KClO3 - - - >KCl+3/2O2 assign oxidation states to each element on each side of the equation. (reactants and produc? KClO3 - - - >KCl+3/2O2 which element is oxidized?

Question

Chemistry

Nikhil Beltran

14 December, 17:55

KClO3 - - - >KCl+3/2O2 assign oxidation states to each element on each side of the equation. (reactants and produc? KClO3 - - - >KCl+3/2O2 which element is oxidized?

+1

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Dayana Shah · Answer 1

K will always have an oxidation state of + 1. Now O is - 2 except in peroxides, this is not a peroxide, so total charge will be - 6, if you subtract the + 1 of K from it, it leaves - 5 charge to be neutralized by Cl in KClO3, so Cl will be + 5. In the product side, K will still have the same oxdiation which is + 1 and Cl would have - 1. O2 will have zero. Now, Cl is gaining the electrons to go from + 5 to - 1, so it is getting reduced while O2 is losing electrons to go from - 2 to zero so it is getting oxidized.