{"id":4088,"date":"2025-03-03T13:17:16","date_gmt":"2025-03-03T13:17:16","guid":{"rendered":"https:\/\/schools.jove.com\/?p=4088"},"modified":"2026-07-23T16:43:52","modified_gmt":"2026-07-23T16:43:52","slug":"reaction-rate-experiments-for-high-school-chemistry-students","status":"publish","type":"post","link":"https:\/\/schools.jove.com\/reaction-rate-experiments-for-high-school-chemistry-students\/","title":{"rendered":"Investigating Catalysts and Reaction Rates with High School Chemistry Labs"},"content":{"rendered":"\t\t<div data-elementor-type=\"wp-post\" data-elementor-id=\"4088\" class=\"elementor elementor-4088\" data-elementor-post-type=\"post\">\n\t\t\t\t<div class=\"elementor-element elementor-element-ef3dc91 e-flex e-con-boxed e-con e-parent\" data-id=\"ef3dc91\" data-element_type=\"container\" data-e-type=\"container\">\n\t\t\t\t\t<div class=\"e-con-inner\">\n\t\t\t\t<div class=\"elementor-element elementor-element-081d7dd elementor-widget elementor-widget-heading\" data-id=\"081d7dd\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"heading.default\">\n\t\t\t\t\t<h1 class=\"elementor-heading-title elementor-size-default\">Investigating Catalysts and Reaction Rates with High School Chemistry Labs\n<\/h1>\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t<div class=\"elementor-element elementor-element-7090152 e-flex e-con-boxed e-con e-parent\" data-id=\"7090152\" data-element_type=\"container\" data-e-type=\"container\">\n\t\t\t\t\t<div class=\"e-con-inner\">\n\t\t\t\t<div class=\"elementor-element elementor-element-44ee0c2 elementor-widget elementor-widget-text-editor\" data-id=\"44ee0c2\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"text-editor.default\">\n\t\t\t\t\t\t\t\t\t<p><span style=\"font-weight: 400;\">Why do some reactions take seconds while others take years? From rusting iron to digesting food, reaction rates influence nearly everything in our world. In high school chemistry, teaching students about <\/span><a href=\"https:\/\/www.jove.com\/schools\/v\/11383\/catalysis-homogenious-and-heterogeneous-catalysis\"><span style=\"font-weight: 400;\">catalysts<\/span><\/a><span style=\"font-weight: 400;\"> and<\/span><a href=\"https:\/\/www.jove.com\/schools\/v\/11374\/experimental-techniques-to-measure-reaction-rates\"><span style=\"font-weight: 400;\"> reaction rates<\/span><\/a><span style=\"font-weight: 400;\"> can be challenging without real-world examples. Hands-on experiments help bridge this gap, making chemical kinetics visual and interactive.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">Studies have demonstrated that incorporating hands-on practical activities in chemistry education significantly enhances students&#8217; engagement and academic performance. For instance, research involving senior high school students revealed that those participating in hands-on experiments showed improved understanding and retention of chemical concepts compared to traditional teaching methods.(<\/span><a href=\"https:\/\/www.ajol.info\/index.php\/ajesms\/article\/view\/261605\"><span style=\"font-weight: 400;\">Source<\/span><\/a><span style=\"font-weight: 400;\">)<\/span><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t<div class=\"elementor-element elementor-element-df603ce e-flex e-con-boxed e-con e-parent\" data-id=\"df603ce\" data-element_type=\"container\" data-e-type=\"container\">\n\t\t\t\t\t<div class=\"e-con-inner\">\n\t\t\t\t<div class=\"elementor-element elementor-element-dead711 elementor-widget elementor-widget-heading\" data-id=\"dead711\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"heading.default\">\n\t\t\t\t\t<h2 class=\"elementor-heading-title elementor-size-default\">The Importance of Understanding Reaction Rates and Catalysts<\/h2>\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t<div class=\"elementor-element elementor-element-1b91fc0 e-flex e-con-boxed e-con e-parent\" data-id=\"1b91fc0\" data-element_type=\"container\" data-e-type=\"container\">\n\t\t\t\t\t<div class=\"e-con-inner\">\n\t\t\t\t<div class=\"elementor-element elementor-element-fe49ccd elementor-widget elementor-widget-text-editor\" data-id=\"fe49ccd\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"text-editor.default\">\n\t\t\t\t\t\t\t\t\t<p><a href=\"https:\/\/www.jove.com\/science-education-library\/859\"><span style=\"font-weight: 400;\">Chemical kinetics<\/span><\/a><span style=\"font-weight: 400;\"> is a fundamental topic in chemistry that explains:<\/span><span style=\"font-weight: 400;\"><br \/><\/span><span style=\"font-weight: 400;\">\u2714 Why temperature, concentration, and surface area affect reaction speed<\/span><span style=\"font-weight: 400;\"><br \/><\/span><span style=\"font-weight: 400;\">\u2714 How catalysts accelerate reactions without being consumed<\/span><span style=\"font-weight: 400;\"><br \/><\/span><span style=\"font-weight: 400;\">\u2714 Real-world applications in biology, medicine, and industry<\/span><\/p>\n<p><span style=\"font-weight: 400;\">By conducting simple experiments, students can visualize reaction rates in action and understand why catalysts play a crucial role in <\/span><a href=\"https:\/\/www.jove.com\/schools\/v\/10662\/chemical-reactions-and-balanced-chemical-equations\"><span style=\"font-weight: 400;\">chemical reactions.<\/span><\/a><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t<div class=\"elementor-element elementor-element-a7775cb e-flex e-con-boxed e-con e-parent\" data-id=\"a7775cb\" data-element_type=\"container\" data-e-type=\"container\">\n\t\t\t\t\t<div class=\"e-con-inner\">\n\t\t\t\t<div class=\"elementor-element elementor-element-662806e elementor-widget elementor-widget-heading\" data-id=\"662806e\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"heading.default\">\n\t\t\t\t\t<h2 class=\"elementor-heading-title elementor-size-default\">Hands-On Experiments to Explore Reaction Rates and Catalysts\n<\/h2>\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t<div class=\"elementor-element elementor-element-6a438df e-flex e-con-boxed e-con e-parent\" data-id=\"6a438df\" data-element_type=\"container\" data-e-type=\"container\">\n\t\t\t\t\t<div class=\"e-con-inner\">\n\t\t\t\t<div class=\"elementor-element elementor-element-8092747 elementor-widget elementor-widget-text-editor\" data-id=\"8092747\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"text-editor.default\">\n\t\t\t\t\t\t\t\t\t<p><span style=\"font-weight: 400;\">Chemical reactions don\u2019t just happen\u2014they depend on factors like surface area, temperature, and catalysts. These hands-on experiments allow students to see reaction rates in action and understand how small changes can make a big impact on chemical processes.<\/span><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t<div class=\"elementor-element elementor-element-74827bf e-flex e-con-boxed e-con e-parent\" data-id=\"74827bf\" data-element_type=\"container\" data-e-type=\"container\">\n\t\t\t\t\t<div class=\"e-con-inner\">\n\t\t\t\t<div class=\"elementor-element elementor-element-cab91e1 elementor-widget elementor-widget-heading\" data-id=\"cab91e1\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"heading.default\">\n\t\t\t\t\t<h3 class=\"elementor-heading-title elementor-size-default\">1. Investigating the Effect of Surface Area on Reaction Speed\n<\/h3>\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t<div class=\"elementor-element elementor-element-bd34933 e-flex e-con-boxed e-con e-parent\" data-id=\"bd34933\" data-element_type=\"container\" data-e-type=\"container\">\n\t\t\t\t\t<div class=\"e-con-inner\">\n\t\t\t\t<div class=\"elementor-element elementor-element-406e770 elementor-widget elementor-widget-text-editor\" data-id=\"406e770\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"text-editor.default\">\n\t\t\t\t\t\t\t\t\t<p><b>Objective:<\/b><span style=\"font-weight: 400;\"> Demonstrate how increasing surface area affects reaction rates.<\/span><\/p>\n<p><b>Materials Needed:<\/b><\/p>\n<ul>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Alka-Seltzer tablets<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Water<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Beakers<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Stopwatch<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Mortar and pestle (or a spoon to crush tablets)<\/span><\/li>\n<\/ul>\n<p><b>Procedure:<\/b><\/p>\n<ol>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Drop a whole Alka-Seltzer tablet into a beaker of water and time the reaction.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Crush another tablet into powder, add it to water, and measure how quickly it dissolves.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Compare the reaction speeds between the two setups.<\/span><\/li>\n<\/ol>\n<p><b>Scientific Explanation:<\/b><b><br \/><\/b><span style=\"font-weight: 400;\">Crushing the tablet increases surface area, exposing more reactant particles to water, which accelerates the reaction. This illustrates the collision theory, which states that more frequent collisions lead to faster reactions.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">\ud83d\udccc Reinforce this concept with <\/span><a href=\"https:\/\/www.jove.com\/science-education-library\/859\/chemical-kinetics\"><span style=\"font-weight: 400;\">JoVE\u2019s Chemical Kinetics Videos<\/span><\/a><span style=\"font-weight: 400;\">, which visually explains reaction rates and surface area effects.<\/span><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t<div class=\"elementor-element elementor-element-81fc225 elementor-widget elementor-widget-heading\" data-id=\"81fc225\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"heading.default\">\n\t\t\t\t\t<h3 class=\"elementor-heading-title elementor-size-default\">2. Exploring Catalysts with Hydrogen Peroxide Decomposition\n<\/h3>\t\t\t\t<\/div>\n\t\t\t\t<div class=\"elementor-element elementor-element-9d8b61e elementor-widget elementor-widget-text-editor\" data-id=\"9d8b61e\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"text-editor.default\">\n\t\t\t\t\t\t\t\t\t<p><b>Objective:<\/b><span style=\"font-weight: 400;\"> Show how catalysts speed up decomposition reactions.<\/span><\/p>\n<p><b>Materials Needed:<\/b><\/p>\n<ul>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Hydrogen peroxide (H\u2082O\u2082)<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Yeast or potassium iodide (as catalysts)<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Dish soap<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Food coloring (optional)<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Beaker<\/span><\/li>\n<\/ul>\n<p><b>Procedure:<\/b><\/p>\n<ol>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Pour hydrogen peroxide into a beaker and add a few drops of dish soap.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Add yeast (or potassium iodide) and observe the rapid production of foam.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Discuss how the catalyst affects the reaction.<\/span><\/li>\n<\/ol>\n<p><b>Scientific Explanation:<\/b><b><br \/><\/b><span style=\"font-weight: 400;\">Hydrogen peroxide naturally decomposes into water and oxygen very slowly. However, catalysts like yeast (which contains the enzyme catalase) speed up the reaction dramatically, causing an exothermic reaction that produces visible bubbles.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">\ud83d\udccc For a step-by-step demonstration, watch JoVE\u2019s <\/span><a href=\"https:\/\/www.jove.com\/schools\/v\/11383\/catalysis-homogenious-and-heterogeneous-catalysis\"><span style=\"font-weight: 400;\">Catalysis<\/span><\/a><span style=\"font-weight: 400;\"> and <\/span><a href=\"https:\/\/www.jove.com\/schools\/v\/11374\/experimental-techniques-to-measure-reaction-rates\"><span style=\"font-weight: 400;\">Reaction Rates<\/span><\/a><span style=\"font-weight: 400;\"> Video to understand how catalysts affect chemical reactions.<\/span><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t<div class=\"elementor-element elementor-element-ef58dab e-flex e-con-boxed e-con e-parent\" data-id=\"ef58dab\" data-element_type=\"container\" data-e-type=\"container\">\n\t\t\t\t\t<div class=\"e-con-inner\">\n\t\t\t\t<div class=\"elementor-element elementor-element-b251fc7 elementor-widget elementor-widget-heading\" data-id=\"b251fc7\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"heading.default\">\n\t\t\t\t\t<h3 class=\"elementor-heading-title elementor-size-default\">3. Measuring the Effect of Temperature on Reaction Rate\n<\/h3>\t\t\t\t<\/div>\n\t\t\t\t<div class=\"elementor-element elementor-element-fa9ce94 elementor-widget elementor-widget-text-editor\" data-id=\"fa9ce94\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"text-editor.default\">\n\t\t\t\t\t\t\t\t\t<p><b>Objective:<\/b><span style=\"font-weight: 400;\"> Observe how temperature influences reaction speed.<\/span><\/p>\n<p><b>Materials Needed:<\/b><\/p>\n<ul>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Sodium thiosulfate (Na\u2082S\u2082O\u2083) solution<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Hydrochloric acid (HCl)<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Beakers<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Hot and cold water baths<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Stopwatch<\/span><\/li>\n<\/ul>\n<p><b>Procedure:<\/b><\/p>\n<ol>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Place beakers of sodium thiosulfate in <\/span><b>hot, room temperature, and cold<\/b><span style=\"font-weight: 400;\"> water baths.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Add hydrochloric acid and time how long it takes for a <\/span><b>cloudy precipitate<\/b><span style=\"font-weight: 400;\"> to form.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Compare reaction speeds across different temperatures.<\/span><\/li>\n<\/ol>\n<p><b>Scientific Explanation:<\/b><b><br \/><\/b><span style=\"font-weight: 400;\">Higher temperatures increase the kinetic energy of molecules, leading to more frequent and forceful collisions, which accelerates the reaction. Conversely, cooler temperatures slow down particle movement, reducing reaction speed.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">\ud83d\udccc Explore<\/span><a href=\"https:\/\/www.jove.com\/science-education-library\/97415\/temperature-and-heat\"><span style=\"font-weight: 400;\"> temperature<\/span><\/a><span style=\"font-weight: 400;\"> and reaction kinetics further with JoVE\u2019s <\/span><a href=\"https:\/\/www.jove.com\/science-education-library\/859\/chemical-kinetics\"><span style=\"font-weight: 400;\">Kinetics <\/span><\/a><span style=\"font-weight: 400;\">and <\/span><a href=\"https:\/\/www.jove.com\/schools\/v\/11697\/rate-laws-and-reaction-orders\"><span style=\"font-weight: 400;\">Rate Laws<\/span><\/a><span style=\"font-weight: 400;\"> Video.<\/span><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t<div class=\"elementor-element elementor-element-d80cff1 elementor-widget elementor-widget-heading\" data-id=\"d80cff1\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"heading.default\">\n\t\t\t\t\t<h2 class=\"elementor-heading-title elementor-size-default\">Enhancing Learning with JoVE Chemistry Videos\n<\/h2>\t\t\t\t<\/div>\n\t\t\t\t<div class=\"elementor-element elementor-element-e54538d elementor-widget elementor-widget-text-editor\" data-id=\"e54538d\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"text-editor.default\">\n\t\t\t\t\t\t\t\t\t<p><span style=\"font-weight: 400;\">While hands-on experiments provide direct experience, visual demonstrations enhance understanding. <\/span><a href=\"https:\/\/www.jove.com\/schools\"><span style=\"font-weight: 400;\">JoVE\u2019s<\/span><\/a><span style=\"font-weight: 400;\"> high-quality <\/span><a href=\"https:\/\/www.jove.com\/education\/chemistry\"><span style=\"font-weight: 400;\">chemistry videos<\/span><\/a><span style=\"font-weight: 400;\"> offer step-by-step animations, expert explanations, and real-world applications to help students master reaction kinetics.<\/span><\/p>\n<p><b>Why Use JoVE Videos?<\/b><b><br \/><\/b><span style=\"font-weight: 400;\">\u2714 <\/span><b>Increases Student Engagement:<\/b><span style=\"font-weight: 400;\"> Clear visuals make abstract concepts easier to grasp.<\/span><span style=\"font-weight: 400;\"><br \/><\/span><span style=\"font-weight: 400;\">\u2714 <\/span><b>Improves Student Outcomes:<\/b><span style=\"font-weight: 400;\"> Structured demonstrations reinforce chemical principles.<\/span><span style=\"font-weight: 400;\"><br \/><\/span><span style=\"font-weight: 400;\">\u2714 <\/span><b>Saves Teachers Time:<\/b><span style=\"font-weight: 400;\"> Ready-to-use instructional resources simplify lesson planning.<\/span><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t<div class=\"elementor-element elementor-element-07347ec e-flex e-con-boxed e-con e-parent\" data-id=\"07347ec\" data-element_type=\"container\" data-e-type=\"container\">\n\t\t\t\t\t<div class=\"e-con-inner\">\n\t\t\t\t<div class=\"elementor-element elementor-element-25f1a42 elementor-widget elementor-widget-heading\" data-id=\"25f1a42\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"heading.default\">\n\t\t\t\t\t<h2 class=\"elementor-heading-title elementor-size-default\">Common Student Challenges and Solutions\n<\/h2>\t\t\t\t<\/div>\n\t\t\t\t<div class=\"elementor-element elementor-element-ff6c39b elementor-widget elementor-widget-text-editor\" data-id=\"ff6c39b\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"text-editor.default\">\n\t\t\t\t\t\t\t\t\t<p><b>Problem: Confusing How Catalysts Work<\/b><\/p>\n<p><b>Solution:<\/b><span style=\"font-weight: 400;\"> Use the hydrogen peroxide experiment to demonstrate how catalysts lower activation energy.<\/span><\/p>\n<p><b>Problem: Struggling with Temperature Effects<\/b><\/p>\n<p><span style=\"font-weight: 400;\">\u00a0<\/span><b>Solution:<\/b><span style=\"font-weight: 400;\"> Conduct the temperature variation experiment and reinforce with JoVE\u2019s video explanations.<\/span><\/p>\n<p><b>Problem: Difficulty Understanding Collision Theory<\/b><\/p>\n<p><span style=\"font-weight: 400;\">\u00a0<\/span><b>Solution:<\/b><span style=\"font-weight: 400;\"> Perform the surface area reaction experiment and show JoVE\u2019s animated breakdown of collision theory.<\/span><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t<div class=\"elementor-element elementor-element-c271786 e-flex e-con-boxed e-con e-parent\" data-id=\"c271786\" data-element_type=\"container\" data-e-type=\"container\">\n\t\t\t\t\t<div class=\"e-con-inner\">\n\t\t\t\t<div class=\"elementor-element elementor-element-febb9a8 elementor-widget elementor-widget-heading\" data-id=\"febb9a8\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"heading.default\">\n\t\t\t\t\t<h2 class=\"elementor-heading-title elementor-size-default\">Conclusion \u2013 Why Teachers Should Incorporate These Experiments\n<\/h2>\t\t\t\t<\/div>\n\t\t\t\t<div class=\"elementor-element elementor-element-653800b elementor-widget elementor-widget-text-editor\" data-id=\"653800b\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"text-editor.default\">\n\t\t\t\t\t\t\t\t\t<p><span style=\"font-weight: 400;\">Studying reaction rates and catalysts through hands-on chemistry labs transforms abstract concepts into engaging experiences. By conducting simple experiments that demonstrate surface area effects, catalysis, and temperature influences, students can better understand collision theory and reaction kinetics.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">Combining these interactive experiments with <\/span><a href=\"https:\/\/www.jove.com\/schools\"><span style=\"font-weight: 400;\">JoVE\u2019s<\/span><\/a> <a href=\"https:\/\/www.jove.com\/education\/chemistry\"><span style=\"font-weight: 400;\">chemistry videos<\/span><\/a><span style=\"font-weight: 400;\"> creates a dynamic learning experience, ensuring students grasp reaction rates and catalysts with clarity and confidence.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">\u00a0<\/span><a href=\"https:\/\/www.jove.com\/schools\/try-for-free\/\"><span style=\"font-weight: 400;\">Make chemistry engaging\u2014use JoVE\u2019s interactive videos and hands-on experiments to bring reaction rates to life in your classroom!<\/span><\/a><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t","protected":false},"excerpt":{"rendered":"<p>Investigating Catalysts and Reaction Rates with High School Chemistry Labs Why do some reactions take seconds while others take years? [&hellip;]<\/p>\n","protected":false},"author":2,"featured_media":4089,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"content-type":"","site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","theme-transparent-header-meta":"default","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"set","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center 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