For the redox reaction,
$M n O_{4}^{-} + C_{2} O_{4}^{2 -} + H^{+} \to M n^{2 +} + C O_{2} + H_{2} O$
the correct coefficients of the reactants for the balanced reaction are

M n O_{4}^{-} = 2, C_{2} O_{4}^{2 -} = 5, H^{+} = 16

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M n O_{4}^{-} = 16, C_{2} O_{4}^{2 -} = 5, H^{+} = 2

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M n O_{4}^{-} = 5, C_{2} O_{4}^{2 -} = 16, H^{+} = 2

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M n O_{4}^{-} = 2, C_{2} O_{4}^{2 -} = 16, H^{+} = 5

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Solution

The correct option is A $M n O_{4}^{-} = 2, C_{2} O_{4}^{2 -} = 5, H^{+} = 16$
Balanced equation for the given unbalanced equation is

$2 M n O_{4}^{-} + 5 C_{2} O_{4}^{2 -} + 16 H^{+} \to 2 M n^{2 +} + 10 C O_{2} + 8 H_{2} O$ .
So the correct coefficients of the reactants for the balanced reaction are

$M n O_{4}^{-} = 2, C_{2} O_{4}^{2 -} = 5, H^{+} = 16$ .
Hence option A is correct.

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Similar questions

M n O_{4}^{-} + C_{2} O_{4}^{2 -} + H^{+} \to M n^{2} + C O_{2} + H_{2} O

M n O_{4}^{⊖} + C_{2} O_{4}^{2 -} + H^{\oplus} \to M n^{+ 2} + C O_{2} + H_{2} O

M n O_{4}^{-} + C_{2} O_{4}^{2 -} + H^{+} \to M n^{2 +} + C O_{2} + H_{2} O

M n O_{4}^{-}, C_{2} O_{4}^{2 -}, H^{+}

For the redox reaction

$M n o_{4}^{⊝} + C_{2} O_{4}^{2 -} + H^{\oplus} \to M n^{+ 2} + C O_{2} + H_{2} O$

The correct coefficients of the reactants for the balanced reaction are

For the redox reaction

MnO₄^- + C₂O₄^2- + H⁺ → Mn²⁺ + CO₂ + H₂O

The correct coefficients of the reactants for the balanced reaction are:

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