{"id":221635,"date":"2025-05-29T21:02:10","date_gmt":"2025-05-29T21:02:10","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=221635"},"modified":"2025-05-29T21:02:12","modified_gmt":"2025-05-29T21:02:12","slug":"dehydration-of-cyclohexanol-a-dehydration-reaction","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/29\/dehydration-of-cyclohexanol-a-dehydration-reaction\/","title":{"rendered":"Dehydration Of Cyclohexanol A. Dehydration Reaction"},"content":{"rendered":"\n
Dehydration Of Cyclohexanol A. Dehydration Reaction: Write A Balanced Chemical Equation For Dehydration Of Cyclohexanol: .OH H+ +H2O Percent Yield Calculations: 0.685 Amount Of Cyclohexanol Used: 1.5 ML = 8 Moles Of Cyclohexanol Used \u2013 0.006% MoL Moles Of Cyclohexene Expected (Theoretical Yield): Amount Of Cyclohexene Isolated (Isolated Yield):<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
A. Balanced Chemical Equation for the Dehydration of Cyclohexanol<\/strong><\/h3>\n\n\n\n
The acid-catalyzed dehydration<\/strong> of cyclohexanol<\/strong> to form cyclohexene<\/strong> is an elimination (E1) reaction<\/strong> that involves the removal of a water molecule: C6H11OH\u2192H+, \u0394C6H10+H2O\\text{C}_6\\text{H}_{11}\\text{OH} \\xrightarrow{\\text{H}^+, \\ \\Delta} \\text{C}_6\\text{H}_{10} + \\text{H}_2\\text{O}<\/p>\n\n\n\n
Balanced Chemical Equation:<\/strong> C6H11OH\u2192H+, heatC6H10+H2O\\text{C}_6\\text{H}_{11}\\text{OH} \\xrightarrow{\\text{H}^+,\\ \\text{heat}} \\text{C}_6\\text{H}_{10} + \\text{H}_2\\text{O}<\/p>\n\n\n\n\n\n\n\n
Step 2: Convert mass to moles<\/strong> 1.443 g100.16 g\/mol=0.0144 mol cyclohexanol\\frac{1.443\\ \\text{g}}{100.16\\ \\text{g\/mol}} = 0.0144\\ \\text{mol cyclohexanol}<\/p>\n\n\n\n
Since the dehydration is 1:1:<\/p>\n\n\n\n
\n
Theoretical yield of cyclohexene = 0.0144 mol<\/strong><\/li>\n<\/ul>\n\n\n\n
Step 3: Use the provided percent yield (0.685% or 0.00685 as a decimal) to calculate actual yield:<\/strong> Moles of cyclohexene (actual)=0.0144 mol\u00d70.00685=9.864\u00d710\u22125 mol\\text{Moles of cyclohexene (actual)} = 0.0144\\ \\text{mol} \\times 0.00685 = 9.864 \\times 10^{-5}\\ \\text{mol}<\/p>\n\n\n\n
Step 4: Convert moles of cyclohexene to mass (molar mass = 82.15 g\/mol):<\/strong> 9.864\u00d710\u22125 mol\u00d782.15 g\/mol=0.0081 g (\u2248 8.1 mg)9.864 \\times 10^{-5}\\ \\text{mol} \\times 82.15\\ \\text{g\/mol} = 0.0081\\ \\text{g (\u2248 8.1 mg)}<\/p>\n\n\n\n\n\n\n\n
Explanation<\/strong><\/h3>\n\n\n\n
The dehydration of cyclohexanol to cyclohexene<\/strong> is a classic organic reaction used to demonstrate elimination mechanisms and alkene synthesis. This reaction typically occurs in the presence of a strong acid catalyst<\/strong> (such as sulfuric or phosphoric acid) and requires heat<\/strong> to proceed. Under acidic conditions, the hydroxyl group (\u2013OH) of cyclohexanol is protonated to become a better leaving group (water). This leads to the formation of a carbocation intermediate<\/strong>, which then loses a proton to form the double bond of cyclohexene<\/strong>.<\/p>\n\n\n\n
In this lab scenario, 1.5 mL of cyclohexanol was used. After converting to mass and then to moles, we find approximately 0.0144 mol of cyclohexanol were used. Since the reaction is 1:1, the theoretical yield of cyclohexene is also 0.0144 mol.<\/p>\n\n\n\n
The percent yield<\/strong> is calculated based on the actual amount of cyclohexene isolated versus the theoretical maximum. In this case, the percent yield is extremely low (0.685%), which might be due to several factors: incomplete reaction, side reactions, poor separation or distillation, or loss during transfer and purification steps.<\/p>\n\n\n\n
The actual amount of cyclohexene isolated was approximately 8.1 mg (0.0081 g), which aligns with a 0.685% yield. Such a low yield suggests that experimental conditions may need improvement or that significant product loss occurred.<\/p>\n\n\n\n
Understanding and optimizing this reaction is important for organic synthesis, especially when scaling up or improving efficiency in industrial or academic settings.A. Balanced Chemical Equation for the Dehydration of Cyclohexanol<\/strong><\/p>\n\n\n\n
The acid-catalyzed dehydration<\/strong> of cyclohexanol<\/strong> to form cyclohexene<\/strong> is an elimination (E1) reaction<\/strong> that involves the removal of a water molecule: C6H11OH\u2192H+, \u0394C6H10+H2O\\text{C}_6\\text{H}_{11}\\text{OH} \\xrightarrow{\\text{H}^+, \\ \\Delta} \\text{C}_6\\text{H}_{10} + \\text{H}_2\\text{O}<\/p>\n\n\n\n
Balanced Chemical Equation:<\/strong> C6H11OH\u2192H+, heatC6H10+H2O\\text{C}_6\\text{H}_{11}\\text{OH} \\xrightarrow{\\text{H}^+,\\ \\text{heat}} \\text{C}_6\\text{H}_{10} + \\text{H}_2\\text{O}<\/p>\n\n\n\n\n\n\n\n
Step 2: Convert mass to moles<\/strong> 1.443 g100.16 g\/mol=0.0144 mol cyclohexanol\\frac{1.443\\ \\text{g}}{100.16\\ \\text{g\/mol}} = 0.0144\\ \\text{mol cyclohexanol}<\/p>\n\n\n\n
Since the dehydration is 1:1:<\/p>\n\n\n\n
\n
Theoretical yield of cyclohexene = 0.0144 mol<\/strong><\/li>\n<\/ul>\n\n\n\n
Step 3: Use the provided percent yield (0.685% or 0.00685 as a decimal) to calculate actual yield:<\/strong> Moles of cyclohexene (actual)=0.0144 mol\u00d70.00685=9.864\u00d710\u22125 mol\\text{Moles of cyclohexene (actual)} = 0.0144\\ \\text{mol} \\times 0.00685 = 9.864 \\times 10^{-5}\\ \\text{mol}<\/p>\n\n\n\n
Step 4: Convert moles of cyclohexene to mass (molar mass = 82.15 g\/mol):<\/strong> 9.864\u00d710\u22125 mol\u00d782.15 g\/mol=0.0081 g (\u2248 8.1 mg)9.864 \\times 10^{-5}\\ \\text{mol} \\times 82.15\\ \\text{g\/mol} = 0.0081\\ \\text{g (\u2248 8.1 mg)}<\/p>\n\n\n\n\n\n\n\n
Dehydration Of Cyclohexanol A. Dehydration Reaction: Write A Balanced Chemical Equation For Dehydration Of Cyclohexanol: .OH H+ +H2O Percent Yield Calculations: 0.685 Amount Of Cyclohexanol Used: 1.5 ML = 8 Moles Of Cyclohexanol Used \u2013 0.006% MoL Moles Of Cyclohexene Expected (Theoretical Yield): Amount Of Cyclohexene Isolated (Isolated Yield): The Correct Answer and Explanation is: […]<\/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-221635","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/221635","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=221635"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/221635\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=221635"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=221635"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=221635"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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