`Ag+PCl_(5)overset(Delta)to AgCl+PCl_(3)`

Options

A. For disproportionation reaction.
B. For comproportionation reaction.
C. For either intermolecular redox reaction or displacement reaction
D. For either thermal combination redox reaction or thermal decomposition redox reaction.

Answer

To solve the question regarding the reaction of silver (Ag) with phosphorus pentachloride (PCl₅) to form silver chloride (AgCl) and phosphorus trichloride (PCl₃), we will analyze the reaction step by step.

### Step-by-Step Solution:

1. **Identify the Reaction Type**:
- The reaction can be written as:
\[ \text{Ag} + \text{PCl}_5 \overset{\Delta}{\rightarrow} \text{AgCl} + \text{PCl}_3 \]
- This reaction is a **displacement reaction** because silver (Ag) is displacing phosphorus from phosphorus pentachloride (PCl₅).

**Hint**: Look for elements that are replacing others in a compound to identify displacement reactions.

2. **Determine the Oxidation States**:
- In the reactants:
- Ag is in the elemental state, so its oxidation state is 0.
- In PCl₅, chlorine (Cl) has an oxidation state of -1, thus phosphorus (P) must be +5.
- In the products:
- In AgCl, Ag has an oxidation state of +1 and Cl remains at -1.
- In PCl₃, phosphorus has an oxidation state of +3 (since Cl is still -1).

**Hint**: Assign oxidation states based on known values (e.g., Cl is typically -1 in compounds).

3. **Analyze Changes in Oxidation States**:
- For silver (Ag):
- Changes from 0 (in Ag) to +1 (in AgCl) → **Oxidation** occurs.
- For phosphorus (P):
- Changes from +5 (in PCl₅) to +3 (in PCl₃) → **Reduction** occurs.

**Hint**: Remember that oxidation is an increase in oxidation state, while reduction is a decrease.

4. **Classify the Reaction**:
- Since both oxidation and reduction are occurring, this reaction is classified as a **redox reaction**.
- Additionally, because it involves the displacement of one element by another, it is also a **thermal displacement reaction** due to the heat involved in the process.

**Hint**: A redox reaction involves both oxidation and reduction; look for changes in oxidation states to confirm.

5. **Conclusion**:
- The reaction is a **displacement reaction** and a **redox reaction**. It is not a disproportionation or comproportionation reaction because those involve a single species undergoing both oxidation and reduction.

**Final Answer**: The correct classification of the reaction is that it is a **displacement reaction** and a **redox reaction**.