A popular chemistry; . 58 INORGANIC CHEMISTRY. known odor of the S02. FeS2 is used as a source ofS, and is roasted to furnish S02 in the manufactureof H2S04. Ferrous Sulphate (FeS04,7H20), Green Vitriol,Copperas, is made by the action of H2S04 on Fe, and,at Stafford, Connecticut, and other places, from FeS2,by exposure to air and moisture. It is used in dyeing,making ink, and in photography. ZINC. Symbol, Zn Atomic Weight, 65 Specific Gravity, Fusing Point, 811° F. or 433° C. Source.—Zn is found as ZnO, or red oxide, in NewJersey, and as ZnS, or zinc blende, in many places. Preparation.—Z
A popular chemistry; . 58 INORGANIC CHEMISTRY. known odor of the S02. FeS2 is used as a source ofS, and is roasted to furnish S02 in the manufactureof H2S04. Ferrous Sulphate (FeS04,7H20), Green Vitriol,Copperas, is made by the action of H2S04 on Fe, and,at Stafford, Connecticut, and other places, from FeS2,by exposure to air and moisture. It is used in dyeing,making ink, and in photography. ZINC. Symbol, Zn Atomic Weight, 65 Specific Gravity, Fusing Point, 811° F. or 433° C. Source.—Zn is found as ZnO, or red oxide, in NewJersey, and as ZnS, or zinc blende, in many places. Preparation.—ZnO* is smeltedon the same principle as iron ore,by heating with C. The reactionis as follows: ZnO + C = Zn + CO. The Zn distils from the cruciblea and is collected in the receiverd while the CO escapes. Properties.—Zn is ordinarilybrittle, but when heated to 200°or 300° F., it becomes malleable,and can be rolled out into thesheet Zn in common use. At about400° F. it is so brittle that it can be powdered in a. Reduction of Zinc Ore. * ZnS is roasted to convert it into ZnO. zinc. 159 mortar. It burns in the air with a magnificent bluishlight, forming flakes of ZnO, formerly called Phi-losophers Wool. When exposed to the air Zn soonoxidizes, and the thin film of oxide formed over thesurface protects it from further change. Uses.—Its economic uses are familiar. Sheet ironcoated with Zn by being dipped in melted Zn formswhat is termed galvanized iron. Water-pipes linedin this way with Zn are as unsafe as lead (see p. 162)until the Zn is entirely corroded. The oxide andcarbonate of zinc are rapidly formed, and thesepoisonous salts remain in the H20. There is thesame objection to metallic-lined ice-pitchers. Gal-vanic action between the metals promotes standing in reservoirs lined with Zn should notbe used for drinking purposes. In the case of zinc-covered roofs the rain-water contains zinc* Compounds. — Zinc Oxide, ZnO, is sold as zinc-white, and is value
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Keywords: ., bookcentury1800, bookdecade18, booksubjectchemistry, bookyear1887
