{"id":191766,"date":"2025-02-16T07:09:30","date_gmt":"2025-02-16T07:09:30","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=191766"},"modified":"2025-02-16T07:09:39","modified_gmt":"2025-02-16T07:09:39","slug":"the-heat-of-combustion-of-propane-c3h8-2220-kj-mol-the-specific-heat-of-copper-is-385j-g-c","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/16\/the-heat-of-combustion-of-propane-c3h8-2220-kj-mol-the-specific-heat-of-copper-is-385j-g-c\/","title":{"rendered":"the heat of combustion of propane C3H8 2220 kj\/mol the specific heat of copper is .385j\/g C"},"content":{"rendered":"\n
the heat of combustion of propane C3H8 2220 kj\/mol the specific heat of copper is .385j\/g C how many grams of propane. must be burned. to raise the temp. of a 10kg block of copper. from 25 C to 65C assuming. nonof the heat is lose of the surrounding<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n
To solve this problem, we need to determine how many grams of propane are required to raise the temperature of a 10 kg block of copper from 25\u00b0C to 65\u00b0C, assuming no heat is lost to the surroundings.<\/p>\n\n\n\n
Step-by-step solution:<\/h3>\n\n\n\n\n
Calculate the heat required to raise the temperature of the copper:<\/strong> The formula for heat is: [ Q = mc\\Delta T ] where:<\/li>\n<\/ol>\n\n\n\n
\n
( Q ) is the heat absorbed (in joules),<\/li>\n\n\n\n
( m ) is the mass of copper (in grams),<\/li>\n\n\n\n
( c ) is the specific heat of copper (in joules per gram per degree Celsius),<\/li>\n\n\n\n
( \\Delta T ) is the change in temperature (in Celsius). Given:<\/li>\n\n\n\n
( c = 0.385 \\, \\text{J\/g\u00b0C} ),<\/li>\n\n\n\n
( \\Delta T = 65\u00b0C – 25\u00b0C = 40\u00b0C ). Substituting these values: [ Q = (10,000 \\, \\text{g}) \\times (0.385 \\, \\text{J\/g\u00b0C}) \\times (40\u00b0C) ] [ Q = 154,000 \\, \\text{J} ] This is the amount of heat needed to raise the temperature of the copper block.<\/li>\n<\/ul>\n\n\n\n\n
Determine the amount of propane needed:<\/strong> The heat of combustion of propane is given as 2220 kJ\/mol. We need to convert this value to joules: [ 2220 \\, \\text{kJ\/mol} = 2,220,000 \\, \\text{J\/mol} ] Now, we calculate how many moles of propane are needed to produce 154,000 J: [ \\text{Moles of propane} = \\frac{\\text{Heat required}}{\\text{Heat of combustion per mole}} = \\frac{154,000 \\, \\text{J}}{2,220,000 \\, \\text{J\/mol}} ] [ \\text{Moles of propane} \\approx 0.0694 \\, \\text{mol} ]<\/li>\n\n\n\n
Convert moles of propane to grams:<\/strong> The molar mass of propane (C\u2083H\u2088) is: [ 3 \\times 12 + 8 \\times 1 = 44 \\, \\text{g\/mol} ] Now, calculate the mass of propane required: [ \\text{Mass of propane} = 0.0694 \\, \\text{mol} \\times 44 \\, \\text{g\/mol} ] [ \\text{Mass of propane} \\approx 3.05 \\, \\text{g} ]<\/li>\n<\/ol>\n\n\n\n
Conclusion:<\/h3>\n\n\n\n
To raise the temperature of a 10 kg block of copper from 25\u00b0C to 65\u00b0C, approximately 3.05 grams<\/strong> of propane must be burned.<\/p>\n\n\n\n
Let me now generate an image illustrating the calculation process.<\/p>\n\n\n\n
Here is the educational diagram illustrating the calculation process for determining the grams of propane required to raise the temperature of the copper block. It shows the steps in a clear and simple manner.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"
the heat of combustion of propane C3H8 2220 kj\/mol the specific heat of copper is .385j\/g C how many grams of propane. must be burned. to raise the temp. of a 10kg block of copper. from 25 C to 65C assuming. nonof the heat is lose of the surrounding The Correct Answer and Explanation is […]<\/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-191766","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191766","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=191766"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191766\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=191766"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=191766"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=191766"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/02\/image-651.png\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"