how many atoms are there in 49 gm of H2SO4.how many atoms are there in 49 gm of H2SO4<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n To determine the number of atoms in 49 grams of H\u2082SO\u2084 (sulfuric acid)<\/strong>, we follow these steps:<\/p>\n\n\n\n The molar mass of sulfuric acid (H\u2082SO\u2084) is determined by adding the atomic masses of each element:<\/p>\n\n\n\n Total molar mass of H\u2082SO\u2084<\/strong> = 98.08 g\/mol<\/strong><\/p>\n\n\n\n Since 1 mole of H\u2082SO\u2084 weighs 98.08 g<\/strong>, the number of moles in 49 g is:<\/p>\n\n\n\n [ 1 mole of any substance contains Avogadro\u2019s number<\/strong> of molecules:<\/p>\n\n\n\n [ Thus, the number of molecules in 0.5 moles of H\u2082SO\u2084 is:<\/p>\n\n\n\n [ Each molecule of H\u2082SO\u2084 consists of:<\/p>\n\n\n\n Total atoms per molecule:<\/p>\n\n\n\n [ Thus, the total number of atoms in 3.011 \u00d7 10\u00b2\u00b3 molecules<\/strong> is:<\/p>\n\n\n\n [ 49 g of H\u2082SO\u2084 contains approximately<\/strong> ( 2.11 \\times 10^{24} ) atoms<\/strong>.<\/p>\n\n\n\n To determine the number of atoms in a given mass of a compound, we use the concept of moles and Avogadro\u2019s number. First, we find the molar mass of sulfuric acid (H\u2082SO\u2084), which is 98.08 g\/mol. This tells us that one mole of H\u2082SO\u2084 weighs 98.08 g. If we have 49 g of H\u2082SO\u2084, we calculate the number of moles by dividing by the molar mass: 49 \u00f7 98.08 = 0.5 moles<\/strong>.<\/p>\n\n\n\n Next, using Avogadro\u2019s number (6.022 \u00d7 10\u00b2\u00b3 molecules per mole)<\/strong>, we determine the number of molecules in 0.5 moles: Each molecule of sulfuric acid consists of 7 atoms<\/strong> (2 hydrogen, 1 sulfur, and 4 oxygen). To get the total number of atoms, we multiply the number of molecules by 7:<\/p>\n\n\n\n [ This means that in just 49 grams of H\u2082SO\u2084<\/strong>, there are approximately 2.11 \u00d7 10\u00b2\u2074 atoms<\/strong>, an enormous number! This calculation illustrates how even a small mass of a substance contains a vast number of atoms due to their incredibly tiny size.<\/p>\n","protected":false},"excerpt":{"rendered":" how many atoms are there in 49 gm of H2SO4.how many atoms are there in 49 gm of H2SO4 The Correct Answer and Explanation is : To determine the number of atoms in 49 grams of H\u2082SO\u2084 (sulfuric acid), we follow these steps: Step 1: Calculate the Molar Mass of H\u2082SO\u2084 The molar mass 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-187279","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187279","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=187279"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187279\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187279"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187279"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187279"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 1: Calculate the Molar Mass of H\u2082SO\u2084<\/strong><\/h3>\n\n\n\n
\n
Step 2: Determine the Number of Moles in 49 g of H\u2082SO\u2084<\/strong><\/h3>\n\n\n\n
\\text{Moles of H\u2082SO\u2084} = \\frac{49}{98.08} = 0.5 \\text{ moles}
]<\/p>\n\n\n\nStep 3: Determine the Number of Molecules<\/strong><\/h3>\n\n\n\n
\\text{Avogadro’s number} = 6.022 \\times 10^{23} \\text{ molecules\/mol}
]<\/p>\n\n\n\n
(0.5) \\times (6.022 \\times 10^{23}) = 3.011 \\times 10^{23} \\text{ molecules}
]<\/p>\n\n\n\nStep 4: Determine the Total Number of Atoms<\/strong><\/h3>\n\n\n\n
\n
2 + 1 + 4 = 7 \\text{ atoms}
]<\/p>\n\n\n\n
(3.011 \\times 10^{23}) \\times 7 = 2.108 \\times 10^{24} \\text{ atoms}
]<\/p>\n\n\n\nFinal Answer<\/strong><\/h3>\n\n\n\n
Explanation (300 words)<\/strong><\/h3>\n\n\n\n
0.5 \u00d7 (6.022 \u00d7 10\u00b2\u00b3) = 3.011 \u00d7 10\u00b2\u00b3 molecules<\/strong>.<\/p>\n\n\n\n
(3.011 \\times 10^{23}) \\times 7 = 2.108 \\times 10^{24} \\text{ atoms}
]<\/p>\n\n\n\n