a. In this cell, the aluminum electrode is undergoing oxidation, and the zinc electrode is undergoing reduction.
Oxidation occurs at the anode, and reduction occurs at the cathode. Remember, "anode" starts with the letter "A," just like "oxidation," and "cathode" starts with the letter "C," just like "reduction." Therefore, the aluminum electrode is the anode where oxidation takes place, and the zinc electrode is the cathode where reduction occurs.
b. The reduction potential of aluminum can be determined by subtracting the cell potential from the reduction potential of zinc.
Given that the cell potential is +0.92 V and zinc is the cathode, we can assume that the reduction potential of zinc is +0.92 V.
To find the reduction potential of aluminum, we subtract the cell potential from the reduction potential of zinc:
Reduction potential of aluminum = Reduction potential of zinc - Cell potential
Reduction potential of aluminum = +0.92 V - (+0.92 V)
Therefore, the reduction potential of aluminum is 0 V.
Please note that in this context, the reduction potential of aluminum is considered to be 0 V, which means it is a reference point for comparison with other elements. It does not have a positive or negative value like the reduction potential of zinc.