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## Homework Statement

Balance the equation for disproportionation reactions.

## Homework Equations

S

_{8}(s) ----> S

^{2-}+S

_{2}O

_{3}

^{2-}(basic solution)

## The Attempt at a Solution

I attempted in to do this with the ion electron method, obtaining an answer:

3S

_{8}+ 24OH

^{-}----> 16S

^{2-}+ 4S

_{2}O

_{3}

^{2-}+ 12H

_{2}O

However, I didn't follow the conventions that I was given, like using systematic steps to come to an answer... I was basically just guessing and checking, but I would like to know how to do it systematically.

Apparently though, I'm supposed to be doing my redox equations with the half reaction method instead.. which rather confuses me. When I attempted to do the half reaction...

reduction: S

_{8}+ 16e

^{-}----> 8S

^{2-}

oxidation: 2S

_{8}+ 24OH

^{-}(???) ----> 4S

_{2}O

_{3}

^{2-}+ 8e

^{-}+ 12H

_{2}O

The oxidation portion of the half reaction just doesn't seem to add up when I'm trying it.

I'd like to know if there is a systematic method to figuring out these sorts of equations so in the future I can have some sort of guideline in solving them. Help would be greatly appreciated :)!