Course Content
Section Name Topic Name 3 Classification of Elements and Periodicity in Properties 3.1 Why do we Need to Classify Elements ? 3.2 Genesis of Periodic Classification 3.3 Modern Periodic Law and the present form of the Periodic Table 3.4 Nomenclature of Elements with Atomic Numbers > 100 3.5 Electronic Configurations of Elements and the Periodic Table 3.6 Electronic Configurations and Types of Elements: s-, p-, d-, f – Blocks 3.7 Periodic Trends in Properties of Elements
Section Name Topic Name 7 Equilibrium 7.1 Equilibrium in Physical Processes 7.2 Equilibrium in Chemical Processes – Dynamic Equilibrium 7.3 Law of Chemical Equilibrium and Equilibrium Constant 7.4 Homogeneous Equilibria 7.5 Heterogeneous Equilibria 7.6 Applications of Equilibrium Constants 7.7 Relationship between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G 7.8 Factors Affecting Equilibria 7.9 Ionic Equilibrium in Solution 7.10 Acids, Bases and Salts 7.11 Ionization of Acids and Bases 7.12 Buffer Solutions 7.13 Solubility Equilibria of Sparingly Soluble Salts
Section Name Topic Name 10 The s-Block Elements 10.1 Group 1 Elements: Alkali Metals 10.2 General Characteristics of the Compounds of the Alkali Metals 10.3 Anomalous Properties of Lithium 10.4 Some Important Compounds of Sodium 10.5 Biological Importance of Sodium and Potassium 10.6 Group 2 Elements : Alkaline Earth Metals 10.7 General Characteristics of Compounds of the Alkaline Earth Metals 10.8 Anomalous Behaviour of Beryllium 10.9 Some Important Compounds of Calcium 10.10 Biological Importance of Magnesium and Calcium
Section Name Topic Name 12 Organic Chemistry – Some Basic Principles and Techniques 12.1 General Introduction 12.2 Tetravalence of Carbon: Shapes of Organic Compounds 12.3 Structural Representations of Organic Compounds 12.4 Classification of Organic Compounds 12.5 Nomenclature of Organic Compounds 12.6 Isomerism 12.7 Fundamental Concepts in Organic Reaction Mechanism 12.8 Methods of Purification of Organic Compounds 12.9 Qualitative Analysis of Organic Compounds 12.10 Quantitative Analysis
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About Lesson

Partial pressure in terms of mole fraction

  • Let three gases be enclosed at

T = temperature three gases,
V = volume,
p1, p2 and p3 = partial pressure exerted on three gases respectively.

  • PA = xA pTotal

Similarly, pB = xB pTotal

PC = xC pTotal


A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.


Pressure of the gas mixture = 1 bar

Let the amount of mixture = 100g

Mass of hydrogen in mixture = 20 g

Mass of oxygen in mixture = 80 g

nH = 20/ 2  = 10 mol

nO = 80 / 32 = 2.5 mol

Using the formula,

pH = XH x Ptotal = (n/ nH + nO) x P total   = (10 / 10 + 2.5 ) x  1 

= 0.8 bar

Kinetic molecular theory of gases

  • Molecules are point masses having no volume.
  • Gas atoms apply no constrain on different atoms unless they suffer collision.
  • Collisions of particles with each other or with the boundaries of container do not result in decreased energy system.
  • The atoms of a gas are in consistent and irregular movement.
  • The temperature of a gas relies upon its average kinetic energy 1/2 mv2 = 3/2 KT
  • Ideal gas possesses kinetic energy.

Behaviour of real gases: deviation from ideal gas behaviour

  • The isotherm obtained in the graph by plotting the pressure (P) vs Volume (V) for real gas does not coincide with the slope of ideal gas.
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