a galvanic cell based on the reaction between silver ions and copper is constructed equation 2Ag+(aq) + Cu(s)-> 2AG(s) + Cu2+(aq) (see details)
Identify the chemical that is oxidized and the chemical that is reduced.
identify the anode and cathode in this cell.
which electrode increases in mass as the reaction proceeds? why?
If the voltage across the electrodes is oberved to be 1.1 V, what would be the voltage if three of these cells are connected in series.
1. To determine which chemical was oxidized and which one is reduced you need to locate a standard potential table. According to the table,
Ag is the oxidizer because it's higher on the table meaning it's oxidizing
Cu is the reducing because it's lower on the table
Ag is oxidizer and Cu is reducing
2. We know that oxidizers are the anode because they accept electrons and the reducer are the cathode because they donate electrons. Therefore,
Ag is the anode and Cu is the cathode
3. In order to determine this, we need to know the molarity of the solutions that were added to each of the cells.
4. Each of the cells would have the same voltage because they are all the same solution. The total voltage would be 3.3V.