Subject | chemistry | Medium | ENGLISH |
---|---|---|---|
Faculty | NV Sir | Status | AVAILABLE |
Category | COMPLETE COURSE | Lecture | 143 |
Target | XI XII XIII | Books | QUESTION BANK ATTACHED |
You May Pay in Installments through Credit Card |
Product Type | Prices | Validity | |
---|---|---|---|
USB | 22500 60%^{OFF} 9000 | 2 year |
Lecture# | Description | Duration |
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01 | Dalton atomic theory, isotope ,isobar, atomic mass, atomic mass unit amu, molecule, molecular mass | 41 Minutes |
02 | molar mass. Gram atomic mass, gram molecular mass, avogadro law | 48 Minutes |
03 | Relative atomic mass, relative density, vapour density, specific gravity, average atomic mass, average molar mass | 44 Minutes |
04 | Percentage composition, molecular formula, empirical formula, gay-lussac law | 30 Minutes |
05 |
Stoichiometry, mole-mole analysis, combustion of hydrocarbon |
34 Minutes |
06 |
limiting reagent, percentage yield , consecutive reaction |
39 Minutes |
07 | Principle of atomic conservation POAC | 37 Minutes |
08 | Percentage purity of sample, combustion of carbon, analysis of mixture | 29 Minutes |
09 | Numerical on analysis of mixture, law of mass conservation, law of definite proportions, law of multiple proportions, law of reciprocal proportions | 24 Minutes |
10 | Solution, solute , solvent, mole fraction, %w/w/, | 18 Minutes |
11 | %w/v, % v/v, strength of solution, molarity, molality, ppm | 35 Minutes |
12 | Interconversion of concentration terms | 46 Minutes |
13 | Molarity of pure water , volume strength of hydrogen peroxide solution, relation between volume strength and molarity | 35 Minutes |
14 | Silver salt method , Eudiometry | 38 Minutes |
15 | examples of eudiometry | 27 Minutes |
16 | Significant figure, rules for counting , rounding off, scientific notation, addition/subtraction, multiplication of significant figure | 42 Minutes |
Lecture# | Description | Duration |
---|---|---|
01 | Oxidation number calculation, average O.N. individual O. N. | 44 Minutes |
02 | Oxidizing agent, reducing agent, disproportion reactions | 58 Minutes |
03 | Balancing of redox and disproportion reaction , balancing of molecular reaction | 46 Minutes |
04 | Equivalent concept. Law of chemical equivalence, relation between mole and equivalent, equivalent mass, valence factor calculation for acid & base | 45 Minutes |
05 | n- factor for salt, n - factor for disproportion reaction | 49 Minutes |
06 | Titration, acid base titration, permanganate titration, dichromate titration | 39 Minutes |
07 | Back titration , double titration | 34 Minutes |
08 | Numerical on double titration, iodometric titration, limitation of equivalent concept | 33 Minutes |
09 | Bleaching powder and calculation of available chlorine from bleaching powder sample | 31 Minutes |
10 | Hardne ss of water ( temporary & permanent hardness) strength of oleum | 35 Minutes |
11 | Volume strength of hydrogen peroxide solution | 20 Minutes |
Lecture# | Description | Duration |
---|---|---|
01 | Reversible & irreversible reactions, physical and chemical eq, homogeneous and heterogeneous eq, properties of eq, Kp, Kc, Kx, relation between Kp & Kc, relation between Kp and Kx, degree of dissociation | 1 hr 13 Minutes |
02 | Effect of stoichiometry on kp & Kc, examples of homogeneous equilibrium | 38 Minutes |
03 | Numericals of homogeneous eq. | 29 Minutes |
04 | Heterogeneous eq., homogeneous liquid eq., significance of value of k, reaction quotient | 53 Minutes |
05 | Approximation during calculation, relation between vapour density and degree of dissociation | 53 Minutes |
06 | Thermodynamics for chemical eq, factor affecting composition of eq mixture , le-chatelier's principle, effect of concentration , effect of temperature | 38 Minutes |
07 | Effect of change in pressure and volume , effect of catalyst | 36 Minutes |
08 | Addition of inert gas at constant volume and constant pressure, le-chatelier's principle for physical eq, evaporation of water, boiling of water, melting of ice , melting of metal | 1 hr |
09 | Solubility of gas in liquid , allotropic change , simultaneous eq. | 42 Minutes |
Lecture# | Description | Duration |
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01 | Strong electrolyte, weak electrolyte, strong acids, weak acids, strong base, weak base , acid base theory, arrhenius concept, bronsted lowry concept , amphiprotic species | 31 Minutes |
02 | Lewis concept , pH scale, properties of water, ionisation constant of water, ionic product of water | 45 Minutes |
03 | pH calculation for strong acid, strong base, mixture of strong acid , mixture of strong acid and base , common ion effect | 43 Minutes |
04 | pH for monobasic weak acid, weak base, ostwald dilution law, pH for very dilute strong acid | 41 Minutes |
05 | Very dilute weak base , mixture of weak acid and strong acid,polyprotic weak acid | 40 Minutes |
06 | Numerical on polyprotic weak acid, mixture of two weak acids | 33 Minutes |
07 | Hydrolysis of salt, salt of strong acid and strong base, salt of weak acid and strong base , salt of weak base and strong acid | 52 Minutes |
08 | Hydrolysis of salt of weak acid and weak base | 39 Minutes |
09 | pH for polyvalent anion, ph for amphiprotic anion , introduction of buffer solution | 37 Minutes |
10 | Acidic buffer and basic buffer | 43 Minutes |
11 | Buffer capacity, titration ( strong acid v/s strong base, strong acid v/s weak base , weak acid v/s strong base) | 53 Minutes |
12 | Titration of H3PO4 v/s NaOH | 35 Minutes |
13 | Indicator, phenolphthalein, methyl orange, pH range for a buffer ,double titration | 38 Minutes |
14 | Solubility of sparingly soluble salt, Ksp, effect of common ion on solubility, simultaneous solubility | 44 Minutes |
15 | Ionic product v/s solubility product,selective precipitation, | 41 Minutes |
16 | solubility of salt in buffer solution, complex formation by salt | 37 Minutes |
17 | Solubility of amphoteric insoluble hydroxide, solubility of salt if cation is hydrolyzed , solubility of salt if anion is hydrolyzed | 43 Minutes |
Lecture# | Description | Duration |
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01 | System ,surrounding,open system, closed system, isolated system, thermodynamic variable, process, open cycle ,closed cycle,intensive prop. Extensive prop., state function, path function, heat, work, heat capacity, molar heat capacity, specific heat capacity ,IUPAC , types of process, isothermal, isobaric, isochoric, adiabatic process,convention for heat and work | 41 Minutes |
02 | Reversible and irreversible process, reversible isothermal compression, single step isothermal compression, two stage isothermal compression | 56 Minutes |
03 | Reversible isothermal expansion, single stage isothermal expansion, two stage isothermal expansion, internal energy, degree of freedom, first law of thermodynamics | 50 Minutes |
04 | Enthalpy change , phase transformation | 46 Minutes |
05 | Free expansion, reversible adiabatic process, work calculation for reversible Adiabatic and irreversible Adiabatic processes | 43 Minutes |
06 | comparison between reversible adiabatic and irreversible adiabatic processes, comparison between reversible adiabatic and reversible isothermal processes | 42 Minutes |
07 | Spontaneous and nonspontaneous process, entropy, second law of thermodynamics , entropy change for system and surrounding | 55 Minutes |
08 | Numerical on entropy change , entropy change during free expansion | 40 Minutes |
09 | Gibbs energy change, heat pump, carnot cycle | 56 Minutes |
10 | Thermochemistry, enthalpy of formation, enthalpy of combustion | 48 Minutes |
11 | Enthalpy of fusion, vaporization,sublimation,bomb calorimeter, enthalpy of neutralisation, enthalpy of ionisation | 57 Minutes |
12 | Bond enthalpy, hess law, resonance energy. Lattice energy , hydration energy, enthalpy of formation of ion, kirchhoff equation, integral enthalpy of solution, calculation of lattice energy using born haber cycle | 1 hr 7 Minutes |
Lecture# | Description | Duration |
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01 | State of matter (solid, Liq, gas) ideal gas equation, Boyle’s law. | 32 Minutes |
02 | Barometer, faulty Barometer | 33 Minutes |
03 | Problems on barometer, Charles law | 40 Minutes |
04 | Gay-lussac’s law, Avogadro's law, ideal gas equation | 21 Minutes |
05 | Numerical | 45 Minutes |
06 | Graham’s law for diffusion. | 36 Minutes |
07 | Kinetic theory of gas, root mean square velocity | 40 Minutes |
08 | Compressibility factor (Z) pressure correction factor, volume correction factor, excluded volume, van der waal gas equation | 50 Minutes |
09 | Virial equation, liquification of gas, critical temperature (Tc) Critical pressure (Pc) Critical volume (Vc) Boyle’s temperature | 46 Minutes |
10 | Liquification of gas manometer (Open end, Closed end, reduced equation of state), Collision diameter, Collision frequency |
52 Minutes |
Lecture# | Description | Duration |
---|---|---|
01 | Cathode tube experiment anode rays, radioactive decay. | 33 Minutes |
02 | Thomson plum pudding model. Rutherford model, Nearest distance of approach. | 51 Minutes |
03 | Electromagnetic theory, Planck Quantum Theory, Blackbody radiation, electron volt. | 50 Minutes |
04 | Photoelectric effect, Work function, Threshold frequency stopping potential. | 41 Minutes |
05 | Photo current photo intensity, Bohr model, Bohr Radius | 34 Minutes |
06 | Velocity, Kinetic Energy, Total energy, Potential energy of electron in Bohr orbit | 29 Minutes |
07 | Time period, frequency, ionisation energy, ionisation potential, Excitation energy, excitation potential Binding energy. | 35 Minutes |
08 | Spectrum, emission, line spectrum, band spectrum , H-spectrum, lyman series. | 45 Minutes |
09 | Balmer series, Paschen, Brackett, Pfund, humphrey series, maximum number of spectral lines. | 50 Minutes |
10 | Limitations of bohr model, dual nature of particle, de broglie's equation | 41 Minutes |
11 | Heisenberg’s uncertainty principle Difference between orbit & orbital | 39 Minutes |
12 | Types of orbitals {s, p, d, f}, quantum numbers, (principal, azimuthal, magnetic, spin) | 37 Minutes |
13 | Electron filling rule, Aufbau principle, Hund’s rule, pauli’s exclusion principle, magnetic nature, magnetic moment | 47 Minutes |
14 | Wave quantum theory, schrodinger wave equation, radial node, angular node. | 42 Minutes |
Lecture# | Description | Duration |
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01 | Introduction Different concentration terms interconversion, colligative properties, van’t hoff factor calculation, osmotic pressure. |
33 Minutes |
02 | Osmosis , Osmotic pressure (different cases) | 47 Minutes |
03 | Numericals on osmotic pressure | 46 Minutes |
04 | Vapour pressure, relative lowering of vapour pressure, | 41 Minutes |
05 | Numericals on RLVP, Ostwald walker method | 40 Minutes |
06 | Elevation in boiling point, calculation of Kb (molal elevation boiling point constant) . Depression in freezing point, Calculation of Kf, | 54 Minutes |
07 | Numericals on elevation in boiling point and depression in freezing point | 36 Minutes |
08 | Thermodynamic explanation of 𝝙Tb & 𝝙Tf | 6 Minutes |
09 | Raoult’s law when two volatile liquids are mixed | 49 Minutes |
10 | Ideal and nonideal solution | 34 Minutes |
11 | Azeotropes, mixture of two immiscible liquids, solubility of gas in liquid, henry law | 58 Minutes |
Lecture# | Description | Duration |
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01 | Types of solid, Crystal, Amorphous, unit cell, 2D, 3D, space,lattice. | 42 Minutes |
02 | Primitive, body centred, face centered contribution of atoms in cubic unit cell. Packing fraction of square packing and hexagonal packing | 47 Minutes |
03 | Coordination Number, packing fraction, density of solid.,Simple cubic, BCC, FCC, CCP | 44 Minutes |
04 | Closed packing in 3D HCP packing, Linear void, Triangular void, Tetrahedral void, octahedral void, Cubical void Types of void in FCC |
57 Minutes |
05 | Voids in FCC,Different radius ratio for ionic compounds. | 47 Minutes |
06 | Calculation of nearest, next nearest and next to next nearest atoms in SC, BCC, FCC. | 29 Minutes |
07 | Structure of NaCl type, Zns type, CaF2 type, Na2O type, CSCl type, Diamond | 50 Minutes |
08 | Spinal structure, perovskite corundum structure, packing fraction of NaCl, Defect In crystal, Schottky, Frenkel, Interstitial | 39 Minutes |
09 | Non stoichiometric defect, cation excess defect cation deficiency defect, Paramagnetic, Diamagnetic Ferromagnetic, Ferrimagnetic, Antiferromagnetic compound | 31 Minutes |
Lecture# | Description | Duration |
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01 | Fast reaction , slow reaction, moderate reaction, average rate of reaction, instantaneous rate of reaction, relation of rate of reaction between various reagents , order | 57 Minutes |
02 | Order law, zero order reaction | 35 Minutes |
03 | First order reaction | 28 Minutes |
04 | Half life period for first order reaction | 27 Minutes |
05 | Average life period for first order, generation time , first order bacterial growth, second order reaction | 24 Minutes |
06 | nth order reaction, pseudo first order reaction | 35 Minutes |
07 | Rate of reaction of two or reactant are taken, calculation of order by half life method | 32 Minutes |
08 | Initial rate method , integrated rate law, ostwald isolation method to determine order | 40 Minutes |
09 | Monitoring of first order reaction using pressure measurement | 30 Minutes |
10 | Monitoring of first order reaction using titration and optical rotation | 42 Minutes |
11 | Arrhenius transition state theory | 29 Minutes |
12 | Arrhenius equation | 32 Minutes |
13 | Effect of catalyst on rate constant, temperature coefficient for reaction | 39 Minutes |
14 | Simple and complex reaction, molecularity, rate determining step RDS | 29 Minutes |
15 | Determination of rate if RDS is given , steady state approximation,complexity in first order reaction, parallel first order reactions | 48 Minutes |
16 | Reversible first order reaction | 29 Minutes |
17 | Consecutive first order reaction | 19 Minutes |
Lecture# | Description | Duration |
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01 | Cause of radioactivity belt of stability , comparison between alpha particle, beta particle and gamma rays | 15 Minutes |
02 | Group displacement law soddy fajan rule,, k– electron capture ,first order decay. | 28 Minutes |
03 | Radioactive decay | 28 Minutes |
04 | Carbon dating, Age of rock using U & Pb,Age of rock using U & He | 53 Minutes |
05 | Mass defect ,Binding energy, Binding energy per nucleon. Nuclear fission and fusion. | 51 Minutes |
Lecture# | Description | Duration |
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01 | Adsorption, Adsorbate, Adsorbent, Thermodynamics of Adsorption, Adsorption v/s Absorption, Physical Adsorption. | 47 Minutes |
02 | Freundlich & Langmuir isotherm, catalytic action of Homogeneous catalyst & Heterogeneous catalyst, Positive & negative catalyst, Homogeneous catalyst, Promoters, Catalytic poison, zeolites, enzyme catalyst, Types of solution, Dispersed phase & Dispersion medium. | 48 Minutes |
03 | Types of colloidal solution, Lyophobic, Lyophilic, macromolecular, micromolecular, Associated colloid/ micelle, cleansing action of soap, Bredig’s arc method,Peptization | 43 Minutes |
04 | Chemical method to prepare colloidal solution, Tyndall effect, Brownian motion, Electrophoresis, coagulation, protection of colloid. | 53 Minutes |
05 | Gold number, Helmholtz double layer theory ,emulsion. | 22 Minutes |
Lecture# | Description | Duration |
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01 | Electrochemical cell, Oxidation half cell, Reduction half cell, Galvanic cell | 1 hr 05 Minutes |
02 | Salt bridge, Daniel cell net cell reaction reaction Quotient cell representation relation between DG & E properties of DG & E,nernst equation | 44 Minutes |
03 | Spontaneity of reaction in cell, nernst equation cell at equilibrium, concentration cell. Hydrogen electrode and standard hydrogen electrode | 44 Minutes |
045 | Metal + insoluble salt + soluble anion type half cell Eg. Ag + AgCl + Cl– |
1 hr 15 Minutes |
05 | Calomel electrode, electrochemical series, thermodynamics for electrochemical cell, 𝝙G, 𝝙H, 𝝙S | 59 Minutes |
06 | Electrolysis & electrolytic cell, electrolysis of nacl, nabr, H2SO4,H2O, first law of electrolysis Faraday law | 1 hr 11 Minutes |
07 | Examples of first law of faraday, second law of faraday | 51 Minutes |
08 | Primary cell ,leclanche cell, secondary cell, lead storage battery , Ni-Cd cell , H2-O2 fuel cell, electrolytic conduction | 50 Minutes |
09 | Molar conductivity, equivalent conductivity , relation between molar cond. And equv. Cond., kohlrausch law, calculation of molar cond using wheatstone bridge , relation between molar cond. And concentration for weak electrolyte and strong electrolyte ,huckel onsager equation | 54 Minutes |
10 | Ionic mobility, conductometric titration for strong acid V/s strong base , strong acid v/s weak base and other examples | 51 Minutes |