1. Chemical kinetics: a branch of chemistry which deal about the rate of reaction.
Rate of reaction: The change in concentration of reactant or product in a given interval of time is called rate of reaction.
Rate of reaction=change in conc. of reactant
Time interval
Chemical kinetics

2. A+B C+D
Rate=-[d A]\dt = -[dB]\dt =[dC]\dt =[dD]/dt

3. Factor affecting the rate of reaction .
Concentration of reactants: The rate of reaction is directly proportional to the conc. Of reactant.
The effect of conc. of reactant is also given by law of mass action.
2 Nature of reactants: The nature of reactant is determined by its inner composition thus for ionic reaction. The ratio is very high while if the reactant not strong chemical bond the rate of reaction less

4. Temperature: the rate of chemical reaction increase with increase in temperature generally rate of reaction increase twich as the temperature is increased by 10k such effect of temperature is called temperature coefficient.
Catalyst: A catalysts is a substance which do not participate in a reaction but alter the rate of reaction.
Law of Mass action: according to this law the rate of chemical reaction is directly preoperational to the product of the molar conc. Of the reactants with each term raised to the power equal to its coefficient
aA bB Product
rate [A

5. Characteristic of rate constant
For a particular reaction the rate constant is independent of conc.
The rate constant only depends upon temperature.
The value of K is different for different reaction.
Greater the value of K greater will be the rate of reaction
A B C D K1
C D A b K2
K2=1\K1

6. If two chemical reaction are added than the rate constant are multiply
If two reaction is subtracted then the rate constant are divided.
If a chemical reaction is multiplied by n than rate constant than K2 =K1n
Molecularity: Number of molecules which participate in the elementary state in any chemical reaction is called molecularity.
On the basis of moleculatity reaction are three type.

7. Unimolecular reaction: O3 O2+[O] N2O5 N2O4 +O2\2 Bimolecular reaction:
1HI H2+ I2
NO+ O No2+ O2
Trimolecular reaction:
2NO +O NO2
2SS2+O So3
In case of complex reactions The molecularity of slowest step is considered 1

8. Order of reaction: The sum of all exponent of concentration of reaction which appear in differential rate equation is know as order of reaction it is denoted by n.
Order of reaction is an experimental value its fractional value are possible .it zero value is also possible it provided information about machanism of reaction .
aA+bB+cC=product

9. Zero order reaction : in this reactions the rate of reaction does not depend upon conc. Of reaction .
2NH N H2
rate = K[NH3]0
First order reaction:
All radioactive changes
Dissociation of ammonium nitrate
NH4NO N2O H2O
rate = k[NH4NO3]1
Decomposition of hydrogen peroxide
H2O H2O +O

10. Rate = k H2O2]
Second order reaction:
Desociation of hydrogen iodide
2HI H I2
Rate =k[HI]2
Desociation of nitrogen peroxide
2NO NO+ O2
RATE = K[NO2]
Third order reaction
Reaction between nitric oxide and oxygen
2NO +O N2O4
RATE =K[NO]2[O2]1

11. Soudo unimolecular reaction or Soudo first order reaction
Such reaction in which the molar concentration of a reactant remain partially unchanged and the small change in conc. Does not effect the rate of reaction are called soudo unimolecular reactions.
Thus , a reaction which is first order reaction but it look like second order reaction known as soudo unimolecular reaction.
Example:- hydrolysis of ester
CH3COOC2H5 +H2O CH3COOH +C2H5OH
Rate = K[CH3COOC2H5] =

12. Hydrolysis of Sucrose:-
C12H22O H2O C6H12O6 +C6H12O6
Rate = k[C12H22O11]
Units of rate constant for different order of reaction
rate = k[concentration]
Unit of k= moles/liter.sec
For first order reaction
rate =k[conc.]1
Unit of k =1\sec
For second order reaction
rate = k[conc.]2
Unit of k = liter\moles.second

13. For third order reaction
Rate = k[conc.]3
Unit of k =liter2\moles2.sec
* Rate constant for the first order reaction
A product
rate =k[A]1
consider initial conc. Of reaction be ‘a’ after ‘t’ time ‘x’ amount of product is formed
Thus the conc. Of reactant after ‘t’ time equal to (a-x) .thus
k = 1\t*log a\a-x

14. The time in which half of the reaction is called half life period.
k = log10 a
t a-x
Half life period:-
The time in which half of the reaction is called half life period.
It is denoted by ‘t1\2‘
For the half order reaction
if t =t1\2
a-x = a\2

15. t1\2 a\2 k =2.303 log10 a log102=0.3010 k =2.303*0.3010\t1\2
t1\2 =0.693\k
Expression for rate constant of first order reaction
A product
Rate =-[dA]\dt
rate = k[a]
-[dA]\dt = k.[a]
t1\2
a\2

16. -[dA]\dt = k.dt on integrating the above equation -log A =kt +c [integration constant] At t=0 , A = A0 -loge A0 = c -loge A =kt -loge A0 loge A0 -loge A =kt loge A0\A =kt k =1\t logeA0\A k = 2.303\t .log10 A0\A

17. Effect of temperature on rate constantOR
Arrhenius equation
Arrhenius gave a relation between rate constant and temperature which is known as Arrhenius equation.
According to this equation
k = A.e–Eq/RT
where , k = rate constant
A = frequency factor
EA = Activation energy
R = Universal gas constant

18. T =Temperature in Kelvin
on taking log both the side
loge K = loge A.e –Eq/RT
loge K = loge A + loge e –Ea/RT
loge K = loge A -Ea/RT loge e
loge e = 1
loge K =loge A - Ea/RT
2.303 log10 K = log10 A - Ea/RT
log1 K = log10 A - Ea/2.303 RT
for a reaction , the rate constant at t1 temperature, while at t2 temperature it will be K2 (T2 > T1) than,

19. log10 K1 = log10 A -Ea/2.303 RT1 ------------(1)
on subtracting (1) from (2)
log10 K log10 K2 =Ea/2.303 RT2 -Ea/ RT1
log10 K1/K2 = Ea/2.303R [1/T /T1]
*Theracehold Energy :
The minimum amount of energy which is required by molecules of reactant for the fruitful collision is called teracehold energy.
*Energy barrio :
The amount of energy at which molecules of reactant collides and converted into product is called energy barrier

20. Activation energy :
The amount of energy which is required by the molecules of reactant to cross the energy Barrier is called activation energy.
Activation energy = Theracehold energy - Energy of reactant