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Chapter 12: Problem 63

What is the relationship between intermolecular forces in a liquid and the liquid's boiling point and critical temperature? Why is the critical temperature of water greater than that of most other substances?

Short Answer

Expert verified
The relationship is that the stronger the intermolecular forces within a liquid, the higher its boiling point and critical temperature will be. Water's critical temperature is greater than most other substances due to its ability to form strong hydrogen bonds, which are a type of intermolecular force.

Step by step solution

01

Understanding intermolecular forces

Intermolecular forces are the forces of attraction between molecules. They dictate many of a substance's physical properties, including its phase at different temperatures and pressures. The primary types of intermolecular forces are London dispersion forces, dipole-dipole interactions, and hydrogen bonds.
02

Relation to boiling point and critical temperature

The boiling point of a substance, the temperature at which it transitions from a liquid to a gas, is directly influenced by its intermolecular forces. A higher boiling point indicates stronger intermolecular forces, as more energy is needed to overcome them. Similarly, the critical temperature, the highest temperature at which a substance can exist as a liquid, regardless of the pressure, is also directly related to intermolecular forces: the stronger the forces, the higher the critical temperature.
03

Understanding water's unique properties

Water has a higher critical temperature than most other substances due to its ability to form hydrogen bonds, which are stronger than the London dispersion forces and dipole-dipole interactions typical in many other substances. Each water molecule can form up to four of these bonds, resulting in a complex,
04

Conclusion

Therefore, it's fair to conclude that the intermolecular forces in a substance greatly determine its boiling point and critical temperature. The stronger these forces (as with water and its capability to form powerful hydrogen bonds), the higher these temperatures will be. This is why water has a higher critical temperature compared to many other substances.

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Most popular questions from this chapter

Vapor pressure measurements at several different temperatures are shown here for mercury. Determine graphically the molar heat of vaporization for mercury. \(\begin{array}{cccccc}t\left({ }^{\circ} \mathrm{C}\right) & 200 & 250 & 300 & 320 & 340 \\ P(\mathrm{mmHg}) & 17.3 & 74.4 & 246.8 & 376.3 & 557.9\end{array}\)

What kind of attractive forces must be overcome to (a) melt ice, (b) boil molecular bromine, (c) melt solid iodine, and (d) dissociate \(\mathrm{F}_{2}\) into \(\mathrm{F}\) atoms?

Name the kinds of attractive forces that must be overcome to (a) boil liquid ammonia, (b) melt solid phosphorus \(\left(\mathrm{P}_{4}\right),\) (c) dissolve CsI in liquid \(\mathrm{HF},\) (d) melt potassium metal.

Use water and mercury as examples to explain adhesion and cohesion.

A solid is soft and has a low melting point (below \(100^{\circ} \mathrm{C}\) ). The solid, its melt, and a solution containing the substance are all nonconductors of electricity. Classify the solid.
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