{"id":160465,"date":"2024-11-03T04:33:08","date_gmt":"2024-11-03T04:33:08","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=160465"},"modified":"2024-11-03T04:33:10","modified_gmt":"2024-11-03T04:33:10","slug":"calculate-the-molar-mass-of-nh4no3-molar-mass-of-nh4no3-__-g-mol","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/03\/calculate-the-molar-mass-of-nh4no3-molar-mass-of-nh4no3-__-g-mol\/","title":{"rendered":"Calculate the molar mass of NH4\u200bNO3\u200b.Molar mass of NH4\u200bNO3\u200b= __ g\/mol"},"content":{"rendered":"\n

Calculate the molar mass of NH
4
\u200b
NO
3
\u200b
.
Molar mass of NH
4
\u200b
NO
3
\u200b
= __<\/strong> g\/mol.<\/p>\n\n\n\n

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

To calculate the molar mass of ammonium nitrate (NH\u2084NO\u2083), we need to determine the molar masses of each element in the compound and then sum them up according to their proportions in the formula.<\/p>\n\n\n\n

Step 1: Identify the elements and their quantities<\/h3>\n\n\n\n

In ammonium nitrate (NH\u2084NO\u2083), the elements and their quantities are as follows:<\/p>\n\n\n\n

    \n
  • Nitrogen (N): 2 atoms (1 from NH\u2084 and 1 from NO\u2083)<\/li>\n\n\n\n
  • Hydrogen (H): 4 atoms (from NH\u2084)<\/li>\n\n\n\n
  • Oxygen (O): 3 atoms (from NO\u2083)<\/li>\n<\/ul>\n\n\n\n

    Step 2: Find the molar mass of each element<\/h3>\n\n\n\n

    Using the periodic table, we find the molar masses of the elements:<\/p>\n\n\n\n

      \n
    • Nitrogen (N): approximately 14.01 g\/mol<\/li>\n\n\n\n
    • Hydrogen (H): approximately 1.01 g\/mol<\/li>\n\n\n\n
    • Oxygen (O): approximately 16.00 g\/mol<\/li>\n<\/ul>\n\n\n\n

      Step 3: Calculate the total molar mass<\/h3>\n\n\n\n

      Now, we can calculate the total molar mass of NH\u2084NO\u2083 by multiplying the number of atoms by the molar mass of each element:<\/p>\n\n\n\n

        \n
      • For Nitrogen:
        [
        2 \\, \\text{N} \\times 14.01 \\, \\text{g\/mol} = 28.02 \\, \\text{g\/mol}
        ]<\/li>\n\n\n\n
      • For Hydrogen:
        [
        4 \\, \\text{H} \\times 1.01 \\, \\text{g\/mol} = 4.04 \\, \\text{g\/mol}
        ]<\/li>\n\n\n\n
      • For Oxygen:
        [
        3 \\, \\text{O} \\times 16.00 \\, \\text{g\/mol} = 48.00 \\, \\text{g\/mol}
        ]<\/li>\n<\/ul>\n\n\n\n

        Step 4: Sum the contributions<\/h3>\n\n\n\n

        Now, we sum all the contributions:
        [
        \\text{Total Molar Mass} = 28.02 \\, \\text{g\/mol} + 4.04 \\, \\text{g\/mol} + 48.00 \\, \\text{g\/mol} = 80.06 \\, \\text{g\/mol}
        ]<\/p>\n\n\n\n

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

        Therefore, the molar mass of ammonium nitrate (NH\u2084NO\u2083) is 80.06 g\/mol<\/strong>.<\/p>\n\n\n\n

        Understanding the molar mass is crucial in stoichiometry, which allows chemists to calculate the amounts of reactants and products in chemical reactions. Molar mass plays a key role in converting grams to moles and vice versa, facilitating the quantification of substances involved in chemical processes. This concept is fundamental for various applications in chemistry, including solution preparation, reaction yield predictions, and laboratory measurements.<\/p>\n","protected":false},"excerpt":{"rendered":"

        Calculate the molar mass of NH4\u200bNO3\u200b.Molar mass of NH4\u200bNO3\u200b= __ g\/mol. The Correct Answer and Explanation is : To calculate the molar mass of ammonium nitrate (NH\u2084NO\u2083), we need to determine the molar masses of each element in the compound and then sum them up according to their proportions in the formula. Step 1: Identify […]<\/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-160465","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/160465","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=160465"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/160465\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=160465"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=160465"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=160465"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}