Phosphoric acid (H3PO4, molar mass 98.0) can be prepared from P4 and O2 by the following series of reactions:
P4 + 5O2 ? P4O10
P4O10 + 6H2O ? 4H3PO4
16.5 grams of H3PO4 were formed by reacting 0.0500 mole of P4 with sufficient O2 and H2O. Calculate the percent yield.<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n To calculate the percent yield of phosphoric acid (H\u2083PO\u2084), we need to follow a few steps:<\/p>\n\n\n\n From the balanced reaction:<\/p>\n\n\n\n [ P_4 + 5O_2 \\to P_4O_{10} ] We are given that 0.0500 mole of P\u2084 reacts to form H\u2083PO\u2084. The second reaction shows that 1 mole of P\u2084O\u2081\u2080 (formed from 1 mole of P\u2084) produces 4 moles of H\u2083PO\u2084. Therefore, we can calculate the theoretical amount of H\u2083PO\u2084:<\/p>\n\n\n\n [ Now, we can calculate the theoretical mass of H\u2083PO\u2084 produced:<\/p>\n\n\n\n [ The percent yield is calculated using the formula:<\/p>\n\n\n\n [ We are given that the actual yield is 16.5 grams. So:<\/p>\n\n\n\n [ In this problem, the theoretical yield of phosphoric acid (H\u2083PO\u2084) is determined by stoichiometry, where we use the number of moles of the reactant (P\u2084) to predict how much product (H\u2083PO\u2084) should be formed under ideal conditions. Since we know the actual yield of H\u2083PO\u2084 is 16.5 grams, the percent yield measures the efficiency of the reaction by comparing the actual yield to the theoretical yield. In this case, the reaction achieved 84.2% of the expected product, which indicates a relatively efficient synthesis of phosphoric acid.<\/p>\n","protected":false},"excerpt":{"rendered":" Phosphoric acid (H3PO4, molar mass 98.0) can be prepared from P4 and O2 by the following series of reactions:P4 + 5O2 ? P4O10P4O10 + 6H2O ? 4H3PO416.5 grams of H3PO4 were formed by reacting 0.0500 mole of P4 with sufficient O2 and H2O. Calculate the percent yield. The Correct Answer and Explanation is : To […]<\/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-182216","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182216","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=182216"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182216\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=182216"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=182216"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=182216"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 1: Moles of Phosphoric Acid (H\u2083PO\u2084) Expected<\/h3>\n\n\n\n
[ P_4O_{10} + 6H_2O \\to 4H_3PO_4 ]<\/p>\n\n\n\n
\\text{Moles of H\u2083PO\u2084} = 0.0500 \\, \\text{mol of P\u2084} \\times \\frac{4 \\, \\text{mol of H\u2083PO\u2084}}{1 \\, \\text{mol of P\u2084}} = 0.200 \\, \\text{mol of H\u2083PO\u2084}
]<\/p>\n\n\n\nStep 2: Theoretical Mass of H\u2083PO\u2084<\/h3>\n\n\n\n
\\text{Mass of H\u2083PO\u2084} = 0.200 \\, \\text{mol of H\u2083PO\u2084} \\times 98.0 \\, \\text{g\/mol} = 19.6 \\, \\text{g}
]<\/p>\n\n\n\nStep 3: Percent Yield<\/h3>\n\n\n\n
\\text{Percent Yield} = \\frac{\\text{Actual Yield}}{\\text{Theoretical Yield}} \\times 100
]<\/p>\n\n\n\n
\\text{Percent Yield} = \\frac{16.5 \\, \\text{g}}{19.6 \\, \\text{g}} \\times 100 = 84.2\\%
]<\/p>\n\n\n\nExplanation<\/h3>\n\n\n\n