It is shown that the electrolytic oxidation of three terpene hydrocarbons, namely, α‐pinene, terpinolene and dipentene, can be carried out efficiently at a lead dioxide anode in dilute aqueous sulfuric acid as electrolyte. The addition of an emulsifying agent is not necessary, provided mechanical emulsification is maintained by agitation. The efficiency of oxidation is increased by raising the temperature, but is markedly decreased by making the electrolyte neutral or alkaline. Inorganic oxygen carriers, e.g., ceric ions, increase the current efficiency for the oxidation of the terpene hydrocarbons.
{"title":"The Electrolytic Oxidation of α‐Pinene, Terpinolene and Dipentene","authors":"S. Glasstone, H. Stanley","doi":"10.1149/1.3071823","DOIUrl":"https://doi.org/10.1149/1.3071823","url":null,"abstract":"It is shown that the electrolytic oxidation of three terpene hydrocarbons, namely, α‐pinene, terpinolene and dipentene, can be carried out efficiently at a lead dioxide anode in dilute aqueous sulfuric acid as electrolyte. The addition of an emulsifying agent is not necessary, provided mechanical emulsification is maintained by agitation. The efficiency of oxidation is increased by raising the temperature, but is markedly decreased by making the electrolyte neutral or alkaline. Inorganic oxygen carriers, e.g., ceric ions, increase the current efficiency for the oxidation of the terpene hydrocarbons.","PeriodicalId":118206,"journal":{"name":"Transactions of the Electrochemical Society","volume":"1 1","pages":"0"},"PeriodicalIF":0.0,"publicationDate":"1947-10-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"125817051","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
{"title":"Self Discharge in Lead‐Acid Storage Batteries","authors":"A. C. Zachlin","doi":"10.1149/1.3071819","DOIUrl":"https://doi.org/10.1149/1.3071819","url":null,"abstract":"","PeriodicalId":118206,"journal":{"name":"Transactions of the Electrochemical Society","volume":"14 1","pages":"0"},"PeriodicalIF":0.0,"publicationDate":"1947-10-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"121230636","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
A continuous process has been developed for the electrolytic reduction of acetone to pinacol which upon dehydration is converted to 2, 3‐di‐ methyl butadiene. The following observations were made during this investigation: (1) The process consists of electrolyzing a 4/1 acetone‐20% sulfuric acid mixture maintained at 15° to 20° C in the cathode compartment of a metal‐free electrolytic cell with a newly developed lead‐deposited copper cathode at a c. d. of one amp./dm.2 of effective cathode surface. Using these operating conditions in a 267‐1/3 hour continuous run, the acetone to the extent of 10% to 20% conversion was reduced to pinacol hydrate (50% to 55% current efficiency), isopropyl alcohol, and propane in approximate mol ratio of 16.8/2/1; 60% of the acetone converted going to pinacol. (2) In order to maintain the high 50% to 55% pinacol current efficiency, it was found necessary to renew the cathodes with fresh ones once every 24 hour period of operation. However, the cathodes are easily prepared by electrodepositing a relatively thin film of lead on a copper surface. (3) Studies made with numerous alternate type of cathodes indicated that zirconium‐deposited copper is the only other one that shows any promise.
{"title":"Electrolytic Reduction of Acetone to Pinacol","authors":"O. Slotterbeck","doi":"10.1149/1.3071827","DOIUrl":"https://doi.org/10.1149/1.3071827","url":null,"abstract":"A continuous process has been developed for the electrolytic reduction of acetone to pinacol which upon dehydration is converted to 2, 3‐di‐ methyl butadiene. The following observations were made during this investigation: (1) The process consists of electrolyzing a 4/1 acetone‐20% sulfuric acid mixture maintained at 15° to 20° C in the cathode compartment of a metal‐free electrolytic cell with a newly developed lead‐deposited copper cathode at a c. d. of one amp./dm.2 of effective cathode surface. Using these operating conditions in a 267‐1/3 hour continuous run, the acetone to the extent of 10% to 20% conversion was reduced to pinacol hydrate (50% to 55% current efficiency), isopropyl alcohol, and propane in approximate mol ratio of 16.8/2/1; 60% of the acetone converted going to pinacol. (2) In order to maintain the high 50% to 55% pinacol current efficiency, it was found necessary to renew the cathodes with fresh ones once every 24 hour period of operation. However, the cathodes are easily prepared by electrodepositing a relatively thin film of lead on a copper surface. (3) Studies made with numerous alternate type of cathodes indicated that zirconium‐deposited copper is the only other one that shows any promise.","PeriodicalId":118206,"journal":{"name":"Transactions of the Electrochemical Society","volume":"7 1","pages":"0"},"PeriodicalIF":0.0,"publicationDate":"1947-10-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"127429263","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
{"title":"The Rate of Oxygen Absorption by Alpha Ray Cuprene","authors":"G. Glockler, C. A. Hollingsworth","doi":"10.1149/1.3071829","DOIUrl":"https://doi.org/10.1149/1.3071829","url":null,"abstract":"","PeriodicalId":118206,"journal":{"name":"Transactions of the Electrochemical Society","volume":"41 1","pages":"0"},"PeriodicalIF":0.0,"publicationDate":"1947-10-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"132880470","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
W. Kroll, A. W. Schlechten, W. Carmody, L. Yerkes, H. P. Holmes, H. Gilbert
{"title":"Recent Progress in The Metallurgy of Malleable Zirconium","authors":"W. Kroll, A. W. Schlechten, W. Carmody, L. Yerkes, H. P. Holmes, H. Gilbert","doi":"10.1149/1.3071808","DOIUrl":"https://doi.org/10.1149/1.3071808","url":null,"abstract":"","PeriodicalId":118206,"journal":{"name":"Transactions of the Electrochemical Society","volume":"10 1","pages":"0"},"PeriodicalIF":0.0,"publicationDate":"1947-10-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"133332003","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
{"title":"The Electrolytic Reduction of Carbonyl Compounds at Carbon Cathodes","authors":"Sherlock Swann, H. D. Kerfman","doi":"10.1149/1.3071831","DOIUrl":"https://doi.org/10.1149/1.3071831","url":null,"abstract":"","PeriodicalId":118206,"journal":{"name":"Transactions of the Electrochemical Society","volume":"1 1","pages":"0"},"PeriodicalIF":0.0,"publicationDate":"1947-10-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"125797099","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
{"title":"A New Method for Particle Size Determination in the Sub‐Sieve Range","authors":"J. Musgrave, H. Harner","doi":"10.1149/1.3071842","DOIUrl":"https://doi.org/10.1149/1.3071842","url":null,"abstract":"","PeriodicalId":118206,"journal":{"name":"Transactions of the Electrochemical Society","volume":"1 1","pages":"0"},"PeriodicalIF":0.0,"publicationDate":"1947-10-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"121916098","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
The classical theory for the phenomenon of the "residual current" is rejected as unsatisfactory, particularly as applied to solutions of heavy metal salts. It is suggested that in such cases the residual current is due to the discharge of hydrogen ions rather than metal ions. The discharge potentials of the tetraalkyl ammonium ions from methyl to amyl have been determined and, in general, found to increase with an increase in the number of carbon atoms. The decomposition voltages of zinc chloride, mercuric bromide, cadmium bromide and silver nitrate in pyridine have been determined and compared with those obtained in aqueous solution. Existence of a complex silver anion is indicated.
{"title":"Some Observations on Decomposition Voltages","authors":"J. Bockris, S. Ignatowicz","doi":"10.1149/1.3071834","DOIUrl":"https://doi.org/10.1149/1.3071834","url":null,"abstract":"The classical theory for the phenomenon of the \"residual current\" is rejected as unsatisfactory, particularly as applied to solutions of heavy metal salts. It is suggested that in such cases the residual current is due to the discharge of hydrogen ions rather than metal ions. The discharge potentials of the tetraalkyl ammonium ions from methyl to amyl have been determined and, in general, found to increase with an increase in the number of carbon atoms. The decomposition voltages of zinc chloride, mercuric bromide, cadmium bromide and silver nitrate in pyridine have been determined and compared with those obtained in aqueous solution. Existence of a complex silver anion is indicated.","PeriodicalId":118206,"journal":{"name":"Transactions of the Electrochemical Society","volume":"27 1","pages":"0"},"PeriodicalIF":0.0,"publicationDate":"1947-10-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"122074433","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
Potentiometric titration procedure is described briefly and the application of the potentiometric method to both analytical and general research work is discussed. Instrumentation for the potentiometric titration is reviewed with particular emphasis on automatic apparatus developments tending to simplify the use of the potentiometric method. An instrument, capable of automatically performing and plotting potentiometric titrations, and adaptable to a variety of electrode systems, is described. The construction and operating principle of the instrument, as well as its calibration, method of use, and performance characteristics, are described in detail.
{"title":"Automatic Potentiometric Titrations","authors":"H. A. Robinson","doi":"10.1149/1.3071833","DOIUrl":"https://doi.org/10.1149/1.3071833","url":null,"abstract":"Potentiometric titration procedure is described briefly and the application of the potentiometric method to both analytical and general research work is discussed. Instrumentation for the potentiometric titration is reviewed with particular emphasis on automatic apparatus developments tending to simplify the use of the potentiometric method. An instrument, capable of automatically performing and plotting potentiometric titrations, and adaptable to a variety of electrode systems, is described. The construction and operating principle of the instrument, as well as its calibration, method of use, and performance characteristics, are described in detail.","PeriodicalId":118206,"journal":{"name":"Transactions of the Electrochemical Society","volume":"758 1","pages":"0"},"PeriodicalIF":0.0,"publicationDate":"1947-10-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"123279429","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
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