Liquid Hydrogen Sulfide Research Articles

Synthesis of 4-thiouridine derivatives

The thionation of a protected uridine with the aid of P2S5 has given the corresponding 4-thiouridine derivatives, which have been phosphorylated at the 5′ or the 2′(3′)hydroxyl. On being heated in aqueous pyridine solution with liquid hydrogen sulfide, cytidine phosphates also form 4-thiouridine phosphates. 4-Thiouridine 2′,3′-cyclophosphate has been obtained.

The Thermodynamics of Liquid Hydrogen Sulphide and Carbon Monoxide and Significant Structure Theory

The Thermodynamics of Liquid Hydrogen Sulphide and Carbon Monoxide and Significant Structure Theory

Liquid hydrogen sulfide in contact with sulfur

Liquid hydrogen sulfide in contact with sulfur

Near-infrared spectrum of liquid hydrogen sulfide

Near-infrared spectrum of liquid hydrogen sulfide

Liquid hydrogen sulphide as an ionising solvent. Part I. Base analogues and their neutralisation with hydrogen halides

Tetra-alkylammonium hydrogen sulphides, R4NSH, have been prepared. The salts co-ordinate hydrogen sulphide loosely at low temperatures; the hydrogen-bond energy is about 5 kcal. mole–1. Solutions of the salts in liquid hydrogen sulphide are strongly conducting, compared with solutions of amines and phosphines. A hydrogen dichloride salt was formed in the neutralisation of tetra-n-propylammonium hydrogen sulphide in liquid hydrogen sulphide. Similar reaction of hydrogen halides with tetra-alkylammonium halides in liquid hydrogen sulphide gave salts containing the anions, HCl2–, HBr2–, Hl2–, HBrCl–, and HCll–.

Liquid hydrogen sulphide as an ionising solvent. Part II. Reactions of Lewis acids of boron with base analogues

Neutralisations of base analogues by volatile boron Lewis acids have been examined in liquid hydrogen sulphide. Salts containing the new anions BF3SH–, BCl3SH–, BBr3SH–, and BEt3SH– have been prepared. The reaction of diborane is more complicated but seems to proceed, at least initially, through the formation of the ion BH3,SH·BH3–, which subsequently loses hydrogen. The ions BF3SH– and BCl3SH– react with excess of boron trihalide to give tetrafluoroborate and tetrachloroborate ions, respectively.

Liquid hydrogen sulphide as an ionising solvent. Part III. Reactions of compounds of Groups IV, V, and VI

The chemical behaviour of a number of compounds of Groups IV, V, and VI in liquid hydrogen sulphide has been studied. Tetra-alkylammonium salts containing the new anions (SiF4)2S2–, SiCl4S2–, SiCl4(SH)22–, and GeF4(SH)22–, have been isolated after neutralisations.

Radiation chemistry of liquid hydrogen sulphide

G(H2) for cobalt-60 γ-irradiated liquid hydrogen sulphide at –78°C is 8.1±0.3 and is unaffected by the addition of I2 or DPPH. G(S) is 6.6±0.7 for the pure liquid, and when DPPH is present increases through a flat maximum about 8 at DPPH concentrations of 10–4 to 10–3 M, thereafter decreasing to 3 in 10–2 M DPPH. The yields suggest that H atoms abstract hydrogen atoms from the solvent, and SH radicals combine to form H2S and S atoms which later polymerize. Although H2S2 was not detected, the lack of stoichiometry suggests it is formed in the pure liquid and the following yields were calculated assuming GH2 is zero. GH=G–H2S= 8.1±0.3; GSH= 5.1±1.7; G(H2S2)= 1.5±1.0. The value for G–H2S is greater than the maximum value calculated from mass spectrometric and ionization efficiency data for the reactions of the primary ions alone and suggests that some decomposition may result from excitation also. The ineffectiveness of I2 and DPPH in changing G(H2) is probably due to an inability to add sufficient of these solutes to compete with solvent for H atoms. In iodine solutions, sulphur is formed in a chain reaction.

New Observations on the Low Temperature Reaction between Hydrogen Sulphide and Sulphur Dioxide : A Novel Method for Analysing Milligram Quantities of Hydrogen Sulphide in the Presence of Carbon Dioxide

When an anhydrous mixture of liquid hydrogen sulphide and liquid sulphur dioxide contained in a sealed tube at -78 �C is gently warmed, the liquid remains clear until the temperature reaches c. -40 �C, when sulphur is slowly deposited. Careful measurements reveal that the two compounds always react in the mole ratio, H2S : SO2 = 3 : 2, which contrasts with the stoichiometric equation 2H2S + SO2 =2H2O + 3S, widely quoted for their reaction in the moist gaseous phase or in aqueous solution. This low temperature reaction forms the basis of a novel high vacuum method for estimating milligram quantities of hydrogen sulphide when in the presence of gases, such as carbon dioxide, whose volatilities are sufficiently similar to preclude the use of normal low-temperature vacuum fractionation methods.

Effect of Antifreeze Agents on the Formation of Hydrogen Sulphide Hydrate

Abstract The effects of various antifreeze agents on the formation of hydrogensulphide hydrate have been studied. On a molar basis the relative lowering ofTM (the maximum temperature at which solid hydrogen sulphide hydrate can existin equilibrium with the given solution) for the various agents is: sodiumchloride 1.00, calcium chloride 1.71, methyl alcohol 0.57, ethyl alcohol 0.68, ethylene glycol 0.73, diethylene glycol 0.73, sucrose 0.87, dextrose 0.71. On aweight basis the relative lowering of TM is: sodium chloride 1.00, calciumchloride 0.91, methyl alcohol 1.08, ethyl alcohol 0.89, ethylene glycol 0.69, diethylene glycol 0.41, dextrose 0.23, and sucrose 0.15. Introduction The solid hydrate of hydrogen sulphide, H2S?6H2O1, is in equilibrium withwater and liquid hydrogen sulphide at 85?F at a partial pressure of hydrogensulphide approximately equal to the vapor pressure of hydrogen sulphide at thattemperature. At temperatures below 85?F, in the presence of excess hydrogensulphide (greater than the amount required to react with the water present) thehydrate is in equilibrium with liquid hydrogen sulphide at approximately thevapor pressure of hydrogen sulphide. In the presence of excess water, the solid hydrate is in equilibrium withliquid water, containing dissolved hydrogen sulphide, at a pressure lower thanthe vapor pressure of liquid hydrogen sulphide at the same temperature. Thelower the temperature, the greater the difference between the decompositionpressure of the hydrate and the vapor pressure of liquid hydrogen sulphide atthat temperature. Conditions conducive to the formation of solid hydrogen sulphide hydrate mayexist in wells producing a gas containing a high percentage of hydrogensulphide under high pressure, or in the lead lines from such wells. This papergives the results of tests made with various antifreeze agents which might beuseful in decomposing the hydrate or in preventing the formation of the hydrateof hydrogen sulphide. Apparatus Fig I shows a diagram of the apparatus used. The sample under observationwas contained in a glass tube 34 cm long, having a 6 mm id and a wall thicknessof 2.5 mm. The lower end of this tube was closed with a plug of butyl rubber.The upper end of the tube was connected to a diaphragm gauge, with a stainlesssteel diaphragm, a manometer, a vacuum pump, and a cylinder of hydrogensulphide. The tube was held nearly horizontal, with the liquid resting along the lowerside of the tube. It was found that when the tube was held in a verticalposition, it broke with explosive violence as soon as it became filled withsolid hydrate. Presumably this was caused by the expansion which occurred onsolidification of the hydrate. The difficulty disappeared when the tube washeld in an inclined position during the tests. T.P. 2450

The Conductance of Tetraethylammonium Sulfamate in Liquid Hydrogen Sulfide1

The Conductance of Tetraethylammonium Sulfamate in Liquid Hydrogen Sulfide¹

The Conductance of Iodine in Liquid Hydrogen Sulfide

The Conductance of Iodine in Liquid Hydrogen Sulfide

The Conductance of Solutions of Organosubstituted Ammonium Chlorides in Liquid Hydrogen Sulfide

The Conductance of Solutions of Organosubstituted Ammonium Chlorides in Liquid Hydrogen Sulfide

Raman Spectra of Gaseous, Liquid and Solid Hydrogen Sulfide

Raman Spectra of Gaseous, Liquid and Solid Hydrogen Sulfide

Liquid Hydrogen Sulfide as a Reaction Medium.

Liquid Hydrogen Sulfide as a Reaction Medium.

Raman Effect in Hydrogen Sulphide

THE Raman spectrum of hydrogen sulphide, both in the gaseous and liquid states, has been successfully photographed by me. The liquid exhibits a single intense and quite sharp line shifted by 2578 wave-numbers from the exciting mercury radiation. With the gas, the line appears in a slightly different position, with a frequency shift of 2615 wave-numbers, and is distinctly more diffuse than in the liquid. According to Barker and Meyer (Trans. Far. Soc., 25, 912; 1929) the infra-red absorption spectrum of gaseous hydrogen sulphide shows a complex band at about 3.7μ which evidently represents the superposition of rotation on this vibrational frequency. The plates for both the liquid and the gas showed indications of other faint lines or bands which were adjacent to the exciting mercury radiations and presumably could be ascribed to a rotational Raman effect. It may be remarked that the line observed with the liquid hydrogen sulphide is identically in the same position as a prominent line obtained in the Raman spectra of a series of organic hydro-sulphides studied at Calcutta by Venkateswaran, and also in its frequency shift with an important infra-red absorption frequency of these compounds.

REACTIONS IN LIQUID HYDROGEN SULFIDE. V. REACTION WITH FURFURAL

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTREACTIONS IN LIQUID HYDROGEN SULFIDE. V. REACTION WITH FURFURALR. E. Meints and J. A. WilkinsonCite this: J. Am. Chem. Soc. 1929, 51, 3, 803Publication Date (Print):March 1, 1929Publication History Published online1 May 2002Published inissue 1 March 1929https://doi.org/10.1021/ja01378a019RIGHTS & PERMISSIONSArticle Views78Altmetric-Citations-LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InReddit PDF (97 KB) Get e-Alerts Get e-Alerts

Handbuch der Arbeitsmethoden in der anorganischen Chemie

THE special operations described in the second part of the second volume of this work include micro-chemical methods, membrane-filtration, electrometric analysis and electrolytic purification, decomposition with a silent electric discharge and in the arc, the use of radio-elements as indicators, identification of crystals and X-ray analysis, the use of high vacua and of high pressures, mass-spectrography, the use of liquid ammonia, sulphur dioxide, hydrogen chloride and hydrogen sulphide as solvents, and the general operations of photochemistry. The technique of these diverse operations has been described by fifteen authors, in a volume of about 1000 pages. It will form a most valuable work of reference for those who may have occasion from time to time to make use of one or other of the special methods with which it deals.

Liquid Hydrogen Sulfide as a Source of Laboratory Supply of the Gas.

Liquid Hydrogen Sulfide as a Source of Laboratory Supply of the Gas.