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(D) The standard reduction potentials $(E^{0})$ at $298 \; K$ are as follows:$Au^{3+} + 3e^{-} \rightarrow Au_{(s)}, E^{0} = +1.40 \; V$$Fe^{2+} + 2e^

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$Au^{3+} + 3e^{-} \rightarrow Au_{(s)}$

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(D) The standard reduction potentials $(E^{0})$ at $298 \; K$ are as follows:$Au^{3+} + 3e^{-} \rightarrow Au_{(s)}, E^{0} = +1.40 \; V$$Fe^{2+} + 2e^{-} \rightarrow Fe_{(s)}, E^{0} = -0.44 \; V$$Mg^{2+} + 2e^{-} \rightarrow Mg_{(s)}, E^{0} = -2.36 \; V$$K^{+} + 1e^{-} \rightarrow K_{(s)}, E^{0} = -2.93 \; V$According to the electrochemical series,the species with the highest positive standard reduction potential occupies the top position. Therefore,$Au^{3+} + 3e^{-} \rightarrow Au_{(s)}$ is at the top.

Identify the reaction from the following that occupies the top position in the $EMF$ series (standard reduction potential) at $298 \; K$.

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