# How do you know how to...?

## $\left(i\right)$ represent the complete oxidation of iron metal to ferric oxide? $\left(i i\right)$ represent the thermal decomposition of ferrous oxalate? $\left(i i i\right)$ represent the disproportionation of ferrous oxide?

Jul 8, 2017

So how do you know? Got me.....?

#### Explanation:

Of course, you have to look at the context of the question.......$\text{Iron metal is heated under excess dioxygen gas for a }$
$\text{prolonged period........}$ Such conditions, would favour oxidation to $\text{ferric iron}$.

$2 F e \left(s\right) + \frac{3}{2} {O}_{2} \left(g\right) + \Delta \rightarrow F {e}_{2} {O}_{3} \left(s\right)$

On the other hand, $\text{iron oxalate}$ can be thermally decomposed to $\text{iron oxide}$ and $\text{carbon dioxide}$ and $\text{carbon monoxide}$.

$F e {C}_{2} {O}_{4} \left(s\right) + \Delta \rightarrow F e O \left(s\right) + C O \left(g\right) + C {O}_{2} \left(g\right)$

On the other, other hand, $\text{ferrous oxide}$ could disproportionate to give iron metal and the mixed oxidation state $\text{magnetite}$.....

$3 F e O \left(s\right) + \Delta \rightarrow F e \left(s\right) + F {e}_{2} {O}_{3} \left(s\right)$

.........here $F {e}_{2} {O}_{3}$ $\text{aka magnetite}$ is a mixed oxidation state iron oxide.......$F e O \cdot F e {O}_{2}$, i.e. an $F e \left(+ I V\right)$ centre........

Depending where you are, you should be spoon-fed this info.