chapter 18 heat, work, and the first law of thermodynamics
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Chapter 18 Heat, Work, and the First Law of Thermodynamics. Heat and work Thermodynamic cycle. Heat and work Work is done by the system: Work is done on the system :. The first law of thermodynamics Work and heat are path-dependent quantities - PowerPoint PPT PresentationTRANSCRIPT
Chapter 18
Heat, Work, and the First Law of Thermodynamics
Heat and work
Thermodynamic cycle
sdFdW
dsPA )( )(AdsP PdV
f
i
V
VPdVW
Heat and work
• Work is done by the system:
• Work is done on the system :
f
i
V
VPdVW
f
i
V
VPdVW
The first law of thermodynamics
• Work and heat are path-dependent quantities
• Quantity Q + W = ΔEint (change of internal energy)
is path-independent
• 1st law of thermodynamics: the internal energy of a system increases if heat is added to the system or work is done on the system
WQEEE if int,int,int
The first law of thermodynamics
• Adiabatic process: no heat transfer between the system and the environment
• Isochoric (constant volume) process
• Free expansion:
• Cyclical process:
WWE 0int
QQE 0int
000int E
0int WQE
WQ
Chapter 18Problem 19
In a certain automobile engine, 17% of the total energy released in burning gasoline ends up as mechanical work. What’s the engine’s mechanical power output if its heat output is 68 kW?
Work done by an ideal gas at constant temperature
• Isothermal process – a process at a constant temperature
• Work (isothermal expansion)
nRTPV VconstVnRTP //)(
f
i
V
VPdVW f
i
V
VdV
V
nRT
f
i
V
V V
dVnRT
i
f
V
VnRT ln
i
f
V
VnRTW ln
Work done by an ideal gas at constant volume and constant pressure
• Isovolumetric process – a process at a constant volume
• Isobaric process – a process at a constant pressure
0if
f
i VV
V
VPdVW
VPW
0W
f
i
V
VPdVW f
i
V
VdVP VP
Molar specific heat at constant volume
• Heat related to temperature change:
• Internal energy change:
TNnmcQ AV )( 0 TnCV
WTnCE V int TnCTnC VV 0
Tn
ECV
int
Tn
nRT
23
T
TR
2
3R
2
3
KmolJRCV / 5.122
3TnCE V int
Molar specific heat at constant pressure
• Heat related to temperature change:
• Internal energy change:
TnCQ P
WQE int
RCC VP
VPTnCP
TnRTnCTnC PV
RCV 2
3R
2
5
Adiabatic expansion of an ideal gas
PdVdTnCV 0PdVdQdE int
nRTPV )()( nRTdPVd nRdTVdPPdV
R
VdPPdVndT
VC
PdVndT
VP CC
VdPPdV
VPV CC
VdPPdV
C
PdV
Adiabatic expansion of an ideal gas
VPV CC
VdPPdV
C
PdV
0
V
dV
C
C
P
dP
V
P
constVC
CP
V
P
lnln constPVPV V
P
C
C
ffii VPVP
nRTPV V
nRTP
constVV
nRT
constTV 1
Chapter 18Problem 24
How much work does it take to compress 2.5 mol of an ideal gas to half its original volume while maintaining a constant 300 K temperature?
Free expansion of an ideal gas
0int E
fi TT
nRTPV
ffii VPVP
Degrees of freedom and molar specific heat
• Degrees of freedom:3 translations, 3 rotations, + oscillations
RCV 2
3
Degrees of freedom and molar specific heat
• Degrees of freedom:3 translations, 3 rotations, + oscillations
• In polyatomic molecules different degrees of freedom contribute at different temperatures
Rf
CV 2
3f
5f
6f
RCV 2
3
Chapter 18Problem 26
A gas mixture contains 2.5 mol of O2 and 3.0 mol of Ar. What are this mixture’s molar specific heats at constant volume and at constant pressure?
Questions?
Answers to the even-numbered problems
Chapter 18
Problem 22
1.2 kJ