How do we represent the formation of $F e_{3} O_{4}$ $Fe_3O_4$ by the oxidation of iron metal in basic conditions?

Question

How do we represent the formation of $F e_{3} O_{4}$ $Fe_3O_4$ by the oxidation of iron metal in basic conditions?

1 Answer

Impact of this question

1502 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2017-07-11T15:33:17

$3 F e (s) + 8 H_{2} O \to F e^{2 +} + 2 F e^{3 +} + 4 H_{2} (g) + 8 H O^{-}$ $3Fe(s) +8H_2Orarr Fe^(2+) + 2Fe^(3+)+4H_2(g) +8HO^-$

Explanation:

If you got $F e_{3} O_{4}$ $Fe_3O_4$ , this is mixed valence oxide of iron ......it occurs as the mineral magnetite, which we could formulate as $F e O \cdot F e_{2} O_{3} \equiv F e_{3} O_{4}$ $FeO*Fe_2O_3-=Fe_3O_4$ .......

And so metallic iron is oxidized to $F e^{2 +} + 2 \times F e^{3 +}$ $Fe^(2+) + 2xxFe^(3+)$ ............

$3 F e (s) \to F e^{2 +} + 2 F e^{3 +} + 8 e^{-}$ $3Fe(s) rarr Fe^(2+) + 2Fe^(3+)+8e^(-)$ $(i)$ $(i)$

But something must be correspondingly reduced.....and here it is the protium ion in water........

$H_{2} O + e^{-} \to \frac{1}{2} H_{2} (g) + H O^{-}$ $H_2O+e^(-) rarr1/2H_2(g) + HO^-$ $(i i)$ $(ii)$

And so I take $(i) + 8 \times (i i)$ $(i)+8xx(ii)$ to gives...........

$3 F e (s) + 8 H_{2} O \to F e^{2 +} + 2 F e^{3 +} + 4 H_{2} (g) + 8 H O^{-}$ $3Fe(s) +8H_2Orarr Fe^(2+) + 2Fe^(3+)+4H_2(g) +8HO^-$

Charge and mass are balanced as is required...........

Science

Math

Humanities

... and beyond

How do we represent the formation of $F e_{3} O_{4}$ $Fe_3O_4$ by the oxidation of iron metal in basic conditions?

1 Answer

Explanation:

Related questions

Impact of this question

Science

Math

Humanities

... and beyond

How do we represent the formation of Fe3O4Fe_3O_4 by the oxidation of iron metal in basic conditions?

1 Answer

Explanation:

Related questions

Impact of this question

How do we represent the formation of $F e_{3} O_{4}$ $Fe_3O_4$ by the oxidation of iron metal in basic conditions?