To convert the given redox reaction into the correct oxidation half-reaction, we need to identify which species is being oxidized.
In the reaction:
\[ 2 \text{Al} + 3 \text{Fe}^{3+} \rightarrow 2 \text{Al}^{3+} + 3 \text{Fe} \]
Aluminum (Al) is oxidized from its elemental form (0 oxidation state) to aluminum ions (\( \text{Al}^{3+} \)), while iron (\( \text{Fe}^{3+} \)) is reduced to elemental iron (Fe).
The oxidation half-reaction involves the loss of electrons. For aluminum, this is expressed as:
\[ \text{Al} \rightarrow \text{Al}^{3+} + 3e^- \]
This corresponds to option C:
C: Al → Al^(3+) + 3e
Thus, the correct oxidation half-reaction is C.
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