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A comprehensive overview of thermodynamics, covering fundamental concepts, definitions, and key principles. It includes detailed explanations of various thermodynamic processes, such as isobaric, isochoric, isothermal, and adiabatic processes, along with their applications. The document also explores important thermodynamic functions, including internal energy, enthalpy, entropy, and gibbs free energy. It further delves into the concept of heat capacity and its different forms, including specific heat capacity and molar heat capacity. The document concludes with a discussion of the laws of thermodynamics, emphasizing the first law and its implications for energy conservation. Enriched with numerous exercises and examples to reinforce understanding and facilitate learning.
Typology: Study notes
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System
part
of
is
for
thermodynamics
is
called
system
types
open system
closed
system
Isolated
system
Isolated
Heat
fax
heat gain
heat
2
The rest part
of
is
known as
surrounding
boundary
3
Boundary
which
separate system (^) surrounding
of
boundary
1
Rigid
ΔV O^ volume
fixed
Non
Rigid
ΔV
O volume flexible
Ballon
Diathermic 19
0
flow
allowed
Adiabatic 19
0
5 Permeable
Am 0
of
matter
allowed
6
Impermeable
AM (^0)
IFImaginary
f
IS
4
Thermodynamic
Process
If
any
thermodynamic
is
changed
is
called process
PUT HUGS (^) WE
Isobaric process (^) PressureConstant P O
2 Iso (^) choric Process
0
3
Temp
constant Δ
T O
Adiabatic
0
5
Cyclic
process
made
of
two or^ more procex
Question
Prove
that Volume
of
an (^) ideal
gas is
PV NRT
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J
V f
ever's
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p
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81
1
1
4
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YE
I
pressure
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step
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time (^) It occurs
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steps
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in eqbm
at
only
equilibrium initial final
state
4 occurs against
constant external
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ΔH Enthalpy Concentration term
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molarity
molality
mole
etc
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of
extensive
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time Force
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mass
capacity
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or
specific
specific
etc
heat
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nature
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Index
PH
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etc
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8
Capacity
C
forany
Specific
Heat
Capacity
for
gram
Molar
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capacity
for
mole
what
is
a
system
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energy
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is
form
of
energy
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at
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of
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re
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capacity
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of
required
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of
a
mole
substance
by
IK
e
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gram
n molesubstance Ko AT^ temp Seine (^) Kaineke
g
heatrequired
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g
heat
h (^) mole
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Capacity
em
nay
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Heat
capacity
em
what
is
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T T
Capacity
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nIygy1g
m
mwt_sxm.wt
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ka (^) special
Meeting
9
Molar
Heat
Capacity
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Heat
capacity
at constant
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heat
can
vary
from
0 too
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for
Isothermal
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Gy
Adiabatic prose
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y
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an
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volume
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not
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not
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y Pressure
0
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me
ER
y
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R
Ti
eyer's
10
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work
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a Fx
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angle
between
force displacement
is
mechanical
If
displaced (^) from
one
place
to another then
is
done
I
what
is thermodynamic^
work
If
Volume
of
system is
changed
by any
process
is
done
Isobaric Isochoric Isothermal
1
p p
site
v v
open
cyclic
cyclic
cloxed closed
a 3
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e
a.no
re
p P
20
v v v
Prove
that (^) close wixe Work
done
is
negative
Process W.D
(^0) to
of
Isochoric Procex
0 a
work re
re
a
work ve
Isobaric compression
the
V
more
to the^ work^ done
work
done will be^ we
Prove
that (^) AntiClose^ wixe Work
done
is
positive
Process WD 0 a a
gap B (^) C Isobaric compression
WD re
Isochoric Procex
wD o
work
WD the^ work ve
work
done
of
cloxed
cyclic
system
in AnticYock direction
if
positive
Q work (^) done
Isobaric
E
W D
(^12 )
(^6) litre atm
W D
atm
king
ID
work
done
5am
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work
Done Area
WD
Ar
Peat
IT
litre
fire
glitre
T
5
atmility
work
I
(^1) atm litre Iatm^
1
litre
105
x
10
3
m
102
N.MG
Joule
forcetdisplacement
Joule
