{"id":252954,"date":"2025-07-11T15:33:48","date_gmt":"2025-07-11T15:33:48","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=252954"},"modified":"2025-07-11T15:33:49","modified_gmt":"2025-07-11T15:33:49","slug":"calculate-the-relative-molecular-masses-of","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/11\/calculate-the-relative-molecular-masses-of\/","title":{"rendered":"Calculate the relative molecular masses of"},"content":{"rendered":"\n

Calculate the relative molecular masses of: Potassium chlorate<\/p>\n\n\n\n

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

To calculate the relative molecular mass (also called molecular weight) of potassium chlorate (KClO\u2083), we need to sum the atomic masses of all the atoms in one molecule of the compound.<\/p>\n\n\n\n

Step-by-step calculation:<\/h3>\n\n\n\n
    \n
  1. Identify the elements in potassium chlorate (KClO\u2083)<\/strong>:\n
      \n
    • Potassium (K)<\/li>\n\n\n\n
    • Chlorine (Cl)<\/li>\n\n\n\n
    • Oxygen (O)<\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • Determine the atomic masses<\/strong>:\n
        \n
      • Potassium (K) has an atomic mass of approximately 39.1 g\/mol.<\/li>\n\n\n\n
      • Chlorine (Cl) has an atomic mass of approximately 35.5 g\/mol.<\/li>\n\n\n\n
      • Oxygen (O) has an atomic mass of approximately 16.0 g\/mol.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • Account for the number of atoms of each element in the formula<\/strong>:\n
          \n
        • KClO\u2083 contains 1 atom of potassium (K),<\/li>\n\n\n\n
        • 1 atom of chlorine (Cl),<\/li>\n\n\n\n
        • 3 atoms of oxygen (O).<\/li>\n<\/ul>\n<\/li>\n\n\n\n
        • Multiply the atomic masses by the number of atoms<\/strong>:\n
            \n
          • Potassium: 1\u00d739.1=39.1\u2009g\/mol1 \\times 39.1 = 39.1 \\, \\text{g\/mol}1\u00d739.1=39.1g\/mol<\/li>\n\n\n\n
          • Chlorine: 1\u00d735.5=35.5\u2009g\/mol1 \\times 35.5 = 35.5 \\, \\text{g\/mol}1\u00d735.5=35.5g\/mol<\/li>\n\n\n\n
          • Oxygen: 3\u00d716.0=48.0\u2009g\/mol3 \\times 16.0 = 48.0 \\, \\text{g\/mol}3\u00d716.0=48.0g\/mol<\/li>\n<\/ul>\n<\/li>\n\n\n\n
          • Add them together to get the relative molecular mass<\/strong>: Molecular\u00a0mass\u00a0of\u00a0KClO\u2083=39.1+35.5+48.0=122.6\u2009g\/mol\\text{Molecular mass of KClO\u2083} = 39.1 + 35.5 + 48.0 = 122.6 \\, \\text{g\/mol}Molecular\u00a0mass\u00a0of\u00a0KClO\u2083=39.1+35.5+48.0=122.6g\/mol<\/li>\n<\/ol>\n\n\n\n

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

            The relative molecular mass of potassium chlorate (KClO\u2083) is 122.6 g\/mol.<\/p>\n\n\n\n

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

            Calculate the relative molecular masses of: Potassium chlorate The Correct Answer and Explanation is: To calculate the relative molecular mass (also called molecular weight) of potassium chlorate (KClO\u2083), we need to sum the atomic masses of all the atoms in one molecule of the compound. Step-by-step calculation: Conclusion: The relative molecular mass of potassium chlorate […]<\/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-252954","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/252954","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=252954"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/252954\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=252954"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=252954"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=252954"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}