The standard free energy of formation of `AgCl(s)` at `25^(@)C` is `-109.7kJ mol^(-1)` and `[H^(o+)+Cl^(c-)](aq)` is `-131.2kJ mol^(-1)`. Find `E^(c-)` of a cell up cells, with standard hydrogen electrode, and `Cl^(c-)|Ag|AgCl(s)`.

Explanation

To solve the problem, we need to find the standard cell potential (E°) for the cell composed of the standard hydrogen electrode and the Ag/AgCl electrode. We will use the given standard free energy values to calculate this.

### Step-by-Step Solution:

1. **Identify the Given Data:**
- Standard free energy of formation of AgCl(s): ΔG°(AgCl) = -109.7 kJ/mol
- Standard free energy of formation of H⁺ + Cl⁻(aq): ΔG°(H⁺ + Cl⁻) = -131.2 kJ/mol

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