Question

A solution contains 4.08 g of chloroform (CHCl3) and 9.29 g of acetone (CH3COCH3). The vapor pressures at 35 ∘C of pure chloroform and pure acetone are 295 torr and 332 torr, respectively. Assuming ideal behavior, calculate the vapor pressures of each of the components and the total vapor pressure above the solution.

Answer 1

Explanation:

Below is an attachment containing the solution.

Answer 2

Answer:

Vp chloroform  = 51.92 torr

Vp acetone = 273.57torr

total Vp = 325.49torr

Explanation:

Step 1: Data given

Mass of chloroform = 4.08 grams

Mass of acetone = 9.29 grams

The vapor pressure at 35 °C of chloroform = 295 torr

The vapor pressure at 35 °C of acetone = 332 torr

Step 2: Calculate moles

Pressure of solution = Pressure solvent * mole fraction

mole fraction = moles solvent / total moles

Moles chloroform = mass chloroform / molar mass chloroform

Moles chloroform = 4.08 grams / 119.5g/mole = 0.0341moles  

Moles acetone = 9.29 grams  / 58g/mole = 0.160 moles

Step 3: Calculate mol fractions

Mol fraction chloroform = 0.0341 moles / (0.0341+0.160)moles

Mol fraction chloroform = 0.176

Mol fraction acetone = 0.160 /(0.0341+0.160)

Mol fraction acetone = 0.824

Step 4: Calculate vapor pressure

Vp = pressure  * mole fraction

Vp chloroform  = 295torr * 0.176 = 51.92 torr

Vp acetone = 332 torr * 0.824 = 273.57torr

total Vp = 325.49torr