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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 that of pure B is 40 mmHg, what is the vapor pressure of the solution if the mole fraction of A is 0.6?

Options:

  1. 64 mmHg
  2. 72 mmHg
  3. 80 mmHg
  4. 56 mmHg

Correct Answer: 72 mmHg

Solution: 

Using Raoult\'s Law, the vapor pressure of the solution = (0.6 * 80 mmHg) + (0.4 * 40 mmHg) = 64 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 that of pure B is 40 mmHg, what is the vapor pressure of the solution if the mole fraction of A is 0.6?
  1. 64 mmHg
  2. 72 mmHg
  3. 80 mmHg
  4. 56 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 vapor pressure of the solution if 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 in the solution, which is given as 0.6.
  • Step 4: Calculate the mole fraction of B by subtracting the mole fraction of A from 1: 1 - 0.6 = 0.4.
  • Step 5: Use Raoult's Law to 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 6: 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 7: Add the contributions from A and B to find the total vapor pressure of the solution: 48 mmHg + 16 mmHg = 64 mmHg.
  • Raoult's Law – Raoult's Law states that the vapor pressure of a solution is equal to the sum of the partial pressures of each component, which can be calculated using the mole fraction of each component multiplied by its pure vapor pressure.
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