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# Balancing equations watch

1. KClO3 + H2SO4 ---> ClO2 + K2SO4 + KClO + H2O
Can someone tell me how to balance this equation? I got oxidation number for K in KClO3 equals +7 and the K in KClO equals +3. So there is a reduction of -5. Other than that i'm lost
2. It is +5 in KClO3 to +4 in ClO2 and +1 in KClO, which is reduction in both cases - where's the oxidation?
3. (Original post by Pigster)
It is +5 in KClO3 to +4 in ClO2 and +1 in KClO, which is reduction in both cases - where's the oxidation?
Why is it +5 in KClO3?
4. K is +1
Each O is -2 (-6 total)
You need Cl at +5 to make it add up to zero.
5. (Original post by Pigster)
K is +1
Each O is -2 (-6 total)
You need Cl at +5 to make it add up to zero.
I couldn't find the oxidation.
6. (Original post by Snowie9)
I couldn't find the oxidation.
My point exactly. You need one! Have you looked down the back of the settee?

Also, the only reason I can think of that an oxidising agent (KClO3 in this case) would produce two different reduced products (ClO2 and KClO in this case) is if the reducing agent (not present in this case) were to run out half way through the reaction.

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Updated: October 17, 2017
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