Answer:- Fe changes from 0 to +3 and O changes from 0 to -2.
Explanations:- As per the rules for oxidation numbers:-
(1) Oxidation number of an atom in its elemental form is zero. Both the reactants Fe and [tex]O_2[/tex] are in their elemental forms and so the oxidation numbers are zero.
(2) Oxidation umber of oxygen in it's compounds is -2. Let's say the oxidation number of Fe in the product is [tex]x[/tex] .
Also, the sum of oxidation numbers of all the atoms in a compounds is zero. So:
[tex]2x+3(-2)=0[/tex]
[tex]2x-6=0[/tex]
[tex]2x=6[/tex]
[tex]x=\frac{6}{2}[/tex]
[tex]x=3[/tex]
So, the oxidation number of Fe in [tex]Fe_2O_3[/tex] is +3 and the oxidation number of O is -2.
Hence, the oxidation number of Fe changing from 0 to +3 and O is changing from 0 to -2.
In terms of oxidation and reduction, Iron is oxidized and oxygen is reduced.
Answer:
b. Fe is oxidized from 0 to +3
a. O is reduced from 0 to -2
Explanation:
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