`Sn+PCl_(5)overset(Delta)toSnCl_(4)+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 analyze the given reaction \( \text{Sn} + \text{PCl}_5 \overset{\Delta}{\rightarrow} \text{SnCl}_4 + \text{PCl}_3 \), we can break it down into a step-by-step solution.

### Step 1: Identify the Reactants and Products
The reactants in this reaction are tin (Sn) and phosphorus pentachloride (PCl₅). The products are tin(IV) chloride (SnCl₄) and phosphorus trichloride (PCl₃).

### Step 2: Determine the Oxidation States
- **Tin (Sn)**: In elemental form, the oxidation state of Sn is 0. In SnCl₄, the oxidation state of Sn is +4.
- **Phosphorus (P)**: In PCl₅, the oxidation state of P is +5. In PCl₃, the oxidation state of P is +3.
- **Chlorine (Cl)**: In both PCl₅ and PCl₃, the oxidation state of Cl is -1.

### Step 3: Analyze the Changes in Oxidation States
- Tin (Sn) is oxidized from 0 to +4.
- Phosphorus (P) is reduced from +5 in PCl₅ to +3 in PCl₃.
- Chlorine (Cl) is not changing its oxidation state in this reaction.

### Step 4: Classify the Reaction
This reaction involves both oxidation (of Sn) and reduction (of P). Therefore, it is classified as a redox reaction. Specifically, it can be identified as a disproportionation reaction because one element (phosphorus) is being reduced while another (tin) is being oxidized.

### Step 5: Write the Balanced Equation
The balanced equation is already provided:
\[ \text{Sn} + \text{PCl}_5 \rightarrow \text{SnCl}_4 + \text{PCl}_3 \]

### Conclusion
This reaction is a redox reaction where tin is oxidized and phosphorus is reduced.

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