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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States of Matter Notes &  Solution Class 11 Chemistry

States of Matter Notes &  Solution Class 11 Chemistry

States of Matter Notes &  Solution Class 11 Chemistry

Charles’ Law

  • It states that for a fixedmass of a gas at constant pressure, volumeof a gas increases on increasing temperatureand decreases on cooling. Mathematically,

V/T = k

  • Let V1 = initial volume

 T1 = initial temperature

After performing the experiment let V= final volume

T2 = final temperature

Hence, V1 ÷ T1 = k

Again V2 ÷ T2 = k

Since k = k, it can be concluded 

V1 / T1 = V2 / T2

Solution: According to Charles’s law

V2/T2  =  V1/ T1

Volume of gas expelled out = V2 – V1 ……………….. (I)

Fraction of gas expelled out = (V2 – V1) / V2 = 1- (V1/ V2)     ……………. (II)

From equation (I) V1/ V2 = T1/ T2   ………….. (III)

Putting the values of (III) in (II)

Fraction of the air expelled out = 1- T1/ T2 = (T2 – T1)/ T2

 = 750- 300 /750 = 0.6

Fraction of air expelled out is 0.6 or 3/5 th


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