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For a solution containing 2 components A and B, if the mole fraction of A is 0.6

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Question: For a solution containing 2 components A and B, if the mole fraction of A is 0.6, what is the vapor pressure of the solution if the vapor pressure of pure A is 100 mmHg?

Options:

  1. 60 mmHg
  2. 100 mmHg
  3. 40 mmHg
  4. 80 mmHg

Correct Answer: 80 mmHg

Solution: 

According to Raoult\'s Law, the vapor pressure of the solution is P_A = X_A * P_A^0 = 0.6 * 100 mmHg = 60 mmHg.

For a solution containing 2 components A and B, if the mole fraction of A is 0.6

Practice Questions

Q1
For a solution containing 2 components A and B, if the mole fraction of A is 0.6, what is the vapor pressure of the solution if the vapor pressure of pure A is 100 mmHg?
  1. 60 mmHg
  2. 100 mmHg
  3. 40 mmHg
  4. 80 mmHg

Questions & Step-by-Step Solutions

For a solution containing 2 components A and B, if the mole fraction of A is 0.6, what is the vapor pressure of the solution if the vapor pressure of pure A is 100 mmHg?
  • Step 1: Understand that the mole fraction of A (X_A) is given as 0.6.
  • Step 2: Know that the vapor pressure of pure A (P_A^0) is given as 100 mmHg.
  • Step 3: Recall Raoult's Law, which states that the vapor pressure of the solution (P_A) is equal to the mole fraction of A (X_A) multiplied by the vapor pressure of pure A (P_A^0).
  • Step 4: Substitute the values into the formula: P_A = X_A * P_A^0.
  • Step 5: Calculate P_A by multiplying 0.6 (X_A) by 100 mmHg (P_A^0).
  • Step 6: The result is P_A = 0.6 * 100 mmHg = 60 mmHg.
  • Raoult's Law – Raoult's Law states that the vapor pressure of a solution is equal to the mole fraction of the solvent multiplied by the vapor pressure of the pure solvent.
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