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Chapter 11: Problem 64

What can we learn about the intermolecular forces in a liquid from the molar heat of vaporization?

Short Answer

Expert verified
The molar heat of vaporization can tell us about the strength of intermolecular forces in a liquid. A high molar heat of vaporization indicates strong intermolecular forces, while a low molar heat of vaporization suggests weak intermolecular forces.

Step by step solution

01

Understanding Intermolecular Forces

Intermolecular forces are the forces of attraction between molecules. They are generally weaker than ionic or covalent bonds. However, they are significant when considering phenomena like vaporization, condensation, and melting. The stronger the intermolecular forces in a substance, the more attraction between molecules, and thus, more energy, in the form of heat, is required to overcome these forces.
02

Understanding Molar Heat of Vaporization

The molar heat of vaporization is the amount of heat required to convert one mole of a liquid at its boiling point into vapour without any change in temperature, at a constant pressure. It's an indicator of the strength of intermolecular forces, since greater energy is needed to break stronger forces.
03

Connect the Concepts

In relation to intermolecular forces, a high molar heat of vaporization signals strong intermolecular forces. This is because strong intermolecular forces hold molecules tightly in liquid form, requiring more energy to break these forces and convert the liquid to a gas. Conversely, a lower molar heat of vaporization indicates weaker intermolecular forces.

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Most popular questions from this chapter

Crystalline silicon has a cubic structure. The unit cell edge length is \(543 \mathrm{pm}\). The density of the solid is \(2.33 \mathrm{~g} / \mathrm{cm}^{3}\). Calculate the number of Si atoms in one unit cell.

Select the substance in each pair that should have the higher boiling point. In each case identify the principal intermolecular forces involved and account briefly for your choice. (a) \(\mathrm{K}_{2} \mathrm{~S}\) or \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{~N},\) (b) \(\mathrm{Br}_{2}\) or \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3}\)

Use the concept of intermolecular forces to explain why the far end of a walking cane rises when one raises the handle.

Argon crystallizes in the face-centered cubic arrangement at \(40 \mathrm{~K}\). Given that the atomic radius of argon is \(191 \mathrm{pm}\), calculate the density of solid argon.

The fluorides of the second-period elements and their melting points are: \(\mathrm{LiF}, 845^{\circ} \mathrm{C} ; \mathrm{BeF}_{2}\), \(800^{\circ} \mathrm{C} ; \mathrm{BF}_{3},-126.7^{\circ} \mathrm{C} ; \mathrm{CF}_{4},-184^{\circ} \mathrm{C} ; \mathrm{NF}_{3}\) \(-206.6^{\circ} \mathrm{C} ; \quad \mathrm{OF}_{2},-223.8^{\circ} \mathrm{C} ; \quad \mathrm{F}_{2},-219.6^{\circ} \mathrm{C}\) Classify the type(s) of intermolecular forces present in each compound.
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