{"id":4033,"date":"2026-03-30T12:36:13","date_gmt":"2026-03-30T12:36:13","guid":{"rendered":"https:\/\/ksquareinstitute.in\/blog\/?p=4033"},"modified":"2026-04-03T12:41:34","modified_gmt":"2026-04-03T12:41:34","slug":"chemical-kinetics-class-12-notes-pdf","status":"publish","type":"post","link":"https:\/\/ksquareinstitute.in\/blog\/chemical-kinetics-class-12-notes-pdf\/","title":{"rendered":"Chemical Kinetics Class 12 Notes PDF: Complete NEET Revision &amp; Formula Sheet"},"content":{"rendered":"\n<!DOCTYPE html>\n<html lang=\"en\">\n<head>\n    <meta charset=\"UTF-8\">\n    <meta name=\"viewport\" content=\"width=device-width, initial-scale=1.0\">\n    <link rel=\"preconnect\" href=\"https:\/\/fonts.googleapis.com\">\n    <link rel=\"preconnect\" href=\"https:\/\/fonts.gstatic.com\" crossorigin>\n    <link href=\"https:\/\/fonts.googleapis.com\/css2?family=DM+Sans:ital,opsz,wght@0,9..40,300..600;1,9..40,300..600&#038;family=JetBrains+Mono:wght@400;500;700&#038;family=Plus+Jakarta+Sans:wght@400;600;700;800&#038;display=swap\" rel=\"stylesheet\">\n    <style>\n        :root {\n            --accent: #e8600a;\n            --accent-light: #fff3ec;\n            --accent-mid: #fde3cc;\n            --dark: #111827;\n            --text: #1a1a1a;\n            --text-muted: #4b5563;\n            --border: #e5e7eb;\n            --green-bg: #f0fdf4;\n            --green-border: #16a34a;\n            --blue-bg: #eff6ff;\n            --blue-border: #3b82f6;\n        }\n\n        * { box-sizing: border-box; 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}\n        .btn { padding: 14px 32px; border-radius: 8px; font-weight: 700; text-decoration: none; transition: 0.3s; }\n        .btn-white { background: white; color: var(--accent); }\n        .btn-outline { border: 2px solid white; color: white; }\n\n        .internal-links { background: #f9fafb; border: 1px solid var(--border); border-radius: 10px; padding: 24px; margin: 40px 0; }\n        .internal-links-title { color: var(--text-muted); font-weight: 700; font-size: 0.9rem; margin-bottom: 16px; display: block; }\n        .internal-links a { display: block; color: var(--accent); text-decoration: none; font-weight: 600; margin-bottom: 8px; }\n\n        .download-btn { background: var(--dark); color: white; display: inline-flex; align-items: center; gap: 10px; padding: 12px 24px; border-radius: 8px; text-decoration: none; font-weight: 600; margin-top: 20px; }\n    <\/style>\n<\/head>\n<body>\n\n<div class=\"content-wrapper\">\n    <div class=\"container\">\n\n        <p>Mastering reaction speeds and mechanisms is fundamental to physical chemistry. This <strong>chemical kinetics class 12 notes pdf<\/strong> guide provides a deep dive into how chemical reactions occur and the factors that control their speed. For NEET aspirants, this chapter is high-yield, offering scoring opportunities through both conceptual questions on order and molecularity and numerical problems on half-life and the Arrhenius equation.<\/p>\n\n        <h2><div class=\"badge\">01<\/div>Introduction to Chemical Kinetics<\/h2>\n        <p>Chemical kinetics is the branch of chemistry that deals with the study of reaction rates and the mechanisms by which they occur. While thermodynamics tells us if a reaction is feasible (\u0394G < 0), kinetics tells us how fast that reaction will actually proceed. Understanding this distinction is vital for any comprehensive <strong>chemical kinetics class 12 notes pdf<\/strong> study resource.<\/p>\n        \n        <div class=\"card-grid\">\n            <div class=\"card\">\n                <span class=\"card-title\">SCOPE<\/span>\n                Measurement of reaction rates under varying conditions such as concentration, temperature, and pressure.\n            <\/div>\n            <div class=\"card\">\n                <span class=\"card-title\">MECHANISM<\/span>\n                The stepwise path (elementary steps) that leads from reactants to the final products.\n            <\/div>\n        <\/div>\n\n        <h2><div class=\"badge\">02<\/div>Rate of Reaction<\/h2>\n        <p>The rate of a chemical reaction is defined as the change in the concentration of any one of the reactants or products per unit time. It can be expressed as the rate of disappearance of reactants or the rate of appearance of products.<\/p>\n\n        <div class=\"formula-dark\">\n            <span class=\"formula-dark-label\">AVERAGE RATE FORMULA<\/span>\n            <div class=\"formula-dark-content\">Rate = \u2212\u0394[R] \/ \u0394t = +\u0394[P] \/ \u0394t<\/div>\n        <\/div>\n\n        <div class=\"table-container\">\n            <table>\n                <thead>\n                    <tr>\n                        <th>Type of Rate<\/th>\n                        <th>Definition<\/th>\n                        <th>Expression<\/th>\n                    <\/tr>\n                <\/thead>\n                <tbody>\n                    <tr>\n                        <td>Average Rate<\/td>\n                        <td>Rate over a measurable time interval.<\/td>\n                        <td>\u0394[C] \/ \u0394t<\/td>\n                    <\/tr>\n                    <tr>\n                        <td>Instantaneous Rate<\/td>\n                        <td>Rate at a specific instant of time.<\/td>\n                        <td>d[C] \/ dt<\/td>\n                    <\/tr>\n                    <tr>\n                        <td>Unit<\/td>\n                        <td>Standard SI unit of reaction rate.<\/td>\n                        <td>mol L<sup>\u22121<\/sup> s<sup>\u22121<\/sup><\/td>\n                    <\/tr>\n                <\/tbody>\n            <\/table>\n        <\/div>\n\n        <!-- Promotional Banner 1 -->\n        <a href=\"https:\/\/courses.ksquare.co.in\/new-courses\/3-mission-180-neet-physics-rankers-batch\" target=\"_blank\" rel=\"nofollow noopener noreferrer\" style=\"display:block; margin-bottom:40px;\">\n            <img decoding=\"async\" src=\"https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/03\/Course-Poromo-Banner-scaled.png\" alt=\"Mission 180 NEET Physics Rankers Batch - KSquare Career Institute\" style=\"width:100%; height:auto; border-radius:10px; display:block;\">\n        <\/a>\n\n        <h2><div class=\"badge\">03<\/div>Factors Affecting Rate of Reaction<\/h2>\n        <p>Several variables influence the speed of a reaction. In your <strong>chemical kinetics class 12 notes pdf<\/strong>, make sure to categorize these as intensive and extensive factors.<\/p>\n\n        <div class=\"card-grid\">\n            <div class=\"card\">\n                <span class=\"card-title\">CONCENTRATION<\/span>\n                Rate generally increases with concentration as the number of effective collisions per unit volume increases.\n            <\/div>\n            <div class=\"card\">\n                <span class=\"card-title\">TEMPERATURE<\/span>\n                For most reactions, a 10\u00b0C rise in temperature nearly doubles the rate constant.\n            <\/div>\n            <div class=\"card\">\n                <span class=\"card-title\">CATALYST<\/span>\n                Provides an alternative pathway with lower activation energy (E<sub>a<\/sub>), thus increasing the rate.\n            <\/div>\n            <div class=\"card\">\n                <span class=\"card-title\">SURFACE AREA<\/span>\n                In heterogeneous reactions, increasing surface area (by grinding solids) increases the rate.\n            <\/div>\n        <\/div>\n\n        <h2><div class=\"badge\">04<\/div>Rate Law and Order of Reaction<\/h2>\n        <p>The rate law is the mathematical expression that relates the rate of reaction to the molar concentration of reactants. Unlike stoichiometric coefficients, the exponents in a rate law must be determined experimentally.<\/p>\n\n        <div class=\"formula-orange\">\n            <div class=\"formula-orange-content\">Rate = k [A]<sup>m<\/sup> [B]<sup>n<\/sup> | Overall Order = m + n<\/div>\n        <\/div>\n\n        <div class=\"callout warning\">\n            <div class=\"callout-pill\">WARN<\/div>\n            Order can be zero, fractional, or even negative. Molecularity, however, is always a whole number and can never be zero or fractional.\n        <\/div>\n\n        <h3>Order vs Molecularity<\/h3>\n        <div class=\"table-container\">\n            <table>\n                <thead>\n                    <tr>\n                        <th>Property<\/th>\n                        <th>Order of Reaction<\/th>\n                        <th>Molecularity<\/th>\n                    <\/tr>\n                <\/thead>\n                <tbody>\n                    <tr>\n                        <td>Basis<\/td>\n                        <td>Experimental value.<\/td>\n                        <td>Theoretical value.<\/td>\n                    <\/tr>\n                    <tr>\n                        <td>Applicability<\/td>\n                        <td>Elementary and complex reactions.<\/td>\n                        <td>Only elementary reactions.<\/td>\n                    <\/tr>\n                    <tr>\n                        <td>Values<\/td>\n                        <td>Can be zero or fractional.<\/td>\n                        <td>Whole numbers only (1, 2, 3).<\/td>\n                    <\/tr>\n                <\/tbody>\n            <\/table>\n        <\/div>\n\n        <h2><div class=\"badge\">05<\/div>Integrated Rate Equations<\/h2>\n        <p>Integrating the differential rate laws allows us to calculate the concentration of reactants at any time. This is a core focus of the <strong>chemical kinetics class 12 notes pdf<\/strong> guide.<\/p>\n\n        <h3>1. Zero Order Reaction<\/h3>\n        <div class=\"formula-dark\">\n            <span class=\"formula-dark-label\">ZERO ORDER FORMULA<\/span>\n            <div class=\"formula-dark-content\">[A] = [A]<sub>0<\/sub> \u2212 kt<\/div>\n        <\/div>\n\n        <h3>2. First Order Reaction<\/h3>\n        <div class=\"formula-orange\">\n            <div class=\"formula-orange-content\">k = (2.303 \/ t) log([A]<sub>0<\/sub> \/ [A])<\/div>\n        <\/div>\n\n        <div class=\"callout tip\">\n            <div class=\"callout-pill\">TIP<\/div>\n            The plot of log[A] vs time for a first-order reaction is a straight line with a slope equal to \u2212k \/ 2.303.\n        <\/div>\n\n        <h2><div class=\"badge\">06<\/div>Half-Life of Reactions (t<sub>1\/2<\/sub>)<\/h2>\n        <p>Half-life is the time required for the concentration of a reactant to decrease to half of its initial value. This is one of the most frequently tested numerical topics in the <strong>chemical kinetics class 12 notes pdf<\/strong>.<\/p>\n        \n        <ul>\n            <li><strong>Zero Order:<\/strong> t<sub>1\/2<\/sub> = [A]<sub>0<\/sub> \/ 2k (Depends on initial concentration).<\/li>\n            <li><strong>First Order:<\/strong> t<sub>1\/2<\/sub> = 0.693 \/ k (Independent of initial concentration).<\/li>\n        <\/ul>\n\n        <!-- Promotional Banner 2 -->\n        <a href=\"https:\/\/ksquareinstitute.in\/neet-2026-rank-predictor\/\" target=\"_blank\" rel=\"nofollow noopener noreferrer\" style=\"display:block; margin-bottom:40px;\">\n            <img decoding=\"async\" src=\"https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/03\/neet-2026-college-and-rank-predictor-scaled.png\" alt=\"NEET 2026 Rank Predictor - KSquare Career Institute\" style=\"width:100%; height:auto; border-radius:10px; display:block;\">\n        <\/a>\n\n        <h2><div class=\"badge\">07<\/div>Temperature Dependence: Arrhenius Equation<\/h2>\n        <p>The rate constant (k) is highly sensitive to temperature changes. This relationship is quantified by the Arrhenius Equation. Mastery of this formula is essential for solving advanced <strong>chemical kinetics class 12 notes pdf<\/strong> problems.<\/p>\n\n        <div class=\"formula-dark\">\n            <span class=\"formula-dark-label\">ARRHENIUS FORMULA<\/span>\n            <div class=\"formula-dark-content\">k = A e<sup>\u2212E<sub>a<\/sub>\/RT<\/sup><\/div>\n        <\/div>\n\n        <p>Logarithmic form for calculations at two different temperatures:<\/p>\n        <div class=\"formula-orange\">\n            <div class=\"formula-orange-content\">log(k<sub>2<\/sub> \/ k<sub>1<\/sub>) = (E<sub>a<\/sub> \/ 2.303R) [(T<sub>2<\/sub> \u2212 T<sub>1<\/sub>) \/ (T<sub>1<\/sub>T<sub>2<\/sub>)]<\/div>\n        <\/div>\n\n        <h2><div class=\"badge\">08<\/div>Collision Theory and Catalysis<\/h2>\n        <p>According to Collision Theory, a chemical reaction occurs only when reactant molecules undergo &#8220;effective collisions.&#8221; This requires two conditions: <strong>Activation Energy Threshold<\/strong> and <strong>Proper Orientation<\/strong>.<\/p>\n\n        <div class=\"card-grid\">\n            <div class=\"card\">\n                <span class=\"card-title\">HOMOGENEOUS CATALYSIS<\/span>\n                Reactants and catalyst are in the same phase (e.g., Lead chamber process).\n            <\/div>\n            <div class=\"card\">\n                <span class=\"card-title\">HETEROGENEOUS CATALYSIS<\/span>\n                Reactants and catalyst are in different phases (e.g., Haber&#8217;s process).\n            <\/div>\n        <\/div>\n\n        <div class=\"internal-links\">\n            <span class=\"internal-links-title\">ENHANCE YOUR NEET PREPARATION<\/span>\n            <a href=\"https:\/\/ksquareinstitute.in\/blog\/neet-physics-survival-kit-2026\/\">NEET Physics Survival Kit 2026<\/a>\n            <a href=\"https:\/\/ksquareinstitute.in\/blog\/organic-chemistry-strategy-neet\/\">Organic Chemistry Strategy for NEET<\/a>\n            <a href=\"https:\/\/ksquareinstitute.in\/blog\/neet-biology-tricks-for-exams\/\">NEET Biology Tricks for Exams<\/a>\n            <a href=\"https:\/\/ksquareinstitute.in\/blog\/score-340-in-neet-biology\/\">How to Score 340 in NEET Biology<\/a>\n            <a href=\"https:\/\/ksquareinstitute.in\/free-study-material\/\" target=\"_blank\" rel=\"nofollow noopener noreferrer\">Free NEET Study Material<\/a>\n        <\/div>\n\n        <div class=\"revision-box\">\n            <h3>Quick Revision Summary<\/h3>\n            <ul>\n                <li>Reaction Rate = \u00b1 (1\/n) d[C]\/dt. Unit: mol L<sup>\u22121<\/sup> s<sup>\u22121<\/sup>.<\/li>\n                <li>Rate Law is determined experimentally, not stoichiometrically.<\/li>\n                <li>Order can be zero, fraction, or whole number.<\/li>\n                <li>First order t<sub>1\/2<\/sub> = 0.693\/k. Note it is concentration-independent.<\/li>\n                <li>Arrhenius Equation: k = A exp(\u2212E<sub>a<\/sub>\/RT).<\/li>\n                <li>Catalysts lower E<sub>a<\/sub> without affecting \u0394G or equilibrium constant.<\/li>\n                <li>Threshold Energy = Activation Energy + Average Kinetic Energy.<\/li>\n                <li>Radioactive decay follows First Order kinetics.<\/li>\n                <li>Integrated Rate Equation for nth order (n\u22601): k = [1\/t(n\u22121)] [1\/A<sup>n\u22121<\/sup> \u2212 1\/A<sub>0<\/sub><sup>n\u22121<\/sup>].<\/li>\n                <li>Collision frequency (Z) increases with temperature.<\/li>\n            <\/ul>\n            <a href=\"#\" class=\"download-btn\" rel=\"nofollow noopener noreferrer\">\n                <span>Download Chemical Kinetics Formula Sheet<\/span>\n            <\/a>\n        <\/div>\n\n        <h2><div class=\"badge\">09<\/div>Frequently Asked Questions<\/h2>\n        <div class=\"faq-container\">\n            <details>\n                <summary>\n                    <span>What is the physical significance of Activation Energy?<\/span>\n                    <div class=\"toggle-icon\">\n                        <svg viewBox=\"0 0 24 24\"><path class=\"plus-path\" d=\"M12 5v14M5 12h14\"\/><path class=\"minus-path\" d=\"M5 12h14\"\/><\/svg>\n                    <\/div>\n                <\/summary>\n                <div class=\"faq-answer\">Activation energy (E<sub>a<\/sub>) is the minimum extra energy that reactant molecules must absorb to reach the &#8220;activated complex&#8221; state and form products. A higher E<sub>a<\/sub> means a slower reaction at a given temperature.<\/div>\n            <\/details>\n            <details>\n                <summary>\n                    <span>Why are third-order reactions rare?<\/span>\n                    <div class=\"toggle-icon\">\n                        <svg viewBox=\"0 0 24 24\"><path class=\"plus-path\" d=\"M12 5v14M5 12h14\"\/><path class=\"minus-path\" d=\"M5 12h14\"\/><\/svg>\n                    <\/div>\n                <\/summary>\n                <div class=\"faq-answer\">For a reaction to occur, multiple molecules must collide simultaneously with sufficient energy and proper orientation. The probability of three molecules colliding at the exact same point and time is extremely low, making high-order reactions very rare.<\/div>\n            <\/details>\n            <details>\n                <summary>\n                    <span>Does temperature affect activation energy?<\/span>\n                    <div class=\"toggle-icon\">\n                        <svg viewBox=\"0 0 24 24\"><path class=\"plus-path\" d=\"M12 5v14M5 12h14\"\/><path class=\"minus-path\" d=\"M5 12h14\"\/><\/svg>\n                    <\/div>\n                <\/summary>\n                <div class=\"faq-answer\">Generally, no. E<sub>a<\/sub> is a characteristic of the reaction pathway. Temperature increases the kinetic energy of molecules, meaning more molecules possess energy greater than E<sub>a<\/sub>, but it doesn&#8217;t change the E<sub>a<\/sub> value itself unless a catalyst is used.<\/div>\n            <\/details>\n            <details>\n                <summary>\n                    <span>What is a pseudo-first-order reaction?<\/span>\n                    <div class=\"toggle-icon\">\n                        <svg viewBox=\"0 0 24 24\"><path class=\"plus-path\" d=\"M12 5v14M5 12h14\"\/><path class=\"minus-path\" d=\"M5 12h14\"\/><\/svg>\n                    <\/div>\n                <\/summary>\n                <div class=\"faq-answer\">It is a reaction that is actually higher-order (e.g., second-order) but behaves like a first-order reaction because one of the reactants is present in large excess, making its concentration virtually constant. Example: Hydrolysis of ester.<\/div>\n            <\/details>\n            <details>\n                <summary>\n                    <span>How does a catalyst increase reaction rate?<\/span>\n                    <div class=\"toggle-icon\">\n                        <svg viewBox=\"0 0 24 24\"><path class=\"plus-path\" d=\"M12 5v14M5 12h14\"\/><path class=\"minus-path\" d=\"M5 12h14\"\/><\/svg>\n                    <\/div>\n                <\/summary>\n                <div class=\"faq-answer\">A catalyst provides an alternative reaction mechanism or &#8220;shortcut&#8221; with a lower activation energy barrier. This allows a much larger fraction of molecules to have enough energy to cross the barrier and form products.<\/div>\n            <\/details>\n        <\/div>\n\n        <div class=\"cta-section\">\n            <h2>Fast-Track Your NEET preparation with KSquare<\/h2>\n            <p>Ready to accelerate your scores? Join KSquare Institute&#8217;s Mission 180 Rankers Batch and master Physical Chemistry with personalized guidance, error-analysis tools, and top-tier resources.<\/p>\n            <div class=\"cta-buttons\">\n                <a href=\"https:\/\/courses.ksquare.co.in\/new-courses\/3-mission-180-neet-physics-rankers-batch\" class=\"btn btn-white\" target=\"_blank\" rel=\"nofollow noopener noreferrer\">Join Rankers Batch<\/a>\n                <a href=\"https:\/\/ksquareinstitute.in\/free-study-material\/\" class=\"btn btn-outline\" target=\"_blank\" rel=\"nofollow noopener noreferrer\">Get Free Study Material<\/a>\n            <\/div>\n        <\/div>\n    <\/div>\n<\/div>\n\n<\/body>\n<\/html>\n\n\n\n<!DOCTYPE html>\n<html lang=\"en\">\n<head>\n  <meta charset=\"UTF-8\">\n  <meta name=\"viewport\" content=\"width=device-width, initial-scale=1.0\">\n  <title>Table of Contents \u2014 Chemistry Class 12<\/title>\n  \n  <!-- Google Fonts Import -->\n  <link rel=\"preconnect\" href=\"https:\/\/fonts.googleapis.com\">\n  <link rel=\"preconnect\" href=\"https:\/\/fonts.gstatic.com\" crossorigin>\n  <link href=\"https:\/\/fonts.googleapis.com\/css2?family=DM+Sans:ital,opsz,wght@0,9..40,100..1000;1,9..40,100..1000&#038;family=Plus+Jakarta+Sans:ital,wght@0,200..800;1,200..800&#038;display=swap\" rel=\"stylesheet\">\n  \n  <style>\n    \/* Scoped wrapper using a unique ID (#chemistry-toc-wrapper).\n       This ensures these styles do not leak and affect other parts of your website.\n    *\/\n    #chemistry-toc-wrapper {\n      font-family: 'DM Sans', sans-serif;\n      width: 100%;\n      margin: 0;\n      padding: 60px 0;\n      color: #111;\n      background: #fff;\n      -webkit-font-smoothing: antialiased;\n    }\n\n    #chemistry-toc-wrapper .container-inner {\n      width: 100%;\n      margin: 0 auto;\n      padding: 0; \/* Edge-to-edge layout *\/\n    }\n\n    #chemistry-toc-wrapper h1 {\n      font-family: 'Plus Jakarta Sans', sans-serif;\n      font-size: 0.85rem;\n      font-weight: 700;\n      color: #71717a;\n      margin: 0 0 8px;\n      letter-spacing: 0.1em;\n      text-transform: uppercase;\n      padding-left: 16px; \n    }\n\n    #chemistry-toc-wrapper h2 {\n      font-family: 'Plus Jakarta Sans', sans-serif;\n      font-size: 2.25rem;\n      font-weight: 800;\n      margin: 0 0 48px;\n      letter-spacing: -0.02em;\n      color: #09090b;\n      padding-left: 16px;\n    }\n\n    #chemistry-toc-wrapper table {\n      width: 100%;\n      border-collapse: collapse;\n      border-spacing: 0;\n      border-top: 1px solid #e4e4e7;\n      border-bottom: 1px solid #e4e4e7;\n    }\n\n    #chemistry-toc-wrapper tr {\n      border-bottom: 1px solid #e4e4e7;\n      transition: all 0.2s ease;\n    }\n\n    #chemistry-toc-wrapper tr:hover {\n      background-color: #f8fafc;\n    }\n\n    #chemistry-toc-wrapper tr:last-child {\n      border-bottom: none;\n    }\n\n    #chemistry-toc-wrapper td {\n      padding: 24px 16px;\n      vertical-align: middle;\n      font-size: 1.05rem;\n      font-weight: 500;\n      border-right: 1px solid #e4e4e7; \/* Column borders as per reference image *\/\n    }\n\n    #chemistry-toc-wrapper td:last-child {\n      border-right: none;\n    }\n\n    \/* Column 1: Index Numbers *\/\n    #chemistry-toc-wrapper td:first-child {\n      color: #a1a1aa;\n      font-size: 0.9rem;\n      width: 70px;\n      font-weight: 400;\n      font-variant-numeric: tabular-nums;\n      text-align: center;\n      padding-left: 10px;\n    }\n\n    \/* Column 2: Chapter Titles *\/\n    #chemistry-toc-wrapper td:nth-child(2) {\n      padding-left: 32px; \/* Breathing room before chapter text *\/\n      color: #18181b;\n    }\n\n    \/* Column 3: Action Button *\/\n    #chemistry-toc-wrapper td:last-child {\n      text-align: right;\n      width: 180px;\n      padding-right: 24px; \/* Space after the button *\/\n    }\n\n    \/* Premium Button Styling *\/\n    #chemistry-toc-wrapper a.go {\n      display: inline-block;\n      font-family: 'Plus Jakarta Sans', sans-serif;\n      font-size: 0.75rem;\n      font-weight: 800;\n      padding: 12px 24px;\n      border: 1.5px solid #18181b;\n      border-radius: 8px;\n      color: #18181b;\n      text-decoration: none;\n      letter-spacing: 0.05em;\n      text-transform: uppercase;\n      transition: all 0.2s cubic-bezier(0.4, 0, 0.2, 1);\n      white-space: nowrap;\n    }\n\n    #chemistry-toc-wrapper a.go:hover {\n      background: #18181b;\n      color: #ffffff;\n      transform: translateY(-2px);\n      box-shadow: 0 4px 12px rgba(24, 24, 27, 0.15);\n    }\n\n    \/* Responsive Logic *\/\n    @media (max-width: 768px) {\n      #chemistry-toc-wrapper h2 {\n        font-size: 1.75rem;\n        margin-bottom: 32px;\n        padding-left: 12px;\n      }\n      #chemistry-toc-wrapper td {\n        padding: 18px 12px;\n        font-size: 0.95rem;\n      }\n      #chemistry-toc-wrapper td:nth-child(2) {\n        padding-left: 16px;\n      }\n    }\n  <\/style>\n<\/head>\n<body>\n\n<div id=\"chemistry-toc-wrapper\">\n  <div class=\"container-inner\">\n    <h1>Table of Contents<\/h1>\n    <h2>Chemistry &mdash; Class 12<\/h2>\n    \n    <table>\n      <tr><td>01<\/td><td>Solutions<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/solutions-chemistry-class-12-notes-pdf\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>02<\/td><td>Electrochemistry<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/electrochemistry-class-12-notes-pdf\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>03<\/td><td>Chemical Kinetics<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/chemical-kinetics-class-12-notes-pdf\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>04<\/td><td>d- and f-Block Elements<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/d-and-f-block-elements-class-12-pdf\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>05<\/td><td>Coordination Compounds<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/coordination-compounds-class-12-pdf\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>06<\/td><td>Haloalkanes and Haloarenes<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/haloalkanes-and-haloarenes-class-12-pdf\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>07<\/td><td>Alcohols, Phenols and Ethers<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/alcohols-phenols-ethers-class-12-pdf\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>08<\/td><td>Aldehydes, Ketones and Carboxylic Acids<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/aldehydes-ketones-carboxylic-acids-class-12\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>09<\/td><td>Amines<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/amines-class-12-notes-pdf\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>10<\/td><td>Biomolecules<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/biomolecules-class-12-chemistry\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n    <\/table>\n  <\/div>\n<\/div>\n\n<\/body>\n<\/html>\n","protected":false},"excerpt":{"rendered":"<p>Mastering reaction speeds and mechanisms is fundamental to physical chemistry. This chemical kinetics class 12 notes pdf guide provides a deep dive into how chemical reactions occur and the factors that control their speed. For NEET aspirants, this chapter is high-yield, offering scoring opportunities through both conceptual questions on order and molecularity and numerical problems [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[127],"tags":[350,348,352,351,349],"class_list":["post-4033","post","type-post","status-publish","format-standard","hentry","category-free-study-material","tag-chemical-kinetics-class-12","tag-class-12-chemistry-pdf","tag-half-life-reactions","tag-integrated-rate-equations","tag-rate-law-notes"],"blocksy_meta":{"page_structure_type":"type-1","styles_descriptor":{"styles":{"desktop":"","tablet":"","mobile":""},"google_fonts":[],"version":6}},"_links":{"self":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/4033","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/comments?post=4033"}],"version-history":[{"count":2,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/4033\/revisions"}],"predecessor-version":[{"id":4245,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/4033\/revisions\/4245"}],"wp:attachment":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/media?parent=4033"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/categories?post=4033"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/tags?post=4033"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}