In a galvanic cell, the anode is the electrode where oxidation occurs. To determine which material will act as the anode, we need to consider the tendency of each material to oxidize compared to the others.
For a galvanic cell involving magnealum (Magnesium-Aluminum) and zinc, we compare the oxidation tendencies of magnesium (Mg) and zinc (Zn). The standard reduction potentials of these metals help us understand their tendencies to lose electrons (oxidize) or gain electrons (reduce).
Magnesium has a higher tendency to oxidize (lose electrons) compared to zinc. This means that in the galvanic cell, magnesium will serve as the anode because it more readily undergoes oxidation.
Given the choices:
A. [tex]$\operatorname{Zn}(0)$[/tex]
B. [tex]$\operatorname{Mo}(O)$[/tex]
C. [tex]$Mg ^{2+}$[/tex]
D. [tex]$Zn ^{2+}$[/tex]
[tex]$Mg^{2+}$[/tex] (option C) is the correct answer because magnesium, in its ionic form, will serve as the anode in this specific galvanic cell setup.
Thus, the correct answer is:
C. [tex]$Mg ^{2+}$[/tex]
