Make complete cell diagrams of the following cell reactions
(a). `Cd^(2)(aq)+Zn(s)toZn^(2+)(aq)+Cd(s)`
(b). `2Ag^(+)(aq)+H_(2)(g)to2H^(+)(aq)+2Ag(s)`
(c). `Hg_(2)Cl_(2)(s)+Cu(s)toCu^(2+)(aq)+2Cl^(-)(aq)+2Hg(l)`
(d). `Cu_(2)O_(7)^(2-)(aq)+14H^(+)(aq)+6Fe^(2+)(aq)to6Fe^(3+)(aq)+2Cr^(3+)(aq)+7H_(2)O(l)`

Explanation

To create complete cell diagrams for the given cell reactions, we need to follow a systematic approach. A cell diagram typically includes the anode (where oxidation occurs), the cathode (where reduction occurs), and the salt bridge. The general format for a cell diagram is:

**Anode | Anode solution || Cathode solution | Cathode**

Now, let's break down each reaction step by step.

### (a) Cell Reaction: `Cd^(2+)(aq) + Zn(s) → Zn^(2+)(aq) + Cd(s)`

1. **Identify the Anode and Cathode:**
- **Oxidation:** Zn(s) → Zn^(2+)(aq) (Zinc is oxidized)
- **Reduction:** Cd^(2+)(aq) → Cd(s) (Cadmium is reduced)

2. **Write the Cell Diagram:**
- Anode: Zn(s)
- Anode Solution: Zn^(2+)(aq)
- Cathode: Cd(s)
- Cathode Solution: Cd^(2+)(aq)

**Cell Diagram:**
\[ \text{Zn(s) | Zn}^{2+}(aq) || \text{Cd}^{2+}(aq) | \text{Cd(s)} \]

### (b) Cell Reaction: `2Ag^(+)(aq) + H_(2)(g) → 2H^(+)(aq) + 2Ag(s)`

1. **Identify the Anode and Cathode:**
- **Oxidation:** H₂(g) → 2H^(+)(aq) (Hydrogen is oxidized)
- **Reduction:** 2Ag^(+)(aq) → 2Ag(s) (Silver is reduced)

2. **Write the Cell Diagram:**
- Anode: H₂(g)
- Anode Solution: H^(+)(aq)
- Cathode: Ag(s)
- Cathode Solution: Ag^(+)(aq)

**Cell Diagram:**
\[ \text{H}_2(g) | \text{H}^+(aq) || \text{Ag}^+(aq) | \text{Ag(s)} \]

### (c) Cell Reaction: `Hg_(2)Cl_(2)(s) + Cu(s) → Cu^(2+)(aq) + 2Cl^(-)(aq) + 2Hg(l)`

1. **Identify the Anode and Cathode:**
- **Oxidation:** Cu(s) → Cu^(2+)(aq) (Copper is oxidized)
- **Reduction:** Hg₂Cl₂(s) → 2Hg(l) + 2Cl^(-)(aq) (Mercury is reduced)

2. **Write the Cell Diagram:**
- Anode: Cu(s)
- Anode Solution: Cu^(2+)(aq)
- Cathode: Hg(l)
- Cathode Solution: Hg₂Cl₂(s)

**Cell Diagram:**
\[ \text{Cu(s) | Cu}^{2+}(aq) || \text{Hg}_2\text{Cl}_2(s) | \text{Hg(l)} + 2\text{Cl}^-(aq) \]

### (d) Cell Reaction: `Cu_(2)O_(7)^(2-)(aq) + 14H^(+)(aq) + 6Fe^(2+)(aq) → 6Fe^(3+)(aq) + 2Cr^(3+)(aq) + 7H_(2)O(l)`

1. **Identify the Anode and Cathode:**
- **Oxidation:** 6Fe^(2+)(aq) → 6Fe^(3+)(aq) (Iron is oxidized)
- **Reduction:** Cu₂O₇^(2-)(aq) + 14H^(+)(aq) → 2Cr^(3+)(aq) + 7H₂O(l) (Chromium is reduced)

2. **Write the Cell Diagram:**
- Anode: Fe^(2+)(aq)
- Anode Solution: Fe^(3+)(aq)
- Cathode: Cr^(3+)(aq)
- Cathode Solution: Cu₂O₇^(2-)(aq) + H^(+)(aq)

**Cell Diagram:**
\[ \text{Fe}^{2+}(aq) | \text{Fe}^{3+}(aq) || \text{Cu}_2\text{O}_7^{2-}(aq) + 14\text{H}^+(aq) | \text{Cr}^{3+}(aq) + 7\text{H}_2\text{O}(l) \]