Using the standard electrode potentials given in the Table 8.2, predict if the reaction between the following is feasible:
`Ag^(+)(aq)` and `Cu(s)`

Explanation

To determine if the reaction between silver ions (\(Ag^+\)) and solid copper (\(Cu\)) is feasible, we will follow these steps:

### Step 1: Identify the Standard Electrode Potentials
We need to look up the standard electrode potentials for the half-reactions involved. From the given data:
- The standard electrode potential for the reduction of silver ions (\(Ag^+\)) to silver metal (\(Ag\)) is \(E^\circ = +0.80 \, V\).
- The standard electrode potential for the reduction of copper ions (\(Cu^{2+}\)) to copper metal (\(Cu\)) is \(E^\circ = +0.34 \, V\).

### Step 2: Determine the Half-Reactions
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