Half Reactions

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AP Chemistry › Half Reactions

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$Fe_{(s)} + 2HCl_{(aq)} \rightarrow FeCl_{2(aq)} + H_{2(g)}$

For the redox reaction shown, which of the following half reactions occurs in the anode?

$Fe \rightarrow Fe^{2+} + 2e^{-}$

CORRECT

$Fe \rightarrow Fe^{3+} + 3e^{-}$

$Fe^{2+} + 2e^{-} \rightarrow Fe$

$2H_{2} + 2e^{-} \rightarrow H_{2}$

Explanation

Recall that oxidation always occurs at the anode (in both the electrochemical and galvanic cells). loses two electrons in this case to become $Fe^{2+}$ . The presence of $Fe^{2+}$ is hinted by the ionic compound .

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