To calculate the mass of water that would form when 26.9 cm\u00b3 of trisilane reacts completely with excess oxygen, we can follow these steps:<\/p>\n\n\n\n
Step 1: Determine the number of moles of trisilane (Si\u2083H\u2088).<\/h3>\n\n\n\n
We are given the volume of trisilane (26.9 cm\u00b3) and its density (0.739 g\/cm\u00b3). First, we calculate the mass of trisilane using the formula:Mass=Density\u00d7Volume\\text{Mass} = \\text{Density} \\times \\text{Volume}Mass=Density\u00d7VolumeMass of Si\u2083H\u2088=0.739\u2009g\/cm3\u00d726.9\u2009cm3=19.9\u2009g\\text{Mass of Si\u2083H\u2088} = 0.739 \\, \\text{g\/cm}^3 \\times 26.9 \\, \\text{cm}^3 = 19.9 \\, \\text{g}Mass of Si\u2083H\u2088=0.739g\/cm3\u00d726.9cm3=19.9g<\/p>\n\n\n\n
Next, we calculate the number of moles of trisilane using its molar mass. The molar mass of Si\u2083H\u2088 is:Molar mass of Si\u2083H\u2088=(3\u00d728.085\u2009g\/mol)+(8\u00d71.008\u2009g\/mol)=88.258\u2009g\/mol\\text{Molar mass of Si\u2083H\u2088} = (3 \\times 28.085 \\, \\text{g\/mol}) + (8 \\times 1.008 \\, \\text{g\/mol}) = 88.258 \\, \\text{g\/mol}Molar mass of Si\u2083H\u2088=(3\u00d728.085g\/mol)+(8\u00d71.008g\/mol)=88.258g\/mol<\/p>\n\n\n\n
Now, calculate the moles of Si\u2083H\u2088:Moles of Si\u2083H\u2088=Mass of Si\u2083H\u2088Molar mass of Si\u2083H\u2088=19.9\u2009g88.258\u2009g\/mol\u22480.225\u2009mol\\text{Moles of Si\u2083H\u2088} = \\frac{\\text{Mass of Si\u2083H\u2088}}{\\text{Molar mass of Si\u2083H\u2088}} = \\frac{19.9 \\, \\text{g}}{88.258 \\, \\text{g\/mol}} \\approx 0.225 \\, \\text{mol}Moles of Si\u2083H\u2088=Molar mass of Si\u2083H\u2088Mass of Si\u2083H\u2088\u200b=88.258g\/mol19.9g\u200b\u22480.225mol<\/p>\n\n\n\n
Step 2: Write the balanced chemical equation.<\/h3>\n\n\n\n
The balanced reaction between trisilane and oxygen to form silicon dioxide and water is:Si\u2083H\u2088+4\u2009O\u2082\u21923\u2009SiO\u2082+4\u2009H\u2082O\\text{Si\u2083H\u2088} + 4 \\, \\text{O\u2082} \\rightarrow 3 \\, \\text{SiO\u2082} + 4 \\, \\text{H\u2082O}Si\u2083H\u2088+4O\u2082\u21923SiO\u2082+4H\u2082O<\/p>\n\n\n\n
From this equation, we see that 1 mole of Si\u2083H\u2088 produces 4 moles of H\u2082O.<\/p>\n\n\n\n
Step 3: Calculate the moles of water produced.<\/h3>\n\n\n\n
Since 1 mole of Si\u2083H\u2088 produces 4 moles of H\u2082O, the moles of water produced from 0.225 moles of Si\u2083H\u2088 is:Moles of H\u2082O=0.225\u2009mol\u00d74=0.900\u2009mol\\text{Moles of H\u2082O} = 0.225 \\, \\text{mol} \\times 4 = 0.900 \\, \\text{mol}Moles of H\u2082O=0.225mol\u00d74=0.900mol<\/p>\n\n\n\n
Step 4: Calculate the mass of water produced.<\/h3>\n\n\n\n
The molar mass of water (H\u2082O) is:Molar mass of H\u2082O=(2\u00d71.008\u2009g\/mol)+(1\u00d715.999\u2009g\/mol)=18.016\u2009g\/mol\\text{Molar mass of H\u2082O} = (2 \\times 1.008 \\, \\text{g\/mol}) + (1 \\times 15.999 \\, \\text{g\/mol}) = 18.016 \\, \\text{g\/mol}Molar mass of H\u2082O=(2\u00d71.008g\/mol)+(1\u00d715.999g\/mol)=18.016g\/mol<\/p>\n\n\n\n
Now, calculate the mass of water:Mass of H\u2082O=Moles of H\u2082O\u00d7Molar mass of H\u2082O=0.900\u2009mol\u00d718.016\u2009g\/mol\u224816.2\u2009g\\text{Mass of H\u2082O} = \\text{Moles of H\u2082O} \\times \\text{Molar mass of H\u2082O} = 0.900 \\, \\text{mol} \\times 18.016 \\, \\text{g\/mol} \\approx 16.2 \\, \\text{g}Mass of H\u2082O=Moles of H\u2082O\u00d7Molar mass of H\u2082O=0.900mol\u00d718.016g\/mol\u224816.2g<\/p>\n\n\n\n
Final Answer:<\/h3>\n\n\n\n
The mass of water formed is approximately 16.2 grams<\/strong>.<\/p>\n\n\n\n Trisilane (Si3H8) is a liquid with a density of 0.739 g cm-3. It reacts with oxygen to give silicon dioxide (SiO2) and water. Calculate the mass of water that would form if 26.9 cm3 of trisilane reacted completely with excess oxygen. _________g water The Correct Answer and Explanation is: To calculate the mass of water […]<\/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-246079","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246079","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=246079"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246079\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246079"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246079"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246079"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-783.jpeg\")
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