How many moles of KMnO_4 are required to oxid | vedclass

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(A) The balanced redox reaction is: $5Fe^{2+} + 5C_2O_4^{2-} + 3MnO_4^- + 24H^+ \rightarrow 5Fe^{3+} + 10CO_2 + 3Mn^{2+} + 12H_2O$. From the balanced

Vedclass · Accepted Answer

$0.6$

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(A) The balanced redox reaction is: $5Fe^{2+} + 5C_2O_4^{2-} + 3MnO_4^- + 24H^+ \rightarrow 5Fe^{3+} + 10CO_2 + 3Mn^{2+} + 12H_2O$. From the balanced equation,$5 \ mol$ of $FeC_2O_4$ reacts with $3 \ mol$ of $KMnO_4$. Therefore,$1 \ mol$ of $FeC_2O_4$ will react with $\frac{3}{5} \ mol$ of $KMnO_4$. $\frac{3}{5} = 0.6 \ mol$.

How many moles of $KMnO_4$ are required to oxidize $1 \ mol$ of $FeC_2O_4$ in an acidic medium?

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