The correct cell representation for the following reaction is

$Mg(s) +2Ag^+ (0.0001 M) → Mg^{2+} (0.130 M) +2Ag(s)$

$Mg(s) | Mg^{2+} (0.130M) || Ag^+ (0.0001M) | Ag(s)$

The correct answer is Option (1) → $Mg(s) | Mg^{2+} (0.130M) || Ag^+ (0.0001M) | Ag(s)$

Given reaction:

$\text{Mg(s)} + 2\text{Ag}^+ (0.0001\,\text{M}) \rightarrow \text{Mg}^{2+} (0.130\,\text{M}) + 2\text{Ag(s)}$

• Oxidation (anode): Mg(s) → Mg²⁺ + 2e⁻
• Reduction (cathode): Ag⁺ + e⁻ → Ag(s)

In cell representation:

• Anode is written on the left
• Cathode is written on the right
• Format:

$\text{Anode}|\text{Anode ion}||\text{Cathode ion}|\text{Cathode}$

So the correct cell notation is:

$\text{Mg(s)}|\text{Mg}^{2+}(0.130\,\text{M})||\text{Ag}^+(0.0001\,\text{M})|\text{Ag(s)}$