{"id":222295,"date":"2025-05-31T08:08:58","date_gmt":"2025-05-31T08:08:58","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=222295"},"modified":"2025-05-31T08:09:00","modified_gmt":"2025-05-31T08:09:00","slug":"titanium-dioxide-tio2-is-a-white-molecule-that-is-used-as-a-pigment-for-white-paint","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/31\/titanium-dioxide-tio2-is-a-white-molecule-that-is-used-as-a-pigment-for-white-paint\/","title":{"rendered":"Titanium dioxide (TIO2) is a white molecule that is used as a pigment for white paint."},"content":{"rendered":"\n

Titanium dioxide (TIO2) is a white molecule that is used as a pigment for white paint. It is produced industrially by treating a mineral called ilmenite (FeTiO3) with sulfuric acid according the molecular equation below. In one particular reaction, 8,000 Kg of FeTiO3was used as a starting material for the reaction. What is the theoretical yield of TiO2? MW FeTiO3= 151.72 g\/mol, MW TiO2= 79.88 g\/mol. FeTiO3+ H2SO4\u00c3\u00a2\u00e2\u20ac \u00e2\u20ac\u2122 TiO2+ FeSO4+ H2O
Titanium dioxide (TIO2) is a white molecule that is used as a pigment for white paint. It is produced industrially by treating a mineral called ilmenite (FeTiO3) with sulfuric acid according the molecular equation below. In one particular reaction, 8,000 Kg of FeTiO3was used as a starting material for the reaction. What is the theoretical yield of TiO2? MW FeTiO3= 151.72 g\/mol, MW TiO2= 79.88 g\/mol.<\/p>\n\n\n\n

FeTiO3+ H2SO4\u00c3\u00a2\u00e2\u20ac \u00e2\u20ac\u2122 TiO2+ FeSO4+ H2O<\/p>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

Theoretical Yield of TiO\u2082 from FeTiO\u2083 Reaction<\/strong><\/h3>\n\n\n\n

Given:<\/strong><\/p>\n\n\n\n

    \n
  • Reaction:
    FeTiO\u2083 + H\u2082SO\u2084 \u2192 TiO\u2082 + FeSO\u2084 + H\u2082O<\/li>\n\n\n\n
  • Starting amount of FeTiO\u2083: 8000 kg = 8,000,000 g<\/strong><\/li>\n\n\n\n
  • Molar mass (MW) of FeTiO\u2083: 151.72 g\/mol<\/strong><\/li>\n\n\n\n
  • Molar mass (MW) of TiO\u2082: 79.88 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n

    Step-by-Step Calculation:<\/strong><\/h3>\n\n\n\n
      \n
    1. Convert mass of FeTiO\u2083 to moles:<\/strong><\/li>\n<\/ol>\n\n\n\n

      Moles of FeTiO\u2083=8,000,000 g151.72 g\/mol\u224852,712.68 mol\\text{Moles of FeTiO\u2083} = \\frac{8,000,000\\ \\text{g}}{151.72\\ \\text{g\/mol}} \\approx 52,712.68\\ \\text{mol}<\/p>\n\n\n\n

        \n
      1. Use the mole ratio from the balanced equation:<\/strong><\/li>\n<\/ol>\n\n\n\n

        From the reaction:
        1 mol FeTiO\u2083 \u2192 1 mol TiO\u2082
        So, moles of TiO\u2082 produced = moles of FeTiO\u2083 = 52,712.68 mol<\/strong><\/p>\n\n\n\n

          \n
        1. Convert moles of TiO\u2082 to grams:<\/strong><\/li>\n<\/ol>\n\n\n\n

          Mass of TiO\u2082=52,712.68 mol\u00d779.88 g\/mol\u22484,211,751.78 g\\text{Mass of TiO\u2082} = 52,712.68\\ \\text{mol} \\times 79.88\\ \\text{g\/mol} \\approx 4,211,751.78\\ \\text{g}<\/p>\n\n\n\n

            \n
          1. Convert grams to kilograms:<\/strong><\/li>\n<\/ol>\n\n\n\n

            4,211,751.78 g1000=4211.75 kg\\frac{4,211,751.78\\ \\text{g}}{1000} = \\boxed{4211.75\\ \\text{kg}}<\/p>\n\n\n\n

            \n\n\n\n

            \u2705 Theoretical Yield of TiO\u2082: 4211.75 kg<\/strong><\/h3>\n\n\n\n
            \n\n\n\n

            Explanation<\/strong><\/h3>\n\n\n\n

            Titanium dioxide (TiO\u2082) is a crucial white pigment widely used in paint, sunscreen, and food products due to its brightness and opacity. Industrially, TiO\u2082 is produced from ilmenite (FeTiO\u2083), a naturally occurring ore, by reacting it with sulfuric acid (H\u2082SO\u2084). The balanced chemical equation is: FeTiO\u2083+H\u2082SO\u2084\u2192TiO\u2082+FeSO\u2084+H\u2082O\\text{FeTiO\u2083} + \\text{H\u2082SO\u2084} \\rightarrow \\text{TiO\u2082} + \\text{FeSO\u2084} + \\text{H\u2082O}<\/p>\n\n\n\n

            This indicates a 1:1 molar ratio<\/strong> between FeTiO\u2083 and TiO\u2082\u2014each mole of FeTiO\u2083 yields one mole of TiO\u2082.<\/p>\n\n\n\n

            In this problem, the goal is to find the theoretical yield of TiO\u2082 when 8000 kg (8,000,000 g)<\/strong> of FeTiO\u2083 is used. First, we determine how many moles of FeTiO\u2083 are present by dividing its mass by its molar mass (151.72 g\/mol). This gives approximately 52,712.68 moles<\/strong>. Since the reaction produces TiO\u2082 in a 1:1 molar ratio, the same number of moles of TiO\u2082 is produced.<\/p>\n\n\n\n

            Next, to find the mass of TiO\u2082 produced, we multiply the moles by the molar mass of TiO\u2082 (79.88 g\/mol), which results in approximately 4,211,751.78 grams<\/strong>, or 4211.75 kilograms<\/strong>.<\/p>\n\n\n\n

            This value represents the theoretical yield<\/strong>\u2014the maximum possible mass of TiO\u2082 that can be produced under ideal conditions, assuming the reaction goes to completion and there are no losses. In practice, actual yield may be less due to incomplete reactions or process inefficiencies.<\/p>\n\n\n\n

            \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

            Titanium dioxide (TIO2) is a white molecule that is used as a pigment for white paint. It is produced industrially by treating a mineral called ilmenite (FeTiO3) with sulfuric acid according the molecular equation below. In one particular reaction, 8,000 Kg of FeTiO3was used as a starting material for the reaction. What is the theoretical […]<\/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-222295","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/222295","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=222295"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/222295\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=222295"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=222295"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=222295"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}