In the button cells widely used in watches and other devices the following reaction takes place :
`Zn(s)+Ag_(2)O(s)+H_(2)O(l) rarr Zn^(2+)(aq)+2Ag(s)+2OH^(-)(aq)`
Determine `Delta_(r)G^@` and `E^(@)` for the reaction.

Explanation

To determine the standard Gibbs free energy change (ΔG°) and the standard cell potential (E°) for the given reaction, we can follow these steps:

### Step 1: Identify the half-reactions and their standard electrode potentials.

The overall reaction is:
\[ \text{Zn}(s) + \text{Ag}_2\text{O}(s) + \text{H}_2\text{O}(l) \rightarrow \text{Zn}^{2+}(aq) + 2\text{Ag}(s) + 2\text{OH}^-(aq) \]

We need to identify the half-reactions involved:
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