Question 1

How much heat is required to raise the temperature of 12.0 g of water from 15.4°C to 93.0°C? The specific heat of water is 4.184 J/g·°C.

Accepted Answer

A)  223 J
B)  773 J
C)  503 J
D)  4.67 ×103 J
E)  3.90 ×103 JF) B) and C)
G) A) and E)

Question 2

Place the substances in order of increasing viscosity. CH3CH2CH2CH3 H2NCH2CH2NH2 CH3CH2CH2NH2

Accepted Answer

A)  CH3CH2CH2CH3 3CH2CH2NH2 2NCH2CH2NH2
B)  H2NCH2CH2NH2 3CH2CH2NH2 3CH2CH2CH3
C)  H2NCH2CH2NH2 3CH2CH2CH3 3CH2CH2NH2
D)  CH3CH2CH2CH3 2NCH2CH2NH2 3CH2CH2NH2
E)  CH3CH2CH2NH2 2NCH2CH2NH2 3CH2CH2CH3F) A) and E)
G) B) and D)

Question 3

What is the process in which molecules undergo a phase change from the liquid phase to the solid phase?

Accepted Answer

A)  vaporization
B)  condensation
C)  freezing
D)  melting
E)  sublimationF) A) and C)
G) A) and D)

Question 4

Place the substances in order of increasing boiling point. BF3 NF3 BeF2

Accepted Answer

A)  NF3 3 2
B)  BF3 3 2
C)  NF3 2 3
D)  BeF2 3 3
E)  BeF2 3 3F) B) and C)
G) C) and D)

Question 5

Place the substances in order of increasing melting point. CS2 KCl NF3

Accepted Answer

A)  CS2 3 
B)  KCl 3 2
C)  NF3 2 
D)  CS2 3
E)  NF3 2F) C) and D)
G) A) and E)

Question 6

Select the pair of substances in which the one with the lower vapor pressure at a given temperature is listed first.

Accepted Answer

A)  3, NH3 
C)   CF4, CBr4  
D)  C3H8,C4H10 
E)  F2, Cl2" class="answers-bank-image d-inline" rel="preload" > 
B)  PH3, NH3
C)   CF4, CBr4 
D)  C3H8,C4H10
E)  F2, Cl2F) A) and D)
G) None of the above

Question 7

Which one of the following crystallizes in a metallic lattice?

Accepted Answer

A)  C
B)  NaMnO4
C)  K
D)  LiClO4
E)  K2Cr2O7F) A) and D)
G) B) and E)

Question 8

What is the process in which molecules undergo a phase change directly from the gas phase to the solid phase?

Accepted Answer

A)  deposition
B)  sublimation
C)  freezing
D)  condensation
E)  meltingF) B) and D)
G) All of the above A

Question 9

Place the substances in order of increasing viscosity. CH3OH C2H6 HO-CH2CH2-OH

Accepted Answer

A)  C2H6 2CH2-OH 3OH
B)  CH3OH2H6 2CH2-OH
C)  HO-CH2CH2-OH2H6 3OH
D)  CH3OH 2CH2-OH 2H6
E)  C2H6 3OH 2CH2-OHF) None of the above
G) B) and E)

Question 10

Which state of matter is described as taking on the shape and volume of its container?

Accepted Answer

A)  solid
B)  liquid
C)  gas
D)  solution
E)  mixtureF) C) and D)
G) B) and D)

Question 11

What amount of energy (heat)  is required to warm a 65.0-g sample of liquid water from 25.0ºC to 96.5ºC? The specific heat capacity of water is 4.184 J/gºC.

Accepted Answer

A)  4.60 J
B)  1.11 × 103 J
C)  2.62 × 104 J
D)  1.94 ×104 J
E)  1.61 JF) A) and D)
G) B) and C)

Question 12

What quantity of heat is required to melt 2.00 kg of iron at its melting point (1809 K) ? For iron, ∆Hfus = 13.80 kJ/mol.

Accepted Answer

A)  0.385 kJ
B)  6.90 kJ
C)  27.6 kJ
D)  494 kJ
E)  771 kJF) B) and E)
G) B) and D)

Question 13

When Karl Kaveman adds chilled grog to his new granite mug, he removes 10.9 kJ of energy from the mug.If it has a mass of 625 g and was at 25°C, what is its new temperature? Specific heat capacity of granite = 0.79 J/g·°C.

Accepted Answer

A)  3°C
B)  14°C
C)  22°C
D)  47°C
E)  None of these choices is correct.F) A) and B)
G) B) and D)

Question 14

What mass of water would need to evaporate from your skin in order to dissipate 1.70 ×105 J of heat from the surface of your body? H2O(l)  → H2O(g)  ∆Hvap = 40.7 kJ/mol

Accepted Answer

A)  2.26 g
B)  4.18 g
C)  75.2 g
D)  4.18 ×103 g
E)  4.07 × 104 gF) A) and E)
G) C) and E) C

Question 15

If 75.4 J of energy is absorbed by 0.25 mol of CCl4 at constant pressure, what is the change in temperature? The specific heat of CCl4 is 0.861 J/g·°C.

Accepted Answer

A)  17.8°C
B)  21.9°C
C)  2.3°C
D)  9.1°C
E)  44.6°CF) All of the above
G) B) and E) C

Question 16

A glass containing 200.0 g of H2O at 20.0°C was placed in a refrigerator.The water loses 11.7 kJ as it cools to a constant temperature.What is its new temperature? The specific heat of water is 4.184 J/g·°C.

Accepted Answer

A)  0.0°C
B)  4.0°C
C)  6.0°C
D)  14.0°C
E)  34.0°CF) A) and D)
G) A) and C)

Question 17

What is the energy in kJ/mol required to melt 1 mole of a solid?

Accepted Answer

A)  molar heat of freezing
B)  molar heat of fission
C)  molar heat of vaporization
D)  molar heat of fusion
E)  molar heat of condensationF) D) and E)
G) B) and E)

Question 18

Select the pair of substances in which the one with the higher vapor pressure at a given temperature is listed first.

Accepted Answer

A)  C7H16, C5H12 
B)  CCl4, CBr4
C)  H2O, H2S
D)  CH3CH2OH, CH3-O-CH3
E)  Xe, KrF) C) and D)
G) A) and B)

Question 19

A 275-g sample of nickel at l00.0°C is placed in 100.0 g of water at 22.0°C.What is the final temperature of the water? Assume no heat transfer with the surroundings.The specific heat of nickel is 0.444 J/g·°C and the specific heat of water is 4.184 J/g·°C.

Accepted Answer

A)  39.6°C
B)  40.8°C
C)  61.0°C
D)  79.2°C
E)  82.4°CF) A) and C)
G) B) and C)

Question 20

What is determined by the magnitude of intermolecular forces in a liquid and is a measure of a fluid's resistance to flow?

Accepted Answer

A)  Surface tension
B)  Adhesion
C)  Polarity
D)  Viscosity
E)  CohesionF) D) and E)
G) A) and E)

Exam 7: Solids, Liquids, and Phase Changes

How much heat is required to raise the temperature of 12.0 g of water from 15.4°C to 93.0°C? The specific heat of water is 4.184 J/g·°C.

Correct AnswerverifiedShow Answer

Place the substances in order of increasing viscosity. CH3CH2CH2CH3 H2NCH2CH2NH2 CH3CH2CH2NH2

Correct AnswerverifiedShow Answer

What is the process in which molecules undergo a phase change from the liquid phase to the solid phase?

Correct AnswerverifiedShow Answer

Place the substances in order of increasing boiling point. BF3 NF3 BeF2

Correct AnswerverifiedShow Answer

Place the substances in order of increasing melting point. CS2 KCl NF3

Correct AnswerverifiedShow Answer

Select the pair of substances in which the one with the lower vapor pressure at a given temperature is listed first.

Correct AnswerverifiedShow Answer

Which one of the following crystallizes in a metallic lattice?

Correct AnswerverifiedShow Answer

What is the process in which molecules undergo a phase change directly from the gas phase to the solid phase?

Correct AnswerverifiedA

Place the substances in order of increasing viscosity. CH3OH C2H6 HO-CH2CH2-OH

Correct AnswerverifiedShow Answer

Which state of matter is described as taking on the shape and volume of its container?

Correct AnswerverifiedShow Answer

What amount of energy (heat) is required to warm a 65.0-g sample of liquid water from 25.0ºC to 96.5ºC? The specific heat capacity of water is 4.184 J/gºC.

Correct AnswerverifiedShow Answer

What quantity of heat is required to melt 2.00 kg of iron at its melting point (1809 K) ? For iron, ∆Hfus = 13.80 kJ/mol.

Correct AnswerverifiedShow Answer

When Karl Kaveman adds chilled grog to his new granite mug, he removes 10.9 kJ of energy from the mug.If it has a mass of 625 g and was at 25°C, what is its new temperature? Specific heat capacity of granite = 0.79 J/g·°C.

Correct AnswerverifiedShow Answer

What mass of water would need to evaporate from your skin in order to dissipate 1.70 ×105 J of heat from the surface of your body? H2O(l) → H2O(g) ∆Hvap = 40.7 kJ/mol

Correct AnswerverifiedC

If 75.4 J of energy is absorbed by 0.25 mol of CCl4 at constant pressure, what is the change in temperature? The specific heat of CCl4 is 0.861 J/g·°C.

Correct AnswerverifiedC

A glass containing 200.0 g of H2O at 20.0°C was placed in a refrigerator.The water loses 11.7 kJ as it cools to a constant temperature.What is its new temperature? The specific heat of water is 4.184 J/g·°C.

Correct AnswerverifiedShow Answer

What is the energy in kJ/mol required to melt 1 mole of a solid?

Correct AnswerverifiedShow Answer

Select the pair of substances in which the one with the higher vapor pressure at a given temperature is listed first.

Correct AnswerverifiedShow Answer

A 275-g sample of nickel at l00.0°C is placed in 100.0 g of water at 22.0°C.What is the final temperature of the water? Assume no heat transfer with the surroundings.The specific heat of nickel is 0.444 J/g·°C and the specific heat of water is 4.184 J/g·°C.

Correct AnswerverifiedShow Answer

What is determined by the magnitude of intermolecular forces in a liquid and is a measure of a fluid's resistance to flow?

Correct AnswerverifiedShow Answer

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Place the substances in order of increasing viscosity. CH₃CH₂CH₂CH₃ H₂NCH₂CH₂NH₂ CH₃CH₂CH₂NH₂

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Place the substances in order of increasing boiling point. BF₃ NF₃ BeF₂

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Place the substances in order of increasing melting point. CS₂ KCl NF₃

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A

Place the substances in order of increasing viscosity. CH₃OH C₂H₆ HO-CH₂CH₂-OH

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What quantity of heat is required to melt 2.00 kg of iron at its melting point (1809 K) ? For iron, ∆H_fus = 13.80 kJ/mol.

Correct Answer
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What mass of water would need to evaporate from your skin in order to dissipate 1.70 ×10⁵ J of heat from the surface of your body? H₂O(l) → H₂O(g) ∆H_vap = 40.7 kJ/mol

Correct Answer
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C

If 75.4 J of energy is absorbed by 0.25 mol of CCl₄ at constant pressure, what is the change in temperature? The specific heat of CCl₄ is 0.861 J/g·°C.

Correct Answer
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C

A glass containing 200.0 g of H₂O at 20.0°C was placed in a refrigerator.The water loses 11.7 kJ as it cools to a constant temperature.What is its new temperature? The specific heat of water is 4.184 J/g·°C.

Correct Answer
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Correct Answer
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