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 \(\frac{[\text{Sn}^{2+}]}{[\text{Pb}^{2+}]}\) when the electrochemical cell reaches equilibrium. We will use the Nernst equation to do this.

### Step-by-Step Solution:

1. **Identify the Half-Reactions and Standard Potentials**:
- The half-reaction for tin (Sn) is:
\[
\text{Sn}^{2+} + 2e^- \rightarrow \text{Sn} \quad E^\circ = -0.14 \, \text{V}
...