Balance the following equations in acidic medium by both oxidation number and ion electron methods and identify the oxidants and the reductants:
Equations:
(i) MnO4 −(aq) + C2H2O4(aq) ⟶ Mn2+(aq) + CO2(g) + H2O(l)
(ii) H2S(aq) + Cl2(g) ⟶ S(s) + Cl−(aq)
(iii) MnO4 −(aq) + C2H5OH(aq) ⟶ Mn2+(aq) + CO2COOH(aq)
(iv) Bi(s) + NO3 −(aq) ⟶ Bi3+(aq) + NO2(g)
(v) Cr2O7 2−(aq) + C2H4O(aq) ⟶ Cr3+(aq) + C2H4O2(aq)
(vi) MnO4 −(aq) + Br−(aq) ⟶ Mn2+(aq) + Br2(aq)
(vii) Cu(aq) + NO3 −(aq) ⟶ Cu2+(aq) + NO2(g)
(viii) H2S(g) + Fe3+(aq) ⟶ Fe2+(aq) + S(s) + H+(aq)
(ix) I−(aq) + IO3 −(aq) + H+(aq) ⟶ I2(aq) + H2O(l)
(x) I−(aq) + O2(g) + H2O(l) ⟶ I2(aq) + OH−(aq)
(i) 2MnO4 −(aq) + 6H+(aq) + 5C2H2O4(aq) ⟶ 2Mn2+(aq) + 10CO2(g)+ 8H2O(l)
(ii) H2S(g) + Cl2(g) ⟶ S(s) + 2Cl−(aq) + 2H+(aq)
(iii) 4MnO4 −(aq) + 5C2H5OH(aq) + 12H+(aq) ⟶ 4Mn2+ + 5CH3COOH(aq) + 11H2O(l)
(iv) Bi(s) + 3NO3 −(aq) + 6H+(aq) ⟶ Bi3+(aq) + 3NO2(g) + 3H2O(l)
(v) Cr2O7 2−(aq) + 3C2H4O(aq) + 8H+(aq) ⟶ 2Cr3+(aq) + 3C2H4O2(aq) + 4H2O(l)
(vi) 2MnO4 −(aq) + 10Br−(aq) + 16H+(aq) ⟶ 2Mn2+(aq) + 5Br2(aq) + 8H2O(l)
(vii) Cu(s) + 2NO3 −(aq) + 4H+(aq) ⟶ Cu2+(aq) + 2NO2(g) + 2H2O(l)
(viii) H2S(g) + 2Fe3+(aq) ⟶ 2Fe2+(aq) + S(s) + 2H+(aq)
(ix) 5l−(aq) + IO3 −(aq) + 6H+(aq) ⟶ 3I2(aq) + 3H2O(l)
(x) 4l−(aq) + O2(g) + 2H2O(l) ⟶ 2I2(aq) + 4OH−(aq)
