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font="default" size="100%">Zrinyi, N.</style></author><author><style face="normal" font="default" size="100%">Pham, A.L.-T.</style></author></authors></contributors><titles><title><style face="normal" font="default" size="100%">Oxidation of benzoic acid by heat-activated persulfate: Effect of temperature on transformation pathway and product distribution</style></title><secondary-title><style face="normal" font="default" size="100%">Water Research</style></secondary-title></titles><keywords><keyword><style  face="normal" font="default" size="100%">Activated persulfate</style></keyword><keyword><style  face="normal" font="default" size="100%">Advanced Oxidation Processes</style></keyword><keyword><style  face="normal" font="default" size="100%">Article</style></keyword><keyword><style  face="normal" font="default" size="100%">Benzoic acid</style></keyword><keyword><style  face="normal" font="default" size="100%">Carboxylation</style></keyword><keyword><style  face="normal" font="default" size="100%">Chemical</style></keyword><keyword><style  face="normal" font="default" size="100%">Chemical activation</style></keyword><keyword><style  face="normal" font="default" size="100%">chemical compound</style></keyword><keyword><style  face="normal" font="default" size="100%">chemical reaction kinetics</style></keyword><keyword><style  face="normal" font="default" size="100%">Contamination</style></keyword><keyword><style  face="normal" font="default" size="100%">decarboxylation</style></keyword><keyword><style  face="normal" font="default" size="100%">Decarboxylation reactions</style></keyword><keyword><style  face="normal" font="default" size="100%">fragmentation reaction</style></keyword><keyword><style  face="normal" font="default" size="100%">Fragmentation reactions</style></keyword><keyword><style  face="normal" font="default" size="100%">Groundwater</style></keyword><keyword><style  face="normal" font="default" size="100%">Groundwater treatment</style></keyword><keyword><style  face="normal" font="default" size="100%">heat</style></keyword><keyword><style  face="normal" font="default" size="100%">Hot Temperature</style></keyword><keyword><style  face="normal" font="default" size="100%">hydroxyl radical</style></keyword><keyword><style  face="normal" font="default" size="100%">Hydroxyl radical generation</style></keyword><keyword><style  face="normal" font="default" size="100%">Hydroxylation</style></keyword><keyword><style  face="normal" font="default" size="100%">Impurities</style></keyword><keyword><style  face="normal" font="default" size="100%">organic pollutant</style></keyword><keyword><style  face="normal" font="default" size="100%">oxidant</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxidation</style></keyword><keyword><style  face="normal" font="default" size="100%">oxidation reduction reaction</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxidation-Reduction</style></keyword><keyword><style  face="normal" font="default" size="100%">persulfate</style></keyword><keyword><style  face="normal" font="default" size="100%">pollutant removal</style></keyword><keyword><style  face="normal" font="default" size="100%">priority journal</style></keyword><keyword><style  face="normal" font="default" size="100%">soil analysis</style></keyword><keyword><style  face="normal" font="default" size="100%">sulfate</style></keyword><keyword><style  face="normal" font="default" size="100%">Sulfates</style></keyword><keyword><style  face="normal" font="default" size="100%">Sulfur compounds</style></keyword><keyword><style  face="normal" font="default" size="100%">Temperature</style></keyword><keyword><style  face="normal" font="default" size="100%">temperature effect</style></keyword><keyword><style  face="normal" font="default" size="100%">temperature sensitivity</style></keyword><keyword><style  face="normal" font="default" size="100%">Time-concentration profiles</style></keyword><keyword><style  face="normal" font="default" size="100%">transformation</style></keyword><keyword><style  face="normal" font="default" size="100%">Transformation pathways</style></keyword><keyword><style  face="normal" font="default" size="100%">unclassified drug</style></keyword><keyword><style  face="normal" font="default" size="100%">water pollutant</style></keyword><keyword><style  face="normal" font="default" size="100%">Water Pollutants</style></keyword><keyword><style  face="normal" font="default" size="100%">Water treatment</style></keyword></keywords><dates><year><style  face="normal" font="default" size="100%">2017</style></year></dates><urls><web-urls><url><style face="normal" font="default" size="100%">https://www.scopus.com/inward/record.uri?eid=2-s2.0-85018349473&amp;doi=10.1016%2fj.watres.2017.04.066&amp;partnerID=40&amp;md5=bb56844305381cfc146e134f95945c71</style></url></web-urls></urls><publisher><style face="normal" font="default" size="100%">Elsevier Ltd</style></publisher><volume><style face="normal" font="default" size="100%">120</style></volume><pages><style face="normal" font="default" size="100%">43-51</style></pages><language><style face="normal" font="default" size="100%">eng</style></language><abstract><style face="normal" font="default" size="100%">Heat activates persulfate (S2O8 2−) into sulfate radical (SO4 [rad]−), a powerful oxidant capable of transforming a wide variety of contaminants. Previous studies have shown that an increase in temperature accelerates the rates of persulfate activation and contaminant transformation. However, few studies have considered the effect of temperature on contaminant transformation pathway. The objective of this study was to determine how temperature (T = 22–70 °C) influences the activation of persulfate, the transformation of benzoic acid (i.e., a model compound), and the distribution of benzoic acid oxidation products. The time-concentration profiles of the products suggest that benzoic acid was transformed via decarboxylation and hydroxylation mechanisms, with the former becoming increasingly important at elevated temperatures. The pathway through which the products were further oxidized was also influenced by the temperature of persulfate activation. Our findings suggest that the role of temperature in the persulfate-based treatment systems is not limited only to controlling the rates of sulfate and hydroxyl radical generation. The ability of sulfate radical to initiate decarboxylation reactions and, more broadly, fragmentation reactions, as well as the effect of temperature on these transformation pathways could be important to the transformation of a number of organic contaminants. © 2017 Elsevier Ltd</style></abstract><notes><style face="normal" font="default" size="100%">cited By 19</style></notes></record><record><source-app name="Biblio" version="7.x">Drupal-Biblio</source-app><ref-type>17</ref-type><contributors><authors><author><style face="normal" font="default" size="100%">Pham, A.L.-T.</style></author><author><style face="normal" font="default" size="100%">Johnson, C.</style></author><author><style face="normal" font="default" size="100%">Manley, D.</style></author><author><style face="normal" font="default" size="100%">Hsu-Kim, H.</style></author></authors></contributors><titles><title><style face="normal" font="default" size="100%">Influence of Sulfide Nanoparticles on Dissolved Mercury and Zinc Quantification by Diffusive Gradient in Thin-Film Passive Samplers</style></title><secondary-title><style face="normal" font="default" size="100%">Environmental Science &amp; Technology</style></secondary-title></titles><keywords><keyword><style  face="normal" font="default" size="100%">absorption</style></keyword><keyword><style  face="normal" font="default" size="100%">analysis</style></keyword><keyword><style  face="normal" font="default" size="100%">Aquatic environments</style></keyword><keyword><style  face="normal" font="default" size="100%">Article</style></keyword><keyword><style  face="normal" font="default" size="100%">binding affinity</style></keyword><keyword><style  face="normal" font="default" size="100%">chemistry</style></keyword><keyword><style  face="normal" font="default" size="100%">concentration (composition)</style></keyword><keyword><style  face="normal" font="default" size="100%">concentration (parameters)</style></keyword><keyword><style  face="normal" font="default" size="100%">devices</style></keyword><keyword><style  face="normal" font="default" size="100%">Diffusion</style></keyword><keyword><style  face="normal" font="default" size="100%">Diffusive gradients</style></keyword><keyword><style  face="normal" font="default" size="100%">diffusivity</style></keyword><keyword><style  face="normal" font="default" size="100%">Dissolution</style></keyword><keyword><style  face="normal" font="default" size="100%">Dissolved fraction</style></keyword><keyword><style  face="normal" font="default" size="100%">Dissolved metal concentrations</style></keyword><keyword><style  face="normal" font="default" size="100%">Dissolved metals</style></keyword><keyword><style  face="normal" font="default" size="100%">Effective diffusion coefficients</style></keyword><keyword><style  face="normal" font="default" size="100%">Environmental Monitoring</style></keyword><keyword><style  face="normal" font="default" size="100%">film</style></keyword><keyword><style  face="normal" font="default" size="100%">Geologic Sediments</style></keyword><keyword><style  face="normal" font="default" size="100%">measurement</style></keyword><keyword><style  face="normal" font="default" size="100%">mercury</style></keyword><keyword><style  face="normal" font="default" size="100%">mercury (element)</style></keyword><keyword><style  face="normal" font="default" size="100%">Mercury (metal)</style></keyword><keyword><style  face="normal" font="default" size="100%">metal</style></keyword><keyword><style  face="normal" font="default" size="100%">Metal nanoparticles</style></keyword><keyword><style  face="normal" font="default" size="100%">Metals</style></keyword><keyword><style  face="normal" font="default" size="100%">Nano particulates</style></keyword><keyword><style  face="normal" font="default" size="100%">nanoparticle</style></keyword><keyword><style  face="normal" font="default" size="100%">Nanoparticles</style></keyword><keyword><style  face="normal" font="default" size="100%">Passive samplers</style></keyword><keyword><style  face="normal" font="default" size="100%">performance assessment</style></keyword><keyword><style  face="normal" font="default" size="100%">Pore size</style></keyword><keyword><style  face="normal" font="default" size="100%">procedures</style></keyword><keyword><style  face="normal" font="default" size="100%">quantitative analysis</style></keyword><keyword><style  face="normal" font="default" size="100%">sampler</style></keyword><keyword><style  face="normal" font="default" size="100%">sediment</style></keyword><keyword><style  face="normal" font="default" size="100%">sorbent</style></keyword><keyword><style  face="normal" font="default" size="100%">speciation (chemistry)</style></keyword><keyword><style  face="normal" font="default" size="100%">sulfide</style></keyword><keyword><style  face="normal" font="default" size="100%">sulfide nanoparticle</style></keyword><keyword><style  face="normal" font="default" size="100%">Sulfides</style></keyword><keyword><style  face="normal" font="default" size="100%">surface property</style></keyword><keyword><style  face="normal" font="default" size="100%">Thin films</style></keyword><keyword><style  face="normal" font="default" size="100%">thin section</style></keyword><keyword><style  face="normal" font="default" size="100%">unclassified drug</style></keyword><keyword><style  face="normal" font="default" size="100%">X ray absorption spectroscopy</style></keyword><keyword><style  face="normal" font="default" size="100%">X-Ray Absorption Spectroscopy</style></keyword><keyword><style  face="normal" font="default" size="100%">Zinc</style></keyword><keyword><style  face="normal" font="default" size="100%">Zinc compounds</style></keyword><keyword><style  face="normal" font="default" size="100%">Zinc sulfide</style></keyword></keywords><dates><year><style  face="normal" font="default" size="100%">2015</style></year></dates><urls><web-urls><url><style face="normal" font="default" size="100%">https://www.scopus.com/inward/record.uri?eid=2-s2.0-84946593400&amp;doi=10.1021%2facs.est.5b02774&amp;partnerID=40&amp;md5=5c5af87ad0f26f1568696a7858c75897</style></url></web-urls></urls><number><style face="normal" font="default" size="100%">21</style></number><publisher><style face="normal" font="default" size="100%">American Chemical Society</style></publisher><volume><style face="normal" font="default" size="100%">49</style></volume><pages><style face="normal" font="default" size="100%">12897-12903</style></pages><language><style face="normal" font="default" size="100%">eng</style></language><abstract><style face="normal" font="default" size="100%">Diffusive gradient in thin-film (DGT) passive samplers are frequently used to monitor the concentrations of metals such as mercury and zinc in sediments and other aquatic environments. The application of these samplers generally presumes that they quantify only the dissolved fraction and not particle-bound metal species that are too large to migrate into the sampler. However, metals associated with very small nanoparticles (smaller than the pore size of DGT samplers) can be abundant in certain environments, yet the implications of these nanoparticles for DGT measurements are unclear. The objective of this study was to determine how the performance of the DGT sampler is affected by the presence of nanoparticulate species of Hg and Zn. DGT samplers were exposed to solutions containing known amounts of dissolved Hg(II) and nanoparticulate HgS (or dissolved Zn(II) and nanoparticulate ZnS). The amounts of Hg and Zn accumulated onto the DGT samplers were quantified over hours to days, and the rates of diffusion of the dissolved metal (i.e., the effective diffusion coefficient D) into the sampler's diffusion layer were calculated and compared for solutions containing varying concentrations of nanoparticles. The results suggested that the nanoparticles deposited on the surface of the samplers might have acted as sorbents, slowing the migration of the dissolved species into the samplers. The consequence was that the DGT sampler data underestimated the dissolved metal concentration in the solution. In addition, X-ray absorption spectroscopy was employed to determine the speciation of the Hg accumulated on the sampler binding layer, and the results indicated that HgS nanoparticles did not appear to directly contribute to the DGT measurement. Overall, our findings suggest that the deployment of DGT samplers in settings where nanoparticles are relevant (e.g., sediments) may result in DGT data that incorrectly estimated the dissolved metal concentrations. Models for metal uptake into the sampler may need to be reconsidered. © 2015 American Chemical Society.</style></abstract><notes><style face="normal" font="default" size="100%">cited By 5</style></notes></record><record><source-app name="Biblio" version="7.x">Drupal-Biblio</source-app><ref-type>17</ref-type><contributors><authors><author><style face="normal" font="default" size="100%">Pham, A.L.T.</style></author><author><style face="normal" font="default" size="100%">Morris, A.</style></author><author><style face="normal" font="default" size="100%">Zhang, T.</style></author><author><style face="normal" font="default" size="100%">Ticknor, J.</style></author><author><style face="normal" font="default" size="100%">Levard, C.</style></author><author><style face="normal" font="default" size="100%">Hsu-Kim, H.</style></author></authors></contributors><titles><title><style face="normal" font="default" size="100%">Precipitation of nanoscale mercuric sulfides in the presence of natural organic matter: Structural properties, aggregation, and biotransformation</style></title><secondary-title><style face="normal" font="default" size="100%">Geochimica et Cosmochimica Acta</style></secondary-title></titles><keywords><keyword><style  face="normal" font="default" size="100%">aggregation</style></keyword><keyword><style  face="normal" font="default" size="100%">Bacteria (microorganisms)</style></keyword><keyword><style  face="normal" font="default" size="100%">Biotransformation</style></keyword><keyword><style  face="normal" font="default" size="100%">crystal structure</style></keyword><keyword><style  face="normal" font="default" size="100%">crystallinity</style></keyword><keyword><style  face="normal" font="default" size="100%">dissolved organic matter</style></keyword><keyword><style  face="normal" font="default" size="100%">mercury (element)</style></keyword><keyword><style  face="normal" font="default" size="100%">Methylation</style></keyword><keyword><style  face="normal" font="default" size="100%">organic matter</style></keyword><keyword><style  face="normal" font="default" size="100%">precipitation (chemistry)</style></keyword><keyword><style  face="normal" font="default" size="100%">sulfide</style></keyword></keywords><dates><year><style  face="normal" font="default" size="100%">2014</style></year></dates><urls><web-urls><url><style face="normal" font="default" size="100%">https://www.scopus.com/inward/record.uri?eid=2-s2.0-84897103199&amp;doi=10.1016%2fj.gca.2014.02.027&amp;partnerID=40&amp;md5=b4ef1a8932d089ea951c882933ca420e</style></url></web-urls></urls><publisher><style face="normal" font="default" size="100%">Elsevier Ltd</style></publisher><volume><style face="normal" font="default" size="100%">133</style></volume><pages><style face="normal" font="default" size="100%">204-215</style></pages><language><style face="normal" font="default" size="100%">eng</style></language><abstract><style face="normal" font="default" size="100%">Mercuric sulfide species are likely the predominant forms of mercury (Hg) in anoxic environments where the bioavailability of Hg is a key factor for the production of methylmercury (MeHg) by microorganisms. Dissolved organic matter (DOM) is known to affect the formation, aggregation, and dissolution of HgS particles; however the connection of these processes to Hg bioavailability is not well understood. The objectives of this study were to gain insights into the molecular structure and aggregation properties of nanoscale HgS particles that were formed and aged in the presence of DOM and to link this information to bioavailability for methylating bacteria. Characterization of nanoscale HgS was performed with a series of techniques including transmission electron microscopy, photon scattering, X-ray diffraction, and X-ray absorption spectroscopy. The characterization results indicated that the HgS precipitates formed were metacinnabar-like spherical nanoparticles that were 3-5. nm in diameter. Over the course of the aging process, HgS nanoparticles (nano-HgS) agglomerated to form mass-fractal aggregates, although the size of each primary particle within the aggregates remained unchanged. Furthermore, the crystallinity of nano-HgS increased as the particles aged. The methylation potential of nano-HgS by sulfate-reducing bacteria decreased during the aging process. No clear correlation was observed between the net productions of MeHg and the concentrations of dissolved Hg(II) in the culture media, suggesting that the decrease in the methylation potential of aged nano-HgS was not simply because of the slower supply of dissolved Hg(II) by nano-HgS. While the link between the aging of nano-HgS and decrease of methylation potential is not fully understood, the results of our study indicate that freshly formed HgS particles in DOM-rich water will include a variety of nanoscale structures that have a wide range of methylation potentials. This knowledge provides a basis for better prediction of mercury bioavailability and MeHg production in contaminated environments. © 2014 Elsevier Ltd.</style></abstract><notes><style face="normal" font="default" size="100%">cited By 24</style></notes></record><record><source-app name="Biblio" version="7.x">Drupal-Biblio</source-app><ref-type>17</ref-type><contributors><authors><author><style face="normal" font="default" size="100%">Pham, A.L.T.</style></author><author><style face="normal" font="default" size="100%">Sedlak, D.L.</style></author><author><style face="normal" font="default" size="100%">Doyle, F.M.</style></author></authors></contributors><titles><title><style face="normal" font="default" size="100%">Dissolution of mesoporous silica supports in aqueous solutions: Implications for mesoporous silica-based water treatment processes</style></title><secondary-title><style face="normal" font="default" size="100%">Applied Catalysis B: Environmental</style></secondary-title></titles><keywords><keyword><style  face="normal" font="default" size="100%">Advanced Oxidation Processes</style></keyword><keyword><style  face="normal" font="default" size="100%">Alkaline pH</style></keyword><keyword><style  face="normal" font="default" size="100%">Alkalinity</style></keyword><keyword><style  face="normal" font="default" size="100%">Batch experiments</style></keyword><keyword><style  face="normal" font="default" size="100%">Catalytic active sites</style></keyword><keyword><style  face="normal" font="default" size="100%">Column experiments</style></keyword><keyword><style  face="normal" font="default" size="100%">Dissolution</style></keyword><keyword><style  face="normal" font="default" size="100%">Dissolved silica</style></keyword><keyword><style  face="normal" font="default" size="100%">Experiments</style></keyword><keyword><style  face="normal" font="default" size="100%">Fenton reactions</style></keyword><keyword><style  face="normal" font="default" size="100%">Functionalized SBA-15</style></keyword><keyword><style  face="normal" font="default" size="100%">Hydrogen peroxide</style></keyword><keyword><style  face="normal" font="default" size="100%">Initial mass</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron oxides</style></keyword><keyword><style  face="normal" font="default" size="100%">Mesoporous</style></keyword><keyword><style  face="normal" font="default" size="100%">Mesoporous materials</style></keyword><keyword><style  face="normal" font="default" size="100%">Mesoporous Silica</style></keyword><keyword><style  face="normal" font="default" size="100%">Mesoporous silica materials</style></keyword><keyword><style  face="normal" font="default" size="100%">Metallic compounds</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxide surface</style></keyword><keyword><style  face="normal" font="default" size="100%">Silica</style></keyword><keyword><style  face="normal" font="default" size="100%">Silica dissolution</style></keyword><keyword><style  face="normal" font="default" size="100%">Solutions</style></keyword><keyword><style  face="normal" font="default" size="100%">Water treatment process</style></keyword></keywords><dates><year><style  face="normal" font="default" size="100%">2012</style></year></dates><urls><web-urls><url><style face="normal" font="default" size="100%">https://www.scopus.com/inward/record.uri?eid=2-s2.0-84864817642&amp;doi=10.1016%2fj.apcatb.2012.07.018&amp;partnerID=40&amp;md5=d5d016655ea33a833d45dd210cca2f1b</style></url></web-urls></urls><volume><style face="normal" font="default" size="100%">126</style></volume><pages><style face="normal" font="default" size="100%">258-264</style></pages><language><style face="normal" font="default" size="100%">eng</style></language><abstract><style face="normal" font="default" size="100%">Under pH 7-10 conditions, the mesoporous silica supports proposed for use in water treatment are relatively unstable. In batch experiments conducted in pH 7 solutions, the commonly used support SBA-15 dissolved quickly, releasing approximately 30mg/L of dissolved silica after 2h. In column experiments, more than 45% of an initial mass of 0.25g SBA-15 dissolved within 2 days when a pH 8.5 solution flowed through the column. In a mixed iron oxide/SBA-15 system, the dissolution of SBA-15 changed the iron oxide reactivity toward H 2O 2 decomposition, because dissolved silica deposited on iron oxide surface and changed its catalytic active sites. As with SBA-15, other mesoporous silica materials including HMS, MCM-41, four types of functionalized SBA-15, and two types of metal oxide-containing SBA-15 also dissolved under circumneutral pH solutions. The dissolution of mesoporous silica materials raises questions about their use under neutral and alkaline pH in aqueous solutions, because silica dissolution might compromise the behavior of the material. © 2012 Elsevier B.V.</style></abstract><notes><style face="normal" font="default" size="100%">cited By 26</style></notes></record><record><source-app name="Biblio" version="7.x">Drupal-Biblio</source-app><ref-type>17</ref-type><contributors><authors><author><style face="normal" font="default" size="100%">Pham, A.L.-T.</style></author><author><style face="normal" font="default" size="100%">Doyle, F.M.</style></author><author><style face="normal" font="default" size="100%">Sedlak, D.L.</style></author></authors></contributors><titles><title><style face="normal" font="default" size="100%">Inhibitory effect of dissolved silica on H 2O 2 decomposition by iron(III) and manganese(IV) oxides: Implications for H 2O 2-based in situ chemical oxidation</style></title><secondary-title><style face="normal" font="default" size="100%">Environmental Science &amp; Technology</style></secondary-title></titles><keywords><keyword><style  face="normal" font="default" size="100%">adsorption</style></keyword><keyword><style  face="normal" font="default" size="100%">Advanced Oxidation Processes</style></keyword><keyword><style  face="normal" font="default" size="100%">Amorphous iron</style></keyword><keyword><style  face="normal" font="default" size="100%">Article</style></keyword><keyword><style  face="normal" font="default" size="100%">bioremediation</style></keyword><keyword><style  face="normal" font="default" size="100%">catalysis</style></keyword><keyword><style  face="normal" font="default" size="100%">catalyst</style></keyword><keyword><style  face="normal" font="default" size="100%">Catalytic sites</style></keyword><keyword><style  face="normal" font="default" size="100%">Chemical</style></keyword><keyword><style  face="normal" font="default" size="100%">Chemicals removal (water treatment)</style></keyword><keyword><style  face="normal" font="default" size="100%">Clay minerals</style></keyword><keyword><style  face="normal" font="default" size="100%">concentration (composition)</style></keyword><keyword><style  face="normal" font="default" size="100%">controlled study</style></keyword><keyword><style  face="normal" font="default" size="100%">decomposition</style></keyword><keyword><style  face="normal" font="default" size="100%">Dissolution</style></keyword><keyword><style  face="normal" font="default" size="100%">dissolved load</style></keyword><keyword><style  face="normal" font="default" size="100%">Dissolved silica</style></keyword><keyword><style  face="normal" font="default" size="100%">Ferric Compounds</style></keyword><keyword><style  face="normal" font="default" size="100%">ferric hydroxide</style></keyword><keyword><style  face="normal" font="default" size="100%">ferric oxide</style></keyword><keyword><style  face="normal" font="default" size="100%">ground water</style></keyword><keyword><style  face="normal" font="default" size="100%">Groundwater</style></keyword><keyword><style  face="normal" font="default" size="100%">Hydrogen peroxide</style></keyword><keyword><style  face="normal" font="default" size="100%">hydroxyl group</style></keyword><keyword><style  face="normal" font="default" size="100%">hydroxyl radical</style></keyword><keyword><style  face="normal" font="default" size="100%">In-situ</style></keyword><keyword><style  face="normal" font="default" size="100%">inhibitor</style></keyword><keyword><style  face="normal" font="default" size="100%">Inhibitory effect</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron compounds</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron minerals</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron ores</style></keyword><keyword><style  face="normal" font="default" size="100%">iron oxide</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron oxides</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron-coated sands</style></keyword><keyword><style  face="normal" font="default" size="100%">Loss rates</style></keyword><keyword><style  face="normal" font="default" size="100%">Manganese</style></keyword><keyword><style  face="normal" font="default" size="100%">Manganese Compounds</style></keyword><keyword><style  face="normal" font="default" size="100%">Manganese oxide</style></keyword><keyword><style  face="normal" font="default" size="100%">mineral</style></keyword><keyword><style  face="normal" font="default" size="100%">Minerals</style></keyword><keyword><style  face="normal" font="default" size="100%">montmorillonite</style></keyword><keyword><style  face="normal" font="default" size="100%">Natural waters</style></keyword><keyword><style  face="normal" font="default" size="100%">Oh yields</style></keyword><keyword><style  face="normal" font="default" size="100%">Organic Chemicals</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxidation</style></keyword><keyword><style  face="normal" font="default" size="100%">oxidation kinetics</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxidation-Reduction</style></keyword><keyword><style  face="normal" font="default" size="100%">oxide</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxides</style></keyword><keyword><style  face="normal" font="default" size="100%">pH measurement</style></keyword><keyword><style  face="normal" font="default" size="100%">pH value</style></keyword><keyword><style  face="normal" font="default" size="100%">pollution effect</style></keyword><keyword><style  face="normal" font="default" size="100%">Remediation</style></keyword><keyword><style  face="normal" font="default" size="100%">sand</style></keyword><keyword><style  face="normal" font="default" size="100%">Silica</style></keyword><keyword><style  face="normal" font="default" size="100%">silicate</style></keyword><keyword><style  face="normal" font="default" size="100%">Silicon compounds</style></keyword><keyword><style  face="normal" font="default" size="100%">silicon dioxide</style></keyword><keyword><style  face="normal" font="default" size="100%">Soil</style></keyword><keyword><style  face="normal" font="default" size="100%">Soil and groundwater remediation</style></keyword><keyword><style  face="normal" font="default" size="100%">Soil Pollutants</style></keyword><keyword><style  face="normal" font="default" size="100%">soil treatment</style></keyword><keyword><style  face="normal" font="default" size="100%">Strong oxidants</style></keyword><keyword><style  face="normal" font="default" size="100%">Treatment systems</style></keyword><keyword><style  face="normal" font="default" size="100%">Utilization efficiency</style></keyword><keyword><style  face="normal" font="default" size="100%">Waste treatment</style></keyword><keyword><style  face="normal" font="default" size="100%">wastewater</style></keyword><keyword><style  face="normal" font="default" size="100%">water management</style></keyword><keyword><style  face="normal" font="default" size="100%">Water Pollutants</style></keyword><keyword><style  face="normal" font="default" size="100%">Water treatment</style></keyword></keywords><dates><year><style  face="normal" font="default" size="100%">2012</style></year></dates><urls><web-urls><url><style face="normal" font="default" size="100%">https://www.scopus.com/inward/record.uri?eid=2-s2.0-84855926379&amp;doi=10.1021%2fes203612d&amp;partnerID=40&amp;md5=a448282acf793b86c9a95f87e5bd36b8</style></url></web-urls></urls><number><style face="normal" font="default" size="100%">2</style></number><volume><style face="normal" font="default" size="100%">46</style></volume><pages><style face="normal" font="default" size="100%">1055-1062</style></pages><language><style face="normal" font="default" size="100%">eng</style></language><abstract><style face="normal" font="default" size="100%">The decomposition of H 2O 2 on iron minerals can generate •OH, a strong oxidant that can transform a wide range of contaminants. This reaction is critical to In Situ Chemical Oxidation (ISCO) processes used for soil and groundwater remediation, as well as advanced oxidation processes employed in waste treatment systems. The presence of dissolved silica at concentrations comparable to those encountered in natural waters decreases the reactivity of iron minerals toward H 2O 2, because silica adsorbs onto the surface of iron minerals and alters catalytic sites. At circumneutral pH values, goethite, amorphous iron oxide, hematite, iron-coated sand, and montmorillonite that were pre-equilibrated with 0.05-1.5 mM SiO 2 were significantly less reactive toward H 2O 2 decomposition than their original counterparts, with the H 2O 2 loss rates inversely proportional to SiO 2 concentrations. In the goethite/H 2O 2 system, the overall •OH yield, defined as the percentage of decomposed H 2O 2 producing •OH, was almost halved in the presence of 1.5 mM SiO 2. Dissolved SiO 2 also slowed H 2O 2 decomposition on manganese(IV) oxide. The presence of dissolved SiO 2 results in greater persistence of H 2O 2 in groundwater and lower H 2O 2 utilization efficiency and should be considered in the design of H 2O 2-based treatment systems. © 2011 American Chemical Society.</style></abstract><notes><style face="normal" font="default" size="100%">cited By 44</style></notes></record><record><source-app name="Biblio" version="7.x">Drupal-Biblio</source-app><ref-type>17</ref-type><contributors><authors><author><style face="normal" font="default" size="100%">Pham, A.L.T.</style></author><author><style face="normal" font="default" size="100%">Doyle, F.M.</style></author><author><style face="normal" font="default" size="100%">Sedlak, D.L.</style></author></authors></contributors><titles><title><style face="normal" font="default" size="100%">Kinetics and efficiency of H 2O 2 activation by iron-containing minerals and aquifer materials</style></title><secondary-title><style face="normal" font="default" size="100%">Water Research</style></secondary-title></titles><keywords><keyword><style  face="normal" font="default" size="100%">Advanced Oxidation Processes</style></keyword><keyword><style  face="normal" font="default" size="100%">aquifer</style></keyword><keyword><style  face="normal" font="default" size="100%">Aquifer materials</style></keyword><keyword><style  face="normal" font="default" size="100%">Aquifers</style></keyword><keyword><style  face="normal" font="default" size="100%">Article</style></keyword><keyword><style  face="normal" font="default" size="100%">bicarbonate</style></keyword><keyword><style  face="normal" font="default" size="100%">catalyst</style></keyword><keyword><style  face="normal" font="default" size="100%">Chemical</style></keyword><keyword><style  face="normal" font="default" size="100%">chemical reaction</style></keyword><keyword><style  face="normal" font="default" size="100%">chemistry</style></keyword><keyword><style  face="normal" font="default" size="100%">citric acid</style></keyword><keyword><style  face="normal" font="default" size="100%">clay</style></keyword><keyword><style  face="normal" font="default" size="100%">decomposition</style></keyword><keyword><style  face="normal" font="default" size="100%">Dissolved silica</style></keyword><keyword><style  face="normal" font="default" size="100%">dithionite</style></keyword><keyword><style  face="normal" font="default" size="100%">ecosystem restoration</style></keyword><keyword><style  face="normal" font="default" size="100%">Efficiency</style></keyword><keyword><style  face="normal" font="default" size="100%">Environmental Remediation</style></keyword><keyword><style  face="normal" font="default" size="100%">Fenton reactions</style></keyword><keyword><style  face="normal" font="default" size="100%">Ferric Compounds</style></keyword><keyword><style  face="normal" font="default" size="100%">ferric ion</style></keyword><keyword><style  face="normal" font="default" size="100%">ferric oxide</style></keyword><keyword><style  face="normal" font="default" size="100%">Gain insight</style></keyword><keyword><style  face="normal" font="default" size="100%">ground water</style></keyword><keyword><style  face="normal" font="default" size="100%">Groundwater</style></keyword><keyword><style  face="normal" font="default" size="100%">Groundwater resources</style></keyword><keyword><style  face="normal" font="default" size="100%">Groundwater treatment</style></keyword><keyword><style  face="normal" font="default" size="100%">Hydrogen peroxide</style></keyword><keyword><style  face="normal" font="default" size="100%">Hydrogen-Ion Concentration</style></keyword><keyword><style  face="normal" font="default" size="100%">hydroxyl radical</style></keyword><keyword><style  face="normal" font="default" size="100%">in situ measurement</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron</style></keyword><keyword><style  face="normal" font="default" size="100%">iron oxide</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron oxides</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron-containing catalyst</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron-containing clays</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron-containing minerals</style></keyword><keyword><style  face="normal" font="default" size="100%">Kinetics</style></keyword><keyword><style  face="normal" font="default" size="100%">Manganese</style></keyword><keyword><style  face="normal" font="default" size="100%">Manganese Compounds</style></keyword><keyword><style  face="normal" font="default" size="100%">manganese derivative</style></keyword><keyword><style  face="normal" font="default" size="100%">Manganese oxide</style></keyword><keyword><style  face="normal" font="default" size="100%">Manganese oxide coating</style></keyword><keyword><style  face="normal" font="default" size="100%">Materials</style></keyword><keyword><style  face="normal" font="default" size="100%">methodology</style></keyword><keyword><style  face="normal" font="default" size="100%">mineral</style></keyword><keyword><style  face="normal" font="default" size="100%">Minerals</style></keyword><keyword><style  face="normal" font="default" size="100%">Mn content</style></keyword><keyword><style  face="normal" font="default" size="100%">Oh yields</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxidation</style></keyword><keyword><style  face="normal" font="default" size="100%">oxidation reduction reaction</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxidation-Reduction</style></keyword><keyword><style  face="normal" font="default" size="100%">oxide</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxides</style></keyword><keyword><style  face="normal" font="default" size="100%">pH</style></keyword><keyword><style  face="normal" font="default" size="100%">phenol</style></keyword><keyword><style  face="normal" font="default" size="100%">phenol derivative</style></keyword><keyword><style  face="normal" font="default" size="100%">Phenols</style></keyword><keyword><style  face="normal" font="default" size="100%">pollutant removal</style></keyword><keyword><style  face="normal" font="default" size="100%">priority journal</style></keyword><keyword><style  face="normal" font="default" size="100%">process optimization</style></keyword><keyword><style  face="normal" font="default" size="100%">Protective coatings</style></keyword><keyword><style  face="normal" font="default" size="100%">reaction kinetics</style></keyword><keyword><style  face="normal" font="default" size="100%">Silica</style></keyword><keyword><style  face="normal" font="default" size="100%">silicon dioxide</style></keyword><keyword><style  face="normal" font="default" size="100%">Situ chemical oxidation</style></keyword><keyword><style  face="normal" font="default" size="100%">soil pollutant</style></keyword><keyword><style  face="normal" font="default" size="100%">Soil Pollutants</style></keyword><keyword><style  face="normal" font="default" size="100%">stoichiometry</style></keyword><keyword><style  face="normal" font="default" size="100%">United States</style></keyword><keyword><style  face="normal" font="default" size="100%">waste component removal</style></keyword><keyword><style  face="normal" font="default" size="100%">water pollutant</style></keyword><keyword><style  face="normal" font="default" size="100%">Water Pollutants</style></keyword><keyword><style  face="normal" font="default" size="100%">Water treatment</style></keyword></keywords><dates><year><style  face="normal" font="default" size="100%">2012</style></year></dates><urls><web-urls><url><style face="normal" font="default" size="100%">https://www.scopus.com/inward/record.uri?eid=2-s2.0-84868303803&amp;doi=10.1016%2fj.watres.2012.09.020&amp;partnerID=40&amp;md5=de296bdabf6181c9d7c93b936e0fe754</style></url></web-urls></urls><number><style face="normal" font="default" size="100%">19</style></number><volume><style face="normal" font="default" size="100%">46</style></volume><pages><style face="normal" font="default" size="100%">6454-6462</style></pages><language><style face="normal" font="default" size="100%">eng</style></language><abstract><style face="normal" font="default" size="100%">To gain insight into factors that control H 2O 2 persistence and OH yield in H 2O 2-based in situ chemical oxidation systems, the decomposition of H 2O 2 and transformation of phenol were investigated in the presence of iron-containing minerals and aquifer materials. Under conditions expected during remediation of soil and groundwater, the stoichiometric efficiency, defined as the amount of phenol transformed per mole of H 2O 2 decomposed, varied from 0.005 to 0.28%. Among the iron-containing minerals, iron oxides were 2-10 times less efficient in transforming phenol than iron-containing clays and synthetic iron-containing catalysts. In both iron-containing mineral and aquifer materials systems, the stoichiometric efficiency was inversely correlated with the rate of H 2O 2 decomposition. In aquifer materials systems, the stoichiometric efficiency was also inversely correlated with the Mn content, consistent with the fact that the decomposition of H 2O 2 on manganese oxides does not produce OH. Removal of iron and manganese oxide coatings from the surface of aquifer materials by extraction with citrate-bicarbonate-dithionite slowed the rate of H 2O 2 decomposition on aquifer materials and increased the stoichiometric efficiency. In addition, the presence of 2 mM of dissolved SiO 2 slowed the rate of H 2O 2 decomposition on aquifer materials by over 80% without affecting the stoichiometric efficiency. © 2012 Elsevier Ltd.</style></abstract><notes><style face="normal" font="default" size="100%">cited By 46</style></notes></record><record><source-app name="Biblio" version="7.x">Drupal-Biblio</source-app><ref-type>47</ref-type><contributors><authors><author><style face="normal" font="default" size="100%">Pham, A.L.-T.</style></author><author><style face="normal" font="default" size="100%">Sedlak, D.L.</style></author><author><style face="normal" font="default" size="100%">Doyle, F.M.</style></author></authors></contributors><titles><title><style face="normal" font="default" size="100%">Production of oxidizing intermediates during corrosion of iron; implications for remediation of contaminants from mineral and metal processing</style></title><secondary-title><style face="normal" font="default" size="100%">ECS Transactions</style></secondary-title></titles><keywords><keyword><style  face="normal" font="default" size="100%">Bulk iron</style></keyword><keyword><style  face="normal" font="default" size="100%">Corrosion</style></keyword><keyword><style  face="normal" font="default" size="100%">Corrosion behavior</style></keyword><keyword><style  face="normal" font="default" size="100%">Dissolved metals</style></keyword><keyword><style  face="normal" font="default" size="100%">Electrochemistry</style></keyword><keyword><style  face="normal" font="default" size="100%">Electrolytic iron</style></keyword><keyword><style  face="normal" font="default" size="100%">Elemental iron</style></keyword><keyword><style  face="normal" font="default" size="100%">Fenton's reagents</style></keyword><keyword><style  face="normal" font="default" size="100%">History of use</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron deposits</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron powder</style></keyword><keyword><style  face="normal" font="default" size="100%">Metal processing</style></keyword><keyword><style  face="normal" font="default" size="100%">Metal recovery</style></keyword><keyword><style  face="normal" font="default" size="100%">Metals</style></keyword><keyword><style  face="normal" font="default" size="100%">Mineral processing</style></keyword><keyword><style  face="normal" font="default" size="100%">Minerals</style></keyword><keyword><style  face="normal" font="default" size="100%">Nano particulates</style></keyword><keyword><style  face="normal" font="default" size="100%">Near-neutral pH</style></keyword><keyword><style  face="normal" font="default" size="100%">Ore bodies</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxidants</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxidation</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxidation reactions</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxygen</style></keyword><keyword><style  face="normal" font="default" size="100%">Packed powder</style></keyword><keyword><style  face="normal" font="default" size="100%">Rotating disk electrodes</style></keyword><keyword><style  face="normal" font="default" size="100%">Rotating disks</style></keyword><keyword><style  face="normal" font="default" size="100%">Silicate minerals</style></keyword><keyword><style  face="normal" font="default" size="100%">Steel powder metallurgy</style></keyword></keywords><dates><year><style  face="normal" font="default" size="100%">2010</style></year></dates><urls><web-urls><url><style face="normal" font="default" size="100%">https://www.scopus.com/inward/record.uri?eid=2-s2.0-78649669796&amp;doi=10.1149%2f1.3367907&amp;partnerID=40&amp;md5=7a82a06bc9058bf9438982ebeb4705fb</style></url></web-urls></urls><number><style face="normal" font="default" size="100%">6</style></number><pub-location><style face="normal" font="default" size="100%">Vancouver, BC</style></pub-location><volume><style face="normal" font="default" size="100%">28</style></volume><pages><style face="normal" font="default" size="100%">117-127</style></pages><isbn><style face="normal" font="default" size="100%">9781566777964</style></isbn><language><style face="normal" font="default" size="100%">eng</style></language><abstract><style face="normal" font="default" size="100%">Elemental iron has a long history of use for reductive recovery of dissolved metals from waters associated with ore bodies, mining and mineral processing activities. It has recently been recognized that Fenton's reagent, which generates powerful oxidants, may be generated when iron corrodes in the presence of oxygen. If the iron is nanoparticulate, enough oxidant may be generated for practical applications. However, there is ample indication in the literature that oxidation reactions on iron at near-neutral pH are strongly sensitive to the source of the iron, which affects the surface. This was investigated here for electrolytic iron powder, and two types of nanoparticulate iron, using a modified packed powder electrode. The behavior of bulk iron was investigated using a rotating disk electrode. The results revealed significant differences in the corrosion behavior of the different iron samples, indicating that these would yield significantly different results if employed for oxidation reactions. © The Electrochemical Society.</style></abstract><notes><style face="normal" font="default" size="100%">cited By 0; Conference of 8th International Symposium on Electrochemistry in Mineral and Metal Processing - 217th ECS Meeting ; Conference Date: 26 April 2010 Through 28 April 2010; Conference Code:82642</style></notes></record><record><source-app name="Biblio" version="7.x">Drupal-Biblio</source-app><ref-type>17</ref-type><contributors><authors><author><style face="normal" font="default" size="100%">Pham, A.L.-T.</style></author><author><style face="normal" font="default" size="100%">Lee, C.</style></author><author><style face="normal" font="default" size="100%">Doyle, F.M.</style></author><author><style face="normal" font="default" size="100%">Sedlak, D.L.</style></author></authors></contributors><titles><title><style face="normal" font="default" size="100%">A silica-supported iron oxide catalyst capable of activating hydrogen peroxide at neutral pH values</style></title><secondary-title><style face="normal" font="default" size="100%">Environmental Science &amp; Technology</style></secondary-title></titles><keywords><keyword><style  face="normal" font="default" size="100%">Alumina</style></keyword><keyword><style  face="normal" font="default" size="100%">aluminum chloride</style></keyword><keyword><style  face="normal" font="default" size="100%">aluminum oxide</style></keyword><keyword><style  face="normal" font="default" size="100%">aqueous solution</style></keyword><keyword><style  face="normal" font="default" size="100%">Aqueous solutions</style></keyword><keyword><style  face="normal" font="default" size="100%">Article</style></keyword><keyword><style  face="normal" font="default" size="100%">catalysis</style></keyword><keyword><style  face="normal" font="default" size="100%">catalyst</style></keyword><keyword><style  face="normal" font="default" size="100%">Catalysts</style></keyword><keyword><style  face="normal" font="default" size="100%">Chemical</style></keyword><keyword><style  face="normal" font="default" size="100%">controlled study</style></keyword><keyword><style  face="normal" font="default" size="100%">decomposition</style></keyword><keyword><style  face="normal" font="default" size="100%">Electron</style></keyword><keyword><style  face="normal" font="default" size="100%">Ferric Compounds</style></keyword><keyword><style  face="normal" font="default" size="100%">Hydrogen peroxide</style></keyword><keyword><style  face="normal" font="default" size="100%">Hydrogen-Ion Concentration</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron ores</style></keyword><keyword><style  face="normal" font="default" size="100%">iron oxide</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron oxide catalyst</style></keyword><keyword><style  face="normal" font="default" size="100%">Iron oxides</style></keyword><keyword><style  face="normal" font="default" size="100%">Microscopy</style></keyword><keyword><style  face="normal" font="default" size="100%">Mixed oxide</style></keyword><keyword><style  face="normal" font="default" size="100%">Models</style></keyword><keyword><style  face="normal" font="default" size="100%">Neutral pH</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxidant production</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxidants</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxidation</style></keyword><keyword><style  face="normal" font="default" size="100%">oxidation reduction reaction</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxidation-Reduction</style></keyword><keyword><style  face="normal" font="default" size="100%">Oxide minerals</style></keyword><keyword><style  face="normal" font="default" size="100%">oxidizing agent</style></keyword><keyword><style  face="normal" font="default" size="100%">pH</style></keyword><keyword><style  face="normal" font="default" size="100%">pH effects</style></keyword><keyword><style  face="normal" font="default" size="100%">pH measurement</style></keyword><keyword><style  face="normal" font="default" size="100%">pH value</style></keyword><keyword><style  face="normal" font="default" size="100%">phenol</style></keyword><keyword><style  face="normal" font="default" size="100%">Phenols</style></keyword><keyword><style  face="normal" font="default" size="100%">redox conditions</style></keyword><keyword><style  face="normal" font="default" size="100%">Scanning</style></keyword><keyword><style  face="normal" font="default" size="100%">Silica</style></keyword><keyword><style  face="normal" font="default" size="100%">Silica-alumina</style></keyword><keyword><style  face="normal" font="default" size="100%">silicon dioxide</style></keyword><keyword><style  face="normal" font="default" size="100%">Sol-gel process</style></keyword><keyword><style  face="normal" font="default" size="100%">Sol-Gel processing</style></keyword><keyword><style  face="normal" font="default" size="100%">stoichiometry</style></keyword><keyword><style  face="normal" font="default" size="100%">Strong oxidants</style></keyword><keyword><style  face="normal" font="default" size="100%">Surface Properties</style></keyword><keyword><style  face="normal" font="default" size="100%">Surface redox process</style></keyword><keyword><style  face="normal" font="default" size="100%">Tetra-ethyl-ortho-silicate</style></keyword><keyword><style  face="normal" font="default" size="100%">tetraethoxysilane</style></keyword><keyword><style  face="normal" font="default" size="100%">X-Ray Diffraction</style></keyword></keywords><dates><year><style  face="normal" font="default" size="100%">2009</style></year></dates><urls><web-urls><url><style face="normal" font="default" size="100%">https://www.scopus.com/inward/record.uri?eid=2-s2.0-72249112169&amp;doi=10.1021%2fes902296k&amp;partnerID=40&amp;md5=ee0448400897e1bc687218af328296c0</style></url></web-urls></urls><number><style face="normal" font="default" size="100%">23</style></number><volume><style face="normal" font="default" size="100%">43</style></volume><pages><style face="normal" font="default" size="100%">8930-8935</style></pages><language><style face="normal" font="default" size="100%">eng</style></language><abstract><style face="normal" font="default" size="100%">Iron oxides catalyze the conversion of hydrogen peroxide (H 2O2) into oxidants capable of transforming recalcitrant contaminants. Unfortunately, the process is relatively inefficient at circumneutral pH values because of competing reactions that decompose H 2O2 without producing oxidants. Silica- and alumina-containing iron oxides prepared by sol-gel processing of aqueous solutions containing Fe(ClO4)3, AlCl3, and tetraethyl orthosilicate efficiently catalyzed the decomposition of H 2O2 into oxidants capable of transforming phenol at circumneutral pH values. Relative to hematite, goethite, and amorphous FeOOH, the silica-iron oxide catalyst exhibited a stoichiometric efficiency, defined as the number of moles of phenol transformed per mole of H2O 2 consumed, which was 10-40 times higher than that of the iron oxides. The silica-alumina-iron oxide catalyst had a stoichiometric efficiency that was 50-80 times higher than that of the iron oxides. The significant enhancement in oxidant production is attributable to the interaction of Fe with Al and Si in the mixed oxides, which alters the surface redox processes, favoring the production of strong oxidants during H2O2 decomposition. © 2009 American Chemical Society.</style></abstract><notes><style face="normal" font="default" size="100%">cited By 203</style></notes></record></records></xml>