{"id":232811,"date":"2025-06-12T08:20:30","date_gmt":"2025-06-12T08:20:30","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=232811"},"modified":"2025-06-12T08:20:33","modified_gmt":"2025-06-12T08:20:33","slug":"silver-has-an-atomic-mass-of-108-amu","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/12\/silver-has-an-atomic-mass-of-108-amu\/","title":{"rendered":"Silver has an atomic mass of 108 amu."},"content":{"rendered":"\n

Silver has an atomic mass of 108 amu. How many silver atoms does it take to make 1.0 gram of Silver.<\/p>\n\n\n\n

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

Step-by-Step Solution<\/strong><\/h3>\n\n\n\n

Given:<\/strong><\/p>\n\n\n\n

    \n
  • Atomic mass of silver (Ag) = 108 amu<\/li>\n\n\n\n
  • Mass of silver sample = 1.0 gram<\/li>\n\n\n\n
  • Avogadro\u2019s number = 6.022\u00d710236.022 \\times 10^{23}6.022\u00d71023 atoms\/mol<\/li>\n<\/ul>\n\n\n\n

    Step 1: Convert grams of silver to moles.<\/strong> Moles of Ag=1.0 g108 g\/mol=0.00926 mol\\text{Moles of Ag} = \\frac{1.0\\ \\text{g}}{108\\ \\text{g\/mol}} = 0.00926\\ \\text{mol}Moles of Ag=108 g\/mol1.0 g\u200b=0.00926 mol<\/p>\n\n\n\n

    Step 2: Convert moles to atoms using Avogadro\u2019s number.<\/strong> Atoms of Ag=0.00926 mol\u00d76.022\u00d71023 atoms\/mol\\text{Atoms of Ag} = 0.00926\\ \\text{mol} \\times 6.022 \\times 10^{23}\\ \\text{atoms\/mol}Atoms of Ag=0.00926 mol\u00d76.022\u00d71023 atoms\/mol Atoms of Ag\u22485.58\u00d71021 atoms\\text{Atoms of Ag} \\approx 5.58 \\times 10^{21}\\ \\text{atoms}Atoms of Ag\u22485.58\u00d71021 atoms<\/p>\n\n\n\n

    \n\n\n\n

    Explanation <\/strong><\/h3>\n\n\n\n

    Silver is a metallic element with the symbol Ag and an atomic mass of approximately 108 atomic mass units (amu). The atomic mass tells how many grams one mole of silver atoms weighs. In this case, 1 mole of silver weighs 108 grams and contains 6.022\u00d710236.022 \\times 10^{23}6.022\u00d71023 atoms, a constant known as Avogadro\u2019s number.<\/p>\n\n\n\n

    To determine how many atoms are in a smaller sample, such as 1.0 gram of silver, begin by calculating the number of moles in the sample. This is done by dividing the sample mass by the molar mass (atomic mass in g\/mol). For silver: Moles=1.0 g108 g\/mol=0.00926 mol\\text{Moles} = \\frac{1.0\\ \\text{g}}{108\\ \\text{g\/mol}} = 0.00926\\ \\text{mol}Moles=108 g\/mol1.0 g\u200b=0.00926 mol<\/p>\n\n\n\n

    This means the 1.0 gram of silver contains about 0.00926 moles of silver atoms. To find how many individual atoms this represents, multiply the number of moles by Avogadro\u2019s number: 0.00926 mol\u00d76.022\u00d71023 atoms\/mol=5.58\u00d71021 atoms0.00926\\ \\text{mol} \\times 6.022 \\times 10^{23}\\ \\text{atoms\/mol} = 5.58 \\times 10^{21}\\ \\text{atoms}0.00926 mol\u00d76.022\u00d71023 atoms\/mol=5.58\u00d71021 atoms<\/p>\n\n\n\n

    Therefore, 1.0 gram of silver contains approximately 5.58\u00d710215.58 \\times 10^{21}5.58\u00d71021 silver atoms. This large number highlights the tiny mass and size of individual atoms. Even in a sample as small as 1.0 gram, the quantity of atoms present is astronomically large. This concept is central to understanding chemical reactions, where atoms interact in mole-based proportions to form new substances.<\/p>\n\n\n\n

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

    Silver has an atomic mass of 108 amu. How many silver atoms does it take to make 1.0 gram of Silver. The Correct Answer and Explanation is: Step-by-Step Solution Given: Step 1: Convert grams of silver to moles. Moles of Ag=1.0 g108 g\/mol=0.00926 mol\\text{Moles of Ag} = \\frac{1.0\\ \\text{g}}{108\\ \\text{g\/mol}} = 0.00926\\ \\text{mol}Moles of Ag=108 g\/mol1.0 g\u200b=0.00926 mol Step 2: Convert moles to atoms using […]<\/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-232811","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/232811","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=232811"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/232811\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=232811"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=232811"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=232811"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}