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Ferric oxide

Basic information Physical Properties Occurrence and Uses Preparation Reactions Safety Related Supplier
Ferric oxide Basic information
Ferric oxide Chemical Properties
  • Melting point:1538°C
  • Density 5.24
  • Flash point:>230 °F
  • storage temp. 2-8°C
  • solubility It is soluble In Warm Hydrochloric Acid, Slightly Soluble in Sulfuric Acid.
  • form pieces
  • Specific Gravity5.1~5.2
  • color black
  • PH3.7±0.3
  • Water Solubility INSOLUBLE
  • Merck 14,4028
  • Stability:Stable.
  • CAS DataBase Reference1309-37-1(CAS DataBase Reference)
  • NIST Chemistry ReferenceIron(iii) oxide(1309-37-1)
  • IARC3 (Vol. 1, Sup 7) 1987
  • EPA Substance Registry SystemFerric oxide (1309-37-1)
Safety Information
MSDS
  • Language:EnglishProvider:ALFA
Ferric oxide Usage And Synthesis
  • Physical PropertiesReddish-brown hexagonal crystal; refractive index 2.91; density 5.25g/cm3; Moh’s hardness 6.0; melts at 1565°C; insoluble in water; dissolves in acids.
    red iron oxide powder
  • Occurrence and UsesFerric oxide occurs in nature as the mineral hematite. It is the principal ore of iron from which the metal and its alloys are produced. Also, this oxide occurs in the mineral, limonite, 2Fe2O3•3H2O. An important application of this compound involves producing red, orange, and yellow pigments. Other applications are in coatings for metals, steel and rubber; in ceramics; and as a catalyst for oxidation reactions.
  • PreparationFerric oxide is prepared as a reddish-brown hydrated precipitate by treating an aqueous solution of an iron(III) salt with caustic soda:
    2FeCl3 + 6NaOH → Fe2O3•3H2O + 6NaCl
    It also is obtained by thermal decomposition of iron(II) sulfate or the brown oxide hydroxide:
    2FeSO4 → Fe2O3 + SO2 + SO3
    2FeO(OH) → Fe2O3 + H2O
    The oxide is prepared in industrial scale by first precipitating iron(II) hydroxide Fe(OH)2 by treating aqueous solutions of iron(II) sulfate and caustic soda. The Fe(OH)2 is then oxidized to iron(III) hydroxide by aeration. The latter is dehydrated by heating:
    Fe2+ (aq) + OH¯ (aq) → Fe(OH)2(s) → 2Fe(OH)3 → Fe2O3 + 3H2O
    It also is produced by ignition of iron(III) oxalate and iron carbonyls:
    2Fe2(C2O4)3 +3O2 → 2Fe2O3 + 12CO
  • ReactionsFerric oxide decomposes to its elements when heated at elevated temperatures:
    2Fe2O3 → 4Fe + 3O2
    The oxide is reduced by most reducing agents. Reaction with carbon monoxide at elevated temperatures (that occurs in the blast furnace) gives metallic iron. The overall reaction is mildly exothermic (ΔHrxn –113.4 kcal/mol):
    2 Fe2O3 + 6CO → 4Fe + 6CO2
    It also is reduced by powdered aluminum at elevated temperatures, forming aluminum oxide and metallic iron:
    Fe2O3 + 2Al → Al2O3 + 2Fe
    The reaction is highly exothermic and becomes self-sustaining after ignition.
    When heated with sand in an electric furnace, iron(III) oxide forms ferrosilicon alloy. When heated in a vacuum at 1,000°C, it forms triiron tetroxide, Fe3O4.
  • DescriptionIron oxides are produced synthetically and consist essentially of anhydrous and/or hydrated iron oxides. The range of hues includesyellows, reds, browns and blacks. Food quality iron oxides are primarily distinguished from technical grades by the comparatively low levels of contamination by other metals. This is achieved by the selection and control of the source of iron and/or by the extent of chemical purification during the manufacturing process. Iron oxides have been used to color confectionery, fillings and decorations for pastry products, cheese products, fish paste, pet foods, cosmetics and pharmaceutical products.
  • Chemical PropertiesHematite is a noncombustible, black to black red or brick-red mineral (iron ore) composed mainly of ferric oxide, Fe2O3. Ferric oxide
  • OccurrenceIron(III) oxide occurs in nature as the mineral hematite. It is the principal ore of iron from which the metal and its alloys are produced. Also, this oxide occurs in the mineral, limonite, 2Fe2O3?3H2O. An important application of this compound involves producing red, orange, and yellow pigments. Other applications are in coatings for metals, steel and rubber; in ceramics; and as a catalyst for oxidation reactions.
  • UsesRed iron oxide (Fe2O3) is an inorganic pigment of either natural or synthetic origin. It is a low chroma red with excellent durability and low cost. Synthetic pigment is made by heating iron sulfate with quicklime in a furnace. The second preparatory technique involves calcining iron sulfate in the presence of air at high temperatures. Natural and oxides of iron are mined either as the mineral hematite (Fe2O3) or as hematite in its hydrated form.
  • UsesAs pigment for rubber, paints, paper, linoleum, ceramics, glass; in paint for ironwork, ship hulls; as polishing agent for glass, precious metals, diamonds; in electrical resistors and semiconductors; in magnets, magnetic tapes; as catalyst; colloidal solutions as stain for polysaccharides.
  • UsesFerric Oxide is a nutrient and dietary supplement that is a source of iron.
  • DefinitionA high-grade red pigment used as a polishing agent for glass, jewelry, etc. (2) A cosmetic prepared from dried flowers of the saf- flower.
  • DefinitionA black solid prepared by passing either steam or carbon dioxide over redhot iron. It may also be prepared by passing steam over heated iron(II) sulfide. Triiron tetroxide occurs in nature as the mineral magnetite. It is insoluble in water but will dissolve in acids to give a mixture of iron(II) and iron(III) salts in the ratio 1:2. Generally it is chemically unreactive; it is, however, a fairly good conductor of electricity.
  • PreparationIron(III) oxide is prepared as a reddish-brown hydrated precipitate by treating an aqueous solution of an iron(III) salt with caustic soda:
    2FeCl3 + 6NaOH → Fe2O3?3H2O + 6NaCl
    It also is obtained by thermal decomposition of iron(II) sulfate or the brown oxide hydroxide:
    2FeSO4 → Fe2O3 + SO2 + SO3
    2FeO(OH) → Fe2O3 + H2O
    The oxide is prepared in industrial scale by first precipitating iron(II) hydroxide Fe(OH)2 by treating aqueous solutions of iron(II) sulfate and caustic soda. The Fe(OH)2 is then oxidized to iron(III) hydroxide by aeration. The latter is dehydrated by heating:
    Fe2+ (aq) + OHˉ (aq) → Fe(OH)2(s) → 2Fe(OH)3 → Fe2O3 + 3H2O
    It also is produced by ignition of iron(III) oxalate and iron carbonyls:
    2Fe2(C2O4)3 +3O2 → 2Fe2O3 + 12CO
    .
  • HazardPneumoconiosis. Questionable carcinogen.
  • Potential ExposureHematite; as an iron ore composed mainly of ferric oxide, is a major source of iron and is used as a pigment for rubber, paints, paper, linoleum, ceramics, dental restoratives; and as a polishing agent for glass and pre cious metals. It is also used in electrical resistors, semiconduc tors, magnets, and as a catalyst. Human exposure to hematite from underground hematite mining is principally through inhalation and/or ingestion of dusts. No estimates are available concerning the number of underground miners exposed.
  • CarcinogenicityWelders are typically exposed to a complex mixture of dust and fume of metallic oxides, as well as irritant gases, and are subject to mixeddust pneumoconiosis with possible loss of pulmonary function; this should not be confused with benign pneumoconiosis caused by iron oxide.1 Although an increased incidence of lung cancer has been observed among hematite miners exposed to iron oxide, presumably owing to concomitant radon gas exposure, there is no evidence that iron oxide alone is carcinogenic to man or animals.6
  • IncompatibilitiesContact with hydrogen peroxide, ethyl ene oxide, calcium hypochlorite will cause explosion. Violent reaction with powdered aluminum; hydrazine, hydrogen trisulfide.
Ferric oxide Preparation Products And Raw materials
Ferric oxide (1309-37-1)Related Product Information
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