Consider the Following Half-Reactions:
Ag⁺(aq)+ E^- $\to$ Ag(s) $~~~~~~~~$ $~~~~~~~~$ E ^$\circ$ = +0

Multiple Choice

Consider the following half-reactions:
Ag⁺(aq) + e^- $\to$ Ag(s) $~~~~~~~~$$~~~~~~~~$ E ^$\circ$ = +0.80 V
Cu²⁺(aq) + 2 e^- $\to$ Cu(s) $~~~~~~~~$$~ ~~ ~$ E ^$\circ$ = +0.34 V
Pb²⁺(aq) + 2 e^- $\to$ Pb(s) $~~~~~~~~$$~~ ~ ~~$ E ^$\circ$ = -0.13 V
Fe²⁺(aq) + 2 e^- $\to$ Fe(s) $~~~~~~~~$$~~ ~ ~~$ E ^$\circ$ = -0.44 V
Al³⁺(aq) + 3 e^- $\to$ Al(s) $~~~~~~~~$$~~~ ~ ~$ E ^$\circ$ = -1.66 V
Which of the above metals or metal ions will oxidize Pb(s) ?

A) Ag⁺(aq) and Cu²⁺(aq)
B) Ag(s) and Cu(s)
C) Fe²⁺(aq) and Al³⁺(aq)
D) Fe(s) and Al(s)
E) Cu²⁺(aq) and Fe²⁺(aq)