Write the cell reaction for the given cell diagram

Question

A. Cu(s) | Cu^2+ | | Fe^2+ | Fe(s)

B. Ag(s) | Ag^+ | | Mg^2+ | Mg(s)

C. Ag(s) | AgCl1 Cl^- | Na^+ | Na(s)

D. Pt(s) | Sn^+ 1Sn^2+ | | Ni^2+ | Ni(s)

Answer 1

In these diagrams, the anode is generally written on the left, and the cathode on the right. A salt bridge

( || ) is placed in between. Oxidation takes place at the anode and reduction takes place at the cathode.

So, looking at (A), we have...

Cu(s) is the anode and Fe(s) is the cathode.

Oxidation @ the anode and reduction @ the cathode would thus be...

Fe²⁺ + 2e- ==> Fe(s) reduction half reaction

Cu(s) ===> Cu²⁺ + 2e- oxidation half reaction

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Fe²⁺ + Cu ==> Fe(s) + Cu²⁺ Cell Reaction

In (B), we have...

Mg²⁺ + 2e- ==> Mg(s) reduction half reaction

2Ag(s) ==> 2Ag⁺ + 2e- oxidation half reaction

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Mg2+ + 2Ag(s) ==> Mg(s) + 2Ag+ Cell Reaction

Hopefully you can now do (C) and (D)