{"id":66474,"date":"2026-10-06T17:20:08","date_gmt":"2026-10-06T14:20:08","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66474"},"modified":"2026-10-06T17:20:08","modified_gmt":"2026-10-06T14:20:08","slug":"nernst-equation-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/nernst-equation-calculator\/","title":{"rendered":"Nernst Equation Calculator"},"content":{"rendered":"<section class=\"not-prose calculator-box\" aria-labelledby=\"calculator-title\"><div class=\"flex items-baseline sm:items-center justify-between gap-2 sm:gap-3\"><div class=\"flex flex-col sm:flex-row sm:items-center gap-2\"><span class=\"icon icon-calculator text-primary-700! text-base! dark:text-primary-300!\" aria-hidden=\"true\"><\/span><h2 id=\"calculator-title\" class=\"text-lg font-display font-bold\">Find the Cell Potential at Nonstandard Conditions<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66474\" data-favorite-title=\"Nernst Equation\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/nernst-equation-calculator\/\" data-favorite-excerpt=\"Calculate the cell potential of an electrochemical cell under nonstandard conditions using the Nernst equation. Enter the standard potential E\u00b0, temperature, electrons transferred n, and reaction quotient Q.\" aria-label=\"Add to Favorites\" data-favorite-icon=\"icon icon-chemistry-1\">\n    <span class=\"icon icon-shape-star-empty\" aria-hidden=\"true\"><\/span>\n  <\/button>\n  <div class=\"calcdash-favorite__tip\" aria-hidden=\"true\">\n   <span class=\"favorite-tooltip\" id=\"favorite-tooltip\"><\/span>\n  <\/div>\n  <span class=\"sr-only\" role=\"status\" id=\"favorite-status\"><\/span>\n<\/div><\/div><form action=\"https:\/\/wpcalc.com\/en\/chemistry\/nernst-equation-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66474\" data-post=\"66474\"><fieldset class=\"fieldset-input is-1\"><legend class=\"sr-only\">Input Fields<\/legend><div class=\"field has-term\" id=\"input-1\"><label for=\"field-1\">Standard Cell Potential (E\u00b0)<\/label><div class=\"term\">E\u00b0<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><div class=\"field-group\"><input type=\"number\" name=\"standard_cell_potential_e\" id=\"field-1\" aria-describedby=\"calc-info-1\" placeholder=\"e.g. 1.10\" step=\"0.0001\" value=\"1.1\"\/><div class=\"grid grid-cols-1\"><select id=\"field-2\" name=\"unit\" aria-label=\"Unit\"><option value=\"v\" selected>V<\/option><option value=\"mv\">mV<\/option><\/select><svg class=\"pointer-events-none col-start-1 row-start-1 mr-2 size-5 self-center justify-self-end text-gray-500 sm:size-4\" viewBox=\"0 0 16 16\" fill=\"currentColor\" aria-hidden=\"true\" data-slot=\"icon\">\n              <path fill-rule=\"evenodd\" d=\"M4.22 6.22a.75.75 0 0 1 1.06 0L8 8.94l2.72-2.72a.75.75 0 1 1 1.06 1.06l-3.25 3.25a.75.75 0 0 1-1.06 0L4.22 7.28a.75.75 0 0 1 0-1.06Z\" clip-rule=\"evenodd\" \/>\n            <\/svg><\/div><\/div><small id=\"calc-info-1\">Cell potential under standard conditions (1 M, 1 atm); e.g. 1.10 V for the Daniell cell<\/small><\/div><div class=\"field has-term\" id=\"input-2\"><label for=\"field-3\">Temperature (T)<\/label><div class=\"term\">T<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><div class=\"field-group\"><input type=\"number\" name=\"temperature_t\" id=\"field-3\" aria-describedby=\"calc-info-3\" placeholder=\"e.g. 25\" step=\"0.01\" value=\"25\"\/><div class=\"grid grid-cols-1\"><select id=\"field-4\" name=\"unit\" aria-label=\"Unit\"><option value=\"c\" selected>\u00b0C<\/option><option value=\"k\">K<\/option><option value=\"f\">\u00b0F<\/option><\/select><svg class=\"pointer-events-none col-start-1 row-start-1 mr-2 size-5 self-center justify-self-end text-gray-500 sm:size-4\" viewBox=\"0 0 16 16\" fill=\"currentColor\" aria-hidden=\"true\" data-slot=\"icon\">\n              <path fill-rule=\"evenodd\" d=\"M4.22 6.22a.75.75 0 0 1 1.06 0L8 8.94l2.72-2.72a.75.75 0 1 1 1.06 1.06l-3.25 3.25a.75.75 0 0 1-1.06 0L4.22 7.28a.75.75 0 0 1 0-1.06Z\" clip-rule=\"evenodd\" \/>\n            <\/svg><\/div><\/div><small id=\"calc-info-3\">Temperature of the electrochemical cell<\/small><\/div><div class=\"field has-term\" id=\"input-3\"><label for=\"field-5\">Electrons Transferred (n)<\/label><div class=\"term\">n<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"electrons_transferred_n\" id=\"field-5\" aria-describedby=\"calc-info-5\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 2\" min=\"0.001\" value=\"2\"\/><small id=\"calc-info-5\">Number of electrons transferred in the balanced redox reaction (e.g. 2 for Zn + Cu\u00b2\u207a \u2192 Zn\u00b2\u207a + Cu)<\/small><\/div><div class=\"field has-term\" id=\"input-4\"><label for=\"field-6\">Reaction Quotient (Q)<\/label><div class=\"term\">Q<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"reaction_quotient_q\" id=\"field-6\" aria-describedby=\"calc-info-6\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 10\" min=\"0\" value=\"10\"\/><small id=\"calc-info-6\">Ratio of product activities to reactant activities at the given moment; Q = 1 at standard conditions<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66474\">Calculate<\/button><button type=\"reset\">Reset<\/button><\/div><div class=\"field is-checkbox hidden!\" id=\"field-auto-calc\"><input type=\"checkbox\" id=\"auto-calc\"><label for=\"auto-calc\">Calculate automatically<\/label><small>If enabled, the result will update automatically when you change any value.<\/small><\/div><div class=\"fieldset-result is-hidden\" aria-labelledby=\"result-title\" aria-live=\"polite\" role=\"region\"> <h3 class=\"result-title bg-gradient-to-r from-primary-50 to-gray-50 dark:from-primary-900 dark:to-gray-800\" id=\"result-title\"><span class=\"icon icon-s-pulse\" aria-hidden=\"true\"><\/span> Nernst Equation Results<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Cell Potential<\/span><span class=\"result-term\">E<\/span><\/span><span class=\"field-value\" id=\"result-1\" data-unit=\"V\"><\/span><button type=\"button\" class=\"copy-result\" data-tooltip=\"Copy Result\" aria-label=\"Copy Result\"><span class=\"copy-icon icon icon-document-copy\" aria-hidden=\"true\"><\/span><\/button><\/div><div class=\"field-result\" id=\"output-2\"><span class=\"field-title\"><span>Cell Potential<\/span><\/span><span class=\"field-value\" id=\"result-2\" data-unit=\"mV\"><\/span><button type=\"button\" class=\"copy-result\" data-tooltip=\"Copy Result\" aria-label=\"Copy Result\"><span class=\"copy-icon icon icon-document-copy\" aria-hidden=\"true\"><\/span><\/button><\/div><div class=\"field-result\" id=\"output-3\"><span class=\"field-title\"><span>Deviation from Standard Potential<\/span><span class=\"result-term\">E \u2212 E\u00b0<\/span><\/span><span class=\"field-value\" id=\"result-3\" data-unit=\"V\"><\/span><button type=\"button\" class=\"copy-result\" data-tooltip=\"Copy Result\" aria-label=\"Copy Result\"><span class=\"copy-icon icon icon-document-copy\" aria-hidden=\"true\"><\/span><\/button><\/div><\/div><div class=\"result-actions\"><button type=\"button\" class=\"copy-link\"><svg viewBox=\"0 0 20 20\" fill=\"currentColor\" aria-hidden=\"true\"><path d=\"M12.232 4.232a2.5 2.5 0 0 1 3.536 3.536l-1.225 1.224a.75.75 0 0 0 1.061 1.06l1.224-1.224a4 4 0 0 0-5.656-5.656l-3 3a4 4 0 0 0 .225 5.865.75.75 0 0 0 .977-1.138 2.5 2.5 0 0 1-.142-3.667l3-3Z\"\/><path d=\"M11.603 7.963a.75.75 0 0 0-.977 1.138 2.5 2.5 0 0 1 .142 3.667l-3 3a2.5 2.5 0 0 1-3.536-3.536l1.225-1.224a.75.75 0 0 0-1.061-1.06l-1.224 1.224a4 4 0 1 0 5.656 5.656l3-3a4 4 0 0 0-.225-5.865Z\"\/><\/svg><span class=\"copy-link__text\">Copy link to this calculation<\/span><\/button><span class=\"sr-only\" role=\"status\" id=\"copy-link-status\"><\/span><\/div><\/div><a href=\"#respond\" class=\"hidden transition-opacity duration-300 opacity-0 w-50 text-sm justify-center items-center gap-2 px-4 py-2 rounded bg-gray-200 text-gray-700 hover:bg-gray-300\" id=\"leave-comment\"><span class=\"icon icon-comments\" aria-hidden=\"true\"><\/span>Leave a Comment<\/a><\/form><\/section><section id=\"calc-reactions\" class=\"not-prose hidden my-12 bg-gradient-to-r from-primary-50 to-gray-50 border border-indigo-100 rounded-xl px-6 py-4 shadow-sm\" data-post=\"66474\" aria-live=\"polite\" aria-labelledby=\"calc-reactions-title\"><p id=\"calc-reactions-title\" class=\"text-sm text-gray-500 text-center mb-2\">How did this result make you feel?<\/p><div role=\"group\" aria-labelledby=\"calc-reactions-title\" class=\"grid grid-cols-3 sm:flex sm:flex-row sm:justify-around gap-4 sm:items-center sm:flex-wrap\"><button type=\"button\" aria-pressed=\"false\" class=\"reaction-btn flex flex-col items-center gap-1 text-sm text-gray-700 hover:text-primary-600 cursor-pointer transition-transform hover:scale-105\" data-reaction=\"like\"><span class=\"reaction-count\" data-reaction-count=\"like\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\ud83d\ude00 <\/span><span class=\"reaction-description font-medium\">Like <\/span><\/button><button type=\"button\" aria-pressed=\"false\" class=\"reaction-btn flex flex-col items-center gap-1 text-sm text-gray-700 hover:text-primary-600 cursor-pointer transition-transform hover:scale-105\" data-reaction=\"helpful\"><span class=\"reaction-count\" data-reaction-count=\"helpful\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\ud83d\udca1 <\/span><span class=\"reaction-description font-medium\">Helpful <\/span><\/button><button type=\"button\" aria-pressed=\"false\" class=\"reaction-btn flex flex-col items-center gap-1 text-sm text-gray-700 hover:text-primary-600 cursor-pointer transition-transform hover:scale-105\" data-reaction=\"confused\"><span class=\"reaction-count\" data-reaction-count=\"confused\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\ud83d\ude15 <\/span><span class=\"reaction-description font-medium\">Confused <\/span><\/button><button type=\"button\" aria-pressed=\"false\" class=\"reaction-btn flex flex-col items-center gap-1 text-sm text-gray-700 hover:text-primary-600 cursor-pointer transition-transform hover:scale-105\" data-reaction=\"disappointed\"><span class=\"reaction-count\" data-reaction-count=\"disappointed\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\ud83d\ude1e <\/span><span class=\"reaction-description font-medium\">Disappointed <\/span><\/button><button type=\"button\" aria-pressed=\"false\" class=\"reaction-btn flex flex-col items-center gap-1 text-sm text-gray-700 hover:text-primary-600 cursor-pointer transition-transform hover:scale-105\" data-reaction=\"inaccurate\"><span class=\"reaction-count\" data-reaction-count=\"inaccurate\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\u274c <\/span><span class=\"reaction-description font-medium\">Inaccurate <\/span><\/button><\/div><div id=\"reaction-message\" class=\"hidden mt-8 rounded-md border border-primary-100 bg-white\/50 backdrop-blur-sm px-4 py-2 text-sm text-center shadow-sm\"><\/div><\/section><div class=\"calcdash-ad not-prose calcdash-ad--calc_result calcdash-ad--in-article\"><ins class=\"adsbygoogle\" style=\"display:block\" data-ad-client=\"ca-pub-1721569815777345\" data-ad-slot=\"6317458308\" data-ad-layout=\"in-article\" data-ad-format=\"fluid\"><\/ins><script>(adsbygoogle = window.adsbygoogle || []).push({});<\/script><\/div>\n<style id=\"wpcoderpro-inline-1\">.formula-box {\r\n\tborder-bottom: none !important;\r\n}<\/style><section class=\"formula-box\" aria-labelledby=\"formula-title\">\r\n\t<div id=\"formula-title\" class=\"not-prose font-display mb-4\"><span class=\"icon icon-formula\" aria-hidden=\"true\"><\/span><h2>Nernst Equation Formula<\/h2><\/div>\r\n\t<figure class=\"not-prose formula\">\r\n\t\t<figcaption class=\"formula-title\">Formula<\/figcaption>\r\n\t\t<div class=\"text-base text-gray-800\" id=\"formula\">\n\\[ E = E^\\circ - \\frac{R\\,T}{n\\,F}\\,\\ln Q \\]<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(E\\) \u2014 cell potential under the given (nonstandard) conditions, in volts (V)<\/li>\n<li>\\(E^\\circ\\) \u2014 standard cell potential, in volts (V)<\/li>\n<li>\\(R\\) \u2014 universal gas constant, \\(8.314\\ \\mathrm{J\/(mol\\cdot K)}\\)<\/li>\n<li>\\(T\\) \u2014 absolute temperature, in kelvin (K)<\/li>\n<li>\\(n\\) \u2014 number of electrons transferred in the balanced redox reaction<\/li>\n<li>\\(F\\) \u2014 Faraday constant, \\(96\\,485\\ \\mathrm{C\/mol}\\)<\/li>\n<li>\\(Q\\) \u2014 reaction quotient (product activities divided by reactant activities at the given moment)<\/li>\n<\/ul>\n<p>The Nernst equation relates the actual cell potential to the standard cell potential, correcting for temperature and for the concentrations (more precisely, activities) of the reactants and products. When \\(Q = 1\\) (standard conditions), the logarithm term vanishes and \\(E = E^\\circ\\).<\/p>\n<p>At 25 \u00b0C (298.15 K), the equation is often written in the base-10 form:<\/p>\n<p>\\[ E = E^\\circ - \\frac{0.0592}{n}\\,\\log Q \\]<\/p>\n<p>\r\n<\/section>\n<style id=\"wpcoderpro-inline-459\">.calculation-box {\r\n\tborder-bottom: none !important;\r\n}<\/style><section id=\"calculation\" class=\"calculation-box\" aria-labelledby=\"calculation-title\">\r\n\t<div id=\"calculation-title\" class=\"not-prose font-display\"><span class=\"icon icon-unordered-list\" aria-hidden=\"true\"><\/span><h2>Nernst Equation \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<p>{example}<\/p>\n<p><strong>Example:<\/strong> a Daniell cell (Zn | Zn\u00b2\u207a || Cu\u00b2\u207a | Cu) operates at 25 \u00b0C with a standard cell potential of 1.10 V. Two electrons are transferred, and at a given moment the ion concentrations give a reaction quotient \\(Q = 10\\).<\/p>\n<p>\\[ T = 25 + 273.15 = 298.15\\ \\mathrm{K} \\]<\/p>\n<p>\\[ E = 1.10 - \\frac{8.314 \\times 298.15}{2 \\times 96\\,485}\\,\\ln 10 \\]<\/p>\n<p>\\[ E = 1.10 - 0.01285 \\times 2.3026 = 1.10 - 0.0296 \\]<\/p>\n<p><strong>Result:<\/strong> \\(E \\approx 1.0704\\ \\mathrm{V}\\) (about 1070.42 mV), a deviation of \\(-0.0296\\ \\mathrm{V}\\) from the standard potential.<\/p>\n<p>{\/example}<\/p>\n\r\n<\/section>\n<h2>How to Use the Nernst Equation Calculator<\/h2>\n<ol>\n<li>Enter the <strong>Standard Cell Potential (E\u00b0)<\/strong> in volts (V) or millivolts (mV) \u2014 for example, 1.10 V for the Daniell cell.<\/li>\n<li>Enter the <strong>Temperature (T)<\/strong> and choose its unit (\u00b0C, K, or \u00b0F). The calculator converts it to kelvin automatically.<\/li>\n<li>Enter the <strong>Electrons Transferred (n)<\/strong> from your balanced redox reaction \u2014 for example, 2 for Zn + Cu\u00b2\u207a \u2192 Zn\u00b2\u207a + Cu.<\/li>\n<li>Enter the <strong>Reaction Quotient (Q)<\/strong>. Use \\(Q = 1\\) for standard conditions, or compute \\(Q\\) from the actual concentrations.<\/li>\n<li>Read the <strong>Cell Potential<\/strong> in volts and millivolts, along with the <strong>Deviation from Standard Potential<\/strong> (\\(E - E^\\circ\\)).<\/li>\n<\/ol>\n<h2>What Is the Nernst Equation?<\/h2>\n<p>The Nernst equation describes how the voltage of an electrochemical cell changes when the reactants and products are not at standard conditions (1 M solutions, 1 atm gases). Standard tables list cell potentials only for standard states, but real batteries, corrosion systems, and sensors almost never operate under these exact conditions. The Nernst equation closes this gap by adding a concentration- and temperature-dependent correction term to the standard potential.<\/p>\n<p>Physically, the equation expresses the link between electrical energy and chemical free energy: as the reaction proceeds toward equilibrium, the reaction quotient \\(Q\\) grows, the correction term increases, and the cell voltage drops. When \\(Q\\) reaches the equilibrium constant \\(K\\), the cell potential becomes exactly zero \u2014 the battery is \"dead\" because no net driving force remains.<\/p>\n<p>Interpreting the result is straightforward: if \\(Q &lt; 1\\) (reactants favored), the correction term is negative and \\(E &gt; E^\\circ\\) \u2014 the cell delivers more voltage than under standard conditions. If \\(Q &gt; 1\\) (products favored), \\(E &lt; E^\\circ\\). The temperature dependence also matters: higher temperature amplifies the deviation from \\(E^\\circ\\).<\/p>\n<p>Beyond batteries, the Nernst equation underpins pH measurement (a glass-electrode pH meter is a Nernstian device), nerve signal transmission, concentration cells, and corrosion prediction. If you need to determine the ion concentrations that go into \\(Q\\), the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/molarity-calculator\/\">Molarity Calculator<\/a> and the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/ph-calculator\/\">pH Calculator<\/a> can help; to get the correct value of \\(n\\), first balance your half-reactions with the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/balancing-redox-reactions-2\/\">Balancing Redox Reactions Calculator<\/a>.<\/p>\n<h2>Assumptions, Limitations, and Practical Tips<\/h2>\n<ul>\n<li><strong>Use activities, not raw concentrations.<\/strong> The rigorous form of the equation uses activities. For dilute solutions (typically below 0.1 M), molar concentrations are a good approximation; in concentrated solutions, activity coefficients differ noticeably from 1.<\/li>\n<li><strong>Electrons transferred must come from the balanced equation.<\/strong> If the half-reactions are multiplied to equalize electrons, use the smallest whole-number ratio. An incorrect \\(n\\) directly scales the correction term and is the most common source of error.<\/li>\n<li><strong>Pure solids and liquids do not appear in Q.<\/strong> Only dissolved species and gases (relative to 1 M and 1 atm) enter the reaction quotient.<\/li>\n<li><strong>Temperature is converted internally.<\/strong> You can enter \u00b0C, K, or \u00b0F; the calculation always uses kelvin. Note that 25 \u00b0C = 298.15 K, the temperature at which the familiar 0.0592\/n constant applies.<\/li>\n<li><strong>The equation assumes equilibrium-reversible behavior.<\/strong> It predicts the thermodynamic (no-current) voltage. Under heavy load, real cells show lower voltages due to overpotentials and internal resistance \u2014 effects the Nernst equation does not capture.<\/li>\n<li><strong>Sign matters.<\/strong> A negative result means the reaction is non-spontaneous in the written direction under those conditions; reversing the reaction flips the sign of both \\(E\\) and \\(Q\\).<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the cell potential of an electrochemical cell under nonstandard conditions using the Nernst equation. Enter the standard potential E\u00b0, temperature, electrons transferred n, and reaction quotient Q.<\/p>\n","protected":false},"author":3168,"featured_media":0,"comment_status":"open","ping_status":"","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"footnotes":""},"categories":[54],"tags":[57],"class_list":["post-66474","post","type-post","status-publish","format-standard","hentry","category-chemistry","tag-reactions"],"acf":[],"_links":{"self":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66474","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/users\/3168"}],"replies":[{"embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/comments?post=66474"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66474\/revisions"}],"predecessor-version":[{"id":66476,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66474\/revisions\/66476"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66474"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66474"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66474"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}