In dilute aqueous H 2 S O 4 , the complex diaquodioxalatoferrate(II) is oxidized by M n O 4 - For this reaction, the ratio of the rate of change of H + to the rate of change of M n O 4 - is

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The balanced chemical equation for the oxidation of the complex is as given below

$Mn O_{4}^{-} + 5 [Fe (H_{2} O) {(C_{2} O_{4})_{2}]}^{2 -} + 8 H^{+} \to 5 {[Fe (H_{2} O) {(C_{2} O_{4})}_{2}]}^{-} + M n^{2 +} + 4 H_{2} O$

Hence $- \frac{d}{d t} [M n O_{4}^{-}] = - \frac{1}{8} \frac{d}{d t} [H^{+}]$

$\frac{\frac{d}{d t} [H^{+}]}{\frac{d}{d t} [M n O_{4}^{-}]} = 8$

Rate of change of $[H^{+}]$ is 8 times the rate of change of $[M n O_{4}^{-}]$ .

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