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Physics 6C > Midterm 2 > Flashcards

Midterm 2 Flashcards

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1
Q

What would be the greatest effect of the finite size of molecules on the ideal gas law?

A

At high densities, the pressure would be less than that predicted by the ideal gas law.

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2
Q

What would be the greatest effect on the ideal gas law if there is a slight attractive force between the molecules?

A

At low temperatures, the pressure would be less than that predicted by the ideal gas law.

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3
Q

What would be the greatest effect on the ideal gas law if there is a slight repulsive force between the molecules?

A

At low temperatures, the pressure would be greater than that predicted by the ideal gas law.

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4
Q

The average molecular kinetic energy of a gas can be determined by knowing only the – of the gas.

A

temperature

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5
Q

A sample of an ideal gas is slowly compressed to one-half its original volume with no change in temperature. What happens to the average speed of the molecules in the sample

A

It does not change.

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6
Q

A container is filled with a mixture of helium and oxygen gases. A thermometer in the container indicates that the temperature is 22°C. Which gas molecules have the greater average kinetic energy?

A

It is the SAME for both because the temperatures are the same.

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7
Q

A container is filled with a mixture of helium and oxygen gases. A thermometer in the container indicates that the temperature is 22°C. Which gas molecules have the greater average speed?

A

The helium molecules because they are less massive.

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8
Q

Phase change occur as the temperature

A

remains the same

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9
Q

The point in the phase diagram where the fusion curve, the vapor pressure curve, and the sublimation curve join is called the

A

triple point

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10
Q

The point in the phase diagram where the vapor pressure curve ends is called the

A

critical point

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11
Q

When a solid melts, heat energy – the substance

A

enters

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12
Q

When a liquid freezes, heat energy – the substance

A

leaves

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13
Q

By what primary heat transfer mechanism does one end of an iron bar become hot when the other end is
placed in a flame?

A

conduction

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14
Q

The type of heat transfer that occurs between a stove and a pot placed on it is

A

conductive

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15
Q

The type of heat transfer that occurs between the radiator of a car and the atmosphere, when the car is in
motion, is principally

A

convective

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16
Q

The type of heat transfer that occurs between warm food and the air in the room is principally

A

convective

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17
Q

Convection can occur

A

only in liquids and gases

18
Q

The process whereby heat flows in the absence of any medium is referred to as

A

radiation

19
Q

The process whereby heat flows by the mass movement of molecules from one place to another is referred to
as

A

convection

20
Q

The process whereby heat flows by means of molecular collisions is referred to as

A

conduction

21
Q

Consider two cylinders of gas identical in all respects except that one contains O2 and the other He. Both hold the same volume of gas at STP and are closed by a movable piston at one end. Both gases are now
compressed adiabatically to one-third their original volume. Which gas will show the greater pressure increase?

A

the He

22
Q

Consider two cylinders of gas identical in all respects except that one contains O2 and the other He. Both hold the same volume of gas at STP and are closed by a movable piston at one end. Both gases are now
compressed adiabatically to one-third their original volume. Which gas will show the greater temperature increase?

A

the He

23
Q

An ideal gas starts in state A at temperature T. The gas expands to new volume V by an adiabatic process
and its final temperature is T’. What is the relationship between T and T’?

A

T > T’

24
Q

When a gas expands adiabatically,

A

the internal energy of the gas decreases

25
Q

During which type of process applied to an ideal gas is there no change in internal energy of the gas?

A

isothermal

26
Q

During which type of process applied to an ideal gas is there no heat added to the gas?

A

adiabatic

27
Q

During which type of process applied to an ideal gas is there no work done by the gas?

A

isochoric

28
Q

When the first law of thermodynamics, Q = ΔU + W, is applied to an ideal gas that is taken through an
isochoric process,

A

W = 0

29
Q

When the first law of thermodynamics, Q = ΔU + W, is applied to an ideal gas that is taken through an
adiabatic process,

A

Q = 0

30
Q

When the first law of thermodynamics, Q = ΔU + W, is applied to an ideal gas that is taken through an isothermal process,

A

ΔU = 0

31
Q

Is it possible to transfer heat from a cold reservoir to a hot reservoir?

A

Yes, but work will have to be done

32
Q

The internal energy of an ideal gas is changed by adding heat Q to the system and also by doing work W on
the gas. What is the change in internal energy of the gas?

A

Q + W

33
Q

A chunk of ice (T = -20°C) is added to a thermally insulated container of cold water (T = 0°C). What happens
in the container?

A

Some of the water freezes and the chunk of ice gets bigger

34
Q

The heat required to change a substance from the liquid to the vapor state is referred to as the

A

hear of vaporization

35
Q

The heat required to change a substance from the solid to the liquid state is referred to as the

A

heat of fusion

36
Q

A thermally isolated system is made up of a hot piece of aluminum and a cold piece of copper; the
aluminum and the copper are in thermal contact. The specific heat capacity of aluminum is more than
double that of copper. Which object experiences the greater temperature change during the time the system
takes to reach thermal equilibrium?

A

it is impossible to tell without knowing the masses

37
Q

A thermally isolated system is made up of a hot piece of aluminum and a cold piece of copper; the
aluminum and the copper are in thermal contact. The specific heat capacity of aluminum is more than
double that of copper. Which object experiences the greater magnitude gain or loss of heat during the time
the system takes to reach thermal equilibrium?

A

neither; both experience the same size gain or loss of heat

38
Q

It is a well-known fact that water has a higher specific heat capacity than iron. Now, consider equal masses
of water and iron that are initially in thermal equilibrium. The same amount of heat, 30 calories, is added to
each. Which statement is true?

A

They are no longer in thermal equilibrium; the iron is warmer.

39
Q

A cup of water is scooped up from a swimming pool of water. Compare the temperature T and the
internal energy U of the water, in both the cup and the swimming pool.

A

TPool is equal to TCup, and UPool is greater than UCup

40
Q

closed system in which NO ENERGY in any form is transferred

A

isolated system

41
Q

NO MASS enters or leaves but energy may be exchanged

A

closed system

42
Q

mass and energy transfer

A

Open system

Physics 6C (3 decks)

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