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ch15.ppt
1. 1
Ch15. Thermodynamics
Thermodynamics is the branch of physics that is built upon the
fundamental laws that heat and work obey.
In thermodynamics the collection of objects on which
attention is being focused is called the system, while everything
else in the environment is called the surroundings. The system
and its surroundings are separated by walls of some kind.
Walls that permit heat to flow through them, such as those of
the engine block, are called diathermal walls. Perfectly
insulating walls that do not permit heat to flow between the
system and its surroundings are known as adiabatic walls.
3. 3
Thermal equilibrium: Two systems are said to be in thermal
equilibrium if there is no net flow of heat between them
when they are brought into thermal contact.
Temperature is the indicator of thermal equilibrium in the
sense that there is no net flow of heat between two systems in
thermal contact that have the same temperature.
THE ZEROTH LAW OF THERMODYNAMICS
Two systems individually in thermal equilibrium with a third
system* are in thermal equilibrium with each other.
5. 5
THE FIRST LAW OF THERMODYNAMICS
The internal energy of a system changes from an initial
value Ui to a final value of Uf due to heat Q and work.
Q is positive when the system gains heat and negative
when it loses heat. W is positive when work is done by the
system and negative when work is done on the system.
7. 7
The figure illustrates a system and its surroundings. In part a,
the system gains 1500 J of heat from its surroundings, and 2200
J of work is done by the system on the surroundings. In part b,
the system also gains 1500 J of heat, but 2200 J of work is done
on the system by the surroundings. In each case, determine the
change in the internal energy of the system.
(a)
(b)
8. 8
Example 2. An Ideal Gas
The temperature of three moles of a monatomic ideal gas is
reduced from Ti = 540 K to Tf = 350 K by two different
methods. In the first method 5500 J of heat flows into the gas,
while in the second, 1500 J of heat flows into it. In each case
find (a) the change in the internal energy and (b) the work
done by the gas.
(a)
(b)
9. 9
Check Your Understanding 1
A gas is enclosed within a chamber that is fitted with a
frictionless piston. The piston is then pushed in, thereby
compressing the gas. Which statement below regarding this
process is consistent with the first law of thermodynamics?
a. The internal energy of the gas will increase.
b. The internal energy of the gas will decrease.
c. The internal energy of the gas will not change.
d. The internal energy of the gas may increase, decrease, or
remain the same, depending on the amount of heat that the gas
gains or loses.
(d)
10. 10
Thermal Processes
quasi-static means that it occurs slowly enough that a
uniform pressure and temperature exist throughout all
regions of the system at all times.
An isobaric process is one that occurs at constant pressure.
11. 11
The substance in
the chamber is
expanding
isobarically
because the
pressure is held
constant by the
external
atmosphere and
the weight of the
piston and the
block.
12. 12
Example 3.
Isobaric Expansion of Water
One gram of water is placed in the cylinder in above figure, and
the pressure is maintained at 2.0 × 105 Pa. The temperature of the
water is raised by 31 C°. In one case, the water is in the liquid
phase and expands by the small amount of 1.0 × 10–8 m3. In
another case, the water is in the gas phase and expands by the
much greater amount of 7.1 × 10–5 m3. For the water in each case,
find (a) the work done and (b) the change in the internal energy.
c = 4186 J/(kg·C°)
cP = 2020 J/(kg·C°).
14. 14
For an isobaric process, a pressure-versus-volume plot is a
horizontal straight line, and the work done [W = P(V f – V i)]
is the colored rectangular area under the graph.
15. 15
isochoric process, one that occurs at constant
volume.
(a)The substance in the
chamber is being heated
isochorically because the
rigid chamber keeps the
volume constant.
(b)The pressure-volume
plot for an isochoric
process is a vertical
straight line. The area
under the graph is zero,
indicating that no work
is done.
16. 16
isothermal process, one that takes place at constant temperature.
(when the system is an ideal gas.)
There is adiabatic process, one that occurs without the transfer
of heat . Since there is no heat transfer, Q equals zero, and the
first law indicates that U = Q – W = –W. Thus, when work is
done by a system adiabatically, W is positive and the internal
energy of the system decreases by exactly the amount of the
work done. When work is done on a system adiabatically, W is
negative and the internal energy increases correspondingly.
17. 17
The area under a
pressure-volume graph
is the work for any kind
of process.
The colored area gives
the work done by the
gas for the process
from X to Y.
18. 18
Example 4. Work and the Area Under
a Pressure-Volume Graph
Determine the work for the process in
which the pressure, volume, and
temperature of a gas are changed
along the straight line from X to Y in
the figure.
= +180 J
19. 19
Check Your Understanding 2
The drawing shows a
pressure-versus-
volume plot for a
three-step process: A to
B, B to C, and C to A.
For each step, the
work can be positive,
negative, or zero.
Which answer below
correctly describes the
work for the three
steps?
20. 20
A B B C C A
a. Positive Negative Negative
b. Positive Positive Negative
c. Negative Negative Positive
d. Positive Negative Zero
e. Negative Positive Zero
(b)
23. 23
Example 5.
Isothermal Expansion of an Ideal Gas
Two moles of the monatomic gas argon expand isothermally at
298 K, from an initial volume of Vi = 0.025 m3 to a final volume of
Vf = 0.050 m3. Assuming that argon is an ideal gas, find (a) the
work done by the gas, (b) the change in the internal energy of the
gas, and (c) the heat supplied to the gas.
(a)
.
(b)
(c)
26. 26
Type of Thermal
Process
Work Done
First Law of
Thermodynamics
(U = Q – W)
Isobaric (constant
pressure)
W = P(Vf – Vi)
Isochoric (constant
volume)
W = 0 J
Isothermal
(constant
temperature) (for an ideal gas)
Adiabatic (no heat
flow)
(for a monatomic ideal gas)
30. 30
The Second Law of Thermodynamics
THE SECOND LAW OF THERMODYNAMICS:
THE HEAT FLOW STATEMENT
Heat flows spontaneously from a substance at a
higher temperature to a substance at a lower
temperature and does not flow spontaneously in the
reverse direction.
32. 32
Heat Engines
A heat engine is any device that uses heat to perform work. It
has three essential features:
1.Heat is supplied to the engine at a relatively high input
temperature from a place called the hot reservoir.
2.Part of the input heat is used to perform work by the working
substance of the engine, which is the material within the engine
that actually does the work (e.g., the gasoline-air mixture in an
automobile engine).
3.The remainder of the input heat is rejected to a place called
the cold reservoir, which has a temperature lower than the input
temperature.
33. 33
These three symbols refer
to magnitudes only,
without reference to
algebraic signs. Therefore,
when these symbols appear
in an equation, they do not
have negative values
assigned to them.
34. 34
Efficiencies are often quoted as percentages obtained by
multiplying the ratio W/QH by a factor of 100.
35. 35
Example 6. An Automobile Engine
An automobile engine has an efficiency of 22.0% and produces
2510 J of work. How much heat is rejected by the engine?
36. 36
Carnot's Principle and the Carnot
Engine
A reversible process is one in which both the system and its
environment can be returned to exactly the states they were in
before the process occurred.
CARNOT’S PRINCIPLE: AN ALTERNATIVE
STATEMENT OF THE SECOND LAW OF
THERMODYNAMICS
No irreversible engine operating between two reservoirs at
constant temperatures can have a greater efficiency than a
reversible engine operating between the same temperatures.
Furthermore, all reversible engines operating between the
same temperatures have the same efficiency.
37. 37
A Carnot engine is a
reversible engine in which
all input heat QH
originates from a hot
reservoir at a single
temperature TH, and all
rejected heat QC goes into
a cold reservoir at a single
temperature TC. The work
done by the engine is W.
39. 39
Example 7.
A Tropical Ocean as a Heat Engine
Water near the surface of a tropical ocean has a temperature
of 298.2 K (25.0 °C), whereas water 700 m beneath the
surface has a temperature of 280.2 K (7.0 °C). It has been
proposed that the warm water be used as the hot reservoir and
the cool water as the cold reservoir of a heat engine. Find the
maximum possible efficiency for such an engine.
TH = 298.2 K and TC = 280.2 K
40. 40
Conceptual Example 8. Limits on the
Efficiency of a Heat Engine
Consider a hypothetical engine that receives 1000 J of heat as
input from a hot reservoir and delivers 1000 J of work, rejecting
no heat to a cold reservoir whose temperature is above 0 K. Decide
whether this engine violates the first or the second law of
thermodynamics, or both.
It is the second law, not the first law, that limits the
efficiencies of heat engines to values less than 100%.
41. 41
Refrigerators, Air Conditioners, and
Heat Pumps
In the refrigeration process, work W is used to remove heat QC
from the cold reservoir and deposit heat QH into the hot reservoir.
44. 44
Conceptual Example 9.
You Can’t Beat the Second Law of
Thermodynamics
Is it possible to cool your kitchen by leaving the refrigerator
door open or cool your bedroom by putting a window air
conditioner on the floor by the bed?
Rather than cooling the kitchen, the open
refrigerator warms it up. The air conditioner
actually warms the bedroom.
48. 48
Example 10. A Heat Pump
An ideal or Carnot heat pump is used to heat a house to a
temperature of TH = 294 K (21 °C). How much work must
be done by the pump to deliver QH = 3350 J of heat into the
house when the outdoor temperature TC is (a) 273 K (0 °C)
and (b) 252 K (–21 °C)?
(a)
(b)
50. 50
Check Your Understanding 3
Each drawing represents a hypothetical heat engine or a
hypothetical heat pump and shows the corresponding heats and
work. Only one is allowed in nature. Which is it?
(c)
51. 51
Entropy
In general, irreversible processes cause us to lose some, but not
necessarily all, of the ability to perform work. This partial loss
can be expressed in terms of a concept called entropy.
Reversible processes do not alter the total entropy of the
universe.
52. 52
Although the
relation S =
(Q/T)R applies
to reversible
processes, it
can be used as
part of an
indirect
procedure to
find the
entropy change
for an
irreversible
process.
53. 53
Example 11. The Entropy of the
Universe Increases
1200 J of heat flow
spontaneously through a
copper rod from a hot
reservoir at 650 K to a
cold reservoir at 350 K.
Determine the amount by
which this irreversible
process changes the
entropy of the universe,
assuming that no other
changes occur.
55. 55
THE SECOND LAW OF THERMODYNAMICS STATED
IN TERMS OF ENTROPY
The total entropy of the universe does not change when a
reversible process occurs ( Suniverse = 0 J/K) and does
increases when an irreversible process occurs ( Suniverse >
0 J/K).
57. 57
Suppose that 1200 J of heat is used as input for an engine under two
different conditions. In Figure part a the heat is supplied by a hot
reservoir whose temperature is 650 K. In part b of the drawing, the heat
flows irreversibly through a copper rod into a second reservoir whose
temperature is 350 K and then enters the engine. In either case, a 150-K
reservoir is used as the cold reservoir. For each case, determine the
maximum amount of work that can be obtained from the 1200 J of heat.
58. 58
where T0 is the Kelvin temperature of the coldest heat
reservoir.
59. 59
A block of ice is an example of an ordered system
relative to a puddle of water.
60. 60
Example 13. Order to Disorder
Find the change in entropy that results when a 2.3-kg block of
ice melts slowly (reversibly) at 273 K (0 °C).
61. 61
Check Your Understanding 4
Two equal amounts of water are mixed together in an insulated
container. The initial temperatures of the water are different,
but the mixture reaches a uniform temperature. Do the energy
and the entropy of the water increase, decrease, or remain
constant as a result of the mixing process?
Energy of the
Water
Entropy of the
Water
a. Increases Increases
b. Decreases Decreases
c. Remains constant Decreases
d. Remains constant Increases
(d)
62. 62
THE THIRD LAW OF THERMODYNAMICS
It is not possible to lower the temperature of any system to
absolute zero (T = 0 K) in a finite number of steps.
The Third Law of Thermodynamics
63. 63
Concepts & Calculations
Example 14. The Sublimation of Zinc
The sublimation of zinc (mass per mole = 0.0654 kg/mol) occurs
at a temperature of 6.00 × 102 K, and the latent heat of
sublimation is 1.99 × 106 J/kg. The pressure remains constant
during the sublimation. Assume that the zinc vapor can be
treated as a monatomic ideal gas and that the volume of solid
zinc is negligible compared to the corresponding vapor. What is
the change in the internal energy of the zinc when 1.50 kg of
zinc sublimates?
Q = U + W,
Q = mLs,
W = nRT
65. 65
Concepts & Calculations Example 15.
The Work–Energy Theorem
Each of two Carnot engines
uses the same cold reservoir
at a temperature of 275 K
for its exhaust heat. Each
engine receives 1450 J of
input heat.
66. 66
The work from either of these engines is used to drive a pulley
arrangement that uses a rope to accelerate a 125-kg crate from
rest along a horizontal frictionless surface. With engine 1 the
crate attains a speed of 2.00 m/s, while with engine 2 it attains a
speed of 3.00 m/s. Find the temperature of the hot reservoir for
each engine.
68. 68
Conceptual Question 14
T T
C H
/
REASONING AND SOLUTION The efficiency of a Carnot engine is
given by Equation 15.15 . Three reversible
engines A, B, and C, use the same cold reservoir for their exhaust
heats. They use different hot reservoirs with the following
temperatures: (A) 1000 K; (B) 1100 K; and (C) 900 K. We can
rank these engines in order of increasing efficiency according to the
following considerations. The ratio is inversely proportional
to the value of TH. The ratio will be smallest for engine B;
therefore, the quantity 1 – will be largest for engine B. Thus,
engine B has the largest efficiency. Similarly, the ratio will be
largest for engine C; therefore, the quantity 1 – will be
smallest for engine C. Thus, engine C has the smallest efficiency.
Hence, the engines are, in order of increasing efficiency: engine C,
engine A, and engine B.
efficiency C H
1 ( / )
T T
T T
C H
/
T T
C H
/
T T
C H
/
T T
C H
/
69. 69
Conceptual Question 15
REASONING AND SOLUTION The efficiency of a Carnot engine
is given by Equation 15.15:
a. Lowering the Kelvin temperature of the cold reservoir by a
factor of four makes the ratio one-fourth as great.
b. Raising the Kelvin temperature of the hot reservoir by a factor of
four makes the ratio one-fourth as great.
c. Cutting the Kelvin temperature of the cold reservoir in half and
doubling the Kelvin temperature of the hot reservoir makes the
ratio one-fourth as great.
Therefore, all three possible improvements have the same effect on
the efficiency of a Carnot engine.
efficiency C H
1 ( / )
T T
T T
C H
/
T T
C H
/
T T
C H
/
70. 70
Problem 51
REASONING AND SOLUTION The efficiency of the engine
is e = 1 - (TC/TH) so
(i) Increase TH by 40 K; e = 1 - [(350 K)/(690 K)] = 0.493
(ii)Decrease TC by 40 K; e = 1 - [(310 K)/(650 K)] = 0.523
The greatest improvement is made by lowing the temperature
of the cold reservoir.
71. 71
Problem 63
REASONING AND SOLUTION Let CP denote the coefficient
of performance. By definition (Equation 15.16), CP = QC/W,
so that
4
4
C 7.6 10 J
3.8 10 J
CP 2.0
Q
W
Thus, the amount of heat that is pumped out of the back of
the air conditioner is
4 4 5
H C 3.8 10 J + 7.6 10 J = 1.14 10 J
Q W Q
72. 72
The temperature rise in the room can be found as follows:
QH = CV n T
5
H H
5
5
2
2
1.14 10 J
1.4 K
[8.31 J/(mol K)](3800 mol)
V
Q Q
T
C n R n
73. 73
Problem 64
REASONING AND SOLUTION The amount of heat removed
from the ice QC is
QC = mLf = (2.0 kg)(33.5 * 104 J/kg) = 6.7 * 105 J
The amount of heat leaving the refrigerator QH is therefore
QH = QC(TH/TC) = (6.7 * 105 J)(300 K)/(258 K) = 7.8 * 105 J
The amount of work done by the refrigerator is therefore,
W = QH - QC = 1.1 * 105 J
At $0.10 per kWh (or $0.10 per 3.6 * 106 J), the cost is
cents
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