other members of both organizations for vitamin and protein analyses. The graphs and illustrations were prepared by D. V. Alstrand. Cooperation of the meat packing industry in furnishing materials and plant facilities is appreciated. LITERATURE CITED fl) American Can Co., "Canned Food Reference Manual". 2nd od., pp. 245-64 (1943).(2) Assoc, of Official Agr. Chem., Official and Tentative Methods of Analysis, 5th ed., 1940.

The utility of the Debye modification of the Clausius-Mossotti law for the calculation of the electric moments of certain molecules has been shown by several investigators.* 1 At the present writing data for the moments of various types of organic molecules, calculated in the manner referred to above, are accumulating rapidly. In general, these figures are being obtained either from dielectric constant and density data for their solutions in benzene or from the temperature variation of the dielectric constant of their vapors. In this series of articles the dielectric constants of binary mixtures are being studied; therefore, it is concerned only with the first type of calculation, with the important modification, however, that other solvents besides benzene are being used. The third paper of this series2 presented values for the electric moments of certain organic molecules, calculated from dielectric constant and density data of their solutions in carbon tetrachloride. The purpose of this paper is to show that carbon disulfide and hexane may also be used successfully as solvents for the purpose in hand. The electric moments of several organic molecules have been calculated from dielectric constant and density data in these solutions, data similar in all respects to those presented in previous papers of this series. MethodThe method used for the determinations of the dielectric constants of the solvents, carbon disulfide and hexane, and their solutions, was the electrical resonance method described in the first paper of the series.3The same frequency, 10® cycles per second, and the same temperature, 25°, were used for the measurements in every case.Density determinations on the solutions were made at 25°u sing a 50cc. pycnometer of the Ostwald-Sprengel type. The usual precautions for precision work were observed throughout.

The thermal rate of formation of hydrogen bromide from its elements was first accurately studied by Bodenstein and Lind in 1906 (1). They found that the rate of reaction could be expressed by the following equation,"+w m being a constant independent of temperature and having a numerical value of 5.The interpretation of this reaction was arrived at independently by Christiansen (3), Polanyi (9), and Herzfeld (4). The mechanism may be designated in the following steps: Br2 <=t 2Br(1)

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