Consider a cell composed of two cells:
(i). `Cu(s)Cu^(2+)(aq)` and (ii). `Ag(s)|Ag^(+)(aq)`
(b). The cell potential when `[Cu^(2+)]=2M` and `|Ag^(+)|=0.05M`
[Given: `C_(Cu^(2+)//Cu)^(@)=+0.344V,E_(Ag^(+)//Ag)^(@)=+0.80V]`

Explanation

To solve the problem, we need to calculate the cell potential for the electrochemical cell composed of two half-cells: \( \text{Cu(s)} | \text{Cu}^{2+}(aq) \) and \( \text{Ag(s)} | \text{Ag}^{+}(aq) \).

### Step-by-Step Solution:

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