To calculate the formula mass of zinc nitrite (Zn(NO2)2)<\/strong>, you need to find the atomic masses of all the elements in the compound and add them together.<\/p>\n\n\n\n The formula mass of Zn(NO2)2<\/strong> is 157.40 g\/mol<\/strong>.<\/p>\n\n\n\n Formula mass is simply the sum of the atomic masses of all elements in the formula, and it gives us the total mass of one mole of the compound. Each element in the compound has its specific atomic mass, which you can find on the periodic table. By multiplying the atomic mass of each element by the number of atoms of that element in the compound and then adding them together, you get the formula mass.<\/p>\n\n\n\n For Zn(NO2)2<\/strong>, the mass is calculated as follows:<\/p>\n\n\n\n What is the correct formula mass for Zn(NO2)2 The Correct Answer and Explanation is: To calculate the formula mass of zinc nitrite (Zn(NO2)2), you need to find the atomic masses of all the elements in the compound and add them together. Step-by-step Calculation: Final Answer: The formula mass of Zn(NO2)2 is 157.40 g\/mol. Explanation: Formula […]<\/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-240013","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/240013","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=240013"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/240013\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=240013"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=240013"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=240013"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step-by-step Calculation:<\/h3>\n\n\n\n
\n
The atomic mass of zinc is 65.38 g\/mol<\/strong>.<\/li>\n\n\n\n
A nitrite ion (NO2) consists of:
Zinc nitrite has one zinc atom (Zn) and two nitrite ions (NO2). The total formula mass is the sum of the atomic mass of zinc and the mass of two nitrite ions: 1\u00d765.38\u2009(Zn)+2\u00d746.01\u2009(NO2)=65.38+92.02=157.40\u2009g\/mol1 \\times 65.38 \\, (\\text{Zn}) + 2 \\times 46.01 \\, (\\text{NO2}) = 65.38 + 92.02 = 157.40 \\, \\text{g\/mol}1\u00d765.38(Zn)+2\u00d746.01(NO2)=65.38+92.02=157.40g\/mol<\/li>\n<\/ol>\n\n\n\nFinal Answer:<\/h3>\n\n\n\n
Explanation:<\/h3>\n\n\n\n
\n
Thus, the overall mass is 157.40 g\/mol<\/strong>.<\/li>\n<\/ul>\n\n\n\n![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-92.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"