{"id":183788,"date":"2025-01-17T05:59:45","date_gmt":"2025-01-17T05:59:45","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=183788"},"modified":"2025-01-17T05:59:47","modified_gmt":"2025-01-17T05:59:47","slug":"complete-the-table-below-for-calculating-the-molar-mass-of-the-compound-nitrogen-dioxide","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/17\/complete-the-table-below-for-calculating-the-molar-mass-of-the-compound-nitrogen-dioxide\/","title":{"rendered":"Complete the table below for calculating the molar mass of the compound nitrogen dioxide"},"content":{"rendered":"\n

Complete the table below for calculating the molar mass of the compound nitrogen dioxide.<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

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

The molar mass of a compound is calculated by summing the molar masses of all the atoms in its chemical formula. For nitrogen dioxide ((NO_2)), we use the periodic table to find the atomic masses of nitrogen (N) and oxygen (O).<\/p>\n\n\n\n

Table for Molar Mass of (NO_2)<\/h3>\n\n\n\n
Element<\/strong><\/th>Number of Atoms<\/strong><\/th>Atomic Mass (g\/mol)<\/strong><\/th>Total Contribution (g\/mol)<\/strong><\/th><\/tr><\/thead>
Nitrogen (N)<\/td>1<\/td>14.01<\/td>(1 \\times 14.01 = 14.01)<\/td><\/tr>
Oxygen (O)<\/td>2<\/td>16.00<\/td>(2 \\times 16.00 = 32.00)<\/td><\/tr>
Total<\/strong><\/td><\/td><\/td>(14.01 + 32.00 = 46.01)<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

Explanation of the Calculation<\/h3>\n\n\n\n
    \n
  1. Determine the Atomic Masses:<\/strong><\/li>\n<\/ol>\n\n\n\n
      \n
    • The atomic mass of nitrogen (N) is (14.01 \\, \\text{g\/mol}), and oxygen (O) is (16.00 \\, \\text{g\/mol}), as found on the periodic table.<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Count the Number of Atoms:<\/strong><\/li>\n<\/ol>\n\n\n\n
          \n
        • In one molecule of (NO_2), there is 1 nitrogen atom and 2 oxygen atoms.<\/li>\n<\/ul>\n\n\n\n
            \n
          1. Multiply Atomic Mass by the Number of Atoms:<\/strong><\/li>\n<\/ol>\n\n\n\n
              \n
            • For nitrogen: (14.01 \\, \\text{g\/mol} \\times 1 = 14.01 \\, \\text{g\/mol})<\/li>\n\n\n\n
            • For oxygen: (16.00 \\, \\text{g\/mol} \\times 2 = 32.00 \\, \\text{g\/mol})<\/li>\n<\/ul>\n\n\n\n
                \n
              1. Add the Contributions:<\/strong><\/li>\n<\/ol>\n\n\n\n
                  \n
                • Total molar mass of (NO_2 = 14.01 \\, \\text{g\/mol} + 32.00 \\, \\text{g\/mol} = 46.01 \\, \\text{g\/mol}).<\/li>\n<\/ul>\n\n\n\n
                    \n
                  1. Significance of Molar Mass:<\/strong><\/li>\n<\/ol>\n\n\n\n
                      \n
                    • The molar mass allows chemists to convert between moles and grams, facilitating stoichiometric calculations in chemical reactions. For example, one mole of (NO_2) weighs (46.01 \\, \\text{g}).<\/li>\n<\/ul>\n\n\n\n
                        \n
                      1. Applications:<\/strong><\/li>\n<\/ol>\n\n\n\n
                          \n
                        • The calculated molar mass is used in various fields, such as environmental science (studying (NO_2) emissions) and industrial chemistry (where (NO_2) is a key intermediate in processes like nitric acid production).<\/li>\n<\/ul>\n\n\n\n

                          In summary, the molar mass of (NO_2) is (46.01 \\, \\text{g\/mol}), calculated by summing the atomic masses of all its constituent atoms based on their respective quantities in the compound.<\/p>\n","protected":false},"excerpt":{"rendered":"

                          Complete the table below for calculating the molar mass of the compound nitrogen dioxide. The Correct Answer and Explanation is : The molar mass of a compound is calculated by summing the molar masses of all the atoms in its chemical formula. For nitrogen dioxide ((NO_2)), we use the periodic table to find the atomic […]<\/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-183788","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183788","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=183788"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183788\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=183788"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=183788"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=183788"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}