Electrochemical Series

Question

According to the electrochemical series, which metal is the strongest reducing agent among the following and can reduce Fe³⁺ to Fe²⁺?

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Among the given metals, the one with the **lowest (most negative) standard reduction potential ($E^\circ$)** is the **strongest reducing agent** and can reduce $Fe^{3+}$ to $Fe^{2+}$.
- Target couple: $Fe^{3+} + e^- 	o Fe^{2+}$ ($E^\circ = +0.77 	ext{ V}$)
- Standard reduction potentials of the given metals:
  - $Zn^{2+}/Zn$: $E^\circ = -0.76 	ext{ V}$
  - $Cu^{2+}/Cu$: $E^\circ = +0.34 	ext{ V}$
  - $Ag^+/Ag$: $E^\circ = +0.80 	ext{ V}$
  - $Au^{3+}/Au$: $E^\circ = +1.50 	ext{ V}$
- **Selection**: $Zn$ has the lowest $E^\circ$ ($-0.76 	ext{ V}$), making it the strongest reducing agent among the options. Since $E^\circ_{Zn} < E^\circ_{Fe^{3+}/Fe^{2+}}$, $Zn$ will spontaneously reduce $Fe^{3+}$ to $Fe^{2+}$.

Electrochemical Series

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