didn’t pick up on nov. 10 and 12. 4) p.4 … 15 2) p.2 … 12...
TRANSCRIPT
CCh
ap. 1
5: p
V =
nR
T
•M
ole and Avogadro’s num
ber. •
Equations of state. •
Kinetic theory of an ideal gas. •
Heat capacities.
•First Law of Therm
odynamics.
•Therm
odynamic processes.
•Properties of an ideal gas.
1
3 E
xam
s an
d 2
More
2
1)D
EC 1 (Tue): Lecture 2)
DEC 3 (Thu): Exam
4 – Chap. 12, 14 and 15 1)
P.1 … Five quick quizzes from 12, 14 and 15
2)P.2 … 12
3)P.3 … 14
4)P.4 … 15
3)D
EC 8 (Tue): Last class 4)
DEC 8 (Tue): Com
mon M
akeup Test at 7 pm
5)D
EC 11 (Fri): Final Exam – Com
prehensive (all chapters) – Please start reviewing Eaxm
1~Exam3
materials now!
6)BTW
: Your TA has Exam
3. It should have been returned to you on N
ov 16 (Mon) at Recitation if you
didn’t pick up on Nov. 10 and 12.
Calen
dar
3
Final Exam
Exam4
LAST Class
Makeup4
Class
You don’t need to work on W
eek 13 & 14
TTopics in
Ch
ap. 1
5 a
t First G
lan
ce �
Limited subjects – KEEP
checking my PH
YS201 website.
�Special arrangem
ent for MP –
you are not required to do all assigned H
Ws.
4
55
1
EEqu
atio
n o
f Sta
te: pV
= n
RT
�
You are now familiar with “Equation of
motion”: F = m
a
�N
ow, imagine a device that we could
vary temperature (T), volum
e (V), pressure (p), and the am
ount of sam
ple.
�It would show that V is proportional to the m
oles of sample (n), that V varies
inversely with p, and that p and/or V vary in proportion to T.
�Results lead to form
one equation to describe the overall behavior of an ideal gas: pV = nRT
6
Visualize the equation with the figure.
KKey N
um
bers a
nd E
qu
atio
ns
7
Equation of State in “Per mole” basis
in “Per molecule” basis
P V = n R T ; R = ideal gas constant
Two types of equations.
HH2 O
Molecu
les
8
M = N
A x mH2O
mH2O
= 29.9x10-24 g/m
olecule from
Example 15.1
Be familiar with M
olar mass.
MMolecu
lar S
peed
Distrib
utio
ns
�M
olecules move at a distribution of speeds
around a mean velocity for any given
temperature (T). See Exam
ples 15.5 – 15.6.
9
Check visually the locations of “m
p”, “avg” and “rms”.
KKin
etic Molecu
lar T
heo
ry
�Gases m
ay be treated as point particles undergoing rapid elastic collisions with each other and the container�
Pressure
10
Chap. 8
Check two equations
PP, V
, an
d T
Plo
ts �
Especially useful to plot p and V at constant T for a range of tem
peratures. In this way we can generate a 3-D
surface of isotherm
al lines and make
predictions of an ideal gas’s behavior.
11
�Adiabatic: have no heat transfer in
or out of the system
�Isochoric: have no volum
e change. �
Isobaric: no pressure change. �
Isothermal: no tem
perature change.
Read p-V graphs
ppV
= n
RT
(Idea
l Gas)
12
M = N
A x mH2O
mH2O =29.9x10
-24 g/molecule
VVisu
al E
xam
ples o
f “Work
”
13
Note: they are signed num
bers
F x �x = p (A �x) = p �V
Check visually the “work” corresponds to the “area” in p-V graph.
114
[extra Q] total work from
d to a?
115
[Q1] total work from
a � b �
d? [Q
2] total work from d �
b � a?
EExa
mple Q
uestio
ns
16
Note that there is no
dependence on “m”
EExa
mple 1
5.3
17
3
4
p = gauge pressure + 1 atm
1
2 M
olar mass
�Absolute pressure is zero-referenced against a perfect vacuum
, so it is equal to gauge pressure plus atmospheric
pressure. �
Gauge pressure is zero-referenced against ambient air pressure, so it is equal to absolute pressure m
inus atm
ospheric pressure.
EExa
mple 1
5.3
(II)
18
MMore E
xam
ples
23
AAvo
gadro
’s Nu
mber
�6.022x10
23 molecules/m
ol: A
number to describe a set
count of atoms, like “dozen” is
a standard set for eggs.
�Approxim
ately 100 billion (1.0x10
11) stars in in Milky
Way galaxy.
�It would take a trillion (1.0x10
12) Milky W
ay galaxies to contain as m
any stars as there are particles in a m
ole.
24
�Two dozens of eggs �
24
�Two m
oles of gas � 12 x 10
23
�M
olar mass: M
= NA x m
molecule
�W
ater (a liquid at 18g/mol),
Nitrogen (a gas at 28g/m
ol), Table salt (sodium
chloride, a solid at 58g/m
ol).
�m
H2O =29.9x10
-24 g/molecule
from
Example 15.1
RRef. 1
: Model o
f Kin
etic Pro
perty
25
Chap. 8 Eq. 8.3
T2
T3
Fig. 15.12
Kav = (1/2) m
v2
Chap. 7 Eq. 7.3
RRef. 2
: Deta
ils of K
inetic P
roperty
26
V, N, T
�p = pf,i – p
i,x = (040 kg)(+30 m
/s) – (0.40 kg)(-30 m/s)
=2 (Mass) x |v
x | vi,x = 30 m
/s
vi,x = -30 m
/s
Chap. 8
Container
oN = N
umber of particles in
volume V
o
Num
ber of particles per unit volum
e is N/V
RRef. 3
: Deta
ils of K
inetic P
roperty
27
V, N, T, p
oN = N
umber of particles in
volume V
o
Num
ber of particles per unit volum
e is N/V
o
pV = n R T � pV = N
k T
�p = pf,i – p
i,x = (040 kg)(+30 m
/s) – (0.40 kg)(-30 m/s)
=2 (Mass) x |v
x | vi,x = 30 m
/s
vi,x = -30 m
/s
Chap. 8
Container
Kav = (3/2) k T
(3/2) nR T = N
Kav = K
trans
Kav = (1/2) m
v2 22
8
Ch
ap. 1
5 fo
r Exa
m4
Chap. 15.1 Chap. 15.2 Chap. 15.4 Chap. 15.5 (only Eq.15 & 15.16) Chap. 15.6
WWh
ere We A
re as o
f Nov 2
4?
29
Exam 4
330
[Q] H
ow do I study? Repeat MP problem
s? [A
] If you have completed M
Ps with your own notes on problem
s, then review my slides with your notes. M
y slides are reflection of what I was/am
thinking. See “reflection” for each exam
at URL.
[URL]
http://people.physics.tamu.edu/kam
on/teaching/phys201/class/2015C/2015C_U
ntil_Exam3.htm
l
Q&
A a
fter Nov.2
4 C
lass
331
2
m
c
Part 2
: (Reca
p) H
eat C
apacity
�Substances have an ability to “hold heat” that goes to the atom
ic level.
Q
= m c �T
[J] = [kg] [?] [K]
�c = specific heat capacity [J / (kg * K)]
�cwater = 4.19 x 10
3 J/(kg*K) vs. ccopper = 0.39 x 10
3 J/(kg*K)
[Q] W
hat is c? How
effectively the
substance can
hold heat. [Q
]W
hyQ
isproportional
tom?
Thevibration
ofeach
atomis
areason
forholding heat. “M
any atoms” m
eans holding more heat.
[Q] W
hy Q is proportional to �T?
It also
depends on
how much
the heat
transfer is made.
32
“Per kg” basis
333
Mola
r Hea
t Capacities
C = Heat capacity for 6 x 10
23 molecules
“Per mole” basis
Q = m
c �T
334
Fin
din
g CV
Q = �K
35
CV =
(3/2) R
CV = (3/2) R
Q = �K
Monatom
ic molecules
Diatom
ic molecules
Why?
336
�M
olecules can store heat energy in
translation, rotation
and vibration.
�Table 15.3 to guide you through a calculation.
CV =
(3/2) R
+ R
= (5
/2) R
“Per molecule” basis
“Per mole” basis
337
3
PPart 3
: Th
ermodyn
am
ic Pro
cesses �
A process can be isochoric and have no volum
e change. �
A process can be isobaric and have no pressure change.
�A
process can be isothermal and have no tem
perature change. �
A process can be adiabatic and have no heat transfer in or out of the
system.
38
339
�In sim
ple terms, “the heat
added to a system will be
distributed between internal energy (�U
) and work (W)”.
�“W
ork” is defined differently than we did in earlier chapters, here it refers to a p�V (a pressure increasing a volum
e).
Th
e First L
aw
of T
herm
odyn
am
ics
Q = �U
+ W
Q = n C
V �T + p (V2 – V
1 )
440
Th
e First L
aw
of T
herm
odyn
am
ics
Q = n C
V �T + p (V2 – V
1 )
�In sim
ple terms, “the heat
added to a system will be
distributed between internal energy (�U
) and work (W)”.
�“W
ork” is defined differently than we did in earlier chapters, here it refers to a p�V (a pressure increasing a volum
e).
�Note on the sign convention.
Q = �U
+ W
441
�In sim
ple terms, “the incom
e to a household will be distributed between Saving and Spending”.
�“Spending” is defined differently than we did in earlier chapters, here it refers to a p�V (unit price tim
es volume).
Th
e First L
aw
of P
aych
eck
Q = n C
V �T + p (V2 – V
1 )
Paycheck = Saving + Spending
= +
442
Blank Page
443
“Work
” = A
rea in
p-V
graph
Incremental, reproducible
changes may be sum
med.
Example 15.8(a)
Example 15.9
MMore V
isual E
xam
ples
44
445
P1
5-7
8
�A
process can be adiabatic and have no heat transfer in or out of the system
�
Q = 0
�U = n C
V �T
Q = �U
+ W �
W = ���U
446
P1
5-7
8
�A
process can be adiabatic and have no heat transfer in or out of the system
�
Q = 0
�U = n C
V �T
Q = �U
+ W �
W = ���U
551
“Work
” in Iso
therm
al P
rocess
W = n R
T ln(V2 / V
1 )
IIsoth
ermal E
xpan
sion
�
Exam
ples 15.8, 15.9, and 15.10
52
You heat a sample of air to tw
ice its original temperature
in a constant-volume container. The average translational
kinetic energy of the molecules is
A. half the original value. B
. unchanged. C
. twice the original value.
D. four tim
es the original value.
Kav = (3/2) k T
Q = n C
V ��T + p (V2 – V
1 )
53
You heat a sample of air to tw
ice its original temperature
in a constant-volume container. The average translational
kinetic energy of the molecules is
C. tw
ice the original value.
554
You compress a sam
ple of air slowly to half its original
volume, keeping its tem
perature constant. The internal energy of the gas
A. decreases to half its original value. B
. remains unchanged.
C. increases to tw
ice its original value.
Kav = (3/2) k T
Q = n C
V ��T + p (V2 – V
1 )
55
You compress a sam
ple of air slowly to half its original
volume, keeping its tem
perature constant. The internal energy of the gas
B. rem
ains unchanged.
556