Chemistry The Central Science 14th Edition Brown - Test Bank

Chemistry The Central Science 14th Edition Brown – Test Bank

 

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Sample Questions Are Posted Below

 

Chemistry: The Central Science, 14e (Brown, et al.)

Chapter 5   Thermochemistry

 

5.1   Multiple Choice Questions

 

1) Objects can possess energy as ________.

 

(a) endothermic energy

(b) potential energy

(c) kinetic energy

 

1. A) a only
2. B) b only
3. C) c only
4. D) a and c
5. E) b and c

Answer:  E

Diff: 1     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G2

 

2) The internal energy of a system is always increased by ________.

1. A) adding heat to the system
2. B) having the system do work on the surroundings
3. C) withdrawing heat from the system
4. D) adding heat to the system and having the system do work on the surroundings
5. E) a volume decompression

Answer:  A

Diff: 2     Var: 1     Page Ref: Sec. 5.2

LO:  5.2

GO:  G2

 

3) The internal energy of a system ________.

1. A) is the sum of the kinetic energy of all of its components
2. B) is the sum of the rotational, vibrational, and translational energies of all of its components
3. C) refers only to the energies of the nuclei of the atoms of the component molecules
4. D) is the sum of the potential and kinetic energies of the components
5. E) none of the above

Answer:  D

Diff: 1     Var: 1     Page Ref: Sec. 5.2

LO:  5.2

GO:  G2

 

4) Which one of the following conditions would always result in an increase in the internal energy of a system?

1. A) The system loses heat and does work on the surroundings.
2. B) The system gains heat and does work on the surroundings.
3. C) The system loses heat and has work done on it by the surroundings.
4. D) The system gains heat and has work done on it by the surroundings.
5. E) None of the above is correct.

Answer:  D

Diff: 2     Var: 1     Page Ref: Sec. 5.2

LO:  5.2

GO:  G2

 

5) When a system ________, ΔE is always negative.

1. A) absorbs heat and does work
2. B) gives off heat and does work
3. C) absorbs heat and has work done on it
4. D) gives off heat and has work done on it
5. E) None of the above is always

Answer:  B

Diff: 2     Var: 1     Page Ref: Sec. 5.2

LO:  5.2

GO:  G2

 

6) Which one of the following is an endothermic process?

1. A) ice melting
2. B) water freezing
3. C) boiling soup
4. D) Hydrochloric acid and barium hydroxide are mixed at 25 °C: the temperature increases.
5. E) Both A and C

Answer:  E

Diff: 2     Var: 1     Page Ref: Sec. 5.2

LO:  5.2

GO:  G2

 

7) Which one of the following is an exothermic process?

1. A) ice melting
2. B) water evaporating
3. C) boiling soup
4. D) condensation of water vapor
5. E) Ammonium thiocyanate and barium hydroxide are mixed at 25 °C: the temperature drops.

Answer:  D

Diff: 2     Var: 1     Page Ref: Sec. 5.2

LO:  5.2

GO:  G2

 

8) Of the following, which one is a state function?

1. A) H
2. B) q
3. C) w
4. D) heat
5. E) none of the above

Answer:  A

Diff: 2     Var: 1     Page Ref: Sec. 5.2

LO:  5.4

GO:  G2

 

9) Which of the following is a statement of the first law of thermodynamics?

1. A) Ek= mv2
2. B) A negative ΔH corresponds to an exothermic process.
3. C) ΔE = Efinal- Einitial
4. D) Energy lost by the system must be gained by the surroundings.
5. E) 1 cal = 4.184 J (exactly)

Answer:  D

Diff: 3     Var: 1     Page Ref: Sec. 5.2

LO:  5.2

GO:  G2

 

10) The internal energy can be increased by ________.

 

(a) transferring heat from the surroundings to the system

(b) transferring heat from the system to the surroundings

(c) doing work on the system

 

1. A) a only
2. B) b only
3. C) c only
4. D) a and c
5. E) b and c

Answer:  D

Diff: 2     Var: 1     Page Ref: Sec. 5.2

LO:  5.2

GO:  G2

 

 

11) A ________ ΔH corresponds to an ________ process.

1. A) negative, endothermic
2. B) negative, exothermic
3. C) positive, exothermic
4. D) zero, exothermic
5. E) zero, endothermic

Answer:  B

Diff: 1     Var: 1     Page Ref: Sec. 5.3

LO:  5.6

GO:  G2

12) A ________ ΔH corresponds to an ________ process.

1. A) negative, endothermic
2. B) positive, exothermic
3. C) positive, endothermic
4. D) zero, exothermic
5. E) zero, endothermic

Answer:  C

Diff: 1     Var: 1     Page Ref: Sec. 5.3

LO:  5.6

GO:  G2

 

13) ΔH for an endothermic process is ________ while ΔH for an exothermic process is ________.

1. A) zero, positive
2. B) zero, negative
3. C) positive, zero
4. D) negative, positive
5. E) positive, negative

Answer:  E

Diff: 1     Var: 1     Page Ref: Sec. 5.3

LO:  5.6

GO:  G2

 

14) For a given process at constant pressure, w is positive. This means that the process involves ________.

1. A) work being done by the system on the surroundings
2. B) work being done by the surroundings on the system
3. C) no work being done
4. D) an equal amount of work done on the system and by the system
5. E) work being done against a vacuum

Answer:  A

Diff: 1     Var: 1     Page Ref: Sec. 5.3

LO:  5.6

GO:  G2

 

 

15) Which one of the following statements is true?

1. A) Enthalpy is an intensive property.
2. B) The enthalpy change for a reaction is independent of the state of the reactants and products.
3. C) Enthalpy is a state function.
4. D) H is the value of q measured under conditions of constant volume.
5. E) The enthalpy change of a reaction is the reciprocal of the ΔH of the reverse reaction.

Answer:  C

Diff: 2     Var: 1     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

16) All of the following statements are true except ________.

1. A) Internal energy is a state function.
2. B) The enthalpy change for a reaction is equal in magnitude, but opposite in sign, to the enthalpy change for the reverse reaction.
3. C) The enthalpy change for a reaction depends on the state of the reactants and products.
4. D) The enthalpy of a reaction is equal to the heat of the reaction.
5. E) Enthalpy is an intensive property.

Answer:  E

Diff: 3     Var: 1     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

 

17) A chemical reaction that absorbs heat from the surroundings is said to be ________ and has a ________ ΔH at constant pressure.

1. A) endothermic, positive
2. B) endothermic, negative
3. C) exothermic, negative
4. D) exothermic, positive
5. E) exothermic, neutral

Answer:  A

Diff: 2     Var: 1     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

 

18) A chemical reaction that releases heat to the surroundings is said to be ________ and has a ________ ΔH at constant pressure.

1. A) endothermic, positive
2. B) endothermic, negative
3. C) exothermic, negative
4. D) exothermic, positive
5. E) exothermic, neutral

Answer:  C

Diff: 2     Var: 1     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

 

19) The reaction

 

4Al (s) + 3O2 (g) → 2 Al2O3 (s)       ΔH° = -3351 kJ

is ________, and therefore heat is ________ by the reaction.

1. A) endothermic, released
2. B) endothermic, absorbed
3. C) exothermic, released
4. D) exothermic, absorbed
5. E) thermoneutral, neither released nor absorbed

Answer:  C

Diff: 1     Var: 1     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

20) When ________ is constant, the enthalpy change of a process equal to the amount of heat transferred into or out of the system?

1. A) temperature
2. B) volume
3. C) pressure and volume
4. D) temperature and volume
5. E) pressure

Answer:  E

Diff: 3     Var: 1     Page Ref: Sec. 5.4

LO:  5.7

GO:  G2

 

21) The units of heat capacity are ________.

1. A) K/J or °C/J
2. B) J/K or J/°C
3. C) J/g-K or J/g-°C
4. D) J/mol
5. E) g-K/J or g-°C/J

Answer:  B

Diff: 2     Var: 1     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

22) The units of specific heat are ________.

1. A) K/J or °C/J
2. B) J/K or J/°C
3. C) J/g-K or J/g-°C
4. D) J/mol
5. E) g-K/J or g-°C/J

Answer:  C

Diff: 2     Var: 1     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

23) The term Btu which stands for ________ is commonly used in engineering applications.

1. A) Best thermal unit
2. B) Bunsen thermal unit
3. C) British thermal unit
4. D) Bake thermal unit
5. E) Brush thermal unit

Answer:  C

Diff: 3     Var: 1     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

24) Which of the following is a statement of Hess’s law?

1. A) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the sum of the enthalpy changes for the individual steps.
2. B) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the product of the enthalpy changes for the individual steps.
3. C) The ΔH for a process in the forward direction is equal in magnitude and opposite in sign to the ΔH for the process in the reverse direction.
4. D) The ΔH for a process in the forward direction is equal to the ΔH for the process in the reverse direction.
5. E) The ΔH of a reaction depends on the physical states of the reactants and products.

Answer:  A

Diff: 2     Var: 1     Page Ref: Sec. 5.6

LO:  5.9

GO:  G2

 

25) For which one of the following reactions is ΔH°rxn equal to the heat of formation of the product?

1. A) N2(g) + 3H2(g) → 2NH3 (g)
2. B) (1/2)N2(g) + O2(g) → NO2(g)
3. C) 6C (s) + 6H (g) → C6H6 (l)
4. D) P (g) + 4H (g) + Br (g) → PH4Br (l)
5. E) 12C (g) + 11H2 (g) + 11O (g) → C6H22O11(g)

Answer:  B

Diff: 3     Var: 1     Page Ref: Sec. 5.7

LO:  5.10a

GO:  G2

 

 

26) Of the following, ΔH°f is not zero for ________.

1. A) O2(g)
2. B) C (graphite)
3. C) N2(g)
4. D) F2(s)
5. E) Cl2(g)

Answer:  D

Diff: 2     Var: 1     Page Ref: Sec. 5.7

LO:  5.10a

GO:  G2

 

27) Of the following, ΔH°f is not zero for ________.

1. A) Sc (g)
2. B) Si (s)
3. C) P4(s, white)
4. D) Br2(l)
5. E) Ca (s)

Answer:  A

Diff: 3     Var: 1     Page Ref: Sec. 5.7

LO:  5.10a

GO:  G2

28) Consider the following two reactions:

 

A → 2B    ΔH°rxn = 456.7 kJ/mol

A → C      ΔH°rxn = -22.1 kJ/mol

 

Determine the enthalpy change for the process:

 

2B → C

478. A) -478.8 kJ/mol
479. B) -434.6 kJ/mol
480. C) 434.6 kJ/mol
481. D) 478.8 kJ/mol
482. E) More information is needed to solve the problem.

Answer:  A

Diff: 2     Var: 1     Page Ref: Sec. 5.7

LO:  5.10a

GO:  G4

 

 

29) In the reaction below, ΔH°f is zero for ________.

Ni (s) + 2CO (g) + 2PF3 (g) → Ni(CO)2(PF3)2 (l)

 

1. A) Ni (s)
2. B) CO (g)
3. C) PF3(g)
4. D) Ni(CO)2(PF3)2(l)
5. E) both CO (g) and PF3(g)

Answer:  A

Diff: 1     Var: 1     Page Ref: Sec. 5.7

LO:  5.10a

GO:  G4

 

30) For the combustion reaction of methane, ΔH°f is zero for ________.

CH4 (g) + O2 (g)  →  2H2O(g) + CO2 (g)

 

1. A) O2(g)
2. B) CH4(g)
3. C) CO2(g)
4. D) H2O (g)
5. E) Both O2(g) and CH4(g)

Answer:  A

Diff: 1     Var: 1     Page Ref: Sec. 5.7

LO:  5.10a

GO:  G4

31) For the following reactions, the ΔH°rxn is NOT equal to ΔH°f for the product except for ________.

1. A) CH4(g) + 2Cl2(g) → CH2Cl2 (l) + 2HCl (g)
2. B) N2(g) + O3(g) → N2O3 (g)
3. C) Xe (g) + 2F2(g) → XeF4(g)
4. D) 2CO (g) + O2(g) → 2CO2(g)
5. E) C (diamond) + O2(g) → CO2(g)

Answer:  C

Diff: 3     Var: 1     Page Ref: Sec. 5.7

LO:  5.10a

GO:  G4

 

 

32) For the following reactions, the ΔH°rxn is NOT equal to ΔH°f for the product except for ________.

1. A) 2Ca (s) + O2(g) → 2CaO (s)
2. B) 3Mg (s) + N2(g) → Mg3N2(s)
3. C) C2H2(g) + H2(g) → H4 (g)
4. D) 2C (graphite) + O2(g) → 2CO (g)
5. E) C (diamond) + O2 (g) → CO2(g)

Answer:  B

Diff: 3     Var: 1     Page Ref: Sec. 5.7

LO:  5.10a

GO:  G4

 

33) For the following reactions, the ΔH°rxn is NOT equal to ΔH°f for the product except for ________.

1. A) N2(g) + O2(g) → 2NO (g)
2. B) 2H2(g) + O2(g) → 2H2O (l)
3. C) 2H2(g) + O2(g) → 2H2O (g)
4. D) 2C (s, graphite) + 2H2(g) → C2H4(g)
5. E) H2O (l) + 1/2 O2(g) → H2O2(l)

Answer:  D

Diff: 2     Var: 1     Page Ref: Sec. 5.7

LO:  5.10a

GO:  G4

 

34) For the following reactions, the ΔH°rxn is NOT equal to ΔH°f for the product except for ________.

1. A) H2O (l) + 1/2O2(g) → H2O2(l)
2. B) N2(g) + O2(g) → 2NO (g)
3. C) 2H2(g) + O2(g) → 2H2O (l)
4. D) 2H2(g) + O2(g) → 2H2O (g)
5. E) none of the above

Answer:  E

Diff: 2     Var: 1     Page Ref: Sec. 5.7

LO:  5.10a

GO:  G4

 

35) For the following reactions, the ΔH°rxn is NOT equal to ΔH°f for the product except for ________.

1. A) H2(g) + 1/2 O2(g) → H2O (l)
2. B) H2(g) + O2(g) → H2O2 (l)
3. C) 2C (s, graphite) + 2H2(g) → C2H4(g)
4. D) 1/2 N2(g) + O2(g) → NO2 (g)
5. E) all of the above

Answer:  E

Diff: 2     Var: 1     Page Ref: Sec. 5.7

LO:  5.10a

GO:  G4

 

36) The term standard conditions with respect to enthalpy change means ________.

1. A) 1 atm and 0 K
2. B) 1 atm and 1 L
3. C) 1 atm and 298 K
4. D) 1 L and 0 K
5. E) 1 atm and 1 °C

Answer:  C

Diff: 1     Var: 1     Page Ref: Sec. 5.7

LO:  5.10a

GO:  G2

 

37) The energy released by combustion of ________ of a substance is called the fuel value of the substance.

1. A) 1 kJ
2. B) 1 kg
3. C) 1 lb
4. D) 1 J
5. E) 1 g

Answer:  E

Diff: 2     Var: 1     Page Ref: Sec. 5.9

LO:  5.1 – 5.11

GO:  G2

 

38) Fuel values of hydrocarbons increase as the ________ increases.

1. A) C atomic ratio
2. B) H/C atomic ratio
3. C) H atomic ratio
4. D) C/C atomic ratio
5. E) C/H atomic ratio

Answer:  B

Diff: 1     Var: 1     Page Ref: Sec. 5.9

LO:  5.1 – 5.11

GO:  G7

 

39) ________ yields the highest fuel value.

1. A) hydrogen
2. B) charcoal
3. C) bituminous coal
4. D) natural gas
5. E) wood

Answer:  A

Diff: 2     Var: 1     Page Ref: Sec. 5.9

LO:  5.1 – 5.11

GO:  G7

 

40) All of the following are considered fossil fuels except ________.

1. A) hydrogen
2. B) anthracite coal
3. C) crude oil
4. D) natural gas
5. E) petroleum

Answer:  A

Diff: 2     Var: 1     Page Ref: Sec. 5.9

LO:  5.1 – 5.11

GO:  G7

 

41) The most abundant fossil fuel is ________.

1. A) natural gas
2. B) petroleum
3. C) coal
4. D) uranium
5. E) hydrogen

Answer:  C

Diff: 1     Var: 1     Page Ref: Sec. 5.9

LO:  5.1 – 5.11

GO:  G7

 

 

5.2   Bimodal Questions

 

1) Calculate the kinetic energy in J of an electron moving at 6.00 × 106 m/s. The mass of an electron is 9.11 × 10-28 g.

4. A) 4.98 × 10-48J
5. B) 3.28 × 10-14 J
6. C) 1.64 × 10-17J
7. D) 2.49 × 10-48J
8. E) 6.56 × 10-14J

Answer:  C

Diff: 2     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

2) Calculate the kinetic energy in joules of an automobile weighing 2135 lb and traveling at 55 mph.

1. A) 1.2 × 104J
2. B) 2.9 × 105J
3. C) 5.9 × 105J
4. D) 3.2 × 106J
5. E) 3.2 × 10-6J

Answer:  B

Diff: 3     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

 

3) Calculate the kinetic energy in joules of an automobile weighing 4345 lb and traveling at 75 mph.

5. A) 5.5 × 105 J
6. B) 5.5 × 10-5J
7. C) 1.1 × 106J
8. D) 2.2 × 106J
9. E) 2.2 × 10-6J

Answer:  C

Diff: 3     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

 

 

4) The kinetic energy of a 7.3 kg steel ball traveling at 18.0 m/s is ________ J.

1. A) 1.2 × 103
2. B) 66
3. C) 2.4 × 103
4. D) 1.3 × 102
5. E) 7.3

Answer:  A

Diff: 2     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

 

5) The kinetic energy of a 10.3 g golf ball traveling at 48.0 m/s is ________ J.

1. A) 1.20 × 103
2. B) 66
3. C) 11.9
4. D) 1.3 × 102
5. E) 23.7

Answer:  C

Diff: 2     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

6) Calculate the kinetic energy in joules of a 150 lb jogger (68.1 kg) traveling at 12.0 mile/hr (5.36 m/s).

1. A) 1.96 × 103J
2. B) 365 J
3. C) 978 J
4. D) 183 J
5. E) 68.1 J

Answer:  C

Diff: 2     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

 

7) What is the kinetic energy of a 55.2 g object moving at 135 m/s.

1. A) 503 J
2. B) 5.03 × 105J
3. C) 1.01 × 103J
4. D) 3.73 J
5. E) 3.73 × 103J

Answer:  A

Diff: 2     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

 

 

8) The kinetic energy of a 23.2-g object moving at a speed of 81.9 km/hr is ________ J.

1. A) 1900
2. B) 77.8
3. C) 145
4. D) 1.43 × 10-3
5. E) 6.00

Answer:  E

Diff: 3     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

 

9) What is the kinetic energy of a 145 g baseball traveling at 89.9 mi/hr?

1. A) 17 × 105 J
2. B) 2.91 J
3. C) 234 J
4. D) 5.83
5. E) 117 J

Answer:  E

Diff: 3     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

10) A 100-watt electric incandescent light bulb consumes ________ J of energy in 24 hours. [1 Watt (W) = 1 J/sec]

2. A) 2.40 × 103
3. B) 8.64 × 103
4. C) 4.17
5. D) 2.10 × 103
6. E) 8.64 × 106

Answer:  E

Diff: 3     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

 

11) The ΔE of a system that releases 12.4 J of heat and does 4.2 J of work on the surroundings is ________ J.

16. A) 16.6
17. B) 12.4
18. C) 4.2
19. D) -16.6
20. E) -8.2

Answer:  D

Diff: 2     Var: 1     Page Ref: Sec. 5.2

LO:  5.3

GO:  G4

 

12) The ΔE of a system that absorbs 12.4 J of heat and does 4.2 J of work on the surroundings is ________ J.

16. A) 16.6
17. B) 12.4
18. C) 4.2
19. D) -16.6
20. E) 8.2

Answer:  E

Diff: 2     Var: 1     Page Ref: Sec. 5.2

LO:  5.3

GO:  G4

 

13) The change in the internal energy of a system that absorbs 2,500 J of heat and that does 7,655 J of work on the surroundings is ________ J.

1. A) 10,155
2. B) 5,155
3. C) -5,155
4. D) -10,155
5. E) 1.91 × 107

Answer:  C

Diff: 2     Var: 1     Page Ref: Sec. 5.2

LO:  5.3

GO:  G4

14) The change in the internal energy of a system that releases 2,500 J of heat and that does 7,655 J of work on the surroundings is ________ J.

1. A) -10,155
2. B) -5,155
3. C) -1.91 × 107
4. D) 10,155
5. E) 5,155

Answer:  A

Diff: 2     Var: 1     Page Ref: Sec. 5.2

LO:  5.3

GO:  G4

 

15) Hydrogen gas and bromine gas react to form hydrogen bromide gas. How much heat (kJ) is released when 155 grams of HBr is formed in this reaction? ΔH° = -72 kJ.

1. A) 137
2. B) 69
3. C) -69
4. D) -137
5. E) 1.12 × 105

Answer:  B

Diff: 2     Var: 1     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

 

16) The value of ΔH° for the reaction below is -126 kJ.  ________ kj are released when 2.00 mol of NaOH is formed in the reaction?

 

2Na2O2 (s) + 2H2O (l) → 4NaOH (s) + O2 (g)

 

1. A) 252
2. B) 63
3. C) 3.9
4. D) 7.8
5. E) -126

Answer:  B

Diff: 2     Var: 1     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

17) The value of ΔH° for the reaction below is -790 kJ. The enthalpy change accompanying the reaction of 0.95 g of S is ________ kJ.

2S (s) + 3O2 (g) → 2SO3 (g)

 

1. A) 23
2. B) -23
3. C) -12
4. D) 12
5. E) -790

Answer:  C

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18) The value of ΔH° for the reaction below is -6535 kJ.  ________ kJ of heat are released in the combustion of 16.0 g of  (l)?

2C6H6 (l) + 15O2 (g) → 12CO2 (g) + 6H2O (l)

 

1. A) 1.34 × 103
2. B) 5.23 × 104
3. C) 669
4. D) 2.68 × 103
5. E) -6535

Answer:  C

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19) Carbon monoxide and oxygen gas react to form carbon dioxide. How much heat is released when 89.5 grams of O2 (g) reacts with excess CO? ΔH° = -482 kJ.

1. A) 1.35 × 103 kJ
2. B) 2.70 × 103kJ
3. C) 1.35 × 10-3kJ
4. D) 674 kJ
5. E) 4.31 × 104kJ

Answer:  A

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20) The value of ΔH° for the reaction below is -336 kJ. Calculate the heat (kJ) released to the surroundings when 23.0 g of HCl is formed.

 

CH4 (g) + 3Cl2 (g) → CHCl3 (l) + 3HCl (g)

 

1. A) 177 kJ
2. B) 2.57 × 103kJ
3. C) 70.7 kJ
4. D) 211 kJ
5. E) -336 kJ

Answer:  C

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21) How much heat is released when 29.5 grams of Cl2 (g) reacts with excess hydrogen?

 

H2 (g) + Cl2 (g) → 2HCl (g)  ΔH° = -186 kJ.

 

1. A) 186 kJ
2. B) 310 kJ
3. C) -77.4 kJ
4. D) -186 kJ
5. E) 77.4 kJ

Answer:  E

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22) The enthalpy change for the following reaction is -483.6 kJ:

 

2H2 (g) + O2 (g) → 2H2O (g)

 

Therefore, the enthalpy change for the following reaction is ________ kJ.

4H2 (g) + 2O2 (g) → 4H2O (g)

483. A) -483.6
484. B) -967.2
485. C) 2.34 × 105
486. D) 483.6
487. E) 967.2

Answer:  B

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23) The value of ΔH° for the reaction below is +128.1 kJ:

 

CH3OH (l) → CO (g) + 2H2 (g)

How many kJ of heat are consumed when 15.5 g of COH (l) decomposes as shown in the equation?

1. A) 0.48 kJ
2. B) 62.0 kJ
3. C) 1.3 × 102kJ
4. D) 32 kJ
5. E) 8.3 kJ

Answer:  B

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24) The value of ΔH° for the reaction below is +128.1 kJ:

 

CH3OH (l) → CO (g) + 2H2 (g)

How much heat is consumed when 87.1 g of hydrogen gas is formed?

2. A) 2.76 × 103kJ
3. B) 5.52 × 103kJ
4. C) -5.52 × 103kJ
5. D) -2.76 × 103kJ
6. E) -128.1 kJ

Answer:  A

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25) The value of ΔH° for the reaction below is +128.1 kJ:

 

CH3OH (l) → CO (g) + 2H2 (g)

How many kJ of heat are consumed when 5.10 g of CO (g) is formed as shown in the equation?

1. A) 0.182 kJ
2. B) 162 kJ
3. C) 8.31 kJ
4. D) 23.3 kJ
5. E) 62.0 kJ

Answer:  D

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26) CH3OH (l) decomposes into carbon monoxide and hydrogen gas in the presence of heat. How much heat is consumed when 5.75 g of CO (g) is formed? ΔH° = +128.1 kJ.

26. A) 26.3 kJ
27. B) 23.3 kJ
28. C) 62.0 kJ
29. D) 162 kJ
30. E) 8.3 kJ

Answer:  A

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27) The value of ΔH° for the reaction below is -1107 kJ:

 

2Ba (s) + O2 (g) → 2BaO (s)

How many kJ of heat are released when 5.75 g of Ba (s) reacts completely with oxygen to form

96. A) 96.3 kJ
97. B) 26.3 kJ
98. C) 46.4 kJ
99. D) 23.2 kJ
100. E) 193 kJ

Answer:  D

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28) The value of ΔH° for the reaction below is -1107 kJ:

 

2Ba (s) + O2 (g) → 2BaO (s)

How many kJ of heat are released when 5.75 g of BaO (s) is produced?

56. A) 56.9 kJ
57. B) 23.2 kJ
58. C) 20.8 kJ
59. D) 193 kJ
60. E) 96.3 kJ

Answer:  C

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29) How many kJ of heat are released when 15.75 g of Ba (s) reacts completely with oxygen gas to form BaO (s)? ΔH° = -1107 kJ.

63. A) 63.5 kJ
64. B) 20.8 kJ
65. C) 114 kJ
66. D) 70.3 kJ
67. E) 35.1 kJ

Answer:  A

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30) The molar heat capacity of an unknown substance is 92.1 J/mol-K. If the unknown has a molar mass of 118 g/mol, what is the specific heat (J/g-K) of this substance?

1. A) 1.28
2. B) -92.1
3. C) 1.09 × 104
4. D) 0.781
5. E) 92.1

Answer:  D

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31) The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of  of lead from 22 °C to 37 °C?

2. A) 2.0 J
3. B) -0.13 J
4. C) 5.8 × 10-4J
5. D) 29 J
6. E) 0.13 J

Answer:  D

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32) The temperature of a 15-g sample of lead metal increases from 22 °C to 37 °C upon the addition of 29.0 J of heat. The specific heat capacity of the lead is ________ J/g-K.

7. A) 7.8
8. B) 1.9
9. C) 29
10. D) 0.13
11. E) -29

Answer:  D

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33) What is the molar heat capacity (in J/mol-K) of liquid bromine? The specific heat of liquid bromine is 0.226 J/g-K.

36. A) 36.1 J/mol-K
37. B) 707 J/mol-K
38. C) 18.1 J/mol-K
39. D) 9.05 J/mol-K
40. E) 0.226 J/mol-K

Answer:  A

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34) The specific heat of liquid bromine is 0.226 J/g-K.  How much heat (J) is required to raise the temperature of 10.0 mL of bromine from 25.00 °C to 27.30 °C? The density of liquid bromine: 3.12 g/mL.

5. A) 5.20 J
6. B) 16.2 J
7. C) 300 J
8. D) 32.4 J
9. E) 10.4 J

Answer:  B

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35) ΔH for the reaction

 

IF5 (g) → IF3 (g) + F2 (g)

 

is ________ kJ, give the data below.

IF (g) + F2 (g) → IF3 (g)    ΔH = -390 kJ

 

IF (g) + 2F2 (g) → IF5 (g)  ΔH = -745 kJ

 

1. A) +355
2. B) -1135
3. C) +1135
4. D) +35
5. E) -35

Answer:  A

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36) Given the following reactions

Fe2O3 (s) + 3CO (s) → 2Fe (s) + 3CO2 (g)  ΔH = -28.0 kJ

 

3Fe (s) + 4CO2(s) → 4CO (g) + Fe3O4(s) ΔH = +12.5 kJ

 

the enthalpy of the reaction of Fe2O3 with CO

3Fe2O3 (s) + CO (g) → CO2 (g) + 2Fe3O4 (s)

 

is ________ kJ.

59. A) -59.0
60. B) 40.5
61. C) -15.5
62. D) -109
63. E) +109

Answer:  A

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37) Given the following reactions

N2 (g) + 2O2 (g) → 2NO2 (g)    ΔH = 66.4 kJ

 

2NO (g) + O2 (g) → 2NO2 (g)   ΔH = -114.2 kJ

the enthalpy of the reaction of the nitrogen to produce nitric oxide

N2 (g) + O2 (g) → 2NO (g)

 

is ________ kJ.

180. A) 180.6
181. B) -47.8
182. C) 47.8
183. D) 90.3
184. E) -180.6

Answer:  A

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38) Given the following reactions

2NO → N2 + O2              ΔH = -180 kJ

 

2NO + O2 → 2NO2         ΔH = -112 kJ

 

the enthalpy of the reaction of nitrogen with oxygen to produce nitrogen dioxide

 

N2 + 2O2 → 2NO2

 

is ________ kJ.

1. A) 68
2. B) -68
3. C) -292
4. D) 292
5. E) -146

Answer:  A

Diff: 3     Var: 1     Page Ref: Sec. 5.6

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39) Given the following reactions

2S (s) + 3O2 (g) → 2SO3 (g)    ΔH = -790 kJ

 

S (s) + O2 (g) → SO2(g)           ΔH = -297 kJ

 

the enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide

 

2SO2 (g) + O2 (g) → 2SO3 (g)

 

is ________ kJ.

1. A) 196
2. B) -196
3. C) 1087
4. D) -1384
5. E) -543

Answer:  B

Diff: 3     Var: 1     Page Ref: Sec. 5.6

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40) Given the following reactions

CaCO3 (s) → CaO (s) + CO2 (g)       ΔH = 178.1 kJ

C (s, graphite) + O2(g) → CO2(g)     ΔH = -393.5 kJ

the enthalpy of the reaction

CaCO3 (s) → CaO (s) + C (s, graphite) + O2 (g)

 

is ________ kJ.

215. A) 215.4
216. B) 571.6
217. C) -215.4
218. D) -571.6
219. E) 7.01 × 104

Answer:  B

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41) Given the following reactions

H2O (l) → H2O (g)                       ΔH = 44.01 kJ

2H2 (g) + O2 (g) → 2H2O (g)      ΔH = -483.64 kJ

the enthalpy for the decomposition of liquid water into gaseous hydrogen and oxygen

2H2O (l) → 2H2 (g) + O2 (g)

 

is ________ kJ.

395. A) -395.62
396. B) -527.65
397. C) 439.63
398. D) 571.66
399. E) 527.65

Answer:  D

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42) Given the following reactions

 

N2 (g) + O2 (g) → 2NO (g)         ΔH = +180.7 kJ

2NO( g) + O2 (g) → 2NO2 (g)    ΔH = -113.1 kJ

the enthalpy for the decomposition of nitrogen dioxide into molecular nitrogen and oxygen

2NO2 (g) → N2 (g) + 2O2 (g)

 

is ________ kJ.

67. A) 67.6
68. B) -67.6
69. C) 293.8
70. D) -293.8
71. E) 45.5

Answer:  B

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43) Given the following reactions

N2 (g) + O2 (g) → 2NO (g)          ΔH = +180.7 kJ

2NO (g) + O2(g) → 2N (g)      ΔH = -113.1 kJ

the enthalpy of reaction for

4NO (g) → 2NO2 (g) + N2 (g)

 

is ________ kJ.

67. A) 67.6
68. B) 45.5
69. C) -293.8
70. D) -45.5
71. E) 293.8

Answer:  C

Diff: 3     Var: 1     Page Ref: Sec. 5.6

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44) Given the following reactions

N2 (g) + O2 (g) → 2NO (g)          ΔH = +180.7 kJ

2N2O (g) → O2 (g) + 2N2 (g)      ΔH = -163.2 kJ

the enthalpy of reaction for

2N2O (g) → 2NO (g) + N2 (g)

 

is ________ kJ.

145. A) 145.7
146. B) 343.9
147. C) -343.9
148. D) 17.5
149. E) -145.7

Answer:  D

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45) The value of ΔH° for the reaction below is -186 kJ.

H2 (g) + Cl2 (g) → 2HCl (g)

 

The value of ΔH°f for HCl (g) is ________ kJ/mol.

3. A) -3.72 × 102
4. B) -1.27 × 102
5. C) -93.0
6. D) -186
7. E) +186

Answer:  C

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46) The value of ΔH° for the following reaction is -3351 kJ:

2Al (s) + 3O2(g) → 2Al2O3(s)

The value of ΔH°f for Al2 (s) is ________ kJ.

1. A) -3351
2. B) -1676
3. C) -32.86
4. D) -16.43
5. E) +3351

Answer:  B

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47) Given the data in the table below, ΔH°rxn for the reaction

 

Ca(OH)2 + 2H3AsO4 → Ca(H2AsO4)2 + 2H2O

 

is ________ kJ.

 

 

 

744. A) -744.9
745. B) -4519
746. C) -4219
747. D) -130.4
748. E) -76.4

Answer:  D

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48) Given the data in the table below, ΔH°rxn for the reaction

 

4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (l)

 

is ________ kJ.

 

 

 

1. A) -1172
2. B) -150
3. C) -1540
4. D) -1892
5. E) The ΔH°fof O2(g) is needed for the calculation.

Answer:  A

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49) Given the data in the table below, ΔH°rxn for the reaction

C2H5OH (l) + O2 (g) → CH3CO2H (l) + H2O (l)

 

is ________ kJ.

 

 

 

79. A) -79.0
80. B) -1048.0
81. C) -476.4
82. D) -492.6
83. E) The value of ΔH°fof O2 (g) is required for the calculation.

Answer:  D

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50) Given the data in the table below, ΔH°rxn for the reaction

3NO2 (g) + H2O (l) → 2HNO3 (aq) + NO (g)

 

is ________ kJ.

 

 

 

1. A) 64
2. B) 140
3. C) -140
4. D) -508
5. E) -64

Answer:  C

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51) Given the data in the table below, ΔH°rxn for the reaction

 

IF5 (g) + F2 (g) → IF7 (g)

 

is ________ kJ.

 

 

 

1. A) 1801
2. B) -1801
3. C) 121
4. D) -121
5. E) -101

Answer:  E

Diff: 3     Var: 1     Page Ref: Sec. 5.7

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52) Given the data in the table below, ΔH° for the reaction

2CO (g) + O2 (g) → 2CO2 (g)

 

is ________ kJ.

 

 

 

566. A) -566.4
567. B) -283.2
568. C) 283.2
569. D) -677.0
570. E) The ΔH°fof O2(g) is needed for the calculation.

Answer:  A

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53) The value of ΔH° for the following reaction is 177.8 kJ. The value of Δ for CaO(s) is ________ kJ/mol.

CaCO3 (s) → CaO (s) + CO2 (g)

 

 

 

1. A) -1600
2. B) -813.4
3. C) -635.5
4. D) 813.4
5. E) 177.8

Answer:  C

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54) Given the data in the table below, ΔH°rxn for the reaction

2Ag2S (s) + O2 (g) → 2Ag2O (s)  + 2S (s)

 

is ________ kJ.

 

 

 

1. A) -1.6
2. B) +1.6
3. C) -3.2
4. D) +3.2
5. E) The ΔH°fof S (s) and of O2(g) are needed for the calculation.

Answer:  D

Diff: 3     Var: 1     Page Ref: Sec. 5.7

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55) Given the data in the table below, ΔH°rxn for the reaction

Ag2O (s) + H2S (g) → Ag2S (s) + H2O (l)

 

is ________ kJ.

 

 

 

1. A) -267
2. B) -370
3. C) -202
4. D) -308
5. E) More data are needed to complete the calculation.

Answer:  A

Diff: 3     Var: 1     Page Ref: Sec. 5.7

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56) Given the data in the table below, ΔH°rxn for the reaction

2SO2 (g) + O2 (g) → 2SO3 (g)

 

is ________ kJ.

 

 

 

1. A) -99
2. B) 99
3. C) -198
4. D) 198
5. E) The ΔH°fof O2(g) is needed for the calculation.

Answer:  C

Diff: 3     Var: 1     Page Ref: Sec. 5.7

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57) Given the data in the table below, ΔH°rxn for the reaction

SO3 (g) + H2O (l) → H2SO4 (l)

 

is ________ kJ.

 

 

 

1. A) -132
2. B) 1496
3. C) 704
4. D) -704
5. E) -2.16 × 103

Answer:  A

Diff: 3     Var: 1     Page Ref: Sec. 5.7

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58) Given the data in the table below, ΔH°rxn for the reaction

3Cl2 (g) + PH3 (g) → PCl3 (g) + 3HCl (g)

 

is ________ kJ.

 

 

 

385. A) -385.77
386. B) -570.37
387. C) 570.37
388. D) 385.77
389. E) The ΔH°fof Cl2(g) is needed for the calculation.

Answer:  B

Diff: 3     Var: 1     Page Ref: Sec. 5.7

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59) Given the data in the table below, ΔH°rxn for the reaction

PCl3 (g) + 3HCl (g) → 3Cl2 (g) + PH3 (g)

 

is ________ kJ.

 

 

 

570. A) -570.37
571. B) -385.77
572. C) 570.37
573. D) 385.77
574. E) The ΔH°fof Cl2(g) is needed for the calculation.

Answer:  C

Diff: 3     Var: 1     Page Ref: Sec. 5.7

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60) Given the data in the table below and ΔH°rxn for the reaction

SO2Cl2 (g) + 2H2O (l) → H2SO4 (l) + 2HCl (g)     ΔH° = -62 kJ

 

ΔH°f of HCl (g) is ________ kJ/mol.

 

 

 

1. A) -184
2. B) 60
3. C) -92
4. D) 30
5. E) Insufficient data are given.

Answer:  C

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61) A 19.5 g candy bar contains 8% protein, 33% fat, and 18% carbohydrate. The respective fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. What is the fuel value (kJ) for this piece of candy?

1. A) 241
2. B) 331
3. C) 27
4. D) 60.0
5. E) 17.0

Answer:  B

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62) A 3.00 L pitcher of sweetened ice tea contains 600. g of sugar. Assuming that the sugar is the only fuel source, what is the fuel value (in kJ) of a 250. mL serving? The respective fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively.

8. A) 8.50 × 102 kJ
9. B) 10.2 × 104kJ
10. C) 2.55 × 103kJ
11. D) 38 kJ
12. E) 17 kJ

Answer:  A

Diff: 3     Var: 1     Page Ref: Sec. 5.9

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63) A typical fast food meal consists of a burger, fries, and a soft-drink and contains 58.0 grams of fat, 39.0 grams of protein, and 177 grams of carbohydrate. If jogging burns 950.0 kJ/hour, how many minutes would it take to completely burn off the meal? The respective fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively.

6. A) 6.19
7. B) 208
8. C) 371
9. D) 17.3
10. E) 9.70

Answer:  C

Diff: 3     Var: 1     Page Ref: Sec. 5.9

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GO:  G7

 

 

64) A slice of cake contains 29.0 grams of fat, 9.0 grams of protein, and 77 grams of carbohydrate. If swimming burns 1000.0 kJ/hour, how many minutes would it take to completely burn off the slice of cake? The respective fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively.

1. A) 154
2. B) 2.56
3. C) 23.4
4. D) 117
5. E) 262

Answer:  A

Diff: 3     Var: 1     Page Ref: Sec. 5.9

LO:  5.1 – 5.11

GO:  G7

 

5.3   Algorithmic Questions

 

1) A 26.9 g rock rolls down the hill at a speed of 81.9 m/s . What is the kinetic energy of the rock?

90. A) 90.2 J
91. B) 145 J
92. C) 0.950 J
93. D) 90200 J
94. E) 1450 J

Answer:  A

Diff: 2     Var: 7     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

 

2) A 23.2 g piece of space debris is traveling at 81.9 m/s. What is the kinetic energy of the space debris?

1. A) 145 J
2. B) 1450 J
3. C) 0.950 J
4. D) 77800 J
5. E) 77.8 J

Answer:  E

Diff: 2     Var: 7     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

 

 

3) At what velocity (m/s) must a  object be moving in order to possess a kinetic energy of

1. A) 0.35 m/s
2. B) 2.8 m/s
3. C) 0.13 m/s
4. D) 0.031 m/s
5. E) 0.016 m/s

Answer:  A

Diff: 2     Var: 50+     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

 

4) At what velocity (m/s) must a 417.3 g object be moving in order to possess a kinetic energy of

1. A) 0.12 m/s
2. B) 26 m/s
3. C) 0.015 m/s
4. D) 0.0038 m/s
5. E) 0.00024 m/s

Answer:  A

Diff: 2     Var: 50+     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

5) When work is done on a system, w will be a ________ value.

1. A) positive
2. B) negative
3. C) very large
4. D) very small
5. E) There is not enough information given to determine the answer.

Answer:  A

Diff: 3     Var: 4     Page Ref: Sec. 5.2

LO:  5.3

GO:  G4

 

6) The value of ΔE for a system that performs 139 kJ of work on its surroundings and gains  of heat is

1. A) -85
2. B) 193
3. C) 7506
4. D) 85
5. E) -193

Answer:  A

Diff: 2     Var: 50+     Page Ref: Sec. 5.2

LO:  5.3

GO:  G4

 

7) The value of ΔE for a system that performs 19 kJ of work on its surroundings and loses  of heat is

1. A) -28
2. B) 28
3. C) 171
4. D) 10
5. E) -10

Answer:  A

Diff: 2     Var: 50+     Page Ref: Sec. 5.2

LO:  5.3

GO:  G4

 

8) Calculate the work (kJ) done during a reaction in which the internal volume expands from  to  against an outside pressure of

7. A) -7.3 kJ
8. B) 17 kJ
9. C) 7.3 kJ
10. D) -17 kJ
11. E) 0 kJ; No work is done.

Answer:  A

Diff: 3     Var: 50+     Page Ref: Sec. 5.3

LO:  5.5

GO:  G4

9) Calculate the work (kJ) done during a reaction in which the internal volume expands from  to  against a vacuum (an outside pressure of

1. A) 0; kJ No work is done.
2. B) 3.6 kJ
3. C) -3.6 kJ
4. D) 6.5 kJ
5. E) -6.5 kJ

Answer:  A

Diff: 3     Var: 50+     Page Ref: Sec. 5.3

LO:  5.5

GO:  G4

 

10) Calculate the work (kJ) done during a reaction in which the internal volume contracts from  to  against an outside pressure of

1. A) 31 kJ
2. B) 43 kJ
3. C) -31 kJ
4. D) -43 kJ
5. E) 0 kJ; No work is done.

Answer:  A

Diff: 3     Var: 50+     Page Ref: Sec. 5.3

LO:  5.5

GO:  G4

 

11) The value of ΔE for a system that performs 151 kJ of work on its surroundings and loses 79 kJ of heat is ________ kJ.

230. A) +230.
231. B) -230.
232. C) +72
233. D) -72
234. E) -151

Answer:  B

Diff: 2     Var: 9     Page Ref: Sec. 5.2

LO:  5.3

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12) Calculate the value of ΔE in joules for a system that loses 115 J of heat and has 150 J of work performed on it by the surroundings.

1. A) -115 J
2. B) -35 J
3. C) +35 J
4. D) +265 J
5. E) -265 J

Answer:  C

Diff: 2     Var: 10     Page Ref: Sec. 5.2

LO:  5.3

GO:  G4

13) The value of ΔH° for the reaction below is -72 kJ.  ________ kJ of heat are released when 5.5 mol of HBr is formed in this reaction.

 

H2 (g) + Br2 (g) → 2HBr (g)

 

1. A) 144
2. B) 72
3. C) 0.44
4. D) 198
5. E) -72

Answer:  D

Diff: 2     Var: 12     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

 

 

14) The value of ΔH° for the reaction below is -126 kJ. The amount of heat that is released by the reaction of 10.0 g of Na2O2 with water is ________ kJ.

 

2Na2O2 (s) + 2H2O (l) → 4NaOH (s) + O2 (g)

 

8. A) 8.08
9. B) 16.2
10. C) 67.5
11. D) 32.3
12. E) -126

Answer:  A

Diff: 3     Var: 9     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

 

15) The value of ΔH° for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 10.0 g of CO (g) reacts completely.

2CO (g) + O2 (g) → 2CO2 (g)

 

1. A) 2410 kJ
2. B) 172 kJ
3. C) 86.0 kJ
4. D) 482 kJ
5. E) -482 kJ

Answer:  C

Diff: 3     Var: 8     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

16) In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water:

 

CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) △H = -890.0 kJ

 

Calculate the value of q (kJ) in this exothermic reaction when 1.80 g of methane is combusted at constant pressure.

100. A) -100.1 kJ
101. B) 0.0324 kJ
102. C) -0.0100 kJ
103. D) 30.9 kJ
104. E) -1.00 × 105kJ

Answer:  A

Diff: 3     Var: 10     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

 

17) Hydrogen peroxide decomposes to water and oxygen at constant pressure (△H = -196 kJ).  What is the value of q (kJ) for this reaction when 4.60 g of hydrogen peroxide decomposes at constant pressure?

26. A) -26.5 kJ
27. B) -0.0189 kJ
28. C) 1.25 kJ
29. D) -2.65 × 104kJ
30. E) -13.3 kJ

Answer:  E

Diff: 3     Var: 10     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

 

18) The combustion of titanium with oxygen produces titanium dioxide:

 

Ti (s) + O2(g) → TiO2 (s)

 

When 0.610 g of titanium is combusted in a bomb calorimeter, the temperature of the calorimeter increases from 25.00 °C to 50.50 °C. In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ/K. The heat of reaction for the combustion of a mole of Ti in this calorimeter is ________ kJ/mol.

2. A) 2.09
3. B) 4.14
4. C) -311
5. D) -0.154
6. E) -1.98 ×

Answer:  E

Diff: 4     Var: 15     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

19) A sample of aluminum metal absorbs 11.2 J of heat, upon which the temperature of the sample increases from 23.2 °C to 30.5 °C. Since the specific heat capacity of aluminum is 0.90 J/g-K, the mass of the sample is ________ g.

1. A) 72
2. B) 1.7
3. C) 10.
4. D) 65
5. E) 7.3

Answer:  B

Diff: 3     Var: 8     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

 

20) A sample of calcium carbonate [CaCO3 (s)] absorbs  of heat, upon which the temperature of the sample increases from  to  If the specific heat of calcium carbonate is  what is the mass (in grams) of the sample?

7. A) 7.6 g
8. B) 5.1 g
9. C) -7.6 g
10. D) 0.13 g
11. E) 5.3 g

Answer:  A

Diff: 3     Var: 50+     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

21) How many joules of heat are absorbed when the temperature of a 13.9 g sample of CaCO3 (s) increases from  to  Specific heat of calcium carbonate is

1. A) 130 J
2. B) 0.68 J
3. C) s-130 J
4. D) -0.68 J
5. E) 9.5 J

Answer:  A

Diff: 3     Var: 50+     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

22) An 6.11 g sample of calcium carbonate [CaCO3 (s)] absorbs  of heat, upon which the temperature of the sample increases from  to  What is the specific heat of calcium carbonate?

1. A) 0.82 J/g-K
2. B) -0.82 J/g-K
3. C) 31 J/g-K
4. D) 230 J/g-K
5. E) 8600 J/g-K

Answer:  A

Diff: 3     Var: 50+     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

23) A sample of iron absorbs 81.0 J of heat, upon which the temperature of the sample increases from  to  If the specific heat of iron is 0.450 J/g-K, what is the mass (in grams) of the sample?

21. A) 21.2 g
22. B) 4.29 g
23. C) -21.2 g
24. D) 0.0472 g
25. E) 3.83 g

Answer:  A

Diff: 3     Var: 50+     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

24) The temperature of a 35.1 g sample of iron increases from  to  If the specific heat of iron is  how many joules of heat are absorbed?

1. A) 115 J
2. B) 0.0936 J
3. C) -115 J
4. D) 0.722 J
5. E) 3.29 J

Answer:  A

Diff: 3     Var: 50+     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

25) A 22.9 g sample of iron absorbs 155 J of heat, upon which the temperature of the sample increases from  to  What is the specific heat of iron?

1. A) 0.451 J/g-K
2. B) -0.451 J/g-K
3. C) 237 J/g-K
4. D) 102 J/g-K
5. E) 53,200 J/g-K

Answer:  A

Diff: 3     Var: 50+     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

 

26) The specific heat capacity of liquid water is 4.18 J/g-K. How many joules of heat are needed to raise the temperature of 7.25 g of water from 20.0 °C to 44.1 °C?

41. A) 41.8 J
42. B) 730 J
43. C) 1.94 × J
44. D) 2.39 × J
45. E) 66.8 J

Answer:  B

Diff: 3     Var: 15     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

27) The specific heat capacity of methane gas is 2.20 J/g-K. How many joules of heat are needed to raise the temperature of 7.25 g of methane from 22.0 °C to 57.0 °C?

1. A) 115 J
2. B) 558 J
3. C) 1.26 × 103 J
4. D) 8.67 × 10-3 J
5. E) 41.3 J

Answer:  B

Diff: 3     Var: 15     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

28) The specific heat capacity of liquid mercury is 0.14 J/g-K. How many joules of heat are needed to raise the temperature of 6.00 g of mercury from 25.1 °C to 65.3 °C?

1. A) 1.7 × 103J
2. B) 34 J
3. C) 76 J
4. D) 5.8 × 10-4 J
5. E) 2.2 J

Answer:  B

Diff: 3     Var: 15     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

 

29) How much heat is required to raise the temperature of a 1.15 kg piece of copper metal from 25.0 °C to 77.5 °C? The specific heat capacity of solid copper metal is 0.385 J/g-K.

2. A) 2.32 × J
3. B) 1.57 × J
4. C) 23.2 J
5. D) 6.38 × J
6. E) 0.00638 J

Answer:  A

Diff: 3     Var: 15     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

30) A 4.50-g sample of liquid water at 25.0 °C is heated by the addition of 133 J of energy. The final temperature of the water is ________ °C. The specific heat capacity of liquid water is

1. A) 149
2. B) 25.1
3. C) -17.9
4. D) 32.1
5. E) 7.07

Answer:  D

Diff: 3     Var: 20     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

31) A 10.1 g sample of NaOH is dissolved in 250.0 g of water in a coffee-cup calorimeter. The temperature increases from 23.0 °C to ________°C. Specific heat of liquid water is 4.18 J/g-K and ΔH for the dissolution of sodium hydroxide in water is 44.4 kJ/mol.

35. A) 35.2
36. B) 24.0
37. C) 33.7
38. D) 33.3
39. E) 40.2

Answer:  D

Diff: 4     Var: 8     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

 

32) A 50.0-g sample of liquid water at 25.0 °C is mixed with 23.0 g of water at 79.0 °C. The final temperature of the water is ________ °C.

1. A) 123
2. B) 27.3
3. C) 52.0
4. D) 231
5. E) 42.0

Answer:  E

Diff: 3     Var: 30     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

33) A 5.00-g sample of copper metal at 25.0 °C is heated by the addition of 133 J of energy. The final temperature of the copper is ________ °C. The specific heat capacity of copper is

35. A) 35.1
36. B) 25.0
37. C) 45.0
38. D) 95.0
39. E) 70.0

Answer:  D

Diff: 3     Var: 20     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

34) The temperature of a 24.3 g sample of gold increases from  to  If the specific heat of gold is  how many joules of heat are absorbed?

24. A) 24.5 J
25. B) 0.0414 J
26. C) -24.5 J
27. D) 0.293 J
28. E) 1.01 J

Answer:  A

Diff: 3     Var: 50+     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

35) What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 mL of solution having a density of 1.25 g/mL by 3.33 °C? (The specific heat of the solution is 3.74 J/g-K.)

7. A) -7.43 kJ
8. B) -12.51 kJ
9. C) 8.20 kJ
10. D) -3.89 kJ
11. E) 6.51 kJ

Answer:  D

Diff: 4     Var: 10     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

36) An 8 oz. bottle of energy drink contains 6.0 g of protein, 2.0 g of fat, and 16.3 g of carbohydrate. The fuel value of this energy drink bottle is ________ kJ. The fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively.

1. A) 520
2. B) 280
3. C) 720
4. D) 460
5. E) 72

Answer:  D

Diff: 3     Var: 9     Page Ref: Sec. 5.9

LO:  5.1 – 5.11

GO:  G7

 

5.4   Short Answer Questions

 

1) ________ is defined as the energy used to move an object against a force.

Answer:  Work

Diff: 2     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G4

 

2) The ΔHvap of water is 40.7 kJ at 100 °C. How much liquid water in grams can be converted to vapor if 5950 J of heat are absorbed?

Answer:  2.63 grams

Diff: 3     Var: 1     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

 

3) The ΔHvap of water is 40.7 kJ at 100 °C. How much heat energy is required to convert 15.0 grams of liquid water to vapor.

Answer:  33.9 kJ

Diff: 3     Var: 1     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

4) When 0.800 grams of NaOH is dissolved in 100.0 grams of water, the temperature of the solution increases from 25.00 °C to 27.06 °C. The amount of heat absorbed by the water is ________ J. (The specific heat of water is 4.18 J/g-°C.)

Answer:           868

Diff: 3     Var: 1     Page Ref: Sec. 5.5

LO:  5.8

GO:  G4

 

5) The ΔHrxn for the combustion of methane is -890.0 kJ. How much heat energy (kJ) is released if 82.1 grams of methane are burned in an excess amount of oxygen?

Answer:  4555 kJ

Diff: 3     Var: 1     Page Ref: Sec. 5.4

LO:  5.7

GO:  G4

 

6) The ________ of a reaction is the enthalpy change when all reactants and products are at 1 atm pressure and a specific temperature.

Answer:  standard enthalpy change

Diff: 2     Var: 1     Page Ref: Sec. 5.7

LO:  5.10a

GO:  G2

 

7) Coal contains hydrocarbons of high molecular weight as well as compounds containing ________, sulfur, or nitrogen.

Answer:  oxygen

Diff: 2     Var: 1     Page Ref: Sec. 5.9

LO:  5.1 – 5.11

GO:  G7

 

5.5   True/False Questions

 

1) Work equals mass times distance.

Answer:  FALSE

Diff: 1     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G2

 

2) One joule equals 1 kg-m2/s2.

Answer:  TRUE

Diff: 2     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G2

 

 

3) Energy units include watts, volts, and newtons.

Answer:  FALSE

Diff: 1     Var: 1     Page Ref: Sec. 5.1

LO:  5.1

GO:  G2

 

4) The primary component of natural gas is methane.

Answer:  TRUE

Diff: 1     Var: 1     Page Ref: Sec. 5.9

LO:  5.1 – 5.11

GO:  G2

 

5) Renewable energy sources are essentially exhaustible.

Answer:  FALSE

Diff: 1     Var: 1     Page Ref: Sec. 5.9

LO:  5.1 – 5.11

GO:  G2

 

6) Petroleum is a liquid that can be refined to produce fuels such as gasoline, diesel oil, and kerosene.

Answer:  TRUE

Diff: 2     Var: 1     Page Ref: Sec. 5.9

LO:  5.1 – 5.11

GO:  G2