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Forms of iron sulfide
"Iron sulfide" exists in several distinct forms which differ in the stoichiometry and properties:- Pyrrhotite, Fe1-xS, a mineral as well as the waste product of the Desulfovibrio bacteria, pyrrhotite displays ferrimagnetism and crystallizes in monoclinic system.
- Troilite, FeS, which has similar material to pyrrhotite, but does not possess ferromagnetic properties due to stoichiometric composition and crystallizes in hexagonal system.
- Mackinawite, Fe1+xS (often written as (Fe,Ni)9S8), the least stable form of iron sulfide, mackinawite has a layered structure.
- Pyrite, mineral form of the iron disulfide (FeS2) with a gold-like appearance, making it also known as "fool's gold" (the related mineral is marcasite).
- Keilite (Fe,Mg)S was recently found in a meteorite. Read full entry
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- 1.Iron sulfide - Wikipedia, the free encyclopedia
- Iron sulfide. From Wikipedia, the free encyclopedia. Jump to: navigation, search. Iron sulfide or Iron sulphide may refer to a chemical compound of iron and ...
- http://en.wikipedia.org/wiki/I
ron_sulfide
- 2.Iron Disulfide (FeS2) from READE
- Manufacturer, custom toll processor and global distributor of higher tech ... Iron disulfide= FeS2, and Iron sulfide (Iron (II) sulfide)= FeS. Description: ...
- http://www.reade.com/Products/
Sulfides/iron_disulfide.html
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How do I find the mass of iron |
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convert 432 g of Fe2O3 to moles by dividing by its molar mass. then multiply by mole ratio (2/4) then take answer and multiply by the molar mass of FeS |
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How do you remove iron (II) it's a solid piece of iron,
coated in iron sulfide.
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Use a magnet to remove the iron from the iron(II) sulfide. |
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iron (II) sulfide reacts with how many grams of acid are
needed to react with 75.0
grams of iron (II) sulfide ore
which contains 30.0% inert
material?
please provide the formula for
me
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First generate the balanced equation for the reaction. Note; we need 2 HCl's to make everything come out OK: FeS + 2 HCl ---> FeCl2 + H2S Now, correct for actual composition of iron(II) sulfide in 70% pure ore: 75g x [100 - 30]% = 52.5g of FeS present in the sample: Determine no of moles of FeS present: 52.5g/[55.85 + 32.06]g/mole = 0.597mole Now, from the ratios of the balanced equation and the number of moles of iron sulfide present you can calculate moles of HCl reqired. 0.597mole x (2 mole HCl/mole FeS) = 1.194 moles HCl. To get grams of HCl needed, multiply moles HCl by grams HCl: 1.194moles x (35.45 + 1.01) = 43.5g HCl You could put all the steps together as: (75g x 0.70%) x (2/1) x (35.45 + 1.01)g/mole/(55.85 + 32.06)g/mole = 43.5g HCl Remember, this is the weight of HCl as a pure gas that would be required; the hydrochloric acid you have in the lab is HCl dissolved in water so the weight of HCl solution required would depend on the concentration. |
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