{"id":194431,"date":"2025-02-24T06:04:37","date_gmt":"2025-02-24T06:04:37","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=194431"},"modified":"2025-02-24T06:04:40","modified_gmt":"2025-02-24T06:04:40","slug":"calculate-the-molar-mass-of-k2so4-use-masses-k-39-103-o-15-935-and-s32-053","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/24\/calculate-the-molar-mass-of-k2so4-use-masses-k-39-103-o-15-935-and-s32-053\/","title":{"rendered":"Calculate the molar mass of K2SO4 (Use Masses K: 39.103, O: 15.935 and S:32.053)"},"content":{"rendered":"\n

Calculate the molar mass of K2SO4 (Use Masses K: 39.103, O: 15.935 and S:
32.053). You must show full calculation for credit<\/p>\n\n\n\n

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

Calculation of the Molar Mass of K\u2082SO\u2084<\/strong><\/h3>\n\n\n\n

To determine the molar mass of potassium sulfate (K\u2082SO\u2084), we need to sum up the atomic masses of its constituent elements: potassium (K), sulfur (S), and oxygen (O).<\/p>\n\n\n\n

Step-by-Step Calculation:<\/strong><\/h4>\n\n\n\n
    \n
  1. Potassium (K):<\/strong><\/li>\n<\/ol>\n\n\n\n
      \n
    • There are two<\/strong> potassium (K) atoms.<\/li>\n\n\n\n
    • Atomic mass of K = 39.103 g\/mol<\/strong><\/li>\n\n\n\n
    • Total mass from potassium = 2 \u00d7 39.103<\/strong> = 78.206 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n
        \n
      1. Sulfur (S):<\/strong><\/li>\n<\/ol>\n\n\n\n
          \n
        • There is one<\/strong> sulfur (S) atom.<\/li>\n\n\n\n
        • Atomic mass of S = 32.053 g\/mol<\/strong><\/li>\n\n\n\n
        • Total mass from sulfur = 32.053 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n
            \n
          1. Oxygen (O):<\/strong><\/li>\n<\/ol>\n\n\n\n
              \n
            • There are four<\/strong> oxygen (O) atoms.<\/li>\n\n\n\n
            • Atomic mass of O = 15.935 g\/mol<\/strong><\/li>\n\n\n\n
            • Total mass from oxygen = 4 \u00d7 15.935<\/strong> = 63.740 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n

              Final Molar Mass Calculation:<\/strong><\/h4>\n\n\n\n

              [
              \\text{Molar mass of K\u2082SO\u2084} = 78.206 + 32.053 + 63.740
              ]
              [
              = 173.999 \\, \\text{g\/mol}
              ]<\/p>\n\n\n\n

              \n\n\n\n

              Explanation (300 words)<\/strong><\/h3>\n\n\n\n

              The molar mass of a compound represents the mass of one mole of its molecules and is expressed in grams per mole (g\/mol). To find the molar mass, we add the atomic masses of all atoms in the chemical formula.<\/p>\n\n\n\n

              In the case of potassium sulfate (K\u2082SO\u2084), the compound consists of two potassium (K) atoms, one sulfur (S) atom, and four oxygen (O) atoms. Each element has a known atomic mass:<\/p>\n\n\n\n

                \n
              • Potassium (K) has a mass of 39.103 g\/mol<\/strong>,<\/li>\n\n\n\n
              • Sulfur (S) has a mass of 32.053 g\/mol<\/strong>, and<\/li>\n\n\n\n
              • Oxygen (O) has a mass of 15.935 g\/mol<\/strong>.<\/li>\n<\/ul>\n\n\n\n

                By multiplying these atomic masses by the number of atoms present in the formula and summing them, we obtain the total molar mass.<\/p>\n\n\n\n

                This calculation is essential in various chemical applications, such as stoichiometry, where we determine the amount of a substance needed or produced in a reaction. It is also crucial in pharmaceuticals, material science, and industry to ensure the correct amounts of chemicals are used.<\/p>\n\n\n\n

                For example, in agriculture, potassium sulfate is a widely used fertilizer. Knowing its molar mass allows chemists to calculate the precise amount needed to provide an adequate supply of potassium and sulfur to crops.<\/p>\n\n\n\n

                By understanding how to compute molar mass accurately, chemists can make precise calculations for chemical reactions, ensuring efficiency and preventing wastage of materials.<\/p>\n\n\n\n

                Thus, the molar mass of K\u2082SO\u2084 is 173.999 g\/mol<\/strong>.<\/p>\n\n\n\n

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

                I have generated an educational illustration that visually represents the step-by-step molar mass calculation of K\u2082SO\u2084. Let me know if you need any modifications or further explanations!<\/p>\n\n\n\n

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

                Calculate the molar mass of K2SO4 (Use Masses K: 39.103, O: 15.935 and S:32.053). You must show full calculation for credit The Correct Answer and Explanation is : Calculation of the Molar Mass of K\u2082SO\u2084 To determine the molar mass of potassium sulfate (K\u2082SO\u2084), we need to sum up the atomic masses of its constituent […]<\/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-194431","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194431","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=194431"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194431\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=194431"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=194431"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=194431"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}