Which of the following gas mixture is not applicable for Dalton’s law of partial pressure ?

Options

A. `SO_(2)` and `Cl_(2)`
B. `CO_(2)` and `N_(2)`
C. CO and `CO_(2)`
D. CO and `N_(2)`

Answer

To determine which gas mixture is not applicable for Dalton’s law of partial pressure, we need to understand the conditions under which Dalton's law holds true. Dalton's law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of each gas. However, if the gases react with each other, the number of moles of gas changes, which affects the total pressure and the partial pressures.

### Step-by-Step Solution:

1. **Understanding Dalton's Law**:
- Dalton’s law of partial pressures applies to mixtures of non-reacting gases. The total pressure is the sum of the partial pressures of each gas in the mixture.

2. **Identifying the Mixtures**:
- We need to analyze the given gas mixtures to see if any of them involve reacting gases.

3. **Analyzing the Options**:
- **Option 1: SO2 and Cl2**:
- These gases can react to form sulfuryl chloride (SO2Cl2). Therefore, they are not non-reacting gases.
- **Option 2: CO2 and N2**:
- These gases do not react with each other under normal conditions. Hence, they can be considered non-reacting.
- **Option 3: CO and N2**:
- Similar to CO2 and N2, CO and N2 do not react under normal conditions, so they can also be considered non-reacting.

4. **Conclusion**:
- Since SO2 and Cl2 can react with each other, the mixture of SO2 and Cl2 is not applicable for Dalton’s law of partial pressure. The other mixtures (CO2 and N2, CO and N2) are applicable as they consist of non-reacting gases.

### Final Answer:
The gas mixture that is not applicable for Dalton’s law of partial pressure is **SO2 and Cl2**.