How many grams of iron (II) oxide can be produced from 3.4 g of iron in this balanced equation?
4Fe +3022Fe\u2082O3<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n To answer your questions, we need to balance the chemical equations, determine the molar masses of the reactants and products, and use stoichiometry to find the mass of the products formed from the given masses of the reactants.<\/p>\n\n\n\n Balanced Equation:<\/strong> Step 1: Calculate moles of Fe.<\/strong><\/p>\n\n\n\n Step 2: Use stoichiometry to find moles of Fe\u2082O\u2083 produced.<\/strong> Step 3: Calculate grams of Fe\u2082O\u2083.<\/strong><\/p>\n\n\n\n Balanced Equation:<\/strong> Step 1: Calculate moles of MgO.<\/strong><\/p>\n\n\n\n Step 2: Use stoichiometry to find moles of MgCO\u2083 produced.<\/strong> Step 3: Calculate grams of MgCO\u2083.<\/strong><\/p>\n\n\n\n Balanced Equation:<\/strong> Step 1: Calculate moles of CaCl\u2082.<\/strong><\/p>\n\n\n\n Step 2: Use stoichiometry to find moles of Ca(OH)\u2082 produced.<\/strong> Step 3: Calculate grams of Ca(OH)\u2082.<\/strong><\/p>\n\n\n\n The process of determining the mass of products formed from given reactants is based on stoichiometry, which involves balanced chemical equations that reflect the conservation of mass. The molar masses of the compounds are essential to convert grams to moles, allowing us to use the ratios from the balanced equations to predict the amounts of products produced. Each step ensures accurate conversion and results in the final calculations, showcasing the interrelationship between reactants and products in chemical reactions.<\/p>\n","protected":false},"excerpt":{"rendered":" How many grams of iron (II) oxide can be produced from 3.4 g of iron in this balanced equation?4Fe +3022Fe\u2082O3 The Correct Answer and Explanation is : To answer your questions, we need to balance the chemical equations, determine the molar masses of the reactants and products, and use stoichiometry to find the 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-156324","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/156324","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=156324"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/156324\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=156324"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=156324"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=156324"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}1. Iron (II) oxide from iron<\/h3>\n\n\n\n
[ 4 \\text{Fe} + 3 \\text{O}_2 \\rightarrow 2 \\text{Fe}_2\\text{O}_3 ]<\/p>\n\n\n\n\n
[ \\text{Moles of Fe} = \\frac{3.4 \\text{ g}}{55.85 \\text{ g\/mol}} \\approx 0.061 \\text{ mol} ]<\/li>\n<\/ul>\n\n\n\n
From the balanced equation, 4 moles of Fe produce 2 moles of Fe\u2082O\u2083:
[ \\text{Moles of Fe}_2\\text{O}_3 = \\frac{0.061 \\text{ mol Fe}}{4} \\times 2 \\approx 0.0305 \\text{ mol Fe}_2\\text{O}_3 ]<\/p>\n\n\n\n\n
[ \\text{Grams of Fe}_2\\text{O}_3 = 0.0305 \\text{ mol} \\times 159.69 \\text{ g\/mol} \\approx 4.87 \\text{ g} ]<\/li>\n<\/ul>\n\n\n\n2. Magnesium carbonate from magnesium oxide<\/h3>\n\n\n\n
[ \\text{MgO} + \\text{CO}_2 \\rightarrow \\text{MgCO}_3 ]<\/p>\n\n\n\n\n
[ \\text{Moles of MgO} = \\frac{6.7 \\text{ g}}{40.30 \\text{ g\/mol}} \\approx 0.166 \\text{ mol} ]<\/li>\n<\/ul>\n\n\n\n
From the balanced equation, 1 mole of MgO produces 1 mole of MgCO\u2083:
[ \\text{Moles of MgCO}_3 = 0.166 \\text{ mol MgO} ]<\/p>\n\n\n\n\n
[ \\text{Grams of MgCO}_3 = 0.166 \\text{ mol} \\times 84.31 \\text{ g\/mol} \\approx 14.0 \\text{ g} ]<\/li>\n<\/ul>\n\n\n\n3. Calcium hydroxide from calcium chloride<\/h3>\n\n\n\n
[ \\text{CaCl}_2 + 2 \\text{NaOH} \\rightarrow \\text{Ca(OH)}_2 + 2 \\text{NaCl} ]<\/p>\n\n\n\n\n
[ \\text{Moles of CaCl}_2 = \\frac{9.4 \\text{ g}}{110.98 \\text{ g\/mol}} \\approx 0.0846 \\text{ mol} ]<\/li>\n<\/ul>\n\n\n\n
From the balanced equation, 1 mole of CaCl\u2082 produces 1 mole of Ca(OH)\u2082:
[ \\text{Moles of Ca(OH)}_2 = 0.0846 \\text{ mol CaCl}_2 ]<\/p>\n\n\n\n\n
[ \\text{Grams of Ca(OH)}_2 = 0.0846 \\text{ mol} \\times 74.09 \\text{ g\/mol} \\approx 6.26 \\text{ g} ]<\/li>\n<\/ul>\n\n\n\nSummary of Results<\/h3>\n\n\n\n
\n
Explanation<\/h3>\n\n\n\n