The zinc/silver oxide cell is used in hearing aids and electric watches. The following reactions take place: `ZntoZn^(2+)+2e^(-),E^(@)=0.76V`
`Ag_(2)O+H_(2)O+2e^(-)to2Ag+2OH^(-),E^(@)=0.344V`
(a) What is oxidized and reduced?
(b) Find `E^(@)` of the cell and `DeltaG` in joules.

Explanation

To solve the problem step by step, we will address both parts of the question: identifying the oxidized and reduced species, and calculating the standard cell potential (E°) and Gibbs free energy change (ΔG).

### Step 1: Identify Oxidation and Reduction
1. **Oxidation Reaction**:
- The reaction given is:
\[ \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^{-} \]
- Here, zinc (Zn) is losing 2 electrons, which means it is being oxidized.

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