{"id":186183,"date":"2025-01-24T08:35:55","date_gmt":"2025-01-24T08:35:55","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=186183"},"modified":"2025-01-24T08:36:12","modified_gmt":"2025-01-24T08:36:12","slug":"the-following-table-displays-the-vapor-pressure-of-a-noble-gas-at-several-different-temperature","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/24\/the-following-table-displays-the-vapor-pressure-of-a-noble-gas-at-several-different-temperature\/","title":{"rendered":"The following table displays the vapor pressure of a noble gas at several different temperature"},"content":{"rendered":"\n

The following table displays the vapor pressure of a noble gas at several different temperature. Use the date in the table Temperature (\u00b0C) Pressure (torr) 389.0 673.2 -20.5 The following -5.00 789.7 2.00 25.0 1166.8 55.0 1890.0<\/p>\n\n\n\n

The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n

The table provided lists the vapor pressures of a noble gas at various temperatures:<\/p>\n\n\n\n

Temperature (\u00b0C)<\/th>Pressure (torr)<\/th><\/tr><\/thead>
-20.5<\/td>389.0<\/td><\/tr>
-5.00<\/td>673.2<\/td><\/tr>
2.00<\/td>789.7<\/td><\/tr>
25.0<\/td>1166.8<\/td><\/tr>
55.0<\/td>1890.0<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

To determine the boiling point of this noble gas at 1.10 atm, we can use the Clausius-Clapeyron equation, which relates the change in vapor pressure with temperature to the heat of vaporization:<\/p>\n\n\n\n

[ \\ln \\left( \\frac{P_2}{P_1} \\right) = -\\frac{\\Delta H_{\\text{vap}}}{R} \\left( \\frac{1}{T_2} – \\frac{1}{T_1} \\right) ]<\/p>\n\n\n\n

Where:<\/p>\n\n\n\n

    \n
  • ( P_1 ) and ( P_2 ) are the initial and final pressures, respectively.<\/li>\n\n\n\n
  • ( T_1 ) and ( T_2 ) are the initial and final temperatures (in Kelvin).<\/li>\n\n\n\n
  • ( \\Delta H_{\\text{vap}} ) is the heat of vaporization.<\/li>\n\n\n\n
  • ( R ) is the universal gas constant (8.314 J\/mol\u00b7K).<\/li>\n<\/ul>\n\n\n\n

    Given that 1.10 atm is approximately 831.6 torr, we can use the data points closest to this pressure to estimate the boiling point.<\/p>\n\n\n\n

    From the table, the pressures at 25.0\u00b0C and 55.0\u00b0C are 1166.8 torr and 1890.0 torr, respectively.<\/p>\n\n\n\n

    Using these values, we can calculate the heat of vaporization (( \\Delta H_{\\text{vap}} )) and then determine the boiling point at 1.10 atm.<\/p>\n\n\n\n

    However, without the exact heat of vaporization value, we can estimate the boiling point by interpolation.<\/p>\n\n\n\n

    The boiling point at 1.10 atm will be between 25.0\u00b0C and 55.0\u00b0C, closer to 25.0\u00b0C due to the pressure values.<\/p>\n\n\n\n

    Therefore, the boiling point of this noble gas at 1.10 atm is approximately 25.0\u00b0C.<\/p>\n\n\n\n

    This estimation assumes that the heat of vaporization remains relatively constant over the temperature range considered.<\/p>\n\n\n\n

    For more precise calculations, the exact heat of vaporization and additional data points would be necessary.<\/p>\n","protected":false},"excerpt":{"rendered":"

    The following table displays the vapor pressure of a noble gas at several different temperature. Use the date in the table Temperature (\u00b0C) Pressure (torr) 389.0 673.2 -20.5 The following -5.00 789.7 2.00 25.0 1166.8 55.0 1890.0 The Correct Answer and Explanation is : The table provided lists the vapor pressures of a noble gas […]<\/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-186183","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186183","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=186183"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186183\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=186183"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=186183"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=186183"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}