Liquids A and B form ideal solution for all compositions of 𝐀 and 𝐁 at 25^∘ C. Two such solution

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Liquids A and B form ideal solution for all compositions of...

Liquids A and B form ideal solution for all compositions of $\mathbf{A}$ and $\mathbf{B}$ at $25^{\circ} \mathrm{C}$. Two such solutions with $0.25$ and $0.50$ mole fractions of $\mathbf{A}$ have the total vapor pressures of $0.3$ and $0.4$ bar, respectively. What is the vapor pressure of pure liquid $\mathbf{B}$ in bar?

Key Concepts

Ideal Solution

An ideal solution is one in which the intermolecular interactions are similar among all species, meaning that the enthalpy of mixing is zero and the solution obeys Raoult’s law. This assumption greatly simplifies the analysis of vapor-liquid equilibria since each component’s behavior in the mixture is a linear function of its concentration.

Raoult's Law

Raoult's law states that the partial vapor pressure of a component in an ideal solution is equal to the vapor pressure of the pure component multiplied by its mole fraction in the solution. This linear relationship is key in predicting how the vapor pressure of each component contributes to the overall vapor pressure of the mixture.

Mole Fraction

The mole fraction is a way of expressing the composition of a solution, defined as the number of moles of a particular component divided by the total number of moles of all components in the solution. It is a dimensionless quantity that is critical in applying Raoult’s law and in calculating partial pressure contributions.

Vapor Pressure

Vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid (or solid) form. In the context of solutions, knowing the vapor pressures of the pure components is essential for understanding and predicting the behavior of the solution's overall vapor pressure according to the composition.

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