Ch13 Liquids and Solids – Complete Test Bank | 15th

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­Package Title: Hein Test Bank

Course Title: Hein 15e

Chapter Number: 13

Question Type: Multiple Choice

1) The following table lists some compounds and their respective surface tensions at 25°C:

Which of the following alternatives is false?

a) The attractive forces between molecules of butanoic acid are stronger than those between molecules of 1-chlorobutane.

b) The attractive forces between molecules of 1-chlorobutane are stronger than those between molecules of 1-bromobutane.

c) Molecules of 1-chlorobutane experience the least resistance to increase their surface area compared to any of the other compounds.

d) The compounds 1-chlorobutane, 2-bromobutane, 1-bromobutane, and butanoic acid are arranged in order of increasing strength of their intermolecular forces.

Difficulty: hard

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

2) The following table lists normal boiling points for different substances:

Which of the following alternatives is true?

a) The vapor pressure of propionic acid is the highest of all the substances listed under these conditions.

b) The molecules of acetone experience the weakest interactions compared to any other substance listed.

c) The molecules of propionic acid experience the strongest interactions compared to any other substance listed.

d) The vapor pressure of propionic acid is the highest of all the substances listed under these conditions and the molecules of propionic acid experience the strongest interactions compared to any other substance listed.

Difficulty: hard

Learning Objective 1: Define boiling point and melting point and determine the boiling point of a liquid from a graph of temperature versus vapor pressure.

Section Reference 1: Section 13.3

3) Which phase change corresponds to evaporation?

a) solid to liquid

b) solid to gas

c) liquid to gas

d) liquid to solid

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

4) The phase change from liquid water to its vapor form takes place at

a) constant temperature

b) constant pressure

c) constant volume

d) All of the above

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

5) Which phase change corresponds to fusion?

a) liquid to gas

b) solid to liquid

c) solid to gas

d) gas to liquid

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

6) Which phase change corresponds to sublimation?

a) solid to gas

b) liquid to gas

c) gas to liquid

d) solid to liquid

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

7) Which phase change corresponds to condensation?

a) solid to gas

b) liquid to gas

c) gas to liquid

d) solid to liquid

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

8) In a system at equilibrium between the liquid and gas phases

a) the rate at which particles change from gas to liquid exceeds the rate at which they change from liquid to gas.

b) the rate at which particles change from liquid to gas exceeds the rate at which they change from gas to liquid.

c) the rate at which particles change from gas to liquid equals the rate at which they change from liquid to gas.

d) particles stop changing phase.

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

9) The vapor pressure of a liquid is the pressure, at equilibrium, of the

a) solid above its liquid.

b) liquid above its solid.

c) gas above its liquid.

d) liquid above its gas.

Difficulty: easy

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

10) Which has the highest vapor pressure?

a) 125 mL of water at 283 K

b) 0.1 mL of water at 288 K

c) 50 mL of water at 293 K

d) 5 mL of water at 299 K

Difficulty: easy

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

11) Which has the lowest vapor pressure?

a) 25 mL of water at 283 K

b) 10 mL of water at 298 K

c) 50 mL of water at 293 K

d) 5 mL of water at 323 K

Difficulty: easy

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

12) As the rate of evaporation of a liquid decreases, its equilibrium vapor pressure

a) increases.

b) decreases.

c) remains the same.

Difficulty: medium

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

13) Use the following graph to select the boiling point of ethyl alcohol at 400 torr.

a) about 35°C

b) about 78°C

c) about 20°C

d) about 62°C

Difficulty: easy

Learning Objective 1: Define boiling point and melting point and determine the boiling point of a liquid from a graph of temperature versus vapor pressure.

Section Reference 1: Section 13.3

14) As the volatility of a liquid increases, its equilibrium vapor pressure

a) increases.

b) decreases.

c) remains the same.

Difficulty: easy

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

15) As the attractive forces between the molecules of a liquid increase, its equilibrium vapor pressure at a given temperature.

a) increases.

b) decreases.

c) remains the same.

Difficulty: easy

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

16) As the attractive forces between the molecules of a liquid increase, its volatility

a) increases.

b) decreases.

c) remains the same.

Difficulty: easy

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

17) As the attractive forces between the molecules of a liquid increase, its surface tension

a) increases.

b) decreases.

c) remains the same.

Difficulty: easy

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

18) Which segment in the following figure indicated by letters corresponds to melting?

a) AB

b) BC

c) CD

d) DE

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

19) Which phases or states are present within the CD segment in the figure shown below?

a) solid and liquid

b) solid only

c) liquid only

d) liquid and gas

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

20) The boiling point temperature of a liquid is the temperature at which its vapor pressure

a) is less than the external pressure.

b) is greater than the external pressure.

c) is equal to the external pressure.

Difficulty: easy

Learning Objective 1: Define boiling point and melting point and determine the boiling point of a liquid from a graph of temperature versus vapor pressure.

Section Reference 1: Section 13.3

21) Which of the following liquids is more volatile at room temperature?

a) honey

b) water

c) ethyl alcohol

d) diethyl ether

Difficulty: medium

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

22) Under standard conditions, what is the vapor pressure of water at 100.^°C?

a) 0 torr

b) 100 torr

c) 373 torr

d) 760 torr

Difficulty: easy

Learning Objective 1: Define boiling point and melting point and determine the boiling point of a liquid from a graph of temperature versus vapor pressure.

Section Reference 1: Section 13.3

23) The normal boiling point of a liquid is the temperature at which its vapor pressure equals

a) 100 torr

b) 337 torr

c) 373 torr

d) 760 torr

Difficulty: easy

Learning Objective 1: Define boiling point and melting point and determine the boiling point of a liquid from a graph of temperature versus vapor pressure.

Section Reference 1: Section 13.3

24) As the external pressure on a liquid increases, its boiling point temperature

a) increases.

b) decreases.

c) remains the same.

Difficulty: medium

Learning Objective 1: Define boiling point and melting point and determine the boiling point of a liquid from a graph of temperature versus vapor pressure.

Section Reference 1: Section 13.3

25) At which external pressure will water boil at the highest temperature?

a) 0.5 atm

b) 1.0 atm

c) 1.5 atm

d) 2.0 atm

Difficulty: medium

Learning Objective 1: Define boiling point and melting point and determine the boiling point of a liquid from a graph of temperature versus vapor pressure.

Section Reference 1: Section 13.3

26) Among HF, CH₄, CH₃OH and N₂O₄, intermolecular hydrogen bond is expected in

a) all of these

b) In all except one

c) In two

d) none of these

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

27) Which of the liquids below displays the strongest intermolecular forces?

a) H₂O

b) H₂S

c) H₂Se

d) H₂Te

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

28) In which of the following compounds does hydrogen bonding occur?

1. SiH₄
2. LiH
3. HI
4. NH₃

Answer D

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

29) The amount of energy required to change one gram of a liquid, at its boiling point, to a gas is called its heat of

a) fusion.

b) freezing.

c) vaporization.

d) sublimation.

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

30) The normal freezing point of water is zero degrees Celsius. What is its normal melting point?

a) –1^° C

b) 0^° C

c) 1^° C

d) 100^° C

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

31) Which of the following is capable of forming a hydrogen bond?

a) H₂S

b) HF

c) CH₄

d) H₂Te

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

32) Which one of the following bonds will be most polar?

1. N-Cl
2. O-F
3. C-F
4. N-N

Answer C

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

33) Which of the following will have the highest vapor pressure at room temperature?

a) NH₃

b) HF

c) H₂O

d) diethyl ether

Difficulty: medium

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Learning Objective 2: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.2 and 13.5

34) What is the maximum number of hydrogen bonds in which a water molecule can participate?

1. 1
2. 2
3. 3
4. 4

Answer D

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

35) The freezing point of a substance is the temperature at which its

a) solid phase is in equilibrium with its gaseous phase.

b) liquid phase is in equilibrium with its gaseous phase.

c) solid phase is in equilibrium with its liquid phase.

Difficulty: easy

Learning Objective 1: Define boiling point and melting point and determine the boiling point of a liquid from a graph of temperature versus vapor pressure.

Section Reference 1: Section 13.3

36) The amount of energy required to change one gram of a solid, at its freezing point, to a liquid is called its heat of

a) sublimation.

b) vaporization.

c) fusion.

d) condensation.

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

37) Approximately, what percentage of the Earth’s surface is covered with water?

a) 25 %

b) 50 %

c) 75 %

d) 100 %

Difficulty: easy

Learning Objective 1: Describe the characteristics of water in terms of its structure and list the sources of drinking water.

Section Reference 1: Section 13.7

38) When 5.00 g of Al₂(SO₄)₃18H₂O are heated until it dehydrates, how many grams of water are produced?

a) 2.77 g

b) 4.74 g

c) 2.43 g

d) 4.51 g

Difficulty: medium

Learning Objective 1: Explain what hydrates are, write formulas for hydrates, and calculate the percent water in a hydrate.

Section Reference 1: Section 13.6

39) For any substance, which phase of matter contains the greatest amount of energy?

a) solid

b) liquid

c) gas

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

40) How many moles of water will be produced when 15.0 g of calcium chloride dihydrate are heated?

a) 0.134 mol

b) 0.0510 mol

c) 0.204 mol

d) 0.102 mol

Difficulty: medium

Learning Objective 1: Explain what hydrates are, write formulas for hydrates, and calculate the percent water in a hydrate.

Section Reference 1: Section 13.6

41) Which substance contains molecules that will not form hydrogen bonds?

a) hydrogen

b) hydrogen fluoride

c) water

d) ammonia

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

42) Hydrogen bonding will not occur in molecules that contain only bonds between hydrogen and

a) fluorine.

b) oxygen.

c) bromine.

d) nitrogen.

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

43) Which substance below has the largest surface tension at room temperature?

a) H₂O

b) H₂S

c) CH₄

d) Hg

Difficulty: medium

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

44) Hydrogen bonds will form between molecules of compounds in which hydrogen is bonded to atoms of elements with

a) high electronegativity and large atomic radius.

b) high electronegativity and small atomic radius.

c) low electronegativity and large atomic radius.

d) low electronegativity and small atomic radius.

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

45) A sample of water at 20. ^°C contains

a) covalent bonds only.

b) hydrogen bonds only.

c) both, covalent and hydrogen bonds.

d) neither, covalent nor hydrogen bonds.

Difficulty: medium

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

46) Which of the following is weakest?

a) Polar covalent bond

b) Nonpolar covalent bond

c) Ionic bond

d) Hydrogen bond

Difficulty: medium

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

47) Alcohol is soluble in water due to

1. Covalent bond
2. Ionic bond
3. Hydrogen bond with water
4. None of these

Difficulty: medium

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

48) Which of the following is most soluble in water?

1. CS₂
2. C₂H₅OH
3. CCl₄
4. CHCl₃

Difficulty: medium

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

49) The high boiling point of water is due to

a) polar covalent bonds.

b) nonpolar covalent bonds.

c) ionic bonds.

d) hydrogen bonds.

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

50) NH₃ has a much higher boiling point than PH₃ because

1. NH₃ has a larger molecular mass
2. NH₃ forms hydrogen bond
3. NH₃ contains ionic whereas PH₃ contains covalent bonds
4. NH₃ has lower dipole moment than PH₃

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

51) The low equilibrium vapor pressure of water is due to

a) polar covalent bonds.

b) nonpolar covalent bonds.

c) ionic bonds.

d) hydrogen bonds.

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

52) What mass of water is found in one mole of magnesium sulfate heptahydrate?

a) 120.37 g

b) 138.39 g

c) 126.14 g

d) 246.51 g

Difficulty: easy

Learning Objective 1: Explain what hydrates are, write formulas for hydrates, and calculate the percent water in a hydrate.

Section Reference 1: Section 13.6

53) What is the maximum density of water?

a) 0.804 g/mL

b) 1.00 g/mL

c) 18.02 g/mL

d) 22.4 g/mL

Difficulty: easy

Learning Objective 1: Describe the characteristics of water in terms of its structure and list the sources of drinking water.

Section Reference 1: Section 13.7

54) What type of bond exists within the water molecule?

a) polar covalent

b) nonpolar covalent

c) ionic

d) hydrogen bond

Difficulty: easy

Learning Objective 1: Describe the characteristics of water in terms of its structure and list the sources of drinking water.

Section Reference 1: Section 13.7

55) What type of bond exists between water molecules?

a) polar covalent

b) nonpolar covalent

c) ionic

d) hydrogen bond

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

56) Specific heat, heat of fusion and heat of vaporization of water are higher than of H₂S because of

a) hydrogen bonding between water molecules

b) hydrogen bonding between H₂S molecules

c) covalent bonding between water molecules

b) covalent bonding between H₂S molecules

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

57) Use the following information to select the substance with the lowest boiling point.

a) Br₂

b) CH₃CH₂OH

c) CH₃COCH₃

d) C₆H₆

Difficulty: hard

Learning Objective 1: Define boiling point and melting point and determine the boiling point of a liquid from a graph of temperature versus vapor pressure.

Section Reference 1: Section 13.3

58) What quantity of heat is required to change 40.0 g of ice at melting point to liquid water? The heat of fusion of ice is 335 J/g.

a) 13400 J

b) 0.119 J

c) 8.38 J

d) 375 J

Difficulty: medium

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

59) How many moles of ice at 0 ^oC could be melted with the addition of 750 KJ of energy? The heat of fusion of ice is 335 J/g.

a) 8.0 X 10^-3 mol

b) 4.4 X 10^-4 mol

c) 2.2 X 10³ mol

d) 1.2 X 10² mol

Difficulty: medium

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

60) What quantity of heat must be removed from 20.0 g of liquid water at 0 ^°C to completely freeze the water? The heat of fusion of ice is 335 J/g.

a) 315 J

b) 16.8 J

c) 6700 J

d) 0.0597 J

Difficulty: medium

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

61) What quantity of heat would be required to melt 15 g of ice at 0 ^°C? The heat of fusion of ice is 335 J/g.

a) 90. kJ

b) 7.2 kJ

c) 5.0 kJ

d) 0.20 J

Difficulty: medium

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

62) A sample of ice at 0^° C absorbs 6030 J of heat energy. How much of the ice can melt? The heat of fusion of ice is 335 J/g.

a) 6030 g

b) 2.02 10 ⁶ g

c) 18.0 g

d) 5700 g

Difficulty: hard

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

63) What quantity of heat is required to convert 40.0 g of liquid water at its boiling point to steam? The heat of vaporization of water is 2.26 kJ/g.

a) 17.7 kJ

b) 0.0565 kJ

c) 42.3 kJ

d) 90.4 kJ

Difficulty: medium

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

64) What quantity of heat is required to convert 10.0 g of ice at 0 ^°C to steam at 100 ^°C? The heat of fusion of ice is 335 J/g. The heat of vaporization of water is 2.26 kJ/g. specific heat of liquid water is 4.184 J/g ^°C.

a) 30.1 kJ

b) 4.18 kJ

c) 22.6 kJ

d) 4210 kJ

Difficulty: hard

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

65) What amount of heat is required to convert 3.00 kg of water at its boiling point to steam? The heat of vaporization of water is 2.26 kJ/g.

a) 6.78 kJ

b) 6780 kJ

c) 1330 kJ

d) 1.33 kJ

Difficulty: medium

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

66) A sample of liquid water at 100. ^°C absorbs 113 kJ of heat energy. How much of the water will be converted to steam? The heat of vaporization of water is 2.26 kJ/g.

a) 50.0 g

b) 0.0200 g

c) 255 g

d) 113 g

Difficulty: medium

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

67) What quantity of heat is required to change the temperature of 30.0 g of water at 10.0 ^°C to 25.0 ^°C? The specific heat of liquid water is 4.184 J/g ^°C.

a) 62.8 J

b) 126 J

c) 107 J

d) 1880 J

Difficulty: medium

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

68) A sample of water at 10.0 ^°C absorbs 4410 J of heat energy. The temperature of the sample increases to 72.0 ^°C. What is the mass of the water? The specific heat of liquid water is 4.184 J/g^°C.

a) 14.7 g

b) 17.0 g

c) 256 g

d) 297 g

Difficulty: hard

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

69) A total of 506 J of heat are added to 50.0 g of water initially at 15.0 ^°C. What is the final temperature of the water? The specific heat of liquid water is 4.184 J/g ^°C.

a) 17.4 ^° C

b) 12.6 ^° C

c) 57.3 ^° C

d) -27.3 ^° C

Difficulty: medium

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

70) A total of 325 cal of heat are added to 63.0 g of aluminum initially at 25.0 ^°C. What is the final temperature of the aluminum? The specific heat of aluminum is 0.215 cal/g ^°C.

a) 49.0 ^° C

b) 240. ^° C

c) 26.1 ^° C

d) 1.11 ^° C

Difficulty: medium

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

71) A 32.0 g sample of liquid water at 21.0 ^°C absorbs 2276 J of heat energy. What will be the final temperature of the water? The specific heat of liquid water is 4.184 J/g ^°C.

a) 4.0 ⁰ C

b) 17.0 ⁰ C

c) 38.0 ⁰ C

d) 58.0 ⁰ C

Difficulty: medium

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

72) An 18.0 g sample of liquid water at 42.0 ^°C releases 979 J of heat energy. What is the final temperature of the water? The specific heat of liquid water is 4.184 J/g ^°C.

a) 13.0 ^° C

b) 29.0 ^° C

c) 36.0 ^° C

d) 55.0 ^° C

Difficulty: medium

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

73) What is the percent water in MgSO₄⋅7H₂O?

a) 2.05 %

b) 51.2 %

c) 0.488 %

d) 48.8 %

Difficulty: easy

Learning Objective 1: Explain what hydrates are, write formulas for hydrates, and calculate the percent water in a hydrate.

Section Reference 1: Section 13.6

74) What is the percent water in copper(II) sulfate pentahydrate?

a) 22.3 %

b) 36.1 %

c) 63.9 %

d) 77.7 %

Difficulty: medium

Learning Objective 1: Explain what hydrates are, write formulas for hydrates, and calculate the percent water in a hydrate.

Section Reference 1: Section 13.6

75) Which of the following accounts for uniqueness of water?

a) water is a polar molecule.

b) water is bent.

c) water molecules form hydrogen bond.

d) all of these choices

Difficulty: easy

Learning Objective 1: Describe the characteristics of water in terms of its structure and list the sources of drinking water.

Section Reference 1: Section 13.7

76) Which of the following properties of water is not affected by hydrogen bonding?

a) boiling point

b) freezing point

c) vapor pressure

d) molar mass

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

77) The term that best describes the rise of a liquid in a thin glass cylinder is

a) vapor pressure.

b) capillary action.

c) cohesive force.

d) adhesive force.

Difficulty: easy

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

78) A hydrogen bond is

a) a covalent bond between water molecules.

b) a dipole-dipole attraction between molecules that contain H bonded to F, O, or N.

c) an ionic bond between water molecules.

d) a covalent bond between molecules that contain H bonded to F, O, or N.

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

79) The chemical formula for calcium chlorate dihydrate is:

a) CaCl₂2H₂O

b) Ca(ClO₂)₂2H₂O

c) Ca(ClO₃)₂2H₂O

d) Ca(ClO₃)₂H₂

Difficulty: medium

Learning Objective 1: Explain what hydrates are, write formulas for hydrates, and calculate the percent water in a hydrate.

Section Reference 1: Section 13.6

80) The chemical formula for copper (II) sulfate pentahydrate is:

a) CuSO₄5H₂O

b) CuSO₃5H₂O

c) Cu₂SO₄5H₂O

d) Cu(SO₄)₂5H₂O

Difficulty: medium

Learning Objective 1: Explain what hydrates are, write formulas for hydrates, and calculate the percent water in a hydrate.

Section Reference 1: Section 13.6

81) Which of the following substances would exhibit hydrogen bonding?

a)

b)

c)

d)

Difficulty: hard

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

82) The name for (NH₄)₃PO₄3H₂O is:

a) ammonium phosphate trihydrate

b) triammonia phosphate triwater

c) triammonium phosphate trihydrate

d) ammonium phosphide trihydrate

Difficulty: medium

Learning Objective 1: Explain what hydrates are, write formulas for hydrates, and calculate the percent water in a hydrate.

Section Reference 1: Section 13.6

83) Which of the following compounds will not exhibit hydrogen bonding?

a)

b)

c)

d)

Difficulty: hard

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

Question Type: True/False

84) Sublimation is the change from the solid phase to the gas phase.

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

85) At pressures below one atmosphere, water will boil above 100. ^°C.

Difficulty: medium

Learning Objective 1: Define boiling point and melting point and determine the boiling point of a liquid from a graph of temperature versus vapor pressure.

Section Reference 1: Section 13.3

86) Evaporation is an exothermic process.

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

87) The strongest hydrogen bond is formed between fluorine and hydrogen.

Answer :True

Difficulty: easy

Learning Objective 1: Describe the three types of intermolecular forces and explain their significance in liquids.

Section Reference 1: Section 13.5

88) As the temperature of a liquid increases, its vapor pressure decreases.

Difficulty: easy

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

89) Deposition is an endothermic process.

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

90) At the same temperature, all liquids have the same vapor pressure.

Difficulty: easy

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

Question Type: Essay

91) What mass of ice, at 0.00 ^° C, can be converted to steam, at 100. ^°C, if it absorbs 1.00 10 ⁶ J of heat energy? The heat of fusion of ice is 335 J/g, the heat of vaporization of water is 2.26 kJ/g, and the specific heat of liquid water is 4.184 J/g ^v C.

Difficulty: hard

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

92) What quantity of heat energy is required to convert 20.0 g of ice, at 0. ^°C, to steam, at 100.^°C? The heat of fusion of ice is 335 J/g, the heat of vaporization of water is 2.26 kJ/g, and the specific heat of water is 4.184 J/g ^° C.

Difficulty: hard

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

93) Small amounts of water evaporate at room temperature. If one mole of water evaporates from a sample in one day, how many molecules are evaporating per second?

Difficulty: easy

Learning Objective 1: Calculate the amount of energy involved in a change of state.

Section Reference 1: Section 13.4

94) A hydrated sample of cobalt(II) chloride was analyzed and found to consist of 45.44% water. What is the formula of the hydrate?

Difficulty: medium

Learning Objective 1: Explain what hydrates are, write formulas for hydrates, and calculate the percent water in a hydrate.

Section Reference 1: Section 13.6

95) A 3.000 g sample of hydrated calcium chloride was heated to drive off all the water of crystallization. The remaining anhydrous sample had a mass of 2.2646 g. What is the formula of the hydrate?

Difficulty: hard

Learning Objective 1: Explain what hydrates are, write formulas for hydrates, and calculate the percent water in a hydrate.

Section Reference 1: Section 13.6

96) At 50.^° C the vapor pressure of ethanol is 0.30 atm, acetic acid is 0.08 atm, water is 0.12 atm, and acetone is 0.84 atm.

a) Arrange these substances in order of increasing rates of evaporation.
b) Arrange these substances in order of increasing boiling point temperature.

Difficulty: medium

Learning Objective 1: Explain why liquids tend to form drops and explain the process of evaporation and its relationship to vapor pressure.

Section Reference 1: Section 13.2

97) Write the balanced chemical equations for the removal of water from the following hydrated crystals.

a) Copper(II) sulfate pentahydrate
b) Tin(II) chloride dihydrate
c) Cobalt(II) chloride hexahydrate
d) Magnesium sulfate heptahydrate

Difficulty: medium

Learning Objective 1: Explain what hydrates are, write formulas for hydrates, and calculate the percent water in a hydrate.

Section Reference 1: Section 13.6