Formulate the galvanic cell in which the following reaction takes place:
`Zn(s)+2Ag^(+)(aq)toZn^(2+)(aq)+2Ag(s)`
State (i) Which one of the electrodes is negatively charged?
(ii) The reaction taking place at each of its electrode. ltBrgt (iii) The carriers of current within this cell.

Explanation

To formulate the galvanic cell for the reaction \( \text{Zn(s)} + 2\text{Ag}^+(aq) \rightarrow \text{Zn}^{2+}(aq) + 2\text{Ag(s)} \), we can follow these steps:

### Step 1: Identify the Oxidation and Reduction Reactions
- **Oxidation**: Zinc (Zn) is oxidized to zinc ions (\( \text{Zn}^{2+} \)).
\[ \text{Zn(s)} \rightarrow \text{Zn}^{2+}(aq) + 2e^- \]
- **Reduction**: Silver ions (\( \text{Ag}^+ \)) are reduced to silver metal (Ag).
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