Balance_ the following equation in acidic medium Mno4 + c2o42- co2+mn2+
Answers
Explanation:
The unbalanced redox reaction is MnO4^− +C2O4^2− +H^+→Mn^2+ +CO2+H2O
Balance C atoms.
MnO4^− +C2O4^2− +H^+→Mn^2+ +2CO2+H2O
The oxidation number of Mn decreases from +7 to +2.
The decrease in the oxidation number is 7−2=5
The oxidation number of C increases from +3 to +4.
The increase in the oxidation number for 1 C atom
is 4−3=1
The increase in the oxidation number for 2 C atom is 2×1=2
To balance the increase in the oxidation number with decrease in the oxidation number, multiply Mn containing species with 2 and C containing species
with 5.
2MnO4^− +5C2O4^2−→2Mn^2+ +10CO2
Balance O atoms by adding 8 water molecules to the products side.
2MnO4^− +5C2O4^2−→2Mn^2+ +10CO2+
8H2O
Balance H atoms by adding 16 H+ ions to the reactants side.
2MnO4^−+5C2O4^2− +16H^+→2Mn^2++10CO2+8H2O
This is the balanced equation.
Hope it was helpful!