Sulfur zinc with

Precipitation can also occur upon chemical reaction between the impurity and a precipitating agent to form a compound insoluble in the molten metal. The refining of cmde lead is an example of this process. Most copper is removed as a copper dross upon cooling of the molten metal, but the removal of the residual copper is achieved by adding sulfur to precipitate copper sulfide. The precious metals are separated by adding zinc to Hquid lead to form soHd intermetaHic compounds of zinc with gold and silver (Parkes process). The precious metals can then be recovered by further treatment (see Lead). 

Dithionites. Although the free-dithionous acid, H2S2O4, has never been isolated, the salts of the acid, in particular zinc [7779-86-4] and sodium dithionite [7775-14-6] have been prepared and are widely used as industrial reducing agents. The dithionite salts can be prepared by the reaction of sodium formate with sodium hydroxide and sulfur dioxide or by the reduction of sulfites, bisulfites, and sulfur dioxide with metallic substances such as zinc, iron, or zinc or sodium amalgams, or by electrolytic reduction (147). 

Although these curative systems may also be used with the polyepichlorohydrin elastomers containing AGE, the polymers were developed to be cured with conventional mbber curatives, sulfur, and peroxides. These polymers containing the pendent aHyl group are readily cured with a typical sulfur cure system such as zinc oxide, and sulfur along with the activators, tetramethylthiuram mono sulfide [97-74-5] (TMTM) and... 

Sulfur dioxide emissions may affect building stone and ferrous and nonferrous metals. Sulfurous acid, formed from the reaction of sulfur dioxide with moisture, accelerates the corrosion of iron, steel, and zinc. Sulfur oxides react with copper to produce the green patina of copper sulfate on the surface of the copper. Acids in the form of gases, aerosols, or precipitation may chemically erode building materials such as marble, limestone, and dolomite. Of particular concern is the chemical erosion of historical monuments and works of art. Sulfurous and sulfuric acids formed from sulfur dioxide and sulfur trioxide when they react with moisture may also damage paper and leather. 

The product is a random polymer that is vulcanized with sulfur or with metal oxides (zinc oxide, magnesium oxide etc.). Vulcanization with sulfur is very slow, and an accelerator is usually required. 

Sulfur reacts very slowly with rubber, and so is compounded with rubber in the presence of accelerators and activators. Typical accelerators are thia-zoles and a typical activator is a mixture of zinc oxide and a fatty acid. The chemistry of the vulcanisation reactions is complicated, but generates a three-dimensional network in which rubber molecules are connected by short chains of sulfur atoms, with an average of about five atoms in each chain. 

Nickel and selenium interact with incandescence on gentle heating [1], as do also sodium and potassium, the latter mildly explosively [2], Uranium [3] and zinc [4] also incandesce when their mixtures with selenium are heated, and platinum sponge incandesces vividly [5], The particle size of cadmium and selenium must be below a critical size to prevent explosions during synthesis of cadmium selenide by heating the elements together. Similar considerations also apply to interaction of cadmium or zinc with sulfur, selenium or tellurium [6], Interaction of powdered tin and selenium at 350° C is extremely exothermic [7],... 

Reactions of zinc-copper reagents bearing acidic hydrogen and sulfur functionalities with various electrophiles, including nitroalkenes, have been reported, as shown in Eq. 4.86108 and Eq. 4.87,109 respectively. 

Intimate mixtures of chlorates, bromates or iodates of barium, cadmium, calcium, magnesium, potassium, sodium or zinc, with finely divided aluminium, arsenic, copper carbon, phosphorus, sulfur hydrides of alkali- and alkaline earth-metals sulfides of antimony, arsenic, copper or tin metal cyanides, thiocyanates or impure manganese dioxide may react violently or explosively, either spontaneously (especially in presence of moisture) or on initiation by heat, friction, impact, sparks or addition of sulfuric acid [1], Mixtures of sodium or potassium chlorate with sulfur or phosphorus are rated as being exceptionally dangerous on frictional initiation. 

Other substances decrease or annihilate, even in traces, the catalytic properties of iron. Such catalyst poisons had already been known as a nuisance in the catalytic oxidation of sulfur dioxide. With the ammonia catalysis several elements, particularly sulfur proved to be harmful, even in amounts of 4oo of one per cent. Chlorine, phosphorus and arsenic showed a similar behavior (30), just as certain metals, such as lead, tin and zinc. 

The action of zinc in increasing the efficiency and rate of crosslinking is thought to involve chelation of zinc with the accelerator as well as species XVIII and XIX. Zinc polysulfide compounds such as XX are also likely intermediates. Zinc chelated to sulfur or as zinc sulfide bonds probably facilitate cleavage of sulfur-sulfur bonds in the concerted reactions described by Eqs. 9-20 and 9-21. 

Also, zinc sulfate can be prepared by reacting metallic zinc with dilute sulfuric acid followed by evaporation and crystallization ... 

Zinc and zinc-coated products corrode rapidly in moisture present in the atmosphere. The corrosion process and its mechanism were studied in different media, nitrate [283], perchlorate [259], chloride ions [284], and in simulated acid rain [285]. This process was also investigated in alkaline solutions with various iron oxides or iron hydroxides [286] and in sulfuric acid with oxygen and Fe(III) ions [287]. In the solution with benzothia-zole (BTAH) [287], the protective layer of BTAH that formed on the electrode surface inhibited the Zn corrosion. 

Inflammable air from the solution of metals in acids had been observed and commented on for at least a hundred years, but only after the attention of chemists had been directed toward gases generally did a systematic study appear. Cavendish obtained the inflammable air by dissolving zinc, iron, and tin in dilute vitriolic acid or in spirit of salt. The same metals also dissolved readily in nitrous (nitric) acid, and in concentrated vitriolic (sulfuric) acid with heat, but the resulting airs were not at all inflammable. He interpreted these reactions as follows ... 

The function of zinc ions may be either catalytic or stractural. Enzymes with a co-catalytic center of two or even three zinc ions in close proximity are also known. In a new type of zinc-binding site, the protein interface, zinc ions are fixed at the interface of two proteins with the aid of amino acid residues. The ligand residues are usually His, Asp, Glu or Cys, which interact via nitrogen, oxygen or sulfur donors with the metal ion. In catalytic binding sites. His coordination dominates and an additional reactive water molecule is bound. 

The absorption of sulfur dioxide in alkaline (even weakly alkaline) aqueous solutions affords sulfites, bisulfites, and metabisulfites. The chemistry of the interaction of sulfur dioxide with alkaline substances, either in solution, slurry, or solid form, is also of great technological importance in connection with air pollution control and sulfur recovery (25,227,235—241). Even weak bases such as zinc oxide absorb sulfur dioxide. A slurry of zinc oxide in a smelter can be used to remove sulfur dioxide and the resultant product can be recycled to the roaster (242). 

A number of complexes of zinc with benzothiazole and other sulfur-containing ligands have been described and the crystal structure of [NBuJ [ZnQ CNMe (02CMe), which contains a square pyramidal ZnS40 unit, has been reported.91 ... 

Reactions of a typical acid with metals. Use hydrochloric and/or sulfuric acid with magnesium, aluminium, zinc, iron and copper. R... 

Analysis of discharge particles revealed that both spherical and irregular particles were present, with approximately 1 in 12 spherical. The particle size range was from 3 to 160 pm. The elements detected were aluminum, calcium, chlorine, copper, iron, potassium, magnesium, phosphorus, lead, sulfur, antimony, silicon, titanium, and zinc, with calcium, chlorine, potassium, phosphorus, lead, and silicon the major elements. Antimony and lead did not occur together and none of the samples examined would be confused with FDR particles as their elemental profile differed. A small proportion of the particles containing either lead or antimony met the criteria for single element FDR particles. 

Preparation of AIC from Hypoxanthine. A search of the chemical literature revealed a paper by Friedman and Gots,21 who found that hypoxanthine was stable to heating in 1 N sulfuric acid. However, the same authors showed that when hypoxanthine was heated in 1.5 N sulfuric acid, with zinc dust added, extensive degradation occurred. The imidazole moiety of hypoxanthine was shown to be stable to the reducing conditions and the product of degradation was found to be a mixture of AIC and a structurally related compound. However, the mixture could not be separated, nor was the unknown compound identified. 

Summary Hydrogen gas is easily prepared by reacting hydrochloric acid or sulfuric acid with zinc or aluminum, or by reacting lye with aluminum foil. If using hydrochloric acid or sulfuric acid, avoid metal foils or finely divided metals such as aluminum foil, or zinc dust, as the reaction will be quite violent. For aluminum, aluminum pop cans house the best source, as they are cheap and readily available. 

Prepare zinc amalgam for use as follows Add 20- to 30-mesh zinc to a 2% mercuric chloride solution, using about 100 mL of the solution for each 100 g of zinc. After about 10 min, decant the solution from the zinc, then wash the zinc with water by decantation. Transfer the zinc amalgam to the reductor tube, and wash the column with 100-mL portions of 2 N sulfuric acid until 100 mL of the washing does not decolorize 1 drop of 0.1 N potassium permanganate. 

An old way of producing hydrogen gas in the laboratory was by the reaction of sulfuric acid with zinc metal... 

C-Dihydrotoxiferine I chloride, C-tolKsN +Cl, [a]D —600° (1 1 aqueous alcohol), has two N-methyl groups attached at the quaternary Nb nitrogen atoms (39). Molecular distillation of the alkaloid chloride gives nordihydrotoxiferine with loss of methyl chloride this ditertiary base can be converted back into the bisquatemary alkaloid, as the diiodide, by methylation with methyl iodide (39). Dehydrogenation of C-dihydrotoxiferine I with sulfur or with zinc dust gives isoquinoline... 

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