Download ExamView - Quiz 3--Heat and Thermo PRACTICE.tst

Name: ________________________ Class: ___________________ Date: __________
ID: A
Ch 9 (Heat) & Ch 10 (Thermo) Quiz PRACTICE
Multiple Choice
Identify the choice that best completes the statement or answers the question.
1. What happens to the internal energy of an ideal gas when it is heated from 0°C to 4°C?
a. It increases. b. It decreases. c. It remains constant. d. It is impossible to determine.
2. Which of the following is proportional to the kinetic energy of atoms and molecules?
a. elastic energy b. temperature c. potential energy d. thermal equilibrium
3. As the temperature of a substance increases, its volume tends to increase due to
a. thermal equilibrium. b. thermal energy. c. thermal expansion. d. thermal contraction.
4. What is the temperature of a system in thermal equilibrium with another system made up of ice and water at 1 atm of
pressure?
a. 0°F b. 273 K c. 0 K d. 100°C
5. If two small beakers of water, one at 70°C and one at 80°C, are emptied into a large beaker, what is the final temperature of
the water?
a. The final temperature is less than 70°C. b. The final temperature is greater than 80°C. c. The final temperature is
between 70°C and 80°C. d. The water temperature will fluctuate.
6. Which of the following is not a widely used temperature scale?
a. Kelvin b. Fahrenheit c. Celsius d. Joule
7. A substance registers a temperature change from 20°C to 40°C. To what incremental temperature change does this
correspond?
a. 20°F b. 40°F c. 36°F d. 313°F
8. A substance registers a temperature change from 20°C to 40°C. To what incremental temperature change does this
correspond?
a. 20 K b. 40 K c. 36 K d. 313 K
9. The use of fiberglass insulation in the outer walls of a building is intended to minimize heat transfer through what process?
a. conduction b. radiation c. convection d. vaporization
10. If energy is transferred from a table to a block of ice moving across the table, which of the following statements is true?
a. The table and the ice are at thermal equilibrium. b. The ice is cooler than the table. c. The ice is no longer 0°C.
d. Energy is being transferred from the ice to the table.
11. To which of the following is high temperature related?
a. low particle kinetic energy b. high particle kinetic energy c. large volume d. zero net energy transfer
12. Energy transfer as heat between two objects depends on which of the following?
a. The difference in mass of the two objects. b. The difference in volume of the two objects. c. The difference in
temperature of the two objects. d. The difference in composition of the two objects.
13. Why does sandpaper get hot when it is rubbed against rusty metal?
a. Energy is transferred from the sandpaper into the metal. b. Energy is transferred from the metal to the sandpaper.
c. Friction between the sandpaper and metal increases the temperature of both. d. Energy is transferred from a hand to the
sandpaper.
1
Name: ________________________
ID: A
14. In the presence of friction, not all of the work done on a system appears as mechanical energy. What happens to the rest of
the energy provided by work?
a. The remaining energy is stored as mechanical energy within the system. b. The remaining energy is dissipated as
sound. c. The remaining energy causes a decrease in the internal energy of the system. d. The remaining energy causes
an increase in the internal energy of the system.
15. In an elastic collision between two ball bearings, kinetic energy is conserved. If there is no change in potential energy, which
of the following is true?
a. ∆U > 0 b. ∆U = 0 c. ∆U < 0 d. ∆U cannot be determined for this event.
16. Which of the following is a set of particles or interacting components to which energy is added or from which energy is
removed?
a. an ideal gas b. an engine c. a system d. an environment
17. When an ideal gas does positive work on its surroundings, which of the gas’s quantities increases?
a. temperature b. volume c. pressure d. internal energy
18. What thermodynamic process for an ideal gas system has an unchanging internal energy and a heat intake that corresponds
to the value of the work done by the system?
a. isovolumetric b. isobaric c. adiabatic d. isothermal
19. Which thermodynamic process takes place at a constant temperature so that the internal energy of a system remains
unchanged?
a. isovolumetric b. isobaric c. adiabatic d. isothermal
20. Which thermodynamic process takes place at constant volume so that no work is done on or by the system?
a. isovolumetric b. isobaric c. adiabatic d. isothermal
21. According to the first law of thermodynamics, the difference between energy transferred to or from a system as heat and
energy transferred to or from a system by work is equivalent to which of the following?
a. entropy change b. internal energy change c. volume change d. pressure change
22. How is conservation of internal energy expressed for a system during an adiabatic process?
a. Q = W = 0, so ∆U = 0 and U i = U f b. Q = 0, so ∆U = –W c. ∆T = 0, so ∆U = 0; therefore, ∆U = Q – W = 0, or Q =
W d. ∆V = 0, so P∆V = 0 and W = 0; therefore, ∆U = Q
23. How is conservation of internal energy expressed for a system during an isovolumetric process?
a. Q = W = 0, so ∆U = 0 and U i = U f b. Q = 0, so ∆U = –W c. ∆T = 0, so ∆U = 0; therefore, ∆U = Q – W = 0, or Q =
W d. ∆V = 0, so P∆V = 0 and W = 0; therefore, ∆U = Q
24. An ideal gas system undergoes an adiabatic process in which it expands and does 20 J of work on its environment. How
much energy is transferred to the system as heat?
a. –20 J b. 0 J c. 5 J d. 20 J
25. Which of the following is a thermodynamic process in which a system returns to the same conditions under which it started?
a. an isovolumetric process b. an isothermal process c. a cyclic process d. an adiabatic process
26. Which of the following is not a way in which a cyclic process resembles an isothermal process?
a. Energy can be transferred as work. b. Energy can be transferred as heat. c. The temperature of the system remains
constant throughout the process. d. There is no net change in the internal energy of the system.
27. Which equation describes the net work done for a complete cycle of a heat engine?
a. Wnet = Q − ∆U b. Wnet = Q h − Q c c. Wnet = Q c − Q h d. Wnet = P∆V
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Name: ________________________
ID: A
28. The requirement that a heat engine must give up some energy at a lower temperature in order to do work corresponds to
which law of thermodynamics?
a. first b. second c. third d. No law of thermodynamics applies.
29. A heat engine has taken in energy as heat and used a portion of it to do work. What must happen next for the engine to
complete the cycle and return to its initial conditions?
a. It must give up energy as heat to a lower temperature so work can be done on it. b. It must give up energy as heat to a
higher temperature so work can be done on it. c. It must do work to transfer the remaining energy as heat to a lower
temperature. d. It must do work to transfer the remaining energy as heat to a higher temperature.
30. Which of the following is a way to improve the efficiency of a heat engine?
a. increase Q h b. reduce Q h c. reduce W net d. increase Q c
31. An ideal heat engine has an efficiency of 50 percent. Which of the following statements is not true?
a. The amount of energy exhausted as heat equals the energy added to the engine as heat. b. The amount of work done is
half the energy added to the engine as heat. c. The amount of energy exhausted as heat is half the energy added to the
engine as heat. d. The amount of energy exhausted as heat equals the work done.
32. Imagine you could observe the individual atoms that make up a piece of matter and that you observe the motion of the atoms
becoming more orderly. What can you assume about the system?
a. It is gaining thermal energy. b. Its entropy is increasing. c. Its entropy is decreasing. d. Positive work is being
done on the system.
33. When a drop of ink mixes with water, what happens to the entropy of the system?
a. The system’s entropy increases, and the total entropy of the universe increases. b. The system’s entropy decreases, and
the total entropy of the universe increases. c. The system’s entropy increases, and the total entropy of the universe
decreases. d. The system’s entropy decreases, and the total entropy of the universe decreases.
34. Which statement applies when all of the entropy changes in a process are taken into account?
a. The increases in entropy are always less than the decreases. b. The increases in entropy are always equal to the
decreases. c. The increases in entropy are always greater than the decreases. d. The increases in entropy can be greater
or less than the decreases.
35. A thermodynamic process occurs, and the entropy of a system decreases. What can be concluded about the entropy change of
the environment?
a. It decreases. b. It increases. c. It stays the same. d. It could increase or decrease, depending on the process.
36. Which of the following is a direct cause of a substance’s temperature increase?
a. Energy is removed from the particles of the substance. b. Kinetic energy is added to the particles of the substance.
c. The number of atoms and molecules in a substance changes. d. The volume of the substance decreases.
37. What are the energies associated with atomic motion called?
a. kinetic energy b. potential energy c. bond energy d. internal energy
38. Which of the following best describes the relationship between two systems in thermal equilibrium?
a. No net energy is exchanged. b. The volumes are equal. c. The masses are equal. d. The velocity is zero.
39. Energy transferred as heat occurs between two bodies in thermal contact when they differ in which of the following
properties?
a. mass b. specific heat c. density d. temperature
40. Which of the following terms describes a transfer of energy?
a. heat b. internal energy c. temperature d. kinetic energy
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Name: ________________________
ID: A
41. How is energy transferred as heat always directed?
a. from an object at low temperature to an object at high temperature b. from an object at high temperature to an object at
low temperature c. from an object at low kinetic energy to an object at high kinetic energy d. from an object with higher
mass to an object of lower mass
42. A nail is driven into a board with an initial kinetic energy of 150 J. If the potential energy before and after the event is the
same, what is the change in the internal energy of the board and nail?
a. 150 J b. 75 J c. 0 J d. −150 J
Problem
43. A falling stone with a mass of 0.255 kg strikes the ground. Assuming that the stone is initially at rest when it begins falling,
how high must the stone be above the ground for the internal energy of the stone and ground to increase by 2450 J?
(g = 9.81 m/s 2 )
44. A container of gas is at a pressure of 3.7 × 10 5 Pa. How much work is done by the gas if its volume expands by 1.6 m 3 ?
45. A cylinder has a radius of 0.080 m. How much work is done by a gas in the cylinder if the gas exerts a constant pressure of
7.8 × 10 5 Pa on the piston, moving it a distance of 0.060 m?
46. A total of 165 J of work is done on a gaseous refrigerant as it undergoes compression. If the internal energy of the gas
increases by 123 J during the process, what is the total amount of energy transferred as heat?
47. Over several cycles, a refrigerator compressor does work on the refrigerant. This work is equivalent to a constant pressure of
4.13 × 10 5 Pa compressing a circular piston with a radius of 0.019 m a distance of 25.0 m. If the change in the refrigerant’s
internal energy is 0 J after each cycle, how much heat will the refrigerant remove from within the refrigerator?
48. A steam engine takes in 2.06 × 10 5 J of energy added as heat and exhausts 1.53 × 10 5 J of energy removed as heat per cycle.
What is its efficiency?
49. A warm day has a high temperature of 38.0°C. What is this temperature in degrees Fahrenheit?
50. The temperature of an object is measured as 500.0 K. What is this temperature in degrees Celsius?
51. What temperature on the Celsius scale is the equivalent of 88.0°F?
52. Liquid oxygen has a temperature of –183°C. What is this temperature in kelvins?
53. The temperature of an oxygen tank is at 261 K, and the temperature of a nitrogen tank is 11°C. How much greater is the
temperature of the nitrogen tank? (Express the answer in kelvins.)
54. The average normal body temperature for human beings is 98.6°F. What does this temperature equal in kelvins?
55. The surface temperature of Venus is 737 K. What is this temperature in degrees Fahrenheit?
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ID: A
Ch 9 (Heat) & Ch 10 (Thermo) Quiz PRACTICE
Answer Section
MULTIPLE CHOICE
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1
9-1.1
9-1.1
9-1.2
9-1.2
9-1.2
9-1.3
9-1.3
9-1.3
9-2.1
9-2.1
9-2.2
9-2.2
9-2.2
9-2.3
9-2.3
10-1.1
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10-3.3
9-1.1
9-1.1
9-1.2
9-2.1
9-2.1
9-2.1
ID: A
42. ANS: A
Given
KE i = 150 J
KE f = 0 J
∆PE = 0 J
Solution
The nail comes to rest in the board, so the final kinetic energy equals zero. Thus the change in kinetic energy is 150 J. From
the conservation of energy,
∆PE + ∆KE + ∆U = 0
0 + KE f − KEi + ∆U = 0
∆U = KEi = 150 J
PTS:
1
DIF:
IIIA
OBJ:
9-2.3
PROBLEM
43. ANS:
979 m
Given
m = 0.255 kg
∆U = 2450 J
g = 9.81 m/s 2
Solution
∆PE + ∆KE + ∆U = 0
The kinetic energy increases with the decrease in potential energy, and then decreases with the increase in the internal
energy of the water. Thus, the net change in kinetic energy is zero.
∆PE + ∆U = 0
Assuming final potential energy has a value of zero, the change in the internal energy equals:
0 − PEi + ∆U = 0
∆U = PE i = mgh
h=
∆U
2450 J
=
= 979 m
mg
(0.255 kg)(9.81 m/s 2 )
PTS:
1
DIF:
IIIB
OBJ:
9-2.3
2
ID: A
44. ANS:
5.9 × 10 5 J
Given
P = 3.7 × 10 5 Pa
∆V = 1.6 m 3
Solution
W = P∆V = (3.7 × 10 5 Pa)(1.6 m 3 ) = 5.9 × 10 5 J
PTS: 1
45. ANS:
DIF:
IIIA
OBJ:
10-1.2
9.4 × 10 2 J
Given
r = 0.080 m
P = 7.8 × 10 5 Pa
d = 0.060 m
Solution
Work is done by the gas, so W is positive.
W = P∆V = PAd
A = πr 2
W = PAd = Pπ r 2 d = (7.8 × 10 5 Pa)(π )(0.080 m) 2 (0.060 m)
P = 9.4 × 10 2 J
PTS: 1
DIF: IIIB
OBJ:
46. ANS:
–42 J, or 42 J transferred from the system as heat
10-1.2
Given
W = –165 J
∆U = 123 J
Solution
Work is done on the system, so W is negative.
∆U = Q − W
Q = ∆U + W = 123 J + (–165 J) = − 42 J, or 42 J transferred from the system as heat
PTS:
1
DIF:
IIIA
OBJ:
10-2.2
3
ID: A
47. ANS:
–1.2 × 10 4 J
Given
P = 4.13 × 10 5 Pa
r = 0.019 m
d = 25.0 m
∆U = 0 J
Solution
∆U = Q − W = 0
Work is done on the system, so W is negative.
W = P∆V = −PAd
A = πr 2
Q = W = −Pπ r 2 d
Q = −(4.13 × 10 5 Pa)(π )(0.019 m) 2 (25.0 m) = −1.2 × 10 4 J
PTS: 1
48. ANS:
0.257
DIF:
IIIB
OBJ:
10-2.2
OBJ:
10-3.2
Given
Q h = 2.06 × 10 5 J
Q c = 1.53 × 10 5 J
Solution
eff = 1 −
eff = 1 −
Qc
Qh
1.53 × 10 5 J
2.06 × 10 5 J
PTS: 1
49. ANS:
100.4°F
= 1 − 0.743 = 0.257
DIF:
IIIA
Given
T C = 38.0°C
Solution
TF =
9
5
T C + 32.0
ÁÊ
T F = ÁÁÁÁ
Ë
9
5
PTS:
1
˜ˆ
(38.0) + 32.0 ˜˜˜˜ °F = (68.4 + 32.0)°F = 100.4°F
¯
DIF:
IIIA
OBJ:
9-1.3
4
ID: A
50. ANS:
226.8°C
Given
T = 500.0 K
Solution
T = T C + 273.15
T C = T − 273.15 = (500.0 − 273.15)°C = 226.8°C
PTS: 1
51. ANS:
31.1°C
DIF:
IIIA
OBJ:
9-1.3
Given
T F = 88.0°F
Solution
TF =
9
5
T C + 32.0
TC =
5
9
(T F − 32.0) =
PTS: 1
52. ANS:
5
9
(88.0 − 32.0)°C =
DIF:
IIIA
5
9
(56.0)°C = 31.1°C
OBJ:
9-1.3
IIIA
OBJ:
9-1.3
IIIB
OBJ:
9-1.3
9.0 × 10 1 K
Given
T C = –183°C
Solution
T = T C + 273.15
T = (−183 + 273.15) K = 9.0 × 10 1 K
PTS: 1
53. ANS:
23 K
DIF:
Given
T C, nitrogen = 11°C
T oxygen = 261 K
Solution
T = T C + 273.15
T = (11 + 273.15) K = 284 K
∆T = 284 K − 261 K = 23 K
PTS:
1
DIF:
5
ID: A
54. ANS:
3.10 × 10 2 K
Given
T F = 98.6°F
Solution
TF =
9
5
T C + 32.0
TC =
5
9
(T F − 32.0)
T = T C + 273.15 =
ÁÊ
T = ÁÁÁÁ
Ë
5
9
5
9
(T F − 32.0) + 273.15
˜ˆ
(98.6 − 32.0) + 273.15 ˜˜˜˜ K =
¯
PTS: 1
55. ANS:
867°F
DIF:
ÁÊÁÁ
ÁÁ
Ë
5
9
˜ˆ
(66.6) + 273.15 ˜˜˜˜ K = (37.0 + 273.15) K = 3.10 × 10 2 K
¯
IIIB
OBJ:
9-1.3
Given
T = 737 K
Solution
T = T C + 273.15
T C = T − 273.15
TF =
9
5
T C + 32.0 =
ÊÁ
T F = ÁÁÁÁ
Ë
9
5
PTS:
1
9
5
(T − 273.15) + 32.0
ˆ˜
(737 − 273.15) + 32.0 ˜˜˜˜ °F =
¯
DIF:
IIIB
ÊÁÁ
ÁÁÁ
Ë
9
5
ˆ˜
(464) + 32.0 ˜˜˜˜ °F = (835 + 32.0)°F = 867°F
¯
OBJ:
9-1.3
6