Question

From the information provided, use cell notation to describe the following systems:
(a) In one half-cell, a solution of Pt(NO3)2 forms Pt metal, while in the other half-cell, Cu metal goes into a
Cu(NO3)2 solution with all solute concentrations 1 M.
(b) The cathode consists of a gold electrode in a 0.55 M Au(NO3)3 solution and the anode is a magnesium electrode
in 0.75 M Mg(NO3)2 solution.
(c) One half-cell consists of a silver electrode in a 1 M AgNO3 solution, and in the other half-cell, a copper electrode
in 1 M Cu(NO3)2 is oxidized

Answer 1

a)   

Anode half reaction: Oxidation takes place at anode

Cu    ----------> Cu(NO₃)₂ + 2e-

Cathode half reaction: Reduction takes place at cathode

Pt(NO₃)₂ (s) + 2e-    -------> Pt

Cell notation: anode II cathode

Cu I Cu(NO₃)₂ (1 M) II Pt(NO₃)₂ (1 M) I Pt

b)

Anode half reaction: Oxidation takes place at anode

Mg ----------> Mg(NO₃)₂ + 2e-

Cathode half reaction: Reduction takes place at cathode

Au(NO₃)₃ (s) + 3e-    -------> Au

Cell notation: anode II cathode

Mg I Mg(NO₃)₂ (0.75 M) II Au(NO₃)₃ (0.55 M) I Au

c)

Anode half reaction: Oxidation takes place at anode

Cu    ----------> Cu(NO₃)₂ + 2e-

Cathode half reaction: Reduction takes place at cathode

AgNO₃ + e-    -----------> Ag

Cell notation: anode II cathode

Cu I Cu(NO₃)₂ (1 M) II AgNO₃ (1 M) I Ag