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Chapter 11: Problem 12

At room temperature, \(\mathrm{CO}_{2}\) is a gas, \(\mathrm{CCl}_{4}\) is a liquid, and \(\mathrm{C}_{60}\) (fullerene) is a solid. List these substances in order of (a) increasing intermolecular energy of attraction and (b) increasing boiling point.

Short Answer

Expert verified
In terms of (a) increasing intermolecular energy of attraction and (b) increasing boiling point, the order is CO₂ < CCl₄ < C₆₀. CO₂ has the weakest London dispersion forces, followed by CCl₄, and C₆₀ with the strongest London dispersion forces. Consequently, CO₂ has the lowest boiling point, followed by CCl₄, and C₆₀ with the highest boiling point.

Step by step solution

01

CO₂ < CCl₄ < C₆₀

In terms of increasing intermolecular energy of attraction, it will be CO₂ (with the weakest London dispersion forces), followed by CCl₄, and finally C₆₀ (with the strongest London dispersion forces). #b. Increasing Boiling Point # The boiling point of a substance is directly related to its intermolecular forces. Stronger intermolecular forces lead to higher boiling points because more energy is needed to break the bonds between the molecules.
02

CO₂ < CCl₄ < C₆₀

As CO₂ has the weakest intermolecular forces, it will have the lowest boiling point, followed by CCl₄, and then C₆₀ (with the strongest intermolecular forces) will have the highest boiling point.

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Most popular questions from this chapter

Freon, \(\mathrm{CCl}_{2} \mathrm{~F}_{2},\) and dichloromethane, \(\mathrm{CH}_{2} \mathrm{Cl}_{2},\) are common organic substances. Freon is a gas with a normal boiling point of \(-29.8^{\circ} \mathrm{C}\); dichloromethane's normal boiling point is \(39.6^{\circ} \mathrm{C}\). Which statement is the best explanation of these data? (a) Dichloromethane can form hydrogen bonds, but freon cannot. (b) Dichloromethane has a larger dipole moment than freon. (c) Freon is more polarizable than dichloromethane.

You are high up in the mountains and boil water to make some tea. However, when you drink your tea, it is not as hot as it should be. You try again and again, but the water is just not hot enough to make a hot cup of tea. Which is the best explanation for this result? (a) High in the mountains, it is probably very dry, and so the water is rapidly evaporating from your cup and cooling it. (b) High in the mountains, it is probably very windy, and so the water is rapidly evaporating from your cup and cooling it. (c) High in the mountains, the air pressure is significantly less than \(101.3 \mathrm{kPa}\), so the boiling point of water is much lower than at sea level. (d) High in the mountains, the air pressure is significantly less than \(101.3 \mathrm{kPa}\), so the boiling point of water is much higher than at sea level.

The smectic liquid crystalline phase can be said to be more highly ordered than the nematic phase. In what sense is this true?

Which member in each pair has the greater dispersion forces? (a) \(\mathrm{CH}_{3} \mathrm{OH}\) or $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH},\( (b) \)\mathrm{NH}_{3}$ or \(\mathrm{N}\left(\mathrm{CH}_{3}\right)_{3}\), (c) $\mathrm{CH}_{2} \mathrm{Cl}_{2}\( or \)\mathrm{CH}_{2} \mathrm{Br}_{2}$

Referring to Figure 11.28 , describe all the phase changes that would occur in each of the following cases: (a) Water vapor originally at \(500 \mathrm{~Pa}\) and \(-0.5^{\circ} \mathrm{C}\) is slowly compressed at constant temperature until the final pressure is $2000 \mathrm{kPa}\(. (b) Water originally at \)100.0^{\circ} \mathrm{C}\( and \)50 \mathrm{kPa}$ is cooled at constant pressure until the temperature is \(-10^{\circ} \mathrm{C}\).
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