In a binary solution of A and B, if the vapor pressure of pure A is 80 mmHg and pure B is 40 mmHg, what is the vapor pressure of the solution if the mole fraction of A is 0.6?
Practice Questions
1 question
Q1
In a binary solution of A and B, if the vapor pressure of pure A is 80 mmHg and pure B is 40 mmHg, what is the vapor pressure of the solution if the mole fraction of A is 0.6?
64 mmHg
72 mmHg
80 mmHg
56 mmHg
Using Raoult's Law, the vapor pressure of the solution = (0.6 * 80 mmHg) + (0.4 * 40 mmHg) = 64 mmHg.
Questions & Step-by-step Solutions
1 item
Q
Q: In a binary solution of A and B, if the vapor pressure of pure A is 80 mmHg and pure B is 40 mmHg, what is the vapor pressure of the solution if the mole fraction of A is 0.6?
Solution: Using Raoult's Law, the vapor pressure of the solution = (0.6 * 80 mmHg) + (0.4 * 40 mmHg) = 64 mmHg.
Steps: 8
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 must equal 1, mole fraction of B = 1 - 0.6 = 0.4.
Step 5: Apply Raoult's Law to find the vapor pressure of the solution. This is done by multiplying the mole fraction of each component by its respective vapor pressure.
Step 6: Calculate the contribution of A to the vapor pressure: 0.6 (mole fraction of A) * 80 mmHg (vapor pressure of pure A) = 48 mmHg.
Step 7: Calculate the contribution of B to the vapor pressure: 0.4 (mole fraction of B) * 40 mmHg (vapor pressure of pure B) = 16 mmHg.
Step 8: Add the contributions from A and B to get the total vapor pressure of the solution: 48 mmHg + 16 mmHg = 64 mmHg.
