Estimate the boiling point of carbon tetrachloride given the following thermodynamic parameters.<\/p>\n\n\n\n
CCl4(l) CCl4(g)<\/p>\n\n\n\n
Change fH (kj\/mol-rxn) -128.4 -96.0
S (J.K. mol-rxn) 214.4 309.7
Change fG (kj\/mol-rxn) -57.6 -53.6<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n To estimate the boiling point (( T_b )) of carbon tetrachloride (( CCl_4 )), we use the thermodynamic criterion for phase equilibrium:<\/p>\n\n\n\n [ At the boiling point, the liquid and gas phases are in equilibrium, meaning the Gibbs free energy change (( \\Delta G )) for the phase transition is zero.<\/p>\n\n\n\n The enthalpy change of vaporization (( \\Delta H_{vap} )) is given by:<\/p>\n\n\n\n [ [ The entropy change for the phase transition is:<\/p>\n\n\n\n [ [ At equilibrium:<\/p>\n\n\n\n [ Converting ( \\Delta H_{vap} ) to J\/mol:<\/p>\n\n\n\n [ [ The estimated boiling point of carbon tetrachloride is 340 K (67\u00b0C)<\/strong>.<\/p>\n\n\n\n The boiling point of a liquid is the temperature at which its vapor pressure equals atmospheric pressure. At this point, the Gibbs free energy change (( \\Delta G )) for the phase transition is zero, leading to the fundamental relation:<\/p>\n\n\n\n [ where ( \\Delta H ) is the enthalpy change (heat required to convert liquid to gas), and ( \\Delta S ) is the entropy change (degree of molecular disorder increase).<\/p>\n\n\n\n For carbon tetrachloride, we obtained:<\/p>\n\n\n\n By dividing ( \\Delta H_{vap} ) by ( \\Delta S_{vap} ), we determine the boiling temperature as 340 K<\/strong>. This calculation aligns well with experimental values (~349 K or 76\u00b0C), suggesting minor deviations due to ideal assumptions.<\/p>\n\n\n\n The boiling point reflects intermolecular forces: stronger forces lead to higher boiling points. ( CCl_4 ) exhibits only van der Waals interactions (no hydrogen bonding), explaining its relatively low boiling point compared to polar compounds.<\/p>\n\n\n\n This thermodynamic approach provides an accurate estimate and highlights the fundamental role of entropy and enthalpy in phase transitions.<\/p>\n","protected":false},"excerpt":{"rendered":" Estimate the boiling point of carbon tetrachloride given the following thermodynamic parameters. CCl4(l) CCl4(g) Change fH (kj\/mol-rxn) -128.4 -96.0S (J.K. mol-rxn) 214.4 309.7Change fG (kj\/mol-rxn) -57.6 -53.6 The Correct Answer and Explanation is : To estimate the boiling point (( T_b )) of carbon tetrachloride (( CCl_4 )), we use the thermodynamic criterion for phase […]<\/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-187173","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187173","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=187173"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187173\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187173"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187173"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187173"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\\Delta G = \\Delta H – T \\Delta S = 0
]<\/p>\n\n\n\nStep 1: Calculate the Enthalpy Change (( \\Delta H_{vap} ))<\/strong><\/h3>\n\n\n\n
\\Delta H_{vap} = H_g – H_l
]<\/p>\n\n\n\n
\\Delta H_{vap} = (-96.0) – (-128.4) = 32.4 \\text{ kJ\/mol}
]<\/p>\n\n\n\nStep 2: Calculate the Entropy Change (( \\Delta S_{vap} ))<\/strong><\/h3>\n\n\n\n
\\Delta S_{vap} = S_g – S_l
]<\/p>\n\n\n\n
\\Delta S_{vap} = (309.7) – (214.4) = 95.3 \\text{ J\/(mol\u00b7K)}
]<\/p>\n\n\n\nStep 3: Solve for ( T_b )<\/strong><\/h3>\n\n\n\n
T_b = \\frac{\\Delta H_{vap}}{\\Delta S_{vap}}
]<\/p>\n\n\n\n
32.4 \\times 10^3 \\text{ J\/mol}
]<\/p>\n\n\n\n
T_b = \\frac{32.4 \\times 10^3}{95.3} = 340.1 \\text{ K}
]<\/p>\n\n\n\nFinal Answer<\/strong><\/h3>\n\n\n\n
Explanation (300 Words)<\/strong><\/h3>\n\n\n\n
\\Delta G = \\Delta H – T \\Delta S = 0
]<\/p>\n\n\n\n\n