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) to Zn^(2+) (aq) + 2Ag(s) + 2OH^(-)(aq)`
Determine `DeltaG^(@)` and `E^(@)` for the reaction
`Zn(s) to Zn^(2+) + 2e^(-) , E^(@) = 0.76` V
`Ag_(2)O + H_(2)O + 2e^(-) to 2Ag + 2OH^(-)`
`E^(@) = +0.34` V

Explanation

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

### Step 1: Identify the half-reactions and their standard potentials
The overall cell reaction is:
\[ \text{Zn}(s) + \text{Ag}_2\text{O}(s) + \text{H}_2\text{O}(l) \rightarrow \text{Zn}^{2+}(aq) + 2\text{Ag}(s) + 2\text{OH}^-(aq) \]

The half-reactions are:
1. **Oxidation (Anode reaction)**:
...