Mass spectrum of sulfur vapor

Bradt, Paul; Mohler, F. L.; Dibeler, Vernon H.

doi:10.6028/jres.057.027

Cited by 27 publications

(14 citation statements)

References 2 publications

(2 reference statements)

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“…In 1809, the French chemists Louis-Joseph Gay-Lussac and Louis-Jacques Thenard proved the elemental nature of sulfur. In its 1961 report [22], CAWIA recommended A r (S) = 32.064(3) based on the abundances of S isotopes in virgin Texas sulfur reported by Bradt et al [253] and in meteoritic S reported by MacNamara and Thode [254], with atomic masses from Everling et al [23]. CAWIA observed that this value was in good agreement with the results of chemical determinations and that the uncertainty was assigned largely on the basis of natural variability, as documented by Rankama [255] and Duckworth [256].…”

Section: S Sulfurmentioning

confidence: 99%

Atomic weights of the elements. Review 2000 (IUPAC Technical Report)

Laeter¹,

Böhlke²,

Bièvre³

et al. 2003

Pure and Applied Chemistry

915

554

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Republication or reproduction of this report or its storage and/or dissemination by electronic means is permitted without the need for formal IUPAC permission on condition that an acknowledgmentAbstract: A consistent set of internationally accepted atomic weights has long been an essential aim of the scientific community because of the relevance of these values to science and technology, as well as to trade and commerce subject to ethical, legal, and international standards. The standard atomic weights of the elements are regularly evaluated, recommended, and published in updated tables by the Commission on Atomic Weights and Isotopic Abundances (CAWIA) of the International Union of Pure and Applied Chemistry (IUPAC). These values are invariably associated with carefully evaluated uncertainties. Atomic weights were originally determined by mass ratio measurements coupled with an understanding of chemical stoichiometry, but are now based almost exclusively on knowledge of the isotopic composition (derived from isotope-abundance ratio measurements) and the atomic masses of the isotopes of the elements. Atomic weights and atomic masses are now scaled to a numerical value of exactly 12 for the mass of the carbon isotope of mass number 12. Technological advances in mass spectrometry and nuclear-reaction energies have enabled atomic masses to be determined with a relative uncertainty of better than 1 × 10 -7 . Isotope abundances for an increasing number of elements can be measured to better than 1 × 10 -3 . The excellent precision of such measurements led to the discovery that many elements, in different specimens, display significant variations in their isotope-abundance ratios, caused by a variety of natural and industrial physicochemical processes. While such variations increasingly place a constraint on the uncertainties with which some standard atomic weights can be stated, they provide numerous opportunities for investigating a range of important phenomena in physical, chemical, cosmological, biological, and industrial processes. This review reflects the current and increasing interest of science in the measured differences between source-specific and even sample-specific atomic weights. These relative comparisons can often be made with a smaller uncertainty than is achieved in the best calibrated "absolute" (= SI-traceable) atomic-weight determinations. Accurate determinations of the atomic weights of certain elements also influence the values of fundamental constants such as the Avogadro, Faraday, and universal gas constants. This review is in two parts: the first summarizes the development of the science of atomic-weight determinations during the 20 th century; the second summarizes the changes and variations that have been recognized in the values and uncertainties of atomic weights, on an element-by-element basis, in the latter part of the 20 th century.J. R. de LAETER et al.

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Section: S Sulfurmentioning

confidence: 99%

Atomic weights of the elements. Review 2000 (IUPAC Technical Report)

Laeter¹,

Böhlke²,

Bièvre³

et al. 2003

Pure and Applied Chemistry

915

554

View full text Add to dashboard Cite

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“…S, Sz, H2S, HzSz falls into line with the series I.P. 0 , 02, HzO, HzOz, though such comparisons have been used t o justify the correctness of values obtained (27,30).…”

Section: Experiments On S2omentioning

confidence: 95%

“…Sz exist between 8.3 v and 11.0 v (27)(28)(29)(30)(31), while the only published value of I.P. H2S2 (10.2 v) has been obtained indirectly (30).…”

Section: Experiments On S2omentioning

confidence: 99%

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A Mass Spectrometric Study of the Oxidation of Hydrogen Sulphide Part I. Observation and Identification of Some Intermediates

Marsden¹

1963

Can. J. Chem.

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The oxidation of hydrogen sulphide has been followed mass-spectrometrically by direct sampling from a reaction vessel having a small leak. In the neighborhood of the third explosion limit, there is a period of 8-12 seconds of accelerating reaction before the explosion; during this time peaks are observed to grow, disappearing after explosion. By using D2S/lB02 and HzS/1802 mixtures, it has been shown that these peaks arise from the ions HZ+, S20+, H2SO+, Szf, and H2Szf. I t is evident that the first two ions represent the intermediate formation of hydrogen and disulphur monoxide; the parents of the last three ions are discussed, and it is concluded that the most likely possibilities are HzS02, Ss, and H2Sz. Only during the explosion itself is there any evidence for SO radical.

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“…The ~I a s S pe ctrometr.\-Section has published several papers on detection and analy is of heavy mole cules evaporated from a vacuum-tub e furnac e dire ctly into the ionization chamber of a ma s spectrom eter [1, 2,3,4).1 l\lixture of heavy molecules have b een st udied by r eco rding t he spectra as t he temperature is increa ed step b~-step. This afford th e advantage t hat the mixture i fractionated in the proce s of evaporation and t he complexity of the mass pectra is redu ced .…”

Section: Introductionmentioning

confidence: 99%

Mass spectra and relative sensitivities of some polyphenyls

Bradt¹,

Mohler²

1958

J. RES. NATL. BUR. STAN.

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:\Iass s pect m hi\\" e bee n meas ured by e vaporating polypheny ls fr om a tube furnace in to t he ionization chamber of a 60 0 mass spectrom eter operated at constant ion acceleratin g voltage. Mass spec tra of pure t e traphen.vl , h exapltenyl, a nd octaph e ny l are rep orted. A synthet ic mixture of terphe nyl , tetra pheny l, p e nta phenyl, h exaph eny l, a nd octaphenyl in knolyn proportions was eva por ated aR the temperature " 'a s in creased s te p by step fr om 125 0 to 290 0 C a nd t ime in teg ra ls of the fiv e molec ule ion cu rrents were r ecorded over t he t im e r equired to co mpl e tely e vaporate t he sample. The relative sens it ivity in creases rap id ly with in creasing molec ul ar weigh t.

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Mass spectrum of sulfur vapor

Cited by 27 publications

References 2 publications

Atomic weights of the elements. Review 2000 (IUPAC Technical Report)

Atomic weights of the elements. Review 2000 (IUPAC Technical Report)

A Mass Spectrometric Study of the Oxidation of Hydrogen Sulphide Part I. Observation and Identification of Some Intermediates

Mass spectra and relative sensitivities of some polyphenyls

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