In the reaction given in euaqution
Zn(s)+PbCl 2 ​ (aq)→Pb(s)+ZnCl2 ​ (aq)
mention:
I. Which reactant is oxidised? To what?
II. Which reactant is the oxidiser?
III.Which reactant is reduced? To what?
IV. What reactant is the reducer?

Explanation

To analyze the redox reaction given in the equation:

**Zn(s) + PbCl₂(aq) → Pb(s) + ZnCl₂(aq)**

we need to identify the oxidation and reduction processes involved. Let's break it down step by step.

### Step 1: Identify Oxidation States
- **Zinc (Zn)** starts as a neutral element (0 oxidation state) and ends up in **ZnCl₂** where it has an oxidation state of **+2**.
- **Lead (Pb)** in **PbCl₂** has an oxidation state of **+2** and ends up as a neutral element (0 oxidation state).

### Step 2: Determine Oxidation and Reduction
- **Oxidation** is the process where a substance loses electrons. Here, **Zn** is oxidized from 0 to +2, losing 2 electrons:
\[ Zn → Zn^{2+} + 2e^- \]

- **Reduction** is the process where a substance gains electrons. Here, **Pb^{2+}** is reduced from +2 to 0, gaining 2 electrons:
\[ Pb^{2+} + 2e^- → Pb \]

### Step 3: Identify the Reactants
1. **Which reactant is oxidized? To what?**
- **Zn** is oxidized to **Zn²⁺**.

2. **Which reactant is the oxidizer?**
- **Pb²⁺** is the oxidizer because it gains electrons.

3. **Which reactant is reduced? To what?**
- **Pb²⁺** is reduced to **Pb**.

4. **What reactant is the reducer?**
- **Zn** is the reducer because it donates electrons.

### Final Answers:
I. **Zn** is oxidized to **Zn²⁺**.
II. **Pb²⁺** is the oxidizer.
III. **Pb²⁺** is reduced to **Pb**.
IV. **Zn** is the reducer.

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