Asked Jan 14, 2020

Balance the following red ox reaction if it occurs in acidic solution. MnO4^-(aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g)MnO4−(aq)+H2C2O4(aq)→Mn2+(aq)+CO2(g)


Expert Answer

Step 1

Steps in balancing redox reactions:

 1) Divide the overall reaction into an oxidation half-reaction and a reduction half-reaction

2) Balance atoms other thanand.

3)  Balance  by adding  as needed

4) Balance  by adding  ion at the required side.

5) Balance charges by adding, as needed number of electrons,

6) Multiply the oxidation half-reaction with the coefficient of electrons in the reduction part.

7) Multiply the reduction half-reaction with the coefficient of electrons in the oxidation part.

8) Combine the two half-reactions, cancel out the species that appears on both side, so that number of elements that appear on both sides become equal.

9) For the reaction in acidic medium, the presence of  ion allowed.

11) Cancel out the species that appears on both sides and ensure that the number of atoms on the reactant side is equal to the number of atoms on the product side.

Step 2

The given redox reaction is balanced as follows,

Chemistry homework question answer, step 2, image 1
Step 3
Chemistry homework question answer, step 3, image 1

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