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The rates of oxygen evolution from carefully purified solutions of sodium hypochlorite have been measured. Methods of purification are described, and it is found that substantially the same rate is observed regardless of the method of purification. The rate of oxygen evolution is proportional to the square of the concentration of hypochlorite ions. The effect of temperature and ionic strength are examined. The rate constant is 7.5X1OP6 (g-rn~l/l.)-~(min)-I a t 60" C and an ionic strength of 3.5; the activation energy is 26.6 kcal/g-mol. These results are compared with the corresponding quantities for the reaction of hypochlorite ions t o form chlorite and chloride ions, and some tentative explanations are offered.In an earlier paper ( I ) , one of the present authors exa~nined the decomposition of aqueous sodium hypochlorite solutions, particularly the rate of deconlpositioil to sodiuin chlorate and chloride. The accompanying reaction giving sodiuin chloride and oxygen was exanlined more superficially. Rates of oxygen evolution were observed on a nu~nber of solutions a t that time, but it was never proved that the oxygen evolutio~l could not be ascribed to the presence of traces of catalyst. The reasons for this uilcertainty were as follows. Firstly, measurements on the catalyzed reaction (2) showed that the observed rates could be accounted for by the presence ol copper in co~lce~ltrations of the order of a pg/l. Secondly, the rates were somewhat variable. Thirdly, it was fouild that the observed rates were r o u g h l~~ proportional to the co~lcentratio~l of hypochlorite, and it is difficult to suggest a simple first-order ~nechailis~n for the u~lcatalyzed reaction. However, relatively low orders of dependence on l~ypocl~lorite concentration are observed for the catalyzed reaction, which suggests that these earlier solutioils contained traces of catalyst. Finally, and perhaps the most convincing reason for believing some catalyst to be present, it was found that the apparent activation energy for oxygen evolution was 21 l;cal/g-11101, less than the 24.8 l;cal/g-mol found for the reaction giving chlorate and chloride; yet the latter is the predominant reaction.Other worlters have also examined this deconiposition, though they usually did not separate the rates of the two reactions. Giordani (3) found a second-order gas evolution; but his conclusio~~s about the reaction to chlorate had not been confirmed, so it seemed worth while to investigate the reaction in inore detail. EXPERIMENTAL P A R TThe main proble~n was to obtain sodiuin hypochlorite free from traces of catalyst. At present-only cobalt, niclcel, and copper are known t o catalyze this deco~~~position, so that the methods of purification were directed towards the removal or coinplexing of these metals. I t seemed much more promising to purify the sodium hypochlorite solution as opposed t o the chlorine and sodium hydroxide solution from which it was made. The following general methods of purification, or a t least of removal of catalyst, were e...

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Eine Röntgenuntersuchung des Titelkomplexes, der ein saures H‐Atom enthält und als CH, C12 ‐Monosolvat vorliegt, zeigt, daß er Sandwichstruktur hat und in der Raumgruppe P212, 2, kristallisiert.

Many methods of monoacylation of primary amides were studied ; one, the sulphuric acid-catalysed reaction of amides with anhydrides at 100". w a s found to be very general. Several new acyclic imides were synthesised, including compounds as diverse as N-acetylvaleramide, N-valeryl-4-methylvaleramide, and 3a-acetoxy-N-acetylcholanamide. In two cases symmetrical imides related to the anhydride used were identified as minor by-products of the synthesis of mixed imides.WHEREAS cyclic imides such as succinimide and pht.ha1imide are well known and useful compounds, acyclic imides (A'-acylamides, R1*CO*NH*CO*RA) have been practically ignored. The reason is that while a way to make any desired imide can eventually be found, all attempts to devise a general method have fai1ed.lWe are trying to develop the photorearrangement of N-chloro-imides to 4-~hloro-imides,~ which are useful for conversion into lactones and pyrrolidone~,~ into a low and variable yields. Conversions, at least as measured by g.l.c., were improved by lowering the reaction temperature and changing the catalyst to acetyl bromide, but isolation of pure products on a preparative scale remained difficult and tedious. Results of these experiments are given in Table 1, nos. 7,9,10, 13, 17, and 23.The by-products of these reactions may often include not only nitriles, acids and tar, but also other imides.

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