For the cells
`2Ag + Pt^(2+) to 2Ag^(+) + Pt , E^@ = 0.4V`
`2Ag + F_2 to 2Ag^(+) + 2F^(-) , E^@ = 2.07V`
if the potential for the reaction `Pt to Pt^(2+) + 2e` is assigned as zero, determine the potential for the following electrodes.
`(i) Ag to Ag^(+) + e`
`(ii) F^(-) to 1/2 F_2 + e`

Explanation

To determine the electrode potentials for the reactions given in the question, we will follow these steps:

### Step 1: Determine the potential for the reaction \( \text{Ag} \to \text{Ag}^+ + e^- \)

We know from the cell reaction:
\[ 2\text{Ag} + \text{Pt}^{2+} \to 2\text{Ag}^+ + \text{Pt} \]
with a standard cell potential \( E^\circ_{\text{cell}} = 0.4 \, \text{V} \).

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