In the reaction of oxalate with permanganate | vedclass

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(A) The balanced chemical equation for the reaction is: $5C_2O_4^{2-} + 2MnO_4^- + 16H^{+} 	o 10CO_2 + 2Mn^{2+} + 8H_2O$ In this reaction,the oxalate

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$1$

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(A) The balanced chemical equation for the reaction is: $5C_2O_4^{2-} + 2MnO_4^- + 16H^{+} 	o 10CO_2 + 2Mn^{2+} + 8H_2O$ In this reaction,the oxalate ion $(C_2O_4^{2-})$ is oxidized to $CO_2$. The half-reaction for the oxidation is: $C_2O_4^{2-} 	o 2CO_2 + 2e^-$ This shows that $2$ electrons are released when $2$ molecules of $CO_2$ are produced. Therefore,for the production of one molecule of $CO_2$,the number of electrons involved is $2/2 = 1$.

In the reaction of oxalate with permanganate in acidic medium,the number of electrons involved in producing one molecule of $CO_2$ is

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