Please tell me the oxidation numbers for H2O2 [hydrogen peroxide]?
963191
Oxygen in peroxides\n\nPeroxides include hydrogen peroxide, H2O2. This is an electrically neutral compound and so the sum of the oxidation states of the hydrogen and oxygen must be zero.\n\nSince each hydrogen has an oxidation state of +1, each oxygen must have an oxidation state of -1 to balance it
754704
You should write NH4(+) otherwise you will not get the oxidation number right.  H is 1 so H4 is 4.\n\nIn order to be left with 1(+) you need 4 - 3 = 1.  So N will be -3.\n\nCheck -3 + 4*1 = +1 OK.
932271
yields "H2 + Zn2O3"\n\n^^!
306342
in H3P04 u need the oxidation number of what? all these elements have different oxidation numbers in different compounds. the procedure for u to find out the oxidation number is .... if u want the oxidation number of P then write there as x, for H as u know it is +1, for O it is -2.\n then, (+1*3)+(x*1)+(-2*4)=0; 3+x-8=0; x=5 thus, the oxidation number of P in H3P04 is 5.\nin the same way, in H2O2; O is -1\nSi(OH)4 ; Si is x+(4*-2)+4=0; x=4\nin KH2PO4, P is  +1+(+1*2)+x+(-2*4)=0; x=5\nin Fe(HCO3)2 if Fe is +2, H is +1, O is -2 then C is \n+2+2+2x-12=0; x=4\nCu2CrO4, Cu is +2, O is -2 and Cr is 4+x-8=0; x=4\nKMnO4, K is +2, O is -2 and Mn is +2+x-8=0 x=6\nN03, Ois -2, x+(-2*3)=0, x=6\nin HN03, H is +1, O is -2,then N is +1+x-6=0, x=5\nBeH2, H is +2\n\nany doubts u can ask again.
222097
OH-(aq) + HC2H3O2(aq)---> H2O(l) + C2H3O2-(aq)
180166
In this compound lead oxidation number is 2+
603812
The H's are +1, and the O's are -2, and the whole thing is 0, so...\n4(+1) + 2x + 7(-2) = 0\nx=5, so the oxidation number of phosphorus is +5.
715790
H2O2    =  2H+ + 2e + O2\n\nMnO4- + 5e + 8H+ = Mn2+ + 4H2O \n\nso you need 5 moles of H2O2 and 2 moles of MnO4- to get electon balance for the overall reaction which is\n\n5H2O2 + 2MnO4- + 6H+  = 5O2 + 2Mn2+ + 8H2O\n\nremember that you can cancel out most of the H+ which appears on both sides of the equation leaving just the 6H+ as shown above.
714001
1. NO2-\n\n2. tellurite\n\n3. pernitrate\n\n4.NH4NO3\n\n5. OH-
231663
_KCl3 _KCL + _o2? K2Cl4o2 thats the answer i think.:)
775000
2 MnO4-(aq ) + 5 H2C2O4(aq ) + 6 H3O+(aq ) --> 2Mn2+(aq ) + 10 CO2(aq ) + 14 H2O
697397
NaOH\nSn(NO3)2\nCo2O3\nFeF2\nCuS2\nFe(OH)3\nAgBr
1093422
([O2]^(O2 coefficient)*[H2]^(H2 coefficient))/\n[H2O2]^(H2O2 coefficient)
813894
There is an easy one using enzyme catalysis.  Use hydrogen peroxide solution from the local pharmacy or grocery store.  Put some in a test tube and drop a fresh slice of potato in it.\n\nThe potato has catalase enzyme in it.  This enzyme catalyses the decomposition of hydrogen peroxide to water and oxygen as such:\n\n2 H2O2  >(Catalase)> 2 H2O + O2\n\nThe activity of the enzyme catalyst can be observed by the bubbles of oxygen gas that form during the reaction.
470703
reduced: 2H2O + 2e- ---> H2 + 2OH-\n\noxidized: 2I- ---> I2 +2e-
694808
The sum of the oxidation numbers in a compound sum up to the compound's charge. The oxidation number of H is usually +1 and the oxidation number of O is usually -2. Since the charge of H2SO3 is zero, and calling the oxidation number of S b, you get\n\n2*1 + b + 3*-2 = 0.\n\nSolving for b, you get b =+4.
96357
First figure out the chemical reaction,\n\nHydrogen PerOxide deomposes into water and Oxygen gas,\n2H2O2 --> 2H2O + O2\n\nYou now know that there is a 1:1 ratio for each mole of Hdrogen peroxide decomposing to form water.\nFor first figure out how many moles of water .7 grams if from the molar mass of water (18.02 g/mol) and then you know how many moles of H2O2.  The after you know the moles of H2O2 needed, convert to grams using the molar mass of Hydrogen PerOxide (34.02 g/mol).