{"id":182206,"date":"2025-01-13T13:43:29","date_gmt":"2025-01-13T13:43:29","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=182206"},"modified":"2025-01-13T13:43:31","modified_gmt":"2025-01-13T13:43:31","slug":"carbon-disulfide-cs2-has-a-boiling-point-of-46-2c","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/13\/carbon-disulfide-cs2-has-a-boiling-point-of-46-2c\/","title":{"rendered":"Carbon disulfide (CS2) has a boiling point of 46.2\u00b0C"},"content":{"rendered":"\n<p>Carbon disulfide (CS2) has a boiling point of 46.2\u00b0C. ?What is the boiling point elevation of a<\/p>\n\n\n\n<p>solution consisting of 13.7g ?phosphorus (P4) ?dissolved in 62.67g ?of CS2 ? ( {:CS2KK=2.34)<\/p>\n\n\n\n<p>Use the Molar Mass:<\/p>\n\n\n\n<p>C=12.01gmol<\/p>\n\n\n\n<p>P=30.97gmol<\/p>\n\n\n\n<p>S=32.06gmol<\/p>\n\n\n\n<p>Round your answer to 3 ?significant figures.<\/p>\n\n\n\n<p>Calculate the Vapor Pressure of a solution of 11.138g ?of aspirin (C9H8O4) ?in 65.271g ?of methanol<\/p>\n\n\n\n<p>(CH3OH) ?at 21.2\u00b0C.<\/p>\n\n\n\n<p>Methanol has a vapor pressure of 101 ?torr at this temperature.<\/p>\n\n\n\n<p>Use the following Molar Mass:<\/p>\n\n\n\n<p>C=12.01gmol<\/p>\n\n\n\n<p>H=1.01gmol<\/p>\n\n\n\n<p>O=16.00gmol<\/p>\n\n\n\n<p>Round your answer to 5 ?significant figures.<\/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<h3 class=\"wp-block-heading\">Part 1: Boiling Point Elevation Calculation<\/h3>\n\n\n\n<p>To calculate the <strong>boiling point elevation<\/strong> of the solution, we need to use the following formula:<\/p>\n\n\n\n<p>[<br>\\Delta T_b = K_b \\times m<br>]<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>(\\Delta T_b) is the boiling point elevation,<\/li>\n\n\n\n<li>(K_b) is the ebullioscopic constant (boiling point elevation constant) of the solvent (CS2), which is given as 2.34 \u00b0C\u00b7kg\/mol,<\/li>\n\n\n\n<li>(m) is the molality of the solution.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\">Step 1: Calculate the number of moles of phosphorus (P4)<\/h4>\n\n\n\n<p>To find the molality of the solution, we first need to calculate the number of moles of phosphorus (P4) that are dissolved in 62.67 g of CS2.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Molar mass of phosphorus (P) is given as 30.97 g\/mol.<\/li>\n\n\n\n<li>Molar mass of P4 is (4 \\times 30.97 \\, \\text{g\/mol} = 123.88 \\, \\text{g\/mol}).<\/li>\n<\/ul>\n\n\n\n<p>Now, calculate the moles of phosphorus (P4) in 13.7 g of phosphorus:<\/p>\n\n\n\n<p>[<br>\\text{moles of P4} = \\frac{13.7 \\, \\text{g}}{123.88 \\, \\text{g\/mol}} = 0.110 \\, \\text{mol}<br>]<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Step 2: Calculate the molality of the solution<\/h4>\n\n\n\n<p>Molality ((m)) is the number of moles of solute (P4) per kilogram of solvent (CS2).<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Mass of CS2 is 62.67 g, which is 0.06267 kg.<\/li>\n<\/ul>\n\n\n\n<p>[<br>m = \\frac{0.110 \\, \\text{mol}}{0.06267 \\, \\text{kg}} = 1.756 \\, \\text{mol\/kg}<br>]<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Step 3: Calculate the boiling point elevation<\/h4>\n\n\n\n<p>Now, apply the formula for boiling point elevation:<\/p>\n\n\n\n<p>[<br>\\Delta T_b = K_b \\times m = 2.34 \\, \\text{\u00b0C\u00b7kg\/mol} \\times 1.756 \\, \\text{mol\/kg} = 4.11 \\, \\text{\u00b0C}<br>]<\/p>\n\n\n\n<p>The <strong>boiling point elevation<\/strong> is 4.11 \u00b0C.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Step 4: Final boiling point<\/h4>\n\n\n\n<p>The boiling point of pure CS2 is 46.2\u00b0C, so the new boiling point of the solution is:<\/p>\n\n\n\n<p>[<br>\\text{Boiling point of solution} = 46.2 \\, \\text{\u00b0C} + 4.11 \\, \\text{\u00b0C} = 50.31 \\, \\text{\u00b0C}<br>]<\/p>\n\n\n\n<p>Thus, the boiling point of the solution is <strong>50.31\u00b0C<\/strong>.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Part 2: Vapor Pressure of the Aspirin Solution<\/h3>\n\n\n\n<p>To calculate the <strong>vapor pressure<\/strong> of a solution, we use Raoult\u2019s Law:<\/p>\n\n\n\n<p>[<br>P_{\\text{solution}} = X_{\\text{solvent}} \\times P_{\\text{solvent}}<br>]<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>(P_{\\text{solution}}) is the vapor pressure of the solution,<\/li>\n\n\n\n<li>(X_{\\text{solvent}}) is the mole fraction of the solvent (methanol),<\/li>\n\n\n\n<li>(P_{\\text{solvent}}) is the vapor pressure of the pure solvent (methanol), given as 101 torr.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\">Step 1: Calculate the number of moles of aspirin (C9H8O4)<\/h4>\n\n\n\n<p>To find the mole fraction of the solvent, we first need to calculate the moles of aspirin (C9H8O4).<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Molar mass of aspirin (C9H8O4): (9 \\times 12.01 + 8 \\times 1.01 + 4 \\times 16.00 = 180.16 \\, \\text{g\/mol}).<\/li>\n<\/ul>\n\n\n\n<p>Now, calculate the moles of aspirin in 11.138 g:<\/p>\n\n\n\n<p>[<br>\\text{moles of aspirin} = \\frac{11.138 \\, \\text{g}}{180.16 \\, \\text{g\/mol}} = 0.0618 \\, \\text{mol}<br>]<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Step 2: Calculate the moles of methanol (CH3OH)<\/h4>\n\n\n\n<p>Next, calculate the moles of methanol (CH3OH):<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Molar mass of methanol: (12.01 + 4 \\times 1.01 + 16.00 = 32.04 \\, \\text{g\/mol}).<\/li>\n<\/ul>\n\n\n\n<p>[<br>\\text{moles of methanol} = \\frac{65.271 \\, \\text{g}}{32.04 \\, \\text{g\/mol}} = 2.038 \\, \\text{mol}<br>]<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Step 3: Calculate the mole fraction of methanol<\/h4>\n\n\n\n<p>The mole fraction of methanol is the ratio of the moles of methanol to the total moles (moles of methanol + moles of aspirin):<\/p>\n\n\n\n<p>[<br>X_{\\text{methanol}} = \\frac{2.038 \\, \\text{mol}}{2.038 \\, \\text{mol} + 0.0618 \\, \\text{mol}} = \\frac{2.038}{2.0998} = 0.9707<br>]<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Step 4: Calculate the vapor pressure of the solution<\/h4>\n\n\n\n<p>Now, apply Raoult&#8217;s Law to calculate the vapor pressure of the solution:<\/p>\n\n\n\n<p>[<br>P_{\\text{solution}} = X_{\\text{methanol}} \\times P_{\\text{methanol}} = 0.9707 \\times 101 \\, \\text{torr} = 97.99 \\, \\text{torr}<br>]<\/p>\n\n\n\n<p>Thus, the vapor pressure of the aspirin solution is <strong>97.99 torr<\/strong>.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Summary:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The boiling point elevation of the CS2 solution is <strong>50.31\u00b0C<\/strong>.<\/li>\n\n\n\n<li>The vapor pressure of the aspirin solution in methanol is <strong>97.99 torr<\/strong>.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Carbon disulfide (CS2) has a boiling point of 46.2\u00b0C. ?What is the boiling point elevation of a solution consisting of 13.7g ?phosphorus (P4) ?dissolved in 62.67g ?of CS2 ? ( {:CS2KK=2.34) Use the Molar Mass: C=12.01gmol P=30.97gmol S=32.06gmol Round your answer to 3 ?significant figures. Calculate the Vapor Pressure of a solution of 11.138g ?of [&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-182206","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182206","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=182206"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182206\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=182206"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=182206"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=182206"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}