In a binary solution of A and B, if the vapor pressure of pure A is 150 mmHg and pure B is 50 mmHg, what is the total vapor pressure when the mole fraction of A is 0.4?

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90 mmHg
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Q: In a binary solution of A and B, if the vapor pressure of pure A is 150 mmHg and pure B is 50 mmHg, what is the total vapor pressure when the mole fraction of A is 0.4?

Solution: Total vapor pressure = (X_A * P_A^0) + (X_B * P_B^0) = (0.4 * 150) + (0.6 * 50) = 60 + 30 = 90 mmHg.

Steps: 8

Step 1: Identify the given values. The vapor pressure of pure A (P_A^0) is 150 mmHg, and the vapor pressure of pure B (P_B^0) is 50 mmHg.
Step 2: Determine the mole fraction of A (X_A), which is given as 0.4.
Step 3: Calculate the mole fraction of B (X_B). Since the total mole fraction must equal 1, X_B = 1 - X_A = 1 - 0.4 = 0.6.
Step 4: Use the formula for total vapor pressure: Total vapor pressure = (X_A * P_A^0) + (X_B * P_B^0).
Step 5: Substitute the values into the formula: Total vapor pressure = (0.4 * 150) + (0.6 * 50).
Step 6: Calculate (0.4 * 150) = 60 mmHg and (0.6 * 50) = 30 mmHg.
Step 7: Add the two results together: 60 mmHg + 30 mmHg = 90 mmHg.
Step 8: The total vapor pressure of the solution is 90 mmHg.

In a binary solution of A and B, if the vapor pressure of pure A is 150 mmHg and pure B is 50 mmHg, what is the total vapor pressure when the mole fraction of A is 0.4?

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