{"id":27028,"date":"2025-06-19T20:33:30","date_gmt":"2025-06-19T20:33:30","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=27028"},"modified":"2025-06-19T20:33:35","modified_gmt":"2025-06-19T20:33:35","slug":"how-many-grams-are-contained-in-10-00-mol-of-lithium-sulfate-li2so4","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/how-many-grams-are-contained-in-10-00-mol-of-lithium-sulfate-li2so4\/","title":{"rendered":"How many grams are contained in 10.00 mol of lithium sulfate, Li2SO4"},"content":{"rendered":"\n<p>How many grams are contained in 10.00 mol of lithium sulfate, Li2SO4?<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-cyan-blue-color\"><strong>The correct answer and explanation is:<\/strong><\/mark><\/p>\n\n\n\n<p>To find how many grams are contained in 10.00 moles of lithium sulfate (Li\u2082SO\u2084), you need to follow these steps:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Determine the molar mass of lithium sulfate (Li\u2082SO\u2084).<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Lithium (Li) atomic mass = 6.94 g\/mol<\/li>\n\n\n\n<li>Sulfur (S) atomic mass = 32.07 g\/mol<\/li>\n\n\n\n<li>Oxygen (O) atomic mass = 16.00 g\/mol<\/li>\n<\/ul>\n\n\n\n<p>Lithium sulfate has:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>2 lithium atoms<\/li>\n\n\n\n<li>1 sulfur atom<\/li>\n\n\n\n<li>4 oxygen atoms<\/li>\n<\/ul>\n\n\n\n<p>Calculate the molar mass:<br>Molar mass of Li\u2082SO\u2084 = (2 \u00d7 6.94) + (1 \u00d7 32.07) + (4 \u00d7 16.00)<br>= 13.88 + 32.07 + 64.00<br>= <strong>109.95 g\/mol<\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Use the molar mass to convert moles to grams.<\/h3>\n\n\n\n<p>The formula to convert moles to grams is:<br>mass&nbsp;(g)=number&nbsp;of&nbsp;moles\u00d7molar&nbsp;mass&nbsp;(g\/mol)\\text{mass (g)} = \\text{number of moles} \\times \\text{molar mass (g\/mol)}<\/p>\n\n\n\n<p>Given:<br>Number of moles = 10.00 mol<br>Molar mass = 109.95 g\/mol<\/p>\n\n\n\n<p>Calculate the mass:<br>mass=10.00\u00d7109.95=1099.5&nbsp;grams\\text{mass} = 10.00 \\times 109.95 = 1099.5 \\text{ grams}<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Final answer:<\/h3>\n\n\n\n<p><strong>10.00 moles of lithium sulfate contain 1099.5 grams.<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>Moles measure the amount of substance based on the number of particles (atoms, ions, or molecules). Each compound has a characteristic molar mass\u2014the mass of one mole of that compound. This molar mass depends on the sum of the atomic masses of all atoms in the formula.<\/p>\n\n\n\n<p>For lithium sulfate (Li\u2082SO\u2084), the molar mass is calculated by adding the atomic masses of lithium, sulfur, and oxygen in their respective quantities. Lithium is light with a mass of 6.94 g\/mol, sulfur is heavier at 32.07 g\/mol, and oxygen atoms weigh 16.00 g\/mol each. By multiplying these atomic masses by their subscripts in the chemical formula and adding them, you get the total molar mass.<\/p>\n\n\n\n<p>Once the molar mass is known, converting moles to grams is straightforward: multiply the number of moles by the molar mass. Since the user has 10 moles of Li\u2082SO\u2084, the mass will be 10 times the molar mass, yielding approximately 1100 grams.<\/p>\n\n\n\n<p>This conversion is critical in chemistry for preparing solutions, reactions, and understanding stoichiometry \u2014 the quantitative relationships between reactants and products in chemical reactions.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>How many grams are contained in 10.00 mol of lithium sulfate, Li2SO4? The correct answer and explanation is: To find how many grams are contained in 10.00 moles of lithium sulfate (Li\u2082SO\u2084), you need to follow these steps: Step 1: Determine the molar mass of lithium sulfate (Li\u2082SO\u2084). Lithium sulfate has: Calculate the molar mass:Molar [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-27028","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/27028","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=27028"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/27028\/revisions"}],"predecessor-version":[{"id":27031,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/27028\/revisions\/27031"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=27028"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=27028"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=27028"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}