Question

Given the reaction Fe + O2 -> Fe2(3+)O3(2-), what happens to the oxidation states of these elements?

Answer 1

b. Fe is oxidized from 0 to +3

a. O is reduced from 0 to -2

Step-by-step explanation:

edge 2021

Answer 2

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
`O_2` 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
`x` .

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

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

`2x-6=0`

`2x=6`

`x=(6)/(2)`

`x=3`

So, the oxidation number of Fe in
`Fe_2O_3` 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.