{"id":705,"date":"2021-07-23T09:20:29","date_gmt":"2021-07-23T13:20:29","guid":{"rendered":"https:\/\/pressbooks.bccampus.ca\/aperrott\/chapter\/factors-affecting-reaction-rates\/"},"modified":"2022-06-23T09:16:21","modified_gmt":"2022-06-23T13:16:21","slug":"factors-affecting-reaction-rates","status":"publish","type":"chapter","link":"https:\/\/pressbooks.bccampus.ca\/aperrott\/chapter\/factors-affecting-reaction-rates\/","title":{"raw":"12.2 Factors Affecting Reaction Rates","rendered":"12.2 Factors Affecting Reaction Rates"},"content":{"raw":"<div class=\"textbox textbox--learning-objectives\">\r\n<h3><strong>Learning Objectives<\/strong><\/h3>\r\nBy the end of this section, you will be able to:\r\n<ul>\r\n \t<li>Describe the effects of chemical nature, physical state, temperature, concentration, and catalysis on reaction rates<\/li>\r\n<\/ul>\r\n<\/div>\r\n<p id=\"fs-idm233990000\">The rates at which reactants are consumed and products are formed during chemical reactions vary greatly. Five factors typically affecting the rates of chemical reactions will be explored in this section: the chemical nature of the reacting substances, the state of subdivision (one large lump versus many small particles) of the reactants, the temperature of the reactants, the concentration of the reactants, and the presence of a catalyst.<\/p>\r\n\r\n<div id=\"fs-idm58413648\" class=\"bc-section section\" data-depth=\"1\">\r\n<h3 data-type=\"title\"><strong>The Chemical Nature of the Reacting Substances<\/strong><\/h3>\r\n<p id=\"fs-idm103128016\">The rate of a reaction depends on the nature of the participating substances. Reactions that appear similar may have different rates under the same conditions, depending on the identity of the reactants. For example, when small pieces of the metals iron and sodium are exposed to air, the sodium reacts completely with air overnight, whereas the iron is barely affected. The active metals calcium and sodium both react with water to form hydrogen gas and a base. Yet calcium reacts at a moderate rate, whereas sodium reacts so rapidly that the reaction is almost explosive.<\/p>\r\n\r\n<\/div>\r\n<div id=\"fs-idm83714000\" class=\"bc-section section\" data-depth=\"1\">\r\n<h3 data-type=\"title\"><strong>The Physical States of the Reactants<\/strong><\/h3>\r\n<p id=\"fs-idm89852336\">A chemical reaction between two or more substances requires intimate contact between the reactants. When reactants are in different physical states, or phases (solid, liquid, gaseous, dissolved), the reaction takes place only at the interface between the phases. Consider the heterogeneous reaction between a solid phase and either a liquid or gaseous phase. Compared with the reaction rate for large solid particles, the rate for smaller particles will be greater because the surface area in contact with the other reactant phase is greater. For example, large pieces of iron react more slowly with acids than they do with finely divided iron powder (<a class=\"autogenerated-content\" href=\"#CNX_Chem_12_02_AcidDissol\">(Figure)<\/a>). Large pieces of wood smoulder, smaller pieces burn rapidly, and saw dust burns explosively.<\/p>\r\n&nbsp;\r\n<div id=\"CNX_Chem_12_02_AcidDissol\" class=\"scaled-down\">\r\n<div class=\"bc-figcaption figcaption\">(a) Iron powder reacts rapidly with dilute hydrochloric acid and produces bubbles of hydrogen gas: 2Fe(<em data-effect=\"italics\">s<\/em>) + 6HCl(<em data-effect=\"italics\">aq<\/em>) \u27f6 2FeCl<sub>3<\/sub>(<em data-effect=\"italics\">aq<\/em>) + 3H<sub>2<\/sub>(<em data-effect=\"italics\">g<\/em>). (b) An iron nail reacts more slowly because the surface area exposed to the acid is much less.<\/div>\r\n<span id=\"fs-idm108837008\" data-type=\"media\" data-alt=\"This figure shows two photos labeled (a) and (b). Photo (a) shows the bottom of a test tube. The test tube is filled with a dark gas, and there is a dark substance and bubbles in the bottom. Photo (b) shows a rod and bubbles in a test tube similar to photo (a), but the gas in the test tube is not as dark.\"><img src=\"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-content\/uploads\/sites\/1463\/2021\/07\/CNX_Chem_12_02_AcidDissol-2.jpg\" alt=\"This figure shows two photos labeled (a) and (b). Photo (a) shows the bottom of a test tube. The test tube is filled with a dark gas, and there is a dark substance and bubbles in the bottom. Photo (b) shows a rod and bubbles in a test tube similar to photo (a), but the gas in the test tube is not as dark.\" data-media-type=\"image\/jpeg\" \/><\/span>\r\n\r\n<\/div>\r\n<div id=\"fs-idm104157008\" class=\"chemistry link-to-learning\" data-type=\"note\">\r\n<p id=\"fs-idm33181984\">Watch <a href=\"http:\/\/openstaxcollege.org\/l\/16cesium\">this video<\/a> to see the reaction of cesium with water in slow motion and a discussion of how the state of reactants and particle size affect reaction rates.<\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idm100022464\" class=\"bc-section section\" data-depth=\"1\">\r\n<h3 data-type=\"title\"><strong>Temperature of the Reactants<\/strong><\/h3>\r\n<p id=\"fs-idp8529552\">Chemical reactions typically occur faster at higher temperatures. Food can spoil quickly when left on the kitchen counter. However, the lower temperature inside of a refrigerator slows that process so that the same food remains fresh for days. Gas burners, hot plates, and ovens are often used in the laboratory to increase the speed of reactions that proceed slowly at ordinary temperatures. For many chemical processes, reaction rates are approximately doubled when the temperature is raised by 10 \u00b0C.<\/p>\r\n\r\n<\/div>\r\n<div id=\"fs-idm145319392\" class=\"bc-section section\" data-depth=\"1\">\r\n<h3 data-type=\"title\"><strong>Concentrations of the Reactants<\/strong><\/h3>\r\n<p id=\"fs-idm31855392\">The rates of many reactions depend on the concentrations of the reactants. Rates usually increase when the concentration of one or more of the reactants increases. For example, calcium carbonate (CaCO<sub>3<\/sub>) deteriorates as a result of its reaction with the pollutant sulfur dioxide. The rate of this reaction depends on the amount of sulfur dioxide in the air (<a class=\"autogenerated-content\" href=\"#CNX_Chem_12_02_NYSStatue\">(Figure)<\/a>). An acidic oxide, sulfur dioxide combines with water vapor in the air to produce sulfurous acid in the following reaction:<\/p>\r\n\r\n<div id=\"fs-idm37870480\" style=\"text-align: center\" data-type=\"equation\">SO<sub>2<\/sub>(<em>g<\/em>) + H<sub>2<\/sub>O(<em>g<\/em>) \u27f6H<sub>2<\/sub>SO<sub>3<\/sub>(<em>aq<\/em>)<\/div>\r\n<p id=\"fs-idp125234816\">Calcium carbonate reacts with sulfurous acid as follows:<\/p>\r\n\r\n<div id=\"fs-idp86192224\" style=\"text-align: center\" data-type=\"equation\">CaCO<sub>3<\/sub>(<em>s<\/em>) + H<sub>2<\/sub>SO<sub>3<\/sub>(<em>aq<\/em>) \u27f6CaSO<sub>3<\/sub>(<em>aq<\/em>) + CO<sub>2<\/sub>(<em>g<\/em>) + H<sub>2<\/sub>O(<em>l<\/em>)<\/div>\r\n<p id=\"fs-idm233971872\">In a polluted atmosphere where the concentration of sulfur dioxide is high, calcium carbonate deteriorates more rapidly than in less polluted air. Similarly, phosphorus burns much more rapidly in an atmosphere of pure oxygen than in air, which is only about 20% oxygen.<\/p>\r\n&nbsp;\r\n<div id=\"CNX_Chem_12_02_NYSStatue\" class=\"scaled-down\">\r\n<div class=\"bc-figcaption figcaption\">Statues made from carbonate compounds such as limestone and marble typically weather slowly over time due to the actions of water, and thermal expansion and contraction. However, pollutants like sulfur dioxide can accelerate weathering. As the concentration of air pollutants increases, deterioration of limestone occurs more rapidly. (credit: James P Fisher III)<\/div>\r\n<span id=\"fs-idm66889568\" data-type=\"media\" data-alt=\"A photograph is shown of an angel statue. While some details of the statue, including facial features, are present, effects of weathering appear to be diminishing these features.\"><img src=\"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-content\/uploads\/sites\/1463\/2021\/07\/CNX_Chem_12_02_NYSStatue-2.jpg\" alt=\"A photograph is shown of an angel statue. While some details of the statue, including facial features, are present, effects of weathering appear to be diminishing these features.\" data-media-type=\"image\/jpeg\" \/><\/span>\r\n\r\n<\/div>\r\n<div id=\"fs-idp91411184\" class=\"chemistry link-to-learning\" data-type=\"note\">\r\n\r\n&nbsp;\r\n<p id=\"fs-idm30692176\">Phosphorous burns rapidly in air, but it will burn even more rapidly if the concentration of oxygen is higher. Watch this <a href=\"http:\/\/openstaxcollege.org\/l\/16phosphor\">video<\/a> to see an example.<\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idm33945488\" class=\"bc-section section\" data-depth=\"1\">\r\n<h3 data-type=\"title\"><strong>The Presence of a Catalyst<\/strong><\/h3>\r\n<p id=\"fs-idm99481872\">Relatively dilute aqueous solutions of hydrogen peroxide, H<sub>2<\/sub>O<sub>2<\/sub>, are commonly used as topical antiseptics. Hydrogen peroxide decomposes to yield water and oxygen gas according to the equation:<\/p>\r\n\r\n<div id=\"fs-idm641705824\" style=\"text-align: center\" data-type=\"equation\">2H<sub>2<\/sub>O<sub>2<\/sub>(<em>aq<\/em>) \u27f6 2H<sub>2<\/sub>O(<em>l<\/em>) + O<sub>2<\/sub>(<em>g<\/em>)<\/div>\r\n<p id=\"fs-idm237313312\">Under typical conditions, this decomposition occurs very slowly. When dilute H<sub>2<\/sub>O<sub>2<\/sub>(<em>aq<\/em>) is poured onto an open wound, however, the reaction occurs rapidly and the solution foams because of the vigorous production of oxygen gas. This dramatic difference is caused by the presence of substances within the wound\u2019s exposed tissues that accelerate the decomposition process. Substances that function to increase the rate of a reaction are called <strong>catalysts<\/strong>, a topic treated in greater detail later in this chapter.<\/p>\r\n&nbsp;\r\n<div id=\"fs-idm166887552\" class=\"chemistry link-to-learning\" data-type=\"note\">\r\n<p id=\"fs-idm89663808\">Chemical reactions occur when molecules collide with each other and undergo a chemical transformation. Before physically performing a reaction in a laboratory, scientists can use molecular modeling simulations to predict how the parameters discussed earlier will influence the rate of a reaction. Use the <a href=\"http:\/\/openstaxcollege.org\/l\/16PHETreaction\">PhET Reactions &amp; Rates interactive<\/a> to explore how temperature, concentration, and the nature of the reactants affect reaction rates.<\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idm70094032\" class=\"summary\" data-depth=\"1\">\r\n<h3 data-type=\"title\"><strong>Key Concepts and Summary<\/strong><\/h3>\r\n<p id=\"fs-idm63455008\">The rate of a chemical reaction is affected by several parameters. Reactions involving two phases proceed more rapidly when there is greater surface area contact. If temperature or reactant concentration is increased, the rate of a given reaction generally increases as well. A catalyst can increase the rate of a reaction.<\/p>\r\n\r\n<\/div>\r\n<div id=\"fs-idm87447680\" class=\"exercises\" data-depth=\"1\">\r\n<div id=\"fs-idm49710224\" data-type=\"exercise\">\r\n<div id=\"fs-idm123636848\" data-type=\"solution\">\r\n<p id=\"fs-idm111616960\"><\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox shaded\" data-type=\"glossary\">\r\n<h3 data-type=\"glossary-title\"><strong>Glossary<\/strong><\/h3>\r\n<dl id=\"fs-idp102379584\">\r\n \t<dt>catalyst<\/dt>\r\n \t<dd id=\"fs-idm32337456\">substance that increases the rate of a reaction without itself being consumed by the reaction<\/dd>\r\n<\/dl>\r\n<\/div>","rendered":"<div class=\"textbox textbox--learning-objectives\">\n<h3><strong>Learning Objectives<\/strong><\/h3>\n<p>By the end of this section, you will be able to:<\/p>\n<ul>\n<li>Describe the effects of chemical nature, physical state, temperature, concentration, and catalysis on reaction rates<\/li>\n<\/ul>\n<\/div>\n<p id=\"fs-idm233990000\">The rates at which reactants are consumed and products are formed during chemical reactions vary greatly. Five factors typically affecting the rates of chemical reactions will be explored in this section: the chemical nature of the reacting substances, the state of subdivision (one large lump versus many small particles) of the reactants, the temperature of the reactants, the concentration of the reactants, and the presence of a catalyst.<\/p>\n<div id=\"fs-idm58413648\" class=\"bc-section section\" data-depth=\"1\">\n<h3 data-type=\"title\"><strong>The Chemical Nature of the Reacting Substances<\/strong><\/h3>\n<p id=\"fs-idm103128016\">The rate of a reaction depends on the nature of the participating substances. Reactions that appear similar may have different rates under the same conditions, depending on the identity of the reactants. For example, when small pieces of the metals iron and sodium are exposed to air, the sodium reacts completely with air overnight, whereas the iron is barely affected. The active metals calcium and sodium both react with water to form hydrogen gas and a base. Yet calcium reacts at a moderate rate, whereas sodium reacts so rapidly that the reaction is almost explosive.<\/p>\n<\/div>\n<div id=\"fs-idm83714000\" class=\"bc-section section\" data-depth=\"1\">\n<h3 data-type=\"title\"><strong>The Physical States of the Reactants<\/strong><\/h3>\n<p id=\"fs-idm89852336\">A chemical reaction between two or more substances requires intimate contact between the reactants. When reactants are in different physical states, or phases (solid, liquid, gaseous, dissolved), the reaction takes place only at the interface between the phases. Consider the heterogeneous reaction between a solid phase and either a liquid or gaseous phase. Compared with the reaction rate for large solid particles, the rate for smaller particles will be greater because the surface area in contact with the other reactant phase is greater. For example, large pieces of iron react more slowly with acids than they do with finely divided iron powder (<a class=\"autogenerated-content\" href=\"#CNX_Chem_12_02_AcidDissol\">(Figure)<\/a>). Large pieces of wood smoulder, smaller pieces burn rapidly, and saw dust burns explosively.<\/p>\n<p>&nbsp;<\/p>\n<div id=\"CNX_Chem_12_02_AcidDissol\" class=\"scaled-down\">\n<div class=\"bc-figcaption figcaption\">(a) Iron powder reacts rapidly with dilute hydrochloric acid and produces bubbles of hydrogen gas: 2Fe(<em data-effect=\"italics\">s<\/em>) + 6HCl(<em data-effect=\"italics\">aq<\/em>) \u27f6 2FeCl<sub>3<\/sub>(<em data-effect=\"italics\">aq<\/em>) + 3H<sub>2<\/sub>(<em data-effect=\"italics\">g<\/em>). (b) An iron nail reacts more slowly because the surface area exposed to the acid is much less.<\/div>\n<p><span id=\"fs-idm108837008\" data-type=\"media\" data-alt=\"This figure shows two photos labeled (a) and (b). Photo (a) shows the bottom of a test tube. The test tube is filled with a dark gas, and there is a dark substance and bubbles in the bottom. Photo (b) shows a rod and bubbles in a test tube similar to photo (a), but the gas in the test tube is not as dark.\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-content\/uploads\/sites\/1463\/2021\/07\/CNX_Chem_12_02_AcidDissol-2.jpg\" alt=\"This figure shows two photos labeled (a) and (b). Photo (a) shows the bottom of a test tube. The test tube is filled with a dark gas, and there is a dark substance and bubbles in the bottom. Photo (b) shows a rod and bubbles in a test tube similar to photo (a), but the gas in the test tube is not as dark.\" data-media-type=\"image\/jpeg\" \/><\/span><\/p>\n<\/div>\n<div id=\"fs-idm104157008\" class=\"chemistry link-to-learning\" data-type=\"note\">\n<p id=\"fs-idm33181984\">Watch <a href=\"http:\/\/openstaxcollege.org\/l\/16cesium\">this video<\/a> to see the reaction of cesium with water in slow motion and a discussion of how the state of reactants and particle size affect reaction rates.<\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idm100022464\" class=\"bc-section section\" data-depth=\"1\">\n<h3 data-type=\"title\"><strong>Temperature of the Reactants<\/strong><\/h3>\n<p id=\"fs-idp8529552\">Chemical reactions typically occur faster at higher temperatures. Food can spoil quickly when left on the kitchen counter. However, the lower temperature inside of a refrigerator slows that process so that the same food remains fresh for days. Gas burners, hot plates, and ovens are often used in the laboratory to increase the speed of reactions that proceed slowly at ordinary temperatures. For many chemical processes, reaction rates are approximately doubled when the temperature is raised by 10 \u00b0C.<\/p>\n<\/div>\n<div id=\"fs-idm145319392\" class=\"bc-section section\" data-depth=\"1\">\n<h3 data-type=\"title\"><strong>Concentrations of the Reactants<\/strong><\/h3>\n<p id=\"fs-idm31855392\">The rates of many reactions depend on the concentrations of the reactants. Rates usually increase when the concentration of one or more of the reactants increases. For example, calcium carbonate (CaCO<sub>3<\/sub>) deteriorates as a result of its reaction with the pollutant sulfur dioxide. The rate of this reaction depends on the amount of sulfur dioxide in the air (<a class=\"autogenerated-content\" href=\"#CNX_Chem_12_02_NYSStatue\">(Figure)<\/a>). An acidic oxide, sulfur dioxide combines with water vapor in the air to produce sulfurous acid in the following reaction:<\/p>\n<div id=\"fs-idm37870480\" style=\"text-align: center\" data-type=\"equation\">SO<sub>2<\/sub>(<em>g<\/em>) + H<sub>2<\/sub>O(<em>g<\/em>) \u27f6H<sub>2<\/sub>SO<sub>3<\/sub>(<em>aq<\/em>)<\/div>\n<p id=\"fs-idp125234816\">Calcium carbonate reacts with sulfurous acid as follows:<\/p>\n<div id=\"fs-idp86192224\" style=\"text-align: center\" data-type=\"equation\">CaCO<sub>3<\/sub>(<em>s<\/em>) + H<sub>2<\/sub>SO<sub>3<\/sub>(<em>aq<\/em>) \u27f6CaSO<sub>3<\/sub>(<em>aq<\/em>) + CO<sub>2<\/sub>(<em>g<\/em>) + H<sub>2<\/sub>O(<em>l<\/em>)<\/div>\n<p id=\"fs-idm233971872\">In a polluted atmosphere where the concentration of sulfur dioxide is high, calcium carbonate deteriorates more rapidly than in less polluted air. Similarly, phosphorus burns much more rapidly in an atmosphere of pure oxygen than in air, which is only about 20% oxygen.<\/p>\n<p>&nbsp;<\/p>\n<div id=\"CNX_Chem_12_02_NYSStatue\" class=\"scaled-down\">\n<div class=\"bc-figcaption figcaption\">Statues made from carbonate compounds such as limestone and marble typically weather slowly over time due to the actions of water, and thermal expansion and contraction. However, pollutants like sulfur dioxide can accelerate weathering. As the concentration of air pollutants increases, deterioration of limestone occurs more rapidly. (credit: James P Fisher III)<\/div>\n<p><span id=\"fs-idm66889568\" data-type=\"media\" data-alt=\"A photograph is shown of an angel statue. While some details of the statue, including facial features, are present, effects of weathering appear to be diminishing these features.\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-content\/uploads\/sites\/1463\/2021\/07\/CNX_Chem_12_02_NYSStatue-2.jpg\" alt=\"A photograph is shown of an angel statue. While some details of the statue, including facial features, are present, effects of weathering appear to be diminishing these features.\" data-media-type=\"image\/jpeg\" \/><\/span><\/p>\n<\/div>\n<div id=\"fs-idp91411184\" class=\"chemistry link-to-learning\" data-type=\"note\">\n<p>&nbsp;<\/p>\n<p id=\"fs-idm30692176\">Phosphorous burns rapidly in air, but it will burn even more rapidly if the concentration of oxygen is higher. Watch this <a href=\"http:\/\/openstaxcollege.org\/l\/16phosphor\">video<\/a> to see an example.<\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idm33945488\" class=\"bc-section section\" data-depth=\"1\">\n<h3 data-type=\"title\"><strong>The Presence of a Catalyst<\/strong><\/h3>\n<p id=\"fs-idm99481872\">Relatively dilute aqueous solutions of hydrogen peroxide, H<sub>2<\/sub>O<sub>2<\/sub>, are commonly used as topical antiseptics. Hydrogen peroxide decomposes to yield water and oxygen gas according to the equation:<\/p>\n<div id=\"fs-idm641705824\" style=\"text-align: center\" data-type=\"equation\">2H<sub>2<\/sub>O<sub>2<\/sub>(<em>aq<\/em>) \u27f6 2H<sub>2<\/sub>O(<em>l<\/em>) + O<sub>2<\/sub>(<em>g<\/em>)<\/div>\n<p id=\"fs-idm237313312\">Under typical conditions, this decomposition occurs very slowly. When dilute H<sub>2<\/sub>O<sub>2<\/sub>(<em>aq<\/em>) is poured onto an open wound, however, the reaction occurs rapidly and the solution foams because of the vigorous production of oxygen gas. This dramatic difference is caused by the presence of substances within the wound\u2019s exposed tissues that accelerate the decomposition process. Substances that function to increase the rate of a reaction are called <strong>catalysts<\/strong>, a topic treated in greater detail later in this chapter.<\/p>\n<p>&nbsp;<\/p>\n<div id=\"fs-idm166887552\" class=\"chemistry link-to-learning\" data-type=\"note\">\n<p id=\"fs-idm89663808\">Chemical reactions occur when molecules collide with each other and undergo a chemical transformation. Before physically performing a reaction in a laboratory, scientists can use molecular modeling simulations to predict how the parameters discussed earlier will influence the rate of a reaction. Use the <a href=\"http:\/\/openstaxcollege.org\/l\/16PHETreaction\">PhET Reactions &amp; Rates interactive<\/a> to explore how temperature, concentration, and the nature of the reactants affect reaction rates.<\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idm70094032\" class=\"summary\" data-depth=\"1\">\n<h3 data-type=\"title\"><strong>Key Concepts and Summary<\/strong><\/h3>\n<p id=\"fs-idm63455008\">The rate of a chemical reaction is affected by several parameters. Reactions involving two phases proceed more rapidly when there is greater surface area contact. If temperature or reactant concentration is increased, the rate of a given reaction generally increases as well. A catalyst can increase the rate of a reaction.<\/p>\n<\/div>\n<div id=\"fs-idm87447680\" class=\"exercises\" data-depth=\"1\">\n<div id=\"fs-idm49710224\" data-type=\"exercise\">\n<div id=\"fs-idm123636848\" data-type=\"solution\">\n<p id=\"fs-idm111616960\">\n<\/div>\n<\/div>\n<\/div>\n<div class=\"textbox shaded\" data-type=\"glossary\">\n<h3 data-type=\"glossary-title\"><strong>Glossary<\/strong><\/h3>\n<dl id=\"fs-idp102379584\">\n<dt>catalyst<\/dt>\n<dd id=\"fs-idm32337456\">substance that increases the rate of a reaction without itself being consumed by the reaction<\/dd>\n<\/dl>\n<\/div>\n","protected":false},"author":1392,"menu_order":3,"template":"","meta":{"pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[48],"contributor":[],"license":[],"class_list":["post-705","chapter","type-chapter","status-publish","hentry","chapter-type-numberless"],"part":695,"_links":{"self":[{"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/pressbooks\/v2\/chapters\/705","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/wp\/v2\/users\/1392"}],"version-history":[{"count":5,"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/pressbooks\/v2\/chapters\/705\/revisions"}],"predecessor-version":[{"id":2160,"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/pressbooks\/v2\/chapters\/705\/revisions\/2160"}],"part":[{"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/pressbooks\/v2\/parts\/695"}],"metadata":[{"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/pressbooks\/v2\/chapters\/705\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/wp\/v2\/media?parent=705"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/pressbooks\/v2\/chapter-type?post=705"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/wp\/v2\/contributor?post=705"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/wp\/v2\/license?post=705"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}