Apply standard electrode potentials to determine the relative strength of oxidising and reducing agents.

Four metals are arranged in order of their standard reduction potentials: Metal A: $E° = +0.80 \text{ V}$; Metal B: $E° = +0.34 \text{ V}$; Metal C: $E° = -0.44 \text{ V}$; Metal D: $E° = -0.76 \text{ V}$. Which metal is the strongest reducing agent?

Four reduction half-reactions are listed below with their standard electrode potentials. $\mathrm{Ag}^{+}(aq) + e^{-} \rightarrow \mathrm{Ag}(s)$ \ \ $E° = +0.80 \text{ V}$ $\mathrm{Cu}^{2+}(aq) + 2e^{-} \rightarrow \mathrm{Cu}(s)$ \ \ $E° = +0.34 \text{ V}$ $\mathrm{Zn}^{2+}(aq) + 2e^{-} \rightarrow \mathrm{Zn}(s)$ \ \ $E° = -0.76 \text{ V}$ $\mathrm{Al}^{3+}(aq) + 3e^{-} \rightarrow \mathrm{Al}(s)$ \ \ $E° = -1.66 \text{ V}$ Which element is the strongest reducing agent?