Thermal expansion

5. Linear Expansion

13. Superficial Expansion
Volumetric expansion (cubical expansion)

16. Effect of Temperature on Density :-

17. Expansion of liquid in a container :-

18. Anomalous behaviour of water :-

19. Heat

20. Specific heat : (C or S)

25. Heat capacity or (Thermal capacity) :

26. Water equivalent :

27. Principle of calorimetry :

29. Latent heat :

30. Heating Curve :

33. KINETIC THEORY OF GASES (KTG)
Assumption (Postulates of Ideal Gas)
(i) The ideal gas molecules are tiny spherical particles.
(ii) The size of ideal gas molecules is negligible. So the
volume of container taken as volume of gas.
(iii) Their is no attraction or repulsion between ideal gas
molecules.
(iv) The effect of gravitational force on ideal gas
molecules is negligible. So the density of gas in the
container will be uniform.
(v) Ideal gas molecules can move in all direction with all
possible velocities. (0 to  velocity).
(vi) The ideal gas molecule continuously strike with each
other and with the walls of container.

34. KINETIC THEORY OF GASES (KTG)
(vii) The collision of ideal gas molecules will be elastic.
(viii) Ideal gas molecules continuously strike with the walls
of container. So transfer momentum and hence
applying force and pressure on the walls.
(ix) Ideal gas molecules follow newton's second law of
motion.

35. (x) Ideal gas molecules travel in straight line between two
collisions and the distance travelled between two
collisions is known as "free path (l)".

36. Meaning of NTP :

39. Ideal gas equation :

40. DIFFERENT SPEED AND VELOCITY OF GAS :
(1) Instantaneous Velocity :
Velocity of a molecule at any instant is known as
instantaneous velocity.
(2) Average velocity : (3) Average momentum :

41. (4) Average speed (Mean Speed) :

42. (5) Root Mean Square Velocity (Vrms) :

44. (6) Most probable speed (Vmp) :
The speed by which maximum number of molecules of a
gas are moving is known as most probable speed.

45. (7) Velocity of sound in a gas :

49. Total pressure in x-direction-

52. Gas laws:
(1) Gay-lussac law-

54. (2) Charle's law

55. (3) Boyel's law-

56. (4) Dalton's law-
(i) If different gases are mixed in a container then
according to Daltons law the total pressure in the
container will be equal to sum of partial pressure of
each gas

57. Maxwells law of equipartition of energy-
(i) According to maxwells law, the total kinetic energy of a
a gas
is equally divided into its degree of freedom and each
degree of freedom has
1
2
RT or
1
2
kT kinetic energy.
(ii) K.E. of 1 mole and 1 degree of freedom =
1
2
RT
K.E. of n mole and f" degree of freedom =
nfRT
2
K.E. of "1 molecule & 1 degree of freedom =
1
2
kT
K.E. of "N molecule & "f degree of freedom =
NfkT
2

59. LAW OF MIXTURE :-
(i) Law of conservation of moles-
Case-I Initial Final

60. Note: If temperature is not given
Temperature T = constant

61. Case-2 Initial Final

62. (2) Law of conservation of energy-
Initial Final

63. Law of energy constant :

65. Mean Free Path ( l ) :
The average distance travelled by a molecule between
two collision is known as mean free path.
_

66. According to Maxwell :

67. 3. Dependency of l :
_

69. 4. Mean time of collision (t) :

70. Real Gas Equation : (Vander waal Equation)
1. Volume correction :
The size of ideal gas molecule is negligible so volume of
container can be taken as volume of gas but the size of
real gas molecule is not negligible. So that volume of gas
(the volume in which molecules can move freely) will be
less than volume of container and according to Vander
waal the decrease in volume is a constant 'b'.

72. 2. Pressure correction :
There is no attraction and repulsion force between ideal
gas molecules but in case of real gases at low
temperature and high density attraction force between
the molecules exist. So the pressure applied by the
molecules on the container decreases. According to
vander Waal decrease in pressure.

73. Note : The real gas at high temperature and low
density behaves as ideal gas.