egl. MnO+C,O.2-→Mn2+ + CO, (Acidic solution)Mn0:+8H++5e→Mn2++4H0+) C,02- -→2 CO,+2e2 Mn0-+ 5C,0.2-+16H+-→2Mn2++10 CO, +8 H,0
eg1. MnO4 - + C2O4 2- → Mn2+ + CO2 (Acidic solution) MnO4 - + 8H+ + 5e → Mn2+ + 4 H2O +) C2O4 2- → 2 CO2+ 2e 2 MnO4 - + 5C2O4 2- +16 H+ → 2Mn2+ +10 CO2 +8 H2O
eg2. FeS,+HNO,→Fe,(SO),+NOFeS,+8H,O→Fe3++SO2-+16H++15e+) 2H++NO+e→NO, +H,OFeS, + 14 H++ 15 NO → Fe3+ +2 SO.2- + 15 NO, + 7H,O
eg2. FeS2 + HNO3 → Fe2 (SO4 ) 2 +NO2 FeS2 + 8 H2O → Fe3+ + SO4 2- + 16 H+ +15e +) 2 H+ + NO3 - + e → NO2 + H2O FeS2 + 14 H+ + 15 NO3 - → Fe3+ +2 SO4 2- + 15 NO2 + 7H2O
eg3. CIO- + CrO, →CI + CrO 2- (Basic solution)CI0- +H,0+2e→CI +2 0H+) Cr0z- + 40H- -3 e →2H,0+ Cr0 23CI0-+2Cr0,+20H→H0+3CI+Cr02
eg3. ClO- + CrO2 - → Cl- + CrO4 2- （Basic solution） ClO- + H2O + 2e → Cl- + 2 OH- +) CrO2 - + 4OH- -3 e → 2H2O+ CrO4 2- 3ClO- + 2CrO2 - + 2 OH- → H2O + 3 Cl- + CrO4 2-
1-3 Voltaic cells
1-3 Voltaic cells
1-3-1 What kinds of redox reactions can be harnessed toproduceelectricalenergy?In prnciple, the spontaneous redox reactions withenough reaction rate can be harnessed to produceelectrical energy by carrying them out in a voltaic cell.△G<0enough high reactionrate
1-3-1 What kinds of redox reactions can be harnessed to produce electrical energy? In prnciple, the spontaneous redox reactions with enough reaction rate can be harnessed to produce electrical energy by carrying them out in a voltaic cell. u G < 0 u enough high reaction rate