a sample of H2SO4 has a mass of 15.0 grams. 1. calculate the number of moles of H2SO4 molecules in the sample. 2. What is the number of molecules of H2SO4 in the sample? 3. How many atoms are there in the sample? 4. Find the number of oxygen atoms in the sample.<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n [ Using Avogadro\u2019s number<\/strong> (6.022 \u00d7 10\u00b2\u00b3 molecules\/mol): Each H\u2082SO\u2084 molecule contains:<\/p>\n\n\n\n Total atoms in the sample: Each molecule of H\u2082SO\u2084 has 4 oxygen atoms<\/strong>, so: Sulfuric acid (H\u2082SO\u2084<\/strong>) is a strong acid widely used in industries. In this problem, we calculated the number of moles, molecules, total atoms, and oxygen atoms in a 15.0 g<\/strong> sample of sulfuric acid.<\/p>\n\n\n\n First, to find the moles<\/strong>, we used the formula: Next, we determined the number of molecules<\/strong> using Avogadro\u2019s number<\/strong>, which is 6.022 \u00d7 10\u00b2\u00b3 molecules\/mol<\/strong>. By multiplying the moles by Avogadro\u2019s number, we obtained 9.21 \u00d7 10\u00b2\u00b2 molecules<\/strong> of H\u2082SO\u2084.<\/p>\n\n\n\n For the total number of atoms<\/strong>, we noted that each H\u2082SO\u2084 molecule has 7 atoms<\/strong> (2 hydrogen, 1 sulfur, and 4 oxygen). Multiplying the number of molecules by 7<\/strong>, we found 6.45 \u00d7 10\u00b2\u00b3 total atoms<\/strong> in the sample.<\/p>\n\n\n\n Finally, to determine the oxygen atoms<\/strong>, we noted that each H\u2082SO\u2084 molecule contains 4 oxygen atoms<\/strong>. Multiplying the number of molecules by 4<\/strong> resulted in 3.68 \u00d7 10\u00b2\u00b3 oxygen atoms<\/strong>.<\/p>\n\n\n\n These calculations illustrate the atomic composition of sulfuric acid and are essential in chemistry for stoichiometric calculations, reaction balancing, and industrial applications.<\/p>\n","protected":false},"excerpt":{"rendered":" a sample of H2SO4 has a mass of 15.0 grams. 1. calculate the number of moles of H2SO4 molecules in the sample. 2. What is the number of molecules of H2SO4 in the sample? 3. How many atoms are there in the sample? 4. Find the number of oxygen atoms in the sample. The Correct […]<\/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-187277","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187277","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=187277"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187277\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187277"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187277"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187277"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Given data:<\/h3>\n\n\n\n
\n
Step 1: Calculate the number of moles of H\u2082SO\u2084 molecules<\/strong><\/h4>\n\n\n\n
\\text{Moles} = \\frac{\\text{Mass}}{\\text{Molar Mass}} = \\frac{15.0 \\text{ g}}{98.08 \\text{ g\/mol}}
]
[
= 0.153 \\text{ moles of H\u2082SO\u2084}
]<\/p>\n\n\n\nStep 2: Find the number of molecules of H\u2082SO\u2084<\/strong><\/h4>\n\n\n\n
[
\\text{Molecules} = \\text{Moles} \\times \\text{Avogadro\u2019s Number}
]
[
= 0.153 \\times (6.022 \\times 10^{23})
]
[
= 9.21 \\times 10^{22} \\text{ molecules of H\u2082SO\u2084}
]<\/p>\n\n\n\nStep 3: Find the total number of atoms in the sample<\/strong><\/h4>\n\n\n\n
\n
[
\\text{Total atoms} = \\text{Molecules} \\times 7
]
[
= (9.21 \\times 10^{22}) \\times 7
]
[
= 6.45 \\times 10^{23} \\text{ atoms}
]<\/p>\n\n\n\nStep 4: Find the number of oxygen atoms<\/strong><\/h4>\n\n\n\n
[
\\text{Total oxygen atoms} = \\text{Molecules} \\times 4
]
[
= (9.21 \\times 10^{22}) \\times 4
]
[
= 3.68 \\times 10^{23} \\text{ oxygen atoms}
]<\/p>\n\n\n\n
\n\n\n\nExplanation (300 words)<\/strong><\/h3>\n\n\n\n
[
\\text{Moles} = \\frac{\\text{Mass}}{\\text{Molar Mass}}
]
Since the molar mass of H\u2082SO\u2084<\/strong> is 98.08 g\/mol<\/strong>, dividing the sample’s mass (15.0 g<\/strong>) gives 0.153 moles<\/strong> of H\u2082SO\u2084.<\/p>\n\n\n\n