Question

The diagram shows an electrochemical cell with a gold strip (left) and aluminum glasses (right). In your response, do the following: • Label the cathode and the anode, including the charge on each. • Show the flow of electrons. • Describe what type of electrochemical cell is pictured and what its use is. • What are the oxidation and reduction half-reactions in this cell?
( if the link to the picture does not work, the diagram is of a beaker with a gold strip, and glasses connected to a battery and wires)

Answer 1

This is an electrolytic cell used for (most likely) gold plating. The electrode connected to the positive terminal of the battery will be positive and attract anions from a gold salt rich solution to the electrode to undergo oxidation (=> cathode). The electrode connected to the negative terminal of the battery will be negative and attract cations to that electrode and under go reduction (=>anode). If gold plating, the gold electrode (in a gold-ion rich solution) would be connected to the negative electrode When inserted into the Au^+3 ion rich solution =>
----- Au^+3 +3e^- => Au(s)