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Chapter 11: Problem 3

(a) Do you expect the viscosity of glycerol, $\mathrm{C}_{3} \mathrm{H}_{5}(\mathrm{OH})_{3}$, to be larger or smaller than that of 1 -propanol, \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH} ?\) (b) Explain. [Section 11.3\(]\)

Short Answer

Expert verified
(a) The viscosity of glycerol is expected to be larger than that of 1-propanol. (b) Glycerol has three hydroxyl groups, enabling it to form more intermolecular hydrogen bonds with other glycerol molecules compared to 1-propanol, which has only one hydroxyl group. This leads to stronger intermolecular forces and higher viscosity for glycerol compared to 1-propanol.

Step by step solution

01

Analyze the molecular structures of glycerol and 1-propanol

Glycerol is an organic compound with the chemical formula \(\mathrm{C}_{3}\mathrm{H}_{5}(\mathrm{OH})_{3}\). Glycerol has three hydroxyl groups, and its structure is: ``` HO-CH2-CHOH-CH2-OH ``` 1-propanol is an alcohol with the chemical formula \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}\). The structure of 1-propanol is: ``` CH3-CH2-CH2-OH ``` Now that we have seen the molecular structures, it is important to analyze the intermolecular forces between the molecules.
02

Analyze the intermolecular forces present in glycerol and 1-propanol

The primary intermolecular force present in both glycerol and 1-propanol is hydrogen bonding, due to the presence of hydroxyl groups (-OH) in both molecules. However, glycerol has three hydroxyl groups, which means it has more hydrogen bond donors and acceptors than 1-propanol, which only has one hydroxyl group. This difference in the number of hydrogen bonds between glycerol and 1-propanol will have a significant effect on their viscosities.
03

Compare the viscosity of glycerol and 1-propanol

Since glycerol has more hydrogen bond donors and acceptors due to the presence of three hydroxyl groups, it can form more intermolecular hydrogen bonds with other glycerol molecules. As a result, the resistance to flow (viscosity) of glycerol is expected to be higher than that of 1-propanol. Hence, the viscosity of glycerol is expected to be larger than that of 1-propanol. Now let's answer part (b) of the question.
04

Provide an explanation

The viscosity of glycerol is expected to be larger than that of 1-propanol because of the number of hydrogen bonds it can form due to its three hydroxyl groups. More hydrogen bonds lead to stronger intermolecular forces and a greater resistance to flow, resulting in a higher viscosity. In contrast, 1-propanol has only one hydroxyl group, which means fewer hydrogen bonds can form between 1-propanol molecules, leading to a lower viscosity compared to glycerol.

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Most popular questions from this chapter

Ethyl chloride \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Cl}\right)\) boils at \(12^{\circ} \mathrm{C}\). When liquid $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Cl}$ under pressure is sprayed on a room-temperature $\left(25^{\circ} \mathrm{C}\right)$ surface in air, the surface is cooled considerably. (a) What does this observation tell us about the specific heat of \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Cl}(g)\) as compared with that of \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Cl}(l) ?(\mathbf{b})\) Assume that the heat lost by the surface is gained by ethyl chloride. What enthalpies must you consider if you were to calculate the final temperature of the surface?

Appendix \(\mathrm{B}\) lists the vapor pressure of water at various external pressures. (a) Plot the data in Appendix B,vapor pressure versus temperature $\left({ }^{\circ} \mathrm{C}\right) .$ From your plot, estimate the vapor pressure of water at body temperature, \(37^{\circ} \mathrm{C}\). (b) Explain the significance of the data point at $101.3 \mathrm{kPa}, 100^{\circ} \mathrm{C} .(\mathbf{c}) \mathrm{A}\( city at an altitude of \)1525 \mathrm{~m}$ above sea level has a barometric pressure of \(84.3 \mathrm{kPa}\). To what temperature would you have to heat water to boil it in this city? (d) A city at an altitude of \(150 \mathrm{~m}\) below sea level would have a barometric pressure of \(103.14 \mathrm{kPa}\). To what temperature would you have to heat water to boil it in this city?

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

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.

At standard temperature and pressure, the molar volumes of \(\mathrm{Cl}_{2}\) and \(\mathrm{NH}_{3}\) gases are 22.06 and \(22.40 \mathrm{~L}\), respectively. (a) Given the different molecular weights, dipole moments, and molecular shapes, why are their molar volumes nearly the same? (b) On cooling to $160 \mathrm{~K}$, both substances form crystalline solids. Do you expect the molar volumes to decrease or increase on cooling the gases to \(160 \mathrm{~K} ?\) (c) The densities of crystalline \(\mathrm{Cl}_{2}\) and \(\mathrm{NH}_{3}\) at \(160 \mathrm{~K}\) are 2.02 and \(0.84 \mathrm{~g} / \mathrm{cm}^{3}\), respectively. Calculate their molar volumes. (d) Are the molar volumes in the solid state as similar as they are in the gaseous state? Explain. (e) Would you expect the molar volumes in the liquid state to be closer to those in the solid or gaseous state?
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