If two liquids `A(P_(A)^(@)=100` torr) and `B(P_(B)^(@)=200` torr) are completely immiscible with each other, each one will behave independently of the other, are present in a closed vessel. The total vapour pressure of the system will be:

Options

A. less than `100` torr
B. greater than `200` torr
C. between `100` to `200` torr
D. `300` torr

Answer

To solve the problem of calculating the total vapor pressure of two immiscible liquids A and B in a closed vessel, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Given Data**:
- Vapor pressure of liquid A, \( P_{A}^{(@)} = 100 \) torr
- Vapor pressure of liquid B, \( P_{B}^{(@)} = 200 \) torr

2. **Understand the Concept of Immiscible Liquids**:
- Immiscible liquids do not mix and each liquid exerts its own vapor pressure independently in the closed system.

3. **Apply Raoult's Law for Total Vapor Pressure**:
- According to Raoult's Law, the total vapor pressure \( P_{total} \) for a system of two immiscible liquids is the sum of the vapor pressures of the individual liquids:
\[ P_{total} = P_{A}^{(@)} + P_{B}^{(@)} \]

4. **Substitute the Values**:
- Substitute the given vapor pressures into the equation:
\[ P_{total} = 100 \, \text{torr} + 200 \, \text{torr} \]

5. **Calculate the Total Vapor Pressure**:
- Perform the addition:
\[ P_{total} = 300 \, \text{torr} \]

6. **Conclusion**:
- The total vapor pressure of the system is \( 300 \) torr.

### Final Answer:
The total vapor pressure of the system is \( 300 \) torr.

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