{"id":66475,"date":"2026-10-06T17:20:09","date_gmt":"2026-10-06T14:20:09","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66475"},"modified":"2026-10-06T17:20:09","modified_gmt":"2026-10-06T14:20:09","slug":"electrolysis-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/electrolysis-calculator\/","title":{"rendered":"Electrolysis 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\">Electrolysis Deposit from Faraday&#039;s Law<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66475\" data-favorite-title=\"Electrolysis\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/electrolysis-calculator\/\" data-favorite-excerpt=\"Calculate the mass deposited or produced in an electrolysis cell using Faraday&#039;s law. Enter the current, time, molar mass, and electrons transferred per formula unit to get charge, moles, and deposited mass.\" 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\/electrolysis-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66475\" data-post=\"66475\"><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\">Current<\/label><div class=\"term\">I<\/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=\"text\" name=\"current\" id=\"field-1\" aria-describedby=\"calc-info-1\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 2\" min=\"0\" value=\"2\"\/><div class=\"grid grid-cols-1\"><select id=\"field-2\" name=\"unit\" aria-label=\"Unit\"><option value=\"a\" selected>A<\/option><option value=\"ma\">mA<\/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\">Electric current through the cell<\/small><\/div><div class=\"field has-term\" id=\"input-2\"><label for=\"field-3\">Time<\/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=\"text\" name=\"time\" id=\"field-3\" aria-describedby=\"calc-info-3\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 30\" min=\"0\" value=\"30\"\/><div class=\"grid grid-cols-1\"><select id=\"field-4\" name=\"unit\" aria-label=\"Unit\"><option value=\"s\">s<\/option><option value=\"min\" selected>min<\/option><option value=\"h\">h<\/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\">Duration the current flows<\/small><\/div><div class=\"field has-term\" id=\"input-3\"><label for=\"field-5\">Molar Mass<\/label><div class=\"term\">M<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"molar_mass\" id=\"field-5\" aria-describedby=\"calc-unit-5 calc-info-5\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 63.546\" min=\"0\" value=\"63.546\"\/><div class=\"unit\" id=\"calc-unit-5\">g\/mol<\/div><small id=\"calc-info-5\">Molecular weight of the product (e.g. 63.546 for Cu, 107.868 for Ag)<\/small><\/div><div class=\"field has-term\" id=\"input-4\"><label for=\"field-6\">Electrons per Product Unit<\/label><div class=\"term\">z<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"electrons_per_product_unit\" id=\"field-6\" aria-describedby=\"calc-info-6\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 2\" min=\"0.001\" value=\"2\"\/><small id=\"calc-info-6\">Electrons transferred per formula unit of product: 1 for Ag\u207a \u2192 Ag, 2 for Cu\u00b2\u207a \u2192 Cu, 3 for Al\u00b3\u207a \u2192 Al<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66475\">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> Electrolysis Results<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Electric Charge<\/span><span class=\"result-term\">Q<\/span><\/span><span class=\"field-value\" id=\"result-1\" data-unit=\"C\"><\/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>Moles of Product<\/span><span class=\"result-term\">n<\/span><\/span><span class=\"field-value\" id=\"result-2\" data-unit=\"mol\"><\/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>Theoretical Deposited Mass<\/span><span class=\"result-term\">m<\/span><\/span><span class=\"field-value\" id=\"result-3\" data-unit=\"g\"><\/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=\"66475\" 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>Electrolysis 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\\[ Q = I \\cdot t \\\\ n = \\frac{Q}{z \\cdot F} \\\\ m = n \\cdot M = \\frac{I \\cdot t \\cdot M}{z \\cdot F} \\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(Q\\) \u2014 electric charge passed through the cell (coulombs)<\/li>\n<li>\\(I\\) \u2014 current (amperes)<\/li>\n<li>\\(t\\) \u2014 time the current flows (seconds)<\/li>\n<li>\\(z\\) \u2014 electrons transferred per formula unit of product<\/li>\n<li>\\(F\\) \u2014 Faraday constant, \\(96\\,485.33\\ \\text{C\/mol}\\)<\/li>\n<li>\\(n\\) \u2014 moles of product formed (mol)<\/li>\n<li>\\(M\\) \u2014 molar mass of the product (g\/mol)<\/li>\n<li>\\(m\\) \u2014 theoretical deposited mass (g)<\/li>\n<\/ul>\n<p>These equations express Faraday's laws of electrolysis: the amount of a substance produced at an electrode is directly proportional to the quantity of electric charge passed through the cell.<\/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>Electrolysis \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> a copper strip is electroplated in a CuSO<sub>4<\/sub> bath. A current of 2 A flows for 30 minutes. Copper (\\(M = 63.546\\) g\/mol) deposits from Cu<sup>2+<\/sup> ions, so \\(z = 2\\).<\/p>\n<p>\\[ Q = I \\cdot t = 2\\ \\text{A} \\times 1800\\ \\text{s} = 3600\\ \\text{C} \\]<\/p>\n<p>\\[ n = \\frac{Q}{z \\cdot F} = \\frac{3600}{2 \\times 96\\,485.33} = 0.018656\\ \\text{mol} \\]<\/p>\n<p>\\[ m = n \\cdot M = 0.018656 \\times 63.546 \\approx 1.1855\\ \\text{g} \\]<\/p>\n<p><strong>Result:<\/strong> the charge passed is 3600 C, producing 0.018656 mol of copper, which corresponds to approximately 1.1855 g of copper deposited on the electrode.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to Use the Electrorolysis Calculator<\/h2>\n<ol>\n<li>Enter the <strong>Current<\/strong> flowing through the cell and select the unit (A or mA) from the dropdown.<\/li>\n<li>Enter the <strong>Time<\/strong> the current flows and choose seconds, minutes, or hours.<\/li>\n<li>Enter the <strong>Molar Mass<\/strong> of the deposited or produced substance in g\/mol (e.g. 63.546 for Cu, 107.868 for Ag).<\/li>\n<li>Enter the number of <strong>Electrons per Product Unit<\/strong> (\\(z\\)): 1 for Ag<sup>+<\/sup> \u2192 Ag, 2 for Cu<sup>2+<\/sup> \u2192 Cu, 3 for Al<sup>3+<\/sup> \u2192 Al.<\/li>\n<li>Read the results: the <strong>Electric Charge<\/strong> in coulombs, the <strong>Moles of Product<\/strong> formed, and the <strong>Theoretical Deposited Mass<\/strong> in grams.<\/li>\n<\/ol>\n<h2>What Is Electrolysis?<\/h2>\n<p>Electrolysis is a chemical process that uses direct electric current to drive a non-spontaneous redox reaction. Inside an electrolytic cell, ions migrate toward electrodes: positive ions (cations) gain electrons at the cathode, while negative ions (anions) lose electrons at the anode. This is how metals are electroplated, water is split into hydrogen and oxygen, and pure aluminum and chlorine are industrially produced.<\/p>\n<p>The quantitative relationship between electricity and chemical change is described by Faraday's laws. The first law states that the mass of a substance altered at an electrode is proportional to the quantity of charge passed. The second law states that for the same charge, the amounts of different substances produced are proportional to their equivalent weights (molar mass divided by \\(z\\)). Together, they give the single equation implemented in this calculator: \\(m = \\frac{I \\cdot t \\cdot M}{z \\cdot F}\\).<\/p>\n<p>The three results build on each other. The charge \\(Q\\) tells you how much electricity actually flowed. Dividing by \\(z \\cdot F\\) converts that charge into moles of product \u2014 one mole of electrons (96,485 C) reduces one mole of singly charged ions, half a mole of doubly charged ions, and so on. Multiplying by the molar mass finally gives the mass you would expect to deposit, in grams.<\/p>\n<p>If you want to compare the calculated theoretical deposit with what you actually measured on an electrode, you can express the outcome as a percentage using the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/percent-yield-calculator\/\">Percent Yield calculator<\/a>. To understand which species reacts at each electrode, the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/balancing-redox-reactions-2\/\">Balancing Redox Reactions calculator<\/a> helps you work out the half-reactions and the value of \\(z\\).<\/p>\n<h2>Common Values of z and M<\/h2>\n<table>\n<thead>\n<tr>\n<th>Half-reaction<\/th>\n<th>z<\/th>\n<th>M (g\/mol)<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>Ag<sup>+<\/sup> + e<sup>\u2212<\/sup> \u2192 Ag<\/td>\n<td>1<\/td>\n<td>107.868<\/td>\n<\/tr>\n<tr>\n<td>Cu<sup>2+<\/sup> + 2e<sup>\u2212<\/sup> \u2192 Cu<\/td>\n<td>2<\/td>\n<td>63.546<\/td>\n<\/tr>\n<tr>\n<td>Zn<sup>2+<\/sup> + 2e<sup>\u2212<\/sup> \u2192 Zn<\/td>\n<td>2<\/td>\n<td>65.38<\/td>\n<\/tr>\n<tr>\n<td>Ni<sup>2+<\/sup> + 2e<sup>\u2212<\/sup> \u2192 Ni<\/td>\n<td>2<\/td>\n<td>58.693<\/td>\n<\/tr>\n<tr>\n<td>Al<sup>3+<\/sup> + 3e<sup>\u2212<\/sup> \u2192 Al<\/td>\n<td>3<\/td>\n<td>26.982<\/td>\n<\/tr>\n<tr>\n<td>2H<sup>+<\/sup> + 2e<sup>\u2212<\/sup> \u2192 H<sub>2<\/sub><\/td>\n<td>2<\/td>\n<td>2.016<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h2>Assumptions and Limitations<\/h2>\n<ul>\n<li><strong>100% current efficiency:<\/strong> the calculator assumes every electron goes into the target reaction. In real cells, side reactions (such as hydrogen evolution) consume part of the current, so the actual deposit is smaller. Divide the theoretical mass by the efficiency factor if you know it.<\/li>\n<li><strong>Constant current:<\/strong> the formula applies to steady direct current. For varying current, integrate \\(I\\) over time to find \\(Q\\) first, then use \\(n = Q\/(zF)\\).<\/li>\n<li><strong>One product per electrode:<\/strong> if several ions compete at the same electrode, only the favored reaction proceeds appreciably, and you should apply the calculation to that reaction only.<\/li>\n<li><strong>Gas products:<\/strong> for gases such as H<sub>2<\/sub> or O<sub>2<\/sub>, the same equations give moles; convert to volume with the ideal gas law or molar volume at your conditions (see the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/combined-gas-law\/\">Combined Gas Law calculator<\/a>).<\/li>\n<li><strong>Sign convention:<\/strong> enter the magnitude of the current. The direction of the reaction (deposition or dissolution) depends on which electrode you consider.<\/li>\n<\/ul>\n<h2>Practical Tips<\/h2>\n<ul>\n<li>For quick mental checks, remember that 1 mole of electrons \u2248 96,500 C, so 1 A for about 26.8 hours delivers one faraday of charge.<\/li>\n<li>In electroplating shops, mass is often converted to coating thickness: divide the deposited mass by the plated area and the metal's density.<\/li>\n<li>When a solution concentration is needed instead of a deposit mass \u2014 for example, after dissolving the product \u2014 the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/molarity-calculator\/\">Molarity calculator<\/a> or the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/normality-calculator\/\">Normality calculator<\/a> can finish the analysis.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the mass deposited or produced in an electrolysis cell using Faraday's law. Enter the current, time, molar mass, and electrons transferred per formula unit to get charge, moles, and deposited mass.<\/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-66475","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\/66475","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=66475"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66475\/revisions"}],"predecessor-version":[{"id":66477,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66475\/revisions\/66477"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66475"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66475"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66475"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}