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Chapter 9: Problem 38

What are the strongest attractive forces that must be overcome to (a) melt ice? (b) sublime bromine? (c) boil chloroform (CHCl \(_{3}\) )? (d) vaporize benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) ?

Short Answer

Expert verified
Answer: a) For ice, the strongest attractive force is hydrogen bonding. b) For bromine, it is Van der Waals (London dispersion) forces. c) For chloroform, it is dipole-dipole interactions. d) For benzene, it is also Van der Waals (London dispersion) forces.

Step by step solution

01

Identify the molecule and its structure

Ice is a solid form of water (H2O), and its structure contains polar molecules held together by hydrogen bonding.
02

Determine the strongest attractive force that must be overcome

In the case of ice, the strongest attractive force that must be overcome is hydrogen bonding between the water molecules. #b) Sublime Bromine#
03

Identify the molecule and its structure

Bromine (Br2) is a non-polar diatomic molecule.
04

Determine the strongest attractive force that must be overcome

In the case of bromine, the strongest attractive force that must be overcome is the Van der Waals (London dispersion) forces between the non-polar bromine molecules. #c) Boil Chloroform (CHCl \(_{3}\) )#
05

Identify the molecule and its structure

Chloroform (CHCl\(_{3}\)) is a polar molecule with a central carbon atom bonded to one hydrogen and three chlorine atoms.
06

Determine the strongest attractive force that must be overcome

In the case of chloroform, the strongest attractive force that must be overcome is the dipole-dipole interaction between the polar chloroform molecules. #d) Vaporize Benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\)#
07

Identify the molecule and its structure

Benzene (C6H6) is an aromatic hydrocarbon with a planar hexagonal structure containing alternating single and double carbon bonds.
08

Determine the strongest attractive force that must be overcome

In the case of benzene, the strongest attractive force that must be overcome is the Van der Waals (London dispersion) forces between the non-polar benzene molecules.

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Most popular questions from this chapter

Which of the following would show hydrogen bonding? (a) \(\mathrm{CH}_{3} \mathrm{~F}\) (b) \(\mathrm{HO}-\mathrm{OH}\) (c) \(\mathrm{NH}_{3}\) (d) \(\mathrm{H}_{3} \mathrm{C}-\mathrm{O}-\mathrm{CH}_{3}\)

Describe the structural units in (a) NaI (b) \(\mathrm{N}_{2}\) (c) \(\mathrm{KO}_{2}\) (d) \(\mathrm{Au}\)

Explain in terms of forces between structural units why (a) HI has a higher boiling point than \(\mathrm{HBr}\). (b) \(\mathrm{GeH}_{4}\) has a higher boiling point than \(\mathrm{SiH}_{4}\). (c) \(\mathrm{H}_{2} \mathrm{O}_{2}\) has a higher melting point than \(\mathrm{C}_{3} \mathrm{H}_{8}\). (d) \(\mathrm{NaCl}\) has a higher boiling point than \(\mathrm{CH}_{3} \mathrm{OH}\).

Methyl alcohol, \(\mathrm{CH}_{3} \mathrm{OH}\), has a normal boiling point of \(64.7^{\circ} \mathrm{C}\) and has a vapor pressure of \(203 \mathrm{~mm} \mathrm{Hg}\) at \(35^{\circ} \mathrm{C}\). Estimate (a) its heat of vaporization \(\left(\Delta H_{\text {vap }}\right)\). (b) its vapor pressure at \(40.0^{\circ} \mathrm{C}\).

Benzene, a known carcinogen, was once widely used as a solvent. \(\mathrm{A}\) sample of benzene vapor in a flask of constant volume exerts a pressure of \(325 \mathrm{~mm} \mathrm{Hg}\) at \(80^{\circ} \mathrm{C}\). The flask is slowly cooled. (a) Assuming no condensation, use the ideal gas law to calculate the pressure of the vapor at \(50^{\circ} \mathrm{C} ;\) at \(60^{\circ} \mathrm{C}\). (b) Compare your answers in (a) to the equilibrium vapor pressures of benzene: \(269 \mathrm{~mm} \mathrm{Hg}\) at \(50^{\circ} \mathrm{C}, 389 \mathrm{~mm} \mathrm{Hg}\) at \(60^{\circ} \mathrm{C}\). (c) On the basis of your answers to (a) and (b), predict the pressure exerted by the benzene at \(50^{\circ} \mathrm{C} ;\) at \(60^{\circ} \mathrm{C}\).
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