In dilute aqueous H_2SO_4,the complex diaquod | vedclass

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Question

(D) The balanced chemical equation for the reaction is:$5[Fe(C_2O_4)_2(H_2O)_2]^{2-} + 3MnO_4^- + 24H^{+} \longrightarrow 3Mn^{2+} + 5Fe^{3+} + 10CO_2

Vedclass · Accepted Answer

$8$

Vedclass · Answer

(D) The balanced chemical equation for the reaction is:$5[Fe(C_2O_4)_2(H_2O)_2]^{2-} + 3MnO_4^- + 24H^{+} \longrightarrow 3Mn^{2+} + 5Fe^{3+} + 10CO_2 + 22H_2O$From the stoichiometry of the reaction,the rate of change of concentration is related to the stoichiometric coefficients as:$-\frac{1}{24} \frac{d[H^{+}]}{dt} = -\frac{1}{3} \frac{d[MnO_4^-]}{dt}$Therefore,the ratio of the rate of change of $[H^{+}]$ to the rate of change of $[MnO_4^-]$ is:$\frac{d[H^{+}]}{dt} / \frac{d[MnO_4^-]}{dt} = \frac{24}{3} = 8$.

In dilute aqueous $H_2SO_4$,the complex diaquodioxalatoferrate$(II)$ is oxidized by $MnO_4^-$. For this reaction,the ratio of the rate of change of $[H^{+}]$ to the rate of change of $[MnO_4^-]$ is

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