If the vapor pressure of pure solvent is 120 mmHg, what will be the vapor pressu

If the vapor pressure of pure solvent is 120 mmHg, what will be the vapor pressure of a solution containing 0.2 moles of solute in 1 mole of solvent?

If the vapor pressure of pure solvent is 120 mmHg, what will be the vapor pressure of a solution containing 0.2 moles of solute in 1 mole of solvent?

Step 1: Identify the vapor pressure of the pure solvent, which is given as 120 mmHg.
Step 2: Determine the number of moles of solute and solvent. We have 0.2 moles of solute and 1 mole of solvent.
Step 3: Calculate the total number of moles in the solution. This is the sum of moles of solute and moles of solvent: 0.2 + 1 = 1.2 moles.
Step 4: Calculate the mole fraction of the solvent (X_solvent). This is the moles of solvent divided by the total moles: X_solvent = 1 / 1.2.
Step 5: Calculate the vapor pressure of the solution using Raoult's Law: P_solution = P_solvent * X_solvent.
Step 6: Substitute the values into the equation: P_solution = 120 mmHg * (1 / 1.2).
Step 7: Perform the calculation: P_solution = 120 mmHg * 0.8333 = 100 mmHg.

Raoult's Law – Raoult's Law states that the vapor pressure of a solvent in a solution is equal to the vapor pressure of the pure solvent multiplied by the mole fraction of the solvent in the solution.
Mole Fraction – The mole fraction is the ratio of the number of moles of a component to the total number of moles of all components in the solution.