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Iron oxide reaction with hydrogen sulfide

In the acid-leaching process, the oxide ore is leached with sulfuric acid at elevated temperature and pressure, which causes nickel, but not iron, to enter into solution. The leach solution is purified, foHowed by reaction with hydrogen sulfide and subsequent precipitation of nickel and cobalt sulfides. [Pg.3]

The liquid is circulated at such a rate that a two- to threefold excess of ferric hydroxide over the stoichiometric quantity necessary for the complete reaction with hydrogen sulfide is present. Gollmar (1945) states that the process can be operated with less than the stoichiometric concentration of iron oxide and interprets the function of the iron as a catalytic oxygen carrier. Available historical data from several plants indicate that operation with an excess of iron oxide over the stoichiometric amount was commonly practiced. This excess seems to be required for complete removal of hydrogen sulfide and, also, to minimize thiosulfate formation in the thionizer. For a coal gas plant with a 10 MMsef/day capacity and a hydrogen sulfide removal rate of 400 grains/lOO scf, the chemical requirements are approximately 3,500 Ib/day of sodium carbonate and 2,800 Ib/day of iron. [Pg.740]

Excellent discussions on the properties of purification materials have been presented by Smith (1957) and Ward (1964). The physical mechanism of hydrogen sulfide absorption by iron oxide was investigated by Avery (1939) and Dent and Moignard (1950). The studies showed that under proper conditions of temperature, moisture content, and pH, the sulfur formed on the oxide particle is continuously displaced by iron oxide, which migrates from the particle center to the surface, thus exposing ftesh oxide for further reaction with hydrogen sulfide and oxygen. [Pg.1301]

About 70% of the western world s supply of nickel comes from iron and nickel sulfide ores that were brought close to the surface nearly 2 billion years ago by the violent impact of a huge meteor at Sudbury, Ontario. The ore is first roasted (heated in air) to form nickel(II) oxide, which is reduced to the metal either elec-trolytically or by reaction with hydrogen gas in the first step of the Mond process ... [Pg.784]

Iron Sponge Also called Dry box. An obsolete process for removing hydrogen sulfide from gas streams by reaction with iron oxide monohydrate. The ferric sulfide that is formed is periodically re-oxidized to regenerate ferric oxide and elemental sulfur. When this process becomes inefficient because of pore-blockage, the sulfur is either oxidized to sulfur dioxide for conversion to sulfuric acid, or is extracted with carbon disulfide. [Pg.146]

In many cases, well water is chlorinated prior to RO to help oxidize and removal metals such as iron and manganese. Hydrogen sulfide reacts with chlorine to form acids. The overall equation is shown in Equation 7.8, but, just as with the reaction of oxygen with hydrogen sulfide, there are intermediates, which include elemental sulfur (Equation 7.9) ... [Pg.143]

Thus six atoms of iron will produce nine molecules of water compared with six atoms of zinc, which only produce six. Furthermore iron sulfide can release hydrogen sulfide by reaction with hydrogen and steam during plant start-up or shut-down conditions. In practice, therefore, when iron oxide is used it is always followed by a guard bed of zinc oxide. [Pg.361]

Hydrochloric acid reacts with sulfur only in the presence of iron to form hydrogen sulfide. Sulfur dioxide forms when sulfur is heated with concentrated sulfuric acid at 200°C. Dilute nitric acid up to 40% concentration has Htde effect, but sulfur is oxidized by concentrated nitric acid in the presence of bromine with a strongly exothermic reaction (19). [Pg.117]

Hydrogen sulfide reacts with iron oxide [1317-61 -9] to form iron sulfide, according to the following chemical reaction ... [Pg.209]

Claus A process for removing hydrogen sulfide from gas streams by the catalyzed reaction with sulfur dioxide, producing elementary sulfur. The process has two stages in the first, one third of the hydrogen sulfide is oxidized with air to produce sulfur dioxide in the second, this sulfur dioxide stream is blended with the remainder of the hydrogen sulfide stream and passed over an iron oxide catalyst at approximately 300°C. The resulting sulfur vapor is condensed to liquid sulfur. [Pg.65]

Manchester A variation on the Ferrox process for removing hydrogen sulfide from industrial gases in which several absorbers are used, and delay stages permit completion of the reaction with the iron oxide absorbent. Developed by the Manchester Corporation Gas Department in the 1940s and installed in several British gasworks. [Pg.171]


See other pages where Iron oxide reaction with hydrogen sulfide is mentioned: [Pg.709]    [Pg.360]    [Pg.134]    [Pg.135]    [Pg.361]    [Pg.342]    [Pg.134]    [Pg.135]    [Pg.2556]    [Pg.2465]    [Pg.709]    [Pg.241]    [Pg.108]    [Pg.573]    [Pg.1323]    [Pg.1324]    [Pg.506]    [Pg.291]    [Pg.174]    [Pg.188]    [Pg.171]    [Pg.65]    [Pg.124]    [Pg.251]    [Pg.660]    [Pg.296]    [Pg.291]    [Pg.622]    [Pg.899]    [Pg.291]    [Pg.622]    [Pg.6]    [Pg.293]   
See also in sourсe #XX -- [ Pg.371 , Pg.372 , Pg.373 , Pg.374 , Pg.375 , Pg.376 , Pg.377 , Pg.378 , Pg.379 , Pg.380 , Pg.381 , Pg.382 , Pg.383 , Pg.384 , Pg.385 , Pg.386 , Pg.387 , Pg.388 , Pg.389 ]




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Hydrogen sulfide oxidation

Hydrogen sulfide, reactions

Hydrogenation reaction with

Iron oxide reaction

Iron reaction

Iron sulfide, reaction with

Iron, oxidation with

Oxidation with hydrogen

Oxides sulfides

Reaction with hydrogen

Reaction with hydrogen sulfide

Reaction with iron

Reaction with sulfides

Reactions sulfides, oxidation

Sulfides oxidation

With hydrogen sulfide

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