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Chapter 12: Problem 90

At \(-35^{\circ} \mathrm{C}\), liquid HI has a higher vapor pressure than liquid HF. Explain.

Short Answer

Expert verified
Liquid hydrogen iodide (HI) has a higher vapor pressure than liquid hydrogen fluoride (HF) at -35\(°C\) because the intermolecular forces in HI (London dispersion forces) are weaker than those in HF (hydrogen bonds), making it easier for HI molecules to escape to the gas phase.

Step by step solution

01

Understanding Vapor Pressure

Vapor pressure is the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases at a given temperature. It is a measure of the tendency of molecules and atoms to escape from a liquid or solid.
02

Intermolecular Forces and Vapor Pressure

The strength of intermolecular forces in a substance influences its vapor pressure. Weaker intermolecular forces typically lead to a higher vapor pressure, since the molecules have less attraction to each other and more can escape into the gas phase.
03

Characteristics of HI and HF

In the case of HI, it forms London dispersion forces which are weaker than the hydrogen bonds formed by HF. Therefore, it is easier for HI molecules to break free from each other and become gas, hence leading to a higher vapor pressure.

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Most popular questions from this chapter

The liquid-vapor boundary line in the phase diagram of any substance always stops abruptly at a certain point. Why?

A solid contains \(X, Y,\) and \(Z\) atoms in a cubic lattice with \(X\) atoms in the corners, \(Y\) atoms in the bodycentered positions, and \(Z\) atoms on the faces of the cell. What is the empirical formula of the compound?

The vapor pressure of liquid \(X\) is lower than that of liquid \(Y\) at \(20^{\circ} \mathrm{C}\), but higher at \(60^{\circ} \mathrm{C}\). What can you deduce about the relative magnitude of the molar heats of vaporization of \(X\) and \(Y ?\)

The compounds \(\mathrm{Br}_{2}\) and \(\mathrm{ICl}\) have the same number of electrons, yet \(\mathrm{Br}_{2}\) melts at \(-7.2^{\circ} \mathrm{C}\), whereas \(\mathrm{ICl}\) melts at \(27.2^{\circ} \mathrm{C}\). Explain.

Which of these species are capable of hydrogen bonding among themselves: (a) \(\mathrm{C}_{2} \mathrm{H}_{6},\) (b) \(\mathrm{HI},(\mathrm{c}) \mathrm{KF}\) (d) \(\mathrm{BeH}_{2},\) (e) \(\mathrm{CH}_{3} \mathrm{COOH} ?\)
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