Upload
jeffry-matthews
View
214
Download
0
Tags:
Embed Size (px)
Citation preview
1
What is Thermodynamics 1. Understanding why things happens 2. Concerning heat, work, related temperature, pressure, volume and equilibrium
3. Equations relate macroscopic properties
2
The laws of thermodynamics
Number
Basis Property
Zeroth Law
Thermal Equilibrium
Temperature
First Law Relation between work, energy and heat
Internal Energy U
Second Law
Spontaneous process
Entropy
Third Law Absolute Zero Degree of Temperature
Entropy S0 as T0 Kelvin
3
Study of heat engines
Being studied by all students in physical science and engineering
4
5
Concept of State ),( TPVV
6
From Avogadro’s hypothesis the volume per mole of all ideal gases at 0oC and 1atm pressure is 22.414 litres.
molereejoulesmolereeatmlitresR
RTPV
molereeatmlitremolereelitresatm
oToVoP
.deg/3144.8.deg/.082057.0
.deg/.082057.0.deg16.273
414.221
7
For n mole gas
PV=nRT
8
For water vapour, the number of moles for Kg water is obtained by
molmolg
g
M
massn 56.55
.18
10001
9
Thermodynamics
Process
Work and Energy
Heat
10
11
1. Open system- material and energy exchange
2. Closed system- energy exchange only
3. Isolated system- no material and energy exchange
12
What we learn from this module?
1.Internal energy U and entropy S 2.Combining U and S with P, T and V gives enthalpy H=U + PV and Gibbs energy G=H-TS 3.H is related to heat adsorption or release at constant pressure
4. G controls the position of equilibrium in closed systems at constant temperature and pressure.
13
Why is Thermodynamics useful? 1.Qualitative explanation of materials behaviour 2.Quantitatively understanding of materials status.
3. Physical significance of thermodynamic functions.
14
Applications of Thermodynamics 1.Extraction, refining 2.Corrosion 3.Phase transformation-phase diagram calculation 4.Materials processing 5.Design of new materials.
15
The First Law of Thermodynamics Conservation of Energy Principle Same principle in mechanics, physics and chemistry
wqiUf
UU
16
17
18
19
Work done in an Expansion (or contraction) against an External Pressure
dVfinalV
initialVextPw
VVextPVextPw
xAextPw
AextPFAF
extP
xFw
)(
)(
)12
.(
.
20
Expansion against a constant external pressure
final
v
initialv
VextPinitial
vfinal
vextPdVextPw )(
21
W12
Q12
Reversible process
22
Reversible process and Maximum Work
Reversible process for a closed system
W system-environment =W environment-system
Q environment-system =Q system-environment
final
v
initialv
dVextPesw
max
int
wsewesw
dVfinal
v
initalv
Psew
23
24
For an ideal gas
VnRTP
int
dVfinal
v
initialv V
nRTw
)()(lnmax initialv
finalvnRTrevqw
For isothermal process,
ie. T=constant
25
Questions*:
1. How to calculate W for a constant pressure process?
2. How to calculate W for an isothermal reversible process?
3. Is a constant pressure process an reversible process? Explain why?
* All of these questions are concerned with ideal gas systems.
26
Example:Gas compress during quasi-equilibrium processing, with PV=constant. The system is the gas P1=101325 N/m2, V1=0.01m3, V2=0.005m3
Find W
W=-702J
27
Enthalpy U=q-w Q Heat is transferred due to the presence of a temperature difference.
Work here is considered as the work of expansion.
U results from the oscillation of atoms or ions in solid and movement of the particles in gas and liquid.
Q and w depend on how the change is carried out where the difference between them does not.
At constant volume, w=0 and U=q
28
The Enthalpy Function
PVUH
VPU
initialPV
initialU
finalPV
finalU
initialH
finalHH
)()(
VPw
wqU
.
qVpVPqVPwqVPUH
....
When P=constant
29
At constant pressure, the change in enthalpy is equal to the heat
The change of enthalpy is independent of path.Q: Does q or W depend on path?
For the change involving solids and liquids, HU, but for gases, HUQ:explain why?
30
Example 1: Given p=constant=101.3 kPaV1=1m3, V2=2m3
Q12=200kJ
Find a) Ub) an expression for Q12 in terms of
thermodynamics properties for a quasi-equilibrium process.
31
Example 2. Given T=T1=T2=constant for the
processP1=200 kPa, T1=300K
V1=2m3, V2=4m3
Find a) W and b) Q
W=277KJ
32
Heat Capacities (Cp and Cv)
a) Under constant volume conditions Cv- all heat supplied increases energy of sampleb) Under constant pressure conditions Cp- Heat supplied increases energy of sample and provides energy for work performed.
TqC
33
Relation between Cv and U The 1st Law When V=constant Therefore
T
qvC
0
w
wqU
qU
vT
U
vT
UvC
TvCU
.
34
For n moles of materials over small ranges in temperature Cvconstant
TvnCiTf
TvnCU )(
35
Relation between Cp and H At constant pressure
Over small range of T for n moles of materials
T
qpC
pT
H
T
HpC
T
HpC
TpCH
.
TpCH
TpnCiTf
TpnCH )(
36
Summary At constant volume At constant pressure Molar heat capacity at constant pressure Molar heat capacity at constant volume
Uq
Hq
PT
HpC
vT
UvC
37
Questions:
1. For a constant temperature process of an ideal gas, prove H=U.
2. For a gas system, explain why Cp is larger than Cv?
3. For a solid/liquid system, explain why Cp is close to Cv?
4. What are the equations for calculating change of enthalpy and internal energy due to temperature change?