Consider the cell:
`Mg(s)|Mg^(2+)(0.13M)||Ag^(+)(1.0xx10^(-4))M|Ag(s)`
its e.m.f. is `2.96V.` calculate `E_("cell")^(@)`
`(R=8.314JK^(-1),1F=96500Cmol^(-1))`

Explanation

To calculate the standard cell potential \( E^\circ_{\text{cell}} \) for the given electrochemical cell, we can follow these steps:

### Step 1: Identify the half-reactions
The half-reactions for the cell are:
- Oxidation: \( \text{Mg}(s) \rightarrow \text{Mg}^{2+} + 2e^- \)
- Reduction: \( 2\text{Ag}^+ + 2e^- \rightarrow 2\text{Ag}(s) \)

### Step 2: Write the overall cell reaction
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