Converting 53.3g of oxygen to moles will give you???
0.30 mol O<\/p>\n\n\n\n
8.5 mol O<\/p>\n\n\n\n
3.33 mol O<\/p>\n\n\n\n
5.3 mol O<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n To convert grams of oxygen (O\u2082) to moles, you need to use the molar mass of oxygen. The molar mass of O\u2082 (molecular oxygen) is approximately 32.00 grams per mole (g\/mol), since each oxygen atom has a molar mass of about 16.00 g\/mol, and there are two oxygen atoms in an O\u2082 molecule.<\/p>\n\n\n\n This calculation indicates that 53.3 grams of molecular oxygen corresponds to approximately 1.67 moles of O\u2082.<\/p>\n\n\n\n Now, reviewing the provided answer options:<\/p>\n\n\n\n None of the options match our calculated result of 1.67 mol O\u2082. However, if we consider the amount of oxygen atoms in the original question, we must recognize that O\u2082 contains two oxygen atoms. Thus, to find the number of moles of individual oxygen atoms (O), you would double the moles of O\u2082:<\/p>\n\n\n\n [ This leads to the conclusion that approximately 3.33 moles of O atoms<\/strong> are present in 53.3 grams of O\u2082.<\/p>\n\n\n\n Therefore, the correct answer from the options given would be 3.33 mol O<\/strong>.<\/p>\n\n\n\n In summary, the conversion process illustrates how to determine the number of moles of a substance from its mass and how to interpret the results concerning molecular and atomic forms of elements.<\/p>\n","protected":false},"excerpt":{"rendered":" Converting 53.3g of oxygen to moles will give you???0.30 mol O 8.5 mol O 3.33 mol O 5.3 mol O The Correct Answer and Explanation is : To convert grams of oxygen (O\u2082) to moles, you need to use the molar mass of oxygen. The molar mass of O\u2082 (molecular oxygen) is approximately 32.00 grams […]<\/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-145101","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/145101","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=145101"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/145101\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=145101"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=145101"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=145101"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Calculation Steps:<\/h3>\n\n\n\n
\n
[
\\text{Moles of O}_2 = \\frac{\\text{mass of O}_2 (\\text{g})}{\\text{molar mass of O}_2 (\\text{g\/mol})}
]<\/li>\n\n\n\n
[
\\text{Moles of O}_2 = \\frac{53.3 \\, \\text{g}}{32.00 \\, \\text{g\/mol}} \\approx 1.67 \\, \\text{mol O}_2
]<\/li>\n<\/ol>\n\n\n\nAnswer Options:<\/h3>\n\n\n\n
\n
\\text{Moles of O} = 2 \\times 1.67 \\, \\text{mol O}_2 \\approx 3.34 \\, \\text{mol O}
]<\/p>\n\n\n\nCorrect Answer:<\/h3>\n\n\n\n