J. F. Read, B. Griffiths, L. Lynch, K. Maccormick, Nga Chiu Tam
{"title":"高铁酸钾氧化苯硫代乙酸和硫代二乙醇酸的动力学及机理","authors":"J. F. Read, B. Griffiths, L. Lynch, K. Maccormick, Nga Chiu Tam","doi":"10.1515/IRM.2004.5.2.135","DOIUrl":null,"url":null,"abstract":"The kinetics and mechanism of the oxidation of phenylthioacetic acid and thiodiglycolic acid by potassium ferrate were investigated under pseudo and non pseudo first-order conditions. Phenylthioacetic acid was oxidized to the sulfone and Fe(II) within 300s and thiodiglycolic acid was oxidized to the sulfoxide and Fe(III) within 1000s. Above a pH value of 8.7 for phenylthioacetic acid and 8.3 for thiodiglycolic acid the kinetics were firstorder in the concentration of the hydrogen ions, the organosulfur compound and the ferrate ions, whereas below these pH values the kinetics were independent of the hydrogen ion concentration. A possible mechanism involves reaction between protonated ferrate and the organosulfur compound as the rate-determining step with a rate constant of 35 M-1s-1. These results are comparable with other similar compounds.","PeriodicalId":8996,"journal":{"name":"BioInorganic Reaction Mechanisms","volume":"30 2 1","pages":"135 - 150"},"PeriodicalIF":0.0000,"publicationDate":"2004-01-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":"3","resultStr":"{\"title\":\"The Kinetics and Mechanism of the Oxidation of Phenylthioacetic Acid and Thiodiglycolic Acid by Potassium Ferrate\",\"authors\":\"J. F. Read, B. Griffiths, L. Lynch, K. Maccormick, Nga Chiu Tam\",\"doi\":\"10.1515/IRM.2004.5.2.135\",\"DOIUrl\":null,\"url\":null,\"abstract\":\"The kinetics and mechanism of the oxidation of phenylthioacetic acid and thiodiglycolic acid by potassium ferrate were investigated under pseudo and non pseudo first-order conditions. Phenylthioacetic acid was oxidized to the sulfone and Fe(II) within 300s and thiodiglycolic acid was oxidized to the sulfoxide and Fe(III) within 1000s. Above a pH value of 8.7 for phenylthioacetic acid and 8.3 for thiodiglycolic acid the kinetics were firstorder in the concentration of the hydrogen ions, the organosulfur compound and the ferrate ions, whereas below these pH values the kinetics were independent of the hydrogen ion concentration. A possible mechanism involves reaction between protonated ferrate and the organosulfur compound as the rate-determining step with a rate constant of 35 M-1s-1. These results are comparable with other similar compounds.\",\"PeriodicalId\":8996,\"journal\":{\"name\":\"BioInorganic Reaction Mechanisms\",\"volume\":\"30 2 1\",\"pages\":\"135 - 150\"},\"PeriodicalIF\":0.0000,\"publicationDate\":\"2004-01-01\",\"publicationTypes\":\"Journal Article\",\"fieldsOfStudy\":null,\"isOpenAccess\":false,\"openAccessPdf\":\"\",\"citationCount\":\"3\",\"resultStr\":null,\"platform\":\"Semanticscholar\",\"paperid\":null,\"PeriodicalName\":\"BioInorganic Reaction Mechanisms\",\"FirstCategoryId\":\"1085\",\"ListUrlMain\":\"https://doi.org/10.1515/IRM.2004.5.2.135\",\"RegionNum\":0,\"RegionCategory\":null,\"ArticlePicture\":[],\"TitleCN\":null,\"AbstractTextCN\":null,\"PMCID\":null,\"EPubDate\":\"\",\"PubModel\":\"\",\"JCR\":\"\",\"JCRName\":\"\",\"Score\":null,\"Total\":0}","platform":"Semanticscholar","paperid":null,"PeriodicalName":"BioInorganic Reaction Mechanisms","FirstCategoryId":"1085","ListUrlMain":"https://doi.org/10.1515/IRM.2004.5.2.135","RegionNum":0,"RegionCategory":null,"ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":null,"EPubDate":"","PubModel":"","JCR":"","JCRName":"","Score":null,"Total":0}
The Kinetics and Mechanism of the Oxidation of Phenylthioacetic Acid and Thiodiglycolic Acid by Potassium Ferrate
The kinetics and mechanism of the oxidation of phenylthioacetic acid and thiodiglycolic acid by potassium ferrate were investigated under pseudo and non pseudo first-order conditions. Phenylthioacetic acid was oxidized to the sulfone and Fe(II) within 300s and thiodiglycolic acid was oxidized to the sulfoxide and Fe(III) within 1000s. Above a pH value of 8.7 for phenylthioacetic acid and 8.3 for thiodiglycolic acid the kinetics were firstorder in the concentration of the hydrogen ions, the organosulfur compound and the ferrate ions, whereas below these pH values the kinetics were independent of the hydrogen ion concentration. A possible mechanism involves reaction between protonated ferrate and the organosulfur compound as the rate-determining step with a rate constant of 35 M-1s-1. These results are comparable with other similar compounds.
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