{"id":211492,"date":"2025-05-03T21:43:20","date_gmt":"2025-05-03T21:43:20","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=211492"},"modified":"2025-05-03T21:43:22","modified_gmt":"2025-05-03T21:43:22","slug":"in-si-units-the-value-of-the-universal-gas-constant-is","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/03\/in-si-units-the-value-of-the-universal-gas-constant-is\/","title":{"rendered":"In SI units, the value of the universal gas constant is"},"content":{"rendered":"\n<p>In SI units, the value of the universal gas constant is<\/p>\n\n\n\n<p>(a) 0.8314 J\/mole\/K<br>(b) 8.314 J\/mole\/K<br>(c) 83.14 J\/mole\/K<br>(d) 8314 J\/mole\/K<\/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 correct answer is <strong>(b) 8.314 J\/mole\/K<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>The universal gas constant, often denoted by $R$, is a fundamental physical constant used in many equations of state for gases. It appears in the ideal gas law and is important in thermodynamics and chemistry.<\/p>\n\n\n\n<p>The ideal gas law is expressed as:<\/p>\n\n\n\n<p>$$<br>PV = nRT<br>$$<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>$P$ is the pressure of the gas (in pascals, Pa),<\/li>\n\n\n\n<li>$V$ is the volume of the gas (in cubic meters, m\u00b3),<\/li>\n\n\n\n<li>$n$ is the number of moles of the gas,<\/li>\n\n\n\n<li>$R$ is the universal gas constant,<\/li>\n\n\n\n<li>$T$ is the temperature of the gas (in kelvins, K).<\/li>\n<\/ul>\n\n\n\n<p>In SI units, the value of the universal gas constant $R$ is <strong>8.314 J\/(mol\u00b7K)<\/strong>. Here\u2019s why:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Dimensions of $R$<\/strong>: The gas constant is derived from the relationship between pressure, volume, temperature, and the number of moles of gas. The units of the ideal gas law equation are such that the gas constant must have the units of energy per temperature per mole. This is: $$<br>\\text{Units of } R = \\frac{\\text{energy (J)}}{\\text{mol} \\times \\text{temperature (K)}} = \\frac{\\text{J}}{\\text{mol} \\times \\text{K}}<br>$$ This gives the unit of $R$ as joules per mole per kelvin (J\/mol\u00b7K), which matches the value <strong>8.314 J\/mol\u00b7K<\/strong>.<\/li>\n\n\n\n<li><strong>Historical and Experimental Determination<\/strong>: The value of $R$ was experimentally determined by several scientists, including Boyle and Charles, and its current accepted value is 8.314 J\/mol\u00b7K. This value is used in various thermodynamic calculations, such as those involving gas laws, reaction kinetics, and enthalpy.<\/li>\n\n\n\n<li><strong>Other Values of $R$<\/strong>: Different values of the gas constant are sometimes used depending on the units for pressure, volume, or temperature. For instance, in other systems of units like the CGS system, different numerical values might be used (such as 0.08314 for specific units), but the SI unit is <strong>8.314 J\/mol\u00b7K<\/strong>.<\/li>\n<\/ol>\n\n\n\n<p>Thus, the correct and standard value of the universal gas constant in SI units is <strong>8.314 J\/mol\u00b7K<\/strong> (Option b).<\/p>\n","protected":false},"excerpt":{"rendered":"<p>In SI units, the value of the universal gas constant is (a) 0.8314 J\/mole\/K(b) 8.314 J\/mole\/K(c) 83.14 J\/mole\/K(d) 8314 J\/mole\/K The correct answer and explanation is : The correct answer is (b) 8.314 J\/mole\/K. Explanation: The universal gas constant, often denoted by $R$, is a fundamental physical constant used in many equations of state for [&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-211492","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/211492","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=211492"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/211492\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=211492"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=211492"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=211492"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}