The value of `x` in the partial redox equation
`MnO_(4)^(-)+8H^(+)+xe hArr Mn^(2+)+4H_(2)O` is

The value of n in : MnO_(4)^(-)+8H^(+)+n erarr Mn^(2+)+4H_(2)O is

The value of n in : MnO_(4)^(-)+8H^(+)+n erarr Mn^(2+)+4H_(2)O is

Redox reactions are of three types: (i) Intermolernlar redox reactions. (ii) lntramolecular redox reactions, (iii) Auto redox reactions OR Disproportionation reactions. Redox reactions are divided into two main types: (i) Chemical redox reactions, (ii) Electrochemical redox reactions which either produce or consume electricity Oxidation and reduction process takes place in a reaction simultaneously. The value of x in the following reaction, MnO_(4)+8H^(+)+xe to Mn^(2+)+4H_(2)O is

The value of n in the following half equation is MnO4^(-) + 2H_2O + ne rarr MnO_2 + 4O'H

MnO_(4)^(-)+8H^(+)+n e^(-)rarrMn^(2+)+4H_(2)O The value of n is

Balance the equation MnO_4^- +H^+ +Fe^2 rarr Mn^2 + H_2O + Fe^3^+