Question

# Permanganate solution reacts with the oxalate ion in acidic medium and forms manganese(II) ion and carbon dioxide. What is the stoichiometric coefficient in front of manganese(II) in the balanced redox equation? MnO−4+C2O2−4→Mn2++CO2

A
2
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B
1
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C
3
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D
5
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Solution

## The correct option is A 2The redox reaction is : MnO−4+C2O2−4→Mn2++CO2 +7MnO−4++3C2O2−4→+2Mn2+++4CO2 MnO−4 is oxidising agent C2O2−4 is reducing agent. nf=(|O.S.Product−O.S.Reactant|)×number of atom +3C2O2−4→+4CO2---oxidation nf=(|4−3|×2)=2 +7MnO−4→+2Mn2+----reduction nf=(|2−7|×1)=5 Balance atom undergoing oxidation and reduction. MnO−4+C2O2−4→Mn2++2CO2 Cross mutiply the oxidising or reducing agent with simplified n-factor values. 2MnO−4+5C2O2−4→2Mn2++10CO2 Balance atoms oxygen. 2MnO−4+5C2O2−4→2Mn2++10CO2+8H2O balance hydrogen atom 2MnO−4+5C2O2−4+16H+→2Mn2++10CO2+8H2O Balance charge charge in reactant side = +4 charge in product side = +4 so the balanced equation is 2MnO−4+5C2O2−4+16H+→2Mn2++10CO2+8H2O the coefficient of Mn is 2.

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