what is the geochemical significance of manganese to be in road dust and soil
138756
Manganese is one of the more abundant elements in the earth's\n    crust and is widely distributed in soils, sediments, rocks, water, and\n    biological materials. The major sources of man-made environmental\n    pollution by manganese arise in the manufacture of alloys, steel, and\n    iron products. Other sources include mining operations, the production\n    and use of fertilizers and fungicides, and the production of synthetic\n    manganese oxide and dry-cell batteries. Organomanganese fuel\n    additives, though only a minor source at present, could significantly\n    increase exposure, if they come into widespread use. Average manganese\n    concentrationsa in soils range from about 500 to 900 mg/kg and\n    concentrations in sea water range from 0.1 to 5 µg/litre. Surface\n    waters may have a manganese content of 1-500 µg/litre, but in areas\n    where high concentrations of manganese occur naturally, levels may be\n    considerably higher. Average manganese levels in drinking water range\n    from 5 to 25 µg/litre.\n\n        Manganese is present in all foodstuffs, usually at concentrations\n    below 5 mg/kg. However, concentrations in certain cereals, nuts, and\n    shellfish can be much higher, exceeding 30 mg/kg in some cases. Levels\n    in finished tea leaves may amount to several hundred mg/kg.\n\n        Manganese has been found in measurable quantities in practically\n    all air samples of suspended particulate matter. Annual average levels\n    in ambient air in unpolluted urban and rural areas vary from 0.01 to\n    0.07 µg/m3.
530321
The reductive dissolution of goethite ( -FeOOH) and hematite ( -Fe 2 O 3 ) by phenolic reductants has been examined in order to improve the understanding of iron transformations in soils, sediments and aquifers. Rates of goethite reductive dissolution by hydroquinone increased as the pH was increased from pH 1.8 to 4.65, arid the following reaction stoichiometry was obeyed: 2 - FeOOH + QH 2 = 2 Fe 2+ + Q + 4 OH - . As the pH was increased from pH 4.5 to 6.0, the reductive dissolution rate decreased to below the detection limit. At pH 3.4, the reductive dissolution of hematite was two orders of magnitude slower than goethite. The relationship between structure and reactivity was examined for a series of mono-, di-, and tri-hydroxybenzene reductants. Rates of reductive dissolution decreased in the following order: catechol ~- hydroquinone 〉 3,4-dihydroxybenzoic acid 〉 resorcinol-phenol-4-hydroxybenzoic acid.
38717
Some of the matals have multiple oxidation states and these must be indicated in the names:\nAmericurium (III) fluoride\nIndium (III) fluoride\nBarium permanganate\nNeodymium (III) iodide\nCadmium sulfite\nSilicon tetrathiocyanate\nVanadium (III) fluoride\nIron (III) dichromate\nGold (I) cyanide\nBarium bromate\nMagnesium molybdate\nPlutonium (III) bromide\nSamarium (III) sulfate\nTungsten (II) iodide\nPotassium borate
266648
i would imagine you'd have issues with electrochemical reactions between the copper and the various heavy metals in the tailings.  This of course is completley dependant on what is contained in your specific tailings, and what the concentrations of these metals are.  Overall, talk to an engineer familiar with the site for more details
344138
If you assume Iron(III) oxide (ferric oxide, Hematite, red iron oxide, synthetic maghemite, colcothar), then no.
325922
You are looking for element #29 - Copper (Cu).
397695
The "half-life" of an element is important for determining the absolute age of a rock.\n\nThe answer is C.
76621
Yea, the first answer is right.  Among many other factors, soils are made up of parent material that has decomposed.  It mostly depends on what kind of rock they came from.
69427
Iron (III) oxalate ---> Fe2(C2O4)3\n{valency of oxalate i.e. C204 is -2 and of Fe is +3}\n\nLead (II) carbonate---> PbCO3\n{valency of Pb is +2 and of CO3 is -2}
403482
a) 3SiO2 +2 Al --->3 Si + 2Al2O3\n\nb)AgNO3 +HCl---> AgCl +HNO3\n\nc) Mg + CuSO4 ---> MgSO4 + Cu\n\nd) Pb(NO3)4 +4 NaI --->4 NaNO3 + PbI4 (s)
548756
Mn(+3) has the electronic configuration of 1s(2) 2s(2) 2p(6) 3s(2) 3o(6) 3d(2)\n\nthe one before me missed the 4s2 so his is wrong
530524
Just a guess: Because of all the coal around this area, I would suppose that sulfide minerals, especially pyrite (iron sulfide) would be common. Some sphalerite (Zn, Fe sulfide) has been found in Lucerne county. Some rozenite (hydrated Fe sulfate) has been reported from Jeddo Highland coal mine in Hazleton.\n\n"Sulfide minerals typically occur in coal beds as well as in strata overlying and underlying the coal. Weathering and aqueous dissolution of the sulfide mineral oxidation products, including dissociated sulfuric acid and metals (e.g., Fe, Mn, Al), produces surface and groundwater degradation." \nwww.epa.gov/waterscience/ guide/coal/support/support2.pdf\n\n"By far the most serious environmental problem caused by abandoned mines is polluted water. It happens when rain comes into contact with a surface or underground mine and interacts with the mineral pyrite, better known as fools' gold, to form sulfuric acid. The toxic brew discharges into streams and rivers, choking off plants and wildlife and coating streambeds with iron hydroxide, tinting water yellow, red or orange. Aluminum, manganese and other metals also leach into the water.\nOld mining operations have polluted about 4,000 miles, or 5 percent, of the rivers and streams in Pennsylvania, officials estimate. The west branch of the mighty Susquehanna River is dead for its upper 70 miles; 1,000 miles of its tributaries are likewise lifeless. The Jeddo Tunnel, an engineering marvel drilled through miles of solid rock to drain deep mines in the Hazleton area, discharges 40,000 gallons of polluted water a minute into the Little Nescopeck Creek -- the largest such discharge in a state full of them."\nhttp://www.theminingnews.org/news.cfm?newsID=951
667986
You could try passing it through carbon, but that may also remove iron.  You would need to try it with known solutions.\nYou may need to go to AA or ICP analysis.
373228
Fe2O3 is Hematite.  Fe3O4 is Magnetite.\n\nSmelting Hematite would give:\n\nFe2O3 + 3 CO --> 2 Fe + 3 CO2\n\nOne mole (GMW) of Hematite will give 2 atomic weights of Iron.  This means that 159.7 grams of Hematite will produce 2 time 55.8 grams of Iron.\n\nMagnetite contain a higher percentage of Iron than Hematite does.  3 out of 7 atoms is more than 2 out of 5.
514142
Given   X  amount of magnesium, it will form MgO to the extent of the amount of magnesium. The magnesium is the limiting factor. \n\nOxygen is much more reactive than nitrogen. The magnesium would rather react with the oxygen because it takes less energy, despite the very hot and bright light given off when Mg burns.\n\nAbout the only way that nitrogen ever combines with anything from the air is when it is compressed in a cylinder of an internl combustion engine and  forced to combine under pressure and heat and  nitrogen oxides are released to form smog.
264490
Potassium manganate or potassium permanganate?  And I'm assuming a solution of iron(II).\n\nBeyond the corrosivity of the sulfuric acid, and the oxidizing capability of the manganese species, as well as its ability to stain EVERYTHING, there are no additional hazards.  Permanganate stains can be removed by addition of an hydroxylamine solution (either the sulfate or the chloride).
545174
WARNING:  Answer is NOT OXYGEN.\n\nIt is true that when metals rust, it forms metal oxides.  But by definition, Catalyst Speeds up the process of the Rxn but does not get used up.  However as you can see in the equation below, Oxygen is consumed with metal to for metal oxide.  Therefore Oxygen CAN'T be a catalyst.  It is a reactant.\n\nFe + O2 ---> Fe2O3\n\nThe Correct answer is SALT.  (Sodium in NaCl for an example)\n  \nRust is the process of metal oxidizing into metal oxide.  The oxidation needs a transfer medium to occur, such as water. Salt in the water speeds up the oxidation process by acting as a catalyst.  The salt is never used up and the problem with salt is that even when water is gone, it remains and wait to restart the forming of rust once more moisture is present.  This is why metals rust much easily in salty areas such as beaches and cold states where they use salt to melt the icy roads.   \n\nI hope you get my answer in time, if this question if for school.  I know I'm against 3 answers here but let my past records of best answers speak for itself.