Question

The arrangement of using Mg/MgSO4 and Cu/CuSO4 couples as the half-cells to create a galvanic cell.

a) Draw a picture showing a Daniell cell-type experimental apparatus using the half-cells stated in this problem.

b) Write the notation for a cell diagram for this galvanic cell.

c) Identify the anode.

d) Identify the cathode.

e) Indicate the signs of the electrodes.

f) Describe the flow of electrons through the external wire.

g) Describe the flow of ions in the salt bridge.

Answer 1

Here the standard electrode potential of given metals are

Mg²⁺(aq) + 2e^- -> Mg(s)                              -2.38 V

Cu²⁺(aq) + 2 e^–---> Cu(s).                         +0.337 V

So copper will act as cathode (reduction) and Mg will act as anode (oxidation)

b) notation of cell will be

Mg(s) / Mg⁺²(aq) // Cu⁺²/Cu(s)

c) the anode is Magnesium

d) The cathode is Copper

e) The negative electrode is: Anode : Magnesium

The positive electrode is : Cathode : Copper

f) the flow of electrons will be from Magnesium to copper (anode to cathode)

g) the positive ion will flow towards cathode while the negative ions will flow towards anode in the salt bridge.

f)