{"id":2235,"date":"2024-08-04T13:13:23","date_gmt":"2024-08-04T13:13:23","guid":{"rendered":"https:\/\/workhouse.sweetdishy.com\/?p=2235"},"modified":"2024-08-04T13:13:24","modified_gmt":"2024-08-04T13:13:24","slug":"specific-heat","status":"publish","type":"post","link":"https:\/\/workhouse.sweetdishy.com\/index.php\/2024\/08\/04\/specific-heat\/","title":{"rendered":"Specific heat"},"content":{"rendered":"\n<p>The&nbsp;<em>specific heat<\/em>&nbsp;of a substance is the heat energy required to raise the temperature of unit mass of the substance by one degree. In terms of the quantities involved, the specific heat of a substance is the heat energy required to raise the temperature of 1 kg of the material by 1\u00b0C (or K, since they have the same interval on the temperature scale). The units of specific heat are therefore J\/kgK.<\/p>\n\n\n\n<p><a><\/a>Different substances have different specific heats, for instance copper is 390 J\/kgK and cast iron is 500 J\/kgK. In practice this means that if you wish to increase the temperature of a lump of iron it would require more heat energy to do it than if it was a lump of copper of the same mass.<\/p>\n\n\n\n<p><a><\/a>Alternatively, you could say the iron \u2018soaks up\u2019 more heat energy for a given rise in temperature.<\/p>\n\n\n\n<p><a><\/a><a><\/a>\u2022&nbsp;<a><\/a>Remember that heat energy is measured in joules or kilojoules (1000 joules).<\/p>\n\n\n\n<p><a><\/a>\u2022&nbsp;<a><\/a>The only difference between the kelvin and the centigrade temperature scales is where they start from. Kelvin starts at \u2212273 (absolute zero) and centigrade starts at 0. A degree change is the same for each.<\/p>\n\n\n\n<p><a><\/a>The equation for calculating heat energy required to heat a solid is therefore the mass to be heated multiplied by the specific heat of the substance,&nbsp;<em>c<\/em>, available in tables, multiplied by the number of degrees rise in temperature, \u03b4<em>T<\/em>.<\/p>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/learning.oreilly.com\/api\/v2\/epubs\/urn:orm:book:9780750652131\/files\/images\/B9780750652131500027_si1.gif\" alt=\"image\"\/><\/figure>\n\n\n\n<p>Putting in the units,<\/p>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/learning.oreilly.com\/api\/v2\/epubs\/urn:orm:book:9780750652131\/files\/images\/B9780750652131500027_si2.gif\" alt=\"image\"\/><\/figure>\n\n\n\n<p>Note that on the right-hand side, the kg and K terms cancel to leave kJ. It is useful to do a units check on all formulas you use.<\/p>\n\n\n\n<p>The boiler in a canteen contains 6 kg of water at 20\u00b0C. How much heat energy is required to raise the temperature of the water to 100\u00b0C? Specific heat of water = 4190 J\/kgK.<\/p>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/learning.oreilly.com\/api\/v2\/epubs\/urn:orm:book:9780750652131\/files\/images\/B9780750652131500027_si3.gif\" alt=\"image\"\/><\/figure>\n\n\n\n<p>Example 2.1.2<\/p>\n\n\n\n<p><a><\/a><a><\/a>How many kilograms of copper can be raised from 15\u00b0C to 60\u00b0C by the absorption of 80 kJ of heat energy? Specific heat of copper = 390 kJ\/kgK.<\/p>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/learning.oreilly.com\/api\/v2\/epubs\/urn:orm:book:9780750652131\/files\/images\/B9780750652131500027_si4.gif\" alt=\"image\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>The&nbsp;specific heat&nbsp;of a substance is the heat energy required to raise the temperature of unit mass of the substance by one degree. In terms of the quantities involved, the specific heat of a substance is the heat energy required to raise the temperature of 1 kg of the material by 1\u00b0C (or K, since they [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":2236,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[373],"tags":[],"class_list":["post-2235","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-thermodynamics"],"jetpack_featured_media_url":"https:\/\/workhouse.sweetdishy.com\/wp-content\/uploads\/2024\/08\/download-22.png","_links":{"self":[{"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/posts\/2235","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/comments?post=2235"}],"version-history":[{"count":1,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/posts\/2235\/revisions"}],"predecessor-version":[{"id":2237,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/posts\/2235\/revisions\/2237"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/media\/2236"}],"wp:attachment":[{"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/media?parent=2235"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/categories?post=2235"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/tags?post=2235"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}