{"id":189353,"date":"2025-02-09T06:03:56","date_gmt":"2025-02-09T06:03:56","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=189353"},"modified":"2025-02-09T06:03:58","modified_gmt":"2025-02-09T06:03:58","slug":"complete-the-table-below-for-calculating-the-molar-mass-of-the-ionic-compound-ironii-iodide","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/09\/complete-the-table-below-for-calculating-the-molar-mass-of-the-ionic-compound-ironii-iodide\/","title":{"rendered":"Complete the table below for calculating the molar mass of the ionic compound iron(II) iodide"},"content":{"rendered":"\n

Complete the table below for calculating the molar mass of the ionic compound iron(II) iodide. Number of ions Mass of ion in one mole of iron(II) iodide Formula Molar mass of ion Fe2+ g\/mol x Cation mol Anion T g\/mol X mol Molar mass iron(II) iodide g\/mol<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

Complete the table below for calculating the molar mass of the compound nitrogen monoxide. Molar mass of element Moles Mass in one mole of nitrogen monoxide N g\/mol X mol g O g\/mol X mol = 8 Molar mass nitrogen monoxide g\/mol<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

Complete the table below for calculating the molar mass of the ionic compound calcium oxide. Formula Molar mass of lon Number of ions Mass of ion in one mole of calcium oxide Cation Ca2+ g\/mol \u0445 mol 8 Anion 02- g\/mol X mol g Molar mass calcium oxide – g\/mol<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

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

Let’s break down and solve the molar mass calculations for each of the compounds step by step.<\/p>\n\n\n\n

1. Iron(II) Iodide (FeI\u2082)<\/h3>\n\n\n\n

The ionic compound iron(II) iodide consists of iron ions (Fe\u00b2\u207a) and iodide ions (I\u207b).<\/p>\n\n\n\n

Iron(II) iodide formula: FeI\u2082<\/strong><\/p>\n\n\n\n

We need to calculate the molar mass of FeI\u2082, considering the individual masses of Fe\u00b2\u207a and I\u207b ions.<\/p>\n\n\n\n

    \n
  • The molar mass of Fe\u00b2\u207a<\/strong> is equal to the molar mass of Fe (since the ion charge doesn\u2019t affect the mass), which is 55.85 g\/mol<\/strong>.<\/li>\n\n\n\n
  • The molar mass of I\u207b<\/strong> is equal to the molar mass of iodine, which is 126.90 g\/mol<\/strong>.<\/li>\n<\/ul>\n\n\n\n

    Now, let\u2019s calculate the molar mass of FeI\u2082:<\/p>\n\n\n\n

      \n
    • Number of Fe\u00b2\u207a ions: 1<\/strong><\/li>\n\n\n\n
    • Number of I\u207b ions: 2<\/strong><\/li>\n<\/ul>\n\n\n\n

      Molar mass of FeI\u2082:<\/strong>
      [ \\text{Molar mass of FeI\u2082} = (1 \\times 55.85) + (2 \\times 126.90) = 55.85 + 253.80 = 309.65 \\text{ g\/mol} ]<\/p>\n\n\n\n

      Thus, the molar mass of iron(II) iodide (FeI\u2082) is 309.65 g\/mol<\/strong>.<\/p>\n\n\n\n

      2. Nitrogen Monoxide (NO)<\/h3>\n\n\n\n

      Now, let\u2019s calculate the molar mass of nitrogen monoxide (NO), which is made up of nitrogen (N) and oxygen (O).<\/p>\n\n\n\n

        \n
      • The molar mass of nitrogen (N)<\/strong> is 14.01 g\/mol<\/strong>.<\/li>\n\n\n\n
      • The molar mass of oxygen (O)<\/strong> is 16.00 g\/mol<\/strong>.<\/li>\n<\/ul>\n\n\n\n

        The compound nitrogen monoxide (NO) consists of one nitrogen atom and one oxygen atom.<\/p>\n\n\n\n

        Molar mass of NO:<\/strong>
        [ \\text{Molar mass of NO} = 14.01 + 16.00 = 30.01 \\text{ g\/mol} ]<\/p>\n\n\n\n

        Thus, the molar mass of nitrogen monoxide (NO) is 30.01 g\/mol<\/strong>.<\/p>\n\n\n\n

        3. Calcium Oxide (CaO)<\/h3>\n\n\n\n

        Calcium oxide (CaO) consists of calcium ions (Ca\u00b2\u207a) and oxide ions (O\u00b2\u207b).<\/p>\n\n\n\n

          \n
        • The molar mass of Ca\u00b2\u207a<\/strong> is the same as that of calcium, which is 40.08 g\/mol<\/strong>.<\/li>\n\n\n\n
        • The molar mass of O\u00b2\u207b<\/strong> is the same as that of oxygen, which is 16.00 g\/mol<\/strong>.<\/li>\n<\/ul>\n\n\n\n

          Now, let\u2019s calculate the molar mass of CaO:<\/p>\n\n\n\n

            \n
          • Number of Ca\u00b2\u207a ions: 1<\/strong><\/li>\n\n\n\n
          • Number of O\u00b2\u207b ions: 1<\/strong><\/li>\n<\/ul>\n\n\n\n

            Molar mass of CaO:<\/strong>
            [ \\text{Molar mass of CaO} = (1 \\times 40.08) + (1 \\times 16.00) = 40.08 + 16.00 = 56.08 \\text{ g\/mol} ]<\/p>\n\n\n\n

            Thus, the molar mass of calcium oxide (CaO) is 56.08 g\/mol<\/strong>.<\/p>\n\n\n\n

            Summary of Molar Masses:<\/h3>\n\n\n\n
              \n
            • Iron(II) iodide (FeI\u2082): 309.65 g\/mol<\/strong><\/li>\n\n\n\n
            • Nitrogen monoxide (NO): 30.01 g\/mol<\/strong><\/li>\n\n\n\n
            • Calcium oxide (CaO): 56.08 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n

              This approach follows the principle that the molar mass of a compound is the sum of the molar masses of its constituent elements, considering their respective stoichiometric amounts in the formula. Each element contributes based on the number of atoms or ions present in the compound.<\/p>\n","protected":false},"excerpt":{"rendered":"

              Complete the table below for calculating the molar mass of the ionic compound iron(II) iodide. Number of ions Mass of ion in one mole of iron(II) iodide Formula Molar mass of ion Fe2+ g\/mol x Cation mol Anion T g\/mol X mol Molar mass iron(II) iodide g\/mol Complete the table below for calculating the molar […]<\/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-189353","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/189353","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=189353"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/189353\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=189353"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=189353"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=189353"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}