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 📚 Chapter: Chemical Kinetics – Class 12 Chemistry Notes --- 🔸 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. --- 🔹 2. Rate of Reaction Average Rate = ΔConcentration / ΔTime 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 --- 🔹 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 --- 🔹 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 --- 🔹 5. Molecularity vs Order Molecularity Order Theoretical concept Experimental Can’t be zero Can be zero Only whole numbers Can be fractional --- 🔹 6. Integrated Rate Laws Zero Order: Rate = k [A] = [A]₀ – kt Un...

 📚 Chapter: Electrochemistry – Class 12 Chemistry Notes --- 🔸 Introduction: Electrochemistry is the study of the relationship between electricity and chemical reactions. It includes redox reactions, electrochemical cells, electrode potentials, and electrolysis. --- 🔹 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 --- 🔹 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 --- 🔹 3. EMF of Cell E°cell = E°cathode – E°anode If E°cell > 0 → reaction is spontaneous --- 🔹 4. Nernst Equation Used to calculate cell potential under non-standard conditions: E = E° - \frac{0.0591}{n} \log \frac{[Products]}{[Reactants]} W...

 📚 Chapter: Solutions – Class 12 Chemistry Notes --- 🔸 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. --- 🔹 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) --- 🔹 2. Concentration Terms Mass % = (Mass of solute / Mass of solution) × 100 Mole Fraction (χ) = 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 --- 🔹 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) --- 🔹 4. Raoult’s Law For liquid-liquid solutions: Partial vapour pressu...

 📚 Chapter: The Solid State – Class 12 Chemistry Notes --- 🔸 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 --- 🔹 1. Classification of Solids Type Properties Example Crystalline Ordered, definite melting point NaCl, Quartz Amorphous Irregular, softens over a range of temp. Glass, Plastic --- 🔹 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 --- 🔹 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 --- 🔹 4. Packing Efficiency Simple Cubic: 52.4% BCC: 68% FCC / C...

 🧪 Chapter 2: Solutions – Class 12 Chemistry Notes Label: Chemistry, Class 12, Solutions --- 🔹 Introduction A solution is a homogeneous mixture of two or more substances. The component present in larger quantity is called solvent, and the one in smaller quantity is called solute. --- 🧫 Types of Solutions (Based on Physical State) Type Solute Solvent Example Solid in liquid Sugar Water Sugar solution Gas in liquid CO₂ Water Soda water Liquid in liquid Alcohol Water Alcohol in water Solid in solid Copper Gold Alloy (Gold coin) --- 📏 Concentration of Solutions 1. Mass Percentage (w/w): = (Mass of solute / Mass of solution) × 100 2. Volume Percentage (v/v): = (Volume of solute / Volume of solution) × 100 3. Molarity (M): = (Moles of solute / Volume of solution in L) 4. Molality (m): = (Moles of solute / Mass of solvent in kg) 5. Mole Fraction (χ): = (Moles of component / Total moles of all components) --- ⚠️ Solubility Solubility is the maximum amount of solute that can be dissolve...

 📘 Introduction: Haloalkanes and Haloarenes are organic compounds containing halogen atoms attached to alkyl or aryl groups. --- 🔬 Classification: 🧪 Based on Number of Halogen Atoms: Mono, Di, Tri, Poly halogen compounds 🧪 Based on Type of Carbon Chain: Alkyl halides (R–X) Aryl halides (Ar–X) --- 🧪 Nomenclature: IUPAC name: Prefix (halo) + parent hydrocarbon Example: CH₃Cl → Chloromethane C₂H₅Br → Bromoethane --- ⚗️ Preparation of Haloalkanes: 1. From Alcohols: ROH + HX → R–X + H₂O (Using ZnCl₂ as catalyst) 2. From Alkanes (by halogenation): RH + X₂ → R–X + HX (in sunlight) 3. From Alkenes (Addition Reaction): CH₂=CH₂ + HX → CH₃–CH₂X --- 🧪 Physical Properties: Colorless liquids or solids Denser than water Insoluble in water but soluble in organic solvents Boiling point increases with molar mass --- ⚙️ Chemical Reactions: 1. Nucleophilic Substitution (SN1 & SN2): SN1: 2° & 3° haloalkanes (carbocation intermediate) SN2: 1° haloalkanes (one-step reaction) 2. Elimination ...