Raoult's Law
An ideal binary liquid solution is prepared by mixing 3 mol of liquid A (vapour pressure 100 mmHg) with 2 mol of liquid B (vapour pressure 150 mmHg) at a given temperature. The total vapour pressure of the solution is:
Select the correct option:
Solution
120 mmHg
For an ideal solution, Raoult's law applies: P_total = x_A·P°_A + x_B·P°_B. Mole fractions: x_A = 3/(3+2) = 0.6 and x_B = 2/(3+2) = 0.4. Therefore, P_total = (0.6 × 100) + (0.4 × 150) = 60 + 60 = 120 mmHg. The total vapour pressure is the sum of partial pressures of each component weighted by their mole fractions in the liquid phase. This is a direct application of Raoult's law for ideal solutions where no significant intermolecular interactions differ from pure components.
🔒 Solution Hidden from View
Submit your answer to unlock the detailed step-by-step solution.
More raoult's law Practice Questions
About This Question
- Subject
- chemistry
- Chapter
- solutions
- Topic
- raoult's law
- Difficulty
- Easy
- Year
- 2025
Solution
Correct Answer:
120 mmHg
For an ideal solution, Raoult's law applies: P_total = x_A·P°_A + x_B·P°_B. Mole fractions: x_A = 3/(3+2) = 0.6 and x_B = 2/(3+2) = 0.4. Therefore, P_total = (0.6 × 100) + (0.4 × 150) = 60 + 60 = 120 mmHg. The total vapour pressure is the sum of partial pressures of each component weighted by their mole fractions in the liquid phase. This is a direct application of Raoult's law for ideal solutions where no significant intermolecular interactions differ from pure components.
This easy difficulty chemistry question is from the chapter solutions, covering the topic of raoult's law. It appeared in the 2025 exam.
Looking for more practice? Explore all chemistry questions or browse solutions questions on RankGuru.