# What are the oxidation and reduction equations for when zinc is acting as a sacrificial anode for iron?

the oxidation of iron $F e = F {e}^{2 +} + 2 e$, E= -0,44 V, may be prevented if you supply electrons to this reaction.
The Zinc is the best of these metals and is used in the pipes of drinking water . It could give $Z n = Z {n}^{2 +} + 2 e$, E= -0,76 V,.