Answer :
Explanation:
Sure, I can help with that! Let's write the cell reactions for the given electrochemical cells:
(a) Ag | Ag+(aq) || Cu2+(aq) | Cu:
1. Cathode half-reaction (reduction at the cathode):
\[ Cu^{2+}(aq) + 2e^- \rightarrow Cu(s) \]
2. Anode half-reaction (oxidation at the anode):
\[ Ag(s) \rightarrow Ag^+(aq) + e^- \]
Overall cell reaction:
\[ Cu^{2+}(aq) + 2Ag(s) \rightarrow Cu(s) + 2Ag^+(aq) \]
(c) Pt, Cl2 | Cl-(aq) || Ag+(aq) | Ag:
1. Cathode half-reaction (reduction at the cathode):
\[ Ag^+(aq) + e^- \rightarrow Ag(s) \]
2. Anode half-reaction (oxidation at the anode):
\[ Cl_2(g) + 2e^- \rightarrow 2Cl^-(aq) \]
Overall cell reaction:
\[ 2Ag^+(aq) + Cl_2(g) \rightarrow 2Ag(s) + 2Cl^-(aq) \]
(b) Pt | Fe2+, Fe3+ || MnO4-, Mn2+, H+ | Pt:
1. Cathode half-reaction (reduction at the cathode):
\[ 5Fe^{3+}(aq) + 5e^- \rightarrow 5Fe^{2+}(aq) \]
2. Anode half-reaction (oxidation at the anode):
\[ MnO_4^-(aq) + 8H^+ + 5e^- \rightarrow Mn^{2+}(aq) + 4H_2O(l) \]
Overall cell reaction:
\[ 5Fe^{3+}(aq) + MnO_4^-(aq) + 8H^+ \rightarrow 5Fe^{2+}(aq) + Mn^{2+}(aq) + 4H_2O(l) \]
(d) Pt, H2 | H+(aq) || Cd2+(aq) | Cd:
1. Cathode half-reaction (reduction at the cathode):
\[ Cd^{2+}(aq) + 2e^- \rightarrow Cd(s) \]
2. Anode half-reaction (oxidation at the anode):
\[ 2H_2O(l) \rightarrow O_2(g) + 4H^+ + 4e^- \]
Overall cell reaction:
\[ Cd^{2+}(aq) + 2H_2O(l) \rightarrow Cd(s) + O_2(g) + 4H^+ \]
These reactions represent the electrochemical processes occurring in each cell configuration.