Represent the cell in which following reaction takes place `:`
`Mg(s)+2Ag^(o+)(0.0001M)rarr Mg^(2+)(0.130M)+2Ag(s)` calculate its `E_(cell)` if `E^(c-)._(cell)=3.17V. `

Explanation

To solve the problem, we need to represent the electrochemical cell for the given reaction and calculate the cell potential (E_cell).

### Step 1: Write the half-reactions
The overall reaction given is:
\[ \text{Mg}(s) + 2 \text{Ag}^+(aq) \rightarrow \text{Mg}^{2+}(aq) + 2 \text{Ag}(s) \]

We can break this down into two half-reactions:
1. **Oxidation half-reaction (at the anode)**:
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