In a binary solution of A and B, if the vapor pressure of pure A is 80 mmHg and
Practice Questions
Q1
In a binary solution of A and B, if the vapor pressure of pure A is 80 mmHg and that of pure B is 40 mmHg, what is the total vapor pressure when the mole fraction of A is 0.6?
64 mmHg
72 mmHg
80 mmHg
88 mmHg
Questions & Step-by-Step Solutions
In a binary solution of A and B, if the vapor pressure of pure A is 80 mmHg and that of pure B is 40 mmHg, what is the total vapor pressure when the mole fraction of A is 0.6?
Step 1: Identify the vapor pressure of pure A, which is 80 mmHg.
Step 2: Identify the vapor pressure of pure B, which is 40 mmHg.
Step 3: Determine the mole fraction of A, which is given as 0.6.
Step 4: Calculate the mole fraction of B. Since the total mole fraction must equal 1, the mole fraction of B is 1 - 0.6 = 0.4.
Step 5: Use Raoult's Law to calculate the contribution to the total vapor pressure from A: 0.6 (mole fraction of A) * 80 mmHg (vapor pressure of pure A) = 48 mmHg.
Step 6: Calculate the contribution to the total vapor pressure from B: 0.4 (mole fraction of B) * 40 mmHg (vapor pressure of pure B) = 16 mmHg.
Step 7: Add the contributions from A and B to find the total vapor pressure: 48 mmHg + 16 mmHg = 64 mmHg.
