Biology digital notes for highschool students. Easy to read and understand illustrative notes. Detailed explanation of every topic. Reading of this document is tough for understanding the important concepts of the topic
Thermodynamics
Definition: the branch of science which deals with the study of
exchange of energy is known
Note: therm dynamics gives the information about the process wheather
it will take place at a certain condition.
Limitations:
thermodynamics is applicable for those matter which are in bulk . it is
not applicable for individual molecules, atoms, or particles
thermodynamics does not give information about time consumed in
a process imaginary boundary
M
-
~
&
& I
Note: according to thermodynamics this universe is
made up of t wo parts that is system and surroundingsurrounding
~
- -
system
- -
& ~
System is the object which is under the investigation
-
~
~
Surrounding is the part of universe which surrounds the system
Boundary is the the system to device which separates the system to
surrounding
Types of system
Open system: In which both heat & matter isexchange bet ween
system & surrounding. Ex: uncovered cup of hot tea
Closed system: In which only heat is exchanged bet ween system &
surrounding and matter is not. Ex: covered cup of hot tea
, Isolated system: In which neither heat nor matter is exchanged
bet ween system & surrounding. Ex: thermostat
Thermodynamic variables:
The variables which define the state of a system. Ex:T, P, V etc
Thermodynamics process: the process by which the state of a system is
changed from initial to final
Types of thermodynamic process:
Isothermal process : the process in which temperature remains constant
during the change in state of system from initial to final
Isobaric process: the process in which pressure remains constant
during the change in state of system from initial to final
Isochoric process: the process in which volume remains constant during
the change in state of system from initial to final
Adiabatic process : the process in which heat remains constant
during the change in state of system from initial to final
Type of process on the basis of driving and opposing force
Irreversible process Reversible process
→ mono directional → bi directional
→ driving force not = opposing force → Driving force = opposing force
→ P(ext) not = P(gas) →P(ext) = P(gas)
→ Occurs in large & finite steps → occurs in small & infinite steps
→ summation & subtraction take place → integration & differentiation
, !a
Extensive Properties Intensive properties
→ physical properties which depend → physical properties which do not
on the amount of substance depend on the amount of substance
→ Example : Mass, volume, energy → example: temperature,
pressure, density, conductivity,
Note: extensive = intensive resistivity
extensive
State function Path function
→ the functions whose value → the functions whose value
depends on the initial & final depends on the path by which the
state of the system & do not state of a system is changed from
depend on the path followed initial to final state
→ example : T, P, V, U, H,S, G → example: W, q, Cp & Cv
(heat capasity)
→ for cyclic process
→ for cyclic process
Internal energy (U or E) : the summation of all energy present in a
system. It is a state function & an exclusive property.
Internal energy = translational + potential + vibrational + nuclear
1 ATM = 101 joules
1 bar litre = 100 joules
1 calorie = 4.18 joules
Gas constant R = 8.3144598(48) J⋅mol−1⋅K−1
, Sign conventions Expansion Compression
II B II A
Heat given to system q= +ve
Heat released by system = -ve I A I
B
:...
I
. . . R.
Work done by the system w = +ve .
-
-
C
.....
Work done on the system = +ve
-
~
~
"heat heat
Zeroth law of thermodynamics
According to this law, if body A and B are at thermal equilibrium and body
B and C are also in thermal equilibrium at same time and therefore body A
and c will also be in thermal equilibrium.
Note: the thermometer is the device based on the zeroth law of
thermodynamics.
Heat capacity
Total heat capacity is defined as the change in heat with change in
temperature by 1°C or 1K
if d+ =
1 °
X dt
dq
Where C is a constant dt C =
dq
known as total heat dq = c .
capacity of the matter c =
dq
Unit of C = J/K or J/C
dt
Specific heat
→ the heat change of 1 gram/ 1 kg arises by changing the temperature
of 1 C or 1 K
(Heat capacity for 1 gram of substance)
CsH CT 1C 1K
if d+
=
W =
19 -
= =
W
CsH 1 da
CSH =
dq
X
Unit = J/Kg K = J/gm C
=
W dt
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