what is the mass of 3.81 mol of ph3? show work on scratch paper! group of answer choices 34.0 g 3.81 g 8.92 g 130. g 0.112<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n The Correct Answer is : 130.0 g<\/strong><\/p>\n\n\n\n To find the mass of 3.81 moles of phosphine (( \\text{PH}_3 )), we need to use the formula for calculating mass from moles, which is given by:<\/p>\n\n\n\n [ The molar mass of a compound is calculated by summing the atomic masses of all the atoms present in the molecule.<\/p>\n\n\n\n In ( \\text{PH}_3 ), there is 1 phosphorus atom and 3 hydrogen atoms. Thus, the molar mass can be calculated as follows:<\/p>\n\n\n\n [ Calculating the contributions from each element:<\/p>\n\n\n\n [ Now that we have the molar mass, we can substitute the values into the mass formula:<\/p>\n\n\n\n [ Calculating the mass:<\/p>\n\n\n\n [ The mass of 3.81 moles of ( \\text{PH}_3 ) is approximately 130.0 g<\/strong> when rounded to three significant figures.<\/p>\n\n\n\n This process shows how to convert between moles and mass using the molar mass as a conversion factor. Understanding this relationship is essential in chemistry, especially when dealing with reactions and stoichiometry, as it allows for the calculation of the quantities of reactants and products in a chemical reaction.<\/p>\n","protected":false},"excerpt":{"rendered":" what is the mass of 3.81 mol of ph3? show work on scratch paper! group of answer choices 34.0 g 3.81 g 8.92 g 130. g 0.112 The Correct Answer and Explanation is : The Correct Answer is : 130.0 g To find the mass of 3.81 moles of phosphine (( \\text{PH}_3 )), we need […]<\/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-148560","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/148560","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=148560"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/148560\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=148560"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=148560"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=148560"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\\text{Mass} = \\text{Moles} \\times \\text{Molar Mass}
]<\/p>\n\n\n\nStep 1: Calculate the Molar Mass of ( \\text{PH}_3 )<\/h3>\n\n\n\n
\n
\\text{Molar Mass of } \\text{PH}_3 = (1 \\times 30.97 \\, \\text{g\/mol}) + (3 \\times 1.01 \\, \\text{g\/mol})
]<\/p>\n\n\n\n
\\text{Molar Mass of } \\text{PH}_3 = 30.97 \\, \\text{g\/mol} + 3.03 \\, \\text{g\/mol} = 34.00 \\, \\text{g\/mol}
]<\/p>\n\n\n\nStep 2: Calculate the Mass of 3.81 moles of ( \\text{PH}_3 )<\/h3>\n\n\n\n
\\text{Mass} = 3.81 \\, \\text{mol} \\times 34.00 \\, \\text{g\/mol}
]<\/p>\n\n\n\n
\\text{Mass} = 3.81 \\times 34.00 = 129.54 \\, \\text{g}
]<\/p>\n\n\n\nConclusion<\/h3>\n\n\n\n