The overall equation for the reaction occurring in this galvanic cell is A - VCE - SSCE Chemistry - Question 11 - 2011 - Paper 1

To determine the overall reaction in a galvanic cell, we need to identify the half-reactions for both the oxidation and reduction processes, analyze the species involved, and then combine them appropriately.

1. Identify Oxidation and Reduction Half-Reactions:

   • The oxidation half-reaction involves the oxidation of silver ions (Ag ext{(aq)}) to solid silver (Ag ext{(s)}).
   • The reduction half-reaction involves the reduction of copper ions (Cu^{2+} ext{(aq)}) to solid copper (Cu ext{(s)}).

2. Write the Half-Reactions:

   • Oxidation: $Ag^{+}(aq) + e^{-} → Ag(s)$
   • Reduction: $Cu^{2+}(aq) + 2e^{-} → Cu(s)$

3. Balance the Electrons:

   • To balance the electrons, you can multiply the oxidation half-reaction by 2: $2Ag^{+}(aq) + 2e^{-} → 2Ag(s)$
   • Now we can add both half-reactions:
     • Overall reaction: $2Ag^{+}(aq) + Cu(s) → 2Ag(s) + Cu^{2+}(aq)$

4. Select the Correct Answer from Options:

   • The resulting equation matches option C: C. 2Ag^{+}(aq) + Cu(s) → 2Ag(s) + Cu^{2+}(aq).