Understanding the Reaction
In the reaction:
\[ \text{Fe}_2\text{O}_3 + 3\text{CO} \rightarrow 2\text{Fe} + 3\text{CO}_2 \]
we can identify the reducing agent by analyzing the changes in oxidation states.
Oxidation States
- In \(\text{Fe}_2\text{O}_3\), iron (Fe) has an oxidation state of +3.
- In carbon monoxide (CO), carbon has an oxidation state of +2.
- In the products, elemental iron (Fe) has an oxidation state of 0, and in carbon dioxide (CO2), carbon has an oxidation state of +4.
Identifying the Reducing Agent
- A reducing agent is a substance that loses electrons and gets oxidized in a chemical reaction.
- Here, CO is oxidized to CO2, meaning it loses electrons.
Electron Transfer
- The oxidation half-reaction for carbon monoxide can be written as:
\[ \text{CO} \rightarrow \text{CO}_2 + 2\text{e}^- \]
- This shows that CO donates electrons, thereby increasing the oxidation state of carbon from +2 to +4.
Conclusion
- Therefore, in this reaction, the reducing agent is carbon monoxide (CO), as it donates electrons and gets oxidized, leading to the reduction of iron oxide (\(\text{Fe}_2\text{O}_3\)) to elemental iron (Fe).
Summary
- Reducing Agent: CO
- Oxidation Process: CO → CO2
- Result: Reduction of Fe from +3 to 0
This detailed analysis clarifies the role of the reducing agent in the given reaction.