{"id":7939,"date":"2021-06-08T21:58:13","date_gmt":"2021-06-08T21:58:13","guid":{"rendered":"https:\/\/opentextbc.ca\/introductorychemistry\/chapter\/factors-that-affect-the-rate-of-reactions\/"},"modified":"2021-10-25T22:42:57","modified_gmt":"2021-10-25T22:42:57","slug":"factors-that-affect-the-rate-of-reactions","status":"publish","type":"chapter","link":"https:\/\/opentextbc.ca\/introductorychemistry\/chapter\/factors-that-affect-the-rate-of-reactions\/","title":{"raw":"Factors that Affect the Rate of Reactions","rendered":"Factors that Affect the Rate of Reactions"},"content":{"raw":"<div class=\"textbox textbox--learning-objectives\"><header class=\"textbox__header\">\r\n<p class=\"textbox__title\">Learning Objectives<\/p>\r\n\r\n<\/header>\r\n<div class=\"textbox__content\">\r\n<ul>\r\n \t<li>To gain an understanding of collision theory.<\/li>\r\n \t<li>To gain an understanding of the four main factors that affect reaction rate.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<em>Reaction kinetics<\/em> is the study of the rate of chemical reactions, and reaction rates can vary greatly over a large range of time scales. Some reactions can proceed at explosively fast rates like the detonation of fireworks (Figure 17.1 \"Fireworks at Night Over River\"), while others can occur at a sluggish rate over many years like the rusting of barbed wire exposed to the elements (Figure 17.2 \"Rusted Barbed Wire\").\r\n\r\n[caption id=\"attachment_1031\" align=\"aligncenter\" width=\"250\"]<img class=\"wp-image-1031\" src=\"https:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2021\/06\/Fireworks_at_night_over_river-1.jpg\" alt=\"Fireworks explode in the night sky. A reflection of the fireworks is seen on water below.\" width=\"250\" height=\"68\" \/> Figure 17.1 \"Fireworks at Night Over River.\" The chemical reaction in fireworks happens at an explosive rate.[\/caption]\r\n\r\n[caption id=\"attachment_1032\" align=\"aligncenter\" width=\"321\"]<img class=\"wp-image-1032\" src=\"https:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2021\/06\/barbed-wire-1.jpg\" alt=\"A close-up of rusted barbed wire.\" width=\"321\" height=\"241\" \/> Figure 17.2 \"Rusted Barbed Wire.\" The rusting of barbed wire occurs over many years.[\/caption]\r\n<h1>Collision Theory<\/h1>\r\nTo understand the kinetics of chemical reactions, and the factors that affect kinetics, we should first examine what happens during a reaction on the molecular level. According to the <b>collision theory<\/b> of reactivity, reactions occur when reactant molecules \u201ceffectively collide.\u201d For an \u201ceffective collision\u201d to occur, the reactant molecules must be oriented in space correctly to facilitate the breaking and forming of bonds and the rearrangement of atoms that result in the formation of product molecules (see Figure 17.3 \u201cCollision Visualizations\u201d).\r\n\r\n[caption id=\"attachment_1033\" align=\"aligncenter\" width=\"420\"]<img class=\"wp-image-1033 \" src=\"https:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2021\/06\/Effective-collision-1.jpg\" alt=\"Visualization of an ineffective and effective collision based on molecular orientation.\" width=\"420\" height=\"210\" \/> Figure 17.3 \"Collision Visualizations.\" This visualization shows an ineffective and effective collision based on molecular orientation.[\/caption]\r\n\r\nDuring a molecular collision, molecules must also possess a minimum amount of kinetic energy for an effective collision to occur. This energy varies for each reaction, and is known as the <b>activation energy (<em>E<\/em><sub>a<\/sub>) <\/b>(Figure 17.4 \"Potential Energy and\u00a0Activation Energy\"). The rate of reaction therefore depends on the activation energy; a higher activation energy means that fewer\u00a0molecules will have sufficient energy to undergo an effective collision.\r\n\r\n[caption id=\"attachment_1034\" align=\"aligncenter\" width=\"363\"]<img class=\"wp-image-1034 size-full\" src=\"https:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2021\/06\/activation-energy-1-1.jpg\" alt=\"Potential energy diagram for a hypothetical reaction.\" width=\"363\" height=\"261\" \/> Figure 17.4 \"Potential\u00a0Energy and\u00a0Activation\u00a0Energy.\" This potential energy diagram shows the activation energy of a hypothetical reaction.[\/caption]\r\n<h1>Factors That Affect Rate<\/h1>\r\nThere are four main factors that can affect the reaction rate of a chemical reaction:\r\n<ol>\r\n \t<li><b>Reactant concentration.<\/b> Increasing the concentration of one or more reactants will often increase the rate of reaction. This occurs because a higher concentration of a reactant will lead to more collisions of that reactant in a specific time period.<\/li>\r\n \t<li><b>Physical state of the reactants and surface area.<\/b> If reactant molecules exist in different phases, as in a heterogeneous mixture, the rate of reaction will be limited by the surface area of the phases that\u00a0are in contact. For example, if a solid metal reactant and gas reactant are mixed, only the molecules present on the surface of the metal are able to collide with the gas molecules. Therefore, increasing the surface area of the metal by pounding it flat or cutting it into many pieces will increase its reaction rate.<\/li>\r\n \t<li><b>Temperature<\/b>. An increase in temperature typically increases the rate of reaction. An increase in temperature will raise the average kinetic energy of the reactant molecules. Therefore, a greater proportion of molecules will have the minimum energy necessary for an effective collision (Figure. 17.5 \"Temperature and\u00a0Reaction Rate\").\r\n\r\n[caption id=\"attachment_1035\" align=\"aligncenter\" width=\"334\"]<img class=\"wp-image-1035 size-full\" src=\"https:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2021\/06\/Temperature-and-Kinetic-Energy-Distribution-1.jpg\" alt=\"Figure 17.1-4. Effect of temperature on the kinetic energy distribution of molecules in a sample.\" width=\"334\" height=\"287\" \/> Figure 17.5 \"Temperature and Reaction Rate.\" Effect of temperature on the kinetic energy distribution of molecules in a sample[\/caption]<\/li>\r\n \t<li><b>Presence of a catalyst<\/b>. A <b>catalyst<\/b> is a substance that accelerates a reaction by participating in it without being consumed. Catalysts provide an alternate reaction pathway to obtain products. They are critical to many biochemical reactions. They will be examined further in the section \"Catalysis.\"<\/li>\r\n<\/ol>\r\n<div class=\"textbox textbox--key-takeaways\"><header class=\"textbox__header\">\r\n<p class=\"textbox__title\">Key Takeaways<\/p>\r\n\r\n<\/header>\r\n<div class=\"textbox__content\">\r\n<ul>\r\n \t<li>Reactions occur when two reactant molecules effectively collide, each having minimum\u00a0energy and correct orientation.<\/li>\r\n \t<li>Reactant concentration, the physical state of the reactants, and surface area, temperature, and the presence of a catalyst are the four main factors that affect reaction rate.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<h3>Media Attributions<\/h3>\r\n<ul>\r\n \t<li><a href=\"https:\/\/commons.wikimedia.org\/wiki\/File:Fireworks_at_night_over_river.jpg\">\u201cFireworks at night over river\u201d<\/a> \u00a9 Jon Sullivan is licensed under a <a href=\"https:\/\/creativecommons.org\/publicdomain\/mark\/1.0\/\">Public Domain<\/a> license<\/li>\r\n \t<li><a href=\"https:\/\/commons.wikimedia.org\/wiki\/File:Stacheldraht_93.jpg\">\u201cBarbed wire (rusting after years of hard work)\u201d<\/a> \u00a9 <a href=\"https:\/\/commons.wikimedia.org\/wiki\/User:Waugsberg\">2007 by Waugsberg<\/a> is licensed under a <a href=\"https:\/\/creativecommons.org\/licenses\/by-sa\/3.0\/deed.en\">CC BY-SA (Attribution-ShareAlike)<\/a> license<\/li>\r\n<\/ul>","rendered":"<div class=\"textbox textbox--learning-objectives\">\n<header class=\"textbox__header\">\n<p class=\"textbox__title\">Learning Objectives<\/p>\n<\/header>\n<div class=\"textbox__content\">\n<ul>\n<li>To gain an understanding of collision theory.<\/li>\n<li>To gain an understanding of the four main factors that affect reaction rate.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<p><em>Reaction kinetics<\/em> is the study of the rate of chemical reactions, and reaction rates can vary greatly over a large range of time scales. Some reactions can proceed at explosively fast rates like the detonation of fireworks (Figure 17.1 &#8220;Fireworks at Night Over River&#8221;), while others can occur at a sluggish rate over many years like the rusting of barbed wire exposed to the elements (Figure 17.2 &#8220;Rusted Barbed Wire&#8221;).<\/p>\n<figure id=\"attachment_1031\" aria-describedby=\"caption-attachment-1031\" style=\"width: 250px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" class=\"wp-image-1031\" src=\"https:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2021\/06\/Fireworks_at_night_over_river-1.jpg\" alt=\"Fireworks explode in the night sky. A reflection of the fireworks is seen on water below.\" width=\"250\" height=\"68\" \/><figcaption id=\"caption-attachment-1031\" class=\"wp-caption-text\">Figure 17.1 &#8220;Fireworks at Night Over River.&#8221; The chemical reaction in fireworks happens at an explosive rate.<\/figcaption><\/figure>\n<figure id=\"attachment_1032\" aria-describedby=\"caption-attachment-1032\" style=\"width: 321px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" class=\"wp-image-1032\" src=\"https:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2021\/06\/barbed-wire-1.jpg\" alt=\"A close-up of rusted barbed wire.\" width=\"321\" height=\"241\" \/><figcaption id=\"caption-attachment-1032\" class=\"wp-caption-text\">Figure 17.2 &#8220;Rusted Barbed Wire.&#8221; The rusting of barbed wire occurs over many years.<\/figcaption><\/figure>\n<h1>Collision Theory<\/h1>\n<p>To understand the kinetics of chemical reactions, and the factors that affect kinetics, we should first examine what happens during a reaction on the molecular level. According to the <b>collision theory<\/b> of reactivity, reactions occur when reactant molecules \u201ceffectively collide.\u201d For an \u201ceffective collision\u201d to occur, the reactant molecules must be oriented in space correctly to facilitate the breaking and forming of bonds and the rearrangement of atoms that result in the formation of product molecules (see Figure 17.3 \u201cCollision Visualizations\u201d).<\/p>\n<figure id=\"attachment_1033\" aria-describedby=\"caption-attachment-1033\" style=\"width: 420px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" class=\"wp-image-1033\" src=\"https:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2021\/06\/Effective-collision-1.jpg\" alt=\"Visualization of an ineffective and effective collision based on molecular orientation.\" width=\"420\" height=\"210\" \/><figcaption id=\"caption-attachment-1033\" class=\"wp-caption-text\">Figure 17.3 &#8220;Collision Visualizations.&#8221; This visualization shows an ineffective and effective collision based on molecular orientation.<\/figcaption><\/figure>\n<p>During a molecular collision, molecules must also possess a minimum amount of kinetic energy for an effective collision to occur. This energy varies for each reaction, and is known as the <b>activation energy (<em>E<\/em><sub>a<\/sub>) <\/b>(Figure 17.4 &#8220;Potential Energy and\u00a0Activation Energy&#8221;). The rate of reaction therefore depends on the activation energy; a higher activation energy means that fewer\u00a0molecules will have sufficient energy to undergo an effective collision.<\/p>\n<figure id=\"attachment_1034\" aria-describedby=\"caption-attachment-1034\" style=\"width: 363px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" class=\"wp-image-1034 size-full\" src=\"https:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2021\/06\/activation-energy-1-1.jpg\" alt=\"Potential energy diagram for a hypothetical reaction.\" width=\"363\" height=\"261\" \/><figcaption id=\"caption-attachment-1034\" class=\"wp-caption-text\">Figure 17.4 &#8220;Potential\u00a0Energy and\u00a0Activation\u00a0Energy.&#8221; This potential energy diagram shows the activation energy of a hypothetical reaction.<\/figcaption><\/figure>\n<h1>Factors That Affect Rate<\/h1>\n<p>There are four main factors that can affect the reaction rate of a chemical reaction:<\/p>\n<ol>\n<li><b>Reactant concentration.<\/b> Increasing the concentration of one or more reactants will often increase the rate of reaction. This occurs because a higher concentration of a reactant will lead to more collisions of that reactant in a specific time period.<\/li>\n<li><b>Physical state of the reactants and surface area.<\/b> If reactant molecules exist in different phases, as in a heterogeneous mixture, the rate of reaction will be limited by the surface area of the phases that\u00a0are in contact. For example, if a solid metal reactant and gas reactant are mixed, only the molecules present on the surface of the metal are able to collide with the gas molecules. Therefore, increasing the surface area of the metal by pounding it flat or cutting it into many pieces will increase its reaction rate.<\/li>\n<li><b>Temperature<\/b>. An increase in temperature typically increases the rate of reaction. An increase in temperature will raise the average kinetic energy of the reactant molecules. Therefore, a greater proportion of molecules will have the minimum energy necessary for an effective collision (Figure. 17.5 &#8220;Temperature and\u00a0Reaction Rate&#8221;).<br \/>\n<figure id=\"attachment_1035\" aria-describedby=\"caption-attachment-1035\" style=\"width: 334px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" class=\"wp-image-1035 size-full\" src=\"https:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2021\/06\/Temperature-and-Kinetic-Energy-Distribution-1.jpg\" alt=\"Figure 17.1-4. Effect of temperature on the kinetic energy distribution of molecules in a sample.\" width=\"334\" height=\"287\" \/><figcaption id=\"caption-attachment-1035\" class=\"wp-caption-text\">Figure 17.5 &#8220;Temperature and Reaction Rate.&#8221; Effect of temperature on the kinetic energy distribution of molecules in a sample<\/figcaption><\/figure>\n<\/li>\n<li><b>Presence of a catalyst<\/b>. A <b>catalyst<\/b> is a substance that accelerates a reaction by participating in it without being consumed. Catalysts provide an alternate reaction pathway to obtain products. They are critical to many biochemical reactions. They will be examined further in the section &#8220;Catalysis.&#8221;<\/li>\n<\/ol>\n<div class=\"textbox textbox--key-takeaways\">\n<header class=\"textbox__header\">\n<p class=\"textbox__title\">Key Takeaways<\/p>\n<\/header>\n<div class=\"textbox__content\">\n<ul>\n<li>Reactions occur when two reactant molecules effectively collide, each having minimum\u00a0energy and correct orientation.<\/li>\n<li>Reactant concentration, the physical state of the reactants, and surface area, temperature, and the presence of a catalyst are the four main factors that affect reaction rate.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<h3>Media Attributions<\/h3>\n<ul>\n<li><a href=\"https:\/\/commons.wikimedia.org\/wiki\/File:Fireworks_at_night_over_river.jpg\">\u201cFireworks at night over river\u201d<\/a> \u00a9 Jon Sullivan is licensed under a <a href=\"https:\/\/creativecommons.org\/publicdomain\/mark\/1.0\/\">Public Domain<\/a> license<\/li>\n<li><a href=\"https:\/\/commons.wikimedia.org\/wiki\/File:Stacheldraht_93.jpg\">\u201cBarbed wire (rusting after years of hard work)\u201d<\/a> \u00a9 <a href=\"https:\/\/commons.wikimedia.org\/wiki\/User:Waugsberg\">2007 by Waugsberg<\/a> is licensed under a <a href=\"https:\/\/creativecommons.org\/licenses\/by-sa\/3.0\/deed.en\">CC BY-SA (Attribution-ShareAlike)<\/a> license<\/li>\n<\/ul>\n","protected":false},"author":90,"menu_order":1,"template":"","meta":{"pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":["jessie-a-key"],"pb_section_license":"cc-by"},"chapter-type":[],"contributor":[49],"license":[54],"class_list":["post-7939","chapter","type-chapter","status-publish","hentry","contributor-jessie-a-key","license-cc-by"],"part":7933,"_links":{"self":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7939","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/users\/90"}],"version-history":[{"count":4,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7939\/revisions"}],"predecessor-version":[{"id":9014,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7939\/revisions\/9014"}],"part":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/parts\/7933"}],"metadata":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7939\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/media?parent=7939"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapter-type?post=7939"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/contributor?post=7939"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/license?post=7939"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}