For the following reaction
KClO4 → KCl + 2O2
Assign oxidation states to each element on each side of the equation.
Reactant Product
K
Cl
O
Which element is oxidized?
Which element is reduced?
1 answer
The element that is oxidized is the potassium (K), which has an oxidation state of +1 on the reactant side and +2 on the product side. The element that is reduced is the chlorine (Cl), which has an oxidation state of -1 on the reactant side and 0 on the product side. The oxygen (O) has an oxidation state of -2 on both sides of the equation.
1 answer