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For redox reaction,
${MnO}_{4}^{-} + C_{2} O_{4}^{2 -} + H^{+} ⟶ {Mn}^{2 +} + {CO}_{2} + H_{2} O$
the coefficient of reactants in balanced states are

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${MnO}_{4}^{-} \to 2; C_{2} O_{4}^{2 -} \to 5; H^{+} \to 16$

${MnO}_{4}^{-} \to 16; C_{2} O_{4}^{2 -} \to 5; H^{+} \to 2$

${MnO}_{4}^{-} \to 5; C_{2} O_{4}^{2 -} \to 16; H^{+} \to 2$

${MnO}_{4}^{-} \to 2; C_{2} O_{4}^{2 -} \to 16; H^{+} \to 5$

answer is A.

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Detailed Solution

For the balanced equation,

$2 {MnO}_{4}^{-} + 5 C_{2} O_{4}^{2 -} + 16 H^{+} ⟶ 2 {Mn}^{2 +} + 10 {CO}_{2} + 8 H_{2} O$

$Coefficients of {MnO}_{4}^{-} = 2$

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

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