Balance the ffg. redox equations by either the oxidation number method or the ion-electron method. Notice that in this reaction both chromium and iodine are being oxidized.

$CrI_3 + KOH + Cl_2→ K_2CrO_4 + KIO_4 + KCl + H_2O$

Please show step by step..
I want to do it using oxidation number method, but there are two reducing agents, which one should I use?

Question

Balance the ffg. redox equations by either the oxidation number method or the ion-electron method. Notice that in this reaction both chromium and iodine are being oxidized.

$CrI_3 + KOH + Cl_2→ K_2CrO_4 + KIO_4 + KCl + H_2O$

Please show step by step..
I want to do it using oxidation number method, but there are two reducing agents, which one should I use?

aaronq · Answer

Im pretty sure you can just group the oxidation reactions.

$\large \underbrace{Cr}_{+1}\underbrace{I_3}_{-1}\rightarrow \underbrace{Cr}_{+6}O_4^{2-}+5e^-+\underbrace{I}_{+7}O_4^-+8e^-+\underbrace{I_2}_{0}$

$\large CrI_3\rightarrow CrO_4^{2-}+IO_4^-+13e^-+I_2$