1. If two objects are in thermal equilibrium with each other
A.they cannot be moving
B.they cannot be undergoing an elastic collision
C.they cannot have different pressures
D.they cannot be at different temperatures
E.they cannot be falling in the Earth's gravitational field


2. A balloon is filled with cold air and placed in a warm room. It is NOT in thermal equilibrium with the air of the room until
A.it rises to the ceiling
B.it sinks to the floor
C.it stops expanding
D.it starts to contract
E.none of the above


3. Suppose object C is in thermal equilibrium with object A and with object B. The zeroth law of thermodynamics states:
A.that C will always be in thermal equilibrium with both A and B
B.that C must transfer energy to both A and B
C.that A is in thermal equilibrium with B
D.that A cannot be in thermal equilibrium with B
E.nothing about the relationship between A and B


4. The zeroth law of thermodynamics allows us to define
A.work
B.pressure
C.temperature
D.thermal equilibrium
E.internal energy


5. If the zeroth law of thermodynamics were not valid, which of the following could not be considered a property of an object?
A.Pressure
B.Center of mass energy
C.Internal energy
D.Momentum
E.Temperature


6. When a certain constant volume gas thermometer is in thermal contact with water at its triple point (273.16 K) the pressure is 6.30 × 104 Pa. For this thermometer a kelvin corresponds to a change in pressure of about:
A.4.34 × 102 Pa
B.2.31 × 102 Pa
C.1.72 × 103 Pa
D.2.31 × 103 Pa
E.1.72 × 107 Pa


7. Room temperature is about 20 degrees on the:
A.Kelvin scale
B.Celsius scale
C.Fahrenheit scale
D.absolute scale
E.C major scale


8. Heat has the same units as:
A.temperature
B.work
C.energy/time
D.heat capacity
E.energy/volume


9. The heat capacity of an object is:
A.the amount of heat energy to raise its temperature by 1°C
B.the amount of heat energy to change its state without changing its temperature
C.the amount of heat energy per kilogram to raise its temperature by 1°C
D.the ratio of its specific heat to that of water
E.the change in its temperature caused by adding 1 J of heat


10. The specific heat of an object is:
A.the amount of heat energy to change the state of one gram of the substance
B.the amount of heat energy per unit mass emitted by oxidizing the substance
C.the amount of heat energy per unit mass to raise the substance from its freezing to its boiling point
D.the amount of heat energy per unit mass to raise the temperature of the substance by 1 °C
E.the temperature of the object divided by its mass


11. Two different samples have the same mass and temperature. Equal quantities of heat are absorbed as heat by each. Their final temperatures may be different because the samples have different:
A.thermal conductivities
B.coefficients of expansion
C.densities
D.volumes
E.heat capacities


12. The same energy Q enters five different substances as heat.
A.The temperature of 3 g of substance A by 10 K
B.The temperature of 4 g of substance B by 4 K
C.The temperature of 6 g of substance C by 15 K
D.The temperature of 8 g of substance D by 5 K
E.The temperature of 10 g of substance E by 10 K
Which of these has the greatest specific heat?


13. For constant volume processes the heat capacity of gas A is greater than the heat capacity of gas B. We conclude that when they both absorb the same energy as heat at constant volume:
A.the temperature of A increases more than the temperature of B
B.the temperature of B increases more than the temperature of A
C.the internal energy of A increases more than the internal energy of B
D.the internal energy of B increases more than the internal energy of A
E.A does more positive work than B


14. The heat capacity at constant volume and the heat capacity at constant pressure have different values because:
A.heat increases the internal energy at constant volume but not at constant pressure
B.heat increases the internal energy at constant pressure but not at constant volume
C.the system does work at constant volume but not at constant pressure
D.the system does work at constant pressure but not at constant volume
E.the system does more work at constant volume than at constant pressure


15. A cube of aluminum is 20 cm on edge. Aluminum has a density 2.7 times that of water (1 g/cm3)and a specific heat 0.217 times that of water (1 cal/g×C). The heat in calories needed to raise the temperature of the cube from 20°C to 30°C is about:
A.27
B.37
C.47
D.27000
E.47000


16. A insulated container, filled with water, contains a thermometer and a paddle wheel. The paddle wheel can be rotated by an external source. This apparatus can be used to determine:
A.specific heat of water
B.relation between kinetic energy and absolute temperature
C.thermal conductivity of water
D.efficiency of changing work into heat
E.mechanical equivalent of heat


17. Take the mechanical equivalent of heat as 4 J/cal. A 10-gram bullet moving at 2000 m/s plunges into 1 kg of paraffin wax (specific heat 0.7 cal/g ×°C). The wax was initially at 20°C. Assuming that all the bullet's energy heats the wax, its final temperature (°C) is:
A.20.14
B.23.5
C.20.006
D.27.1
E.30.23


18. The energy given off by 300 grams of an alloy as it cools through 50°C raises the temperature of 300 grams of water from 30°C to 40°C. The specific heat of the alloy (in cal/g ×°C) is:
A.0.015
B.0.10
C.0.15
D.0.20
E.0.50


19. Object A, with heat capacity CA and initially at temperature TA, is placed in thermal contact with object B, with heat capacity CB and initially at temperature TB. The combination is thermally isolated. If the heat capacities are independent of the temperature and no phase changes occur, the final temperature of both objects is:
A.(CATA – CBTB)/(CA + CB)
B.(CATA + CBTB)/(CA + CB)
C.(CATA – CBTB)/(CA – CB)
D.(CA – CB)çTA – TBç
E.(CA + CB)çTA – TBç


20. The heat of fusion of water is 333 kJ/kg. This means 333 kJ of heat are required to:
A.raise the temperature of 1 kg of water by 1 K
B.turn 1 kg of water to steam
C.raise the temperature of 1 kg of ice by 1 K
D.melt 1 kg of ice
E.increase the internal energy of 1 kg of water by 1 kJ


21. During the time that latent heat is involved in a change of state:
A.the temperature does not change
B.the substance always expands
C.a chemical reaction takes place
D.molecular activity remains constant
E.kinetic energy changes into potential energy


22. The formation of ice from water is accompanied by:
A.absorption of energy as heat
B.temperature increase
C.decrease in volume
D.an evolution of heat
E.temperature decrease


23. How many calories are required to change one gram of 0°C ice to 100°C steam? The latent heat of fusion is 80 cal/g and the latent heat of vaporization is 540 cal/g. The specific heat of water is 1.00 cal/g × K.
A.100
B.540
C.620
D.720
E.900


24. According to the first law of thermodynamics, applied to a gas, the increase in the internal energy during any process:
A.equals the heat input minus the work done on the gas
B.equals the heat input plus the work done on the gas
C.equals the work done on the gas minus the heat input
D.is independent of the heat input
E.is independent of the work done on the gas


25.

Pressure vs. volume graphs for a certain gas undergoing five different cyclic processes are shown below. During which cycle does the gas do the greatest positive work?




A.I
B.II
C.III
D.IV
E.V


26. During an adiabatic process an object does 100 J of work and its temperature decreases by 5 K. During another process it does 25 J of work and its temperature decreases by 5 K. Its heat capacity for the second process is:
A.20 J/K
B.0.05 K/J
C.5 J/K
D.15 J/K
E.100 K/J


27. A system undergoes an adiabatic process in which its internal energy increases by 20 J. Which of the following (A, B, C, D, E) correctly describes changes in the system?
A.

Heat: none,

Work: 20 J on system


B.

Heat: none,

Work: 20 J by system


C.

Heat: 20 J removed,

Work: none


D.

Heat: 20 J added,

Work: none


E.

Heat: 40 J added,

Work: 20 J by system




28. In an adiabatic process:
A.the energy absorbed as heat equals the work done by the system on its environment
B.the energy absorbed as heat equals the work done by the environment on the system
C.the energy absorbed as heat equals the change in internal energy
D.the work done by the environment on the system equals the change in internal energy
E.the work done by the system on its environment equals to the change in internal energy


29. In a certain process a gas ends in its original thermodynamic state. Of the following, which is possible as the net result of the process?
A.It is adiabatic and the gas does 50 J of work
B.The gas does no work but absorbs 50 J of energy as heat
C.The gas does no work but rejects 50 J of energy as heat
D.The gas rejects 50 J of heat and does 50 J of work
E.The gas absorbs 50 J of energy as heat and does 50 J of work


30. Of the following which might NOT vanish over one cycle of a cyclic process?
A.DEint
B.Dp
C.W
D.DV
E.DT


31. Evidence that a gas consists mostly of empty space is the fact that:
A.the density of a gas becomes much greater when it is liquefied
B.gases exert pressure on the walls of their containers
C.gases are transparent
D.heating a gas increases the molecular motion
E.nature abhors a vacuum


32. 273 cm3 of an ideal gas is at 0°C. It is heated at constant pressure to 10°C. It will now occupy:
A.263 cm3
B.273 cm3
C.283 cm3
D.278 cm3
E.293 cm3


33. Two identical rooms in a house are connected by an open doorway. The temperatures in the two rooms are maintained at different values. Which room contains more air?
A.the room with higher temperature
B.the room with lower temperature
C.the room with higher pressure
D.neither because both have the same pressure
E.neither because both have the same volume


34. An ideal gas occupies 12 liters at 20°C and 1 atm (76 cm Hg). Its temperature is now raised to 100°C and its pressure increased to 215 cm Hg. The new volume is:
A.0.2 liters
B.5.4 liters
C.13.6 liters
D.20.8 liters
E.none of these


35. Use R = 8.2 × 10–5 m3 × atm/mol × K and NA = 6.02 × 1023 mol–1. The approximate number of air molecules in a 1 m3 volume at room temperature and atmospheric pressure is:
A.41
B.450
C.2.5 × 1025
D.2.7 × 1026
E.5.4 × 1026


36. An air bubble doubles in volume as it rises from the bottom of a lake (1000 kg/m3). Ignoring any temperature changes, the depth of the lake is:
A.21 m
B.0.76 m
C.4.9 m
D.10 m
E.0.99 m


37. An isothermal process for an ideal gas is represented on a p-V diagram by:
A.a horizontal line
B.a vertical line
C.a portion of an ellipse
D.a portion of a parabola
E.a hyperbola


38. An ideal gas undergoes an isothermal process starting with a pressure of 2 ´ 105 Pa and a volume of 6 cm3. Which of the following might be the pressure and volume of the final state?
A.1 ´ 105 Pa and 10cm3
B.3 ´ 105 Pa and 6 cm3
C.4 ´ 105 Pa and 4 cm3
D.6 ´ 105 Pa and 2 cm3
E.8 ´ 105 Pa and 2 cm3


39. During slow adiabatic expansion of a gas:
A.the pressure remains constant
B.energy is added as heat
C.work is done on the gas
D.no energy enters or leaves as heat
E.the temperature is constant


40. An adiabatic process for an ideal gas is represented on a p-V diagram by:
A.a horizontal line
B.a vertical line
C.a hyperbola
D.a circle
E.none of these


41. A real gas undergoes a process which can be represented as a curve on a p-V diagram. The work done by the gas during this process is:
A.pV
B.p(V2 – V1)
C.(p2 – p1)V
D.ò p dV
E.V dp


42. A given mass of gas is enclosed in a suitable container so that it may be maintained at constant volume. Under these conditions, there can be no change is what property of the gas?
A.Pressure
B.Density
C.Molecular kinetic energy
D.Internal energy
E.Temperature


43. A quantity of an ideal gas is compressed to half its initial volume. The process may be adiabatic, isothermal or isobaric. The greatest amount of work is required if the process is:
A.adiabatic
B.isothermal
C.isobaric
D.adiabatic or isothermal (both require the same work; isobaric requires less)
E.isothermal or isobaric (both require the same work, adiabatic requires less)


44. During a reversible adiabatic expansion of an ideal gas, which of the following is NOT true?
A.pV 1 = constant
B.pV = nRT
C.TV 1 –1 = constant
D.W = –ò pdV
E.pV = constant


45. In order that a single process be both isothermal and isobaric:
A.one must use an ideal gas
B.such a process is impossible
C.a change of phase is essential
D.one may use any real gas such as N2
E.one must use a solid


46. The temperature of a gas is most closely related to:
A.the kinetic energy of translation of its molecules
B.its total molecular kinetic energy
C.the sizes of its molecules
D.the potential energy of its molecules
E.the total energy of its molecules


47. The number of degrees of freedom of a rigid diatomic molecule is:
A.2
B.3
C.4
D.5
E.6


48. The internal energy of an ideal gas depends on:
A.the temperature only
B.the pressure only
C.the volume only
D.the temperature and pressure only
E.temperature, pressure, and volume


49. When an ideal gas undergoes a slow isothermal expansion:
A.the work done by the gas is the same as the energy absorbed as heat
B.the work done by the environment is the same as the energy absorbed as heat
C.the increase in internal energy is the same as the heat absorbed
D.the increase in internal energy is the same as the work done by the gas
E.the increase in internal energy is the same as the work done by the environment


50. The pressure of an ideal gas is doubled during a process in which the energy given up as heat by the gas equals the work done on the gas. As a result, the volume is:
A.doubled
B.halved
C.unchanged
D.need more information to answer
E.nonsense, the process is impossible


51. An ideal gas has molar specific heat Cp at constant pressure. When the temperature of n moles is increased by DT the increase in the internal energy is:
A.nCpDT
B.n(Cp + R)DT
C.n(Cp – R)DT
D.n(2Cp + R)DT
E.n(2Cp – R)DT


52. The heat capacity at constant volume of an ideal gas depends on:
A.the temperature
B.the pressure
C.the volume
D.the number of molecules
E.none of the above


53. The specific heat Cv at constant volume of a monatomic gas at low pressure is proportional to Tn where the exponent n is:
A.–1
B.0
C.1
D.1/2
E.2


54. TV 1 is constant for an ideal gas undergoing an adiabatic process, where 1 is the ratio of heat capacities Cp/Cv. This is a direct consequence of:
A.the zeroth law of thermodynamics alone
B.the zeroth law and the ideal gas equation of state
C.the first law of thermodynamics alone
D.the ideal gas equation of state alone
E.the first law and the equation of state


55. In a reversible process the system:
A.is always close to equilibrium states
B.is close to equilibrium states only at the beginning and end
C.might never be close to any equilibrium state
D.is close to equilibrium states throughout, except at the beginning and end
E.is none of the above


56. The difference in entropy DS = SB – SA for two states A and B of a system can computed as the integral ò dQ/T provided:
A.A and B are on the same adiabat
B.A and B have the same temperature
C.a reversible path is used for the integral
D.the work done on the system is first computed
E.the energy absorbed as heat by the system is first computed


57. Entropy units are:
A.J
B.J/K
C.J–1
D.liter×atm
E.cal/mol


58. Which of the following is NOT a state variable?
A.Work
B.Internal energy
C.Entropy
D.Temperature
E.Pressure


59. The change in entropy is zero for:
A.reversible adiabatic processes
B.reversible isothermal processes
C.reversible processes during which no work is done
D.reversible isobaric processes
E.all adiabatic processes


60. Which of the following processes leads to a change in entropy of zero for the system undergoing the process?
A.Non-cyclic isobaric (constant pressure)
B.Non-cyclic isochoric (constant volume)
C.Non-cyclic isothermal (constant temperature)
D.Any closed cycle
E.None of these


61.

Rank from smallest to largest, the changes in entropy of a pan of water on a hot plate, as the temperature of the water


1. goes from 20° to 30°C


2. goes from 30° to 40°C


3. goes from 40° to 45°C


4. foes from 80° to 85°C


A.1, 2, 3, 4
B.4, 3, 2, 1
C.1 and 2 tie, then 3 and 4 tie
D.3 and 4 tie, then 1 and 2 tie
E.4, 3, 2, 1


62. Consider all possible isothermal contractions of an ideal gas. The change in entropy of the gas:
A.is zero for all of them
B.does not decrease for any of them
C.does not increase for any of them
D.increases for all of them
E.decreases for all of them


63.

An ideal gas is to taken reversibly from state i, at temperature T1, to another state, at temperature T2. Of the five processes shown on the p-V diagram below, which results in the greatest change in the entropy of the gas?



A.A
B.B
C.C
D.D
E.E


64. An ideal gas, consisting of n moles, undergoes a reversible isothermal process during which the volume changes from Vi to Vf. The change in entropy of the thermal reservoir in contact with the gas is given by:
A.nR(Vf – Vi)
B.nR ln(Vf – Vi)
C.nR ln(Vi/Vf)
D.nR ln(Vf/Vi)
E.none of the above (entropy can't be calculated for an irreversible process)


65. One mole of an ideal gas expands slowly and isothermally at temperature T until its volume is doubled. The change of entropy of this gas for this process is:
A.R ln 2
B.(ln 2)/T
C.zero
D.RT ln 2
E.2R


66. An ideal gas, consisting of n moles, undergoes an irreversible process in which the temperature has the same value at the beginning and end. If the volume changes from Vi to Vf, the change in entropy is given by:
A.n R(Vf – Vi)
B.n R ln(Vf – Vi)
C.n R ln(Vi/Vf)
D.n R ln(Vf/Vi)
E.none of the above (entropy can't be calculated for an irreversible process)


67. The temperature of n moles of a gas is increased from Ti to Tf at constant pressure. If the molar specific heat at constant pressure is Cp and is independent of temperature, then change in the entropy of the gas is:
A.nCp ln(Tf/Ti)
B.nCp ln(Ti/Tf)
C.nCp ln(Tf – Ti)
D.nCp ln(1 – Ti/Tf)
E.nCp (Tf – Ti)


68. Consider the following processes: The temperature of two identical gases are increased from the same initial temperature to the same final temperature. Reversible processes are used. For gas A the process is carried out at constant volume while for gas B it is carried out at constant pressure. The change in entropy:
A.is the same for A and B
B.is greater for A
C.is greater for B
D.is greater for A only if the initial temperature is low
E.is greater for A only if the initial temperature is high


69. A hot object and a cold object are placed in thermal contact and the combination is isolated. They transfer energy until they reach a common temperature. The change DSh in the entropy of the hot object, the change DSc in the entropy of the cold object, and the change DStotal in the entropy of the combination are:
A.DSh > 0, DSc > 0, DStotal > 0
B.DSh < 0, DSc > 0, DStotal > 0
C.DSh < 0, DSc > 0, DStotal < 0
D.DSh > 0, DSc < 0, DStotal > 0
E.DSh > 0, DSc < 0, DStotal < 0


70. Let SI denote the change in entropy of a sample for an irreversible process from state A to state B. Let SR denote the change in entropy of the same sample for a reversible process from state A to state B. Then:
A.SI > SR
B.SI = SR
C.SI < SR
D.SI = 0
E.SR = 0


71. For all adiabatic processes:
A.the entropy does not change
B.the entropy increases
C.the entropy decreases
D.the entropy does not increase
E.the entropy does not decrease


72. For all reversible processes involving a system and its environment:
A.the entropy of the system does not change
B.the entropy of the system increases
C.the total entropy of the system and its environment does not change
D.the total entropy of the system and its environment increases
E.none of the above


73. For all irreversible processes involving a system and its environment:
A.the entropy of the system does not change
B.the entropy of the system increases
C.the total entropy of the system and its environment does not change
D.the total entropy of the system and its environment increases
E.none of the above


74. According to the second law of thermodynamics:
A.heat energy cannot be completely converted to work
B.work cannot be completely converted to heat energy
C.for all cyclic processes we have dQ/T < 0
D.the reason all heat engine efficiencies are less than 100% is friction, which is unavoidable
E.all of the above are true


75.

Consider the following processes:


I.

Energy flows as heat from a hot object to a colder object


II.

Work is done on a system and an equivalent amount of energy is



rejected as heat by the system


III.

Energy is absorbed as heat by a system and an equivalent amount



of work is done by the system


Which are never found to occur?


A.Only I
B.Only II
C.Only III
D.Only II and III
E.I, II and III


76. An inventor suggests that a house might be heated by using a refrigerator to draw energy as heat from the ground and reject energy as heat into the house. He claims that the energy supplied to the house can exceed the work required to run the refrigerator. This:
A.is impossible by first law
B.is impossible by second law
C.would only work if the ground and the house were at the same temperature
D.is impossible since heat flows from the (hot) house to the (cold) ground
E.is possible


77. In a thermally insulated kitchen, an ordinary refrigerator is turned on and its door is left open. The temperature of the room:
A.remains constant according to the first law of thermodynamics
B.increases according to the first law of thermodynamics
C.decreases according to the first law of thermodynamics
D.remains constant according to the second law of thermodynamics
E.increases according to the second law of thermodynamics


78. A heat engine:
A.converts heat input to an equivalent amount of work
B.converts work to an equivalent amount of heat
C.takes heat in, does work, and rejects heat
D.uses positive work done on the system to transfer heat from a low temperature reservoir to a high temperature reservoir
E.uses positive work done on the system to transfer heat from a high temperature reservoir to a low temperature reservoir


79. A heat engine absorbs energy of magnitude çQH ç from a high temperature reservoir, does work of magnitude çW ç, and rejects energy of magnitude çQL ç as heat to a low temperature reservoir. Its efficiency is:
A.çQH ç/ çW ç
B.çQL ç/ çW ç
C.çQH ç/ çQL ç
D.çW ç/ çQH ç
E.çW ç/ çQL ç


80.

The temperature TC of the cold reservoirs and the temperatures TH of the hot reservoirs for four Carnot heat engines are


engine 1: TC = 400 K and TH = 500 K


engine 2: TC = 500 K and TH = 600 K


engine 3: TC = 400 K and TH = 600 K


engine 4: TC = 600 K and TH = 800 K

Rank these engines according to their efficiencies, least to greatest


A.1, 2, 3, 4
B.1 and 2 tie, then 3 and 4 tie
C.2, 1, 3, 4
D.1, 2, 4, 3
E.2, 1, 4, 3


81. An Carnot heat engine runs between a cold reservoir at temperature TC and a hot reservoir at temperature TH. You want to increase its efficiency. Of the following, which change results in the greatest increase in efficiency? The value of DT is the same for all changes.
A.Raise the temperature of the hot reservoir by DT
B.Raise the temperature of the cold reservoir by DT
C.Lower the temperature of the hot reservoir by DT
D.Lower the temperature of the cold reservoir by DT
E.Lower the temperature of the hot reservoir by (1/2)DT and raise the temperature of the cold reservoir by (1/2)DT


82. A certain heat engine draws 500 cal/s from a water bath at 27°C and rejects 400 cal/s to a reservoir at a lower temperature. The efficiency of this engine is:
A.80%
B.75%
C.55%
D.25%
E.20%


83. A heat engine that in each cycle does positive work and rejects energy as heat, with no heat energy input, would violate:
A.the zeroth law of thermodynamics
B.the first law of thermodynamics
C.the second law of thermodynamics
D.the third law of thermodynamics
E.Newton's second law


84. On a warm day a pool of water rejects energy to the air as heat and freezes. This is a direct violation of:
A.the zeroth law of thermodynamics
B.the first law of thermodynamics
C.the second law of thermodynamics
D.the third law of thermodynamics
E.none of the above


85. A Carnot cycle:
A.is bounded by two isotherms and two adiabats on a p-V graph
B.consists of two isothermal and two constant volume processes
C.is any four sided process on a p-V graph
D.only exists for an ideal gas
E.has an efficiency equal to the enclosed area on a p-V diagram


86. By the second law of thermodynamics:
A.all heat engines have the same efficiency
B.all reversible heat engines have the same efficiency
C.the efficiency of any heat engine is independent of its working substance
D.the efficiency of a Carnot engine depends only on the temperatures of the two reservoirs
E.all Carnot engines theoretically have 100% efficiency



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