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      Class 12 CHEMISTRY – JEE

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      • Class 12 CHEMISTRY – JEE
      CoursesClass 12ChemistryClass 12 CHEMISTRY – JEE
      • 1. Solid State
        11
        • Lecture1.1
          Crystalline & Amorphous Solid 50 min
        • Lecture1.2
          Law of Crystallography 01 hour
        • Lecture1.3
          Bravius lattice & Important Terms of solid state 48 min
        • Lecture1.4
          Type of Cubic crystal & Closest packed St. 01 hour
        • Lecture1.5
          Tetrahedral & Octahedral Void 38 min
        • Lecture1.6
          Type of Voids & Radius Ratio 44 min
        • Lecture1.7
          Type of ionic solid 59 min
        • Lecture1.8
          Defect in Solid 48 min
        • Lecture1.9
          Metallic Bonding 52 min
        • Lecture1.10
          Chapter Notes – Solid State
        • Lecture1.11
          NCERT Solutions – Solid State
      • 2. Solution and its C.P
        9
        • Lecture2.1
          Condition of solution formation, TD of Solution, Factors affecting solubility-Henary’s Law 55 min
        • Lecture2.2
          Colligative Properties, Raoult’s Law 49 min
        • Lecture2.3
          Relative lowering of V.P. & Problems 45 min
        • Lecture2.4
          Non ideal solution, Azeotropic Solution 46 min
        • Lecture2.5
          Elevation in B.P., Depression in F.P. 47 min
        • Lecture2.6
          Osmotic Pressure, Abnormal C.P. & Van’t Hoff Factor 59 min
        • Lecture2.7
          Solution – Ostwald Walker Exp. 13 min
        • Lecture2.8
          Chapter Notes – Solution and its C.P
        • Lecture2.9
          NCERT Solutions – Solution and its C.P
      • 3. Chemical Kinetics
        10
        • Lecture3.1
          Rate of reaction 37 min
        • Lecture3.2
          Differential Rate Law 38 min
        • Lecture3.3
          Integrated Rate Law 56 min
        • Lecture3.4
          Integrated Rate problems 53 min
        • Lecture3.5
          Pseudo order Reaction 40 min
        • Lecture3.6
          Reaction Mechanism 47 min
        • Lecture3.7
          Collision Model 34 min
        • Lecture3.8
          Arhenius Equation 34 min
        • Lecture3.9
          Chapter Notes – Chemical Kinetics
        • Lecture3.10
          NCERT Solutions – Chemical Kinetics
      • 4. Electrochemistry
        13
        • Lecture4.1
          Introduction & Galvanic cell 32 min
        • Lecture4.2
          Cell Notation & Cell Reaction 35 min
        • Lecture4.3
          Electrode & Cell Potential 38 min
        • Lecture4.4
          Electrochemical series 39 min
        • Lecture4.5
          The Nernst Equation 39 min
        • Lecture4.6
          Concentration cell, Battery, Corrosion 52 min
        • Lecture4.7
          Electrolysis 20 min
        • Lecture4.8
          Faraday Law 45 min
        • Lecture4.9
          Resistance & Conductance 40 min
        • Lecture4.10
          Molar & Eq. Conductance, Kohlraush’s Law 29 min
        • Lecture4.11
          Problems on Resistance & Conductance 23 min
        • Lecture4.12
          Chapter Notes – Electrochemistry
        • Lecture4.13
          NCERT Solutions – Electrochemistry
      • 5. Surface Chemistry
        11
        • Lecture5.1
          Introduction & Surface tension & surface energy 33 min
        • Lecture5.2
          Adsorption 47 min
        • Lecture5.3
          Factors affecting Adsorption 39 min
        • Lecture5.4
          Catalysis 34 min
        • Lecture5.5
          Type of Catalysis & Enzyme Catalysis 41 min
        • Lecture5.6
          Colloidal Solution 57 min
        • Lecture5.7
          Type of Colloidal Solution 43 min
        • Lecture5.8
          Properties of Colloidal Solution 50 min
        • Lecture5.9
          Protective Colloids 58 min
        • Lecture5.10
          Chapter Notes – Surface Chemistry
        • Lecture5.11
          NCERT Solutions – Surface Chemistry
      • 6. Alcohol & Ether
        8
        • Lecture6.1
          Preparation 35 min
        • Lecture6.2
          Physical Properties & Oxidation Of Alcohol 29 min
        • Lecture6.3
          Hydrates, Acetal, Ketal 38 min
        • Lecture6.4
          Tests Of Alcohol 47 min
        • Lecture6.5
          Ether Preparation & Its Properties 33 min
        • Lecture6.6
          Thiol & Thioether 16 min
        • Lecture6.7
          Chapter Notes – Alcohol & Ether
        • Lecture6.8
          NCERT Solutions – Alcohol & Ether
      • 7. Aldehyde & Ketone
        10
        • Lecture7.1
          Preparation 33 min
        • Lecture7.2
          Physical Properties, Beckmann Rearrangement, Witting Reaction 46 min
        • Lecture7.3
          Schmidt Reaction, Bayer Villegar Oxidation 22 min
        • Lecture7.4
          Aldol Condensation Reaction 40 min
        • Lecture7.5
          Cannizzaro Reaction 32 min
        • Lecture7.6
          Acyloin, Benzoin, Clasien, Perkin Condensation 28 min
        • Lecture7.7
          Reformasky Reaction, Tischenko Reaction 20 min
        • Lecture7.8
          Tests-8 40 min
        • Lecture7.9
          Chapter Notes – Aldehyde & Ketone
        • Lecture7.10
          NCERT Solutions – Aldehyde & Ketone
      • 8. Acid & derivatives
        4
        • Lecture8.1
          Preparation 31 min
        • Lecture8.2
          Chemical Reactions Of Acids 31 min
        • Lecture8.3
          Arndt Eistert, Curtius, Hvz, Hoffmann Reaction 19 min
        • Lecture8.4
          Acid Derivatives 38 min
      • 9. Nitrogen containing compounds
        4
        • Lecture9.1
          Alkyl Nitrites, Nitro Alkane 27 min
        • Lecture9.2
          Alkane Nitrile & Isonitrile 20 min
        • Lecture9.3
          Amine Preparation 24 min
        • Lecture9.4
          Properties Of Amines 13 min
      • 10. Aromatic Compounds
        7
        • Lecture10.1
          Benzene 41 min
        • Lecture10.2
          Aromatic Hydrocarbon 29 min
        • Lecture10.3
          Aryl Halides 18 min
        • Lecture10.4
          Phenol 40 min
        • Lecture10.5
          Aromatic Aldehyde 39 min
        • Lecture10.6
          Aniline 32 min
        • Lecture10.7
          Phenyl Diazonium Salts 37 min
      • 11. Biomolecules
        14
        • Lecture11.1
          Introduction & Types Of Carbohydrates 47 min
        • Lecture11.2
          D-glucose & D-fructose 50 min
        • Lecture11.3
          Reactions Of D-glucose & D-fructose 32 min
        • Lecture11.4
          Reactions Of D-glucose & D-fructose 23 min
        • Lecture11.5
          Sucrose, Maltose, Lactose 31 min
        • Lecture11.6
          Starch, Cellulose, Glycogen 27 min
        • Lecture11.7
          Reducing Sugar, Mutarotation, Osazone Formation 40 min
        • Lecture11.8
          Problems On Carbohydrates 41 min
        • Lecture11.9
          Amino Acids 48 min
        • Lecture11.10
          Peptides 47 min
        • Lecture11.11
          Proteins 18 min
        • Lecture11.12
          Enzyme & Vitamins 30 min
        • Lecture11.13
          Nucleic Acid 36 min
        • Lecture11.14
          Chapter Notes – Biomolecules
      • 12. Polymer Chemistry
        6
        • Lecture12.1
          Polymerisation Addition Reaction 32 min
        • Lecture12.2
          Coordination Addition, Condensation Reaction 24 min
        • Lecture12.3
          Division Of Polymer 41 min
        • Lecture12.4
          Examples Of Polymer 31 min
        • Lecture12.5
          Examples Of Polymer 31 min
        • Lecture12.6
          Chapter Notes – Polymer Chemistry
      • 13. Practical Organic Chemistry
        4
        • Lecture13.1
          Poc Qualitative Analysis 23 min
        • Lecture13.2
          Poc Qualitative Analysis 20 min
        • Lecture13.3
          Poc Quantitative Analysis 29 min
        • Lecture13.4
          Poc Quantitative Analysis 20 min
      • 14. P block elements II
        13
        • Lecture14.1
          VA – Elemental Properties of N family 51 min
        • Lecture14.2
          VA – Compounds of N family 43 min
        • Lecture14.3
          VA – N & Its compounds 45 min
        • Lecture14.4
          VA – Oxides & Oxyacids of Nitrogen 55 min
        • Lecture14.5
          VA – P & its compounds 31 min
        • Lecture14.6
          VA – Oxides & Oxyacids of P 31 min
        • Lecture14.7
          VIA 1 – Elemental Properties of O-Family 36 min
        • Lecture14.8
          VIA 2 – compounds of VIA elements 41 min
        • Lecture14.9
          VIA 3 – Oxygen & Ozone 47 min
        • Lecture14.10
          VIA 4 – Sulphur & oxides of Sulphur 37 min
        • Lecture14.11
          VIA 5 – Sulphuric Acid 25 min
        • Lecture14.12
          Chapter Notes – P block elements
        • Lecture14.13
          NCERT Solutions – P block elements
      • 15. P block elements III
        5
        • Lecture15.1
          VIIA 1 – elemental properties of Halogen 40 min
        • Lecture15.2
          VIIA 2 – Compounds of Halogen 49 min
        • Lecture15.3
          VIIA 3 – Chlorine & its Compounds 41 min
        • Lecture15.4
          VIIIA 1 – Properties of Noble Gas 34 min
        • Lecture15.5
          VIIIA 2 – Compounds of Noble Gas 34 min
      • 16. D block metals
        8
        • Lecture16.1
          D block – Elemental Properties 55 min
        • Lecture16.2
          Elemental Properties 01 hour
        • Lecture16.3
          Elemental Properties 53 min
        • Lecture16.4
          KMnO4 & K2Cr2O7 47 min
        • Lecture16.5
          Problems 40 min
        • Lecture16.6
          Problems 20 min
        • Lecture16.7
          Chapter Notes – The d-and f-Block Elements
        • Lecture16.8
          NCERT Solutions – The d-and f-Block Elements
      • 17. F block metals
        3
        • Lecture17.1
          Lanthanoids 52 min
        • Lecture17.2
          Actinoids 48 min
        • Lecture17.3
          Problems 42 min
      • 18. Co-ordination compounds
        17
        • Lecture18.1
          Introduction of Complex Compound, Ligands 42 min
        • Lecture18.2
          Classification of Ligands, Denticity 35 min
        • Lecture18.3
          Nomenclature of Complex Compounds 46 min
        • Lecture18.4
          Nomenclature of Complex Compounds 2 40 min
        • Lecture18.5
          Bonding in Complex Compound, Primary & Secondary Valency 44 min
        • Lecture18.6
          Concept of EAN 29 min
        • Lecture18.7
          VBT in Complex Compounds 58 min
        • Lecture18.8
          Examples on VBT in complex compounds 31 min
        • Lecture18.9
          CFT in Complex Compounds 43 min
        • Lecture18.10
          CFT for Octahedral & Tetrahedral Complex 35 min
        • Lecture18.11
          Colour & Stability of Complex Compounds 28 min
        • Lecture18.12
          Structural Isomerism in Complex Compounds 49 min
        • Lecture18.13
          Geometrical Isomerism in Complex Compounds 43 min
        • Lecture18.14
          Optical Isomerism in Complex Compounds, use of Complex 01 hour
        • Lecture18.15
          Organometallic Compounds 29 min
        • Lecture18.16
          Chapter Notes – Co-ordination compounds
        • Lecture18.17
          NCERT Solutions – Co-ordination compounds
      • 19. Environmental Chemistry
        4
        • Lecture19.1
          Introduction & Air Pollution 35 min
        • Lecture19.2
          Air Pollution 20 min
        • Lecture19.3
          Water Pollution 23 min
        • Lecture19.4
          Soil Pollution, Prevention of Pollution 16 min

        Chapter Notes – Chemical Kinetics

        The branch of chemistry, which deals with the rate of chemical reactions. the factors affecting the rate of reactions and the mechanism of the reaction. is called chemical kinetics.

        Chemical Reactions on the Basis of Rate of Reaction

        1. Fast/instantaneous reactions Chemical reaction which completes in less than Ips (10– 12 s) time, IS known as fast reaction. It IS practically impossible to measure the speed of such reactions, e.g., ionic reactions. organic substitution reactions.
        2. Slow reactions Chemical re actions which completes in a long time from some minutes to some years are called slow reactions. e.g., rusting of iron. transformation of diamond etc.
        3. Moderately slow reactions Chemical reactions which are intermediate between slow and fast reactions are called moderately slow reactions.

        Rate of Reaction

        Rate of a chemical reaction IS the change in the concentration of any one of the reactants or products per unit time. It is expressed in mol L-1 s-1 or Ms-1 or atm time-1 units.

        Rate of reaction

        = (decrease/increase in the concentration of reactant/product/time taken)

        This rate of reaction is known as average rate of reaction (rav).(rav can be calculated by dividing the concentration difference by the time interval).

        For a chemical reaction,

        Instantaneous Rate of Reaction

        Rate of a chemical reaction at a particular moment of time, is known as instantaneous rate of reaction.

        For reaction,

        Methods for measuring reaction rate (i) pH measurement, (ii) change in optical activity, (iii) change in pressure, (iv) change in conductance.

        The slowest step of a reaction was called rate-determining step by van’t Hoff.

         

        Factors Affecting Rate of Reaction

        1. Nature and concentration of reactant
        2. Temperature
        3. Surface area of reactant
        4. Radiations and catalyst
        5. Pressure of gas

        Rate Law Expressions

        According to the law of mass action, For a chemical reaction,

        aA + bB → Products

        Rate α [A]a [B]b = k[A]a [B]b

        But experimentally, it is observed that the rate of reaction is found to depend upon ‘α’ concentration terms of A and ‘β’ concentration terms of B Then,

        Rate α [A]α [B]β = k[A]α [B]β

        where, [A] and [B] molar concentrations of A and B respectively and k is the velocity constant or rate constant. The above expression is known as rate law.

        Rate Constant

        In the above expression, k is called rate constant or velocity constant.

        Rate constant may be defined as the specific rate of reaction when the molar concentrations of the reactants is taken to be unity, i.e.,

        Rate = k, if [A] = [B] = 1

        Units of rate constant or specific reaction rate for a nth order reaction is given as K = (1/Time) x (1/[Conc.]n – 1)

        Characteristics of rate constant

        1. Greater the value of rate constant, faster is the reaction.
        2. Each reaction has a particular value of rate constant at a particular temperature.
        3. The value of rate constant for the same reaction changes with temperature.
        4. The value of rate constant for a reaction does’t depend upon the concentration of the reactants.

         

        Integrated Rate Equation for Zero Order Reactions

        Integrated Rate Equation for First Order Reactions

        Half-life period (t1/2) : It is concentration independent term.

        For first order chemical reactions,

        (Vo, Vt, and ∞ are the volumes of NaOH solution used for the titration of same volume of the reaction mixture after times 0, t and ∞ respectively.)

         

        Pseudo First Order Reaction

        Chemical reactions which appear to be of higher order but actually are of the lower order are called pseudo order reactions. In case of pseudo first order reaction, chemical reaction between two sr” stances takes place and one of the reactant is present in execess. e.g., hydrolysis of ester.

        [rO rt, and r∞.. are the polarimetric readings at t = 0, t and ∞, respectively.]

        Methods to Determine Order of Reaction

        1. Graphical method

        1. Initial rate method In this method, the order of a reaction is determined by varying the concentration of one of the

        reactants while others are kept constant.

        1. Integrated rate law method In this method out different integrated rate equation which gives the most constant value for the rate constant corresponds to a specific order of reaction.
        2. Half-life period (t1/2) method In general half-life period (t1/2) of a reaction of nth order is related to initial concentration of the reactant as

        This method is employed only when the rate law involved only one concentration term.

        1. Ostwald’s isolation method This method is employed in determining the order of complicated reactions by isolating one

        of the reactants so far as its influence on the reaction rate is concerned. Temperature Dependence of Rate of a Reaction

        For every 10°C rise in temperature, the rate of reaction becomes double, but only 16% collisions increases. It can be explained by Arrhenius equation.

        Temperature coefficient is the ratio of rate constant of a reaction at two temperature differing by 10. Temperature selected are usually 298 K and 308 K

        Temperature coefficient = ℜt + 10/ℜt ≈ 2 to 3

         

        Arrhenius Equation

        Arrhenius equation is a mathematical expression to give a quantitative relationship between rate constant and temperature, and the expression is

        where, A = frequency or Arrhenius factor. It is also called pre-exponential factor

        R = gas constant

        Ea = activation energy

        Activated complex (or transition state)

        Activated complex is the highest energy unstable intermediate between the reactants and products and gets decomposed immediately (having very short life), to give the products. In this state, bonds of reactant are not completely broken while the bonds of products are not completely formed.

        Threshold energy (ET) The minimum amount of energy which the reactant must possess in order to convert into products is known as threshold energy.

        Activation energy (Ea) The additional amount of energy, required by the reactant so that their energy becomes equal to the threshold value is known as activation energy.

        ⇒ Ea = ET – ER

        Lower the activation energy, faster is the reaction.

        Different reactions have different rates because their activation energies are different.

        Larger the value of Eo, smaller the value of rate constant and greater is the effect of a given temperature rise on K

        Important points about Arrhenius equation

        (i) If ℜ2 and ℜ1 are rate constant at temperature T2 and T1; then

         .

        ii) Fraction of molecules with energy equal to or greater than the activation energy is called Boltzmann factor and is given by

        1. Ea is constant for a particular reaction.
        2. Ea does’t depend on temperature, volume, pressure, etc., but gets affected by catalyst.

        In the Arrhenius equation, when T → ∞ then ℜ = Ae° = A when Ea = 0,k = A and the rate of reaction becomes independent temperature.

         

        Role of Catalyst in a Chemical Reaction

        A catalyst is a chemical substance which alters the rate of a reaction WIthout itself undergoing any permanent chemical change.

        In the chemical reactions, catalyst provides an alternate pathway or reaction mechanism by reducing the activation energy between reactants and products and hence. lowering the potential energy barrier as shown.

        In the presence of catalyst, activation energy decreases and hence.

        where, P denotes presence of catalyst and a denotes absence of catalyst.

        Theory of Reaction Rates

        Collision Theory

        According to this theory, the reactant molecules are assumed to be hard spheres and the reaction is postulated to occur, when molecules collide with each other.

        The number of collisions between the reacting molecules taking place per second per unit volume is known as collision frequency (ZAB)·

        But only those collisions in which the colliding species are associated with certain minimum amount of energy and collide in proper orientation result in the product formation, such collisions are called fruitful collisions or effective collision.

        Here, rate = – (dv/dt) = collision frequency x fraction of effective collision

        = ZAB x f = ZAB x e-E /RT

        a

        where, ZAB represents the collision frequency of reactants, A and B e-E /RT represents the

        a

        fraction of molecules with energies equal to or greater than Ea.

        So, to account for effective collisions, another factor, P called the probability or steric factor is introduced.

        So, rate = PZABe-Ea/RT

        The Activated Complex Theory or Transition State Theory

        Reactants ⇔ Activated complex → Products

        This theory is based on the fact that bond cleavage and bond formation, involved in a chemical reaction, must occur simultaneously. Hence, the reactants are not converted directly into the products. There is an energy barrier or activated complex [intermediate product with partially formed bond] between the reactants and products. The reactants must cross this energy barrier before converting into products. The height of the barrier determines the threshold energy.

        Photochemical Reactions

        Chemical reactions, that occur on exposure to visible radiation are called photochemical reactions.

          1. The rate of a photochemical reactions is affected by the the intensity of light.
          2. Temperature has little effect on photochemical reactions.

        Quantum yield or quantum efficiency of a photochemical reaction,

        φ = (number of reactant molecules reacting in a given time / number of photons (quanta) of light absorbed ill the same time)

        Prev Arhenius Equation
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