1 Lec 8: Real gases, specific heats, internal energy, enthalpy
1
Lec 8: Real gases, specific heats, internal energy, enthalpy
2
• For next time:– Read: § 4-1 to 4-4
• Outline:– Real gases (Compressibility factor)– Specific heats– Special relationships for ideal gases
• Important points:– How to manipulate the ideal gas law– Energy relationships to specific heats– How to evaluate properties of ideal
gases
3
TEAMPLAYTEAMPLAY
Under what conditions is it appropriate to apply the ideal gas equation of state?
4
Besides compressibility factor, we can also use more complex
equations of state
• Van der Waals
5
•Beattie-Bridgeman:
where
6
Specific Heats
Another set of properties that is a common combination of properties are the specific heats. They show up often.
For simple compressible systems, these are:
Rlb
Btuor
Kkg
kJ are units theand
T
uc
mvv
vp
p c as units same thehas and T
hc
7
Specific Heats
• cv is called the “constant volume” specific heat
• cp is called the “constant pressure” specific heat
• These names tell you how they are determined or measured.
• These names do not limit the applicability of them to either constant volume or constant pressure processes.
8
Specific Heats
• In general, the specific heats are functions of two variables for simple, compressible systems.
• However, we will show that for ideal gases, solids and liquids, they are functions of temperature alone
9
Specific Heats and Ideal Gases:
• Joule conducted some experiments where he found that the internal energy, u, was only a function of temperature, u = u(T).
• It was independent of P or v.
• This implies that cv is also only a function of temperature for an ideal gas:
dTcdu v
10
We can start with du and integrate to get the change in u:
and dT,c du v
(T)dTcuu2
1
T
T
v12
Note that cv does change with temperature and cannot be automatically pulled from the integral.
11
Let’s look at enthalpy for an ideal gas:
• h = u + pv where pv can be replaced by RT because pv = RT.
• Therefore, h = u + RT => since u is only a function of T, R is a constant, then h is also only a function of T
• so h = h(T)
12
Similarly, for a change in enthalpy for ideal gases:
and dT,c dh p
(T)dTchh2
1
T
T
p12
13
For an ideal gas,
• h = u + RT
RdT
du
dT
dh
Rcc vp
14
Ratio of specific heats is given the symbol, k
k(T)
(T)c
(T)c
c
ck
v
p
v
p
kc
R1
c
c
vv
p
15
Other relations with the ratio of specific heats which can be easily
developed:
1-k
Rcv
1-k
kRc and p
16
For monatomic gases,
constant. isit and R,2
5cp
17
For all other gases,
• cp is a function of temperature and it may be calculated from equations such as those in Table A-2 and A-2E in the appendices
• cv may be calculated from cp=cv+R.
• Next figure shows the temperature behavior….many specific heats go up with temperature.
18
Variation of Specific Heats with Temperature
19
Tabular specific heat data for cv, cp, and k are found in Tables A-2 and A-2E
20
Assumption of constant specific heats: when can you use it?
?TTcdTcThTh 12p
T
T
p1122
2
1
where
2
TTccor
2
TcTcc 21
pp2p1p
p
Either formulation for cp will be adequate because cp is fairly linear with T over a narrow temperature range. Take your choice.
21
Rule of thumb
• Specific heats for ideal gases may be considered to be constant when T2-T1 200 K or 400 °R.
• (Note in many cases the temperature range can be significantly larger.)
22
Changes in enthalpy and internal energy can be calculated from
tabular data:
• Frequently, we wish to know h2-h1 or u2-u1 and we do not want to go to the trouble to integrate
• where cp or cv is a third-degree polynomial in T, as shown in Tables A-2 and A-2E.
dT).c(or dTc vp
23
The integration is done for us in the ideal gas tables:
Reference temperature is = 0 K and h = 0 @ Tref = 0 K for ideal gas tables.
kg
kJ
Tables A-17 and A-17 are for air.
Units are mass-based for both h and u.
24
Example Problem
Calculate the change in enthalpy of air for a temperature rise from 300 to 800 K.
a) assuming constant specific heats
b) using the ideal gas tables
25
Solution
For part a), we calculate the enthalpy difference using:
Tch p
Where,
kgK
kJ040.1)K550(c)(Tcc pavgpp
26
Solution - Page 2
K300800kgK
kJ040.1h
For constant specific heats:
kg
kJ520h
27
Solution - Page 3
For variable specific heats, we’ll use the ideal gas air tables
kg
kJ95.821h800
kg
kJ19.300h300
28
Solution - Page 4
So for variable specific heats:
kg
kJ76.521h
Recall for constant specific heats, h = 520 kJ/kg, which is less than 0.5% difference.
29
Consider incompressible substances
• What’s an incompressible substance?– Liquid– Solid
• For incompressible substances
v = constant dv = 0
30
Incompressible substances
du
dTT
u du
v
Express u = u(T,v)
But dv = 0 for an incompressible substance, so
We can take the derivative of u:
dTT
u
v
dvv
u
T
0
31
Incompressible substances
dTc du v
The right hand side is only dependent on temperature. Thus, u = u(T) only for an incompressible substance.
Recall that vv
cT
u
Thus:
32
Enthalpy of incompressible substances
h = u + pv
vpp
cT
u
T
h
•For an incompressible substance, v=const as before.
•If we hold P constant, then we can take (h/T)p and show:
33
Specific heats of incompressible substances:
dT
du
T
u
T
h
pp
cp cv
Bottom line: cp = cv = c for an incompressible substance.
34
Relationships for incompressible substances.
du = c(T) dT
2
1
2
1
T
T
12
u
u
c(T)dTuudu
35
Relationships for incompressible substances.
We can also show that:
)pv(pc(T)dThh 12
T
T
12
2
1
36
Relationships for incompressible substances
• Now, if the temperature range is small enough, say up to about 200 K (400 °F), then c may be regarded as a constant, and
• u2 - u1=c(T2 - T1)
• and h2 - h1=c(T2 - T1)+v(p2 - p1)