Does Reduced Metal Always End Up as an Element?

[hoedown_j]

I'm wondering when the metal that is being reduced reacts, does it always end up by itself? Example:

Carbon monoxide gas is passed over hot iron (III) oxide.
(II) (III) (IV) (II)
CO + Fe2O3 ---> CO2 + Fe

When i first attempted this problem I got FeO instead of just Fe. So I am wondering will the reduce metal always end up just being an element like in this problem? Or is oxygen not listed in the answer because it is a spectator?

 

[primarygun]

Sorry, I haven't learned redox reaction or professional people on chemistry.
But in this case, I will use carbon to reduce the iron oxide instead.
According to my book, pure iron should be given out.

 

[wais]

In the process of reducing metal, oxygen plays a crucial role in the reaction. When a metal is being reduced, it is reacting with oxygen to form a metal oxide. In the example given, carbon monoxide gas is reacting with iron (III) oxide to form carbon dioxide gas and iron metal. The oxygen in the iron (III) oxide is being reduced by the carbon monoxide gas, resulting in the formation of iron metal. This is why the final product is just Fe and not FeO. Oxygen is not listed in the answer because it is a spectator in this reaction, meaning it is present but does not participate in the overall reaction. It is important to note that in some cases, the reduced metal may not end up as an element, but rather as a different compound depending on the reactants and conditions of the reaction. However, in the case of reducing metal with oxygen, the end product will typically be the metal in its elemental form.