Question

Given the balanced equation representing a reaction:2KClO3(s) → 2KCl(s) + 3O2(

Answer 1

Answer:

+5 in KClO3 to -1 in KCl

Explanation:

The balanced equation is:

$2KClO3(s)\rightarrow 2KCl(s) + 3O2(g)$

In KClO3:

The oxidation state of K = +1

Oxidation state of O = -2

Let the oxidation state of Cl = 'x'

Since the molecule is neutral, the net charge is zero. Therefore,

+1 + x + 3(-2) = 0

x = +5

In KCl:

The oxidation state of K = +1

Let the oxidation state of Cl = 'x'

Since the molecule is neutral, the net charge is zero. Therefore,

+1 + x = 0

x = -1

Therefore, the oxidation state of Cl changes from +5 to -1.

Answer 2

Oxidation state is the charge of the ion when we write the complete ionization reaction for the given above. For chlorine, in the reactant side, the oxidation state is 5. Also, its oxidation state in the product side is -1. The answer is 5 to -1, The answer is therefore, +5 to -1.