Kinetics and mechanisms of the oxidation of methanol and .alpha.-phenylethanol by peroxydisulfate ion

One-Electron Oxidant-Induced Transformations of Aromatic Alcohol to Ketone Moieties in Dissolved Organic Matter Increase Trichloromethane Formation

“…A typical transformation pathway from aromatic alcohols to ketones is presented in eq . SO 4 •– initiates the reactions with aromatic alcohols via single-electron oxidation to generate cation radicals. , The cation radicals undergo deprotonation to yield carbon-centered radicals, which further react with PDS (as SO 4 •– precursor) to form aromatic ketones. , Note that aromatic ketones are the intermediates and can be further degraded by SO 4 •– (Table S4). When the R group is −OH, the cation radicals of phenolic compounds (i.e., 4HPE) deprotonate to yield phenoxyl radicals, which then undergo H-abstraction or addition–elimination to form semiquinones and then rearrange to aromatic ketones (Ar–CO–CH 3 ) .…”

“…•− precursor) to form aromatic ketones. 25,26 Note that aromatic ketones are the intermediates and can be further degraded by SO 4…”

“…Meanwhile, oxygenated aliphatic compounds containing (β-di)­ketone structures also have very high CHCl 3 yields (e.g., 83% for 3-oxohexanedioic acid and 91% for 5,7-dioxooctanoic acid). ,, Due to high THM yields, oxygenated DOM moieties produced during AOP treatment may form more THM upon chlorination than their original precursors (e.g., alcohols) upon chlorination alone. For example, 1-(4-hydroxyphenyl)­ethanol (4HPE) can be transformed to 1-(4-hydroxyphenyl)­ethanone (4HPA) during SO 4 •– oxidation, , but CHCl 3 yield from 4HPA is 16 times greater than the original organic compound (4HPE) . X 2 •– and CO 3 •– may proceed via similar pathways to transform alcohols to ketones.…”

Emulsion Polymerization of Voided Particles by Encapsulation of a Nonsolvent

“…Further, the alcohol can participate in a chain transfer reaction with the growing polymer chains and an oxidation reaction with the thermal initiator, sodium persulfate. , The reaction with the thermal initiator involves the oxidation of the alcohol by a free-radical mechanism . This is a competitive reaction for the persulfate radicals.…”

A comparison of the thermal and photochemical oxidation of 2‐propanol by two peroxoanions

“…The rate constant for the photo-oxidation reaction was evaluated from the slopes of plots of In [S20,z-] against time (i.e., the part of the reaction referred to as reaction B by previous workers) [ 1,2,3,4]. The rate constants were obtained from a least-squares analysis of the data and are the average of three runs carried out after all nonrelevant factors were under control.…”