The chemical formula for potassium bromide is KBr. A chemist measured the amount of potassium bromide produced during an experiment. She finds that 58.1 g of potassium bromide is produced. Calculate the number of moles of potassium bromide produced. Be sure your answer has the correct number of significant digits.<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n To calculate the number of moles of potassium bromide (KBr) produced, we use the formula:<\/p>\n\n\n\n [ The mass of potassium bromide produced is given as 58.1 grams.<\/p>\n\n\n\n Potassium bromide (KBr) consists of two elements: potassium (K) and bromine (Br). To find the molar mass of KBr, we need to sum the atomic masses of these two elements:<\/p>\n\n\n\n The molar mass of KBr is:<\/p>\n\n\n\n [ Now we can use the formula to calculate the number of moles of potassium bromide produced:<\/p>\n\n\n\n [ The mass of KBr is provided to three significant digits (58.1 g), and the molar mass of KBr has three significant digits (119.0 g\/mol). Therefore, the final answer should be reported with three significant digits.<\/p>\n\n\n\n Thus, the number of moles of potassium bromide produced is:<\/p>\n\n\n\n [ The process involves converting the mass of a substance into the number of moles, which is a direct measure of the amount of a substance in terms of its molecular quantity. The conversion relies on the molar mass, a constant derived from the sum of the atomic masses of the constituent elements. The number of moles is crucial in stoichiometric calculations because it relates the mass of a substance to the number of molecules or atoms it contains.<\/p>\n","protected":false},"excerpt":{"rendered":" The chemical formula for potassium bromide is KBr. A chemist measured the amount of potassium bromide produced during an experiment. She finds that 58.1 g of potassium bromide is produced. Calculate the number of moles of potassium bromide produced. Be sure your answer has the correct number of significant digits. The Correct Answer and Explanation […]<\/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-186276","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186276","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=186276"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186276\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=186276"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=186276"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=186276"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\\text{Moles} = \\frac{\\text{Mass}}{\\text{Molar Mass}}
]<\/p>\n\n\n\nStep 1: Identify the mass<\/h3>\n\n\n\n
Step 2: Determine the molar mass of KBr<\/h3>\n\n\n\n
\n
\\text{Molar Mass of KBr} = 39.1 \\, \\text{g\/mol} + 79.9 \\, \\text{g\/mol} = 119.0 \\, \\text{g\/mol}
]<\/p>\n\n\n\nStep 3: Calculate the number of moles<\/h3>\n\n\n\n
\\text{Moles of KBr} = \\frac{58.1 \\, \\text{g}}{119.0 \\, \\text{g\/mol}} = 0.488 \\, \\text{mol}
]<\/p>\n\n\n\nStep 4: Consider significant digits<\/h3>\n\n\n\n
0.488 \\, \\text{mol}
]<\/p>\n\n\n\nExplanation:<\/h3>\n\n\n\n