. "Influence of nitrogen oxides on the electrocatalytic oxidation of sulphur dioxide." Journal of Applied Electrochemistry 22, no. 5 (May 1992): 425–28. http://dx.doi.org/10.1007/bf01077544.

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36

Jeffreys, Brian, J. Bernard Gill, and David C. Goodall. "Reactions in mixed non-aqueous systems containing sulphur dioxide. Part 6. The reaction of metal oxides with dimethyl sulphoxide–sulphur dioxide." J. Chem. Soc., Dalton Trans., no. 1 (1985): 99–100. http://dx.doi.org/10.1039/dt9850000099.

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37

Cocks, Alan T., Rohantha P. Fernando, and Ian S. Fletcher. "The gas-phase reaction of the methylperoxy radical with sulphur dioxide." Atmospheric Environment (1967) 20, no. 12 (January 1986): 2359–66. http://dx.doi.org/10.1016/0004-6981(86)90066-1.

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38

Davini, Paolo, Gennaro DeMichele, and Sisto Bertacchi. "Reaction between calcium-based sorbents and sulphur dioxide: a thermogravimetric investigation." Fuel 70, no. 2 (February 1991): 201–4. http://dx.doi.org/10.1016/0016-2361(91)90153-2.

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39

Esmadi, Fatima T., and Amer J. Al-Hamid. "Reaction of sulphur dioxide with chlorocarbonyls of ruthenium, rhodium and iridium." Transition Metal Chemistry 19, no. 6 (December 1994): 571–74. http://dx.doi.org/10.1007/bf00980405.

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40

Tandy, G. H. "The role of alkali sulphates in vanadium catalysts for sulphur dioxide oxidation." Journal of Applied Chemistry 6, no. 2 (May 4, 2007): 68–74. http://dx.doi.org/10.1002/jctb.5010060204.

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41

Rickett, G. L., V. Dupont, and M. V. Twigg. "Methane oxidation over palladium-washcoated foils in the presence of sulphur dioxide." Catalysis Today 155, no. 1-2 (October 2010): 51–58. http://dx.doi.org/10.1016/j.cattod.2009.03.013.

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42

Lagrange, J., C. Pallares, G. Wenger, and P. Lagrange. "Electrolyte effects on aqueous atmospheric oxidation of sulphur dioxide by hydrogen peroxide." Atmospheric Environment. Part A. General Topics 27, no. 2 (February 1993): 129–37. http://dx.doi.org/10.1016/0960-1686(93)90342-v.

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43

Reichelt, Lydia, Sebastian Hippmann, Vyacheslav Nikolayevich Brichkin, and Martin Bertau. "Oxidation of Sulphur Dioxide using Micro‐ and Nanoparticles of various Iron Oxides." Zeitschrift für anorganische und allgemeine Chemie 647, no. 15 (June 17, 2021): 1583–93. http://dx.doi.org/10.1002/zaac.202100091.

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44

Quijada, C., A. Rodes, J. L. Vázquez, J. M. Pérez, and A. Aldaz. "Electrochemical behaviour of aqueous sulphur dioxide at polycrystalline Pt electrodes in acidic medium. A voltammetric and in-situ FT-IR study Part II. Promoted oxidation of sulphur dioxide. Reduction of sulphur dioxide." Journal of Electroanalytical Chemistry 398, no. 1-2 (December 1995): 105–15. http://dx.doi.org/10.1016/0022-0728(95)04244-6.

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45

Ahmad, N. G., H. S. . Aziz, and G. Th. Sedeek. "Synthesis and Study of some Heterocyclic Compounds from Schiff Base of Pinacolone." Tikrit Journal of Pure Science 24, no. 2 (April 15, 2019): 50. http://dx.doi.org/10.25130/j.v24i2.801.

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In this work, the synthesis of some heterocyclic compound of four, five and seven membered rings were done. On oxidation of the pinacole alcohol using concentrated sulphuric acid pinacolone were obtained and used as a precursor for the synthesis of three new Schiffs base through the reaction with para substituted anilines compounds. These imines were allowed to react with chloroacetyl chloride in dry dioxane to give the azetadine -2- one compounds. Also some thiazoldinone compounds were synthesized from the reaction of the corresponding imines with thioglycolic acid in the presence of zinc chloride in dry benzene and 1, 3-oxazepine-4,7-diones, were obtained from the reaction of imines with maleic and phythalic anhydries in dry benzene. The synthesized compounds were characterized by IR spectroscopy and physical paramrters. http://dx.doi.org/10.25130/tjps.24.2019.031

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46

Pietrzak, Robert, Mieczysław Kozłowski, Helena Wachowska, and Jan Yperman. "Studies of the soluble part of oxidised coals." Open Chemistry 2, no. 2 (June 1, 2004): 278–89. http://dx.doi.org/10.2478/bf02475573.

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AbstractSoluble products obtained from the oxidation of four types of coal, each characterised by different degree of coalification and different degree of sulphur content, are studied. The coals are oxidised with peracetic acid (PAA) and nitric acid. Analyses are performed by Atmospheric Pressure-Temperature Programmed Reduction (AP-TPR) and Fourier Transform Infrared Spectroscopy (FTIR). The soluble products contain much more sulphur than the insoluble products of oxidation. The products obtained from the reaction with HNO3 contain higher amounts of inorganic sulphur compounds, while those obtained from the reaction with PAA are characterised by an increased content of organic sulphur species.

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47

Byanju, R. M., M. B. Gewali, and K. Manandhar. "Low cost Passive Monitoring of Nitrogen dioxide and Sulphur dioxide in ambient air." Journal of Nepal Chemical Society 27 (July 16, 2012): 34–45. http://dx.doi.org/10.3126/jncs.v27i1.6439.

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Standard nitrogen dioxide (NO2) and sulphur dioxide (SO2) monitoring techniques require expensive instrumentation which is not easily adapted for large scale monitoring by resource limited countries. This paper presents the use of locally available relatively cheaper polyethylene tubes to be developed as passive diffusive sampler and use for monitoring of ambient nitrogen dioxide and sulphur dioxide using Triethanolamine (TEA) as absorbent. After extraction with double distilled water, modified Griese-Saltzmann method and West-Gaeke method were used for analysis of nitrite and sulphate adduct formed due to reaction of NO2 and SO2 respectively with TEA using spectrophotometer. The results are successfully compared with other standard methods. The detection limits and precision of the method as expressed as Coefficient of variation are good enough for monitoring of NO2 and SO2 in ambient air.DOI: http://dx.doi.org/10.3126/jncs.v27i1.6439 J. Nepal Chem. Soc., Vol. 27, 2011 34-45Uploaded date: 16 July, 2012

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48

Panagiotidis, Thomas, Ekkehard Richter, and Harald Jüntgen. "Structural changes of an anthracite char during the reaction with sulphur dioxide." Carbon 26, no. 1 (1988): 89–95. http://dx.doi.org/10.1016/0008-6223(88)90013-9.

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49

Candy, Rachel M., Kyle R. Blight, and David E. Ralph. "Analysis of the Bacterial Sulphur System." Advanced Materials Research 825 (October 2013): 190–93. http://dx.doi.org/10.4028/www.scientific.net/amr.825.190.

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Heterogeneous bacterial sulphur systems are inherently complicated. However, developing an understanding of the influence of environmental factors such as pH,Iand PCO2is important for a number of fields. Examples of these include minimising acid mine drainage and maximising metal recovery from low-grade sulphide minerals. Measuring the effect of these factors on the extent and rate of sulphur (S) oxidation is complicated by the presence and nature of solid phase elemental S. The rate and extent of S oxidation can be determined indirectly via the reaction product, H2SO4, which was quantified using pH measurements in this study. The method was critically dependent on the quality of pH data but proved effective in providing rate constants for the catalysed S oxidation reaction and yield (biomass/substrate) estimates in the range pH > 1.5. IncreasingIover the range 0.176 0.367 mol L-1decreased bacterial cell yields but increased the rate of sulphur oxidation significantly. Partial pressures of CO2in the range of 0.039 1.18% v/v produced no significant effect on the rates of S oxidation or bacterial cell yields. Bacterial cell yields were not affected in the pH range 1.5 2.5, however the rate of S oxidation increased significantly from pH 2.0 2.5. In the range pH < 1.5 the batch cultures progressed and although no reliable rate data was recorded cell yields decreased from 7.43 to 2.05 (× 1012cells mol-1) at pH 1.5 to 1.0 respectively.

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50

Bureš, Richard, Martin Klajmon, Jaroslav Fojt, Pavol Rak, Kristýna Jílková, and Jan Stoulil. "Artificial Patination of Copper and Copper Alloys in Wet Atmosphere with Increased Content of SO2." Coatings 9, no. 12 (December 8, 2019): 837. http://dx.doi.org/10.3390/coatings9120837.

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Natural copper patina is usually formed over several decades. This work investigates the possibility of obtaining a stable artificial patina based on brochantite in a more reasonable time. The patination process was based on patina formation from a humid atmosphere containing sulphur dioxide. The studied parameters were humidity (condensation and condensation/drying), sulphur dioxide concentration (4.4–44.3 g·m−3) and surface pre-treatments (grinding, pre-oxidation and pre-patination) prior to the patination process. Samples were evaluated by mass change, digital image analysis, spectrophotometry, scanning electron microscopy (SEM), X-ray photoelectron spectroscopy (XPS) and X-ray diffraction (XRD). A resistometric method was employed in order to observe the patina formation continuously during the exposure. Conditions inside the chamber were monitored during the exposure (pH of water and concentration of SO2 in gaseous phase). According to XRD, it was possible to deliberately grow a brochantite patina of reasonable thickness (approx. 30 µm), even within a couple of days of exposure. The drying phase of the condensation cycle increased the homogeneity of the deposited patina. Formation kinetics were the fastest under a condensation/drying cycle, starting with 17.7 g·m−3 sulphur dioxide and decreasing dosing in the cycle, with an electrolyte pH close to 3. The higher sulphur dioxide content above 17.7 g·m−3 forms too aggressive a surface electrolyte, which led to the dissolution of the brochantite. The pre-oxidation of copper surface resulted in a significant improvement of patina homogeneity on the surface.

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