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Chapter 11: Problem 64

At \(25^{\circ} \mathrm{C}\) gallium is a solid with a density of \(5.91 \mathrm{~g} / \mathrm{cm}^{3}\). Its melting point, \(29.8{ }^{\circ} \mathrm{C},\) is low enough that you can melt it by holding it in your hand. The density of liquid gallium just above the melting point is \(6.1 \mathrm{~g} / \mathrm{cm}^{3} .\) Based on this information, what unusual feature would you expect to find in the phase diagram of gallium?

Short Answer

Expert verified
The unusual feature in the phase diagram of gallium is that it has a negative slope between the solid and liquid phases, as its liquid state has a higher density (\(6.1 \thinspace g/cm^3\)) than the solid state (\(5.91 \thinspace g/cm^3\)). This behavior implies that upon melting, gallium contracts rather than expands, which is uncommon among most substances.

Step by step solution

01

Compare Density of Solid and Liquid Gallium

Compare the density of solid gallium (5.91 g/cm³) and liquid gallium (6.1 g/cm³). We will notice that the density of liquid gallium is larger than the density of solid gallium.
02

Analyze the Unusual Feature

In most substances, the density of a solid state is greater than the liquid state. However, gallium is an exception to this rule as its liquid state has a higher density than the solid state. This implies that upon melting, gallium will contract rather than expand. This unusual behavior will be reflected in its phase diagram as a negative slope between the solid and liquid phases.

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Most popular questions from this chapter

(a) What is meant by the term polarizability? (b) Which of the following atoms would you expect to be most polarizable: \(\mathrm{N}\), \(\mathrm{P},\) As, \(\mathrm{Sb}\) ? Explain. (c) Put the following molecules in order of increasing polarizability: \(\mathrm{GeCl}_{4}\), \(\mathrm{CH}_{4}\), \(\mathrm{SiCl}_{4}, \mathrm{SiH}_{4}\), and \(\mathrm{GeBr}_{4}\). (d) Predict the order of boiling points of the substances in part (c).

(a) Explain why surface tension and viscosity decrease with increasing temperature. (b) Why do substances with high surface tensions also tend to have high viscosities?

As the intermolecular attractive forces between molecules increase in magnitude, do you expect each of the following to increase or decrease in magnitude? (a) vapor pressure, (b) heat of vaporization, (c) boiling point, (d) freezing point, (e) viscosity, (f) surface tension, (g) critical temperature.

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 \(6^{\circ} \mathrm{C}\). (b) Xe is liquid at atmospheric pressure and \(120 \mathrm{~K}\), whereas \(\mathrm{Ar}\) is a gas under the same conditions. (c) \(\mathrm{Kr}\), atomic weight 84 , boils at \(120.9 \mathrm{~K},\) whereas \(\mathrm{Cl}_{2},\) molecular weight about \(71,\) boils at \(238 \mathrm{~K}\). (d) Acetone boils at \(56^{\circ} \mathrm{C}\), whereas 2 -methylpropane boils at \(-12^{\circ} \mathrm{C}\)

Identify the type or types of intermolecular forces present in each substance and then select the substance in each pair that has the higher boiling point: (a) propane \(\mathrm{C}_{3} \mathrm{H}_{8}\) or \(n\) -butane \(\mathrm{C}_{4} \mathrm{H}_{10},\) (b) diethyl ether \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OCH}_{2} \mathrm{CH}_{3}\) or 1 -butanol \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH},\) (c) sulfur dioxide \(\mathrm{SO}_{2}\) or sulfur trioxide (d) phosgene \(\mathrm{Cl}_{2} \mathrm{CO}\) or formaldehyde \(\mathrm{H}_{2} \mathrm{CO}\). \(\mathrm{SO}_{3},\)
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