Holt: Modern Chemistry

Mickey Sarquis, Jerry L. Sarquis

Chapter 10 States of Matter - all with Video Answers

Educators

Chapter Questions

01:16

Problem 1

What idea is the kinetic-molecular theory based on?

Shazia Naz

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01:16

Problem 2

What is an ideal gas?

Shazia Naz

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06:00

Problem 3

State the five basic assumptions of the kinetic molecular theory.

Shazia Naz

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01:11

Problem 4

How do gases compare with liquids and solids in terms of the distance between their molecules?

Shazia Naz

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01:55

Problem 5

What is the relationship between the temperature, speed, and kinetic energy of gas molecules?

Shazia Naz

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03:09

Problem 6

a. What is diffusion?
b. What factors affect the rate of diffusion of one gas through another?

Shazia Naz

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01:11

Problem 7

What is a fluid?

Shazia Naz

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03:56

Problem 8

What is surface tension?

Theodore Donnell

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02:03

Problem 9

Give two reasons why evaporation is a crucial process in nature.

Shazia Naz

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04:14

Problem 10

List six properties of solids, and explain each in terms of the kinetic-molecular theory of solids.

Shazia Naz

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00:27

Problem 11

List four common examples of amorphous solids.

Shazia Naz

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02:14

Problem 12

List and describe the four types of crystals in terms of the nature of their component particles and the
type of bonding between them.

Shazia Naz

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01:01

Problem 13

Using Figure $4.3,$ estimate the approximate equilibrium vapor pressure of each of the following at the specified temperature.

a. water at $80^{\circ} \mathrm{C}$
b. diethyl ether at $20^{\circ} \mathrm{C}$
c. ethanol at $60^{\circ} \mathrm{C}$

Shazia Naz

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03:52

Problem 14

a. What is sublimation?
b. Give two examples of common substances that sublime at ordinary temperatures.

Shazia Naz

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01:18

Problem 15

What is meant by the normal freezing point of a substance?

Shazia Naz

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01:29

Problem 16

Explain how the attractive forces between the particles in a liquid are related to the equilibrium
vapor pressure of that liquid.

Shazia Naz

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01:28

Problem 17

Explain the relationship between atmospheric pressure and the actual boiling point of a liquid.

Shazia Naz

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04:57

Problem 18

Explain the relationship between the molar enthalpy of fusion of a solid and the strength of attraction
between that solid’s particles.

Shazia Naz

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02:25

a. The molar enthalpy of vaporization for water is 40.79 $\mathrm{kJ} / \mathrm{mol}$ . Express this enthalpy of vaporization in joules per gram.
b. The molar enthalpy of fusion for water is 6.009 $\mathrm{kJ} / \mathrm{mol}$ . Express this enthalpy of fusion in joules per gram.

Shazia Naz

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01:00

Problem 20

Calculate the molar enthalpy of vaporization of a substance, given that 0.433 mol of the substance
absorbs 36.5 kJ of energy when it is vaporized.

Shazia Naz

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03:46

Problem 21

Given that a substance has a molar mass of 259.0 $\mathrm{g} / \mathrm{mol}$ and a 71.8 g sample of the substance absorbs 4.307 $\mathrm{kJ}$ when it melts,
a. calculate the number of moles in the sample.
b. calculate the molar enthalpy of fusion.

Khaai Nguyen

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02:24

Problem 22

a. Calculate the number of moles in a liquid sample of a substance that has a molar enthalpy of fusion
of 3.811 $\mathrm{kJ} / \mathrm{mol}$ , given that the sample releases 83.2 kJ when it freezes.
b. Calculate the molar mass of this substance if the mass of the sample is 5519 $\mathrm{g}$ .

Shazia Naz

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02:03

Problem 23

Describe the structure of a water molecule.

Shazia Naz

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04:41

Problem 24

List at least eight physical properties of water.

Shazia Naz

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10:09

Problem 25

Which contains more molecules of water: 5.00 $\mathrm{cm}^{3}$ of ice at $0^{\circ} \mathrm{C}$ or 5.00 $\mathrm{cm}^{3}$ of liquid water at $0 .^{\circ} \mathrm{C} ?$ How many more? What is the ratio of the numbers of molecules in these two samples?

Shazia Naz

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07:43

Problem 26

a. What volume and mass of steam at $100 .^{\circ} \mathrm{C}$ and 1.00 atm would release the same amount of energy during condensation as $100 . \mathrm{cm}^{3}$ of liquid water would release during freezing?
b. What do you note, qualitatively, about the relative volumes and masses of same and liquid water
required to release the same amount of heat? (Hint: See Sample Problem A.)

Shazia Naz

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01:02

Problem 27

Find the molar enthalpy of vaporization for a substance, given that 3.21 mol of the substance
absorbs 28.4 kJ of energy as heat when the substance changes from a liquid to a gas.

Shazia Naz

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03:12

Problem 28

Water's molar enthalpy of fusion is 6.009 $\mathrm{k} / \mathrm{mol}$ .
Calculate the amount of energy as heat required to melt $7.95 \times 10^{5} \mathrm{g}$ of ice.

Shazia Naz

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01:27

Problem 29

A certain substance has a molar enthalpy of vaporization of 31.6 $\mathrm{kJ} / \mathrm{mol}$ . How much of the substance is in a sample that requires 57.0 $\mathrm{kJ}$ to vaporize?

Shazia Naz

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02:07

Problem 30

Given that water has a molar enthalpy of vaporization of $40.79 \mathrm{kJ} / \mathrm{mol},$ how many grams of water could be vaporized by 0.545 $\mathrm{kJ} ?$

Shazia Naz

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01:49

Problem 31

Calculate the amount of energy released as heat by the freezing of 13.3 g of a liquid substance, given that the substance has a molar mass of 82.9 $\mathrm{g} / \mathrm{mol}$ and a molar enthalpy of fusion of 4.60 $\mathrm{kJ} / \mathrm{mol} .$

Shazia Naz

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04:07

Problem 32

What volume and mass of steam at $100 .^{\circ} \mathrm{C}$ and 760 . torr would release the same amount of energy as heat during condensation as 65.5 $\mathrm{cm}^{3}$ of liquid water
would release during freezing?

Shazia Naz

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00:35

Problem 33

The following liquid-vapor system is at equilibrium at a given temperature in a closed system.
liquid + energy $\rightleftarrows$ vapor
Suppose the temperature is increased, and equilibrium is established at the higher temperature. How does the final value of each of the following compare with its initial value? (In each case, answer either higher, lower, or the same.)
a. the rate of evaporation
b. the rate of condensation
c. the final concentration of vapor molecules
d. the final number of liquid molecules

Shazia Naz

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02:10

Problem 34

Given a sample of water at any point on curve AB in Figure 4.5, what effect would each of the following
changes have on that sample?

a. adding energy at constant pressure
b. decreasing the volume at constant temperature
c. removing energy at constant pressure
d. increasing the volume at constant temperature

Shazia Naz

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01:24

Problem 35

Using the phase diagram for $\mathrm{CO}_{2},$ describe all the phase changes that would occur when $\mathrm{CO}_{2}$ is heated from $-100^{\circ} \mathrm{C}$ to $-10^{\circ} \mathrm{C}$ at a constant pressure of 6 $\mathrm{atm} .$

Shazia Naz

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04:02

Problem 36

Interpreting Concepts During the freezing of a substance, energy is being removed from that
substance. Yet the temperature of the liquid-solid system remains constant. Explain this
phenomenon.

Shazia Naz

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05:46

Problem 37

Applying Models At normal atmospheric pressure, the temperature of an ice-water system remains at
$0^{\circ} \mathrm{C}$ as long as both ice and liquid water are present, regardless of the surrounding temperature. Explain why this occurs.

Shazia Naz

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01:46

Problem 38

Predicting Outcomes Given a sample of water at any point on curve AD in Figure 4.5, how could more of
the liquid water in that sample be converted into a solid without changing the temperature? Explain
your reasoning.

Shazia Naz

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02:04

Problem 39

Interpreting Diagrams Refer to the phase diagram in question 35.

a. Explain what happens when solid $\mathrm{CO}_{2}\left(\text { "dry ice }^{\prime \prime}\right)$
warms up to room temperature at normal atmospheric pressure.
b. Is there a pressure below which liquid $\mathrm{CO}_{2}$ cannot exist? Estimate that pressure from the graph.

Shazia Naz

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02:26

Problem 40

The Elements Handbook (Appendix A) contains a table of properties for each group that includes information on the crystal structures of the elements. Most metals crystallize in one of three lattice arrangements: body-centered cubic, face-centered cubic, or hexagonal close-packed. Figure 3.2 shows a model of the face-centered cubic lattice for sodium chloride. Use this figure and the information in the Elements Handbook (Appendix A) to answer the following.

a. What elements in Group 2 have the same lattice structure as sodium chloride?
b. How would the model of an element in a face-centered cubic lattice differ from the compound shown in Figure 3.2?
c. The body-centered cubic lattice is the least-efficient packing structure of the metals. What elements in Groups 1 and 2 show this arrangement?

Himanshu Garg

Numerade Educator

03:17

Problem 41

Ceramics are formed from silicates found in the soil. Artists use them to create pottery, but
engineers and scientists have created ceramics with superconductive properties. Investigate the
growing field of superconductive ceramics.

Shahina -

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00:23

Problem 42

Liquid crystals are substances that possess the combined properties of both liquids and crystals.
Write a report on these substances and the various uses we are finding for them.

Sherry Tsui

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01:32

Problem 43

Compile separate lists of crystalline and amorphous solids found in your home. Compare your lists with
those of your classmates.

Ahmed Ali

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00:33

Problem 44

Design an experiment to grow crystals of various safe, common household materials. Record the conditions under which each type of crystal is best grown.

Amy Jiang

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