For the redox reaction MnO_4^- + C_2O_4^{2-} | vedclass

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Question

(A) The half-reactions are:Reduction: $(MnO_4^- + 8H^{+} + 5e^- 	o Mn^{2+} + 4H_2O) 	imes 2$Oxidation: $(C_2O_4^{2-} 	o 2CO_2 + 2e^-) 	imes 5$Addi

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$2, 5, 16$

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(A) The half-reactions are:Reduction: $(MnO_4^- + 8H^{+} + 5e^- 	o Mn^{2+} + 4H_2O) 	imes 2$Oxidation: $(C_2O_4^{2-} 	o 2CO_2 + 2e^-) 	imes 5$Adding the two half-reactions to balance the electrons:$2MnO_4^- + 16H^{+} + 10e^- + 5C_2O_4^{2-} 	o 2Mn^{2+} + 8H_2O + 10CO_2 + 10e^-$The balanced equation is:$2MnO_4^- + 5C_2O_4^{2-} + 16H^{+} 	o 2Mn^{2+} + 10CO_2 + 8H_2O$Thus,the coefficients of $MnO_4^-$,$C_2O_4^{2-}$,and $H^{+}$ are $2, 5$,and $16$ respectively.

For the redox reaction $MnO_4^- + C_2O_4^{2-} + H^{+} \to Mn^{2+} + CO_2 + H_2O$,the correct coefficients of the reactants for the balanced reaction are:
$MnO_4^-$ : $C_2O_4^{2-}$ : $H^{+}$

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For the redox reaction $MnO_4^- + C_2O_4^{2-} + H^{+} \to Mn^{2+} + CO_2 + H_2O$,the correct coefficients of the reactants for the balanced reaction are:$MnO_4^-$ : $C_2O_4^{2-}$ : $H^{+}$