what happens when you combine FeS and carbon disulfide?
469693
Nothing. The two reactants have the same anion, so no reaction will take place. If you create a hypothetical double displacement reaction, you get:\n\nFeS + CS2 --> FeS + CS2\n\nAnd, so, there is no reaction.
780875
a)4 Fe + 3O2--->2 Fe2O3\n\nCH4 + 2O2 ---> CO2 +2 H2O
797459
mixture of iron and carbon produces steel but there may be some chromium in it.
156923
I don't know if this would be possible. The C atom is able to acheive this state, which is semi-unique to the group IV atoms such as Si, Ge, Pb, and Sn. \n\nFor a hydrogen atom to acheive sp2 hybridization it would have to skip 4 base states. This configuration is 'highly' improbable and would be 'highly' unstable requiring a steady influx of energy to retain this configuration.
7610
Yeah, you can use H2S gas... Hydrogen Sulphid. With just100 parts H2S per a Million parts of Air, it will knock you out in less than a 2 seconds, stop your respiratory functions as it paralyzes your nervous system. It’s made by combining Hydrogen and Sulphur Gases together. \nWell, seeing it comes from crude oil, it is relatively easy to find and make.\nOne short note; if you do not get the person into a breathable atmosphere within 4 minutes and revive them, they will die.
253297
Probably nothing since Arsenic is more electronegative than Mercury therefore no metathesis reaction will occur
532416
It is CS2+3(O2)=CO2+2(SO2)
723259
This lab involves putting iron (steel wool) into a solution of copper sulphate. The reaction produces metallic copper and iron sulphate solution. I've never been really sure if it's iron(II) sulphate or iron(III) sulphate as the product. I've used both equations with good results. \n\n   Fe   +  CuSO4   --->  Cu  +  FeSO4\n   2 Fe   +  3 CuSO4   --->  3 Cu  +  Fe2(SO4)3\n\n\nFor prelab, make up a saturated copper(II) sulphate solution\nTrust me. Otherwise, the kids will be filtering for hours.  \n\nHave containers available for appropriate disposal of reagents. And make sure they clean up all of the bits of steel wool from the lab benches. Those little bits will haunt you for weeks if they don't.\n\n\n\n\nMethod\n\n1. Obtain 100 mL of copper (II) sulphate solution in\n   a clean, dry beaker. \n\n2. Obtain about 10 g of steel wool. Record the exact mass.\n \n3. Place the steel wool into the copper(II) sulphate solution.  Stir with a glass rod. When the solution loses its blue colour, add more copper(II) sulphate solution.\n\n4. Continue stirring (and adding solution, if necessary)until the strands of steel wool are no longer apparent, and only particles of a reddish brown solid are visible.\n\n5. Record the mass of a piece of filter paper.\n   Place it into a funnel.\n \n6. Pour the mixture through filter paper in a funnel.\n   Rinse any residue in the beaker into the filter        paper      with distilled water. Rinse the solid in the filter paper with distilled water.\n\n7. Allow the solid and filter paper to dry, then find the combined mass.\n\n\nAnalysis\n\n1. If iron was the limiting reactant, predict the mass of copper which should have been formed. Show work.\n  \n2. Calculate the percentage difference between  the mass of copper predicted in question 1 and the actual amount of copper produced. Show all work.\n\n3. Discuss possible explanations for your results in question 2.\n\n\n\nGood luck !
11354
What about them?  Please be specific when you ask a question.\n\nIf using the Kodama pathway, you will get disulfides.
61085
it's called an addition reaction, where you are adding some atom or group of atoms to the carbons in acetylene. \nThis specific reaction is called sulfonation, adding a sulfate group to the carbons.
837624
Cassandra C has given you a very good answer.\nYou are interested in a single type of reaction: single displacement. It is a redox reaction so you have to think which compound is more happy having extra electrons (more electronegative).\n\nIn the case of A+BX-> AX + B, B(+) in BX is a cation and is missing an electron. If B is a more electronegative negative element than A, then it will steal away the electron from A and the reaction will occur. If A is more electronegative then B is not "strong" enough to steal the electron and the reaction will mot occur.\n\nIn the case of Y+BX -> BY+X you have the opposite. X(-) in BX has already an extra electron. So if X is more electronegative than Y it will not give away the electron and the reaction will not occur.\n\nThis is an oversimplified reasoning. The proper one is that you have to look at the standard reduction potentials (E0) which give the reactivity series. The half-reaction with the highest reduction potential will be the one favoured or more correctly the reaction will occur if the redox potential of the whole reaction is positive.\n\nFor instance you can find a detailed table at\nhttp://www.northland.cc.mn.us/Chemistry/standard_reduction_potentials.htm\n\nLet's see your reaction\nCu+FeSO4 -> CuSO4+ Fe \nIn this case the half reactions would be\nCu - 2e -> Cu(+2)\nFe(+2) +2e-> Fe\n\nFrom the website we get that for\nCu(+2) + 2e->Cu  E01=+0.342 Volt\nFe(+2) +2e-> Fe E02=-0.447 Volt\n\nE01 is more positive than E02 thus Cu(+2) tends to get electrons from Fe and not the other way around so the reaction will not occur \nOR\nYou find the E of the reaction like this.\nThe second half-reaction is in the form we want it. The first is in the reverse. So we just reverse the reaction and the sign for the potential\n\nCu -> Cu(+2) +2e E01'=-0.342\nFe(+2) +2e-> Fe E02=-0.447 and add\n\nCu + Fe(+2)+2e -> Cu(+2)+ Fe+ 2e with E=E01'+E02= -0.342+(-0.447) \n\nTherefore Cu+Fe(+2) -> Cu(+2) + Fe E= -0.789<0 and so the reaction will not occur.
13313
"Normal" bonding occurs when a ligand donates electrons to a metal. When a metal ion donates electrons back to the ligand, this is called back-bonding. The combination of normal bonding and back-bonding creates a strong bond between the ligand and the metal. The reason that phosphines, carbon monoxide, and cyanide are so poisonous is because they bond readily to iron in biological systems and cannot be displaced by the ligands (such as oxygen) which should bond to iron in normal metabolic processes.
942103
Well other then the obvious answer of sulfur smells like rotten eggs and that sulfur is very brittle, Iron won' burn if thrown in a fire whereas sulfur will combust and give off sulfur dioxide which if you bubble the smoke from burning sulfur through water will produce sulfuric acid.
752683
a) sulfur tetrafluoride\nb) molybdenum tetrachloride\nc) cobaltous sulfide or cobalt sulfide\nd) SnO\ne) ferric chloride\nf) CrO3\n\nComment: the above names are the ones you're most likely to encounter in industry or in a real-world laboratory.  Few chemists out here would call FeCl3 "iron three chloride"!\n\nOh, I know, your teacher probably expects "sulfur (IV) fluoride, molybdenum (IV) chloride, cobalt (II) sulfide, and iron (III) chloride..."
566520
Fe(s)+H2SO4(aq)excess--> Fe2+(aq) + SO42-(aq)+H2(g)\n\nratio is 1:1\n\n5gFe/55.85g/molFe= .090mol\n\nand\n\n1 molar solution =1 mole per liter\n\nso,\n\n.09mol(1 liter/1mol)= .09L or 90mls
504628
you'll have a mixture of hydrogen and oxygen
881429
Fe2O3(s) + 3 CO(g) ----> 2 Fe(l) + 3 CO2(g)\n\nCount up the oxygens; the left side and right side oxygens should match.