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Chapter 12: Problem 138

The following data are given for \(\mathrm{CCl}_{4}\). Normal melting point, \(-23^{\circ} \mathrm{C} ;\) normal boiling point, \(77^{\circ} \mathrm{C} ;\) density of liquid \(1.59 \mathrm{g} / \mathrm{mL} ; \Delta H_{\text {fus }}=3.28 \mathrm{kJ} \mathrm{mol}^{-1} ;\) vapor pressure at \(25^{\circ} \mathrm{C}, 110\) Torr. (a) What phases-solid, liquid, and/or gas-are present if \(3.50 \mathrm{g} \mathrm{CCl}_{4}\) is placed in a closed \(8.21 \mathrm{L}\) container at \(25^{\circ} \mathrm{C} ?\) (b) How much heat is required to vaporize 2.00 L of \(\mathrm{CCl}_{4}(\mathrm{l})\) at its normal boiling point?

Short Answer

Expert verified
a) The CCl4 would be in the liquid phase. b) The heat required to vaporize the CCl4 would be 67.50 kJ.

Step by step solution

01

Determine phase(s) of CCl4

Given that the melting point of \(\mathrm{CCl}_{4}\) is \(-23^{\circ} \mathrm{C}\) and the boiling point is \(77^{\circ} \mathrm{C}\), if \(\mathrm{CCl}_{4}\) is placed in a closed \(8.21 \mathrm{L}\) container at \(25^{\circ} \mathrm{C}\), it would be in liquid state because \(25^{\circ} \mathrm{C}\) is between the melting and boiling points.
02

Calculate molar volume of CCl4

First, use the given density to convert the volume of CCl4 to be vaporized into mass. The density of \(\mathrm{CCl}_{4}\) is given as \(1.59 \mathrm{g}/\mathrm{mL}\). Therefore, \(2.00 \mathrm{L} = 2000 \mathrm{mL} = 2000 \mathrm{mL} \times 1.59 \mathrm{g}/\mathrm{mL} = 3180 \mathrm{g}\). Then, calculate the molar volume using the molar mass of CCl4 (154.5 g/mol): molar volume = \(3180 \mathrm{g} / 154.5 \mathrm{g/mol} = 20.58 \mathrm{mol}\)
03

Find the heat of vaporization

The heat of vaporization can be found by multiplying the number of moles by the heat of fusion (change in enthalpy during phase transition). The given heat of fusion of CCl4 is \(3.28 kJ/mol\). So, the heat of vaporization is \(20.58 \mathrm{mol} \times 3.28 \mathrm{kJ/mol} = 67.50 \mathrm{kJ}\)
04

Transfer heat to vaporize

The heat required to vaporize 2.00 L of liquid CCl4 at its normal boiling point is simply equal to the heat of vaporization, which has been calculated to be 67.50 kJ.

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Most popular questions from this chapter

One popular demonstration in chemistry labs is performed by boiling a small quantity of water in a metal can (such as a used soda can), picking up the can with tongs and quickly submerging it upside down in cold water. The can collapses with a loud and satisfying pop. Give an explanation of this crushing of the can. (Note: If you try this demonstration, do not heat the can over an open flame.)

A television commercial claims that a product makes water "wetter" Can there be any basis to this claim? Explain.

A crystalline solid contains three types of ions, \(\mathrm{Na}^{+}, \mathrm{O}^{2-},\) and \(\mathrm{Cl}^{-}\). The solid is made up of cubic unit cells that have \(\mathrm{O}^{2-}\) ions at each corner, \(\mathrm{Na}^{+}\) ions at the center of each face, and \(\mathrm{Cl}^{-}\) ions at the center of the cells. What is the chemical formula of the compound? What are the coordination numbers for the \(\mathrm{O}^{2-}\) and \(\mathrm{Cl}^{-}\) ions? If the length of one edge of the unit cell is \(a,\) what is the shortest distance from the center of a \(\mathrm{Na}^{+}\) ion to the center of an \(\mathrm{O}^{2-}\) ion? Similarly, what is the shortest distance from the center of a \(\mathrm{Cl}^{-}\) ion to the center of an \(\mathrm{O}^{2-}\) ion?

Equilibrium is established between \(\mathrm{Br}_{2}(\mathrm{l})\) and \(\mathrm{Br}_{2}(\mathrm{g})\) at \(25.0^{\circ} \mathrm{C} .\) A \(250.0 \mathrm{mL}\) sample of the vapor weighs 0.486 g. What is the vapor pressure of bromine at \(25.0^{\circ} \mathrm{C},\) in millimeters of mercury?

Explain the important distinctions between each pair of terms: (a) adhesive and cohesive forces; (b) vaporization and condensation; (c) triple point and critical point; (d) face-centered and body-centered cubic unit cell; (e) tetrahedral and octahedral hole.
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