Answer:
+5 in KClO3 to -1 in KCl
Explanation:
The balanced equation is:
[tex]2KClO3(s)\rightarrow 2KCl(s) + 3O2(g)[/tex]
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.
The oxidation state of chlorine in the given reaction changes from +5 to -1.
Option (d) is correct.
Oxidation state or oxidation number is the total number of electrons either an atom gains or loses.
Given,
[tex]\bold{2KClO_3(s) = 2KCl(s) + 3O_2 (g)}[/tex]
Now, In [tex]\bold{KClO_3}[/tex] -1 is the charge
The oxidation state of K = +1
Oxidation state of O = -2
Let the oxidation state of Cl is x
Thus,
+1 + x + 3(-2) = 0
x = +5
Similarly, In KCl
The oxidation state of K is +1
Let oxidation state of Cl is x
+1 + x = 0
x = -1
Thus, The correct option is (d) the oxidation state of Cl changes from +5 to -1.
Learn more about oxidation numbers, here:
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