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Iron

Iron Suppliers list
Company Name: Sinopharm Chemical Reagent Co,Ltd.  Gold
Tel:86-21-63210123
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Products Intro:Product Name:Iron powder reduced
CAS:7439-89-6
Package:500g
Company Name: Shanghai Aladdin Bio-Chem Technology Co.,LTD  Gold
Tel:021-20337333/400-620-6333
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Products Intro:Product Name:Iron ion standard solution
CAS:7439-89-6
Purity:1mg/ml in 0.005% HN03 Package:859RMB/100ML
Company Name: J & K SCIENTIFIC LTD.  
Tel:400-666-7788 +86-10-82848833
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Products Intro:Product Name:Iron, powder
CAS:7439-89-6
Purity:99% Package:100g,2.5KG,500G
Company Name: Meryer (Shanghai) Chemical Technology Co., Ltd.  
Tel:+86-(0)21-61259100(Shanghai) +86-(0)755-86170099(ShenZhen) +86-(0)10-62670440(Beijing)
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Products Intro:Product Name:Iron
CAS:7439-89-6
Purity:98% Package:500g Remarks:AAA125316
Company Name: Alfa Aesar  
Tel:400-610-6006; 021-67582000
Email:saleschina@alfa-asia.com
Products Intro:Product Name:Iron powder, reduced, 99%
CAS:7439-89-6
Package:250g Remarks:A10411
Iron Chemical Properties
Melting point 1535 °C(lit.)
Boiling point 2750 °C(lit.)
density 7.86 g/mL at 25 °C(lit.)
Fp >230 °F
storage temp. -70°C
solubility H2O: soluble
form wire
color Silvery
Water Solubility INSOLUBLE
Sensitive Moisture Sensitive
Merck 13,5109
Stability:Stable. Reacts slowly with moist air and water. Dust may form an explosive or combustible mixture with air. Incompatible with organic acids, strong oxidizing agents, water, mineral acids.
CAS DataBase Reference7439-89-6(CAS DataBase Reference)
NIST Chemistry ReferenceIron(7439-89-6)
EPA Substance Registry SystemIron(7439-89-6)
Safety Information
Hazard Codes F,Xi
Risk Statements 36/38-11-17
Safety Statements 26-16-33-24/25
RIDADR UN 3264 8/PG 3
WGK Germany 1
RTECS NO4565500
TSCA Yes
HazardClass 8
PackingGroup III
HS Code 72052900
Hazardous Substances Data7439-89-6(Hazardous Substances Data)
MSDS Information
ProviderLanguage
Iron Filings English
SigmaAldrich English
ACROS English
ALFA English
Iron Usage And Synthesis
HistoryIron has been known to mankind from early civilization. In fact, a period of history, the “iron age,” is named for the widespread use of this metal. For almost a thousand years, it remained as the single most-used metal, and its use in mechanization made the industrial revolution possible.
Iron, after oxygen, silicon and aluminum, is the fourth most abundant element in the earth’s crust. It is the prime constituent of earth’s core along with nickel. Its abundance in the crust is 5.63%. Its concentration in the seawater is about 0.002mg/L. The principal ores of iron are hematite, Fe2O3; pyrite, Fe2S2; ilmenite, FeTiO3; magnetite, Fe3O4; siderite, Fe2CO3; and limonite [FeO(OH)]. It also is found in a number of minerals, such as corundum, as an impurity. It also is found in meteorites.
Iron occurs in every mammalian cell and is vital for life processes. It is bound to various proteins and found in blood and tissues. The iron-porphyrin or heme proteins include hemoglobin, myoglobin and various heme enzymes, such as cytochromes and peroxidases. Also, it occurs in non heme compounds, such as ferritin, siderophilin, and hemosiderin. Hemoglobin, found in the red blood cells, is responsible for transport of oxygen to the tissue cells and constitutes about two-thirds (mass) of all iron present in the human body. An adult human may contain about 4 to 6 grams of iron.
Chemical propertiesGray metal; It should be dissolved in hydrochloric acid, sulfuric acid and dilute nitric acid.
Content analysisAccurately weigh approximately 200 mg of the sample and transfer it into a 300 ml Erlenmeyer flask, add 50 ml of a dilute sulfuric acid solution (TS-241). Use a plug containing a Bunsen valve (the production method is to insert a glass tube connected with a short segment of rubber tube to the plug. The side of the rubber tube has a long slit while the other side is inserted of a glass rod so that the gas can escape and the air can’t enter). The solution was heated on a steam bath to dissolve the iron. After cooling, dilute with 50 ml of freshly boiled and cooled water. Add 2 drops of the test solution (TS-162) to 0.1 mol/L
Apply cerium sulfate titration to until the red color becomes light blue color. Each ml of 0.1mol/L of high cerium sulfate are equivalent to 5.585 mg of iron (Fe).
The method is the same as that of "reduced iron (01219)”.
UsesIndustrial uses of iron as carbon steels are numerous and surpass any 410 IRONother alloys. Carbon steels are alloys of iron containing carbon in varying proportions, usually up to 1.7% carbon. Other metals also are incorporated into carbon steels to produce low-alloy steels. Such metals are usually nickel and chromium and are classified as stainless steel, tool steels, and heat-resistant steels. Non-steel iron alloys such as cast iron, wrought iron, nickel iron and silicon iron also have many important applications. Another important application of iron is as an industrial catalyst. It is used in catalyst compositions in the Haber process for synthesis of ammonia, and in Fischer-Tropsch process for producing synthetic gasoline.The followings are some examples of common applications:
  • pharmaceuticals, pesticides, powder metallurgy and so on;
  • as a hot hydrogen generator, gel propellant, combustion activator, catalyst, water cleaning adsorbent, sintered active agent, etc;used for powder metallurgy products, all kinds of mechanical parts and components products, cemented carbide products, etc;
  • as a reducing agent as well as being used for iron salt manufacturing and electronics industry;
  • as nutritional supplements (iron fortifier),for casting,or as reducing agent;
  • in the electronics industry, powder metallurgy.
Production MethodsMost iron produced today is from its oxide minerals, hematite and magnetite. The process involves reducing mineral iron with carbon in a blast furIRON 411nace. There are several types of blast furnaces which vary in design and dimensions. The overall processes, however, are more or less the same. One such process is outlined below:
The mixture of ore, coke and limestone is fed into the blast furnace from the top. The materials are preheated to about 200°C in the top most zone. Hematite is partially reduced to magnetite and then to FeO by the ascending stream of carbon monoxide formed at the bottom and mid zones of the furnace resulting from high temperature oxidation of carbon. The ferrous oxide FeO formed at the top zone is reduced to metallic iron at about 700°C in the mid zone by carbon monoxide. A hot air blast at 900°C passes through the entire furnace for a very short time (usually for a few seconds). This prevents any gassolid reaction product from reaching equilibrium. In the temperature zone 700 to 1,200°C ferrous oxide is completely reduced to iron metal by carbon monoxide. Also, more CO is formed by oxidation of carbon by carbon dioxide. Further down the furnace at higher temperatures, around 1,500°C, iron melts, dripping down into the bottom. Also, in this temperature zone acidic silica particles react with basic calcium oxide produced from the decomposition of limestone, producing calcium silicate. The molten waste calcium silicate also drips down into the bottom. In the hottest zone of the blast furnace, between 1,500 to 2,000°C, some carbon dissolves into the molten iron. Also at these temperatures any remaining silicates and phosphates are reduced to silicon and phosphorus, and dissolve into the molten iron. Additionally, other tract metals such as manganese dissolve into the molten iron. The impure iron melt containing about 3 to 4% carbon is called “pig iron”. At the bottom, the molten waste slag floats over the impure pig iron melt that is heavier than the slag melt and immiscible with it. Pig iron is separated from the slag and purified for making different types of steel. Chemical reactions and processes occurring in various temperature zones of blast furnace are summarized below:  production method   Pig iron produced in the blast furnace is purified and converted to steel in a separate furnace, known as a basic-oxygen furnace. Jets of pure oxygen gas at high pressure are blown over and through the pig iron melt. Metal impurities are converted into oxides. Part of the dissolved carbon in the impure iron melt is converted into carbon dioxide gas. Formation of SiO2, CO2, and other metal oxides are exothermic reactions that raise the temperature to sustain the melt. A lime flux (CaO) also is added into the melt, which converts silica into calcium silicate, CaSiO3, and phosphorus into calcium phosphate, Ca3(PO4)2, forming a molten slag immiscible with molten steel. The lighter molten slag is decanted from the heavier molten steel.  
MiningChina pyrrhotite-type sulfur pyrite mine has less of mining hills resources. Take the MinXi mine in the DaTian City, Fujian Province and Zhangjiagou mine in Dandong City, Liaoning Province as the representatives; both of them are underground mining mines. The former applies the Housing pile mining method while the later one uses the section mining method. The pit mining process is the same as the method of "phosphate rock." Beneficiation methods include flotation process and flotation-magnetic combined process.
ToxicityIron Powder: GRAS (FDA, § 184.1375, 2000); Inhalation of dust can cause pneumoconiosis. Operation personnel should wear overall, wear dust masks and other labor insurance products. Production equipment should be closed, the workshop should be well-ventilated. Be sure to pay attention to dust protection.
UsesAlloyed with C, Mn, Cr, Ni, and other elements to form steels. Nutritional supplement in wheat flours, corn meal, grits and other cereal products. 55Fe and 59Fe used in tracer studies; the former in biological studies.
General DescriptionA gray lustrous powder. Used in powder metallurgy and as a catalyst in chemical manufacture.
Air & Water ReactionsHighly flammable. May react with water to give off hydrogen, a flammable gas. The heat from this reaction may ignite the hydrogen.
Reactivity ProfileIron is pyrophoric [Bretherick, 1979 p. 170-1]. A strong reducing agent and therefore incompatible with oxidizing agents. Burns in chlorine gas [Mellor 2, Supp. 1:380 1956]. Reacts with fluorine with incandescence [Mellor 13:314, 315, 1946-1947].
Health HazardFire may produce irritating and/or toxic gases. Contact may cause burns to skin and eyes. Contact with molten substance may cause severe burns to skin and eyes. Runoff from fire control may cause pollution.
Fire HazardFlammable/combustible material. May be ignited by friction, heat, sparks or flames. Some may burn rapidly with flare burning effect. Powders, dusts, shavings, borings, turnings or cuttings may explode or burn with explosive violence. Substance may be transported in a molten form at a temperature that may be above its flash point. May re-ignite after fire is extinguished.
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