{"id":157979,"date":"2024-10-24T07:35:13","date_gmt":"2024-10-24T07:35:13","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=157979"},"modified":"2024-10-24T07:35:16","modified_gmt":"2024-10-24T07:35:16","slug":"fructose-1-phosphate-can-be-hydrolyzed-into-fructose-inorganic-phosphate-pi-with-a-%ce%b4g-of-16-0-kj-mol","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/10\/24\/fructose-1-phosphate-can-be-hydrolyzed-into-fructose-inorganic-phosphate-pi-with-a-%ce%b4g-of-16-0-kj-mol\/","title":{"rendered":"Fructose-1-phosphate can be hydrolyzed into fructose + inorganic phosphate (Pi) with a \u0394G\u00b0 of \u201316.0 kJ\/mol."},"content":{"rendered":"\n

Fructose-1-phosphate can be hydrolyzed into fructose + inorganic phosphate (Pi) with a \u0394G\u00b0 of \u201316.0 kJ\/mol. If ATP can be hydrolyzed into ADP + Pi with a \u0394G\u00b0 of \u201330.5 kJ\/mol, what is the free energy change for the reaction of fructose + ATP \u2192 fructose 1-phospate + ADP<\/p>\n\n\n\n

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

To calculate the free energy change (\u0394G\u00b0) for the reaction ( \\text{fructose} + \\text{ATP} \\rightarrow \\text{fructose-1-phosphate} + \\text{ADP} ), we can utilize the values of the standard free energy changes (\u0394G\u00b0) for the reactions involved. The key reactions to consider are:<\/p>\n\n\n\n

    \n
  1. Hydrolysis of ATP:
    [
    \\text{ATP} \\rightarrow \\text{ADP} + \\text{P}_i \\quad \\text{with } \\Delta G\u00b0 = -30.5 \\, \\text{kJ\/mol}
    ]<\/li>\n\n\n\n
  2. Hydrolysis of fructose-1-phosphate:
    [
    \\text{fructose-1-phosphate} \\rightarrow \\text{fructose} + \\text{P}_i \\quad \\text{with } \\Delta G\u00b0 = -16.0 \\, \\text{kJ\/mol}
    ]<\/li>\n<\/ol>\n\n\n\n

    In our target reaction, we can reverse the hydrolysis of fructose-1-phosphate because the fructose-1-phosphate is formed, leading to a change in sign of its \u0394G\u00b0:
    [
    \\text{fructose} + \\text{P}_i \\rightarrow \\text{fructose-1-phosphate} \\quad \\Delta G\u00b0 = +16.0 \\, \\text{kJ\/mol}
    ]<\/p>\n\n\n\n

    Now, we can combine the two reactions to find the overall free energy change for the desired reaction:
    [
    \\text{fructose} + \\text{ATP} \\rightarrow \\text{fructose-1-phosphate} + \\text{ADP}
    ]<\/p>\n\n\n\n

    Using the equation for \u0394G\u00b0:
    [
    \\Delta G\u00b0{\\text{overall}} = \\Delta G\u00b0<\/em>{\\text{ATP hydrolysis}} + \\Delta G\u00b0_{\\text{reverse fructose-1-phosphate}}
    ]<\/p>\n\n\n\n

    Substituting the values:
    [
    \\Delta G\u00b0_{\\text{overall}} = (-30.5 \\, \\text{kJ\/mol}) + (+16.0 \\, \\text{kJ\/mol}) = -14.5 \\, \\text{kJ\/mol}
    ]<\/p>\n\n\n\n

    Conclusion<\/h3>\n\n\n\n

    Thus, the free energy change for the reaction ( \\text{fructose} + \\text{ATP} \\rightarrow \\text{fructose-1-phosphate} + \\text{ADP} ) is \u201314.5 kJ\/mol<\/strong>.<\/p>\n\n\n\n

    This negative value indicates that the reaction is energetically favorable and can occur spontaneously under standard conditions. The hydrolysis of ATP provides a significant driving force for the phosphorylation of fructose, making it a vital step in metabolic pathways such as glycolysis. In cellular metabolism, this reaction contributes to the overall energy transfer processes that sustain life.<\/p>\n","protected":false},"excerpt":{"rendered":"

    Fructose-1-phosphate can be hydrolyzed into fructose + inorganic phosphate (Pi) with a \u0394G\u00b0 of \u201316.0 kJ\/mol. If ATP can be hydrolyzed into ADP + Pi with a \u0394G\u00b0 of \u201330.5 kJ\/mol, what is the free energy change for the reaction of fructose + ATP \u2192 fructose 1-phospate + ADP 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-157979","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/157979","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=157979"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/157979\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=157979"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=157979"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=157979"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}