The chemical reaction of 2Ag + S--->AgS?
339176
The result is Ag2S: Ag+ is monovalent, S2- is the sulphide ion.\n\nA solid silver surface will blacken (slowly) when exposed to material containing bound (negatively charged) sulphur atoms (such as the amino acid cystein and proteins containing it). Dissolved silver will precipitate.
853922
These are the right ones:\n\n2K(s) + 2H2O(l) ---> 2KOH(aq) + H2(g)\nH2SO4(aq) + 2KOH(aq) ---> K2SO4(aq) + 2H2O(l)\nCa(OH)2(aq) + 2HCl(aq) ---> CaCl2(aq) + 2H2O(l)
705507
This is a Double Replacement Rxn:\n\nMgCl2 (aq) + Li2CO3 (aq) --> MgCO3(s) + LiCl(aq)\n\nSince the reaction of two aq reactants yield solid MgCO3, it can also be considered Metathesis reaction.  Remember, Metathesis reaction is a double replacement reaction that forms Solid, Liquid or Gas.
744573
You added 0.04 liter * 0.07891 mol/liter = 3.156*10^-3 moles of Ag as AgNO3 to the dissolved unknown sample.  \n\nHowever, there was excess Ag added.  The "extra" Ag amounted to:\n\n0.01127 liter * 0.1 mol/liter = 1.127*10^-3 moles Ag\n\n\nSo the net amount of Ag that reacted with the AsO4(3-) ion was \n\n3.156*10^-3 - 1.127*10^-3 = 2.029*10^-3 moles Ag.\n\nIt takes three moles of Ag for every one mole of As to make Ag3AsO4, so the precipitate consisted of \n\n2.029*10^-3 moles/3 = 6.765*10^-4 moles Ag3AsO4, which, of course, contains 6.765*10^-4 moles of As.\n\nThe molecular mass of As2O3 is 197.8414 gm/mol, but each formula unit of this compound contains 2 As atoms, while the Ag3AsO4 precipitate only contains 1 As atom per formula unit.  If we rewrite the formula of As2O3 as AsO1.5, it would have a molecular mass of 197.8414/2 gm/mol = 98.921 gm/mol.\n\nThe precipitate contains 6.765*10^-4 moles of As, and this amount of As as an oxide would have a mass of:\n\n6.765*10^-4 moles * 98.921 gm/mol =  gm As2O3\n\nIf the initial sample had a mass of 1.223 grams, then this mass of As2O3 constituted a mass fraction of:\n\n6.692*10^-2/1.223 = 5.472*10^-2 = 5.472 wt %
753121
Ok, now this one I can do:\n\nMg3N2  ---> 3Mg (s) + N2 (g)
738281
I have forgotten all the chemical formulas & whatnot... but I'm going to do this assuming that I'm right for the following:\n\n(note that if i get any of these wrong you'll have to make appropriate changes, this is just to show you HOW to do this)\nCu = Copper\nS = Sulfur\nCuS2 = Copper Sulfide\n\nSo first step is to balance the equation\n\nCu + 2S -> CuS2\n\nso then you can set up a problem like this:\n\n0.90 mol Cu * 1 mol CuS2  = # mol copper sulfide yielded\n(this is because there was 1 mole of Copper in 1 mole of CuS2.. so if CuS2 is not the correct formula change the "1 mol CuS2" accordinginly)\n\n\nThen add up the # of grams in 1 mol of copper sulfide\n\ndo that by taking the # of grams in 1 mol of copper + the number of grams in 2 mol of sulfur (again, this is just assuming that copper sulfide IS CuS2).  Once you've gotten that figure, multiply it by the number found from the earlier problem (# mol copper sulfide yielded).  This gives you the amount of grams.  To change this number to kilograms, divide it by 1000.
857176
S(s) + O2(g)------>SO2\n\n2Mg(s) + O2(g) -------> 2MgO(s)\n\nH2(g) + Br2 (g) -------> 2HBr(g)\n\n4Fe(s) + 3O2 -------> 2Fe2O3 (s)\n\nThen there are single replacement \n\nA + BC-------> AC + B\nZn(s) + 2HCl(aq)------->ZnCl2 (aq) + H2 (g)\nwhere one element replaces another\n\nthen there is double replacement \n\nAB+CD -------> AD + BC\n\nIn this one the positive ions in the reacting compounds switch places\n\nBaCl2 (aq) + Na2So4 (aq) --------.BaSo4 (s) + 2NaCl (aq)
893153
2Fe (s) + 3F2 (g) ---> 2FeF3(s)
1123465
Na2S + 2 HCl > H2S + 2 NaCl  \n\nH2SO4 + BaOH > H20 + BaSO4  \n\nNH4Cl + NaOH > NaCl + NH4OH\n\nAgNO3 + NaCl > AgCl + NaNO3\n\nnot sure about complete or reversible..:)
867786
Let's take potassium representing group 1.  All the others will do the same thing.  Here is the reaction:\n\n2K(s) + 2HCl(aq) --> 2KCl(aq) + H2(g)\n\nThe reaction for group 2 will be similar.  Let's take calcium  representing group 2:\n\nCa(s) + 2HCl(aq) → CaCl2(aq) + H2(g)\n\nHope this helps.
55133
S8 + 4 Cl2  ---> S2Cl2\nHence here 1 atom of S reacts with 1 atom of CL\n\n21.51 gm S8 contains 0.67 moles of S atoms and .67/8 moles of S8\n\n82.98 g Cl2 has 1.16 moles of Cl2\n\nHence since 2 atoms of S make 1 S2Cl2 atoms, we get\n\n0.67 / 2 \n= .335 moles of S2Cl2\nmass= 135 x .335\nmass= 45.225 gms of S2Cl2
901730
Na2S (ag) + 2 AgNO3 (ag) --> 2 NaNO3 (ag) + Ag2S (cr)\n\nB. Double displacement.\n\nA. Ba(NO 3)2 and H2O\n\nB. If there is a double arrow (pointing in both directions), then it is an equilibrium reaction.\n\nC. Ba(OH)2 and HNO3\n\nD. Barium\n\nE. 6 oxygen atoms. \n\nF. Ba(OH)2
866145
HCl + AgNO3-----> AgCl +HNO3\nPb(OOC-CH3)2  + 2LiCl -------> PbCl2  + 2Li(OOC-CH3)\nNa3PO4 + CrCl3 -------> Cr(PO4) + 3NaCl\nH2SO4 + BaCl2 ----------> BaSO4 + 2HCl\nAl2(SO4)3  + 6NH4OH ------> 2Al(OH)3  + 3(NH4)2SO4\n2AgNO3 + H2S -------> Ag2S  + 2HNO3\nCaCl2   + Pb(NO3)2 -------> Ca(NO3)2  + PbCl2\nCa(NO3)2 + Na2CO3 ------>CaCO3  + 2 NaNO3
47432
3AgC2H3O2 + Na3PO4 -----> Ag3PO4 + 3NaC2H3O2
1116694
the reaction leads to production of hydrogen gas ...\n\n\n2Al(s) + 6HCl(aq) → 2Al3+(aq) + 6Cl-(aq) + 3H2(g)
1167833
sounds like an AP question.  So you are trying to calculate Ksp for silver acetate. \n\nAgC2H3O2 <--> Ag+  + C2H3O2-\n\nSolubility will be darn low so from there set up your ice chart and go to town.
12053
SO3+2 clearly is an error. It would demand a +8 charge of the sulfur atom (or a stable positive sulfur ion with an isolated peroxide ligand), which is impossible.\n\nA superscript "2-" would indicate a sulfite ion, whereas SO3 is sulfur trioxide, a neutral molecule forming a gas at room temperature.