At 35 ° C the vapor pressure of pure chloroform is 0.359 atm and that of pure acetone is 0.453 atm. Assuming ideal behavior, a solution containing 1 mole of chloroform and 4 moles of acetone has a total vapor pressure of:

Question

Quizplus · Accepted Answer

First, we need to calculate the mole fraction of each component:

Mole fraction of chloroform = 1 / (1+4) = 0.20
Mole fraction of acetone = 4 / (1+4) = 0.80

Next, we can use Raoult's law to find the partial pressure of each component:

Partial pressure of chloroform = mole fraction of chloroform * vapor pressure of chloroform = 0.20 * 0.359 atm = 0.0718 atm
Partial pressure of acetone = mole fraction of acetone * vapor pressure of acetone = 0.80 * 0.453 atm = 0.3624 atm

Finally, we can find the total vapor pressure by adding the partial pressures:

Total vapor pressure = partial pressure of chloroform + partial pressure of acetone = 0.0718 atm + 0.3624 atm = 0.434 atm

Therefore, the best choice is D.

At 35 ° C the Vapor Pressure of Pure Chloroform