To identify the element that was reduced in the given redox reaction:
\[ \text{Fe}_2\text{O}_3 + 3\text{CO} \rightarrow 2\text{Fe} + 3\text{CO}_2 \]
we need to analyze the oxidation states of the elements in the reactants and products.
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In \(\text{Fe}_2\text{O}_3\):
- Iron (\(Fe\)) has an oxidation state of +3.
- Oxygen (\(O\)) has an oxidation state of -2.
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In \(\text{CO}\):
- Carbon (\(C\)) has an oxidation state of +2.
- Oxygen (\(O\)) has an oxidation state of -2.
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In the products:
- In elemental iron (\(Fe\)), the oxidation state is 0.
- In \(\text{CO}_2\):
- Carbon (\(C\)) has an oxidation state of +4.
- Oxygen (\(O\)) remains -2.
Now, let's see what happens to each key element:
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Iron:
- Changes from +3 in \(\text{Fe}_2\text{O}_3\) to 0 in elemental \(Fe\). This is a reduction because the oxidation state decreases.
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Carbon:
- Changes from +2 in \(\text{CO}\) to +4 in \(\text{CO}_2\). This indicates that carbon is oxidized because the oxidation state increases.
Therefore, the element that is reduced, meaning it gains electrons (or is reduced in oxidation state), is iron (Fe).
So, the correct answer is:
C. Fe
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