{"id":2596,"date":"2016-08-24T13:49:32","date_gmt":"2016-08-24T13:49:32","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/?post_type=chapter&#038;p=2596"},"modified":"2017-08-28T21:54:57","modified_gmt":"2017-08-28T21:54:57","slug":"vapor-pressure","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/chapter\/vapor-pressure\/","title":{"raw":"Vapor Pressure","rendered":"Vapor Pressure"},"content":{"raw":"<div class=\"textbox learning-objectives\">\r\n<h3>Learning Objectives<\/h3>\r\n<ul>\r\n \t<li>Define vapor pressure.<\/li>\r\n \t<li>Describe the relationship between the intermolecular forces in a liquid and its vapor pressure.<\/li>\r\n \t<li>Describe the relationship between the vapor pressure of a liquid and temperature.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div class=\"textbox examples\">\r\n<h3>Examples<\/h3>\r\n<h4 id=\"x-ck12-MmIyZDljNjI4YmRlZWQwYTZhZjc1YTMzYjBlZmQ4YzA.-tkc_8-qfn\">What causes this toy to move?<\/h4>\r\n<p id=\"x-ck12-MWMyZjgwMjY3ZjJiM2JiOWYzNWNiYzdhMGY4ZTdjYTE.-z8u\">The drinking duck is a toy that many kids (and adults) enjoy playing with. You can see the drinking duck in action in the video at the link below:<\/p>\r\nhttps:\/\/youtu.be\/Bzw0kWvfVkA\r\n<p id=\"x-ck12-NzAwMTU2ZDY2OGU5ZTU5OTUwNmE0NWY5Y2Y2OGQzY2Y.-rj8\">The motion of the duck illustrates a physical principle called vapor pressure. As the vapor pressure changes, the liquid in the duck moves up and down, causing the duck to move.<\/p>\r\n\r\n<\/div>\r\n&nbsp;\r\n<h3>Vapor Pressure<\/h3>\r\n<p id=\"x-ck12-OTcxNTRhOGQ2ZmNiNGVmZDg0NjIzNmRhZTY2MjdiYmU.-irc\">When a partially filled container of liquid is sealed with a stopper, some liquid molecules at the surface evaporate into the <strong>vapor phase <\/strong>. However, the vapor molecules cannot escape from the container and so after a certain amount of time, the space above the liquid reaches a point where it cannot hold any more vapor molecules. Now some of the vapor molecules condense back into a liquid. The system reaches the point where the rate of evaporation is equal to the rate of condensation (see <strong>Figure <\/strong>below ). This is called a dynamic equilibrium between the liquid and vapor phases.<\/p>\r\n\r\n<div id=\"x-ck12-MmRjNzk1NWVmZTgwMTZjOGQ1NTQwZjI3MmVhZmRiMTA.-yeu\" class=\"x-ck12-img-thumbnail x-ck12-nofloat\">\r\n<p id=\"x-ck12-elp\"><img id=\"x-ck12-OTgwNDUtMTM2MzMzMDMxMC0xMi0xMC00LjEuOC4x\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19212027\/20140811155424458396.png\" alt=\"When the rate of condensation is equal to the rate of evaporation, a dynamic equilibrium is formed\" longdesc=\"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-admin\/Equilibrium%20between%20liquid%20phase%20and%20vapor%20phase.\" \/><\/p>\r\n<strong>Figure 13.10<\/strong>\r\n<p id=\"x-ck12-YjhmYTMyYzlhM2E5MGZkNWQ0MTMzMjNiYzMxMzExOTU.-fdp\">Equilibrium between liquid phase and vapor phase.<\/p>\r\n\r\n<\/div>\r\n<p id=\"x-ck12-N2U2YTY4ZTc1NjI0YWFhODJkZGY5ZWNhMWI2Y2EzNmQ.-tod\">A dynamic equilibrium can be illustrated by an equation with a double arrow, meaning that the reaction is occurring in both directions and at the same rate.<\/p>\r\n<p id=\"x-ck12-0em\" class=\"x-ck12-indent\"><img class=\"x-ck12-block-math\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19212028\/68cb3c8a61996b4764f2ce71c837e768.png\" alt=\"text{H}_2 text{O}(l) rightleftharpoons text{H}_2 text{O}(g)\" width=\"139\" height=\"18\" \/><\/p>\r\n<p id=\"x-ck12-MGFmNDUyNTcxZmUzMDMwNjIxNTkzYjcyNmM1MjQ0NzQ.-uiv\">The forward direction represents the evaporation process, while the reverse direction represents the condensation process.<\/p>\r\n<p id=\"x-ck12-Y2IyZDU5NWMyNTVhNTZlMDUzN2NmOTAwODdmNDFmNTc.-p52\">Because they cannot escape the container, the vapor molecules above the surface of the liquid exert a pressure on the walls of the container. The <strong>vapor pressure <\/strong>is a measure of the presure (force per unit area) exerted by a gas above a liquid in a sealed container. Vapor pressure is a property of a liquid based on the strength of its intermolecular forces. A liquid with weak intermolecular forces evaporates more easily and has a high vapor pressure. A liquid with stronger intermolecular forces does not evaporate easily and thus has a lower vapor pressure. For example, diethyl ether is a nonpolar liquid with weak dispersion forces. Its vapor pressure at 20\u00b0C is 58.96 kPa. Water is a polar liquid whose molecules are attracted to one another by relatively strong hydrogen bonding. The vapor pressure of water at 20\u00b0C is only 2.33 kPa, far less than that of diethyl ether.<\/p>\r\n\r\n<h4>Vapor Pressure and Temperature<\/h4>\r\n<p id=\"x-ck12-ODU0MTZkZWE3NDJmZGU5Mjg1ZDE2YTAwMjI5MTYwMzE.-oyu\">Vapor pressure is dependent upon temperature. When the liquid in a closed container is heated, more molecules escape the <strong>liquid phase <\/strong>and evaporate. The greater number of vapor molecules strike the container walls more frequently, resulting in an increase in pressure. The <strong>Table <\/strong>below shows the temperature dependence of the vapor pressure of three liquids.<\/p>\r\n\r\n<table id=\"x-ck12-YmYyZjlmM2VkOGNlMjM3ODdiY2JhYWI0OTUxOTAwMjI.-g8b\" class=\"x-ck12-nofloat\" border=\"1\"><caption>Vapor Pressure (in kPa) of Three Liquids at Different Temperatures<\/caption>\r\n<tbody>\r\n<tr>\r\n<td><\/td>\r\n<td><strong>0\u00b0C<\/strong><\/td>\r\n<td><strong>20\u00b0C<\/strong><\/td>\r\n<td><strong>40\u00b0C<\/strong><\/td>\r\n<td><strong>60\u00b0C<\/strong><\/td>\r\n<td><strong>80\u00b0C<\/strong><\/td>\r\n<td><strong>100\u00b0C<\/strong><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Water<\/td>\r\n<td>0.61<\/td>\r\n<td>2.33<\/td>\r\n<td>7.37<\/td>\r\n<td>19.92<\/td>\r\n<td>47.34<\/td>\r\n<td>101.33<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Ethanol<\/td>\r\n<td>1.63<\/td>\r\n<td>5.85<\/td>\r\n<td>18.04<\/td>\r\n<td>47.02<\/td>\r\n<td>108.34<\/td>\r\n<td>225.75<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Diethyl ether<\/td>\r\n<td>24.70<\/td>\r\n<td>58.96<\/td>\r\n<td>122.80<\/td>\r\n<td>230.65<\/td>\r\n<td>399.11<\/td>\r\n<td>647.87<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<p id=\"x-ck12-M2Y2MzFmMTM2MmViZTg2YjU2ZjE1ZjgxZjRjN2IwY2Y.-zeh\">Notice that the temperature dependence of the vapor pressure is not linear. From 0\u00b0C to 80\u00b0C, the vapor pressure of water increases by 46.73 kPa, while it increases by 53.99 kPa in only a span of twenty degrees from 80\u00b0C to 100\u00b0C.<\/p>\r\n\r\n<div class=\"textbox key-takeaways\">\r\n<h3>Summary<\/h3>\r\n<ul id=\"x-ck12-MTVkMDI5MGJhMmZmNDk2NGQzNzVmZGJiZWQxNTY0ODE.-sfg\">\r\n \t<li>Vapor pressure is a measure of the pressure exerted by a gas above a liquid in a sealed container.<\/li>\r\n \t<li>Strong intermolecular forces produce a lower rate of evaporation and a lower vapor pressure.<\/li>\r\n \t<li>Weak intermolecular forces produce a higher rate of evaporation and a higher vapor pressure.<\/li>\r\n \t<li>As the temperature increases, the vapor pressure increases.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Practice<\/h3>\r\n<p id=\"x-ck12-Y2JlMjQ5M2YzMTNmNmRjMzNmZTI0MTMzYzcwM2IzZmY.-don\">Use the link below to answer the following questions:<\/p>\r\n<p id=\"x-ck12-NzAzZGFhMTJiZTQ3MTdmMWY5NGJkYTA2YTIxOTVmMTM.-bz3\"><a href=\"http:\/\/www.chem.purdue.edu\/gchelp\/liquids\/vpress.html\">http:\/\/www.chem.purdue.edu\/gchelp\/liquids\/vpress.html<\/a><\/p>\r\n\r\n<ol id=\"x-ck12-ZDk2MzZhZTJjYzY0OTZhMDg2YmQzMTE1MGRlZDJkNTI.-zyx\">\r\n \t<li>What material has the highest vapor pressure at 25\u00b0C?<\/li>\r\n \t<li>What material has the lowest vapor pressure at 25\u00b0C?<\/li>\r\n \t<li>What device is used to measure vapor pressure?<\/li>\r\n \t<li>Does the surface area of the liquid affect the vapor pressure?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Review<\/h3>\r\n<ol id=\"x-ck12-MDVlYmJhMDNhOWVkNGJmMWQyZmI0ZDNiMTg2YmZmYmY.-hk1\">\r\n \t<li>Define vapor pressure.<\/li>\r\n \t<li>How do intermolecular forces affect vapor pressure?<\/li>\r\n \t<li>How does temperature affect vapor pressure?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<div class=\"x-ck12-data-problem-set\">\r\n<div class=\"textbox learning-objectives\">\r\n<h3>Glossary<\/h3>\r\n<div class=\"x-ck12-data-vocabulary\">\r\n<ul id=\"x-ck12-YmUwNmUwZWY5MmRkMGI1MDQzMWI2ZTNlMTQ2YWIzNGE.-vaj\">\r\n \t<li><strong>liquid phase: <\/strong>A substance in the liquid state of matter.<\/li>\r\n \t<li><strong>vapor phase: <\/strong>A substance in the gaseous state of matter.<\/li>\r\n \t<li><strong>vapor pressure: <\/strong>A measure of the force exerted by a gas above a liquid in a sealed container.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<\/div>","rendered":"<div class=\"textbox learning-objectives\">\n<h3>Learning Objectives<\/h3>\n<ul>\n<li>Define vapor pressure.<\/li>\n<li>Describe the relationship between the intermolecular forces in a liquid and its vapor pressure.<\/li>\n<li>Describe the relationship between the vapor pressure of a liquid and temperature.<\/li>\n<\/ul>\n<\/div>\n<div class=\"textbox examples\">\n<h3>Examples<\/h3>\n<h4 id=\"x-ck12-MmIyZDljNjI4YmRlZWQwYTZhZjc1YTMzYjBlZmQ4YzA.-tkc_8-qfn\">What causes this toy to move?<\/h4>\n<p id=\"x-ck12-MWMyZjgwMjY3ZjJiM2JiOWYzNWNiYzdhMGY4ZTdjYTE.-z8u\">The drinking duck is a toy that many kids (and adults) enjoy playing with. You can see the drinking duck in action in the video at the link below:<\/p>\n<p><iframe loading=\"lazy\" id=\"oembed-1\" title=\"Drinking Duck\" width=\"500\" height=\"375\" src=\"https:\/\/www.youtube.com\/embed\/Bzw0kWvfVkA?feature=oembed&#38;rel=0\" frameborder=\"0\" allowfullscreen=\"allowfullscreen\"><\/iframe><\/p>\n<p id=\"x-ck12-NzAwMTU2ZDY2OGU5ZTU5OTUwNmE0NWY5Y2Y2OGQzY2Y.-rj8\">The motion of the duck illustrates a physical principle called vapor pressure. As the vapor pressure changes, the liquid in the duck moves up and down, causing the duck to move.<\/p>\n<\/div>\n<p>&nbsp;<\/p>\n<h3>Vapor Pressure<\/h3>\n<p id=\"x-ck12-OTcxNTRhOGQ2ZmNiNGVmZDg0NjIzNmRhZTY2MjdiYmU.-irc\">When a partially filled container of liquid is sealed with a stopper, some liquid molecules at the surface evaporate into the <strong>vapor phase <\/strong>. However, the vapor molecules cannot escape from the container and so after a certain amount of time, the space above the liquid reaches a point where it cannot hold any more vapor molecules. Now some of the vapor molecules condense back into a liquid. The system reaches the point where the rate of evaporation is equal to the rate of condensation (see <strong>Figure <\/strong>below ). This is called a dynamic equilibrium between the liquid and vapor phases.<\/p>\n<div id=\"x-ck12-MmRjNzk1NWVmZTgwMTZjOGQ1NTQwZjI3MmVhZmRiMTA.-yeu\" class=\"x-ck12-img-thumbnail x-ck12-nofloat\">\n<p id=\"x-ck12-elp\"><img decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MzMzMDMxMC0xMi0xMC00LjEuOC4x\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19212027\/20140811155424458396.png\" alt=\"When the rate of condensation is equal to the rate of evaporation, a dynamic equilibrium is formed\" longdesc=\"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-admin\/Equilibrium%20between%20liquid%20phase%20and%20vapor%20phase.\" \/><\/p>\n<p><strong>Figure 13.10<\/strong><\/p>\n<p id=\"x-ck12-YjhmYTMyYzlhM2E5MGZkNWQ0MTMzMjNiYzMxMzExOTU.-fdp\">Equilibrium between liquid phase and vapor phase.<\/p>\n<\/div>\n<p id=\"x-ck12-N2U2YTY4ZTc1NjI0YWFhODJkZGY5ZWNhMWI2Y2EzNmQ.-tod\">A dynamic equilibrium can be illustrated by an equation with a double arrow, meaning that the reaction is occurring in both directions and at the same rate.<\/p>\n<p id=\"x-ck12-0em\" class=\"x-ck12-indent\"><img loading=\"lazy\" decoding=\"async\" class=\"x-ck12-block-math\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19212028\/68cb3c8a61996b4764f2ce71c837e768.png\" alt=\"text{H}_2 text{O}(l) rightleftharpoons text{H}_2 text{O}(g)\" width=\"139\" height=\"18\" \/><\/p>\n<p id=\"x-ck12-MGFmNDUyNTcxZmUzMDMwNjIxNTkzYjcyNmM1MjQ0NzQ.-uiv\">The forward direction represents the evaporation process, while the reverse direction represents the condensation process.<\/p>\n<p id=\"x-ck12-Y2IyZDU5NWMyNTVhNTZlMDUzN2NmOTAwODdmNDFmNTc.-p52\">Because they cannot escape the container, the vapor molecules above the surface of the liquid exert a pressure on the walls of the container. The <strong>vapor pressure <\/strong>is a measure of the presure (force per unit area) exerted by a gas above a liquid in a sealed container. Vapor pressure is a property of a liquid based on the strength of its intermolecular forces. A liquid with weak intermolecular forces evaporates more easily and has a high vapor pressure. A liquid with stronger intermolecular forces does not evaporate easily and thus has a lower vapor pressure. For example, diethyl ether is a nonpolar liquid with weak dispersion forces. Its vapor pressure at 20\u00b0C is 58.96 kPa. Water is a polar liquid whose molecules are attracted to one another by relatively strong hydrogen bonding. The vapor pressure of water at 20\u00b0C is only 2.33 kPa, far less than that of diethyl ether.<\/p>\n<h4>Vapor Pressure and Temperature<\/h4>\n<p id=\"x-ck12-ODU0MTZkZWE3NDJmZGU5Mjg1ZDE2YTAwMjI5MTYwMzE.-oyu\">Vapor pressure is dependent upon temperature. When the liquid in a closed container is heated, more molecules escape the <strong>liquid phase <\/strong>and evaporate. The greater number of vapor molecules strike the container walls more frequently, resulting in an increase in pressure. The <strong>Table <\/strong>below shows the temperature dependence of the vapor pressure of three liquids.<\/p>\n<table id=\"x-ck12-YmYyZjlmM2VkOGNlMjM3ODdiY2JhYWI0OTUxOTAwMjI.-g8b\" class=\"x-ck12-nofloat\">\n<caption>Vapor Pressure (in kPa) of Three Liquids at Different Temperatures<\/caption>\n<tbody>\n<tr>\n<td><\/td>\n<td><strong>0\u00b0C<\/strong><\/td>\n<td><strong>20\u00b0C<\/strong><\/td>\n<td><strong>40\u00b0C<\/strong><\/td>\n<td><strong>60\u00b0C<\/strong><\/td>\n<td><strong>80\u00b0C<\/strong><\/td>\n<td><strong>100\u00b0C<\/strong><\/td>\n<\/tr>\n<tr>\n<td>Water<\/td>\n<td>0.61<\/td>\n<td>2.33<\/td>\n<td>7.37<\/td>\n<td>19.92<\/td>\n<td>47.34<\/td>\n<td>101.33<\/td>\n<\/tr>\n<tr>\n<td>Ethanol<\/td>\n<td>1.63<\/td>\n<td>5.85<\/td>\n<td>18.04<\/td>\n<td>47.02<\/td>\n<td>108.34<\/td>\n<td>225.75<\/td>\n<\/tr>\n<tr>\n<td>Diethyl ether<\/td>\n<td>24.70<\/td>\n<td>58.96<\/td>\n<td>122.80<\/td>\n<td>230.65<\/td>\n<td>399.11<\/td>\n<td>647.87<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p id=\"x-ck12-M2Y2MzFmMTM2MmViZTg2YjU2ZjE1ZjgxZjRjN2IwY2Y.-zeh\">Notice that the temperature dependence of the vapor pressure is not linear. From 0\u00b0C to 80\u00b0C, the vapor pressure of water increases by 46.73 kPa, while it increases by 53.99 kPa in only a span of twenty degrees from 80\u00b0C to 100\u00b0C.<\/p>\n<div class=\"textbox key-takeaways\">\n<h3>Summary<\/h3>\n<ul id=\"x-ck12-MTVkMDI5MGJhMmZmNDk2NGQzNzVmZGJiZWQxNTY0ODE.-sfg\">\n<li>Vapor pressure is a measure of the pressure exerted by a gas above a liquid in a sealed container.<\/li>\n<li>Strong intermolecular forces produce a lower rate of evaporation and a lower vapor pressure.<\/li>\n<li>Weak intermolecular forces produce a higher rate of evaporation and a higher vapor pressure.<\/li>\n<li>As the temperature increases, the vapor pressure increases.<\/li>\n<\/ul>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Practice<\/h3>\n<p id=\"x-ck12-Y2JlMjQ5M2YzMTNmNmRjMzNmZTI0MTMzYzcwM2IzZmY.-don\">Use the link below to answer the following questions:<\/p>\n<p id=\"x-ck12-NzAzZGFhMTJiZTQ3MTdmMWY5NGJkYTA2YTIxOTVmMTM.-bz3\"><a href=\"http:\/\/www.chem.purdue.edu\/gchelp\/liquids\/vpress.html\">http:\/\/www.chem.purdue.edu\/gchelp\/liquids\/vpress.html<\/a><\/p>\n<ol id=\"x-ck12-ZDk2MzZhZTJjYzY0OTZhMDg2YmQzMTE1MGRlZDJkNTI.-zyx\">\n<li>What material has the highest vapor pressure at 25\u00b0C?<\/li>\n<li>What material has the lowest vapor pressure at 25\u00b0C?<\/li>\n<li>What device is used to measure vapor pressure?<\/li>\n<li>Does the surface area of the liquid affect the vapor pressure?<\/li>\n<\/ol>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Review<\/h3>\n<ol id=\"x-ck12-MDVlYmJhMDNhOWVkNGJmMWQyZmI0ZDNiMTg2YmZmYmY.-hk1\">\n<li>Define vapor pressure.<\/li>\n<li>How do intermolecular forces affect vapor pressure?<\/li>\n<li>How does temperature affect vapor pressure?<\/li>\n<\/ol>\n<\/div>\n<div class=\"x-ck12-data-problem-set\">\n<div class=\"textbox learning-objectives\">\n<h3>Glossary<\/h3>\n<div class=\"x-ck12-data-vocabulary\">\n<ul id=\"x-ck12-YmUwNmUwZWY5MmRkMGI1MDQzMWI2ZTNlMTQ2YWIzNGE.-vaj\">\n<li><strong>liquid phase: <\/strong>A substance in the liquid state of matter.<\/li>\n<li><strong>vapor phase: <\/strong>A substance in the gaseous state of matter.<\/li>\n<li><strong>vapor pressure: <\/strong>A measure of the force exerted by a gas above a liquid in a sealed container.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<\/div>\n","protected":false},"author":1507,"menu_order":10,"template":"","meta":{"_candela_citation":"[]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-2596","chapter","type-chapter","status-publish","hentry"],"part":2334,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2596","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/users\/1507"}],"version-history":[{"count":8,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2596\/revisions"}],"predecessor-version":[{"id":3606,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2596\/revisions\/3606"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/parts\/2334"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2596\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/media?parent=2596"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapter-type?post=2596"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/contributor?post=2596"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/license?post=2596"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}