[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"doc-seo-343380-105":3,"detail-sidebar-cat-0-en-105":81,"doc-detail-343380-en":130},{"code":4,"msg":5,"data":6},0,"ok",{"site_id":7,"language":8,"slug":9,"title":10,"keywords":11,"description":12,"schema_data":13,"social_meta":74,"head_meta":76,"extra_data":78,"updated_unix":80},105,"en","chapter-17-spontaneity-entropy-and-free-energy-key-notes","Chapter 17 - Spontaneity, Entropy, and Free Energy - Key Notes","","Chapter 17 notes explain spontaneity in thermodynamics through entropy and Gibbs free energy. The First Law establishes energy conservation, while spontaneous processes are linked to an increase in universe entropy and the Second Law. Entropy is treated via randomness/disorder, microstates, and positional entropy. Temperature influences spontaneity through heat flow, and free energy criteria are developed using ΔG = ΔH − TΔS, including effects of pressure, chemical reaction entropy, and equilibrium relations such as ΔG = 0 and ΔG° = −RT ln(K).",{"@graph":14,"@context":73},[15,34,56],{"@type":16,"itemListElement":17},"BreadcrumbList",[18,23,27,31],{"item":19,"name":20,"@type":21,"position":22},"https://docshare.wps.com","Home","ListItem",1,{"item":24,"name":25,"@type":21,"position":26},"https://docshare.wps.com/document/","Document",2,{"item":28,"name":29,"@type":21,"position":30},"https://docshare.wps.com/document/exam/","Exam",3,{"item":32,"name":10,"@type":21,"position":33},"https://docshare.wps.com/document/chapter-17-spontaneity-entropy-and-free-energy-key-notes/343380/",4,{"url":32,"name":10,"@type":35,"image":36,"author":41,"headline":10,"publisher":44,"fileFormat":47,"inLanguage":8,"description":12,"dateModified":48,"datePublished":49,"encodingFormat":47,"isAccessibleForFree":50,"interactionStatistic":51},"DigitalDocument",{"url":37,"@type":38,"width":39,"height":40},"https://docshare.wps.com/thumbnails/chapter-17-spontaneity-entropy-and-free-energy-key-notes/343380.png","ImageObject",300,407,{"name":42,"@type":43},"Himbo","Person",{"url":19,"name":45,"@type":46},"DocShare","Organization","application/pdf","2026-10-29","2026-09-22",true,{"@type":52,"interactionType":53,"userInteractionCount":55},"InteractionCounter",{"@type":54},"ViewAction",7,{"@type":57,"mainEntity":58},"FAQPage",[59,65,69],{"name":60,"@type":61,"acceptedAnswer":62},"How does entropy determine whether a process is spontaneous?","Question",{"text":63,"@type":64},"A process is spontaneous when the entropy of the universe increases (ΔSuniv > 0). This is expressed as ΔSuniv = ΔSsys + ΔSsurr.","Answer",{"name":66,"@type":61,"acceptedAnswer":67},"What is the role of temperature in spontaneity?",{"text":68,"@type":64},"Heat flow governs entropy changes in the surroundings, and the impact of transferring a fixed amount of heat is greater at lower temperatures. Temperature therefore affects whether entropy contributions favor spontaneity.",{"name":70,"@type":61,"acceptedAnswer":71},"How do you use Gibbs free energy to predict reaction direction?",{"text":72,"@type":64},"Use ΔG = ΔH − TΔS. Reactions proceed in the direction that lowers free energy, meaning −ΔG indicates spontaneity and reaching equilibrium.","https://schema.org",{"og:url":32,"og:type":75,"og:title":10,"og:site_name":45,"og:description":12},"article",{"robots":77,"canonical":32},"index,follow",{"doc_id":79,"site_id":7},343380,1790649971,{"code":4,"msg":82,"data":83},"success",[84,88,92,95,100,105,109,114,119,122,126],{"id":22,"doc_module":4,"doc_module_name":25,"category_name":85,"show_sort_weight":86,"slug":87},"Story & Novel",90,"story-novel",{"id":26,"doc_module":4,"doc_module_name":25,"category_name":89,"show_sort_weight":90,"slug":91},"Literature",80,"literature",{"id":33,"doc_module":4,"doc_module_name":25,"category_name":29,"show_sort_weight":93,"slug":94},70,"exam",{"id":96,"doc_module":4,"doc_module_name":25,"category_name":97,"show_sort_weight":98,"slug":99},5,"Comic",60,"comic",{"id":101,"doc_module":4,"doc_module_name":25,"category_name":102,"show_sort_weight":103,"slug":104},6,"Technology",50,"technology",{"id":55,"doc_module":4,"doc_module_name":25,"category_name":106,"show_sort_weight":107,"slug":108},"Healthcare",40,"healthcare",{"id":110,"doc_module":4,"doc_module_name":25,"category_name":111,"show_sort_weight":112,"slug":113},8,"Research & Report",30,"research-report",{"id":115,"doc_module":4,"doc_module_name":25,"category_name":116,"show_sort_weight":117,"slug":118},9,"Religion & Spirituality",20,"religion-spirituality",{"id":117,"doc_module":4,"doc_module_name":25,"category_name":120,"show_sort_weight":117,"slug":121},"World Cup","world-cup",{"id":123,"doc_module":4,"doc_module_name":25,"category_name":124,"show_sort_weight":123,"slug":125},10,"Lifestyle","lifestyle",{"id":127,"doc_module":4,"doc_module_name":25,"category_name":128,"show_sort_weight":96,"slug":129},19,"General","general",{"code":4,"msg":82,"data":131},{"doc_id":79,"user_id":132,"nickname":42,"user_avatar":133,"doc_module":4,"category_id":33,"category_name":29,"doc_title":10,"doc_description":12,"doc_content":134,"file_id":135,"file_url":136,"file_type":137,"file_size":138,"view_count":55,"is_deleted":4,"is_public":22,"is_downloadable":22,"audit_status":22,"page_count":33,"language":139,"language_code":8,"site_id":7,"html_lang":8,"table_of_contents":140,"faqs":141,"seo_title":142,"seo_description":12,"update_tm":143,"read_time":123,"preview_page_count":4},687197100911,"https://ap-avatar.wpscdn.com/avatar/a000239b6f1da00475?x-image-process=image/resize,m_fixed,w_180,h_180&k=1785132997149421697","Chapter 17-Spontaneity, Entropy, and Free Energy  \n17.1 Spontaneous Processes and Entropy  \nA. First Law  \n1. \"Energy can neither be created nor destroyed\"  \n2. The energy of the universe is constant  \nB. Spontaneous Processes  \n1. Processes that occur without outside intervention  \n2. Spontaneous processes may be fast or slow  \na. Many forms of combustion are fast  \nb. Conversion of diamond to graphite is slow  \nC. Entropy (S)  \n1. A measure of the randomness or disorder  \n2. The driving force for a spontaneous process is an increase in the entropy of the universe  \n3. Entropy is a thermodynamic function describing the number of arrangements that are available to a system  \na. Nature proceeds toward the states that have the highest probabilities of existing  \nD. Positional Entropy  \n1. The probability of occurrence of a particular state depends on the number of ways (microstates) in which that arrangement can be achieved  \nSsolid \u003C Sliquid \u003C\u003C Sgas  \n17.2 Entropy and the Second Law of Thermodynamics  \nA. Second Law of Thermodynamics  \n1. \"In any spontaneous process there is always an increase in the entropy of the universe\"  \n2. \"The entropy of the universe is increasing\"  \n3. For a given change to be spontaneous, ∆Suniv must be positive  \n∆Suniv = ∆Ssys + ∆Ssurr  \n17.3 The Effect of Temperature on Spontaneity  \nA. Direction of Heat Flow  \n1. Entropy changes in the surroundings are primarily determined by heat flow  \na. Exothermic reactions in a system at constant temperature increase the entropy of surroundings  \nb. Endothermic reactions in a system at constant temperature decrease the entropy of surroundings  \nc. The impact of the transfer of a given quantity of energy as heat to or from the surroundings will be greater at lower temperatures  \n17.4 Free Energy (G), also called \"Gibbs Free Energy\"  \nA. Calculating Free Energy Change (constant temperature and pressure)  \n1. ∆G = ∆ H-T∆S  \na. H is enthalpy  \nb. T is Kelvin temperature  \nB. Free Energy and Spontaneity  \n1. Reactions proceed in the direction that lowers their free energy (-∆G)  \n\n| Value of ∆H | Value of T∆S | Value of ∆G | Spontaneity |\n| --- | --- | --- | --- |\n| Negative | Positive | Negative | Spontaneous |\n| Positive | Negative | Positive | Nonspontaneous |\n| Negative | Negative | ??? | Spontaneous if the absolute value of ∆ H is greater than the absolute value of T∆S (low temperature) |\n\n\n| Positive | Positive | ??? | Spontaneous if the absolute value of T∆S is greater than the absolute value of ∆ H (high temperature) |\n| --- | --- | --- | --- |\n\n17.5 Entropy Changes in Chemical Reactions  \nA. Constant Temperature and Pressure  \n1. Reactions involving gaseous molecules  \na. The change in positional entropy is dominated by the relative numbers of molecules of gaseous reactants and products  \n2C2 H6(g) + 7O2(g) 􀃆 4CO2(g) + 6H2O(g)  \n9 molecules 10 molecules  \n∆S increases  \nB. Third Law of Thermodynamics  \n1. \"The entropy of a perfect crystal at O K is zero\" (NO disorder, since everything is in perfect position)  \nC. Calculating Entropy Change in a Reaction  \n∆S0reaction = ∑ npS0products − ∑ nr Soreac tan ts  \n1. Entropy is an extensive property (a function of the number of moles)  \n2. Generally, the more complex the molecule, the higher the standard entropy value  \n17.6 Free Energy and Chemical Reactions  \nA. Standard Free Energy Change  \n1. ∆G0 is the change in free energy that will occur if the reactants in their standard states are converted to the products in their standard states  \n2. ∆G0 cannot be measured directly  \n3. The more negative the value for ∆G0 , the farther to the right the reaction will proceed in order to achieve equilibrium  \na. Equilibrium is the lowest possible free energy position for a reaction  \nB. Calculating Free Energy Change  \n1. Method \\#1, for reactions at constant temperature:  \n∆G0 = ∆ H0-T∆S0  \n2. Method \\#2, an adaptation of Hess's Law:  \nCdiamond(s) + O2(g) 􀃆 CO2(g) ∆G0 = -397 kJ  \nCgraphite(s) + O2(g) 􀃆 CO2(g) ∆G0 = -394","cbCaidyjmUkloCic","https://ap.wps.com/l/cbCaidyjmUkloCic","pdf",40730,"English","# 17.1 Spontaneous Processes and Entropy\n## First Law\n## Spontaneous Processes\n## Entropy (S)\n## Positional Entropy\n# 17.2 Entropy and the Second Law of Thermodynamics\n## Second Law of Thermodynamics\n# 17.3 The Effect of Temperature on Spontaneity\n## Direction of Heat Flow\n# 17.4 Free Energy (G) - Gibbs Free Energy\n## Calculating Free Energy Change\n## Free Energy and Spontaneity\n# 17.5 Entropy Changes in Chemical Reactions\n## Constant Temperature and Pressure\n## Third Law of Thermodynamics\n## Calculating Entropy Change in a Reaction\n# 17.6 Free Energy and Chemical Reactions\n## Standard Free Energy Change\n## Calculating Free Energy Change\n# 17.7 The Dependence of Free Energy on Pressure\n## Enthalpy, H\n## Entropy, S\n## Pressure relations for free energy\n# 17.8 Free Energy and Equilibrium\n## Thermodynamic View of Equilibrium\n## Temperature Dependence of K","[{\"question\":\"How does entropy determine whether a process is spontaneous?\",\"answer\":\"A process is spontaneous when the entropy of the universe increases (ΔSuniv \\u003e 0). This is expressed as ΔSuniv = ΔSsys + ΔSsurr.\"},{\"question\":\"What is the role of temperature in spontaneity?\",\"answer\":\"Heat flow governs entropy changes in the surroundings, and the impact of transferring a fixed amount of heat is greater at lower temperatures. Temperature therefore affects whether entropy contributions favor spontaneity.\"},{\"question\":\"How do you use Gibbs free energy to predict reaction direction?\",\"answer\":\"Use ΔG = ΔH − TΔS. Reactions proceed in the direction that lowers free energy, meaning −ΔG indicates spontaneity and reaching equilibrium.\"}]","Chapter 17 - Spontaneity, Entropy, and Free Energy - Key Notes | PDF",1790050975]