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The Vibration Spectra of Hydrazoic Acid, Methyl Azide, and Methyl Isocyanate The Thermodynamic Functions of Hydrazoic Acid

dc.contributor.authorEyster, Eugene H.en_US
dc.contributor.authorGillette, R. H.en_US
dc.date.accessioned2010-05-06T22:37:59Z
dc.date.available2010-05-06T22:37:59Z
dc.date.issued1940-05en_US
dc.identifier.citationEyster, Eugene H.; Gillette, R. H. (1940). "The Vibration Spectra of Hydrazoic Acid, Methyl Azide, and Methyl Isocyanate The Thermodynamic Functions of Hydrazoic Acid." The Journal of Chemical Physics 8(5): 369-377. <http://hdl.handle.net/2027.42/70737>en_US
dc.identifier.urihttps://hdl.handle.net/2027.42/70737
dc.description.abstractThe vibration spectra of hydrazoic acid, methyl azide, and methyl isocyanate have been investigated in the spectral region between 2 and 20μ. Correlation of the spectra of these structurally similar molecules has made possible the determination of all the fundamental frequencies of hydrazoic acid and all but the methyl torsion frequency in the methyl compounds. From these fundamental frequencies and the known rotational constants, the usual thermodynamic functions of hydrazoic acid have been calculated to the harmonic oscillator‐rigid rotator approximation. Equilibrium constants for some characteristic reactions have also been obtained.en_US
dc.format.extent3102 bytes
dc.format.extent571825 bytes
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dc.format.mimetypeapplication/pdf
dc.publisherThe American Institute of Physicsen_US
dc.rights© The American Institute of Physicsen_US
dc.titleThe Vibration Spectra of Hydrazoic Acid, Methyl Azide, and Methyl Isocyanate The Thermodynamic Functions of Hydrazoic Aciden_US
dc.typeArticleen_US
dc.subject.hlbsecondlevelPhysicsen_US
dc.subject.hlbtoplevelScienceen_US
dc.description.peerreviewedPeer Revieweden_US
dc.contributor.affiliationumDepartment of Physics, University of Michigan, Ann Arbor, Michiganen_US
dc.contributor.affiliationumDepartment of Chemistry, University of Michigan, Ann Arbor, Michiganen_US
dc.description.bitstreamurlhttp://deepblue.lib.umich.edu/bitstream/2027.42/70737/2/JCPSA6-8-5-369-1.pdf
dc.identifier.doi10.1063/1.1750669en_US
dc.identifier.sourceThe Journal of Chemical Physicsen_US
dc.identifier.citedreferenceEyster, J. Chem. Phys. 8, 135 (1940).en_US
dc.identifier.citedreferencePauling and Brockway, J. Am. Chem. Soc. 59, 13 (1937).en_US
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dc.identifier.citedreferenceBarker and Meyer, Trans. Faraday Soc. 25, 912 (1929).en_US
dc.identifier.citedreferenceGoubeau, Ber. 68, 912 (1935).en_US
dc.identifier.citedreferenceBadger and Bauer, J. Am. Chem. Soc. 59, 303 (1937).en_US
dc.identifier.citedreferenceBuswell, McMillan, Rodebush, and Wall, J. Am. Chem. Soc. 61, 2809 (1939). These workers did not study the fundamental itself, but the evidence is clear from the effect on the harmonic.en_US
dc.identifier.citedreferencePauling, The Nature of the Chemical Bond (Cornell University Press, 1939), p. 180.en_US
dc.identifier.citedreferenceThese are either the base constants chosen by DuMond, or values derived with their aid, and we impute to them no more absolute significance than would he; they have been chosen for convenience, and because they are in essential agreement with “best values” chosen by others. See: DuMond, Phys. Rev. 56, 153 (1939); Wensel, Nat. Bur. Stand. J. Research 22, 375 (1939); and Skiba, Sci. Papers of the I.P.C.R., Tokyo, 34, 1308 (1939).en_US
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dc.identifier.citedreferenceGiauque, J. Am. Chem. Soc. 52, 4816 (1930).en_US
dc.identifier.citedreferenceGunther, Meyer, and Muller‐Skold, Zeits. f. Physik. Chemie A175, 154 (1935).en_US
dc.identifier.citedreferenceBerthelot, Thermochemie (Paris, 1897), Vol. 2, p. 72.en_US
dc.identifier.citedreferenceStephenson and McMahon, J. Am. Chem. Soc. 61, 437 (1939).en_US
dc.owningcollnamePhysics, Department of


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