{"id":194305,"date":"2025-02-23T07:56:02","date_gmt":"2025-02-23T07:56:02","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=194305"},"modified":"2025-02-23T07:56:07","modified_gmt":"2025-02-23T07:56:07","slug":"calculate-the-average-atomic-mass-of-silver","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/23\/calculate-the-average-atomic-mass-of-silver\/","title":{"rendered":"Calculate the average atomic mass of silver"},"content":{"rendered":"\n

Calculate the average atomic mass of silver. The percentages denote the relative abundances. Isotope 109 Ag 47 107 amu Rel. Abundance Atomic Mass 48.16% 51.84% 108.905 amu 106.905 amu<\/p>\n\n\n\n

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

To calculate the average atomic mass of silver (Ag)<\/strong>, we use the formula:<\/p>\n\n\n\n

[
\\text{Average Atomic Mass} = (\\text{mass of isotope}_1 \\times \\text{relative abundance}_1) + (\\text{mass of isotope}_2 \\times \\text{relative abundance}_2)
]<\/p>\n\n\n\n

Given Data:<\/h3>\n\n\n\n
    \n
  • Isotope 1:<\/strong> ( ^{107}Ag )<\/li>\n\n\n\n
  • Mass = 106.905 amu<\/strong><\/li>\n\n\n\n
  • Relative Abundance = 51.84% = 0.5184<\/strong><\/li>\n\n\n\n
  • Isotope 2:<\/strong> ( ^{109}Ag )<\/li>\n\n\n\n
  • Mass = 108.905 amu<\/strong><\/li>\n\n\n\n
  • Relative Abundance = 48.16% = 0.4816<\/strong><\/li>\n<\/ul>\n\n\n\n

    Calculation:<\/h3>\n\n\n\n

    [
    \\text{Average Atomic Mass} = (106.905 \\times 0.5184) + (108.905 \\times 0.4816)
    ]<\/p>\n\n\n\n

    [
    = 55.456 \\, + \\, 52.434
    ]<\/p>\n\n\n\n

    [
    = 107.87 \\, \\text{amu}
    ]<\/p>\n\n\n\n

    Explanation:<\/h3>\n\n\n\n

    The average atomic mass<\/strong> of an element is a weighted average<\/strong> of all its isotopes based on their natural abundances. Silver has two stable isotopes<\/strong>: (^{107}Ag) and (^{109}Ag), which occur in almost equal proportions.<\/p>\n\n\n\n

      \n
    1. Why use a weighted average?<\/strong><\/li>\n<\/ol>\n\n\n\n
        \n
      • Elements exist as mixtures of isotopes in nature, and their atomic mass depends on the relative proportion of each isotope<\/strong>.<\/li>\n<\/ul>\n\n\n\n
          \n
        1. Importance of Relative Abundance<\/strong><\/li>\n<\/ol>\n\n\n\n
            \n
          • If an isotope is more abundant, it contributes more<\/strong> to the average atomic mass. In silver, (^{107}Ag)<\/strong> has a slightly higher abundance (51.84%)<\/strong>, so the average mass is closer to its atomic mass<\/strong> (106.905 amu).<\/li>\n<\/ul>\n\n\n\n
              \n
            1. Final Value in Periodic Table<\/strong><\/li>\n<\/ol>\n\n\n\n
                \n
              • The calculated 107.87 amu<\/strong> matches the atomic mass of silver in the periodic table.<\/li>\n<\/ul>\n\n\n\n

                Thus, the average atomic mass of silver is 107.87 amu<\/strong>.<\/p>\n\n\n\n

                \n\n\n\n

                Now, I will generate an image representing this calculation.<\/p>\n\n\n\n

                Here is the image illustrating the calculation of the average atomic mass of silver. Let me know if you need any modifications or additional details!<\/p>\n\n\n\n

                \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

                Calculate the average atomic mass of silver. The percentages denote the relative abundances. Isotope 109 Ag 47 107 amu Rel. Abundance Atomic Mass 48.16% 51.84% 108.905 amu 106.905 amu The Correct Answer and Explanation is : To calculate the average atomic mass of silver (Ag), we use the formula: [\\text{Average Atomic Mass} = (\\text{mass of […]<\/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-194305","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194305","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=194305"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194305\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=194305"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=194305"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=194305"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}