Isotopic exchange reactions of hydrogen sulfide in nonaqueous solutions
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Isotopic exchange reactions of hydrogen sulfide in nonaqueous solutions

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Published .
Written in English

Subjects:

  • Hydrogen sulphide.,
  • Chemical kinetics.

Book details:

Edition Notes

Statementby Thomas Miles Beasley.
The Physical Object
Pagination89 leaves, bound :
Number of Pages89
ID Numbers
Open LibraryOL14298482M

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sulfide and a solution of sulfuric acid. There was good agreement between the amount of hydrogen sulfide calculated from the weight of cadmium sulfide and the amount calculated from the quantity of sulfuric acid. SOURCE AND PURITY OF MATERIALS: 1. Prepared from 25% solution of sodium sulfide by treatment with concentrated acid. Washed with.   The Chemistry of Nonaqueous Solvents, Volume III: Inert, Aprotic, and Acidic Solvents is a compilation of critical surveys of specific solvent systems. The compendium contains discussions on the solution chemistry of sulfur dioxide and acyl halides; the solvent properties of hydrogen sulfide and carboxylic acids; and the Bronsted acid-base Book Edition: 1.   The hydrogen isotope exchange reaction between hydrogen and water, i.e., liquid phase catalytic exchange, has an interesting role in water detritiation and heavy water production. This reaction has many advantages over the hydrogen sulfide–water (H 2 S–H 2 O) and ammonia–hydrogen (NH 3 –H 2) exchange processes because of the reaction's Cited by: 5. The isotope exchange between35S-labeled sulfur compounds of sulfate (SO4 2−), elemental sulfur (S0), polysulfide (Sn 2−), hydrogen sulfide (ΣHS−: H2S + HS− + S2−), iron sulfide (FeS), and pyrite (FeS2) was studied at pH and 20 °C in anoxic, sterile seawater. Isotope exchange was observed between S0, S2 2− ΣHS−, and FeS, but not between35S labeled SO4 2− or FeS2 and the.

quinoline gave -with liquid hydrogen sulfide solutions of con-sidei^ble conducting pocer. Unsaturated Hydrocarhona. Amylene and tri-nettG'! ettQrlene vere siscible -srith liquid iDydrogen 'sulfide at -TT^C* hut showed no reaction at this low temperature. After contact •sith the liquid hydrogen sulfide for four. At high temperatures the dominant effect is interaction of hydrogen sulfide, an HDS reaction product, with the catalyst to improve its hydrogenolysis (hydrocracking) activity. This increases the rate of piperidine hydrogenolysis, which is rate determining at the . For example, if hydrogen chloride HC1, enriched by the heavy isotope of chlorine 37 C1, is mixed with chlorine Cl 2 with the normal isotope composition ( percent 35 C1 and percent 37 C1), then as a result of the isotopic exchange reactions.   If methane is in isotopic equilibrium with water vapor, the HCH4 hydrogen exchange reaction is responsible for the D/H variation of volcanic methane. At isotopic equilibrium between CH4 and Hz0, for example at a temperature range of , the methanes should be %o depleted in deuterium as compared to cogenetic water vapor [30].

Reactions of Hydrogen Sulfide with NO Donors. The discovery of peroxynitrite (− OONO) scavenging of H 2 S prompted the study of the reactions of NO donors and H 2 S by Moore and co-workers. [] In this work, the mixture of various NO donors and H 2 S (in the form of sodium sulfide, NaSH) forms a new species that demonstrates the general chemical and biochemical characteristics of an S. The review considers thermodynamics and kinetics of isotope exchange in the H2O-H2S system. The temperature dependences of separation factor α are considered for all binary H-T, H-D, and DT mixtures. The effect of equilibrium constants of homo-molecular exchange reactions involving water and hydrogen sulfide on concentration dependence of α is demonstrated. HYDROGEN SULFIDE reacts as an acid and as a reducing agent. Explodes on contact with oxygen difluoride, bromine pentafluoride, chlorine trifluoride, dichlorine oxide, silver fulminate. May ignite and explode when exposed to powdered copper in oxygen [Mertz, V. et al., Ber., , 13, p. ].   The solution is initially clear, but clouds up over time due to the slow reaction of hydrogen sulfide with the oxygen in the water. Over time, elemental sulfur is precipitated out of the solution.