Label the redox components of each reaction. Indicatethe number of electrons mov
ID: 75506 • Letter: L
Question
Label the redox components of each reaction. Indicatethe number of electrons moving for each half reaction. Include alloxidation states. 0 0 +20 -20 P4 + 5O2 --> P4O10 P = 0 to+20 = Oxidation (20e- moving) O= 0 to -20 = Reduction (20e-moving) +4 -4 +2 +8 -8 +2 +4 -4 +2 -2 2MnO4-1 + 16H+1 + 5C2O4-2 --> 2Mn+2 + 10CO2 + 8H2O Mn = NoChange O = 0 to (-4) = reduction = (4e-moving) C = NoChange H = 0 to +2 = oxidation = (2e-moving) +3 -3 +4-4 +4 -2 -2 +2 -2 PbS + 4H2O2 --> PbSO4 + 4H2O H = Nochange Pb = +3 to +4 = oxidation = ( 1e- moving) C = NoCharge S = -3 to -4 = reduction = (1 e-moving) +4-4 +1-2 +1 +3 -4 +1 +5 -6 2NO2 + H2O --> HNO2 + HNO3 H = No change O = 0 to -6 = reduction = (2e-moving) N = 0 to +5 = oxidation = (1 e-moving) Are these correct if not what needs to be done to make themcorrect? Label the redox components of each reaction. Indicatethe number of electrons moving for each half reaction. Include alloxidation states. 0 0 +20 -20 P4 + 5O2 --> P4O10 P = 0 to+20 = Oxidation (20e- moving) O= 0 to -20 = Reduction (20e-moving) +4 -4 +2 +8 -8 +2 +4 -4 +2 -2 2MnO4-1 + 16H+1 + 5C2O4-2 --> 2Mn+2 + 10CO2 + 8H2O Mn = NoChange O = 0 to (-4) = reduction = (4e-moving) C = NoChange H = 0 to +2 = oxidation = (2e-moving) +3 -3 +4-4 +4 -2 -2 +2 -2 PbS + 4H2O2 --> PbSO4 + 4H2O H = Nochange Pb = +3 to +4 = oxidation = ( 1e- moving) C = NoCharge S = -3 to -4 = reduction = (1 e-moving) +4-4 +1-2 +1 +3 -4 +1 +5 -6 2NO2 + H2O --> HNO2 + HNO3 H = No change O = 0 to -6 = reduction = (2e-moving) N = 0 to +5 = oxidation = (1 e-moving) H = No change O = 0 to -6 = reduction = (2e-moving) N = 0 to +5 = oxidation = (1 e-moving) Are these correct if not what needs to be done to make themcorrect?Explanation / Answer
1)The first reaction is correct 2) Oxygen has a -2 charge not -1 so in MnO4- Oxygen is -2which gives a total of -8. Since the compound has a -1 charge, Mnis +7 not +4. H+ is a +1 charge, it looks like you have a +2charge listed. The C2O4 molecule is not correct, the total moleculehas a -2 charge. Therefore the C2 will be +6 not +8. Thewater is not correct as well. It should be +2 and -2 not +4 and-4. 3) For the third reaction Sulfur has a -2 charge not -3,therefore lead has a +2 charge, not +3. H2O2 is a specialcompound wilh oxygen having only a -1 charge, this is an exceptionto the rule. Hyrdogen will always have a +1 charge though. So iH2)2 it should be +2/-2. In PbSO4 the compound is neutral thereorethe oxygen is a total of -8. Sulfur is is +6 and Pb is +2 4) In the last reaction is totally correct, but see myexplanation below regarding the redox component Just keep in mind that oxygen is always -2 unlss in a peroxidemolecule, H2O2. H+ is always +1. The sum of all charges in thecompound has to equal the total charge of the molecule. Make sureyou stay consistent Make sure you understand that for example O4 has a -8charge total, but this is because oxygen has a -2 charge per ion.Therefore keep in mind that reduction and oxidation reactions referto individual elements and not the whole compound. For example: H2O2 to H2O, the reduction is O- to O2-, so itgains 1e-. It is not -2 to -2 as you have listed in th lastreaction. Redox is for individual elements such as Mn, Pb, O notwhole compounds such as O2, PbS, etc For example: H2O2 to H2O, the reduction is O- to O2-, so itgains 1e-. It is not -2 to -2 as you have listed in th lastreaction. Redox is for individual elements such as Mn, Pb, O notwhole compounds such as O2, PbS, etc Good LuckRelated Questions
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