Iron (III) carbonate heated strongly yields iron (III) oxide plus carbon dioxide

Question

Iron (III) carbonate heated strongly yields iron (III) oxide plus carbon dioxide: complete, balance, and classify the chemical reaction. direct combination/decomposition/single replacement/double replacement (circle one)

Explanation / Answer

follow this Here's the first problem. You have mentioned iron(III) carbonate. It doesn't exist. With iron in the +3 oxidation state, the solution will be too acidic, and will cause the decomposition of the carbonate into carbon dioxide. You might want to consider this reaction: Fe2O3(s) + CO(g) --> 2FeO(s) + CO2(g) The carbon monoxide will reduce the iron from +3 to +2, and the carbon will be oxidized from +2 to +4. =========== Follow up ============= Lets go back to the beginning. If we're talking about the refining of iron ore, then the reaction is as follows: Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g) There is no formation of Fe2(CO3)3, also known as iron(III) carbonate. Iron(III) carbonate does not exist. There is no listing for iron(III) carbonate in the Handbook of Chemistry and Physics. This "reaction" is simply nonsense: Fe2O3 + CO ---> Fe2(CO3)3 For one thing, the oxidation state of carbon is going from +2 in CO to +4 in Fe2(CO3)3. That's called oxidation, and it must be accompanied by reduction, which it isn't. You can't have oxidation without reduction. The two always go together. In this reaction ... Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g) ... carbon is oxidized to the +4 state in CO2, and iron is reduced to the metallic state.

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