how on earth do you balance this equation. we haven‘t learned anything beyond balancing by inspection, and i was pretty good at it most of the time, but i honestly think this one is impossible.
except for nitrogen everytin else is heterogenous
except for nitrogen everytin else is heterogenous
Fe2O3 + 3CO --- 2Fe + 3CO2 U can do this for the period of two strategies one is the person-friendly atom conservation device and different one is redox technique 2d technique Fe3+ + 3e -- Fe CO + O2- --- CO2 + 2e Now stability for the no of electrons on the two part
Fe2O3 + 3CO --- 2Fe + 3CO2 U can do this for the period of two strategies one is the person-friendly atom conservation device and different one is redox technique 2d technique Fe3+ + 3e -- Fe CO + O2- --- CO2 + 2e Now stability for the no of electrons on the two part
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.
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.
