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Physics I The First Law of Thermodynamics Prof. WAN, Xin [email protected] xinwan
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Transcript of Physics I The First Law of Thermodynamics Prof. WAN, Xin [email protected] xinwan
Physics IPhysics I
The First Law of The First Law of ThermodynamicsThermodynamics
Prof. WAN, Xin
[email protected]://zimp.zju.edu.cn/~xinwan/
Heat ConductionHeat Conduction
dx
dTA
t
Qt
Fourier heat conduction law
Remind you of Ohm’s law?
Energy Transfer Through Two SlabsEnergy Transfer Through Two Slabs
Kinetic TheoryKinetic Theory
Q
l l
UL, NL UR, NR
T
md
f
m
1~
2
TlvT
Pf Tltht
22
1
TCUUQ VLR 2
1
2
1
dx
dTA
t
Qt
ldx
dT BkAlV
Nf
2
Energy exchange across plane A
tt for Air at Room Temperature for Air at Room Temperature
m1025.2 7l m/s500v
500m/sm1025.2300K
N/m10
2
5
2
1
22
1 75
tht lv
T
Pf
K)W/(m047.0
From last lecture
A factor less than 2 larger than the measured value of 0.026. Not bad after so many crude approximations.
Transport in ComparisonTransport in Comparison
Phenomena Imbalance Things being transported
Experimental observation
Unit of Coefficient
Thermal conduction
temperature energy W/m·K
Viscosity velocity momentum N·s/m2
Diffusion density particle m2/s
Charge conduction
voltage charge -1m-1
dy
dvAF
dx
dTA
t
Qt
dx
dnDAI n
x )(
dx
dVAI e
x )(
Internal Energy, Heat & WorkInternal Energy, Heat & Work
Heat is defined as the transfer of energy across the boundary of a system due to a temperature difference between the system and its surroundings.
Energy can also be transferred to or from the system by work.
Internal energy is all the energy of a system that is associated with its microscopic components —atoms and molecules —when viewed from a reference frame at rest with respect to the object.
Mechanical Equivalence of HeatMechanical Equivalence of Heat
The amount of energy transfer necessary to raise the temperature of 1 g of water from 14.5oC to 15.5oC.
Specific HeatSpecific Heat
Note: Last time we defined molar specific heat. In physics, we also use specific heat per particle.
Help Young Leonardo DiCaprioHelp Young Leonardo DiCaprio
A cowboy fires a silver bullet with a mass of 2 g and with a muzzle speed of 200 m/s into the pine wall of a saloon. Assume that all the internal energy generated by the impactremains with the bullet. What is the temperature change of the bullet?
Kinetic energy J 40m/s 200kg 1022
1
2
1 232 mv
C5.85CJ/kg 234kg 102
J 403
mc
QT
convert to heat
Latent Heat in Phase ChangesLatent Heat in Phase Changes
Latent HeatLatent Heat
The latent heat of vaporization for a given substance is usually somewhat higher than the latent heat of fusion. Why?
Work in Thermodynamic ProcessesWork in Thermodynamic Processes
PdVPAdyFdydW
Quasi-static assumption: the gas expands slowly enough to allow the system to remain essentially in thermal equilibrium at all times.
Work done by the gas
f
i
V
VPdVW
Work in Thermodynamic ProcessesWork in Thermodynamic Processes
PdVPAdyFdydW
Work done by the gas
f
i
V
VPdVW
The work done by a gas in the expansion from an initial state to a final state is the area under the curve connecting the states in a PV diagram.
Warning:Warning: Sign Convention Sign Convention
Historically, people are interested in the amount of work done by the expansion of gas, say, to drive a steam engine. The common treatment is
– Positive work: gas expands– Negative work: gas compressed
In mechanics we use the opposite sign, unfortunately.
But some books follow the same convention in thermal physics as in mechanics.
Trust your common sense!
Work Depends on the PathWork Depends on the Path
)()(iff
a VVPW )()(
ifib VVPW
)()()( bca WWW
The work done by a system depends on the initial, final, and intermediate states of the system.
• The gas does work on the piston
• Energy is transferred slowly to the gas
Isothermal ExpansionIsothermal Expansion
0W
An energy reservoiris a source of energy that is considered to be so great that a finite transfer of energy from the reservoir does not change its temperature.
0Q
Free ExpansionFree Expansion
• No heat or energy is transferred
• The value of the work done is zero
Energy transfer by heat, like work done, depends on the initial, final, and intermediate states of the system.
0Q
0W
The 1st Law of ThermodynamicsThe 1st Law of Thermodynamics
Although Q and W both depend on the path, the quantity Q-W is independent of the path change.
The change in the internal energy U of the system can be expressed as:
The infinitesimal change:
WQU
PdVdQdU
reminding you that it is path dependent
Discussion on the 1st LawDiscussion on the 1st Law
The 1st law is a statement of energy conservation (now with the internal energy included).
The internal energy of an isolated system remains constant. In a cyclic process,
– The net work done by the systemper cycle equals the area enclosed by the path representing the process on a PV diagram.
WQU ,0
Discussion on the 1st LawDiscussion on the 1st Law
On a microscopic scale, no distinction exists between the result of heat and that of work.
The internal energy function is therefore called a state function, whose value is determined by the state of the system.
– In general,
),( VTUU
Digression on Multivariate CalculusDigression on Multivariate Calculus
If we take energy and volume as parameters, how comes heat is path dependent?
In mathematical language, dU + pdV is an inexact differential.
– In multivariate calculus, a differential is said to be exact (or perfect), as contrasted with an inexact differential, if it is of the form dQ, for some differentiable function Q.
PdVdUdQ
Inexact DifferentialInexact Differential
12ln)2,2(
)2,1(
)2,1(
)1,1(
dy
y
xdx
0lnln),( fyxyxf
2ln21)2,2(
)1,2(
)1,2(
)1,1(
dy
y
xdx
dyy
xdxdg Assume
Note: is an exact differential.
Integrating factor
y
dy
x
dx
x
dgdf
Ideal GasIdeal Gas
Tkmv B2
3
2
1 2
Tkf
NU B2 BV Nk
f
T
UC
2Vfixed
TNkpV B
Experiments found Kinetic theory found
2
2
1
3
2mv
NVp
Generalized equipartition theorem (can be proved based on statistical principles
Isobaric & Isovolumetric ProcessesIsobaric & Isovolumetric Processes
TNkTC BVTNkPV B
BVP NkCT
QC
Pfixed
TCU V)( if VVPW
VPTCWUQ V
isobaric
f
fC
CNkfCV
PBV
22/
Isobaric & Isovolumetric ProcessesIsobaric & Isovolumetric Processes
TNkTC BVTNkPV B
BVP NkCT
QC
Pfixed
isobaric TCU V)( if VVPW
VPTCWUQ V
Molar specific heat: RCC VP
Isobaric & Isovolumetric ProcessesIsobaric & Isovolumetric Processes
0W
isovolumetric
TCU V
TCUQ V
)( if VVPW
TCU V
TCWUQ P
isobaric
Isothermal ExpansionIsothermal Expansion
i
fB V
VTNkWQ ln
i
fB
V
V
BV
V V
VTNkdV
V
TNkPdVW
f
i
f
i
ln 0U
Adiabatic ExpansionAdiabatic Expansion
V
dVNk
T
dTC BVV
TNkP B
constTV 1
PdVdUdTCV
V
B
V
PC
NkC
C 1
adiabatic 0dQ
constPV or
(Adiabatic) Free Expansion(Adiabatic) Free Expansion
0WQ0U
Questions:
• Is it possible to show the process on the PV diagram?
• Is it reversible?
Degrees of Freedom, AgainDegrees of Freedom, Again
BV Nkf
C2
BP Nkf
C2
2
f
fC
CV
P2
f 3 5 7
1.67 1.4 1.28
HomeworkHomework
CHAP. 22 Exercises 11, 19, 21 (P540) 24, 25 (P541)