Given the reaction fe + o2 -> fe2(3+)o3( what happens to the oxidation states of these elements?

- 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 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 .

Also, the sum of oxidation numbers of all the atoms in a compounds is zero. So:

So, the oxidation number of Fe in 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.

b. Fe is oxidized from 0 to +3

a. O is reduced from 0 to -2

Explanation:

edge 2021

dynamic equilibrium is the answer.

58750.08068 is the answer i think