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Chapter 11: Problem 52

True or false: (a) \(\mathrm{CBr}_{4}\) is more volatile than \(\mathrm{CCl}_{4} .(\mathbf{b}) \mathrm{CBr}_{4}\) has a higher boiling point than \(\mathrm{CCl}_{4}\) . (c) CBr. has weaker intermolecular forces than \(\mathrm{CCl}_{4}\) . (d) \(\mathrm{CBr}_{4}\) has a higher vapor pressure at the same temperature than \(\mathrm{CCl}_{4}\) .

Short Answer

Expert verified
(a) False, (b) True, (c) False, (d) False

Step by step solution

01

Statement (a): \(\mathrm{CBr}_{4}\) is more volatile than \(\mathrm{CCl}_{4}\).

Comparing the molecular weights of these two compounds, we find that \(\mathrm{CBr}_{4}\) has a higher molecular weight due to the heavier mass of the Br atoms. This leads to stronger London dispersion forces between the molecules, which are the primary intermolecular forces in these two compounds. Because \(\mathrm{CBr}_{4}\) has stronger intermolecular forces, it should be less volatile than \(\mathrm{CCl}_{4}\). Therefore, statement (a) is false. #b) Determine the boiling point#
02

Statement (b): \(\mathrm{CBr}_{4}\) has a higher boiling point than \(\mathrm{CCl}_{4}\).

As mentioned before, the heavier mass of the Br atoms in \(\mathrm{CBr}_{4}\) creates stronger London dispersion forces between the molecules. These stronger intermolecular forces require more energy to overcome, leading to a higher boiling point for \(\mathrm{CBr}_{4}\). Thus, statement (b) is true. #c) Determine the intermolecular forces#
03

Statement (c): \(\mathrm{CBr}_{4}\) has weaker intermolecular forces than \(\mathrm{CCl}_{4}\).

As discussed earlier, the higher molecular weight of \(\mathrm{CBr}_{4}\) causes it to have stronger London dispersion forces between the molecules compared to \(\mathrm{CCl}_{4}\). So, statement (c) is false. #d) Determine the vapor pressure#
04

Statement (d): \(\mathrm{CBr}_{4}\) has a higher vapor pressure at the same temperature than \(\mathrm{CCl}_{4}\).

Since we established earlier that \(\mathrm{CBr}_{4}\) is less volatile than \(\mathrm{CCl}_{4}\), it will have a lower vapor pressure at the same temperature. Thus, statement (d) is false. In summary: - Statement (a) is false - Statement (b) is true - Statement (c) is false - Statement (d) is false

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Most popular questions from this chapter

One of the attractive features of ionic liquids is their low vapor pressure, which in turn tends to make them nonflammable. Why do you think ionic liquids have lower vapor pressures than most room-temperature molecular liquids?

Rationalize the difference in boiling points in each pair: (a) HF \(\left(20^{\circ} \mathrm{C}\right)\) and \(\mathrm{HCl}\left(-85^{\circ} \mathrm{C}\right),\) (b) CHCl \(_{3}\left(61^{\circ} \mathrm{C}\right)\) and \(\mathrm{CHBr}_{3}\left(150^{\circ} \mathrm{C}\right),(\mathbf{c}) \mathrm{Br}_{2}\left(59^{\circ} \mathrm{C}\right)\) and \(\mathrm{ICl}\left(97^{\circ} \mathrm{C}\right)\)

(a) What is the relationship between surface tension and temperature? (b) What is the relationship between viscosity and temperature? (c) Why do substances with high surface tension also tend to have high viscosities?

Indicate whether each statement is true or false: (a) The liquid crystal state is another phase of matter, just like solid, liquid, and gas. (b) Liquid crystalline molecules are generally spherical in shape. (c) Molecules that exhibit a liquid crystalline phase do so at well-defined temperatures and pressures. (d) Molecules that exhibit a liquid crystalline phase show weaker- than-expected intermolecular forces. (e) Molecules containing only carbon and hydrogen are likely to form liquid crystalline phases. (f) Molecules can exhibit more than one liquid crystalline phase.

Which type of intermolecular force accounts for each of these differences? (a) \(\mathrm{CH}_{3} \mathrm{OH}\) boils at \(65^{\circ} \mathrm{C} ; \mathrm{CH}_{3} \mathrm{SH}\) boils at \(6^{\circ} \mathrm{C} .(\mathbf{b}) \mathrm{Xe}\) is a liquid at atmospheric pressure and \(120 \mathrm{K},\)whereas Ar is a gas under the same conditions. (c) Kr, atomic weight 84 amu, boils at \(120.9 \mathrm{K},\) whereas \(\mathrm{Cl}_{2},\) molecular weight about 71 amu, boils at 238 \(\mathrm{K}\) . (d) Acetone boils at \(56^{\circ} \mathrm{C},\) whereas 2 -methylpropane boils at \(-12^{\circ} \mathrm{C}\) .
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