Write the half equations for each of the following redox reactions.
`Zn(s)+PbCl_(2)(aq)toZnCl_(2)(aq)+Pb(s)`

Explanation

To write the half equations for the given redox reaction \( \text{Zn(s)} + \text{PbCl}_2(aq) \rightarrow \text{ZnCl}_2(aq) + \text{Pb(s)} \), we need to identify the oxidation and reduction processes occurring in the reaction.

### Step-by-Step Solution:

1. **Identify the oxidation and reduction components:**
- In this reaction, zinc (Zn) is being oxidized as it goes from solid zinc to zinc ions (\( \text{Zn}^{2+} \)).
- Lead (Pb) in lead(II) chloride (\( \text{PbCl}_2 \)) is being reduced as it goes from lead ions (\( \text{Pb}^{2+} \)) to solid lead (Pb).

...