The Rectilinear Diameter of Hydrogen. E. MATHIAS, C. A. CROMMELIN, and H. KAMERLINGH ONNES (Ann. Physique, 1922, 17, 463-474).-A r6sum6 of work already published (A., 1921, ii, 256; this vol., ii: 440). W. G. The Rectilinear Diameter of Oxygen. E. MATHIAS and H. KAMERLINGH ONNES (An92. Physique, 1922, 17, 416-441).-'A resum@ of work already published (A., 1910, ii, 771, 829; 1911, ii, 387). W. G. Equilibrium between Sulphur and Iodine in Solution. M. AMADORI (Gazxetta, 1922, 52, i, 387-394).-In

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... view of the fact that the results of recent investigations indicate that the so-called compounds of sulphur with iodine described by various authors are merely mixtures of the two elements, the author has examined the solubility and cryoscopic relations of sulphur and iodine when present together. It is found that the separate solubilities of each of these elements in carbon disulphide, benzene, and bromoform are less than those which obtain in presence of the other element ; in the first of these solvents both solubilities are increased by more than l OOyo by mixing the sulphur and iodine. The corresponding solubility curves of the mixtures in benzene and in carbon disulphide consist of two branches meeting in a point of double saturation. Cryoscopic measurements of the mixtures in bromoform solution show that the depression of the freezing point of the solvent is somewhat less than that calculated from the molecular weights of the sulphur and iodine. No evidence is obtained of the existence of a solid compound of the two elements. The Crystallisation of Amorphous Tellurium. A. DAMIENS (Corn@. rend., 1922, 174, 1548--1550.-From a Btudy of the heats of reaction of different forms of tellurium with a mixture of bromine and bromine water, Berthelot and Fabre have found the relationship Tecryst. = Te""",. + 12.096 cal. (for 64 grains). Previous work on the allotropy of tellurium did not confirm this equation (cf. this vol., ii, 498), and the author has accordingly repeated the work of Berthelot and Fabre, using, however, a mixture of bromine and concentrated hydrochloric acid diluted with its own volume of water. His results do not confirm those TeCrYRt. + 2.63 cal., which is in accord. with his work on the allotropy of tellurium (Zoc. cit.) . The Rectilinear Diameter of Nitrogen. E. MATIIIAS, H. KAMERLINGII ONNES, and C. A. CROMMELIN (Ann. Physique, 1922, 17, 4 5 5 4 6 3 ) . A more detailed account of work already published (A., 1915, ii, 143). Normal Density of [Chemically Pure] Nitrogen. E. MOLES ( J . Ghim. physique, 1922, 19, 283--289).-The results of twenty-nine determinations of the density of pure nitrogen have been systematically discussed, and from calculations, the weight of the litre of nitrogen a t O", 760 mm., and 45" latitude is found to be L, = 1.2507 & 0.0001 grams. The measurements used are those of Rayleigh and Ramsay, Leduc, Gray, and Moles, in which two entirely different methods were used, and the ninterial was drawn from eight different sources. Under the conditions O", 760 mrn., and g = 980.665, the rounded value is L, = 1.2507 grams. The actual value obtained from nitrogen obtained from sodium nitrite is L, = 1.2506 grams, a value which is almost identical with the above-cited mean. This result is remarkable, since it was obtained from volumetric determinations. The Synthesis of Ammonia by Collision with Slowmoving Electrons. E. RUCK ANDERSEK (2. PhysiE, 1922, 10, 54-62).-A study of the action of a stream of electrons on the production of ammonia from mixtures of nitrogen and hydrogen a t low pressures. A current was passed between a glowing tungsten wire and two p1at)inum electrodes in an atmosphere of the two gases. The current was kept constant and the effect of variations in the coniposition of the gas mixture and in the applied E.M.P. were investigated. The maxiinurn rate of formation of ammonia did not correspond with the stojcheiornetric mixture, but with mixtures containing a great excess of nitrogen. This result is in agreement with the view that the first step in the production of ammonia is the ionisation of the nitrogen molecule. Curves a're given showing the velocity of formation of ammonia plotted against the applied electromotive force. These curves show a series of maxima at 22, 26, and 33 volts. No appreciable quantities of ammonia were produced below an applied electromotive force of of Berthelot and Fabre, but establish the equation Team",. --W. G .