{"id":183642,"date":"2025-01-16T18:56:19","date_gmt":"2025-01-16T18:56:19","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=183642"},"modified":"2025-01-16T18:56:21","modified_gmt":"2025-01-16T18:56:21","slug":"the-specific-heat-capacity-of-solid-zinc-is-0-388-j-g","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/16\/the-specific-heat-capacity-of-solid-zinc-is-0-388-j-g\/","title":{"rendered":"The specific heat capacity of solid zinc is 0.388 J g"},"content":{"rendered":"\n<p>The specific heat capacity of solid zinc is 0.388 J g<\/p>\n\n\n\n<p>\u00b0<\/p>\n\n\n\n<p>C (a) Determine the amount of heat energy that is a5sociated with heating a 11.0-g sample of solid zinc from 23.5<\/p>\n\n\n\n<p>\u00b0<\/p>\n\n\n\n<p>C to 36.5<\/p>\n\n\n\n<p>\u00b0<\/p>\n\n\n\n<p>C. (b) Caleulate the final temperature teached when 284 J of heat is added to a 20.8 g sample of solid zinc initially at 23.5%C<\/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><strong>(a) Determining the Heat Energy for Heating Zinc<\/strong><\/p>\n\n\n\n<p>To calculate the heat energy required to heat a 11.0-g sample of solid zinc from 23.5\u00b0C to 36.5\u00b0C, we use the formula:<\/p>\n\n\n\n<p>[ Q = m \\times c \\times \\Delta T ]<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( Q ) is the heat energy (in joules)<\/li>\n\n\n\n<li>( m ) is the mass of the zinc sample (in grams)<\/li>\n\n\n\n<li>( c ) is the specific heat capacity of zinc (in J\/g\u00b0C)<\/li>\n\n\n\n<li>( \\Delta T ) is the change in temperature (in \u00b0C)<\/li>\n<\/ul>\n\n\n\n<p>Given:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( m = 11.0 \\, \\text{g} )<\/li>\n\n\n\n<li>( c = 0.388 \\, \\text{J\/g\u00b0C} )<\/li>\n\n\n\n<li>( \\Delta T = 36.5\u00b0C &#8211; 23.5\u00b0C = 13.0\u00b0C )<\/li>\n<\/ul>\n\n\n\n<p>Substituting these values into the formula:<\/p>\n\n\n\n<p>[ Q = 11.0 \\, \\text{g} \\times 0.388 \\, \\text{J\/g\u00b0C} \\times 13.0\u00b0C ]<\/p>\n\n\n\n<p>Calculating:<\/p>\n\n\n\n<p>Therefore, the heat energy required is approximately 55.48 joules.<\/p>\n\n\n\n<p><strong>(b) Calculating the Final Temperature After Adding Heat<\/strong><\/p>\n\n\n\n<p>To find the final temperature when 284 J of heat is added to a 20.8-g sample of solid zinc initially at 23.5\u00b0C, we rearrange the heat energy formula to solve for the final temperature (( T_f )):<\/p>\n\n\n\n<p>[ Q = m \\times c \\times (T_f &#8211; T_i) ]<\/p>\n\n\n\n<p>Rearranging to solve for ( T_f ):<\/p>\n\n\n\n<p>[ T_f = \\frac{Q}{m \\times c} + T_i ]<\/p>\n\n\n\n<p>Given:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( Q = 284 \\, \\text{J} )<\/li>\n\n\n\n<li>( m = 20.8 \\, \\text{g} )<\/li>\n\n\n\n<li>( c = 0.388 \\, \\text{J\/g\u00b0C} )<\/li>\n\n\n\n<li>( T_i = 23.5\u00b0C )<\/li>\n<\/ul>\n\n\n\n<p>Substituting these values into the equation:<\/p>\n\n\n\n<p>[ T_f = \\frac{284 \\, \\text{J}}{20.8 \\, \\text{g} \\times 0.388 \\, \\text{J\/g\u00b0C}} + 23.5\u00b0C ]<\/p>\n\n\n\n<p>Calculating:<\/p>\n\n\n\n<p>Therefore, the final temperature reached is approximately 58.69\u00b0C.<\/p>\n\n\n\n<p><strong>Explanation<\/strong><\/p>\n\n\n\n<p>The specific heat capacity (( c )) of a substance indicates how much heat energy is required to raise the temperature of a unit mass of the substance by one degree Celsius. For zinc, this value is 0.388 J\/g\u00b0C.<\/p>\n\n\n\n<p>In part (a), we calculated the heat energy required to heat a 11.0-g sample of zinc from 23.5\u00b0C to 36.5\u00b0C. By applying the formula ( Q = m \\times c \\times \\Delta T ), we determined that 55.48 joules of heat energy are needed.<\/p>\n\n\n\n<p>In part (b), we calculated the final temperature after adding 284 J of heat to a 20.8-g sample of zinc initially at 23.5\u00b0C. By rearranging the heat energy formula to solve for the final temperature, we found that the final temperature reached is approximately 58.69\u00b0C.<\/p>\n\n\n\n<p>These calculations demonstrate how the specific heat capacity of a material influences the amount of heat energy required to change its temperature.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>The specific heat capacity of solid zinc is 0.388 J g \u00b0 C (a) Determine the amount of heat energy that is a5sociated with heating a 11.0-g sample of solid zinc from 23.5 \u00b0 C to 36.5 \u00b0 C. (b) Caleulate the final temperature teached when 284 J of heat is added to a 20.8 [&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-183642","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183642","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=183642"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183642\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=183642"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=183642"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=183642"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}