In the reaction 2Fe2O3 + 3C → 4Fe + 3CO2, what is being oxidized?

• A. O in Fe2O3
• B. Fe in Fe
• C. C in C
• D. Fe in Fe2O3

Answer: (C)

Verified step by step guidance

1. Identify the oxidation states of each element in the reactants and products. This helps determine which element loses electrons (is oxidized) and which gains electrons (is reduced).
2. For Fe in Fe2O3, assign oxidation numbers: oxygen is typically -2, so for Fe2O3, calculate Fe's oxidation state using the formula \$2 \times x + 3 \times (-2) = 0\(, where \)x$ is the oxidation state of Fe.
3. For carbon (C) in elemental form, the oxidation state is 0. In the product CO2, oxygen is -2, so calculate carbon's oxidation state using \(x + 2 \times (-2) = 0\).
4. Compare the oxidation states of carbon before and after the reaction. An increase in oxidation state indicates oxidation (loss of electrons).
5. Conclude which element is oxidized by identifying the one whose oxidation state increases during the reaction.