Question 1

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) melting 
A) deposition 
B) sublimation 
C) freezing 
D) condensation 
E) melting A

Question 2

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

Question 3

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°C 
A) 17.8°C 
B) 21.9°C 
C) 2.3°C 
D) 9.1°C 
E) 44.6°C C

Question 4

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

Question 5

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 condensation 
A) molar heat of freezing 
B) molar heat of fission 
C) molar heat of vaporization 
D) molar heat of fusion 
E) molar heat of condensation

Question 6

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

Question 7

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

Question 8

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

Question 9

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 3 
A) NF3 3 2 
B) BF3 3 2 
C) NF3 2 3 
D) BeF2 3 3 
E) BeF2 3 3

Question 10

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-OH 
A) C2H6 2CH2-OH 3OH 
B) CH3OH2H6 2CH2-OH 
C) HO-CH2CH2-OH2H6 3OH 
D) CH3OH 2CH2-OH 2H6 
E) C2H6 3OH 2CH2-OH

Question 11

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

Accepted Answer

A)   
B) PH3, NH3 
C)  CF4, CBr4 
D) C3H8,C4H10 
E) F2, Cl2 
A)   
B) PH3, NH3 
C)  CF4, CBr4 
D) C3H8,C4H10 
E) F2, Cl2

Question 12

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) sublimation 
A) vaporization 
B) condensation 
C) freezing 
D) melting 
E) sublimation

Question 13

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

Question 14

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) mixture 
A) solid 
B) liquid 
C) gas 
D) solution 
E) mixture

Question 15

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

Question 16

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

Question 17

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

Question 18

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) Cohesion 
A) Surface tension 
B) Adhesion 
C) Polarity 
D) Viscosity 
E) Cohesion

Question 19

Which one of the following crystallizes in a metallic lattice?

Accepted Answer

A) C 
B) NaMnO4 
C) K 
D) LiClO4 
E) K2Cr2O7 
A) C 
B) NaMnO4 
C) K 
D) LiClO4 
E) K2Cr2O7

Question 20

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

Accepted Answer

A) CS2 3 3 2 
C) NF3 2 2 3 
E) NF3 2 
A) CS2 3 3 2 
C) NF3 2 2 3 
E) NF3 2

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

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

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.

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

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

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.

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.

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.

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

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

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

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

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

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

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.

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.

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.

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

Which one of the following crystallizes in a metallic lattice?

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

Atoms and Elements

Electrons and the Periodic Table

Compounds and Chemical Bonds

How Chemists Use Numbers

The Mole and Chemical Formulas

Molecular Shape

Gases

Physical Properties of Solutions

Chemical Reactions and Chemical Equations

Using Balanced Chemical Equations

Acids and Bases

Equilibrium

Organic Chemistry

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Exam 7: Solids, Liquids, and Phase Changes

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

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

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.

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

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

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.

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.

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.

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

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

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

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

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

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

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.

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.

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.

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

Which one of the following crystallizes in a metallic lattice?

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

Atoms and Elements

Electrons and the Periodic Table

Compounds and Chemical Bonds

How Chemists Use Numbers

The Mole and Chemical Formulas

Molecular Shape

Gases

Physical Properties of Solutions

Chemical Reactions and Chemical Equations

Using Balanced Chemical Equations

Acids and Bases

Equilibrium

Organic Chemistry

Biochemistry

Nuclear Chemistry

Electrochemistry

Filters

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

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.

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.

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

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

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

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.

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