Sulfuric acid (H2SO4 Molar Mass = 98.1) can be prepared from S8, O2 and H2O by the following series of reactions. Balance!<\/p>\n\n\n\n
S8 + 8O2 -> 8SO2<\/p>\n\n\n\n
2SO2 + O2 -> 2SO3<\/p>\n\n\n\n
SO3 + H2O -> H2SO4<\/p>\n\n\n\n
What volume of sulfuric acid is produced from reacting 70.0 grams sulfur with sufficient oxygen and water?
(Specify gravity sulfuric acid = 1.12)<\/p>\n\n\n\n
The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n To calculate the volume of sulfuric acid produced from 70.0 grams of sulfur (S8), we will proceed step by step using stoichiometry and the chemical equations provided. Here\u2019s the breakdown:<\/p>\n\n\n\n The chemical reactions provided are:<\/p>\n\n\n\n The molar mass of sulfur is 32.07 g\/mol. For the molecule ( S_8 ), the molar mass is:<\/p>\n\n\n\n [ To determine how many moles of sulfur are in 70.0 grams, we use the formula:<\/p>\n\n\n\n [ [ Next, we calculate how many moles of sulfuric acid (H2SO4) are produced. From the reactions, the stoichiometric relationship is 1 mole of ( S_8 ) produces 1 mole of ( H_2SO_4 ). Therefore, the moles of ( H_2SO_4 ) produced is:<\/p>\n\n\n\n [ The molar mass of sulfuric acid (H2SO4) is 98.1 g\/mol. Thus, the mass of sulfuric acid produced is:<\/p>\n\n\n\n [ [ Given the density of sulfuric acid is 1.12 g\/mL, we can now calculate the volume of sulfuric acid produced using the formula:<\/p>\n\n\n\n [ [ Thus, from 70.0 grams of sulfur, approximately 23.93 mL<\/strong> of sulfuric acid is produced, assuming sufficient oxygen and water are available for the reactions.<\/p>\n","protected":false},"excerpt":{"rendered":" Sulfuric acid (H2SO4 Molar Mass = 98.1) can be prepared from S8, O2 and H2O by the following series of reactions. Balance! S8 + 8O2 -> 8SO2 2SO2 + O2 -> 2SO3 SO3 + H2O -> H2SO4 What volume of sulfuric acid is produced from reacting 70.0 grams sulfur with sufficient oxygen and water?(Specify gravity […]<\/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-209637","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/209637","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=209637"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/209637\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=209637"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=209637"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=209637"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}1. Balanced Reactions<\/strong><\/h3>\n\n\n\n
\n
[
S_8 + 8O_2 \\rightarrow 8SO_2
]<\/li>\n\n\n\n
[
2SO_2 + O_2 \\rightarrow 2SO_3
]<\/li>\n\n\n\n
[
SO_3 + H_2O \\rightarrow H_2SO_4
]<\/li>\n<\/ol>\n\n\n\n2. Molar Mass of Sulfur (S8)<\/strong><\/h3>\n\n\n\n
\\text{Molar Mass of } S_8 = 32.07 \\times 8 = 256.56 \\, \\text{g\/mol}
]<\/p>\n\n\n\n3. Moles of Sulfur (S8)<\/strong><\/h3>\n\n\n\n
\\text{moles of } S_8 = \\frac{\\text{mass of sulfur}}{\\text{molar mass of } S_8}
]<\/p>\n\n\n\n
\\text{moles of } S_8 = \\frac{70.0 \\, \\text{g}}{256.56 \\, \\text{g\/mol}} \\approx 0.2735 \\, \\text{mol}
]<\/p>\n\n\n\n4. Moles of Sulfuric Acid (H2SO4)<\/strong><\/h3>\n\n\n\n
\\text{moles of H}_2\\text{SO}_4 = 0.2735 \\, \\text{mol}
]<\/p>\n\n\n\n5. Mass of Sulfuric Acid<\/strong><\/h3>\n\n\n\n
\\text{mass of H}_2\\text{SO}_4 = \\text{moles of H}_2\\text{SO}_4 \\times \\text{molar mass of H}_2\\text{SO}_4
]<\/p>\n\n\n\n
\\text{mass of H}_2\\text{SO}_4 = 0.2735 \\, \\text{mol} \\times 98.1 \\, \\text{g\/mol} \\approx 26.8 \\, \\text{g}
]<\/p>\n\n\n\n6. Volume of Sulfuric Acid<\/strong><\/h3>\n\n\n\n
\\text{volume of H}_2\\text{SO}_4 = \\frac{\\text{mass of H}_2\\text{SO}_4}{\\text{density of H}_2\\text{SO}_4}
]<\/p>\n\n\n\n
\\text{volume of H}_2\\text{SO}_4 = \\frac{26.8 \\, \\text{g}}{1.12 \\, \\text{g\/mL}} \\approx 23.93 \\, \\text{mL}
]<\/p>\n\n\n\nConclusion<\/h3>\n\n\n\n