# Problem: A solution contains 4.08 g of chloroform (CHCl3 ) and 9.29 g of acetone (CH3 COCH3 ). The vapor pressures at 35 oC of pure chloroform and pure acetone are 295 torr and 332 torr, respectively.Assuming ideal behavior, calculate the vapor pressure of acetone.

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###### FREE Expert Solution

We’re being asked to determine the partial pressure of acetone (CH3COCH3) in the solution

Recall that the vapor pressure of a solution can be given by Raoult’s Law.

$\overline{){{\mathbit{P}}}_{\mathbit{s}\mathbit{o}\mathbit{l}\mathbit{u}\mathbit{t}\mathbit{i}\mathbit{o}\mathbit{n}}{\mathbit{=}}\left(\mathbit{P}{\mathbit{°}}_{\mathbit{s}\mathbit{o}\mathbit{l}\mathbit{u}\mathbit{t}\mathbit{e}}{\mathbit{X}}_{\mathbit{s}\mathbit{o}\mathbit{l}\mathbit{u}\mathbit{t}\mathbit{e}}\right)\left(\mathbit{P}{\mathbit{°}}_{\mathbit{s}\mathbit{o}\mathbit{l}\mathbit{v}\mathbit{e}\mathbit{n}\mathbit{t}}{\mathbit{X}}_{\mathbit{s}\mathbit{o}\mathbit{l}\mathbit{v}\mathbit{e}\mathbit{n}\mathbit{t}}\right)}$

where:

P˚ = vapor pressure of pure component

χ = mole fraction of component.

Recall that mole Fraction (X) relates the moles of solute and solvent within a solution.

To solve this problem:

Step 1. Solve for the number of mole from grams of solute and solvent given.
Step 2. Find the mole fraction for acetone.
Step 3. Determine the partial pressure for acetone. ###### Problem Details

A solution contains 4.08 g of chloroform (CHCl3 ) and 9.29 g of acetone (CH3 COCH3 ). The vapor pressures at 35 oC of pure chloroform and pure acetone are 295 torr and 332 torr, respectively.

Assuming ideal behavior, calculate the vapor pressure of acetone.