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For the redox reaction MnO4−+C2O42−+H+→Mn2++CO2+H2O\text{MnO}_4^- + \text{C}_2\text{O}_4^{2-} + \text{H}^+ \rightarrow \text{Mn}^{2+} + \text{CO}_2 + \text{H}_2\text{O}. The correct coefficients of the reactants for the balanced equation are MnO4−\text{MnO}_4^-, C2O42−\text{C}_2\text{O}_4^{2-}, H+\text{H}^+ respectively:

1

2, 16, 5

2

2, 5, 16

3

16, 5, 2

4

5, 16, 2

Step-by-Step Solution

The n-factor of MnO4−\text{MnO}_4^- is 5 and the n-factor of C2O42−\text{C}_2\text{O}_4^{2-} is 2. The ratio of n-factors is 5:2, so the molar ratio in the balanced reaction is 2:5. The balanced equation is 2MnO4−+5C2O42−+16H+→2Mn2++10CO2+8H2O2\text{MnO}_4^- + 5\text{C}_2\text{O}_4^{2-} + 16\text{H}^+ \rightarrow 2\text{Mn}^{2+} + 10\text{CO}_2 + 8\text{H}_2\text{O}.

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