For the cell `Zn|ZnCl_(2)(m)|AgCl,E` is `1.24V` at `25^(@)C` and `1.260V` at `35^(@)C` of `m=10^(-3)`. Write down the cell reaction and calculate `DeltaG, DeltaH,` and `DeltaS` at `25^(@)C`.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Write down the cell reaction
The cell consists of zinc (Zn) and silver chloride (AgCl). The oxidation and reduction reactions can be expressed as follows:

- Oxidation: \( \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^- \)
- Reduction: \( \text{AgCl} + e^- \rightarrow \text{Ag} + \text{Cl}^- \)

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