{"id":66486,"date":"2026-10-06T17:28:48","date_gmt":"2026-10-06T14:28:48","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66486"},"modified":"2026-10-06T17:28:48","modified_gmt":"2026-10-06T14:28:48","slug":"calorimetry-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/calorimetry-calculator\/","title":{"rendered":"Calorimetry 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 Heat Absorbed or Released from a Temperature Change<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66486\" data-favorite-title=\"Calorimetry\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/calorimetry-calculator\/\" data-favorite-excerpt=\"Calculate the heat absorbed or released by a substance using Q = mc\u0394T. Enter the mass, specific heat capacity and the initial and final temperatures to get Q in joules, kilojoules and kilocalories.\" 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\/calorimetry-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66486\" data-post=\"66486\"><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\">Mass (m)<\/label><div class=\"term\">m<\/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=\"mass_m\" id=\"field-1\" aria-describedby=\"calc-info-1\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 250\" min=\"0\" value=\"250\"\/><div class=\"grid grid-cols-1\"><select id=\"field-2\" name=\"unit\" aria-label=\"Unit\"><option value=\"g\" selected>g<\/option><option value=\"kg\">kg<\/option><option value=\"lb\">lb<\/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\">Mass of the substance being heated or cooled<\/small><\/div><div class=\"field has-term\" id=\"input-2\"><label for=\"field-3\">Specific Heat Capacity (c)<\/label><div class=\"term\">c<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"specific_heat_capacity_c\" id=\"field-3\" aria-describedby=\"calc-unit-3 calc-info-3\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 4.186\" min=\"0\" value=\"4.186\"\/><div class=\"unit\" id=\"calc-unit-3\">J\/(g\u00b7\u00b0C)<\/div><small id=\"calc-info-3\">Water: 4.186 J\/(g\u00b7\u00b0C); aluminum: 0.900; iron: 0.450<\/small><\/div><div class=\"field has-term\" id=\"input-3\"><label for=\"field-4\">Initial Temperature (T\u2081)<\/label><div class=\"term\">T\u2081<\/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=\"initial_temperature_t\" id=\"field-4\" aria-describedby=\"calc-info-4\" placeholder=\"e.g. 20\" step=\"any\" value=\"20\"\/><div class=\"grid grid-cols-1\"><select id=\"field-5\" name=\"unit\" aria-label=\"Unit\"><option value=\"c\" selected>\u00b0C<\/option><option value=\"f\">\u00b0F<\/option><option value=\"k\">K<\/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-4\">Temperature before heating or cooling<\/small><\/div><div class=\"field has-term\" id=\"input-4\"><label for=\"field-6\">Final Temperature (T\u2082)<\/label><div class=\"term\">T\u2082<\/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=\"final_temperature_t\" id=\"field-6\" aria-describedby=\"calc-info-6\" placeholder=\"e.g. 95\" step=\"any\" value=\"95\"\/><div class=\"grid grid-cols-1\"><select id=\"field-7\" name=\"unit\" aria-label=\"Unit\"><option value=\"c\" selected>\u00b0C<\/option><option value=\"f\">\u00b0F<\/option><option value=\"k\">K<\/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-6\">Temperature after heating or cooling<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66486\">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> Calorimetry Results<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Heat Absorbed or Released<\/span><span class=\"result-term\">Q<\/span><\/span><span class=\"field-value\" id=\"result-1\" data-unit=\"J\"><\/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>Heat Absorbed or Released<\/span><span class=\"result-term\">Q<\/span><\/span><span class=\"field-value\" id=\"result-2\" data-unit=\"kJ\"><\/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>Heat Absorbed or Released<\/span><span class=\"result-term\">Q<\/span><\/span><span class=\"field-value\" id=\"result-3\" data-unit=\"kcal\"><\/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>Direction of Heat Flow<\/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><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=\"66486\" 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>Calorimetry 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 = m \\cdot c \\cdot \\Delta T \\quad \\text{where} \\quad \\Delta T = T_2 - T_1 \\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(Q\\) \u2014 heat absorbed or released (J)<\/li>\n<li>\\(m\\) \u2014 mass of the substance (g)<\/li>\n<li>\\(c\\) \u2014 specific heat capacity, J\/(g\u00b7\u00b0C)<\/li>\n<li>\\(T_1\\) \u2014 initial temperature (\u00b0C)<\/li>\n<li>\\(T_2\\) \u2014 final temperature (\u00b0C)<\/li>\n<li>\\(\\Delta T\\) \u2014 temperature change (\u00b0C)<\/li>\n<\/ul>\n<p>This is the fundamental calorimetry equation: the heat transferred to or from a substance equals its mass times its specific heat capacity times the change in temperature.<\/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>Calorimetry \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> 250 g of water is heated from 20 \u00b0C to 95 \u00b0C. The specific heat capacity of water is 4.186 J\/(g\u00b7\u00b0C).<\/p>\n<p>\\[ \\Delta T = T_2 - T_1 = 95 - 20 = 75\\ \u00b0C \\]<\/p>\n<p>\\[ Q = m \\cdot c \\cdot \\Delta T = 250 \\times 4.186 \\times 75 = 78\\,487.5\\ \\text{J} \\]<\/p>\n<p><strong>Result:<\/strong> \\(Q = 78\\,487.5\\) J \u2248 78.49 kJ \u2248 18.76 kcal. Since \\(Q\\) is positive, the water absorbed this heat and warmed up (endothermic process).<\/p>\n<p>\n\r\n<\/section>\n<h2>How to Use the Calorimetry Calculator<\/h2>\n<ol>\n<li>Enter the <strong>Mass (m)<\/strong> of the substance and choose its unit (g, kg or lb). The calculator converts it to grams internally.<\/li>\n<li>Enter the <strong>Specific Heat Capacity (c)<\/strong> in J\/(g\u00b7\u00b0C). For water use 4.186; other common values are listed in the table below.<\/li>\n<li>Enter the <strong>Initial Temperature (T\u2081)<\/strong> and select its unit (\u00b0C, \u00b0F or K).<\/li>\n<li>Enter the <strong>Final Temperature (T\u2082)<\/strong> and select its unit. The two temperatures may use different units.<\/li>\n<li>Read the results: the heat \\(Q\\) in J, kJ and kcal, plus a statement of the direction of heat flow (absorbed or released).<\/li>\n<\/ol>\n<h2>What Is Calorimetry?<\/h2>\n<p>Calorimetry is the measurement of heat transfer during a physical or chemical process. Whenever a substance warms up, it absorbs energy from its surroundings; whenever it cools down, it releases energy. The instrument used to measure this heat is called a calorimeter, and the same calculation is at the heart of every calorimeter \u2014 from a simple coffee-cup calorimeter in a school lab to a bomb calorimeter used to measure the energy content of foods and fuels.<\/p>\n<p>The key property in the equation is the <strong>specific heat capacity<\/strong> \\(c\\): the amount of heat needed to raise the temperature of 1 gram of a substance by 1 \u00b0C. Water has an unusually high specific heat (4.186 J\/(g\u00b7\u00b0C)), which is why it takes a great deal of energy to heat water and why water is such an effective coolant. Metals, by contrast, heat up and cool down quickly because their specific heats are low.<\/p>\n<p>The sign of \\(Q\\) tells you the direction of energy flow. A <strong>positive<\/strong> \\(Q\\) means the substance gained heat (an endothermic change \u2014 the temperature rose). A <strong>negative<\/strong> \\(Q\\) means the substance lost heat (an exothermic change \u2014 the temperature fell). For example, cooling the same 250 g of water from 95 \u00b0C back to 20 \u00b0C gives \\(Q = -78\\,487.5\\) J: the water releases exactly as much heat as it absorbed.<\/p>\n<p>Because the temperature change is what matters, you only need the <em>difference<\/em> \\(\\Delta T\\). A change of 1 \u00b0C equals a change of 1 K, and a change of 1 \u00b0F equals 5\/9 of a degree Celsius \u2014 the calculator handles all of these conversions automatically, so you can mix units for \\(T_1\\) and \\(T_2\\).<\/p>\n<h2>Specific Heat Capacities of Common Substances<\/h2>\n<table>\n<thead>\n<tr>\n<th>Substance<\/th>\n<th>c, J\/(g\u00b7\u00b0C)<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>Water (liquid, 25 \u00b0C)<\/td>\n<td>4.186<\/td>\n<\/tr>\n<tr>\n<td>Ice (0 \u00b0C)<\/td>\n<td>2.09<\/td>\n<\/tr>\n<tr>\n<td>Steam (100 \u00b0C)<\/td>\n<td>2.01<\/td>\n<\/tr>\n<tr>\n<td>Aluminum<\/td>\n<td>0.900<\/td>\n<\/tr>\n<tr>\n<td>Iron<\/td>\n<td>0.450<\/td>\n<\/tr>\n<tr>\n<td>Copper<\/td>\n<td>0.385<\/td>\n<\/tr>\n<tr>\n<td>Gold<\/td>\n<td>0.129<\/td>\n<\/tr>\n<tr>\n<td>Ethanol<\/td>\n<td>2.44<\/td>\n<\/tr>\n<tr>\n<td>Air (approx.)<\/td>\n<td>1.01<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h2>Assumptions and Limitations<\/h2>\n<ul>\n<li><strong>No phase changes.<\/strong> The formula \\(Q = mc\\Delta T\\) applies only to a change in temperature within one phase. Melting, freezing, boiling or condensation involve latent heat, which must be calculated separately and added to the sensible heat.<\/li>\n<li><strong>Constant specific heat.<\/strong> The value of \\(c\\) actually varies slightly with temperature. For most everyday problems the tabulated value is accurate enough, but for precise work over a wide temperature range use an average or temperature-dependent value.<\/li>\n<li><strong>Heat losses are ignored.<\/strong> In a real experiment some heat leaks into the container or the surroundings. A well-insulated (adiabatic) calorimeter minimises this, and the calorimeter's own heat capacity can be accounted for with a calibration factor.<\/li>\n<li><strong>Units must match.<\/strong> The calculator expects \\(c\\) in J\/(g\u00b7\u00b0C) and converts the mass to grams, so the result is always in joules. If your data uses J\/(kg\u00b7K), divide that value by 1000 before entering it (1 J\/(kg\u00b7K) = 0.001 J\/(g\u00b7\u00b0C)).<\/li>\n<\/ul>\n<h2>Related Calculators<\/h2>\n<p>Calorimetry often appears alongside other chemistry calculations. If you are working on solution stoichiometry, try the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/molarity-calculator\/\">Molarity Calculator<\/a> or the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/molality-calculator\/\">Molality Calculator<\/a>. For reaction energetics, the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/gibbs-free-energy-calculator\/\">Gibbs Free Energy Calculator<\/a> and the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/percent-yield-calculator\/\">Percent Yield Calculator<\/a> may also be useful.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the heat absorbed or released by a substance using Q = mc\u0394T. Enter the mass, specific heat capacity and the initial and final temperatures to get Q in joules, kilojoules and kilocalories.<\/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-66486","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\/66486","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=66486"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66486\/revisions"}],"predecessor-version":[{"id":66487,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66486\/revisions\/66487"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66486"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66486"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66486"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}