In the button cell, widely used in watches, the following reaction takes place
`Zn(s)+Ag_(2)O(s)+H_(2)O to Zn^(2+)(aq)+2Ag(s)+2OH^(-)(aq)`
Determine `E^(@)` and `DeltaG^(@)` for the reaction.
(Given : `E_(Ag^(+)//Ag)^(@)=+0.80 V,E_(Zn^(2+)//Zn)^(@)=-0.76 V`

Explanation

To determine the standard cell potential \( E^\circ \) and the standard Gibbs free energy change \( \Delta G^\circ \) for the reaction given in the button cell, we can follow these steps:

### Step 1: Identify the Half-Reactions
The overall reaction is:
\[ \text{Zn(s)} + \text{Ag}_2\text{O(s)} + \text{H}_2\text{O} \rightarrow \text{Zn}^{2+}(aq) + 2\text{Ag(s)} + 2\text{OH}^-(aq) \]

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