{"id":204309,"date":"2025-03-21T17:17:33","date_gmt":"2025-03-21T17:17:33","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=204309"},"modified":"2025-03-21T17:17:34","modified_gmt":"2025-03-21T17:17:34","slug":"the-specific-heat-of-ethylene-glycol-is-2-42-j-g-k","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/21\/the-specific-heat-of-ethylene-glycol-is-2-42-j-g-k\/","title":{"rendered":"The specific heat of ethylene glycol is 2.42 J\/g-K"},"content":{"rendered":"\n<p>The specific heat of ethylene glycol is 2.42 J\/g-K. <\/p>\n\n\n\n<p>How many J of heat are needed to raise the temperature of 62.0 g of ethylene glycol from 13.1 degrees celsius to 40.5 degrees celsius?<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>To calculate the heat required to raise the temperature of ethylene glycol, we use the heat equation:<\/p>\n\n\n\n<p>[<br>q = mc\\Delta T<br>]<\/p>\n\n\n\n<p>where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( q ) = heat energy (J)<\/li>\n\n\n\n<li>( m ) = mass of the substance (g)<\/li>\n\n\n\n<li>( c ) = specific heat capacity (J\/g\u00b7K)<\/li>\n\n\n\n<li>( \\Delta T ) = change in temperature (\u00b0C or K)<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Identify Given Values<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( m = 62.0 ) g<\/li>\n\n\n\n<li>( c = 2.42 ) J\/g\u00b7K<\/li>\n\n\n\n<li>Initial temperature ( T_i = 13.1 )\u00b0C<\/li>\n\n\n\n<li>Final temperature ( T_f = 40.5 )\u00b0C<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Calculate Temperature Change<\/h3>\n\n\n\n<p>[<br>\\Delta T = T_f &#8211; T_i = 40.5 &#8211; 13.1 = 27.4 \\text{\u00b0C}<br>]<\/p>\n\n\n\n<p>Since the Celsius and Kelvin scales have the same interval size, we can use \u00b0C directly in the equation.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Calculate Heat Energy<\/h3>\n\n\n\n<p>[<br>q = (62.0 \\text{ g}) \\times (2.42 \\text{ J\/g\u00b7K}) \\times (27.4 \\text{ K})<br>]<\/p>\n\n\n\n<p>[<br>q = 4107.5 \\text{ J}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 4: Round to Significant Figures<\/h3>\n\n\n\n<p>Since the given values have three significant figures, we round the final answer to three significant figures:<\/p>\n\n\n\n<p>[<br>q = 4110 \\text{ J}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation<\/h3>\n\n\n\n<p>The specific heat capacity of a substance indicates how much heat energy is needed to raise the temperature of 1 gram of that substance by 1 K (or 1 \u00b0C). Ethylene glycol has a specific heat of 2.42 J\/g\u00b7K, meaning it requires 2.42 joules of energy to raise the temperature of 1 gram of ethylene glycol by 1\u00b0C.<\/p>\n\n\n\n<p>In this case, 62.0 g of ethylene glycol undergoes a temperature increase of 27.4\u00b0C. Since energy is proportional to mass and temperature change, we use the formula ( q = mc\\Delta T ) to determine that 4110 J of heat energy is needed.<\/p>\n\n\n\n<p>This calculation is useful in real-life applications like engine coolants, where ethylene glycol is commonly used due to its high specific heat, helping regulate engine temperature efficiently.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>The specific heat of ethylene glycol is 2.42 J\/g-K. How many J of heat are needed to raise the temperature of 62.0 g of ethylene glycol from 13.1 degrees celsius to 40.5 degrees celsius? The correct answer and explanation is : To calculate the heat required to raise the temperature of ethylene glycol, we use [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-204309","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/204309","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=204309"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/204309\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=204309"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=204309"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=204309"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}