Sorry, I didn't want to start a new post. Could someone please check my answer to see if it's correct. Here's the question:
2 half-cells in a galvanic cell consist of one iron (Fe) electrode in a solution of iron (II) sulphate (FeSO4) and a silver (Ag) electrode in a silver nitrate solution. Assumimg that the cell is operating as a galvanic cell, State the: oxidation half-reaction, reduction half-reaction, and the overall cell reaction. Remember to eliminate any spectator ions. Describe what will happen to the mass of the cathode and the mass of the anode while the cell is operating.
Fe = Fe^(+2) + 2e-
Ag^(+2) + 2e- = Ag
Fe + Ag^(+2) = Fe^(+2) + Ag
The mass of the Anode decreases as the reacting material becomes aqueous. The mass of the cathode increases as aqueous ions turn into a solid.