{"id":155369,"date":"2024-10-16T05:26:34","date_gmt":"2024-10-16T05:26:34","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=155369"},"modified":"2024-10-16T05:26:36","modified_gmt":"2024-10-16T05:26:36","slug":"what-is-the-value-of-r-ideal-gas-constant-in-kj-molk","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/10\/16\/what-is-the-value-of-r-ideal-gas-constant-in-kj-molk\/","title":{"rendered":"What is the value of R (ideal gas constant) in kJ\/molK"},"content":{"rendered":"\n<p>What is the value of R (ideal gas constant) in kJ\/molK?<\/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>The ideal gas constant ( R ) has a value of <strong>8.314 kJ\/(mol\u00b7K)<\/strong>. This constant plays a crucial role in thermodynamics, particularly in the Ideal Gas Law, which is expressed as:<\/p>\n\n\n\n<p>[<br>PV = nRT<br>]<\/p>\n\n\n\n<p>where ( P ) is the pressure of the gas, ( V ) is its volume, ( n ) is the number of moles, ( R ) is the ideal gas constant, and ( T ) is the temperature in Kelvin.<\/p>\n\n\n\n<p>To understand why ( R ) is expressed in kJ\/(mol\u00b7K), we can break it down:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Units<\/strong>: The ideal gas constant links pressure, volume, temperature, and the amount of substance (in moles). The common units of pressure (e.g., atm, Pa), volume (e.g., L, m\u00b3), and temperature (K) must be consistent for the equation to hold true. The value of ( R ) in different unit systems varies; for example, in L\u00b7atm\/(K\u00b7mol), ( R ) equals 0.0821 L\u00b7atm\/(K\u00b7mol).<\/li>\n\n\n\n<li><strong>Energy Relationship<\/strong>: The use of kJ relates to the concept of energy. In thermodynamic processes, especially those involving gases, we often deal with energy changes. The value of ( R ) in kJ\/(mol\u00b7K) provides a convenient way to relate the heat exchanged in a system to the changes in temperature and the amount of substance involved.<\/li>\n\n\n\n<li><strong>Applications<\/strong>: The ideal gas law and the constant ( R ) are foundational in various fields, including chemistry, physics, and engineering. They are used in calculations involving gas behaviors, chemical reactions, and phase changes, making ( R ) essential for both theoretical and practical applications in science and industry.<\/li>\n<\/ol>\n\n\n\n<p>In summary, ( R = 8.314 \\, \\text{kJ\/(mol\u00b7K)} ) is not only a fundamental constant in the Ideal Gas Law but also serves as a bridge connecting macroscopic gas behaviors to microscopic molecular interactions, facilitating a deeper understanding of gas dynamics.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>What is the value of R (ideal gas constant) in kJ\/molK? The Correct Answer and Explanation is : The ideal gas constant ( R ) has a value of 8.314 kJ\/(mol\u00b7K). This constant plays a crucial role in thermodynamics, particularly in the Ideal Gas Law, which is expressed as: [PV = nRT] where ( P [&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-155369","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/155369","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=155369"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/155369\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=155369"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=155369"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=155369"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}