Modern Chemistry: Student Edition 2012 1st Edition solutions

Modern Chemistry: Student Edition 2012 1
What idea is the kinetic-molecular theory based on?

Modern Chemistry: Student Edition 2012 1
What is an ideal gas?

Modern Chemistry: Student Edition 2012 1
State the five basic assumptions of the kineticmolecular theory.

Modern Chemistry: Student Edition 2012 1
How do gases compare with liquids and solids in terms of the distance between their molecules?

Modern Chemistry: Student Edition 2012 1
What is the relationship between the temperature, speed, and kinetic energy of gas molecules?

Modern Chemistry: Student Edition 2012 1
a. What is diffusion? b. What factors affect the rate of diffusion of one gas through another?

Modern Chemistry: Student Edition 2012 1
What is a fluid?

Modern Chemistry: Student Edition 2012 1
What is surface tension?

Modern Chemistry: Student Edition 2012 1
Give two reasons why evaporation is a crucial process in nature. 1

Modern Chemistry: Student Edition 2012 1
List six properties of solids, and explain each in terms of the kinetic-molecular theory of solids. 1

Modern Chemistry: Student Edition 2012 1
List four common examples of amorphous solids. 1

Modern Chemistry: Student Edition 2012 1
List and describe the four types of crystals in terms of the nature of their component particles and the type of bonding between them. 1

Modern Chemistry: Student Edition 2012 1
Using Figure 4.3, estimate the approximate equilibrium vapor pressure of each of the following at the specified temperature. a. water at 80C b. diethyl ether at 20C c. ethanol at 60C 1

Modern Chemistry: Student Edition 2012 1
a. What is sublimation? b. Give two examples of common substances that sublime at ordinary temperatures. 1

Modern Chemistry: Student Edition 2012 1
What is meant by the normal freezing point of a substance? 1

Modern Chemistry: Student Edition 2012 1
Explain how the attractive forces between the particles in a liquid are related to the equilibrium vapor pressure of that liquid. 1

Modern Chemistry: Student Edition 2012 1
Explain the relationship between atmospheric pressure and the actual boiling point of a liquid. 1

Modern Chemistry: Student Edition 2012 1
Explain the relationship between the molar enthalpy of fusion of a solid and the strength of attraction between that solids particles. 1

Modern Chemistry: Student Edition 2012 1
a. The molar enthalpy of vaporization for water is 40.79 kJ/mol. Express this enthalpy of vaporization in joules per gram. b. The molar enthalpy of fusion for water is 6.009 kJ/mol. Express this enthalpy of fusion in joules per gram. 2

Modern Chemistry: Student Edition 2012 1
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. 2

Modern Chemistry: Student Edition 2012 1
Given that a substance has a molar mass of 259.0 g/mol and a 71.8 g sample of the substance absorbs 4.307 kJ when it melts, a. calculate the number of moles in the sample. b. calculate the molar enthalpy of fusion. 2

Modern Chemistry: Student Edition 2012 1
a. Calculate the number of moles in a liquid sample of a substance that has a molar enthalpy of fusion of 3.811 kJ/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 g. 2

Modern Chemistry: Student Edition 2012 1
Describe the structure of a water molecule

Modern Chemistry: Student Edition 2012 1
List at least eight physical properties of water. 2

Modern Chemistry: Student Edition 2012 1
Which contains more molecules of water: \(5.00\mathrm{\ cm}^3\) of ice at 0C or \(5.00\mathrm{\ cm}^3\) of liquid water at 0.C? How many more? What is the ratio of the numbers of molecules in these two samples?

Modern Chemistry: Student Edition 2012 1
a. What volume and mass of steam at 100.C and 1.00 atm would release the same amount of energy during condensation as 100. cm3 of liquid water would release during freezing? b. What do you note, qualitatively, about the relative volumes and masses of steam and liquid water required to release the sam

Modern Chemistry: Student Edition 2012 1
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. 2

Modern Chemistry: Student Edition 2012 1
Waters molar enthalpy of fusion is 6.009 kJ/mol. Calculate the amount of energy as heat required to melt 7.95 105 g of ice. 2

Modern Chemistry: Student Edition 2012 1
A certain substance has a molar enthalpy of vaporization of 31.6 kJ/mol. How much of the substance is in a sample that requires 57.0 kJ to vaporize? 3

Modern Chemistry: Student Edition 2012 1
Given that water has a molar enthalpy of vaporization of 40.79 kJ/mol, how many grams of water could be vaporized by 0.545 kJ?

Modern Chemistry: Student Edition 2012 1
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 g/mol and a molar enthalpy of fusion of 4.60 kJ/mol. 3

Modern Chemistry: Student Edition 2012 1
What volume and mass of steam at 100.C and 760. torr would release the same amount of energy as heat during condensation as 65.5 cm3 of liquid water would release during freezing? 3

Modern Chemistry: Student Edition 2012 1
The following liquid-vapor system is at equilibrium at a given temperature in a closed system. liquid + energy 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

Modern Chemistry: Student Edition 2012 1
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 temp

Modern Chemistry: Student Edition 2012 1
Using the phase diagram for CO2, describe all the phase changes that would occur when CO2 is heated from 100C to 10C at a constant pressure of 6 atm. 3

Modern Chemistry: Student Edition 2012 1
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. 3

Modern Chemistry: Student Edition 2012 1
A pplying Models At normal atmospheric pressure, the temperature of an ice-water system remains at 0C as long as both ice and liquid water are present, regardless of the surrounding temperature. Explain why this occurs. 3

Modern Chemistry: Student Edition 2012 1
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. 3

Modern Chemistry: Student Edition 2012 1
Interpreting Diagrams Refer to the phase diagram in question 35. a. Explain what happens when solid CO2 (dry ice) warms up to room temperature at normal atmospheric pressure. b. Is there a pressure below which liquid CO2 cannot exist? Estimate that pressure from the graph. USING THE HANDBOOK 4

Modern Chemistry: Student Edition 2012 1
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 m

Modern Chemistry: Student Edition 2012 1
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.

Modern Chemistry: Student Edition 2012 1
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. ALTERNATIVE ASSESSMENT 4

Modern Chemistry: Student Edition 2012 1
Compile separate lists of crystalline and amorphous solids found in your home. Compare your lists with those of your classmates. 4

Modern Chemistry: Student Edition 2012 1
Design an experiment to grow crystals of various safe, common household materials. Record the conditions under which each type of crystal is best grown.

Modern Chemistry: Student Edition 2012 1
Surface tension is A. skin on the surface of a liquid. B. the tendency of the surface of liquids to decrease the area. C. the spontaneous mixing of two substances. D. the same as vapor pressure.

Modern Chemistry: Student Edition 2012 1
Pure liquids boil at higher temperatures under high pressures than they do under low pressures, because A. the molecules of liquid are closer together under higher pressures. B. it takes a higher temperature for the vapor pressure to equal the higher external pressure. C. the molecules of vapor are f

Modern Chemistry: Student Edition 2012 1
The formation of frost is an example of A. condensation. B. evaporation. C. deposition. D. melting point.

Modern Chemistry: Student Edition 2012 1
A graph that shows the pressure and temperature conditions under which the phases of a substance exist is called A. a phase diagram. B. a vapor pressure curve. C. a unit cell. D. the kinetic-molecular theory of matter.

Modern Chemistry: Student Edition 2012 1
Water boils at 100C. Ethanol boils at 78.5C. Which of the following statements is true? A. Water has the higher vapor pressure at 78.5C. B. Ethanol has the higher vapor pressure at 78.5C. C. Both have the same vapor pressure at 78.5C. D. Vapor pressure is not related to boiling point.

Modern Chemistry: Student Edition 2012 1
Which of the following is not a property of typical solids? A. definite melting point B. high density C. easily compressible D. low rate of diffusion

Modern Chemistry: Student Edition 2012 1
The kinetic-molecular theory states that ideal gas molecules A. are in constant, rapid, random motion. B. have mass and take up space. C. exert forces of attraction and repulsion on each other. D. have high densities compared with liquids and solids.

Modern Chemistry: Student Edition 2012 1
Using this graph of vapor pressures of substances at various temperatures, estimate the boiling point of ethanol at an applied (external) pressure of 300 torr.

Modern Chemistry: Student Edition 2012 1
It is found that 60.0 J of energy are required to melt 15 g of a substance. The molar mass of the substance is 120 g/mol. Calculate the enthalpy of fusion of the substance in kilojoules per mole. 1

Modern Chemistry: Student Edition 2012 1
Describe how a pressure cooker works. 1

Modern Chemistry: Student Edition 2012 1
What is meant by the statement that a liquid and its vapor in a closed container are in a state of dynamic equilibrium?