To solve this problem, we first need to determine the limiting reactant between calcium (Ca) and oxygen (O2) and then calculate the mass of calcium oxide (CaO) produced.<\/p>\n\n\n\n
Step 1: Write the balanced equation<\/h3>\n\n\n\n
The balanced chemical equation is:<\/p>\n\n\n\n
2Ca(s)+O2(g)\u21922CaO(s)2Ca (s) + O_2 (g) \\rightarrow 2CaO (s)2Ca(s)+O2\u200b(g)\u21922CaO(s)<\/p>\n\n\n\n
This means that 2 moles of calcium react with 1 mole of oxygen gas to produce 2 moles of calcium oxide.<\/p>\n\n\n\n
Step 2: Calculate moles of each reactant<\/h3>\n\n\n\n
To convert grams of each reactant to moles, we use the molar masses of calcium and oxygen:<\/p>\n\n\n\n
- \n
- Molar mass of calcium (Ca) = 40.08 g\/mol<\/li>\n\n\n\n
- Molar mass of oxygen (O2) = 32.00 g\/mol<\/li>\n<\/ul>\n\n\n\n
Moles of calcium (Ca):<\/h4>\n\n\n\n
moles of Ca=10.0\u2009g40.08\u2009g\/mol=0.249\u2009mol\\text{moles of Ca} = \\frac{10.0 \\, \\text{g}}{40.08 \\, \\text{g\/mol}} = 0.249 \\, \\text{mol}moles of Ca=40.08g\/mol10.0g\u200b=0.249mol<\/p>\n\n\n\n
Moles of oxygen (O2):<\/h4>\n\n\n\n
moles of O2=5.00\u2009g32.00\u2009g\/mol=0.15625\u2009mol\\text{moles of O}_2 = \\frac{5.00 \\, \\text{g}}{32.00 \\, \\text{g\/mol}} = 0.15625 \\, \\text{mol}moles of O2\u200b=32.00g\/mol5.00g\u200b=0.15625mol<\/p>\n\n\n\n
Step 3: Determine the limiting reactant<\/h3>\n\n\n\n
From the balanced equation, 2 moles of Ca react with 1 mole of O2. Therefore, the mole ratio is:Ca:O2=2:1\\text{Ca} : \\text{O}_2 = 2 : 1Ca:O2\u200b=2:1<\/p>\n\n\n\n
For 0.249 moles of calcium, the required moles of oxygen are:moles of O2=0.2492=0.1245\u2009mol\\text{moles of O}_2 = \\frac{0.249}{2} = 0.1245 \\, \\text{mol}moles of O2\u200b=20.249\u200b=0.1245mol<\/p>\n\n\n\n
Since we have 0.15625 moles of O2, which is more than enough (0.1245 mol), calcium (Ca)<\/strong> is the limiting reactant.<\/p>\n\n\n\n
Step 4: Calculate the moles of CaO produced<\/h3>\n\n\n\n
From the balanced equation, 2 moles of Ca produce 2 moles of CaO. Therefore, the moles of CaO produced will be equal to the moles of Ca reacted, which is 0.249 moles.<\/p>\n\n\n\n
Step 5: Convert moles of CaO to grams<\/h3>\n\n\n\n
Now, we calculate the mass of CaO produced. The molar mass of CaO is:Molar mass of CaO=40.08\u2009g\/mol (Ca)+16.00\u2009g\/mol (O)=56.08\u2009g\/mol\\text{Molar mass of CaO} = 40.08 \\, \\text{g\/mol (Ca)} + 16.00 \\, \\text{g\/mol (O)} = 56.08 \\, \\text{g\/mol}Molar mass of CaO=40.08g\/mol (Ca)+16.00g\/mol (O)=56.08g\/mol<\/p>\n\n\n\n
Now, multiply the moles of CaO by its molar mass:mass of CaO=0.249\u2009mol\u00d756.08\u2009g\/mol=13.95\u2009g\\text{mass of CaO} = 0.249 \\, \\text{mol} \\times 56.08 \\, \\text{g\/mol} = 13.95 \\, \\text{g}mass of CaO=0.249mol\u00d756.08g\/mol=13.95g<\/p>\n\n\n\n
Step 6: Round the result<\/h3>\n\n\n\n
The answer is approximately 14.0 g<\/strong> of calcium oxide (CaO).<\/p>\n\n\n\n
Final Answer:<\/h3>\n\n\n\n
The correct mass of CaO formed is 14.0 g<\/strong>.<\/p>\n\n\n\n
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-523.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"Consider the following balanced chemical equation: 2Ca + O2 (g) -> 2CaO. What mass of CaO, in grams, is formed when 10.0 grams of Ca reacts with 5.00 grams of O2? 10.0 g CaO 17.5 g CaO 8.76 g CaO 5.00 g CaO 14.0 g CaO The Correct Answer and Explanation is: To solve this […]<\/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-244812","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/244812","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=244812"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/244812\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=244812"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=244812"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=244812"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}