{"id":866323,"date":"2025-08-07T11:22:10","date_gmt":"2025-08-07T05:52:10","guid":{"rendered":"https:\/\/leverageedu.com\/discover\/?p=866323"},"modified":"2025-08-07T11:22:10","modified_gmt":"2025-08-07T05:52:10","slug":"ncert-notes-class-11-chemistry-part-i-chapter-5-thermodynamics-free-pdf","status":"publish","type":"post","link":"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-5-thermodynamics-free-pdf\/","title":{"rendered":"NCERT Notes Class 11 Chemistry (Part-I) Chapter-5: Thermodynamics (Free PDF)"},"content":{"rendered":"\n<p>Thermodynamics is an important branch of Chemistry that deals with the study of energy transformations and the laws that govern them. You may already know that energy can neither be created nor destroyed\u2014but where does this energy come from? This unit on thermodynamics will answer that question along with many other related concepts. We have provided detailed notes on Class 11 Chemistry (Part I), Chapter 5, to help you understand the fundamental principles of thermodynamics in a clear and structured manner.<\/p>\n\n\n\n\n\n\n<p><strong>Explore Notes of Class 11 Chemistry<\/strong><\/p>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-background has-fixed-layout\" style=\"background-color:#f1c9d3\"><tbody><tr><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-1-some-basic-concepts-of-chemistry\/\">Chapter 1<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-2-structure-of-atom\/\">Chapter 2<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-3-classification-of-elements-and-periodicity-in-properties\/\">Chapter 3<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-class-11-chemistry-part-i-chapter-iv-chemical-bonding-and-molecular-structure\/\">Chapter 4<\/a><\/strong><\/td><td><strong>Chapter <\/strong>6<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-background has-fixed-layout\" style=\"background-color:#b5f6de\"><tbody><tr><td><a href=\"https:\/\/drive.google.com\/file\/d\/1tcPhXSVFsa3dKCiQY3v6f0Bf7G40Vu6K\/view?usp=drive_link\"><strong>Download PDF of NCERT Notes Class 11 Chemistry (Part-I) Chapter-5:Thermodynamics<\/strong><\/a><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-introduction\">Introduction<\/h2>\n\n\n\n<p>Different forms of energy (chemical, thermal, mechanical, electrical) transform into one another under various conditions. For example, chemical energy stored in molecules can be released as heat during the combustion of fuels (e.g., methane, LPG, coal). The same chemical energy may be converted to mechanical work (e.g., in engines) or electrical energy (e.g., in dry cells).<br>Thermodynamics focuses on macroscopic systems containing large numbers of molecules, not on the microscopic mechanisms or rates of transformation. It considers only the initial and final equilibrium states of a system. Laws of thermodynamics describe energy changes only under such equilibrium or quasi\u2010equilibrium conditions.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-thermodynamic-terms\">Thermodynamic Terms<\/h2>\n\n\n\n<p>In this section, we have provided the thermodynamic terms and their definitions.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-the-system-and-the-surroundings\">The System and the Surroundings<\/h3>\n\n\n\n<p>In thermodynamics, the system refers to the specific part of the universe under observation. The surroundings include everything else apart from the system. Together, the system and the surroundings constitute the universe:<\/p>\n\n\n\n<p><strong>Universe = System + Surroundings<\/strong><\/p>\n\n\n\n<p>In practical terms, the surroundings are considered to be the portion of the universe that can interact with the system. Usually, the immediate region around the system forms the surroundings.<\/p>\n\n\n\n<p><strong>Example:<\/strong> If a reaction occurs between substances A and B in a beaker, the beaker and its contents form the system, while the room in which the beaker is placed is the surroundings.<\/p>\n\n\n\n<p>The boundary is the separation between the system and the surroundings. It can be real or imaginary and is used to track the movement of matter and energy.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-types-of-the-system\">Types of the System<\/h3>\n\n\n\n<p>Systems are classified based on the exchange of energy and matter:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Open System<\/strong>: Both energy and matter can be exchanged with the surroundings.<br>Example: Reactants in an open beaker.<br><\/li>\n\n\n\n<li><strong>Closed System<\/strong>: Energy can be exchanged, but matter cannot.<br>Example: Reactants in a closed metallic vessel.<br><\/li>\n\n\n\n<li><strong>Isolated System<\/strong>: Neither energy nor matter is exchanged with the surroundings.<br>Example: Reactants in a thermos flask or insulated container.<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-the-state-of-the-system\">The State of the System<\/h3>\n\n\n\n<p>A thermodynamic system is described by specifying measurable properties such as pressure (p), volume (V), temperature (T), and composition. These properties are called state variables or state functions because they depend only on the current state of the system, not on how it reached that state. Not all properties need to be specified to define the system. A minimum set of independent properties can define the state, and all other properties are then fixed.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-the-internal-energy-as-a-state-function\">The Internal Energy as a State Function<\/h3>\n\n\n\n<p>The internal energy (U) of a system is the total energy, including chemical, electrical, mechanical, and other forms of energy. It changes when:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Heat is absorbed or released<\/li>\n\n\n\n<li>Work is done on or by the system<\/li>\n\n\n\n<li>Matter enters or leaves the system<\/li>\n<\/ul>\n\n\n\n<p><strong>(a) Work<\/strong><\/p>\n\n\n\n<p>In an adiabatic process (no heat exchange), only work changes the internal energy.<\/p>\n\n\n\n<p>If a system changes from state A (temperature TA, internal energy UA) to state B (TB &gt; TA, internal energy UB) by doing work, the internal energy change is:<br>\u0394U = UB \u2212 UA = w (for adiabatic process)<\/p>\n\n\n\n<p>Sign convention:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>w &gt; 0: Work is done on the system.<\/li>\n\n\n\n<li>w &lt; 0: Work is done by the system.<\/li>\n<\/ul>\n\n\n\n<p><strong>(b) Heat<\/strong><\/p>\n\n\n\n<p>Heat (q) is the energy transferred between the system and surroundings due to temperature difference.<\/p>\n\n\n\n<p>If only heat is involved (no work), the internal energy change is:<br>\u0394U = q<\/p>\n\n\n\n<p>Sign convention:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>q &gt; 0: Heat is absorbed by the system.<\/li>\n\n\n\n<li>q &lt; 0: Heat is released by the system.<\/li>\n<\/ul>\n\n\n\n<p><strong>The General Case<\/strong><\/p>\n\n\n\n<p>When both heat and work are involved, the internal energy change is given by the First Law of Thermodynamics:<br>\u0394U = q + w<\/p>\n\n\n\n<p>For an isolated system, q = 0 and w = 0, so:<br>\u0394U = 0<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-applications\">Applications<\/h2>\n\n\n\n<p>Chemical reactions often involve heat and mechanical work. Thermodynamics helps relate energy changes to internal energy.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-work\">Work<\/h3>\n\n\n\n<p>When a gas expands or contracts, the work done is:<br>w = \u2013 p_ext \u00d7 \u0394V<br>(\u0394V = Vf \u2212 Vi)<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>If \u0394V &gt; 0 (expansion), then w &lt; 0<\/li>\n\n\n\n<li>If \u0394V &lt; 0 (compression), then w &gt; 0<br><\/li>\n<\/ul>\n\n\n\n<p>Reversible Work (external pressure \u2248 internal pressure):<br>w = \u2013 \u222b p dV<\/p>\n\n\n\n<p>For isothermal reversible expansion of an ideal gas:<br>w = \u2013 nRT ln(Vf \/ Vi)<\/p>\n\n\n\n<p>Free Expansion (into vacuum):<br>p_ext = 0, so w = 0<\/p>\n\n\n\n<p>At constant volume:<br>w = 0, so \u0394U = qV<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-enthalpy-h\">Enthalpy, H<\/h3>\n\n\n\n<p>Enthalpy (H) is defined as:<br>H = U + pV<\/p>\n\n\n\n<p>At constant pressure, the enthalpy change is:<br>\u0394H = \u0394U + p\u0394V<\/p>\n\n\n\n<p>Since qp = \u0394H, enthalpy equals the heat absorbed at constant pressure.<\/p>\n\n\n\n<p>For reactions involving gases:<br>\u0394H = \u0394U + \u0394ngRT, where \u0394ng is the change in moles of gas.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-heat-capacity\">Heat Capacity<\/h3>\n\n\n\n<p>Heat capacity (C) is defined as:<br>q = C \u00d7 \u0394T<\/p>\n\n\n\n<p>Specific heat (c):<br>q = m \u00d7 c \u00d7 \u0394T<\/p>\n\n\n\n<p>Molar heat capacity (Cm): heat required for 1 mole of substance.<\/p>\n\n\n\n<p>Cp and Cv for Ideal Gases<\/p>\n\n\n\n<p>At constant volume:<br>qV = nCv\u0394T<\/p>\n\n\n\n<p>At constant pressure:<br>qp = nCp\u0394T<\/p>\n\n\n\n<p>Relation:<br>Cp \u2013 Cv = R<\/p>\n\n\n\n<p class=\"has-pale-ocean-gradient-background has-background\"><strong>Also Read: <a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-psychology-chapter-1-what-is-psychology\/\"><strong>NCERT Notes Class 11 Psychology Chapter 1: What is Psychology? (Free PDF)<\/strong><\/a><\/strong><\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-measurement-of-\u03b4u-and-\u03b4h-calorimetry\">Measurement of \u0394U and \u0394H: Calorimetry<\/h2>\n\n\n\n<p>Carried out in a bomb calorimeter, which is a strong steel container (the &#8220;bomb&#8221;) immersed in water. The substance is ignited electrically. The rise in water temperature helps calculate the heat released:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-\u03b4u-measurements\">\u0394U Measurements<\/h3>\n\n\n\n<p>Done using constant pressure calorimetry (e.g., in a coffee cup). The change in temperature gives the heat exchanged at constant pressure:<\/p>\n\n\n\n<p>qV = \u0394U<br>q = Ccalorimeter \u00d7 \u0394T<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-\u03b4h-measurements\">\u0394H Measurements<\/h3>\n\n\n\n<p>Measured using a constant pressure calorimeter (e.g., coffee cup).<\/p>\n\n\n\n<p>qp = \u0394H<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Exothermic: \u0394H &lt; 0<\/li>\n\n\n\n<li>Endothermic: \u0394H &gt; 0<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-enthalpy-change-\u03b4rh-of-a-reaction-reaction-enthalpy\">Enthalpy Change, \u0394rH of a Reaction \u2013 Reaction Enthalpy<\/h2>\n\n\n\n<p>For a reaction:<br>\u2211 bi Reactants \u2192 \u2211 ai Products<\/p>\n\n\n\n<p>The reaction enthalpy is:<br>\u0394rH = \u2211 ai H(products) \u2212 \u2211 bi H(reactants)<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-standard-enthalpy-of-reactions\">Standard Enthalpy of Reactions<\/h3>\n\n\n\n<p>\u0394rH\u00b0: All substances in standard states (1 bar, 298 K).<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-enthalpy-changes-during-phase-transformations\">Enthalpy Changes during Phase Transformations<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Fusion: \u0394fusH\u00b0 &gt; 0<\/li>\n\n\n\n<li>Vaporisation: \u0394vapH\u00b0 &gt; 0<\/li>\n\n\n\n<li>Sublimation: \u0394subH\u00b0 &gt; 0<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-standard-enthalpy-of-formation\">Standard Enthalpy of Formation<\/h3>\n\n\n\n<p>\u0394fH\u00b0 is the enthalpy change for forming 1 mole of a compound from elements.<br>\u0394fH\u00b0 = 0 for elements in the standard state.<\/p>\n\n\n\n<p>\u0394rH\u00b0 = \u03a3 \u0394fH\u00b0 (products) \u2212 \u03a3 \u0394fH\u00b0 (reactants)<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-thermochemical-equations\">Thermochemical Equations<\/h3>\n\n\n\n<p>Thermochemical equations include physical states and \u0394rH\u00b0.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-hess-s-law-of-constant-heat-summation\">Hess\u2019s Law of Constant Heat Summation<\/h3>\n\n\n\n<p>Total enthalpy change is the same, whether the reaction occurs in one or multiple steps.<\/p>\n\n\n\n<p>\u0394H(overall) = \u0394H1 + \u0394H2 + \u2026<\/p>\n\n\n\n<p class=\"has-pale-ocean-gradient-background has-background\"><strong>Also Read: <strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-psychology-chapter-4-sensory-attentional-and-perceptual-processes\/\"><strong>NCERT Notes Class 11 Psychology Chapter 4: Sensory, Attentional, and Perceptual Processes (Free PDF)<\/strong><\/a><\/strong><\/strong><\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-enthalpies-for-different-types-of-reactions\">Enthalpies for Different Types of Reactions<\/h2>\n\n\n\n<p>The enthalpies for different types of reactions are discussed below.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-standard-enthalpy-of-combustion\">Standard Enthalpy of Combustion<\/h3>\n\n\n\n<p>\u0394cH\u00b0: Enthalpy change when 1 mole of substance burns completely in oxygen.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-enthalpy-of-atomization\">Enthalpy of Atomization<\/h3>\n\n\n\n<p>\u0394aH\u00b0: Enthalpy change to convert 1 mole of element into gaseous atoms.<br>Example: H\u2082(g) \u2192 2H(g)<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-bond-enthalpy\">Bond Enthalpy<\/h3>\n\n\n\n<p>Energy to break 1 mole of specific bonds in gas phase.<\/p>\n\n\n\n<p>\u0394rH\u00b0 \u2248 \u03a3 (bond enthalpies of reactants) \u2013 \u03a3 (bond enthalpies of products)<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-lattice-enthalpy\">Lattice Enthalpy<\/h3>\n\n\n\n<p>Energy required to convert 1 mole of ionic solid into gaseous ions.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-enthalpy-of-solution\">Enthalpy of Solution<\/h3>\n\n\n\n<p>\u0394solH\u00b0: Enthalpy change when 1 mole of solute dissolves in a solvent.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-spontaneity\">Spontaneity<\/h2>\n\n\n\n<p>A spontaneous process occurs without external aid. Examples: flow of heat from hot to cold body, diffusion of gas, melting of ice at room temperature. Thermodynamics helps to determine if a process is spontaneous. Spontaneity does not depend solely on energy change (\u0394U or \u0394H); some endothermic reactions are spontaneous.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-entropy-and-second-amp-third-laws-of-thermodynamics\">Entropy and Second &amp; Third Laws of Thermodynamics<\/h2>\n\n\n\n<p>Entropy is a measure of disorder or randomness. It is a state function. Entropy increases with:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Temperature<\/li>\n\n\n\n<li>Phase transition: solid \u2192 liquid \u2192 gas<\/li>\n\n\n\n<li>Mixing of substances<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-third-law-of-thermodynamics\">Third Law of Thermodynamics<\/h3>\n\n\n\n<p>The entropy of a perfect crystal at absolute zero (0 K) is zero.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-gibbs-energy-change-and-equilibrium\">Gibbs Energy Change and Equilibrium<\/h2>\n\n\n\n<p>G = H \u2013 TS (Gibbs free energy)<br>\u0394G = \u0394H \u2013 T\u0394S<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>\u0394G &lt; 0: Spontaneous<\/li>\n\n\n\n<li>\u0394G &gt; 0: Non-spontaneous<\/li>\n\n\n\n<li>\u0394G = 0: Equilibrium<\/li>\n<\/ul>\n\n\n\n<p>\u0394rG\u00b0 = \u2013 RT ln K, where K is the equilibrium constant.<\/p>\n\n\n\n<p class=\"has-pale-ocean-gradient-background has-background\"><strong>Also Read: <strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-psychology-chapter-4-sensory-attentional-and-perceptual-processes\/\"><strong><\/strong><\/a><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-solutions-class-11-psychology-chapter-5-learning\/\"><strong>NCERT Solutions Class 11 Psychology Chapter 5: Learning (Free PDF)<\/strong><\/a><\/strong><\/strong><\/strong><\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-important-definitions-in-ncert-notes-class-11-chemistry-part-i-chapter-5-thermodynamics\">Important Definitions in NCERT Notes Class 11 Chemistry (Part-I) Chapter 5: Thermodynamics<\/h2>\n\n\n\n<p>Here are the important definitions from NCERT Class 11 Chemistry Chapter 5: Thermodynamics:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Open System<\/strong>: A system in which both energy and matter can be exchanged with the surroundings. Example: Reactants in an open beaker.<\/li>\n\n\n\n<li><strong>Closed System<\/strong>: A system in which energy can be exchanged with the surroundings, but matter cannot. Example: A reaction in a closed metallic vessel.<\/li>\n\n\n\n<li><strong>Isolated System<\/strong>: A system that can exchange neither energy nor matter with the surroundings. Example: A substance in a thermos flask.<\/li>\n\n\n\n<li><strong>State Function<\/strong>: A property of the system that depends only on its current state and not on how it got there. Examples: Pressure (p), Volume (V), Temperature (T), Internal Energy (U), Enthalpy (H), Entropy (S).<\/li>\n\n\n\n<li><strong>Adiabatic Process<\/strong>: A process in which no heat is exchanged between the system and its surroundings. Any change in internal energy is due to work only.<\/li>\n\n\n\n<li><strong>Isothermal Process<\/strong>: A process in which the temperature of the system remains constant during the change.<\/li>\n\n\n\n<li><strong>Isobaric Process<\/strong>: A process that occurs at constant pressure.<\/li>\n\n\n\n<li><strong>Isochoric Process<\/strong>: A process that occurs at constant volume.<\/li>\n\n\n\n<li><strong>Standard State<\/strong>: The most stable form of a substance at 1 bar pressure and a specified temperature (usually 298 K).<\/li>\n\n\n\n<li><strong>Lattice Enthalpy<\/strong>: The amount of energy required to completely separate one mole of an ionic solid into its gaseous ions.<\/li>\n<\/ul>\n\n\n\n<p><strong>Explore Notes of Class 11 Chemistry<\/strong><\/p>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-background has-fixed-layout\" style=\"background-color:#f1c9d3\"><tbody><tr><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-1-some-basic-concepts-of-chemistry\/\">Chapter 1<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-2-structure-of-atom\/\">Chapter 2<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-3-classification-of-elements-and-periodicity-in-properties\/\">Chapter 3<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-class-11-chemistry-part-i-chapter-iv-chemical-bonding-and-molecular-structure\/\">Chapter 4<\/a><\/strong><\/td><td><strong>Chapter <\/strong>6<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<p><strong>Download the Solutions of Other Chapters of Class 11 Chemistry<\/strong><\/p>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-background has-fixed-layout\" style=\"background-color:#d0a0f9\"><tbody><tr><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-solutions-class-11-chemistry-part-1-chapter-1-some-basic-concepts-of-chemistry\/\">Chapter 1<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-solutions-class-11-chemistry-part-i-chapter-2-structure-of-atom-free-pdf\/\">Chapter 2<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-solutions-class-11-chemistry-part-1-chapter-3-classification-of-elements-and-periodicity-in-properties\/\">Chapter 3<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-solutions-class-11-chemistry-part-1-chapter-iv-chemical-bonding-molecular-structure\/\">Chapter 4<\/a><\/strong><\/td><td><strong>Chapter <\/strong>6<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<p><strong>Additional Reads<\/strong><\/p>\n\n\n\n<figure class=\"wp-block-table is-style-stripes\"><table class=\"has-pale-ocean-gradient-background has-background has-fixed-layout\"><tbody><tr><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/the-rise-of-nationalism-in-europe-ncert-solutions-for-class-10-history-social-science-chapter-1\/\">The \u201cRise of Nationalism in Europe\u201d NCERT Solutions for Class 10 History Social Science Chapter 1<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-cbse-history-class-10-chapter-2-notes-nationalism-in-india\/\">NCERT CBSE History Class 10 Chapter 2 Notes Nationalism in India<\/a><\/strong><\/td><\/tr><tr><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/solutions-for-ncert-notes-of-chapter-2-history-class-10-%c2%a8nationalism-in-india%c2%a8-pdf\/\">Solutions for NCERT Notes of Chapter 2 History Class 10 \u00a8Nationalism in India\u00a8 (PDF)<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-cbse-history-chapter-4-class-10-notes-the-age-of-industralisation\/\">NCERT CBSE History Chapter 4 Class 10 Notes The Age of Industralisation<\/a><\/strong><\/td><\/tr><tr><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-psychology-chapter-8-motivation-and-emotion\/\">NCERT Notes Class 11 Psychology Chapter 8: Motivation and Emotion (Free PDF)<\/a><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-solutions-class-11-psychology-chapter-8-motivation-and-emotion\/\">NCERT Solutions Class 11 Psychology Chapter 8: Motivation and Emotion (Free PDF)<\/a><\/strong><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<figure class=\"wp-block-embed is-type-video is-provider-youtube wp-block-embed-youtube wp-embed-aspect-16-9 wp-has-aspect-ratio\"><div class=\"wp-block-embed__wrapper\">\n<iframe loading=\"lazy\" title=\"Thermodynamics-1 One Shot Lecture for 11th Class with Ashu sir | Science and Fun 11th 12th\" width=\"1200\" height=\"675\" src=\"https:\/\/www.youtube.com\/embed\/lwe269bVEIo?feature=oembed\" frameborder=\"0\" allow=\"accelerometer; autoplay; clipboard-write; encrypted-media; gyroscope; picture-in-picture; web-share\" referrerpolicy=\"strict-origin-when-cross-origin\" allowfullscreen><\/iframe>\n<\/div><\/figure>\n\n\n\n<p>Source- Science and Fun Motivation<\/p>\n\n\n\n<p><strong>Explore notes on other subjects in the NCERT Class 11<\/strong><\/p>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-background has-fixed-layout\" style=\"background-color:#ffc7c7\"><tbody><tr><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-and-solutions-class-11-english\/\"><strong>English<\/strong><\/a><\/td><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-and-solutions-class-11-sociology\/\"><strong>Sociology<\/strong><\/a><\/td><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-and-solutions-class-11-geography\/\"><strong>Geography<\/strong><\/a><\/td><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-and-solutions-class-11-political-science\/\"><strong>Political Science<\/strong><\/a><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-and-solutions-class-11-psychology\/\">Psychology<\/a><\/strong><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-faqs\">FAQs<\/h2>\n\n\n\n<div class=\"schema-faq wp-block-yoast-faq-block\"><div class=\"schema-faq-section\" id=\"faq-question-1754544938329\"><strong class=\"schema-faq-question\"><strong>Q.1 What is the difference between internal energy and enthalpy?<\/strong><\/strong> <p class=\"schema-faq-answer\"><strong>Answer: <\/strong>Internal energy (U) is the total energy contained within a system, including all forms such as kinetic, potential, chemical, and electrical energy. Enthalpy (H) is defined as the sum of internal energy and the product of pressure and volume of the system:<br\/>H = U + pV. Enthalpy is particularly useful for studying heat changes at constant pressure, whereas internal energy is useful for constant volume processes.<\/p> <\/div> <div class=\"schema-faq-section\" id=\"faq-question-1754544956846\"><strong class=\"schema-faq-question\"><strong>Q.2 How does the First Law of Thermodynamics relate to chemical reactions?<\/strong><\/strong> <p class=\"schema-faq-answer\"><strong>Answer: <\/strong>The First Law of Thermodynamics states that energy cannot be created or destroyed, only converted from one form to another. In chemical reactions, this is represented as:<br\/>\u0394U = q + w, where \u0394U is the change in internal energy, q is the heat added to the system, and w is the work done on the system. It ensures that the total energy change in a chemical reaction accounts for both heat exchange and work done.<\/p> <\/div> <div class=\"schema-faq-section\" id=\"faq-question-1754544998944\"><strong class=\"schema-faq-question\"><strong>Q.3 What determines whether a chemical reaction is spontaneous?<\/strong><\/strong> <p class=\"schema-faq-answer\"><strong>Answer: <\/strong>The spontaneity of a chemical reaction is determined by the Gibbs free energy change (\u0394G), which is given by the equation:<br\/>\u0394G = \u0394H \u2013 T\u0394S, where \u0394H is the enthalpy change, T is the temperature, and \u0394S is the entropy change.<br\/>If \u0394G &lt; 0, the reaction is spontaneous.<br\/>If \u0394G > 0, the reaction is non-spontaneous.<br\/>If \u0394G = 0, the system is at equilibrium.<\/p> <\/div> <\/div>\n\n\n\n<p>For more topics, follow LeverageEdu <a href=\"https:\/\/leverageedu.com\/discover\/category\/school-education\/ncert-study-material\/\"><strong>NCERT Study Material<\/strong><\/a> today!<\/p>\n","protected":false},"excerpt":{"rendered":"Thermodynamics is an important branch of Chemistry that deals with the study of energy transformations and the laws&hellip;\n","protected":false},"author":133,"featured_media":866333,"comment_status":"open","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"editor_notices":[],"footnotes":""},"categories":[477,389],"tags":[],"class_list":{"0":"post-866323","1":"post","2":"type-post","3":"status-publish","4":"format-standard","5":"has-post-thumbnail","7":"category-ncert-study-material","8":"category-school-education"},"yoast_head":"<!-- This site is optimized with the Yoast SEO Premium plugin v27.3 (Yoast SEO v27.3) - https:\/\/yoast.com\/product\/yoast-seo-premium-wordpress\/ -->\n<title>NCERT Notes Class 11 Chemistry (Part-I) Chapter-5: Thermodynamics (Free PDF) - Leverage Edu Discover<\/title>\n<meta name=\"description\" content=\"NCERT Notes for Class 11 Chemistry Chapter 5: Thermodynamics. 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His expertise lies in simplifying complex information into engaging, student-friendly content. Passionate about global education, Devanshu crafts stories that empower students to make informed decisions about their academic and career journeys.","sameAs":["https:\/\/www.linkedin.com\/in\/devsrivastava3"],"url":"https:\/\/leverageedu.com\/discover\/author\/devanshusrivastava\/"},{"@type":"Question","@id":"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-5-thermodynamics-free-pdf\/#faq-question-1754544938329","position":1,"url":"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-5-thermodynamics-free-pdf\/#faq-question-1754544938329","name":"Q.1 What is the difference between internal energy and enthalpy?","answerCount":1,"acceptedAnswer":{"@type":"Answer","text":"<strong>Answer: <\/strong>Internal energy (U) is the total energy contained within a system, including all forms such as kinetic, potential, chemical, and electrical energy. Enthalpy (H) is defined as the sum of internal energy and the product of pressure and volume of the system:<br\/>H = U + pV. Enthalpy is particularly useful for studying heat changes at constant pressure, whereas internal energy is useful for constant volume processes.","inLanguage":"en-US"},"inLanguage":"en-US"},{"@type":"Question","@id":"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-5-thermodynamics-free-pdf\/#faq-question-1754544956846","position":2,"url":"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-5-thermodynamics-free-pdf\/#faq-question-1754544956846","name":"Q.2 How does the First Law of Thermodynamics relate to chemical reactions?","answerCount":1,"acceptedAnswer":{"@type":"Answer","text":"<strong>Answer: <\/strong>The First Law of Thermodynamics states that energy cannot be created or destroyed, only converted from one form to another. In chemical reactions, this is represented as:<br\/>\u0394U = q + w, where \u0394U is the change in internal energy, q is the heat added to the system, and w is the work done on the system. It ensures that the total energy change in a chemical reaction accounts for both heat exchange and work done.","inLanguage":"en-US"},"inLanguage":"en-US"},{"@type":"Question","@id":"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-5-thermodynamics-free-pdf\/#faq-question-1754544998944","position":3,"url":"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-5-thermodynamics-free-pdf\/#faq-question-1754544998944","name":"Q.3 What determines whether a chemical reaction is spontaneous?","answerCount":1,"acceptedAnswer":{"@type":"Answer","text":"<strong>Answer: <\/strong>The spontaneity of a chemical reaction is determined by the Gibbs free energy change (\u0394G), which is given by the equation:<br\/>\u0394G = \u0394H \u2013 T\u0394S, where \u0394H is the enthalpy change, T is the temperature, and \u0394S is the entropy change.<br\/>If \u0394G &lt; 0, the reaction is spontaneous.<br\/>If \u0394G > 0, the reaction is non-spontaneous.<br\/>If \u0394G = 0, the system is at equilibrium.","inLanguage":"en-US"},"inLanguage":"en-US"}]}},"acf":[],"_links":{"self":[{"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/posts\/866323","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/users\/133"}],"replies":[{"embeddable":true,"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/comments?post=866323"}],"version-history":[{"count":0,"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/posts\/866323\/revisions"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/media\/866333"}],"wp:attachment":[{"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/media?parent=866323"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/categories?post=866323"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/tags?post=866323"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}