Write Nernst equation and calculate e.m.f of the following cells at 298 K :
`Sn (s) |Sn^(2+) (0.050 M) ||H^(+) (0.020 M) |H_(2) ` (1atm) | Pt
Given : `E_((Sn^(2+) | Sn))^(Theta) = -0.14 V`

Explanation

To solve the problem, we will follow these steps:

### Step 1: Write the half-reactions
Identify the oxidation and reduction half-reactions for the cell.

- **Oxidation half-reaction (Anode):**
\[
\text{Sn (s)} \rightarrow \text{Sn}^{2+} + 2e^-
...