Use the result of the previous problem to calculate the mole fraction of chloroform in the vapor above a solution obtained by three successive separations and condensations of the vapors above the original solution of carbon tetrachloride and chloroform. Show how this result explains the use of distillation as a separation method.

Verified step by step guidance

1. <insert step 1: Understand the concept of mole fraction and how it applies to vapor-liquid equilibrium. Mole fraction is the ratio of the number of moles of a component to the total number of moles in the mixture.>
2. <insert step 2: Recall Raoult's Law, which states that the partial vapor pressure of a component in a solution is equal to the mole fraction of the component in the liquid phase multiplied by the vapor pressure of the pure component.>
3. <insert step 3: Use the result from the previous problem to determine the initial mole fraction of chloroform in the vapor above the original solution. This will be your starting point for the first separation.>
4. <insert step 4: For each successive separation and condensation, apply Raoult's Law to calculate the new mole fraction of chloroform in the vapor. This involves using the mole fraction from the previous step as the new starting point.>
5. <insert step 5: Explain how the process of distillation, which involves repeated vaporization and condensation, increases the concentration of the more volatile component (chloroform) in the vapor phase, thus allowing for separation based on differences in volatility.>