11. For the spontaneous reaction below, choose the correct battery setup:Cd(s) + Sn2+(aq) → Cd2+(aq) + Sn(s)

The correct battery setup for the spontaneous reaction Cd(s) + Sn2+(aq) → Cd2+(aq) + Sn(s) would be as follows:

1. Anode (oxidation): The anode is the electrode where oxidation occurs. In this reaction, Cd(s) is oxidized to Cd2+(aq), so the anode is made of Cd(s).

2. Cathode (reduction): The cathode is the electrode where reduction occurs. In this reaction, Sn2+(aq) is reduced to Sn(s), so the cathode is in a solution of Sn2+(aq).

3. Salt bridge: A salt bridge is used to maintain electrical neutrality within the internal circuit, preventing the cell from rapidly running its reaction to equilibrium. It could be a U-tube filled with a salt solution, such as KNO3.

4. Direction of electron flow: Electrons flow from the anode (where oxidation occurs) to the cathode (where reduction occurs). So, in this case, electrons flow from Cd to Sn2+.

5. Overall cell reaction: The overall cell reaction is the given spontaneous reaction, which is Cd(s) + Sn2+(aq) → Cd2+(aq) + Sn(s).