Chapter 13, Problem 13.113P

Interpretation Introduction

Interpretation:

The partial pressures of ${\text{CH}}_2{\text{Cl}}_2$ and ${\text{CCl}}_4$ are to be calculated.

Concept introduction:

Raoult’s law is a chemical law which states the relationship between vapor pressure and the mole fraction of the solute. It states that the partial pressure of each component of an ideal mixture is calculated by the multiplication of the vapor pressure of the pure component and its mole fraction in the mixture. It is not valid for a volatile solute.

According to Raoult’s law, the vapor pressure of the solvent is given as follows:

$P_{\text{solvent}}=X_{\text{solvent}}{P}_{\text{solvent}}^{°}$        (1)

Here,

$P_{\text{solvent}}$ is the vapor pressure of the solvent.

$X_{\text{solvent}}$ is the mole fraction of the solvent.

$P_{\text{solvent}}^{°}$ is the vapor pressure of the pure solvent.

The formula to calculate the mole fraction is as follows:

$\text{Mole}\text{fraction}\left(X\right)=\frac{\text{amount}\left(\text{mol}\right)\text{of}\text{component 1}}{\left(\begin{array}{l}\text{amount}\left(\text{mol}\right)\text{of}\text{component 1}+\\ \text{amount}\left(\text{mol}\right)\text{of}\text{component 2}\end{array}\right)}$        (2)