Summary: Thermodynamics

Reversible Irreversible process
Thermodynamics process
beoeiieised cannot beoeveosed
Reactant > Product
energy changes .
Changes can .



Changes .




force is much
Bond Endothermic Driving force should be infinite Driving greater
Breaking Bond formation Exothermic
-
-




simally greater than opposing than
opposing force .




Some
important teams :
force .




System of universe which is under observation
specific part Place in small steps and takes finite time and
usually
-




.




very
surrounding part excluding Rest of universe the
system takes infinite time to
complete a
single step process
-




. .




Boundary Anything which separates system
-


and
surrounding .
the
process .




Ideal All natural process
of process .




Types system :



virtual
which system is in
system is in
equilibrium
1) Open system -


can
exchange energy as well as matey .




at
Closed but not matter
equilibrium any state .




only at initial and final state
exchange
.




2)
system can
energy
-



.




Pextis variable text is constant
3) Isolated
.




system cannot
exchange energy and matter
-




.




flow due to temperature different
State of which define state of
Heat /
g) Energy
:



properties any system
.




system
-



.




^ Units :

Pressure temperature volume etc w=+ve w= ve
-




> ,
.
,



1cal 4.2 Joule 25=10
>
egg
=

System
state Function -

Variable which depend upon initial and final state
1Latm= 101.3 Joule
^
.




q=+×e q= ve
-




,


Pressure Volume temperature Internal
, .
.
energy Entropy , .
1L Bat =
100 Joule
Gibbs free
energy .




Internal too V1
energy :(
Path Function -

Variable which depends on the
path followed
by sum of different
energies associated with its atoms and

system .
Wook and Heat . molecules like P E. KE
-



,
electronic
energy .
nuclear
energy
Intensive properties -


which are independent of mass Extensive
property
Density temperature pressure specific
, , .
heat ,
molar specific Heat , state Function
and
Boiling point melting point Vapour pressure viscosity we cannot find the absolute value of internal
energy
.

, ,
.




Extensive properties dependent AE
Ef Ei AE + Ve
Ef >
Ei
-

of
-
which
-




are mass
-



.




Mass Volume moles
entropy Gibbs free
energy enthalpy AE= ve
Ef< Ei
-




. , , , , ,




Internal Heat
capacity Note Gravitational is not part of internal
energy energy energy
:
. .
.




Types of
processes
:
First law of
thermodynamics AU
q -1W
: -




a) Isothermal -


Tis constant -


A-1=0
Based conservation of
b) Isobaric -



Pis constant -



AP=0
on
energy
c) Isochoiic -

His constant -111=0 Energy neither be created noo be destroyed but can

transformed from one form to another
Adiabatic
d) Heat
exchange is
9=0
.




zero
-
-




Total of universe is constant
energy always .




Cyclic process -

Initial state -_
Final state .




Isothermal process Tis constant AT=0
in state Function
-




A. > •
B
Change -_
0

a r AE=0 As -_
0
For ideal
gas ,
internal
energy depends only on -1

All =D w
AH 0 IG =D q=
-

--
<
.




D- •
c



under P
Wook Area V
graph Isochoiic His constant
- -




AV=0
process
:




W= -




/ PDV W= -


PAY 111=42-11 ,
W=0
AU=qv
internal is to heat released
Expansion V2 > V1 w= ve work done
by system change in
energy equal or
-
-




compression 1121111 W + ve work done on
system absorbed at const Volume
-
-
_

.
.
.