For a cell `Ag(s)|AgNO_(3)(0.01M)||AgNO_(3)(1.0M)|Ag(s)`
(i). Calculate the e.m.f. of the cell at `25^(@)C`
(ii). Write the net cell reaction.
(iii). Will the cell generate e.m.f when two concentrations become equal?

Explanation

To solve the given problem step by step, we will address each part of the question systematically.

### (i) Calculate the e.m.f. of the cell at `25°C`

1. **Identify the half-reactions:**
The cell consists of silver (Ag) reactions:
- Reduction: \( \text{Ag}^+ + e^- \rightarrow \text{Ag} \) (at 1.0 M concentration)
- Oxidation: \( \text{Ag} \rightarrow \text{Ag}^+ + e^- \) (at 0.01 M concentration)
...