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Iron(II,III) sulfide is a blue-black (sometimes pinkish [citation needed]) chemical compound of iron and sulfur with formula Fe 3 S 4 or FeS·Fe 2 S 3, which is much similar to iron(II,III) oxide. It occurs naturally as the sulfide mineral greigite and is magnetic. It is a bio-mineral produced by and found in magnetotactic bacteria.
Iron sulfide or Iron sulphide can refer to range of chemical compounds composed of iron and sulfur. Minerals
The resulting solid decays at a temperature over 20 °C into iron(II) sulfide (FeS) and elemental sulfur: [3] Fe 2 S 3 → 2 FeS + S. With hydrochloric acid it decays according to the following reaction equation: [4] Fe 2 S 3 + 4 HCl → 2 FeCl 2 + 2 H 2 S + S
A task included an educational video with an explanation and examples on the topic. Afterwards, there was a quiz to complete, containing topic specific questions. The site was regularly updated and more topics were added to keep up with the General Certificate of Secondary Education (GCSE) mathematics curriculum. Students could complete tasks ...
Iron–sulfur clusters are molecular ensembles of iron and sulfide. They are most often discussed in the context of the biological role for iron–sulfur proteins , which are pervasive. [ 2 ] Many Fe–S clusters are known in the area of organometallic chemistry and as precursors to synthetic analogues of the biological clusters.
Iron sulfides occur widely in nature in the form of iron–sulfur proteins. As organic matter decays under low-oxygen (or hypoxic ) conditions such as in swamps or dead zones of lakes and oceans, sulfate-reducing bacteria reduce various sulfates present in the water, producing hydrogen sulfide .
A chemical equation is the symbolic representation of a chemical reaction in the form of symbols and chemical formulas.The reactant entities are given on the left-hand side and the product entities are on the right-hand side with a plus sign between the entities in both the reactants and the products, and an arrow that points towards the products to show the direction of the reaction. [1]
Consider the equation of roasting lead(II) sulfide (PbS) in oxygen (O 2) to produce lead(II) oxide (PbO) and sulfur dioxide (SO 2): 2 PbS + 3 O 2 → 2 PbO + 2 SO 2. To determine the theoretical yield of lead(II) oxide if 200.0 g of lead(II) sulfide and 200.0 g of oxygen are heated in an open container: