The correct cell representation for the following reaction is
$Mg(s) +2Ag^+ (0.0001 M) → Mg^{2+} (0.130 M) +2Ag(s)$
Answer & explanation
Correct answer: option 1
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:
$\text{Mg(s)}|\text{Mg}^{2+}(0.130\,\text{M})||\text{Ag}^+(0.0001\,\text{M})|\text{Ag(s)}$