{"id":3963,"date":"2026-03-28T07:54:07","date_gmt":"2026-03-28T07:54:07","guid":{"rendered":"https:\/\/ksquareinstitute.in\/blog\/?p=3963"},"modified":"2026-04-03T12:18:48","modified_gmt":"2026-04-03T12:18:48","slug":"kinetic-theory-11-notes","status":"publish","type":"post","link":"https:\/\/ksquareinstitute.in\/blog\/kinetic-theory-11-notes\/","title":{"rendered":"Kinetic Theory 11 Notes: Comprehensive Guide for NEET Physics"},"content":{"rendered":"\n<style>\n@import url('https:\/\/fonts.googleapis.com\/css2?family=Plus+Jakarta+Sans:wght@400;600;700;800&family=DM+Sans:wght@300;400;500;600&family=JetBrains+Mono:wght@400;500;700&display=swap');\n\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\nbody {\nmargin: 0;\npadding: 0;\nfont-family: 'DM Sans', sans-serif;\ncolor: var(--text);\nline-height: 1.6;\nbackground-color: #fff;\n}\n\n.content-wrapper {\npadding: 0 0px;\n}\n\n@media (max-width: 640px) {\n.content-wrapper {\npadding: 0 10px;\n}\n}\n\nh1 {\nfont-family: 'Plus Jakarta Sans', sans-serif;\nfont-weight: 800;\nfont-size: 2.5rem;\ncolor: var(--dark);\nmargin-bottom: 30px;\n}\n\nh2 {\nfont-family: 'Plus Jakarta Sans', sans-serif;\nfont-weight: 700;\nfont-size: 1.8rem;\ndisplay: flex;\nalign-items: center;\ngap: 15px;\nmargin-top: 40px;\nmargin-bottom: 20px;\n}\n\nh3 {\nfont-family: 'Plus Jakarta Sans', sans-serif;\nfont-weight: 600;\nfont-size: 1.4rem;\n}\n\n.badge {\nwidth: 42px;\nheight: 42px;\nbackground-color: var(--accent);\ncolor: white;\ndisplay: flex;\nalign-items: center;\njustify-content: center;\nborder-radius: 4px;\nfont-weight: 700;\nfont-size: 1.1rem;\nflex-shrink: 0;\n}\n\n\/* Formula Boxes *\/\n.formula-dark {\nbackground: var(--dark);\nborder-left: 4px solid var(--accent);\npadding: 20px;\nmargin: 20px 0;\n}\n.formula-label {\ncolor: #9ca3af;\nfont-size: 0.75rem;\ntext-transform: uppercase;\nfont-weight: 700;\nmargin-bottom: 8px;\ndisplay: block;\n}\n.formula-dark code {\ncolor: var(--accent);\nfont-family: 'JetBrains Mono', monospace;\nfont-size: 1.1rem;\n}\n\n.formula-orange {\nbackground: var(--accent-light);\nborder: 1px solid var(--accent-mid);\nborder-left: 4px solid var(--accent);\npadding: 20px;\nmargin: 20px 0;\n}\n.formula-orange code {\ncolor: #9a3412;\nfont-family: 'JetBrains Mono', monospace;\nfont-size: 1.1rem;\n}\n\n\/* Callouts *\/\n.callout {\npadding: 16px 20px;\nborder-radius: 8px;\nmargin: 20px 0;\nborder: 1px solid;\nposition: relative;\n}\n.callout-warn {\nbackground: #fff7ed;\nborder-color: #fed7aa;\n}\n.callout-tip {\nbackground: var(--blue-bg);\nborder-color: #bfdbfe;\n}\n.pill {\nfont-size: 0.7rem;\nfont-weight: 800;\npadding: 2px 8px;\nborder-radius: 99px;\nmargin-bottom: 8px;\ndisplay: inline-block;\n}\n.pill-warn { background: var(--accent); 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}\nsummary::after {\ncontent: '+';\nwidth: 24px;\nheight: 24px;\nbackground: var(--accent);\ncolor: white;\nborder-radius: 50%;\ndisplay: flex;\nalign-items: center;\njustify-content: center;\n}\ndetails[open] summary { background: var(--accent-light); color: var(--accent); }\ndetails[open] summary::after { content: '\u2212'; }\n.faq-content { padding: 16px 20px; background: white; color: var(--text-muted); }\n\n\/* Revision Box *\/\n.revision-box {\nbackground: var(--green-bg);\nborder: 2px solid var(--green-border);\nborder-radius: 12px;\npadding: 25px;\nmargin: 30px 0;\n}\n.revision-box h3 { color: var(--green-border); margin-top: 0; }\n.revision-box ul { color: #166534; padding-left: 20px; }\n\n\/* CTA *\/\n.cta-section {\nbackground: linear-gradient(135deg, #e8600a, #c2410c, #9a3412);\npadding: 60px 20px;\ntext-align: center;\nmargin-top: 50px;\n}\n.cta-section h2 { color: white; justify-content: center; margin-top: 0; }\n.cta-section p { color: rgba(255,255,255,0.85); font-size: 1.1rem; max-width: 800px; margin: 0 auto 30px; }\n.btn-group { display: flex; gap: 15px; justify-content: center; flex-wrap: wrap; }\n.btn-solid { background: white; color: var(--accent); padding: 12px 30px; border-radius: 6px; font-weight: 700; text-decoration: none; }\n.btn-outline { border: 2px solid white; color: white; padding: 10px 30px; border-radius: 6px; font-weight: 700; text-decoration: none; }\n\n\/* Internal Links *\/\n.internal-box {\nbackground: #f9fafb;\nborder: 1px solid var(--border);\nborder-radius: 10px;\npadding: 20px;\nmargin: 30px 0;\n}\n.internal-box p { font-weight: 700; color: var(--text-muted); font-size: 0.9rem; margin-top: 0; }\n.internal-box a { color: var(--accent); font-weight: 600; text-decoration: none; display: block; margin-bottom: 8px; }\n\n\/* Download Button *\/\n.btn-download {\nbackground: var(--dark);\ncolor: white;\ndisplay: inline-flex;\nalign-items: center;\ngap: 10px;\npadding: 12px 24px;\nborder-radius: 8px;\ntext-decoration: none;\nfont-weight: 600;\nmargin-top: 15px;\n}\n<\/style>\n\n<div class=\"content-wrapper\">\n\n<div style=\"display: flex; align-items: center; gap: 15px; margin-top: 40px; margin-bottom: 20px;\">\n    <div class=\"badge\">01<\/div>\n    <h2 style=\"margin: 0;\">Introduction to Kinetic Theory<\/h2>\n<\/div>\n<p>The <strong>Kinetic Theory 11 Notes<\/strong> provide a foundational understanding of how matter behaves at a microscopic level. Instead of viewing gases as static fluids, kinetic theory treats them as a dynamic collection of rapidly moving atoms or molecules. This shift in perspective allows us to explain macroscopic properties like pressure and temperature through the lens of molecular collisions and individual particle energy. For NEET aspirants, mastering this chapter is crucial as it bridges the gap between pure mechanics and thermodynamics.<\/p>\n\n<div style=\"display: flex; align-items: center; gap: 15px; margin-top: 40px; margin-bottom: 20px;\">\n    <div class=\"badge\">02<\/div>\n    <h2 style=\"margin: 0;\">Assumptions of the Kinetic Theory of Gases<\/h2>\n<\/div>\n<p>To simplify the complex behavior of real gases, we use the &#8220;Ideal Gas&#8221; model based on these specific postulates:<\/p>\n<ul>\n    <li>Gases consist of large numbers of identical, point-like molecules.<\/li>\n    <li>The actual volume of molecules is negligible compared to the total volume of the gas.<\/li>\n    <li>Molecules are in constant, random motion, obeying Newton&#8217;s laws.<\/li>\n    <li>Intermolecular forces (attraction or repulsion) are zero except during collisions.<\/li>\n    <li>Collisions between molecules and with the walls are perfectly elastic.<\/li>\n<\/ul>\n\n<div class=\"callout callout-tip\">\n    <span class=\"pill pill-tip\">TIP<\/span>\n    <p>Remember that &#8220;perfectly elastic&#8221; means both momentum and kinetic energy are conserved during collisions. This is a favorite theoretical question in NEET.<\/p>\n<\/div>\n\n<div style=\"display: flex; align-items: center; gap: 15px; margin-top: 40px; margin-bottom: 20px;\">\n    <div class=\"badge\">03<\/div>\n    <h2 style=\"margin: 0;\">Molecular Motion and Randomness<\/h2>\n<\/div>\n<p>Molecular motion in a gas is chaotic and isotropic, meaning there is no preferred direction. Because molecules move with varying speeds in every possible direction, the gas properties remain uniform throughout the container. This randomness is the source of pressure and ensures that the average velocity of gas molecules in any direction is zero, even though their average speed is quite high.<\/p>\n\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:20px;\">\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<div style=\"display: flex; align-items: center; gap: 15px; margin-top: 40px; margin-bottom: 20px;\">\n    <div class=\"badge\">04<\/div>\n    <h2 style=\"margin: 0;\">Pressure of an Ideal Gas (Derivation)<\/h2>\n<\/div>\n<p>Pressure is defined as the force exerted per unit area by gas molecules hitting the container walls. When a molecule of mass <i>m<\/i> hits a wall with velocity <i>v<sub>x<\/sub><\/i>, its momentum change is 2<i>mv<sub>x<\/sub><\/i>. Summing this over all molecules leads to the fundamental pressure equation.<\/p>\n\n<div class=\"formula-dark\">\n    <span class=\"formula-label\">Ideal Gas Pressure Formula<\/span>\n    <code>P = (1\/3) * (M\/V) * v<sub>rms<\/sub><sup>2<\/sup> = (1\/3) * \u03c1 * v<sub>rms<\/sub><sup>2<\/sup><\/code>\n<\/div>\n\n<div style=\"display: flex; align-items: center; gap: 15px; margin-top: 40px; margin-bottom: 20px;\">\n    <div class=\"badge\">05<\/div>\n    <h2 style=\"margin: 0;\">Kinetic Interpretation of Temperature<\/h2>\n<\/div>\n<p>One of the most profound conclusions of <strong>Kinetic Theory 11 Notes<\/strong> is that temperature is a direct measure of average molecular kinetic energy. Absolute zero (0 K) is the theoretical temperature where all molecular motion stops.<\/p>\n\n<div class=\"formula-orange\">\n    <span class=\"formula-label\">Average Kinetic Energy per Molecule<\/span>\n    <code>K.E. = (3\/2) * k<sub>B<\/sub> * T<\/code>\n<\/div>\n\n<div style=\"display: flex; align-items: center; gap: 15px; margin-top: 40px; margin-bottom: 20px;\">\n    <div class=\"badge\">06<\/div>\n    <h2 style=\"margin: 0;\">Root Mean Square Speed (RMS Speed)<\/h2>\n<\/div>\n<p>Since molecules move at different speeds, we use the Root Mean Square (RMS) speed as a representative value for thermodynamic calculations. It is defined as the square root of the average of the squares of the speeds.<\/p>\n\n<div class=\"formula-dark\">\n    <span class=\"formula-label\">RMS Speed Relations<\/span>\n    <code>v<sub>rms<\/sub> = \u221a(3RT \/ M) = \u221a(3k<sub>B<\/sub>T \/ m) = \u221a(3P \/ \u03c1)<\/code>\n<\/div>\n\n<div class=\"grid-container\">\n    <div class=\"mini-card\">\n        <span class=\"card-title\">Molar Mass Effect<\/span>\n        <p>At a constant temperature, heavier molecules move slower than lighter molecules (v<sub>rms<\/sub> \u221d 1\/\u221aM).<\/p>\n    <\/div>\n    <div class=\"mini-card\">\n        <span class=\"card-title\">Temperature Effect<\/span>\n        <p>RMS speed is directly proportional to the square root of the absolute temperature (v<sub>rms<\/sub> \u221d \u221aT).<\/p>\n    <\/div>\n<\/div>\n\n<a href=\"https:\/\/ksquareinstitute.in\/free-study-material\/\" rel=\"nofollow noopener noreferrer\" target=\"_blank\" class=\"btn-download\">\n    Download Kinetic Theory Formula PDF\n<\/a>\n\n<div style=\"display: flex; align-items: center; gap: 15px; margin-top: 40px; margin-bottom: 20px;\">\n    <div class=\"badge\">07<\/div>\n    <h2 style=\"margin: 0;\">Degrees of Freedom<\/h2>\n<\/div>\n<p>Degrees of freedom (f) refer to the number of independent ways a molecule can possess energy. This includes translation, rotation, and vibration at high temperatures.<\/p>\n\n<table class=\"data-table\">\n    <thead>\n        <tr>\n            <th>Gas Type<\/th>\n            <th>Translational<\/th>\n            <th>Rotational<\/th>\n            <th>Total (f)<\/th>\n        <\/tr>\n    <\/thead>\n    <tbody>\n        <tr>\n            <td>Monoatomic (He, Ar)<\/td>\n            <td>3<\/td>\n            <td>0<\/td>\n            <td>3<\/td>\n        <\/tr>\n        <tr>\n            <td>Diatomic (O2, N2)<\/td>\n            <td>3<\/td>\n            <td>2<\/td>\n            <td>5<\/td>\n        <\/tr>\n        <tr>\n            <td>Polyatomic (Non-linear)<\/td>\n            <td>3<\/td>\n            <td>3<\/td>\n            <td>6<\/td>\n        <\/tr>\n    <\/tbody>\n<\/table>\n\n<div style=\"display: flex; align-items: center; gap: 15px; margin-top: 40px; margin-bottom: 20px;\">\n    <div class=\"badge\">08<\/div>\n    <h2 style=\"margin: 0;\">Law of Equipartition of Energy<\/h2>\n<\/div>\n<p>According to this law, for a system in thermal equilibrium, the total energy is equally distributed among all its degrees of freedom. The energy associated with each degree of freedom per molecule is:<\/p>\n<div class=\"formula-orange\">\n    <code>Energy per d.o.f = (1\/2) * k<sub>B<\/sub> * T<\/code>\n<\/div>\n\n<a href=\"https:\/\/ksquareinstitute.in\/neet-2026-rank-predictor\/\" target=\"_blank\" rel=\"nofollow noopener noreferrer\" style=\"display:block; margin-bottom:20px;\">\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<div style=\"display: flex; align-items: center; gap: 15px; margin-top: 40px; margin-bottom: 20px;\">\n    <div class=\"badge\">09<\/div>\n    <h2 style=\"margin: 0;\">Specific Heat Capacities of Gases<\/h2>\n<\/div>\n<p>Using the law of equipartition, we can calculate the molar specific heats C<sub>v<\/sub> and C<sub>p<\/sub>, and their ratio \u03b3 (gamma).<\/p>\n<ul>\n    <li>C<sub>v<\/sub> = (f\/2)R<\/li>\n    <li>C<sub>p<\/sub> = C<sub>v<\/sub> + R = (f\/2 + 1)R<\/li>\n    <li>\u03b3 = C<sub>p<\/sub> \/ C<sub>v<\/sub> = 1 + 2\/f<\/li>\n<\/ul>\n\n<div style=\"display: flex; align-items: center; gap: 15px; margin-top: 40px; margin-bottom: 20px;\">\n    <div class=\"badge\">10<\/div>\n    <h2 style=\"margin: 0;\">Mean Free Path<\/h2>\n<\/div>\n<p>The mean free path (\u03bb) is the average distance a molecule travels between two successive collisions. It is inversely proportional to the density of the gas and the square of the molecular diameter.<\/p>\n<div class=\"formula-dark\">\n    <code>\u03bb = 1 \/ (\u221a2 * n * \u03c0 * d<sup>2<\/sup>)<\/code>\n<\/div>\n\n<div style=\"display: flex; align-items: center; gap: 15px; margin-top: 40px; margin-bottom: 20px;\">\n    <div class=\"badge\">11<\/div>\n    <h2 style=\"margin: 0;\">Real Gases and Deviations<\/h2>\n<\/div>\n<p>Real gases only behave like ideal gases at <strong>Low Pressure and High Temperature<\/strong>. Under other conditions, intermolecular forces and the finite size of molecules cause deviations. This is corrected using the van der Waals equation:<\/p>\n<div class=\"formula-orange\">\n    <code>(P + a\/V<sup>2<\/sup>)(V - b) = RT<\/code>\n<\/div>\n\n<div style=\"display: flex; align-items: center; gap: 15px; margin-top: 40px; margin-bottom: 20px;\">\n    <div class=\"badge\">12<\/div>\n    <h2 style=\"margin: 0;\">PYQ Trends: Kinetic Theory<\/h2>\n<\/div>\n<table class=\"data-table\">\n    <thead>\n        <tr>\n            <th>Topic<\/th>\n            <th>Frequency<\/th>\n            <th>Common Question Type<\/th>\n        <\/tr>\n    <\/thead>\n    <tbody>\n        <tr>\n            <td>RMS Speed Calc<\/td>\n            <td>High<\/td>\n            <td>Ratio of speeds at different Temps<\/td>\n        <\/tr>\n        <tr>\n            <td>Degrees of Freedom<\/td>\n            <td>Medium<\/td>\n            <td>Calculating \u03b3 for gas mixtures<\/td>\n        <\/tr>\n        <tr>\n            <td>Mean Free Path<\/td>\n            <td>Medium<\/td>\n            <td>Dependence on P and T<\/td>\n        <\/tr>\n    <\/tbody>\n<\/table>\n\n<div class=\"revision-box\">\n    <h3>Quick Revision: Kinetic Theory 11 Notes<\/h3>\n    <ul>\n        <li>Pressure P = (1\/3)\u03c1v<sub>rms<\/sub><sup>2<\/sup><\/li>\n        <li>v<sub>rms<\/sub> = \u221a(3RT\/M); v<sub>avg<\/sub> = \u221a(8RT\/\u03c0M); v<sub>mp<\/sub> = \u221a(2RT\/M)<\/li>\n        <li>Ratio v<sub>mp<\/sub> : v<sub>avg<\/sub> : v<sub>rms<\/sub> = 1 : 1.128 : 1.224<\/li>\n        <li>Avg K.E. of molecule = (3\/2)k<sub>B<\/sub>T<\/li>\n        <li>Total Internal Energy U = (f\/2)nRT<\/li>\n        <li>Mayer&#8217;s Formula: C<sub>p<\/sub> &#8211; C<sub>v<\/sub> = R<\/li>\n        <li>Mean Free Path \u03bb is proportional to T\/P<\/li>\n        <li>Monoatomic \u03b3 = 1.67, Diatomic \u03b3 = 1.4, Triatomic \u03b3 = 1.33<\/li>\n        <li>Ideal behavior: High T and Low P<\/li>\n        <li>Boltzman Constant k<sub>B<\/sub> = R \/ N<sub>A<\/sub><\/li>\n    <\/ul>\n<\/div>\n\n<div class=\"internal-box\">\n    <p>EXPLORE MORE NEET GUIDES<\/p>\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 Exam Tricks<\/a>\n<\/div>\n\n<div style=\"display: flex; align-items: center; gap: 15px; margin-top: 40px; margin-bottom: 20px;\">\n    <div class=\"badge\">13<\/div>\n    <h2 style=\"margin: 0;\">Frequently Asked Questions (FAQs)<\/h2>\n<\/div>\n\n<details>\n    <summary>What is the difference between average speed and RMS speed?<\/summary>\n    <div class=\"faq-content\">\n        Average speed is the arithmetic mean of all speeds, while RMS speed is the square root of the mean of squared speeds. RMS speed is always higher than average speed and is used in kinetic energy calculations.\n    <\/div>\n<\/details>\n\n<details>\n    <summary>How does temperature affect the mean free path?<\/summary>\n    <div class=\"faq-content\">\n        At constant volume, temperature does not affect the mean free path. However, at constant pressure, increasing temperature increases the volume and decreases density, thus increasing the mean free path.\n    <\/div>\n<\/details>\n\n<details>\n    <summary>Why do we use the &#8220;Ideal Gas&#8221; model in Kinetic Theory 11 Notes?<\/summary>\n    <div class=\"faq-content\">\n        The ideal gas model simplifies the math by ignoring intermolecular forces and molecular volume. Most real gases follow these rules at low pressure and high temperature, making it a reliable approximation for NEET problems.\n    <\/div>\n<\/details>\n\n<details>\n    <summary>What are the degrees of freedom for a diatomic gas at high temperature?<\/summary>\n    <div class=\"faq-content\">\n        At high temperatures, vibrational modes become active. A diatomic gas typically has 3 translational + 2 rotational + 2 vibrational = 7 degrees of freedom.\n    <\/div>\n<\/details>\n\n<details>\n    <summary>What is the physical significance of Boltzman&#8217;s Constant?<\/summary>\n    <div class=\"faq-content\">\n        Boltzman&#8217;s constant (k<sub>B<\/sub>) relates the average relative kinetic energy of particles in a gas with the thermodynamic temperature of the gas. It is the gas constant per molecule.\n    <\/div>\n<\/details>\n\n<div class=\"callout callout-warn\">\n    <span class=\"pill pill-warn\">WARN<\/span>\n    <p>Common Mistake: Don&#8217;t forget to convert temperature to Kelvin (K) in all Kinetic Theory formulas. Using Celsius will lead to incorrect results.<\/p>\n<\/div>\n\n<div class=\"cta-section\">\n    <h2>Master NEET Physics with KSquare<\/h2>\n    <p>Join our Mission 180 Rankers Batch and get personalized mentorship, high-yield notes, and comprehensive test series designed by experts.<\/p>\n    <div class=\"btn-group\">\n        <a href=\"https:\/\/courses.ksquare.co.in\/new-courses\/3-mission-180-neet-physics-rankers-batch\" target=\"_blank\" rel=\"nofollow noopener noreferrer\" class=\"btn-solid\">Enroll in Mission 180<\/a>\n        <a href=\"https:\/\/ksquareinstitute.in\/free-study-material\/\" target=\"_blank\" rel=\"nofollow noopener noreferrer\" class=\"btn-outline\">Explore Free Resources<\/a>\n    <\/div>\n<\/div>\n<\/div>\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 Physics Class 11<\/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 to prevent CSS conflicts. *\/\n    #physics-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    #physics-toc-wrapper .container-inner {\n      width: 100%;\n      margin: 0 auto;\n      padding: 0; \/* Set left\/right padding to 0 *\/\n    }\n\n    #physics-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; \/* Keeping a small offset for headings so they aren't touching the screen edge *\/\n    }\n\n    #physics-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; \/* Keeping a small offset for headings *\/\n    }\n\n    #physics-toc-wrapper table {\n      width: 100%;\n      border-collapse: collapse;\n      border-spacing: 0;\n      \/* Border-left and border-right set to none or removed if you want it truly edge-to-edge with the screen *\/\n      border-top: 1px solid #e4e4e7;\n      border-bottom: 1px solid #e4e4e7;\n    }\n\n    #physics-toc-wrapper tr {\n      border-bottom: 1px solid #e4e4e7;\n      transition: all 0.2s ease;\n    }\n\n    #physics-toc-wrapper tr:hover {\n      background-color: #f8fafc;\n    }\n\n    #physics-toc-wrapper tr:last-child {\n      border-bottom: none;\n    }\n\n    #physics-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;\n    }\n\n    #physics-toc-wrapper td:last-child {\n      border-right: none;\n    }\n\n    \/* First column (Numbers) alignment and padding *\/\n    #physics-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    \/* Middle column (Chapter Name) alignment and padding *\/\n    #physics-toc-wrapper td:nth-child(2) {\n      padding-left: 24px;\n      color: #18181b;\n    }\n\n    \/* Last column (Button) alignment and padding *\/\n    #physics-toc-wrapper td:last-child {\n      text-align: right;\n      width: 180px;\n      padding-right: 16px;\n    }\n\n    \/* Button Styling *\/\n    #physics-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    #physics-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 adjustments *\/\n    @media (max-width: 768px) {\n      #physics-toc-wrapper h2 {\n        font-size: 1.75rem;\n        margin-bottom: 32px;\n      }\n      #physics-toc-wrapper td {\n        padding: 18px 12px;\n        font-size: 0.95rem;\n      }\n    }\n  <\/style>\n<\/head>\n<body>\n\n<div id=\"physics-toc-wrapper\">\n  <div class=\"container-inner\">\n    <h1>Table of Contents<\/h1>\n    <h2>Physics &mdash; Class 11<\/h2>\n    \n    <table>\n      <tr><td>01<\/td><td>Units and Measurements<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/units-and-measurements-class-11-notes\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>02<\/td><td>Motion in a Straight Line<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/motion-in-a-straight-line-class-11-notes\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>03<\/td><td>Motion in a Plane<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/motion-in-a-plane-class-11-notes\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>04<\/td><td>Laws of Motion<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/laws-of-motion-class-11-notes\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>05<\/td><td>Work, Energy and Power<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/work-energy-and-power-class-11-notes\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>06<\/td><td>System of Particles and Rotational Motion<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/system-of-particles-and-rotational-motion-class-11-notes\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>07<\/td><td>Gravitation<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/gravitation-class-11-notes\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>08<\/td><td>Mechanical Properties of Solids<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/mechanical-properties-of-solids-class-11-notes\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>09<\/td><td>Mechanical Properties of Fluids<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/mechanical-properties-of-fluids-11-notes\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>10<\/td><td>Thermal Properties of Matter<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/thermal-properties-of-matter-11-notes\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>11<\/td><td>Thermodynamics<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/thermodynamics-11-notes\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>12<\/td><td>Kinetic Theory<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/kinetic-theory-11-notes\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>13<\/td><td>Oscillations<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/oscillations-11-notes\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>14<\/td><td>Waves<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/waves-11-notes\" 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>01 Introduction to Kinetic Theory The Kinetic Theory 11 Notes provide a foundational understanding of how matter behaves at a microscopic level. Instead of viewing gases as static fluids, kinetic theory treats them as a dynamic collection of rapidly moving atoms or molecules. This shift in perspective allows us to explain macroscopic properties like pressure [&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":[151,162,160,163,161],"class_list":["post-3963","post","type-post","status-publish","format-standard","hentry","category-free-study-material","tag-class-11-physics-notes","tag-kinetic-theory-class-11","tag-kinetic-theory-notes","tag-mean-free-path","tag-rms-speed-formula"],"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\/3963","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=3963"}],"version-history":[{"count":4,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/3963\/revisions"}],"predecessor-version":[{"id":4215,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/3963\/revisions\/4215"}],"wp:attachment":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/media?parent=3963"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/categories?post=3963"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/tags?post=3963"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}