Silver-Cadmium Electrochemical Cell

[Wardling]

You are given the following materials:
 Silver wire
 A 0.10 mol L-1 solution of cadmium nitrate
 Cadmium wire
 A 0.10 mol L-1 solution of silver nitrate
 A salt bridge
 Copper wire
 Beakers and other glassware as required
Draw a labelled sketch of your cell. Describe how the electrochemical cell will function. Include equations for the reactions and what you would expect to see happen.

I know that if I ignore the copper wire, I can put the AgNO3 and the Ag wire into one beaker, and the Cd(NO3)2 and Cd wire into another beaker. I can connect the two using the salt bridge. The electrons will flow from the Cd to the Ag. The Cd will be oxidised (Cd >><< Cd2+ + 2e-), and the Ag will be reduced (2AG+ + 2e- >><< 2Ag). The net ionic equation is: 2Ag+(aq) + Cd(s) >><< Cd2+(aq) + 2Ag(s).

My question is what does the copper wire do? Is it to make the current reversible? Or for plating?

 

[Wardling]

Silly me, the copper wire connects the two electrodes providing a path for the electrons to travel through!