{"id":66889,"date":"2026-10-13T10:07:15","date_gmt":"2026-10-13T07:07:15","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66889"},"modified":"2026-10-13T10:07:15","modified_gmt":"2026-10-13T07:07:15","slug":"standard-cell-potential-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/standard-cell-potential-calculator\/","title":{"rendered":"Standard Cell Potential 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 Voltage from Two Half-Cell Potentials<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66889\" data-favorite-title=\"Standard Cell Potential\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/standard-cell-potential-calculator\/\" data-favorite-excerpt=\"Enter the standard reduction potentials of the cathode and anode to get the standard cell potential E\u00b0cell, the spontaneity verdict, and the free energy change \u0394G\u00b0 per mole of electrons.\" 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\/standard-cell-potential-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66889\" data-post=\"66889\"><fieldset class=\"fieldset-input is-2\"><legend class=\"sr-only\">Input Fields<\/legend><div class=\"field has-term\" id=\"input-1\"><label for=\"field-1\">Cathode Potential (E\u00b0cat)<\/label><div class=\"term\">E\u00b0cat<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"number\" name=\"cathode_potential_ecat\" id=\"field-1\" aria-describedby=\"calc-unit-1 calc-info-1\" placeholder=\"e.g. 0.34\" step=\"any\" value=\"0.34\"\/><div class=\"unit\" id=\"calc-unit-1\">V<\/div><small id=\"calc-info-1\">Standard reduction potential of the half-reaction occurring at the cathode (reduction), e.g. +0.34 V for Cu\u00b2\u207a + 2e\u207b \u2192 Cu.<\/small><\/div><div class=\"field has-term\" id=\"input-2\"><label for=\"field-2\">Anode Potential (E\u00b0an)<\/label><div class=\"term\">E\u00b0an<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"number\" name=\"anode_potential_ean\" id=\"field-2\" aria-describedby=\"calc-unit-2 calc-info-2\" placeholder=\"e.g. -0.76\" step=\"any\" value=\"-0.76\"\/><div class=\"unit\" id=\"calc-unit-2\">V<\/div><small id=\"calc-info-2\">Standard reduction potential of the half-reaction occurring at the anode (oxidation), e.g. \u22120.76 V for Zn\u00b2\u207a + 2e\u207b \u2192 Zn.<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66889\">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> Standard Cell Potential Results<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Standard Cell Potential<\/span><span class=\"result-term\">E\u00b0cell<\/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 is-column\" id=\"output-2\"><span class=\"field-title\"><span>Cell Reaction Under Standard Conditions<\/span><\/span><span class=\"field-value\" id=\"result-2\"><\/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>Free Energy per Mole of Electrons<\/span><span class=\"result-term\">\u0394G\u00b0<\/span><\/span><span class=\"field-value\" id=\"result-3\" data-unit=\"kJ\/mol e\u207b\"><\/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 is-column\" id=\"output-4\"><span class=\"field-title\"><span>Calculation Details<\/span><\/span><span class=\"field-value\" id=\"result-4\"><\/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 is-column\" id=\"output-5\"><span class=\"field-title\"><span>About the Calculation<\/span><\/span><span class=\"field-value\" id=\"result-5\"><\/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=\"66889\" 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>Standard Cell Potential 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\u00b0_{cell} = E\u00b0_{cathode} - E\u00b0_{anode} \\]\n\\[ \\Delta G\u00b0 = -nFE\u00b0_{cell} \\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(E\u00b0_{cathode}\\) \u2014 standard reduction potential of the half-reaction occurring at the cathode (V)<\/li>\n<li>\\(E\u00b0_{anode}\\) \u2014 standard reduction potential of the half-reaction occurring at the anode (V)<\/li>\n<li>\\(n\\) \u2014 number of electrons transferred in the balanced cell reaction<\/li>\n<li>\\(F\\) \u2014 Faraday constant, 96 485 C\/mol<\/li>\n<li>\\(\\Delta G\u00b0\\) \u2014 standard free energy change (J\/mol, or kJ\/mol when divided by 1000)<\/li>\n<\/ul>\n<p>The first formula gives the voltage of the cell from two tabulated standard reduction potentials; the second links that voltage to the thermodynamic driving force of the cell reaction.<\/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>Standard Cell Potential \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> a Daniell cell with a copper electrode in Cu\u00b2\u207a solution as the cathode (E\u00b0 = +0.34 V) and a zinc electrode in Zn\u00b2\u207a solution as the anode (E\u00b0 = \u22120.76 V). These are the calculator's default values.<\/p>\n<p>\\[ E\u00b0_{cell} = E\u00b0_{cathode} - E\u00b0_{anode} = 0.34\\ \\text{V} - (-0.76\\ \\text{V}) = 1.10\\ \\text{V} \\]<\/p>\n<p>The reaction transfers \\(n = 2\\) electrons (Cu\u00b2\u207a + 2e\u207b \u2192 Cu and Zn \u2192 Zn\u00b2\u207a + 2e\u207b), so the free energy is:<\/p>\n<p>\\[ \\Delta G\u00b0 = -nFE\u00b0_{cell} = -2 \\times 96\\,485 \\times 1.10 = -212\\,267\\ \\text{J} \\approx -212\\ \\text{kJ\/mol} \\]<\/p>\n<p><strong>Result:<\/strong> E\u00b0cell = 1.10 V; \u0394G\u00b0 \u2248 \u2212106.13 kJ per mole of electrons (\u2212212.27 kJ per mole of reaction). The positive cell potential and negative free energy confirm the reaction is spontaneous under standard conditions.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to Use the Calculator<\/h2>\n<ol>\n<li>Enter the <strong>Cathode Potential (E\u00b0cat)<\/strong> \u2014 the standard reduction potential of the half-reaction where reduction occurs. For the default example this is +0.34 V (Cu\u00b2\u207a + 2e\u207b \u2192 Cu).<\/li>\n<li>Enter the <strong>Anode Potential (E\u00b0an)<\/strong> \u2014 the standard reduction potential of the half-reaction where oxidation occurs, entered with the sign found in tables. Do not flip the sign yourself; the subtraction in the formula handles that. For the default example this is \u22120.76 V (Zn\u00b2\u207a + 2e\u207b \u2192 Zn).<\/li>\n<li>Read the <strong>Standard Cell Potential<\/strong> in volts, along with the spontaneity verdict, the free energy per mole of electrons, and a step-by-step breakdown of the calculation.<\/li>\n<li>If the result is negative, the calculator tells you what the potential would be with the electrodes swapped \u2014 the half-cell with the higher reduction potential is always the cathode of a spontaneous cell.<\/li>\n<\/ol>\n<h2>What Is Standard Cell Potential?<\/h2>\n<p>The standard cell potential \\(E\u00b0_{cell}\\) is the maximum voltage an electrochemical cell can deliver when both half-cells operate under standard conditions: 25 \u00b0C (298.15 K), 1 M concentrations of all dissolved species, and 1 atm (1 bar) gas pressures. It measures the tendency of the overall cell reaction to move electrons from the anode to the cathode, and every standard potential is measured relative to the standard hydrogen electrode (SHE), which is assigned exactly 0 V by convention.<\/p>\n<p>The key rule is simple: both potentials must be entered as <em>standard reduction potentials<\/em> taken directly from a table, with their original signs. The cell potential is then just the cathode value minus the anode value. Many students make the mistake of manually reversing the sign of the anode potential before using it \u2014 this double-counts the reversal, because subtracting a reduction potential is mathematically identical to adding its oxidation potential.<\/p>\n<p>The sign of \\(E\u00b0_{cell}\\) tells you the direction of the reaction. A positive value means the reaction is spontaneous as written: the cell is galvanic (voltaic) and produces electrical work, with \\(\\Delta G\u00b0 &lt; 0\\). A negative value means the reaction is non-spontaneous and would require an external power source \u2014 an electrolytic cell. If the value is exactly zero, the two half-cells are identical and the cell is at equilibrium.<\/p>\n<p>Two properties are worth remembering. First, \\(E\u00b0_{cell}\\) is independent of stoichiometry: multiplying a half-reaction by any factor does not change its potential, because a potential is an intensive quantity (energy per charge), not an extensive one. Second, \\(E\u00b0_{cell}\\) relates to the equilibrium constant through \\(\\log K = nE\u00b0_{cell}\/0.0592\\) at 25 \u00b0C, so even modest voltages correspond to very large equilibrium constants \u2014 the Daniell cell's 1.10 V corresponds to \\(K \\approx 10^{37}\\) for n = 2.<\/p>\n<h2>Common Standard Reduction Potentials (25 \u00b0C)<\/h2>\n<table>\n<thead>\n<tr>\n<th>Half-reaction<\/th>\n<th>E\u00b0 (V)<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>F\u2082 + 2e\u207b \u2192 2F\u207b<\/td>\n<td>+2.87<\/td>\n<\/tr>\n<tr>\n<td>MnO\u2084\u207b + 8H\u207a + 5e\u207b \u2192 Mn\u00b2\u207a + 4H\u2082O<\/td>\n<td>+1.51<\/td>\n<\/tr>\n<tr>\n<td>Cl\u2082 + 2e\u207b \u2192 2Cl\u207b<\/td>\n<td>+1.36<\/td>\n<\/tr>\n<tr>\n<td>Ag\u207a + e\u207b \u2192 Ag<\/td>\n<td>+0.80<\/td>\n<\/tr>\n<tr>\n<td>Fe\u00b3\u207a + e\u207b \u2192 Fe\u00b2\u207a<\/td>\n<td>+0.77<\/td>\n<\/tr>\n<tr>\n<td>Cu\u00b2\u207a + 2e\u207b \u2192 Cu<\/td>\n<td>+0.34<\/td>\n<\/tr>\n<tr>\n<td>2H\u207a + 2e\u207b \u2192 H\u2082 (SHE)<\/td>\n<td>0.00<\/td>\n<\/tr>\n<tr>\n<td>Pb\u00b2\u207a + 2e\u207b \u2192 Pb<\/td>\n<td>\u22120.13<\/td>\n<\/tr>\n<tr>\n<td>Ni\u00b2\u207a + 2e\u207b \u2192 Ni<\/td>\n<td>\u22120.26<\/td>\n<\/tr>\n<tr>\n<td>Fe\u00b2\u207a + 2e\u207b \u2192 Fe<\/td>\n<td>\u22120.44<\/td>\n<\/tr>\n<tr>\n<td>Zn\u00b2\u207a + 2e\u207b \u2192 Zn<\/td>\n<td>\u22120.76<\/td>\n<\/tr>\n<tr>\n<td>2H\u2082O + 2e\u207b \u2192 H\u2082 + 2OH\u207b<\/td>\n<td>\u22120.83<\/td>\n<\/tr>\n<tr>\n<td>Al\u00b3\u207a + 3e\u207b \u2192 Al<\/td>\n<td>\u22121.66<\/td>\n<\/tr>\n<tr>\n<td>Mg\u00b2\u207a + 2e\u207b \u2192 Mg<\/td>\n<td>\u22122.37<\/td>\n<\/tr>\n<tr>\n<td>Li\u207a + e\u207b \u2192 Li<\/td>\n<td>\u22123.04<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h2>Assumptions, Limitations and Tips<\/h2>\n<ul>\n<li><strong>Standard conditions only.<\/strong> The result applies at 25 \u00b0C, 1 M activities and 1 atm gas pressures. At other concentrations, the actual voltage follows the Nernst equation and can differ substantially from \\(E\u00b0_{cell}\\).<\/li>\n<li><strong>Activities, not concentrations.<\/strong> In concentrated or ionic solutions, effective activities deviate from molar concentrations; the tabulated potentials assume ideal behaviour.<\/li>\n<li><strong>Junction potentials neglected.<\/strong> Real cells include small liquid-junction voltages at the salt bridge (typically a few millivolts) that this calculation ignores.<\/li>\n<li><strong>The free energy is given per mole of electrons.<\/strong> To obtain \\(\\Delta G\u00b0\\) for the full balanced reaction, multiply the displayed value by the number of electrons transferred, \\(n\\).<\/li>\n<li><strong>Signs matter.<\/strong> Always enter the tabulated signs. A common error is entering +0.76 V for the zinc anode, which would give \u22120.42 V instead of +1.10 V for the Daniell cell.<\/li>\n<li><strong>Electrode roles are determined by the potentials.<\/strong> In any galvanic cell the half-reaction with the more positive (higher) reduction potential runs as reduction at the cathode; the other runs as oxidation at the anode.<\/li>\n<\/ul>\n<h2>Related Calculators<\/h2>\n<p>Electrochemistry pairs naturally with other thermodynamic tools: to combine reaction energies from tabulated values, see the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/hesss-law-calculator\/\">Hess's Law calculator<\/a>; for solubility-driven potentials of sparingly soluble salts, try the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/solubility-product-ksp-calculator\/\">Solubility Product (Ksp) calculator<\/a>; and to study temperature effects on equilibrium constants, use the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/van-t-hoff-equation-calculator\/\">Van 't Hoff Equation calculator<\/a>.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Enter the standard reduction potentials of the cathode and anode to get the standard cell potential E\u00b0cell, the spontaneity verdict, and the free energy change \u0394G\u00b0 per mole of electrons.<\/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-66889","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\/66889","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=66889"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66889\/revisions"}],"predecessor-version":[{"id":66890,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66889\/revisions\/66890"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66889"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66889"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66889"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}