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Chemical Kinetics – Class 12 Chemistry Notes | CBSE NCERT Based

 πŸ“š Chapter: Chemical Kinetics – Class 12 Chemistry Notes --- πŸ”Έ 1. Introduction to Chemical Kinetics Deals with the rate of chemical reactions and factors affecting them. Tells us how fast a reaction occurs, and what mechanism it follows. --- πŸ”Ή 2. Rate of Reaction Average Rate = Ξ”Concentration / Ξ”Time Instantaneous Rate = Rate at a particular moment Units: mol L⁻¹ s⁻¹ For a reaction: A → B Rate = –d[A]/dt = +d[B]/dt --- πŸ”Ή 3. Factors Affecting Rate Concentration – ↑ Conc = ↑ Rate Temperature – ↑ Temp = ↑ Rate (Arrhenius Eq.) Catalyst – Alters rate without being consumed Surface Area – ↑ Area = ↑ Rate Nature of Reactants --- πŸ”Ή 4. Rate Law and Order of Reaction For reaction: aA + bB → Products Rate law: Rate = k[A]^x[B]^y x, y = Order w.r.t A, B Overall order = x + y --- πŸ”Ή 5. Molecularity vs Order Molecularity Order Theoretical concept Experimental Can’t be zero Can be zero Only whole numbers Can be fractional --- πŸ”Ή 6. Integrated Rate Laws Zero Order: Rate = k [A] = [A]₀ – kt Un...
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Electrochemistry – Class 12 Chemistry Notes | CBSE NCERT Based

 πŸ“š Chapter: Electrochemistry – Class 12 Chemistry Notes --- πŸ”Έ Introduction: Electrochemistry is the study of the relationship between electricity and chemical reactions. It includes redox reactions, electrochemical cells, electrode potentials, and electrolysis. --- πŸ”Ή 1. Electrochemical Cell Converts chemical energy → electrical energy Also called Galvanic Cell or Voltaic Cell Example: Daniel Cell (Zn | Zn²⁺ || Cu²⁺ | Cu) Cell Notation: Anode (oxidation) || Cathode (reduction) e.g., Zn | Zn²⁺ || Cu²⁺ | Cu --- πŸ”Ή 2. Electrode Potential Reduction Potential (E°red): Tendency to gain electrons Oxidation Potential (E°ox): Tendency to lose electrons Standard electrode potential measured under: 1 M concentration 1 atm pressure 25°C temperature --- πŸ”Ή 3. EMF of Cell E°cell = E°cathode – E°anode If E°cell > 0 → reaction is spontaneous --- πŸ”Ή 4. Nernst Equation Used to calculate cell potential under non-standard conditions: E = E° - \frac{0.0591}{n} \log \frac{[Products]}{[Reactants]} W...
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Solutions – Class 12 Chemistry Notes | CBSE NCERT Based

 πŸ“š Chapter: Solutions – Class 12 Chemistry Notes --- πŸ”Έ Introduction: A solution is a homogeneous mixture of two or more substances. This chapter discusses different types of solutions, concentration terms, Raoult's law, and colligative properties. --- πŸ”Ή 1. Types of Solutions Solute Solvent Example Solid Liquid Sugar in water Liquid Liquid Alcohol in water Gas Liquid Oxygen in water Binary solution: Two components (solute + solvent) --- πŸ”Ή 2. Concentration Terms Mass % = (Mass of solute / Mass of solution) × 100 Mole Fraction (Ο‡) = moles of one component / total moles Molarity (M) = moles of solute / volume of solution in L Molality (m) = moles of solute / mass of solvent in kg --- πŸ”Ή 3. Solubility Solubility of solid in liquid increases with temperature Solubility of gas in liquid decreases with temperature but increases with pressure Henry’s Law: p = KH × x (p = partial pressure, x = mole fraction of gas) --- πŸ”Ή 4. Raoult’s Law For liquid-liquid solutions: Partial vapour pressu...
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The Solid State – Class 12 Chemistry Notes | CBSE NCERT Based

 πŸ“š Chapter: The Solid State – Class 12 Chemistry Notes --- πŸ”Έ Introduction to Solid State Solids have definite shape, volume, and are incompressible. Intermolecular forces are strongest in solids. Two main types: 1. Crystalline Solids 2. Amorphous Solids --- πŸ”Ή 1. Classification of Solids Type Properties Example Crystalline Ordered, definite melting point NaCl, Quartz Amorphous Irregular, softens over a range of temp. Glass, Plastic --- πŸ”Ή 2. Crystal Lattices and Unit Cell Crystal lattice: 3D arrangement of points representing atoms. Unit cell: Smallest repeating unit in crystal lattice. Types of Unit Cells: Primitive: Atoms only at corners Body-centered (BCC): One atom at center Face-centered (FCC): One atom at each face --- πŸ”Ή 3. Number of Atoms in Unit Cell Type of Unit Cell Formula to Calculate Atoms Total Atoms Simple Cubic 8 corners × 1/8 1 BCC 8 corners × 1/8 + 1 center 2 FCC 8 corners × 1/8 + 6 faces × 1/2 4 --- πŸ”Ή 4. Packing Efficiency Simple Cubic: 52.4% BCC: 68% FCC / C...
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