{"id":66466,"date":"2026-10-06T17:17:43","date_gmt":"2026-10-06T14:17:43","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66466"},"modified":"2026-10-06T17:17:43","modified_gmt":"2026-10-06T14:17:43","slug":"limiting-reactant-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/limiting-reactant-calculator\/","title":{"rendered":"Limiting Reactant 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 Limiting Reactant and Product Yield<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66466\" data-favorite-title=\"Limiting Reactant\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/limiting-reactant-calculator\/\" data-favorite-excerpt=\"Enter the balanced-equation coefficients and available moles of two reactants to find which one is limiting, the maximum product yield, and how much excess reactant is left over.\" aria-label=\"Add to Favorites\" data-favorite-icon=\"icon icon-chemistry\">\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\/limiting-reactant-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66466\" data-post=\"66466\"><fieldset class=\"fieldset-input is-1\"><legend class=\"sr-only\">Input Fields<\/legend><div class=\"is-single field\" id=\"input-1\"><span class=\"font-semibold\">Reactant A<\/span><\/div><div class=\"field\" id=\"input-2\"><label for=\"field-2\">Reactant A Name (optional)<\/label><input type=\"text\" name=\"reactant_a_name_optional\" id=\"field-2\" placeholder=\"e.g. H\u2082\" step=\"any\" value=\"H\u2082\"\/><\/div><div class=\"field has-term\" id=\"input-3\"><label for=\"field-3\">Coefficient of A<\/label><div class=\"term\">a<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"coefficient_of_a\" id=\"field-3\" aria-describedby=\"calc-info-3\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 2\" min=\"0.001\" value=\"2\"\/><small id=\"calc-info-3\">Coefficient in the balanced equation<\/small><\/div><div class=\"field has-term\" id=\"input-4\"><label for=\"field-4\">Moles of A<\/label><div class=\"term\">n(A)<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"moles_of_a\" id=\"field-4\" aria-describedby=\"calc-unit-4\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 5\" min=\"0\" value=\"5\"\/><div class=\"unit\" id=\"calc-unit-4\">mol<\/div><\/div><div class=\"is-single field\" id=\"input-5\"><span class=\"font-semibold\">Reactant B<\/span><\/div><div class=\"field\" id=\"input-6\"><label for=\"field-6\">Reactant B Name (optional)<\/label><input type=\"text\" name=\"reactant_b_name_optional\" id=\"field-6\" placeholder=\"e.g. O\u2082\" step=\"any\" value=\"O\u2082\"\/><\/div><div class=\"field has-term\" id=\"input-7\"><label for=\"field-7\">Coefficient of B<\/label><div class=\"term\">b<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"coefficient_of_b\" id=\"field-7\" aria-describedby=\"calc-info-7\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 1\" min=\"0.001\" value=\"1\"\/><small id=\"calc-info-7\">Coefficient in the balanced equation<\/small><\/div><div class=\"field has-term\" id=\"input-8\"><label for=\"field-8\">Moles of B<\/label><div class=\"term\">n(B)<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"moles_of_b\" id=\"field-8\" aria-describedby=\"calc-unit-8\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 3\" min=\"0\" value=\"3\"\/><div class=\"unit\" id=\"calc-unit-8\">mol<\/div><\/div><div class=\"is-single field\" id=\"input-9\"><span class=\"font-semibold\">Product<\/span><\/div><div class=\"field\" id=\"input-10\"><label for=\"field-10\">Product Name (optional)<\/label><input type=\"text\" name=\"product_name_optional\" id=\"field-10\" placeholder=\"e.g. H\u2082O\" step=\"any\" value=\"H\u2082O\"\/><\/div><div class=\"field has-term\" id=\"input-11\"><label for=\"field-11\">Coefficient of Product<\/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=\"coefficient_of_product\" id=\"field-11\" aria-describedby=\"calc-info-11\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 2\" min=\"0.001\" value=\"2\"\/><small id=\"calc-info-11\">Coefficient of the target product in the balanced equation<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66466\">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> Reaction Analysis<\/h3><div class=\"result-box\"><div class=\"field-result is-column\" id=\"output-1\"><span class=\"field-title\"><span>Limiting Reactant<\/span><\/span><span class=\"field-value\" id=\"result-1\"><\/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>Maximum Product Formed<\/span><span class=\"result-term\">n(product)<\/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 is-column\" id=\"output-3\"><span class=\"field-title\"><span>Excess Reactant<\/span><\/span><span class=\"field-value\" id=\"result-3\"><\/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-4\"><span class=\"field-title\"><span>Excess Reactant Remaining<\/span><\/span><span class=\"field-value\" id=\"result-4\" 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-5\"><span class=\"field-title\"><span>Excess Remaining<\/span><\/span><span class=\"field-value\" id=\"result-5\" data-unit=\"%\"><\/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=\"66466\" 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>Limiting Reactant<\/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\\[ \\xi_A = \\frac{n_A}{a}, \\qquad \\xi_B = \\frac{n_B}{b} \\\\\\ \\xi_{\\min} = \\min\\!\\left( \\frac{n_A}{a},\\ \\frac{n_B}{b} \\right) \\\\\\ n_{\\text{product}} = c \\cdot \\xi_{\\min} \\\\\\ n_{\\text{excess left}} = n_{\\text{excess}} - b_{\\text{excess}} \\cdot \\xi_{\\min} \\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(n_A\\), \\(n_B\\) \u2014 moles of reactant A and reactant B available (mol)<\/li>\n<li>\\(a\\), \\(b\\) \u2014 stoichiometric coefficients of A and B in the balanced equation<\/li>\n<li>\\(c\\) \u2014 stoichiometric coefficient of the product in the balanced equation<\/li>\n<li>\\(\\xi\\) \u2014 the maximum extent of reaction each reactant allows (mol)<\/li>\n<\/ul>\n<p>Each reactant is divided by its coefficient. The reactant with the smaller result is the limiting reactant, because it allows the smaller extent of reaction and runs out first.<\/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>Limiting Reactant \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> hydrogen burns in oxygen according to the balanced equation \\(2H_2 + O_2 \\rightarrow 2H_2O\\). You have 5 mol of \\(H_2\\) and 3 mol of \\(O_2\\). Which reactant is limiting, and how much water forms?<\/p>\n<p>\\[ \\xi_{H_2} = \\frac{5}{2} = 2.5 \\ \\text{mol}, \\qquad \\xi_{O_2} = \\frac{3}{1} = 3 \\ \\text{mol} \\]<\/p>\n<p>Since \\(2.5 &lt; 3\\), the hydrogen runs out first: \\(H_2\\) is the limiting reactant.<\/p>\n<p>\\[ n_{H_2O} = 2 \\times 2.5 = 5 \\ \\text{mol} \\]<\/p>\n<p>Oxygen consumed: \\(1 \\times 2.5 = 2.5\\) mol, so the leftover oxygen is \\(3 - 2.5 = 0.5\\) mol, which is \\(\\frac{0.5}{3} \\times 100 \\approx 16.67\\%\\) of the original amount.<\/p>\n<p><strong>Result:<\/strong> limiting reactant \u2014 \\(H_2\\); maximum product \u2014 5 mol \\(H_2O\\); excess reactant \u2014 \\(O_2\\), with 0.5 mol (16.67%) remaining.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to Use the Limiting Reactant Calculator<\/h2>\n<ol>\n<li>Make sure your chemical equation is balanced first \u2014 the coefficients must reflect the true mole ratios. If needed, use the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/balancing-chemical-equations\/\">Chemical Equation Balancer<\/a>.<\/li>\n<li>Enter the <strong>Reactant A Name<\/strong> (optional, e.g. H\u2082) as a label for the results.<\/li>\n<li>Fill in the <strong>Coefficient of A<\/strong> from the balanced equation and the available <strong>Moles of A<\/strong>.<\/li>\n<li>Repeat the same for <strong>Reactant B<\/strong>: name (optional), <strong>Coefficient of B<\/strong>, and <strong>Moles of B<\/strong>.<\/li>\n<li>Enter the <strong>Product Name<\/strong> (optional) and the <strong>Coefficient of Product<\/strong> from the balanced equation.<\/li>\n<li>Read the results: the <strong>Limiting Reactant<\/strong>, the <strong>Maximum Product Formed<\/strong> in moles, the <strong>Excess Reactant<\/strong>, how many moles of it remain, and the leftover percentage.<\/li>\n<\/ol>\n<h2>What Is a Limiting Reactant?<\/h2>\n<p>In a chemical reaction, reactants are consumed in fixed proportions defined by the stoichiometric coefficients of the balanced equation. In practice, the reactants are rarely supplied in exactly these proportions \u2014 one of them is usually present in a smaller relative amount than the equation demands. That reactant is the <em>limiting reactant<\/em>: once it is fully consumed, the reaction stops, no matter how much of the other reactant is still available.<\/p>\n<p>The reactant left over is the <em>excess reactant<\/em>. The amount of product you can actually obtain is determined entirely by the limiting reactant, not by the total amount of material present. This is why chemists always identify the limiting reactant before predicting a yield: adding more of the excess reactant will not produce any additional product.<\/p>\n<p>A convenient way to compare the two reactants is to divide the available moles of each by its coefficient, giving the maximum extent of reaction \\(\\xi\\). The smaller value wins \u2014 it belongs to the limiting reactant. Multiplying that extent by the product's coefficient \\(c\\) gives the theoretical (maximum) yield. If both extents are equal, the mixture is stoichiometric: both reactants are consumed completely and there is no excess at all.<\/p>\n<h2>Assumptions, Limitations and Practical Tips<\/h2>\n<ul>\n<li><strong>The equation must be balanced.<\/strong> The calculator trusts the coefficients you enter. Wrong coefficients produce a wrong limiting reactant and a wrong yield.<\/li>\n<li><strong>Amounts must be in moles.<\/strong> If your data is in grams, convert it first: divide the mass by the molar mass (see the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/atomic-mass\/\">Atomic Mass<\/a> calculator) or use the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/convert-atoms-to-moles\/\">Convert Atoms to Moles<\/a> calculator for particle counts.<\/li>\n<li><strong>The reaction is assumed to go to completion.<\/strong> The result is a theoretical maximum. Real yields are lower due to incomplete reactions, side reactions, equilibrium limitations and losses during isolation.<\/li>\n<li><strong>Two reactants only.<\/strong> For reactions with three or more reactants, compute \\(n\/a\\) for each; the smallest value identifies the limiting reactant by the same principle.<\/li>\n<li><strong>Zero moles are handled<\/strong> as a special case: a reactant with zero amount is automatically limiting, and no product can form.<\/li>\n<li>For gas-phase problems where amounts are given as volumes at the same temperature and pressure, volume ratios equal mole ratios, so you can enter the volumes directly \u2014 the same logic applies, as described by the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/ideal-gas-law\/\">Ideal Gas Law<\/a>.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Enter the balanced-equation coefficients and available moles of two reactants to find which one is limiting, the maximum product yield, and how much excess reactant is left over.<\/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":[56],"class_list":["post-66466","post","type-post","status-publish","format-standard","hentry","category-chemistry","tag-stoichiometry"],"acf":[],"_links":{"self":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66466","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=66466"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66466\/revisions"}],"predecessor-version":[{"id":66467,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66466\/revisions\/66467"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66466"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66466"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66466"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}