{"id":4178,"date":"2025-03-23T00:12:59","date_gmt":"2025-03-23T00:12:59","guid":{"rendered":"https:\/\/schools.jove.com\/?p=4178"},"modified":"2026-07-23T16:44:55","modified_gmt":"2026-07-23T16:44:55","slug":"exploring-electrochemistry-galvanic-cell-experiments","status":"publish","type":"post","link":"https:\/\/schools.jove.com\/exploring-electrochemistry-galvanic-cell-experiments\/","title":{"rendered":"Exploring Electrochemistry with Galvanic Cells"},"content":{"rendered":"\t\t<div data-elementor-type=\"wp-post\" data-elementor-id=\"4178\" class=\"elementor elementor-4178\" 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\">Exploring Electrochemistry with Galvanic Cells\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<h3><b>Introduction: The Lemon Battery Mystery<\/b><\/h3>\n<p><span style=\"font-weight: 400;\">During a science fair, a student powered an LED light using just a lemon, two metal strips, and some wires. The amazed crowd asked, \u201cHow can a lemon create electricity?\u201d<\/span><\/p>\n<p><span style=\"font-weight: 400;\">The answer lies in <\/span><a href=\"https:\/\/www.jove.com\/schools\/v\/14548\/electrochemistry-overview\"><span style=\"font-weight: 400;\">electrochemistry<\/span><\/a><span style=\"font-weight: 400;\"> \u2014 a field that explores how chemical reactions produce electric energy. This fascinating concept is the foundation of <\/span><a href=\"https:\/\/www.jove.com\/schools\/v\/11177\/galvanic-cells-construction-reduction-potential-measurement?trialstart=1&amp;redirectTo=https:\/\/www.jove.com\/schools\/v\/11177\/galvanic-cells-construction-reduction-potential-measurement&amp;__hstc=265155024.c73482deb51619779b372105310aa908.1730073600231.1730073600232.1730073600233.1&amp;__hssc=265155024.1.1730073600234&amp;__hsfp=2375820541\"><span style=\"font-weight: 400;\">galvanic cells<\/span><\/a><span style=\"font-weight: 400;\">, which convert chemical energy into electrical energy through redox reactions.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">Research from<\/span><a href=\"https:\/\/www.jove.com\/schools\"><span style=\"font-weight: 400;\"> JoVE\u2019s<\/span><\/a><span style=\"font-weight: 400;\"> Science Education Resources found that incorporating visual demonstrations and interactive experiments improved student understanding of complex scientific concepts like electrochemistry by up to <\/span><b>50%<\/b><span style=\"font-weight: 400;\"> compared to text-based learning alone<\/span><a href=\"https:\/\/www.jove.com\/files\/media\/pdf\/JoVE%20Advantage%201%20-%20Video%20Effectiveness%20in%20Education.pdf\"> <span style=\"font-weight: 400;\">(JoVE Video Effectiveness in Education)<\/span><\/a><span style=\"font-weight: 400;\">. Additionally, educators reported that using JoVE videos increased student engagement and participation by <\/span><b>82%<\/b><span style=\"font-weight: 400;\">, further reinforcing the value of visual learning in science education.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">In this article, we\u2019ll explore how galvanic cells work, highlight common misconceptions, and share engaging experiments \u2014 all supported by <\/span><a href=\"https:\/\/www.jove.com\/schools\/science-video\/\"><span style=\"font-weight: 400;\">JoVE\u2019s educational videos<\/span><\/a><span style=\"font-weight: 400;\"> to simplify this essential chemistry concept.<\/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\">What is a Galvanic Cell?\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-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><span style=\"font-weight: 400;\">A<\/span><a href=\"https:\/\/www.jove.com\/schools\/v\/11177\/galvanic-cells-construction-reduction-potential-measurement?trialstart=1&amp;redirectTo=https:\/\/www.jove.com\/schools\/v\/11177\/galvanic-cells-construction-reduction-potential-measurement&amp;__hstc=265155024.c73482deb51619779b372105310aa908.1730073600231.1730073600232.1730073600233.1&amp;__hssc=265155024.1.1730073600234&amp;__hsfp=2375820541\"><span style=\"font-weight: 400;\"> galvanic cell<\/span><\/a><span style=\"font-weight: 400;\"> (also called a voltaic cell) is an electrochemical cell that generates electrical energy from spontaneous chemical reactions. These reactions involve the transfer of electrons during a <\/span><a href=\"https:\/\/www.jove.com\/schools\/v\/11144\/redox-reaction-oxidation-states-concept\"><span style=\"font-weight: 400;\">redox reaction<\/span><\/a><span style=\"font-weight: 400;\"> (reduction-oxidation).<\/span><\/p>\n<h3><b>Key Components of a Galvanic Cell<\/b><\/h3>\n<ol>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Anode:<\/b><span style=\"font-weight: 400;\"> The electrode where oxidation occurs (loses electrons).<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Cathode:<\/b><span style=\"font-weight: 400;\"> The electrode where reduction occurs (gains electrons).<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Electrolyte Solutions:<\/b><span style=\"font-weight: 400;\"> Provide ions to balance the charges during the reaction.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Salt Bridge:<\/b><span style=\"font-weight: 400;\"> Maintains electrical neutrality by allowing ion flow between the two half-cells.<\/span><\/li>\n<\/ol>\n<p><span style=\"font-weight: 400;\">In this <\/span><a href=\"https:\/\/www.jove.com\/schools\/v\/11177\/galvanic-cells-construction-reduction-potential-measurement?trialstart=1&amp;redirectTo=https:\/\/www.jove.com\/schools\/v\/11177\/galvanic-cells-construction-reduction-potential-measurement&amp;__hstc=265155024.c73482deb51619779b372105310aa908.1730073600231.1730073600232.1730073600233.1&amp;__hssc=265155024.1.1730073600234&amp;__hsfp=2375820541\"><span style=\"font-weight: 400;\">JoVE video on galvanic cells<\/span><\/a><span style=\"font-weight: 400;\">, students can visualize how electrons flow from the anode to the cathode, producing an electric current that powers devices.<\/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<h2 class=\"elementor-heading-title elementor-size-default\">Why Do Students Struggle with Electrochemistry Concepts?\n<\/h2>\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><a href=\"https:\/\/www.jove.com\/schools\/v\/14548\/electrochemistry-overview\"><span style=\"font-weight: 400;\">Electrochemistry<\/span><\/a><span style=\"font-weight: 400;\"> can confuse students due to common misconceptions, such as:<\/span><\/p>\n<ul>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Believing electrons move through the salt bridge (when they actually flow through the external circuit).<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Thinking the cathode is always positive (in galvanic cells, the cathode is positive, but in electrolytic cells, it\u2019s negative).<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Assuming the salt bridge carries electrons rather than ions.<\/span><\/li>\n<\/ul>\n<p><span style=\"font-weight: 400;\">In <\/span><a href=\"https:\/\/www.jove.com\/schools\/v\/14548\/electrochemistry-overview\"><span style=\"font-weight: 400;\">JoVE\u2019s demonstration video of electrochemistry<\/span><\/a><span style=\"font-weight: 400;\">, students can watch clear visual explanations of electron flow, electrode reactions, and salt bridge behavior \u2014 addressing these common misunderstandings.<\/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\">Demonstrating a Galvanic Cell in the Classroom<\/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;\">Building a simple galvanic cell is a powerful hands-on experiment that allows students to see electrochemistry in action.<\/span><\/p>\n<h3><b>Materials Needed<\/b><\/h3>\n<ul>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Copper strip (Cu)<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Zinc strip (Zn)<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Two beakers<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Copper sulfate (CuSO\u2084) solution<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Zinc sulfate (ZnSO\u2084) solution<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Salt bridge (filter paper soaked in potassium nitrate solution)<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Wires and a voltmeter<\/span><\/li>\n<\/ul>\n<h3><b>Steps to Build the Galvanic Cell<\/b><\/h3>\n<ol>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Prepare the Electrodes:<\/b><span style=\"font-weight: 400;\"> Place the copper strip in the <\/span><b>CuSO\u2084<\/b><span style=\"font-weight: 400;\"> solution and the zinc strip in the ZnSO\u2084 solution.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Insert the Salt Bridge:<\/b><span style=\"font-weight: 400;\"> Dip the potassium nitrate-soaked filter paper into both beakers to connect the solutions.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Connect the Circuit:<\/b><span style=\"font-weight: 400;\"> Use wires to connect the copper and zinc strips to the voltmeter.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Observe the Voltage:<\/b><span style=\"font-weight: 400;\"> Students should observe a voltage reading on the meter \u2014 demonstrating that chemical energy is being converted into electrical energy.<\/span><\/li>\n<\/ol>\n<p><a href=\"https:\/\/www.jove.com\/schools\/v\/11177\/galvanic-cells-construction-reduction-potential-measurement?trialstart=1&amp;redirectTo=https:\/\/www.jove.com\/schools\/v\/11177\/galvanic-cells-construction-reduction-potential-measurement&amp;__hstc=265155024.c73482deb51619779b372105310aa908.1730073600231.1730073600232.1730073600233.1&amp;__hssc=265155024.1.1730073600234&amp;__hsfp=2375820541\"><span style=\"font-weight: 400;\">In JoVE\u2019s galvanic cell video<\/span><\/a><span style=\"font-weight: 400;\">, students can watch this setup in action while learning why electron flow from zinc (anode) to copper (cathode) generates a measurable current.<\/span><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t<div class=\"elementor-element elementor-element-f22f062 elementor-widget elementor-widget-heading\" data-id=\"f22f062\" 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\">Real-World Applications of Galvanic Cells<\/h2>\t\t\t\t<\/div>\n\t\t\t\t<div class=\"elementor-element elementor-element-c023321 elementor-widget elementor-widget-text-editor\" data-id=\"c023321\" 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;\">Galvanic cells are the foundation of many everyday technologies, including:<\/span><\/p>\n<ul>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Batteries:<\/b><span style=\"font-weight: 400;\"> Standard AA and AAA batteries operate based on galvanic cell principles.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Corrosion Prevention:<\/b><span style=\"font-weight: 400;\"> Galvanic cells explain why sacrificial anodes are used to protect metal structures.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Fuel Cells:<\/b><span style=\"font-weight: 400;\"> These advanced systems generate clean energy using similar electrochemical principles.<\/span><\/li>\n<\/ul>\n<p><span style=\"font-weight: 400;\">In <\/span><a href=\"https:\/\/www.jove.com\/education\/chemistry\"><span style=\"font-weight: 400;\">JoVE\u2019s real-world chemistry videos<\/span><\/a><span style=\"font-weight: 400;\">, students can explore how electrochemistry drives essential technologies and innovations.<\/span><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t<div class=\"elementor-element elementor-element-97f0197 elementor-widget elementor-widget-heading\" data-id=\"97f0197\" 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\">Try This! Classroom Challenge\n<\/h2>\t\t\t\t<\/div>\n\t\t\t\t<div class=\"elementor-element elementor-element-8d9d028 elementor-widget elementor-widget-text-editor\" data-id=\"8d9d028\" data-element_type=\"widget\" data-e-type=\"widget\" data-widget_type=\"text-editor.default\">\n\t\t\t\t\t\t\t\t\t<h3><b>Lemon Battery Experiment<\/b><\/h3>\n<p><b>Materials:<\/b><span style=\"font-weight: 400;\"> Lemon, copper coin, galvanized nail (zinc-coated), wires, LED bulb<\/span><\/p>\n<ol>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Prepare the Lemon Battery:<\/b><span style=\"font-weight: 400;\"> Insert the copper coin and galvanized nail into the lemon, ensuring they don\u2019t touch.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Connect the Circuit:<\/b><span style=\"font-weight: 400;\"> Use wires to connect the metal strips to the LED bulb.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Test the Voltage:<\/b><span style=\"font-weight: 400;\"> Ask students to predict whether adding more lemons increases the voltage.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><b>Explain the Science:<\/b><span style=\"font-weight: 400;\"> Use JoVE\u2019s electrochemistry video to connect this experiment to galvanic cell principles.<\/span><\/li>\n<\/ol>\n<p><span style=\"font-weight: 400;\">This engaging activity helps students see real-world electrochemistry concepts in action while reinforcing the roles of electrodes, ion flow, and voltage generation.<\/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-22d072d e-flex e-con-boxed e-con e-parent\" data-id=\"22d072d\" 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-68622e8 elementor-widget elementor-widget-heading\" data-id=\"68622e8\" 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: Bringing Electrochemistry to Life with JoVE Videos\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-a61d4f1 e-flex e-con-boxed e-con e-parent\" data-id=\"a61d4f1\" 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-fe5a523 elementor-widget elementor-widget-text-editor\" data-id=\"fe5a523\" 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\/64483\/electrochemistry\"><span style=\"font-weight: 400;\">Electrochemistry<\/span><\/a><span style=\"font-weight: 400;\"> plays a vital role in both science education and real-life applications. By combining JoVE\u2019s interactive educational videos with hands-on experiments like the galvanic cell, teachers can simplify complex electrochemical concepts and improve student engagement.<\/span><\/p>\n<h3><b>Next Steps:<\/b><\/h3>\n<ul>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Explore <\/span><a href=\"https:\/\/www.jove.com\/schools\/\"><span style=\"font-weight: 400;\">JoVE\u2019s <\/span><\/a><span style=\"font-weight: 400;\">electrochemistry videos to simplify galvanic cell concepts for your students.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Try the<\/span><a href=\"https:\/\/www.jove.com\/schools\/v\/11177\/galvanic-cells-construction-reduction-potential-measurement?trialstart=1&amp;redirectTo=https:\/\/www.jove.com\/schools\/v\/11177\/galvanic-cells-construction-reduction-potential-measurement&amp;__hstc=265155024.c73482deb51619779b372105310aa908.1730073600231.1730073600232.1730073600233.1&amp;__hssc=265155024.1.1730073600234&amp;__hsfp=2375820541\"><span style=\"font-weight: 400;\"> Galvanic Cell Experiment<\/span><\/a><span style=\"font-weight: 400;\">\u00a0 to create hands-on learning moments.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400;\">Ask students to identify real-life examples of electrochemistry, from batteries to rust prevention.<\/span><\/li>\n<\/ul>\n<p><span style=\"font-weight: 400;\">With the right tools and teaching strategies, electrochemistry becomes more than just theory \u2014 it becomes a concept students can see, test, and understand.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">Power up your classroom experiments with<\/span><a href=\"https:\/\/www.jove.com\/schools\/solutions\/\"> <span style=\"font-weight: 400;\">JoVE<\/span><\/a><span style=\"font-weight: 400;\"> and turn complex science into unforgettable learning moments!- <\/span><a href=\"https:\/\/www.jove.com\/highschool\/request-trial\"><span style=\"font-weight: 400;\">Unlock full access to JoVE\u2019s library for free. Book a demo with us today!<\/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>Exploring Electrochemistry with Galvanic Cells Introduction: The Lemon Battery Mystery During a science fair, a student powered an LED light [&hellip;]<\/p>\n","protected":false},"author":2,"featured_media":4179,"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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