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 problem step by step, we will address each part of the question regarding the electrochemical cell.

### Step 1: Calculate the e.m.f. of the cell at 25°C

1. **Identify the cell type**: The cell is a concentration cell involving silver (Ag) and silver nitrate (AgNO₃) solutions of different concentrations.

2. **Write the half-cell reactions**:
- At the anode (oxidation):
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