{"id":229434,"date":"2025-06-08T07:37:55","date_gmt":"2025-06-08T07:37:55","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=229434"},"modified":"2025-06-08T07:37:57","modified_gmt":"2025-06-08T07:37:57","slug":"what-is-the-molar-mass-of-hbr","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/08\/what-is-the-molar-mass-of-hbr\/","title":{"rendered":"What is the molar mass of HBr"},"content":{"rendered":"\n

What is the molar mass of HBr?
What is the molar mass of HBr?<\/p>\n\n\n\n

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

ChatGPT said:<\/h6>\n\n\n\n

Correct Answer:<\/h3>\n\n\n\n

The molar mass of HBr (hydrogen bromide)<\/strong> is 80.91 g\/mol<\/strong>.<\/p>\n\n\n\n

\n\n\n\n

Explanation <\/h3>\n\n\n\n

The molar mass<\/strong> of a compound is the mass of one mole of that substance, typically expressed in grams per mole (g\/mol). It is calculated by summing the atomic masses of all atoms in the molecule, based on the periodic table.<\/p>\n\n\n\n

For hydrogen bromide (HBr)<\/strong>, the molecule consists of:<\/p>\n\n\n\n

    \n
  • 1 hydrogen (H) atom<\/strong><\/li>\n\n\n\n
  • 1 bromine (Br) atom<\/strong><\/li>\n<\/ul>\n\n\n\n

    Let\u2019s determine their atomic masses:<\/p>\n\n\n\n

      \n
    • Hydrogen (H):<\/strong> 1.008 g\/mol<\/li>\n\n\n\n
    • Bromine (Br):<\/strong> 79.904 g\/mol<\/li>\n<\/ul>\n\n\n\n

      To calculate the molar mass of HBr:Molar mass of HBr=Atomic mass of H+Atomic mass of Br\\text{Molar mass of HBr} = \\text{Atomic mass of H} + \\text{Atomic mass of Br}Molar mass of HBr=Atomic mass of H+Atomic mass of Br=1.008 g\/mol+79.904 g\/mol=80.912 g\/mol= 1.008\\ \\text{g\/mol} + 79.904\\ \\text{g\/mol} = 80.912\\ \\text{g\/mol}=1.008 g\/mol+79.904 g\/mol=80.912 g\/mol<\/p>\n\n\n\n

      Rounded to two decimal places, the molar mass of HBr is 80.91 g\/mol<\/strong>.<\/p>\n\n\n\n

      This value is essential in chemistry for various calculations. For example, when working with gases, knowing the molar mass allows chemists to convert between grams and moles using the formula:Moles=Mass (g)Molar mass (g\/mol)\\text{Moles} = \\frac{\\text{Mass (g)}}{\\text{Molar mass (g\/mol)}}Moles=Molar mass (g\/mol)Mass (g)\u200b<\/p>\n\n\n\n

      Hydrogen bromide is a diatomic molecule<\/strong> and an important hydrogen halide<\/strong>, used in both industrial and laboratory settings. It exists as a gas at room temperature and forms hydrobromic acid (HBr(aq))<\/strong> when dissolved in water.<\/p>\n\n\n\n

      Understanding the molar mass is also important in stoichiometry<\/strong>, where balanced chemical equations require mole ratios. For example, in reactions involving HBr, you would use its molar mass to determine how much reactant or product is needed or formed.<\/p>\n\n\n\n

      In summary, the molar mass of HBr is 80.91 g\/mol<\/strong>, calculated by summing the atomic masses of hydrogen and bromine. This value is fundamental for performing precise chemical calculations involving hydrogen bromide.<\/p>\n\n\n\n

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

      What is the molar mass of HBr?What is the molar mass of HBr? The Correct Answer and Explanation is: ChatGPT said: Correct Answer: The molar mass of HBr (hydrogen bromide) is 80.91 g\/mol. Explanation The molar mass of a compound is the mass of one mole of that substance, typically expressed in grams per mole […]<\/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-229434","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/229434","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=229434"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/229434\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=229434"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=229434"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=229434"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}