{"id":199607,"date":"2025-03-12T07:25:44","date_gmt":"2025-03-12T07:25:44","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=199607"},"modified":"2025-03-12T07:25:46","modified_gmt":"2025-03-12T07:25:46","slug":"given-the-balanced-equation-below-and-knowing-that-0-0470-grams-of-magnesium-metal-fully-reacted","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/12\/given-the-balanced-equation-below-and-knowing-that-0-0470-grams-of-magnesium-metal-fully-reacted\/","title":{"rendered":"Given the balanced equation below and knowing that 0.0470 grams of magnesium metal fully reacted"},"content":{"rendered":"\n

Given the balanced equation below and knowing that 0.0470 grams of magnesium metal fully reacted, determine how many grams of hydrogen gas formed as a result of that reaction.<\/p>\n\n\n\n

Mg (s) + 2 HCl (aq) = MgCl2 (aq) + H2 (g)<\/p>\n\n\n\n

The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n

Solution:<\/h3>\n\n\n\n
    \n
  1. Balanced Chemical Equation:<\/strong> Mg(s)+2HCl(aq)\u2192MgCl2(aq)+H2(g)\\text{Mg} (s) + 2 \\text{HCl} (aq) \\rightarrow \\text{MgCl}_2 (aq) + \\text{H}_2 (g)<\/li>\n\n\n\n
  2. Find the Molar Masses:<\/strong>\n
      \n
    • Magnesium (Mg) = 24.305 g\/mol<\/strong><\/li>\n\n\n\n
    • Hydrogen gas (H\u2082) = 2.016 g\/mol<\/strong><\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • Convert Mass of Mg to Moles:<\/strong> Moles\u00a0of\u00a0Mg=0.0470\u00a0g24.305\u00a0g\/mol\\text{Moles of Mg} = \\frac{0.0470 \\text{ g}}{24.305 \\text{ g\/mol}} =0.001934\u00a0moles\u00a0of\u00a0Mg= 0.001934 \\text{ moles of Mg}<\/li>\n\n\n\n
    • Use Stoichiometry to Find Moles of H\u2082:<\/strong>\n
        \n
      • From the balanced equation, 1 mole of Mg produces 1 mole of H\u2082<\/strong>.<\/li>\n\n\n\n
      • Therefore, moles of H\u2082 produced<\/strong>: 0.001934\u00a0moles\u00a0of\u00a0H\u20820.001934 \\text{ moles of H\u2082}<\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • Convert Moles of H\u2082 to Mass:<\/strong> Mass\u00a0of\u00a0H2=0.001934\u00d72.016\u00a0g\/mol\\text{Mass of H}_2 = 0.001934 \\times 2.016 \\text{ g\/mol} =0.00390\u00a0g\u00a0of\u00a0H2= 0.00390 \\text{ g of H}_2<\/li>\n<\/ol>\n\n\n\n

        Final Answer: 0.00390 g of H\u2082<\/strong><\/h3>\n\n\n\n
        \n\n\n\n

        Explanation:<\/h3>\n\n\n\n

        This reaction is a classic example of a single replacement reaction<\/strong>, where magnesium reacts with hydrochloric acid to produce magnesium chloride and hydrogen gas<\/strong>. Since magnesium is more reactive than hydrogen, it displaces hydrogen from the acid.<\/p>\n\n\n\n

        To determine the amount of hydrogen gas formed, we used stoichiometry:<\/p>\n\n\n\n

          \n
        1. Converted given Mg mass to moles<\/strong> using its molar mass.<\/li>\n\n\n\n
        2. Used the molar ratio (1:1) from the balanced equation<\/strong> to find moles of H\u2082 produced.<\/li>\n\n\n\n
        3. Converted moles of H\u2082 to grams<\/strong> using the molar mass of hydrogen gas.<\/li>\n<\/ol>\n\n\n\n

          Thus, when 0.0470 g of Mg fully reacts<\/strong>, it produces 0.00390 g of H\u2082 gas<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"

          Given the balanced equation below and knowing that 0.0470 grams of magnesium metal fully reacted, determine how many grams of hydrogen gas formed as a result of that reaction. Mg (s) + 2 HCl (aq) = MgCl2 (aq) + H2 (g) The correct answer and explanation is : Solution: Final Answer: 0.00390 g of H\u2082 […]<\/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-199607","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/199607","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=199607"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/199607\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=199607"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=199607"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=199607"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}