{"id":198567,"date":"2025-03-10T07:01:57","date_gmt":"2025-03-10T07:01:57","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=198567"},"modified":"2025-03-10T07:01:59","modified_gmt":"2025-03-10T07:01:59","slug":"a-sample-of-liquid-mercury-hg-has-a-mass-of-90-3-g","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/10\/a-sample-of-liquid-mercury-hg-has-a-mass-of-90-3-g\/","title":{"rendered":"A sample of liquid mercury (Hg) has a mass of 90.3 g"},"content":{"rendered":"\n

A sample of liquid mercury (Hg) has a mass of 90.3 g.<\/p>\n\n\n\n

a) Find the molar mass of mercury (Hg).<\/p>\n\n\n\n

b) Determine the number of moles (mol) of mercury in the sample.<\/p>\n\n\n\n

1 mol<\/p>\n\n\n\n

c) Determine the number of mercury atoms in the sample.<\/p>\n\n\n\n

The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n

Let’s go step by step to solve this problem.<\/p>\n\n\n\n

Given Data:<\/strong><\/h3>\n\n\n\n
    \n
  • Mass of liquid mercury (( m )) = 90.3 g<\/strong><\/li>\n\n\n\n
  • Avogadro\u2019s number = ( 6.022 \\times 10^{23} ) atoms\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n
    \n\n\n\n

    Part A: Molar Mass of Mercury (Hg)<\/strong><\/h3>\n\n\n\n

    The molar mass of an element is its atomic weight in grams per mole. According to the periodic table:<\/p>\n\n\n\n

    [
    Molar\\ mass\\ of\\ Hg = 200.59\\ g\/mol
    ]<\/p>\n\n\n\n

    \n\n\n\n

    Part B: Number of Moles of Mercury in the Sample<\/strong><\/h3>\n\n\n\n

    We use the formula:<\/p>\n\n\n\n

    [
    n = \\frac{m}{M}
    ]<\/p>\n\n\n\n

    where:<\/p>\n\n\n\n

      \n
    • ( n ) = number of moles<\/li>\n\n\n\n
    • ( m ) = mass of the sample<\/li>\n\n\n\n
    • ( M ) = molar mass of mercury<\/li>\n<\/ul>\n\n\n\n

      [
      n = \\frac{90.3\\ g}{200.59\\ g\/mol}
      ]<\/p>\n\n\n\n

      [
      n \\approx 0.4502\\ \\text{moles of Hg}
      ]<\/p>\n\n\n\n

      \n\n\n\n

      Part C: Number of Mercury Atoms in the Sample<\/strong><\/h3>\n\n\n\n

      To find the number of atoms, we multiply the number of moles by Avogadro’s number:<\/p>\n\n\n\n

      [
      N = n \\times N_A
      ]<\/p>\n\n\n\n

      [
      N = (0.4502\\ mol) \\times (6.022 \\times 10^{23} \\text{ atoms\/mol})
      ]<\/p>\n\n\n\n

      [
      N \\approx 2.71 \\times 10^{23} \\text{ atoms}
      ]<\/p>\n\n\n\n

      \n\n\n\n

      Explanation:<\/strong><\/h3>\n\n\n\n
        \n
      1. Molar Mass<\/strong>
        The molar mass of mercury is the mass of one mole of Hg atoms, which is 200.59 g\/mol. This value is taken from the periodic table and represents the average atomic mass of mercury.<\/li>\n\n\n\n
      2. Moles Calculation<\/strong>
        To determine how many moles are in 90.3 g of mercury, we divide the given mass by the molar mass. This tells us how many units (moles) of mercury atoms are present.<\/li>\n\n\n\n
      3. Atoms Calculation<\/strong>
        Since one mole of any substance contains ( 6.022 \\times 10^{23} )<\/strong> representative particles (Avogadro’s number), we multiply the moles of Hg by this value to get the number of individual mercury atoms.<\/li>\n<\/ol>\n\n\n\n

        Thus, a 90.3 g sample of mercury contains approximately ( 2.71 \\times 10^{23} ) atoms<\/strong> of mercury.<\/p>\n\n\n\n

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

        A sample of liquid mercury (Hg) has a mass of 90.3 g. a) Find the molar mass of mercury (Hg). b) Determine the number of moles (mol) of mercury in the sample. 1 mol c) Determine the number of mercury atoms in the sample. The correct answer and explanation is : Let’s go step by […]<\/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-198567","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198567","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=198567"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198567\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=198567"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=198567"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=198567"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}