Course Content
Topic Name 10 Haloalkanes and Haloarenes 10.1 Classification 10.2 Nomenclature 10.3 Nature of C–X Bond 10.4 Methods of Preparation of Haloalkanes 10.5 Preparation of Haloarenes 10.6 Physical Properties 10.7 Chemical Reactions
Topic Name 11 Alcohols, Phenols and Ethers 11.1 Classification 11.2 Nomenclature 11.3 Structures of Functional Groups 11.4 Alcohols and Phenols 11.5 Some Commercially Important Alcohols 11.6 Ethers
Topic Name 13 Amines 13.1 Structure of Amines 13.2 Classification 13.3 Nomenclature 13.4 Preparation of Amines 13.5 Physical Properties 13.6 Chemical Reactions 13.7 Method of Preparation of Diazonium Salts 13.8 Physical Properties 13.9 Chemical Reactions 13.10 Importance of Diazonium Salts in Synthesis of Aromatic Compounds
Topic Name 14 Biomolecules 14.1 Carbohydrates 14.2 Proteins 14.3 Enzymes 14.4 Vitamins 14.5 Nucleic Acids 14.6 Hormones
Topic Name 15 Polymers 15.1 Classification of Polymers 15.2 Types of Polymerisation Reactions 15.3 Molecular Mass of Polymers 15.4 Biodegradable Polymers 15.5 Polymers of Commercial Importance
Topic Name 16 Chemistry in Everyday Life 16.1 Drugs and their Classification 16.2 Drug-Target Interaction 16.3 Therapeutic Action of Different Classes of Drugs 16.4 Chemicals in Food 16.5 Cleansing Agents
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  • As we know that molecules need to collide to bring about a chemical reaction, so the number of molecules participating in an elementary chemical reaction that collides to bring about the chemical reaction is called molecularity of a reaction.
  • The value of molecularity of a reaction is always a positive value.
  • Let us consider a following reaction:

A + 2B –> C + D

Here reactants are: 1 molecule of A ,2 molecules of B

Products are: 1 molecule of C , 1 molecule of D.

Therefore we can conclude that reaction is trimolecular.

 A reaction with molecularity =1 is called unimolecular.

Example, PCl–> PCl3 + Cl2

  • A reaction with molecularity =2 is called bimolecular.

Example, Cl + CH4 –> HCl + CH3

  • A reaction with molecularity =3 is called trimolecular.

2FeCl3 + SnCl2 –> 2FeCl2 + SnCl4

  • It is theoretical value and does not determine the rate of reaction. Nor does it depend upon external factors like temperature or pressure, etc.

Integrated rate equation

Chemical Kinetics

Consider the reaction

aA + bB –> cC + dD

Rate = k [A]x[B]y

-dR/dt = k[A]x[B]y

dR/dt is instantaneous rate.

Integrated rate equation for zero order reaction

-dR/dt = k[R]0=k

dR/dt = -k

∫ dR = -k ∫ dt

[R]=-kt +I

At t = 0

R0= -k .0 + I

I = R0

So the equation becomes R = -kt + R0

Graph for this is as follows:

Chemical Kinetics

Integrated rate equation for first order reaction

Rate = -dR/dt = k[R]2

 ∫ dR/R= – ∫ kt

ln R = -kt + I

At t = 0

R = R0

ln R0=-k X 0 +I

I = ln R0

So equation becomes

ln R = -kt + ln R0

ln [R0/ R]=-kt

Chemical Kinetics

Rate law

  • The representation of rate of reaction in terms of molar concentration of the reactants participating in a reaction raised to some power is called rate law.
  • It is also called rate expression or rate equation.
  • Consider a reaction:

2NO (g) + O2 (g) –> 2NO2

Rate ∝ [NO]2

Rate ∝ [O2]

Combining these two rates we derive

Rate ∝ [NO]2 [O2]

Rate =k [NO]2 [O2]

  • Where k is the proportionality constant with a definite value at a specific temperature for a specific reaction and is called Rate Constant.
  • Rate law expression = -d[R]/ dt = k [NO]2 [O2]

Half life reactions : The time elapsed in reduction of the concentration of a reactant participating in a chemical reaction to one half of its original concentration is called half-life reaction and is represented by t1/2.

Half-life for zero order reactions:

A –> B

At time t = 0 concentration of A (reactant) is a and B (product) is 0. At time t = t the concentration of A (reactant) is (a-x) and that of B (product) is x.

x = k0t à a/2 = k0t1/2 = a/2k0

t1/2 =a/2k0


y = mx

t = Independent variable. It is taken at x-axis.

m = 2k0

Half-life for first order reactions:

t = 2.303/k1 log a/(a-x)

For half-life x = a/2; t = t 1/2

½ = 2.303/k1 log a/(a-a/2) –> t1/2 = 2.303/k1 log2

½ = 2.303/kX 3.010

½ = 0.693/ k1

Rate determining step

  • The slowest step during a chemical reaction determines the overall speed of a reaction towards completion is called rate determining step.
  • Let us consider the following reaction,


  • The elementary steps of the reaction are as follows: 

Step 1:   NO2+NO2→NO+NO(Rate constant = k1, slow)

Step 2: NO3+CO→NO2+CO(Rate constant = k2, fast)

  • As the first step is the slowest step in the reaction it will determine the rate of the overall reaction. Therefore Step1 is the rate determining step of the given reaction and hence the rate expression for the given reaction is the product of rate constant and the reactants of this step.

Rate = k1[NO2][NO2]=k1[NO2]2

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