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In a binary solution of A and B, if the vapor pressure of pure A is 80 mmHg and

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Question: 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 total vapor pressure when the mole fraction of A is 0.5?

Options:

  1. 60 mmHg
  2. 70 mmHg
  3. 80 mmHg
  4. 50 mmHg

Correct Answer: 70 mmHg

Solution:

Total vapor pressure = P_A + P_B = (0.5 * 80) + (0.5 * 40) = 40 + 20 = 60 mmHg.

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 pure B is 40 mmHg, what is the total vapor pressure when the mole fraction of A is 0.5?
  1. 60 mmHg
  2. 70 mmHg
  3. 80 mmHg
  4. 50 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 pure B is 40 mmHg, what is the total vapor pressure when the mole fraction of A is 0.5?
  • 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 0.5.
  • Step 4: Calculate the contribution to the vapor pressure from A using the formula: P_A = mole fraction of A * vapor pressure of pure A. So, P_A = 0.5 * 80 = 40 mmHg.
  • Step 5: Calculate the contribution to the vapor pressure from B using the formula: P_B = mole fraction of B * vapor pressure of pure B. Since the mole fraction of B is 1 - mole fraction of A, it is 1 - 0.5 = 0.5. So, P_B = 0.5 * 40 = 20 mmHg.
  • Step 6: Add the contributions from A and B to find the total vapor pressure: Total vapor pressure = P_A + P_B = 40 mmHg + 20 mmHg = 60 mmHg.
  • Raoult's Law – The total vapor pressure of a solution is the sum of the partial pressures of each component, which can be calculated using the mole fraction and the vapor pressure of the pure components.
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