How many moles of K2SO4 are in 15.0 grams of K2SO4<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n To calculate the number of moles of K\u2082SO\u2084 in 15.0 grams of the compound, we need to follow these steps:<\/p>\n\n\n\n The molar mass of a compound is the sum of the atomic masses of all the elements in that compound, based on the periodic table. Potassium (K), sulfur (S), and oxygen (O) are the elements in potassium sulfate (K\u2082SO\u2084).<\/p>\n\n\n\n To find the molar mass of K\u2082SO\u2084, multiply the atomic masses by the number of atoms of each element in the formula:<\/p>\n\n\n\n [ [ Now that we know the molar mass of K\u2082SO\u2084 is 174.3 g\/mol, we can use the formula:<\/p>\n\n\n\n [ Substitute the given mass (15.0 grams) and the molar mass (174.3 g\/mol):<\/p>\n\n\n\n [ The number of moles of K\u2082SO\u2084 in 15.0 grams is 0.086 moles<\/strong>.<\/p>\n\n\n\n The process of converting grams to moles involves using the molar mass of the substance. The molar mass tells us how many grams one mole of a substance weighs. By dividing the mass of the substance by the molar mass, we determine how many moles are present in the sample. This concept is critical in stoichiometry for converting between mass and the amount of substance in moles, allowing us to perform calculations in chemical reactions.<\/p>\n","protected":false},"excerpt":{"rendered":" How many moles of K2SO4 are in 15.0 grams of K2SO4 The Correct Answer and Explanation is: To calculate the number of moles of K\u2082SO\u2084 in 15.0 grams of the compound, we need to follow these steps: Step 1: Find the molar mass of K\u2082SO\u2084 The molar mass of a compound is the sum of […]<\/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-169998","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/169998","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=169998"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/169998\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=169998"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=169998"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=169998"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 1: Find the molar mass of K\u2082SO\u2084<\/h3>\n\n\n\n
\n
\\text{Molar mass of K\u2082SO\u2084} = (2 \\times 39.1 \\, \\text{g\/mol}) + (1 \\times 32.1 \\, \\text{g\/mol}) + (4 \\times 16.0 \\, \\text{g\/mol})
]<\/p>\n\n\n\n
\\text{Molar mass of K\u2082SO\u2084} = 78.2 \\, \\text{g\/mol} + 32.1 \\, \\text{g\/mol} + 64.0 \\, \\text{g\/mol} = 174.3 \\, \\text{g\/mol}
]<\/p>\n\n\n\nStep 2: Use the molar mass to calculate the number of moles<\/h3>\n\n\n\n
\\text{Moles of K\u2082SO\u2084} = \\frac{\\text{Mass of K\u2082SO\u2084}}{\\text{Molar mass of K\u2082SO\u2084}}
]<\/p>\n\n\n\n
\\text{Moles of K\u2082SO\u2084} = \\frac{15.0 \\, \\text{g}}{174.3 \\, \\text{g\/mol}} = 0.086 \\, \\text{moles}
]<\/p>\n\n\n\nFinal Answer:<\/h3>\n\n\n\n
Explanation:<\/h3>\n\n\n\n