{"id":151737,"date":"2024-10-10T10:38:14","date_gmt":"2024-10-10T10:38:14","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=151737"},"modified":"2024-10-10T10:38:17","modified_gmt":"2024-10-10T10:38:17","slug":"determine-the-empirical-formula-for-a-compound-that-is-36-86-n-and-63-14-o-by-mass","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/10\/10\/determine-the-empirical-formula-for-a-compound-that-is-36-86-n-and-63-14-o-by-mass\/","title":{"rendered":"Determine the empirical formula for a compound that is 36.86% n and 63.14% o by mass"},"content":{"rendered":"\n

Determine the empirical formula for a compound that is 36.86% n and 63.14% o by mass. determine the empirical formula for a compound that is 36.86% n and 63.14% o by mass. no<\/p>\n\n\n\n

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

The correct answer is: ( \\text{N}_2\\text{O}_3 )<\/strong><\/mark>.<\/p>\n\n\n\n

To determine the empirical formula of a compound composed of 36.86% nitrogen (N) and 63.14% oxygen (O) by mass, we follow these steps:<\/p>\n\n\n\n

    \n
  1. Convert percentages to grams<\/strong>: Assume we have 100 grams of the compound. This means we have 36.86 grams of nitrogen and 63.14 grams of oxygen.<\/li>\n\n\n\n
  2. Convert grams to moles<\/strong>: Use the molar mass of each element to convert grams to moles. The molar mass of nitrogen (N) is approximately 14.01 g\/mol, and for oxygen (O), it is approximately 16.00 g\/mol. [
    \\text{Moles of N} = \\frac{36.86 \\, \\text{g}}{14.01 \\, \\text{g\/mol}} \\approx 2.63 \\, \\text{mol}
    ] [
    \\text{Moles of O} = \\frac{63.14 \\, \\text{g}}{16.00 \\, \\text{g\/mol}} \\approx 3.95 \\, \\text{mol}
    ]<\/li>\n\n\n\n
  3. Find the mole ratio<\/strong>: To get the simplest whole number ratio, divide the number of moles of each element by the smallest number of moles calculated. [
    \\text{Mole ratio of N} = \\frac{2.63 \\, \\text{mol}}{2.63} = 1
    ] [
    \\text{Mole ratio of O} = \\frac{3.95 \\, \\text{mol}}{2.63} \\approx 1.50
    ]<\/li>\n\n\n\n
  4. Convert to whole numbers<\/strong>: The ratio of N to O is approximately 1:1.5. To convert this to whole numbers, we can multiply both by 2 to eliminate the fraction: [
    \\text{N} : \\text{O} = 1 \\times 2 : 1.5 \\times 2 = 2 : 3
    ]<\/li>\n\n\n\n
  5. Write the empirical formula<\/strong>: The empirical formula is expressed as ( \\text{N}_2\\text{O}_3 ).<\/li>\n<\/ol>\n\n\n\n

    In summary, the empirical formula for the compound with 36.86% nitrogen and 63.14% oxygen is ( \\text{N}_2\\text{O}_3 ). This process illustrates how to convert mass percentages into an empirical formula by calculating moles, determining ratios, and converting to whole numbers, which are foundational skills in chemistry for understanding compound composition.<\/p>\n","protected":false},"excerpt":{"rendered":"

    Determine the empirical formula for a compound that is 36.86% n and 63.14% o by mass. determine the empirical formula for a compound that is 36.86% n and 63.14% o by mass. no The Correct Answer and Explanation is : The correct answer is: ( \\text{N}_2\\text{O}_3 ). To determine the empirical formula of a compound […]<\/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-151737","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/151737","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=151737"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/151737\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=151737"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=151737"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=151737"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}