how can h2s be breakdown?
480571
H2S in solution is a weak acid and so will react to produce Water plus a sulphide salt with any strong base.
497024
H2S---> 2 H^+ + S^2-\nK(eq) = \n[2H^+]^2 [S^2-]\n ---------------\n     [H2S]\n\nNH4+----> NH3  + H^+\nK(eq) =\n [H^+][NH3]\n       ------------\n         [NH4+]\n\nC6H5COOH----> C6H5COO-  + H+\n\nK(eq) = \n[H^+][C6H5COO-]\n        ---------------\n         [C6H5COOH]
374732
i think it may be that SO2 will react with water to give sulphurous acid (H2SO3).  This is the common acid found in acid rain.  The concentrated ammonia may be to neutralise the acid should it be formed from the SO2 leak.\n\nPossibly anyway....
756485
The water isn't involved in the reaction, so take it out.  Then, just put a 2 in front of the Nh2(SO3)H and a 2 in front of HNO3, and you're finished.\n\nNow, go take a nap or go to sleep...
80011
hydrolysis. the splitting of the water molecule. or just seperate the densities of the different components of air, then isolate the one that's the density of hydrogen and viola, you have pure hydrogen.
975090
Thiosulfate \n\nThiosulfate is the anion S2O32-. Thiosulfates are only stable in neutral or alkaline solutions, but not in acidic solutions, due to decomposition to sulfite and sulfur, the sulfite being reduced to sulfur dioxide:\n\nS2O32-(aq) + 2H+(aq) → SO2(g) + S(s) + H2O\n\nThis reaction is usually used to generate a temporary aqueous suspension to demonstrate diffraction of light in physics. If the light is shone from below, blue light is seen from above, and orange from sideways.\n\nUses of thiosulfates include the dissolving of silver salts from photographic film.
850750
The two hydrogen atoms' single electrons fill the outer shell of the oxygen atom... this makes water (mostly) chemically inert.  Since combustion is simply rapid oxidation... it could be argued that the hydrogen is already oxidized... making water...\n\nElectrolysis can seperate the hydrogen and oxygen... but this is not combustion.
738544
yes SO2 is liberated.The reaction is \nNa2SO3 + 2HCl -> 2NaCl + H2O + SO2\nformation of SO2 is favoured as water & sodium chloride are also formed with it , NaCl & H2O 's  formation is  thermodynamically favoured .
479909
Electrolysis is the process that would produce hydrogen gas from water by sends electric currents through water, breaking its bonds and thus separating the two hydrogen atoms from the oxygen.
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..:)
63677
na+2h2o=na(oh)2 + h2\n1.Note that na is a highly reactive metalk reacts even with cold water producing sodium hydroxide and liberating hydrogen.\n2h2so4+naoh = na(so4)2 +2h2o\nNote that h2so4 (sulphuric acid) reacts with naoh(sodium hydroxide),abase and the reaction b/w acid and base forming water and a salt is called neutralization reaction
145956
MY ANSWER IS :\n\n18.2g  of Na2S is produced.
991620
http://video.google.com/videoplay?docid=-2134266654801392897\n\nmentos and diet soda, baking soda and vinegar.\n\nthough i'm wondering how the hell you're supposed to drop elemental hydrogen in water.  if you make it a solid that would be new and it wouldn't do anything...
402204
H2SO4 - HCl - H3PO4 - HSO4(1-) - H2PO4(1-) - HPO4(2-)\n\nHCl is quite strong, but suffers the disadvantage at atmospheric pressure that it is volatile and will dissolve in water only up to 37%. It can be driven out of watery solutions by addition of less volatile but not necessarily stronger acids.\n\nH2CO3 would rank fairly high in this list too if you could prevent the CO2 from evaporating.\n\nWhen ranking H2SO4 and H3PO4 you'll have to state how far you want the protolysis to go. Taking the average of H2SO4 and HSO4(1-) makes it weaker than HCl, and worse so for H3PO4.
536199
follow the above.. to get gas.. electrolysis is the safest bet\n\nbut if you want to have fun???\n\nput some soap in the water and stir it around before you put the electrodes, this creates hydrogen bubbles that float and when put next to fire make a sweet pop sound.. do it safely, in a lab\n\nits a good demo for a highschool chem class
746377
The equation is S + O2 ===> SO2. That says that 1 g-atom of S reacts with 1 mol of O2 to give 1 mol SO2. The first step is to find the limiting reagent--the one that runs out first.\n\n20g S x (1 g-atomS/32g S)  = 0.675 g-atomS\n\n160g O2 x (1 molO2/32g O2) = 5 molO2\n\nSo the S runs out first; that is the limiting reagent.\n\nSo 0.675 g-atomS  x (1 mol SO2/1 g-atomS) x (64gSO2/1 molSO2) = 5/8 x 64 = 40g SO2
806865
Na2SO4 + H2O\n\nYou always get a type of salt plus water in acid-base neutralization.