{"id":241142,"date":"2025-07-03T15:17:54","date_gmt":"2025-07-03T15:17:54","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=241142"},"modified":"2025-07-03T15:17:55","modified_gmt":"2025-07-03T15:17:55","slug":"calculate-the-heat-required-to-warm-16-9-g-of-water-from-87-4-c-to-100-0-c","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/03\/calculate-the-heat-required-to-warm-16-9-g-of-water-from-87-4-c-to-100-0-c\/","title":{"rendered":"Calculate the heat required to warm 16.9 g of water from 87.4 C to 100.0 C"},"content":{"rendered":"\n<p>Calculate the heat required to warm 16.9 g of water from 87.4 C to 100.0 C.<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To calculate the heat required to warm water, we use the specific heat capacity formula: Q=mc\u0394TQ = mc\\Delta T<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>QQ is the heat energy (in joules, J),<\/li>\n\n\n\n<li>mm is the mass of the substance (in grams, g),<\/li>\n\n\n\n<li>cc is the specific heat capacity of the substance (for water, it is 4.18\u2009J\/g\u00b0C4.18 \\, \\text{J\/g\u00b0C}),<\/li>\n\n\n\n<li>\u0394T\\Delta T is the change in temperature (in \u00b0C).<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Identify the given values<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Mass m=16.9\u2009gm = 16.9 \\, \\text{g},<\/li>\n\n\n\n<li>Specific heat capacity c=4.18\u2009J\/g\u00b0Cc = 4.18 \\, \\text{J\/g\u00b0C},<\/li>\n\n\n\n<li>Initial temperature T1=87.4\u00b0CT_1 = 87.4\u00b0C,<\/li>\n\n\n\n<li>Final temperature T2=100.0\u00b0CT_2 = 100.0\u00b0C.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Calculate the temperature change<\/h3>\n\n\n\n<p>The temperature change \u0394T\\Delta T is: \u0394T=T2\u2212T1=100.0\u00b0C\u221287.4\u00b0C=12.6\u00b0C\\Delta T = T_2 &#8211; T_1 = 100.0\u00b0C &#8211; 87.4\u00b0C = 12.6\u00b0C<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Apply the formula<\/h3>\n\n\n\n<p>Now, substitute the values into the formula: Q=(16.9\u2009g)\u00d7(4.18\u2009J\/g\u00b0C)\u00d7(12.6\u00b0C)Q = (16.9 \\, \\text{g}) \\times (4.18 \\, \\text{J\/g\u00b0C}) \\times (12.6\u00b0C) Q=16.9\u00d74.18\u00d712.6=876.7\u2009JQ = 16.9 \\times 4.18 \\times 12.6 = 876.7 \\, \\text{J}<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Final Answer:<\/h3>\n\n\n\n<p>The heat required to warm 16.9 g of water from 87.4\u00b0C to 100.0\u00b0C is <strong>876.7 J<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>When you heat a substance, the amount of energy required depends on the mass, the specific heat capacity, and the temperature change. The specific heat capacity of water is relatively high, meaning it requires a significant amount of energy to raise its temperature. In this case, a relatively small mass of water (16.9 g) requires 876.7 joules of energy to be warmed by 12.6\u00b0C. This calculation assumes there is no phase change (such as water turning into steam), which is the case here since the temperature does not exceed 100\u00b0C.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the heat required to warm 16.9 g of water from 87.4 C to 100.0 C. The correct answer and explanation is: To calculate the heat required to warm water, we use the specific heat capacity formula: Q=mc\u0394TQ = mc\\Delta T Where: Step 1: Identify the given values Step 2: Calculate the temperature change The [&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-241142","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/241142","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=241142"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/241142\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=241142"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=241142"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=241142"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}