Answer
The reaction will occur.
Solid aluminium $Al(s)$ has oxidized; the copper (II) ion $Cu^{2+}$ has been reduced.
The oxidizing agent is the $Cu^{2+}$, and the reducing agent is the solid aluminium $Al(s)$.
Work Step by Step
- According to the Table 3.4, $Al$ is higher on the activity series than $Cu$, making that reaction possible.
- The aluminium has, initially, zero as its oxidation number, and after the reaction, it has +3, which makes it a reducing agent.
- The copper had, initially, +2 as its oxidation number, and after the reaction, it has 0, which makes it an oxidizing agent.
