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Chapter 13: Problem 124

An ideal liquid solution has two volatile components. In the vapor in equilibrium with the solution, the mole fractions of the components are (a) both \(0.50 ;\) (b) equal, but not necessarily \(0.50 ;\) (c) not very likely to be equal; (d) 1.00 for the solvent and 0.00 for the solute.

Short Answer

Expert verified
For case (a) and (b), the components have same volatilities but may not have equal molar quantities. For case (c), the components have different volatilities and hence different mole fractions in the vapor phase. In case (d), only the solvent is volatile and contributes to the total vapor pressure, while the solute does not.

Step by step solution

01

Case (a)

In this case, both components are said to be equally represented in the vapor phase with a mole fraction of 0.5. This means that both components are equally volatile and will have the same contribution to the total vapor pressure according to Dalton's law.
02

Case (b)

Here, the mole fractions of the components are equal, but not necessarily 0.5. This indicates that while the components might not have equal molar quantities, they contribute equally to the vapor pressure due to their identical volatilities.
03

Case (c)

This scenario refers to a case where it's likely that the mole fractions of the components are not equal. This would occur if the volatilities of the components differ significantly. The more volatile component will have a larger mole fraction in the vapor phase.
04

Case (d)

In the last case, the mole fraction of the solvent is 1.00, and the mole fraction of the solute is 0.00 in the vapor phase. In this scenario, only the solvent is volatile and so the total vapor pressure is due to the solvent alone. The solute does not contribute because it is not volatile.

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Most popular questions from this chapter

The concentration of Ar in the ocean at \(25^{\circ} \mathrm{C}\) is \(11.5 \mu \mathrm{M} .\) The Henry's law constant for \(\mathrm{Ar}\) is \(1.5 \times 10^{-3}\) \(\mathrm{mol} \mathrm{L}^{-1} \mathrm{atm}^{-1} .\) Calculate the mass of \(\mathrm{Ar}\) in a liter of ocean water. Calculate the partial pressure of \(\mathrm{Ar}\) in the atmosphere.

At \(25^{\circ} \mathrm{C}\) and under an \(\mathrm{O}_{2}(\mathrm{g})\) pressure of \(1 \mathrm{atm},\) the solubility of \(\mathrm{O}_{2}(\mathrm{g})\) in water is \(28.31 \mathrm{mL} / 1.00 \mathrm{L} \mathrm{H}_{2} \mathrm{O}\) At \(25^{\circ} \mathrm{C}\) and under an \(\mathrm{N}_{2}(\mathrm{g})\) pressure of \(1 \mathrm{atm},\) the solubility of \(\mathrm{N}_{2}(\mathrm{g})\) in water is \(14.34 \mathrm{mL} / 1.00 \mathrm{L} \mathrm{H}_{2} \mathrm{O}\) The composition of the atmosphere is \(78.08 \% \mathrm{N}_{2}\) and \(20.95 \% \mathrm{O}_{2},\) by volume. What is the composition of air dissolved in water expressed as volume percents of \(\mathrm{N}_{2}\) and \(\mathrm{O}_{2} ?\)

A solution contains \(750 \mathrm{g}\) of ethanol and \(85.0 \mathrm{g}\) of sucrose \(\left(180 \mathrm{g} \mathrm{mol}^{-1}\right) .\) The volume of the solution is \(810.0 \mathrm{mL} .\) Determine (a) the density of the solution (b) the percent of sucrose in the solution (c) the mole fraction of sucrose (d) the molality of the solution (e) the molarity of the solution

Two of the substances listed here are highly soluble in water, two are only slightly soluble in water, and two are insoluble in water. Indicate the situation you expect for each one. (a) iodoform, \(\mathrm{CHI}_{3}\) (b) benzoic acid, (c) formic acid, (d) 1-butanol, (e) chlorobenzene, (f) propylene glycol, \(\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{2} \mathrm{OH}\)

Calculate the mole fraction of solute in the following aqueous solutions: (a) \(21.7 \% \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH},\) by mass; (b) \(0.684 m \mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2}\) (urea).
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