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(C) The given unbalanced reaction is $Cr_2O_7^{2-} + Fe^{2+} + C_2O_4^{2-} 	o Cr^{3+} + Fe^{3+} + CO_2$.Step $1$: Oxidation half-reactions:$Fe^{2+} \

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$6$

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(C) The given unbalanced reaction is $Cr_2O_7^{2-} + Fe^{2+} + C_2O_4^{2-} 	o Cr^{3+} + Fe^{3+} + CO_2$.Step $1$: Oxidation half-reactions:$Fe^{2+} 	o Fe^{3+} + e^-$ $(i)$$C_2O_4^{2-} 	o 2CO_2 + 2e^-$ $(ii)$Adding $(i)$ and $(ii)$: $Fe^{2+} + C_2O_4^{2-} 	o Fe^{3+} + 2CO_2 + 3e^-$.Step $2$: Reduction half-reaction:$Cr_2O_7^{2-} + 14H^+ + 6e^- 	o 2Cr^{3+} + 7H_2O$ $(iii)$.Step $3$: To balance the electrons,multiply the oxidation half-reaction by $2$ and the reduction half-reaction by $1$:$2(Fe^{2+} + C_2O_4^{2-} 	o Fe^{3+} + 2CO_2 + 3e^-) \implies 2Fe^{2+} + 2C_2O_4^{2-} 	o 2Fe^{3+} + 4CO_2 + 6e^-$.Step $4$: Adding the balanced half-reactions:$Cr_2O_7^{2-} + 2Fe^{2+} + 2C_2O_4^{2-} + 14H^+ 	o 2Cr^{3+} + 2Fe^{3+} + 4CO_2 + 7H_2O$.The total number of electrons involved in the balanced redox reaction is $6$.

How many electrons are involved in the following redox reaction?
$Cr_2O_7^{2-} + Fe^{2+} + C_2O_4^{2-} \to Cr^{3+} + Fe^{3+} + CO_2$ (Unbalanced)

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How many electrons are involved in the following redox reaction?$Cr_2O_7^{2-} + Fe^{2+} + C_2O_4^{2-} \to Cr^{3+} + Fe^{3+} + CO_2$ (Unbalanced)