this is my maharashtra board topic cover chapter chemical kinetic still improving them.

1. Chemical
Kinetics

2. Chemical Kinetic
-
- 'Movement'
Branch of Science that deals with
“rate of reaction, mechanism of
reaction and Factor affecting rate of

3. Industry company very much interested in
chemical kintic.
becouse when two molecule interact
collision occure and chemical reaction
take place. product is formed.
company intereseted in how much product
formed what time it take.
if reaction fast product form fast net
profit fast.

7. Fast reaction:-
This rxn we already
done in qualitative
analysis practical.
For detect of
halogen. When we
mix AgNO3 quickly
white ppt form.

8. It take
million of
year for
rusting
metal.

14. RATE OF
REACTION IS
“change in
concentration
per unit Time.”

16. Graphically
Representation of Rate of
reaction

19. Concentra
tion = n/V

24. the rate at any
particular instant.
change in
concentration at
definite time.

25. Average rate
of reaction &
Graph

35. Pressure
Light
1.
2.
3.
4.
5.
6.

39. Suppose we
take glass of
water
But we have two
type of sugar
with us.

44. Law of mass
action
Rate Law

53. Unit Rate of reaction

58. Molecularity of
Reaction

60. Molecularity
2HI → H2 + I2 Bimolecular
NO + O3 → NO2 + O2 Bimolecular

62. Difference between Order
and Molecularity

63. Moleculariy Order of Reaction
It is the total number of reacting
species (molecules, atoms or
ions) which bring the chemical
change.
It is the sum of powers of molar
concentration of the reacting
species in the rate equation of
the reaction.
It is always a whole number. It may be a whole number, zero,
fractional,
It is a theoretical concept. It is experimentally determined.
It is meaningful only for simple
reactions or individual steps of a
complex reaction. It is
meaningless for overall complex
reaction.
It is meant for the reaction and
not for its individual steps

64. Such type of
reaction take
place through a
sequence of two
or more
consecutive
steps.

65. Complex and elimantory
reaction
Mechanism and rate
detemining step, Intermediate

70. Integrate rate laws for 1st order

75. First order reaction
Graphical Representation
integrated

76. A  Product
R = -d[A]/dt = k[A]t + 0
Y = m x + c

79. First order reaction
Graphical Representation

84. First order reaction
Three fourth life

88. Zero order reaction defined as Reaction
whose rate is independent of the
reactant concentration and remains
constant throughout the course of the
reaction.
Differential rate law of
Zero order reactio

91. Zero order reaction
Integrated Rate law
Alternative fomr of integrated

96. Zero order reaction
Graphical Representation

98. [A]t

99. Zero order reaction
Half life
Graphical Representation

103. Example of zero order reactions
• Decompostion- on Pt surface
2NH3(g) → 𝑵𝟐 𝒈 + 𝟑𝑯𝟐(𝒈)
2N2O(g) → 𝟐𝑵𝟐 𝒈 + 𝑶𝟐
PH3 on hot tungston at high pressure
unreacted fully.

104. Such reaction that have higher
order true rate law but are found
to behave as first order are
called….
Pseudo first order reaction

105. Order is an
experimentally
determined
value.
Every reaction can
have only one
particular order.

106. It happened
in those
reaction
which
contain one
solvent.

110. Apparent
order also
called fake
order.

114. Determining
order of
reaction
Integrated
method
isolation
method
Initial rate
method
Half time
method

123. Arrhenius Equation

124. Svante
Arrhenius
Svante August
Arrhenius
19 February 1859
Wik Castle, Sweden

127. Effect of Temperature on rate of reaction

132. Maxwell and Boltzmen Destribution

136. Effect of Catalyst on rate of reaction
'+' and '-' Catalyst

141. Catalyst lower the energy
barrier.

142. Svante August
Arrhenius
19 February 1859
Wik Castle, Sweden

143. Relationship between rate
constat at Different
Temperature

145. Collision Theory

150. 2. Energy requirement:- (Activation Energy)
REACTANT
PRODUCT

154. Affective
collision
when
element are
arranged in
proper
orientation.