Balance the following redox reactions by ion electron method
`MnO_4^-(aq) + SO_2 (g) to Mn^(2+) (aq) + HSO_4^-` (aq) (acid medium)

Balance the following redox reaction by ion electron method MnO_4^- (aq) + I^- (aq) to MnO_2 (s) + I_2(s) (base medium)

Balance the following redox reaction by ion electron method H_2O_2 (aq) + Fe^(2+) (aq) toFe^(3+)(aq) + H_2O (l) (acid medium)

Balance the following Redox reaction by ion-electron method or oxidation number method (Acid medium). Cr_2O_(7(aq))^(2-) + SO_(2) .............> Cr^(3+) SO_(4(aq))^(2-)

Balance the following equation by the half reaction method. Fe^(2+) (aq) + Cr_2O_7^(2-) (aq) +H^(+) (aq) rarr Fe^(3+) (aq) + Cr^(3+) (aq) +H_2O (I)

Balance the following equation using oxidation number method: MnO_2 +Cl^(-) rarr Mn^(2+)+Cl_2

Balance the following Redox process by ion-electron method or oxidation number method: P_(4(s)) + OH_(aq)^(- )rarr PH_(3(g)) + HPO_(2(aq))^-

Chimical reactions which involve oxidation and reduction are called redox reactions. The unbalanced equation in the ionic form of a redox reaction is shown below Fe^(2+) (aq) +Cr_2O_7^(2-) (aq) overset(acidic medium) (rarr)Fe^(3+) (aq) +Cr^(3+) (aq) a) Identify the oxidizing agent in this reaction