For the reaction SO2   +   O2   -->   SO3?
956489
2 SO2 + O2 --> 2 SO3\n\n\nok, 64.00 g oxygen times the molar mass of 02( 32.00) to get mols of O2 then time the mole ratio of O2 to SO2 which is (2 mol SO2/2 Mol O2) and then u have the mols of SO2 times that by the molar mass of SO2 to get the mass of SO2\n\n64.00 x 32.00 x 2/2 x molar mass of SO2
170129
CuSO4 (s)  --H2O-->  Cu+2 (aq) + SO4-2 (aq)
774704
S + O2 --> SO2\n\nmole of S needed to be converted = 5.00 / 32 = 0.15 mole\nmole of O2 = 0.15 mole\nBy using ideal gas theory:\nP * V = n * R * T\n5.15 * V = 0.15 * 0.082 * 310\nV = 0.74 litre\n\npeace\nvixklen
895751
Al2S3 + 6H2O -> 2Al(OH)3 + 3H2S\n\nP4O10 + 6H2O -> 4H3PO4\n\n\nShould be right.
36586
Ag+ + SO4(2-) ---> Ag2SO4\nYeah, it's double replacement, and according to my solubility rules, AgSO4 is insoluble.
870720
Theoretically this would yield H2SO4, sulphuric acid (c).\n\nIn praxis, SO3 doesn't dissolve well in water and is prone to dissociate into SO2 and 1/2 O2, which then may form sulphurous acid H2SO3 which in turn will re-oxidize to H2SO4.
751855
The first step is to balance the equation first, which yields\n\n2SO2 + O2 ---> 2SO3\n\nNow, find the total number of moles of 160 g O2:\n\n# of mole = 160/(16*2)\n= 5 moles.\n\nAccording to the balanced equation, the mole ratio between SO2 and O2 is 2:1. In other words, it takes twice amount (in moles) of SO2 to react with 1 unit of O2.\n\nSince we react 5 moles of O2, we need 10 moles of SO2.\n\nMass of SO2 = # mole * molecular weight\n= 10 * (32 + 16*2)\n= 640 g of SO2 is needed.
606075
Cu(s) + 4HNO3 (aq)--> Cu(NO3)2(aq) + 2H2O(l) +2NO2(g)
35280
The Ksp of the reaction\n\nHgS <--> Hg + S\n\nis 2*10^-53. Extremely insoluble.
589750
SO4 2-\nCO3 2-\nOH -\nPO4 3-
195778
1.  C(s)+O2--> CO2(g) - 393.5 kj\n2.  H2(g)+1/2 O2(g)--> H20 -285.8 kj\n3.  2C2H2(g)+5O(g)-->4CO2(g)+2H2O(... -2598.8\nCALCULATE the value for the reaction 2C+H2-->C2H2\n\nFirst balance eqn 3 with 5O2 (g) then reverse it so that you have 2C2H2(g) on the RHS. Of course, you will change the sign of the eqn as well. Now halve it so you have one C2H2 instead of 2. Let's call the new eqn number 4\n\nSecond, double the 1st eqn. Let's call it eqn 5\n\nLastly, add eqns 3, 4 and 5:\n\n4 2CO2(g)+H2O --> C2H2(g)+5O2(g) +1299.4 kJmol-1\n5 2C(s)+ 2O2--> 2CO2(g) -787.0 kJmol-1\n3 H2(g)+1/2 O2(g)--> H20 -285.8 kj\n----------------------------------------------\n  2C(s)+ H2(g) --> C2H2(g) + 226.6 kJmol-1
532416
It is CS2+3(O2)=CO2+2(SO2)
954811
C3H8 + 5O2 --> 3CO2 + 4H2O
422969
AgNO3(aq)+2Na2S2O3(aq)--> [Ag(S2O3)2]3-(aq) + 4Na+(aq)+ NO3-(aq)
412413
I'm assuming you're asking for the reactions.  Here are a couple:\nH2 + F2 → 2HF \n\n4Fe + 3O2 → 2 Fe2O3
329297
decomposition reaction\n\n2H2O2 -------- O2   +  2H20
610699
Pb(NO3)2(aq) + H2SO4(aq/l)[depending on concentration] --> PbSO4(s) + 2HNO3(aq)\nPb2+(aq) + SO42-(aq) --> PbSO4(s)\n\nI don't see how an redox reaction could occur.