electrochemistry

Question

Determine the standard cell potential for the following galvanic cell: Ag(s) | Ag + (aq) || Mg 2+ (aq) | Mg(s)

Answer 1

Looking up the standard reduction potentials, I find the following values:

Ag+ + e- ==> Ag(s) Eº = 0.80 V

Mg2+ + 2e- ==> Mg(s) Eº = -2.37 V

Given these standard reduction potentials and the cell notation of Ag(s) | Ag⁺ (aq) || Mg²⁺ (aq) | Mg(s), we can find the standard potential of the cell.

From the cell notation, the Mg will be the cathode and the Ag will be the anode. The cell potential can be calculated as Eºcathode - Eºanode = -2.37 - 0.80 = -3.17 V. Note that is will not be a spontaneous reaction since the potential is negative. To have this be a spontaneous reaction, the electrodes would need to be switched and the cell would have to be Mg(s) | Mg²⁺(aq) || Ag⁺(aq) | Ag(s)