For an electrochemical cell `Sn(s)Sn^(2+) (aq,1M)||pb^(2+) (Aq,1M)|Pb(s)` the ratio `([Sn^(2+)])/([Pb^(2+)]` when this cell attians equilibrium is_______ (Given : `E_(sn^(2+)|Sn)^(@) = -0.14V, E_(pb^(2+|Pb^(@))= -0.13V, (2.303RT)/(F = 0.06))`

Explanation

To solve the problem, we need to find the ratio of the concentrations of \( \text{Sn}^{2+} \) to \( \text{Pb}^{2+} \) when the electrochemical cell reaches equilibrium. We will use the Nernst equation and the standard reduction potentials provided.

### Step-by-Step Solution:

1. **Identify the Half-Reactions**:
- Oxidation (Anode):
\[
\text{Sn}(s) \rightarrow \text{Sn}^{2+}(aq) + 2e^-
...