What is the vapor pressure of a solution containing 2 moles of solute and 4 mole

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Question: What is the vapor pressure of a solution containing 2 moles of solute and 4 moles of solvent compared to pure solvent? (2022)

Options:

Correct Answer: 1/2

Exam Year: 2022

Solution:

Vapor pressure lowering = (moles of solute / total moles) = 2 / (2 + 4) = 2/6 = 1/3. Thus, vapor pressure is 1/2 of pure solvent.

What is the vapor pressure of a solution containing 2 moles of solute and 4 moles of solvent compared to pure solvent? (2022)

What is the vapor pressure of a solution containing 2 moles of solute and 4 moles of solvent compared to pure solvent? (2022)

Step 1: Identify the number of moles of solute and solvent. Here, we have 2 moles of solute and 4 moles of solvent.
Step 2: Calculate the total number of moles in the solution. Total moles = moles of solute + moles of solvent = 2 + 4 = 6 moles.
Step 3: Calculate the fraction of moles of solute compared to the total moles. This is done by dividing the moles of solute by the total moles: 2 moles of solute / 6 total moles = 1/3.
Step 4: Understand that the vapor pressure lowering is equal to the fraction of solute. This means the vapor pressure of the solution is lowered by 1/3 compared to the pure solvent.
Step 5: Since the vapor pressure of the pure solvent is considered 1 (or 100%), we can find the vapor pressure of the solution by subtracting the lowering: 1 - 1/3 = 2/3.
Step 6: Conclude that the vapor pressure of the solution is 2/3 of the vapor pressure of the pure solvent.

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