Acidified potassium permanganate solution oxi | vedclass

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Question

(D) The balanced chemical equation for the reaction is: $2 \ KMnO_4 + 5 \ H_2C_2O_4 + 3 \ H_2SO_4 \rightarrow K_2SO_4 + 2 \ MnSO_4 + 10 \ CO_2 + 8 \ H

Vedclass · Accepted Answer

$6$

Vedclass · Answer

(D) The balanced chemical equation for the reaction is: $2 \ KMnO_4 + 5 \ H_2C_2O_4 + 3 \ H_2SO_4 \rightarrow K_2SO_4 + 2 \ MnSO_4 + 10 \ CO_2 + 8 \ H_2O$. In this reaction,the manganese product is $MnSO_4$,where manganese exists as the $Mn^{2+}$ ion. The electronic configuration of $Mn^{2+}$ is $[Ar] \ 3d^5$. It contains $5$ unpaired electrons. The spin-only magnetic moment is calculated using the formula $\mu = \sqrt{n(n+2)} \, B.M.$,where $n$ is the number of unpaired electrons. $\mu = \sqrt{5(5+2)} = \sqrt{35} \approx 5.92 \, B.M.$ Rounding to the nearest integer,we get $6 \, B.M.$

Acidified potassium permanganate solution oxidises oxalic acid. The spin-only magnetic moment of the manganese product formed from the above reaction is $.... \, B.M.$ (Nearest Integer)

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