A voltaic cell is made with aluminum and zinc electrodes. (For Ag+(aq) + e- → Ag(s), E0 = 0.80 V and for Cu2+(aq) + 2e- → Cu(aq), E0 = 0.34 V)On the diagram below, draw and label: the salt bridge, the electrical connection between the two jars, the anode and cathode, the reaction that happens at each electrode, and the direction of electron flow. Oxidation happens at the anode. Reduction happens at the cathode.Write the standard cell notation for this cell.
To draw and label the diagram for the voltaic cell, follow these steps:
1. Draw two jars or compartments to represent the two halves of the cell. Label one as the "Aluminum Half-Cell" and the other as the "Zinc Half-Cell."
2. Inside each half-cell, draw the respective metal electrode. Label one as "Al" for aluminum and the other as "Zn" for zinc.
3. Draw a dotted line or a tube connecting the two half-cells. This represents the "electrical connection" between the two jars.
4. Inside the electrical connection, draw a salt bridge. Label it as "Salt Bridge." A salt bridge consists of an inverted U-shaped tube filled with an electrolyte solution, such as KCl or NaCl.
5. Now, identify the anode and cathode. The anode is where oxidation occurs, so label the aluminum electrode as the "Anode." The cathode is where reduction occurs, so label the zinc electrode as the "Cathode."
6. Write the half-reactions that occur at each electrode:
- At the anode: Aluminum (Al) is oxidized to form Al3+ ions and release electrons. The half-reaction is: Al(s) → Al3+(aq) + 3e-
- At the cathode: Zinc (Zn) is reduced as it accepts the released electrons and forms Zn2+ ions. The half-reaction is: Zn2+(aq) + 2e- → Zn(s)
7. Finally, indicate the direction of electron flow from the anode to the cathode. Draw an arrow showing the flow of electrons from the aluminum electrode (anode) to the zinc electrode (cathode).
The standard cell notation for this cell can be written as:
Al(s) | Al3+(aq) || Zn2+(aq) | Zn(s)