Consider the following standard reduction potentials:
O₂ (g) + 4 H⁺ (aq) + 4e− → 2 H₂O (l) +1.23 V
Ni²⁺ (aq) + 2 e− → Ni (s) −0.28 V
Fe²⁺ (aq) + 2 e− → Fe (s) −0.45 V
Zn²⁺ (aq) + 2 e− → Zn (s) −0.77 V
Which process will occur to act as a sacrificial anode for iron?
a. 2 H₂O (l) to O₂ (g)
b. Ni²⁺ (aq) to Ni (s)
c. Zn²⁺ (aq) to Zn (s)
d. Ni (s) to Ni²⁺ (aq)
e. Zn (s) to Zn²⁺ (aq)
f. O₂ (g) to 2 H₂O (l)
