{"id":3649,"date":"2023-01-09T10:10:15","date_gmt":"2023-01-09T10:10:15","guid":{"rendered":"https:\/\/9thclass.deltapublications.in\/?page_id=3649"},"modified":"2025-01-06T17:12:54","modified_gmt":"2025-01-06T17:12:54","slug":"s-3-e-molecular-mass-and-mole-concept","status":"publish","type":"page","link":"https:\/\/9thclass.deltapublications.in\/index.php\/s-3-e-molecular-mass-and-mole-concept\/","title":{"rendered":"S-3.e Molecular Mass And Mole Concept"},"content":{"rendered":"\n<h2 class=\"wp-block-heading has-text-align-center has-text-color\" style=\"color:#00056d;text-transform:uppercase\"><strong>Molecular Mass And Mole Concept<\/strong><\/h2>\n\n\n\n<p class=\"has-text-color has-link-color has-huge-font-size wp-elements-1b66da20fd6ce2f6c501f5f1f826f2fd\" style=\"color:#74008b;text-transform:capitalize\">Key notes :<\/p>\n\n\n\n<h3 class=\"wp-block-heading has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-879ea08e601565cc4345b36e2e53bfaf\" style=\"color:#000060;background-color:#dfc816\"><strong>Molecular Mass:<\/strong><\/h3>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li><strong>Definition<\/strong>: Molecular mass is the mass of one molecule of a substance, calculated by adding the atomic masses of the atoms in the molecule.<\/li>\n\n\n\n<li><strong>Unit<\/strong>: It is expressed in <strong>atomic mass units (amu)<\/strong> or <strong>g\/mol<\/strong>.<\/li>\n\n\n\n<li><strong>Example<\/strong>: The molecular mass of water (H\u2082O) is: <\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-large-font-size\"><strong>Molecular&nbsp;mass&nbsp;of&nbsp;H\u2082O = (2\u00d71) + (1\u00d716) = 18&nbsp;amu<\/strong><\/p>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li><strong>Importance<\/strong>: It helps in calculating the amount of substance needed for reactions and determining the number of molecules.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-eba00487d7420fd5cb7a4fb8efea6fef\" style=\"color:#000060;background-color:#dfc816\"><strong>Mole Concept:<\/strong><\/h3>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full is-resized\"><img loading=\"lazy\" decoding=\"async\" width=\"676\" height=\"564\" src=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-66.png\" alt=\"\" class=\"wp-image-16085\" style=\"width:385px;height:auto\" srcset=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-66.png 676w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-66-300x250.png 300w\" sizes=\"auto, (max-width: 676px) 100vw, 676px\" \/><\/figure><\/div>\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li><strong>Definition<\/strong>: A <strong>mole<\/strong> is a quantity used to count particles (atoms, molecules, ions, etc.). One mole of any substance contains <strong>6.022 \u00d7 10\u00b2\u00b3 particles<\/strong> (Avogadro\u2019s number).<\/li>\n\n\n\n<li><strong>Unit<\/strong>: Moles are expressed in <strong>mol<\/strong>.<\/li>\n\n\n\n<li><strong>Formula<\/strong>: <\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-large-font-size\"><strong>Number&nbsp;of&nbsp;moles = Mass&nbsp;of&nbsp;substance&nbsp;(in&nbsp;grams) \/ Molar&nbsp;mass&nbsp;(g\/mol)\u200b<\/strong><\/p>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li><strong>Example<\/strong>: If 18 grams of water (H\u2082O) is taken, the number of moles of water is:<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-large-font-size\"><strong>Moles&nbsp;of&nbsp;H\u2082O = 18&nbsp;g \/ 18&nbsp;g \/ mol = 1&nbsp;mole<\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-e71191772b68f18b8c25dbca1a75447c\" style=\"color:#000060;background-color:#dfc816\"><strong>Molar Mass:<\/strong><\/h3>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li><strong>Definition<\/strong>: The molar mass is the mass of one mole of a substance, usually in units of grams per mole (g\/mol).<\/li>\n\n\n\n<li><strong>Relationship with Molecular Mass<\/strong>: Molar mass (g\/mol) is numerically equal to molecular mass (amu), but the unit is grams per mole instead of atomic mass units.<\/li>\n\n\n\n<li><strong>Example<\/strong>: For water (H\u2082O), the molecular mass is 18 amu, and the molar mass is 18 g\/mol.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-cc1b40f0d7e41e24965cc75da4ee2b95\" style=\"color:#000060;background-color:#dfc816\"><strong>Avogadro\u2019s Number:<\/strong><\/h3>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li><strong>Definition<\/strong>: Avogadro&#8217;s number (6.022 \u00d7 10\u00b2\u00b3) is the number of particles in one mole of a substance.<\/li>\n\n\n\n<li><strong>Example<\/strong>: One mole of carbon atoms contains 6.022 \u00d7 10\u00b2\u00b3 carbon atoms.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-97d2ab74cc79a45aef96af3d2ac4f8a0\" style=\"color:#000060;background-color:#dfc816\"><strong>Mole and Chemical Reactions:<\/strong><\/h3>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li><strong>Stoichiometry<\/strong>: The mole concept is essential in stoichiometry to calculate the amount of reactants and products in a chemical reaction.<\/li>\n\n\n\n<li><strong>Balanced Equation<\/strong>: The coefficients in a balanced chemical equation represent the number of moles of each reactant and product involved.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-27c5dd2692afd770a47b7e6b8486d02d\" style=\"color:#000060;background-color:#dfc816\"><strong>Conversions:<\/strong><\/h3>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li><strong>From grams to moles<\/strong>: Use the formula:<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-large-font-size\"><strong>Moles = Mass&nbsp;(g) \/ Molar&nbsp;mass&nbsp;(g\/mol)<\/strong><\/p>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li><strong>From moles to molecules<\/strong>: Use Avogadro\u2019s number: <\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-large-font-size\"><strong>Number&nbsp;of&nbsp;molecules = Moles \u00d7 (6.022 \u00d7 10<sup>23<\/sup>)<\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-fed593f0f1b73e8c43c2c5c636e62588\" style=\"color:#000060;background-color:#dfc816\"><strong>Application in Chemistry:<\/strong><\/h3>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li><strong>Empirical Formula<\/strong>: The mole concept helps determine the simplest whole-number ratio of elements in a compound.<\/li>\n\n\n\n<li><strong>Molecular Formula<\/strong>: The actual number of atoms of each element in a molecule, determined using moles.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-82a62ddd71371839d89733245a2ecbeb\" style=\"color:#000060;background-color:#dfc816\"><strong>Summary:<\/strong><\/h3>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li>The mole concept links the atomic and macroscopic worlds.<\/li>\n\n\n\n<li>Molecular mass is the mass of a molecule, and molar mass is the mass of one mole of molecules.<\/li>\n\n\n\n<li>The mole is a convenient way to express quantities of substances involved in chemical reactions.<\/li>\n<\/ul>\n\n\n\n<div class=\"wp-block-group has-large-font-size\"><div class=\"wp-block-group__inner-container is-layout-constrained wp-block-group-is-layout-constrained\">\n<p class=\"has-text-color has-large-font-size\" style=\"color:#d90000\">Let&#8217;s practice!<\/p>\n<\/div><\/div>\n\n\n\n<div class=\"wp-block-columns is-layout-flex wp-container-core-columns-is-layout-9d6595d7 wp-block-columns-is-layout-flex\">\n<div class=\"wp-block-column is-layout-flow wp-block-column-is-layout-flow\">\n<figure class=\"wp-block-image size-full\"><a href=\"https:\/\/wordwall.net\/play\/75921\/503\/625\"><img loading=\"lazy\" decoding=\"async\" width=\"500\" height=\"500\" src=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-2-14.png\" alt=\"\" class=\"wp-image-6379\" srcset=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-2-14.png 500w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-2-14-300x300.png 300w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-2-14-150x150.png 150w\" sizes=\"auto, (max-width: 500px) 100vw, 500px\" \/><\/a><\/figure>\n<\/div>\n\n\n\n<div class=\"wp-block-column is-layout-flow wp-block-column-is-layout-flow\">\n<figure class=\"wp-block-image size-full\"><a href=\"https:\/\/wordwall.net\/play\/58851\/018\/998\"><img loading=\"lazy\" decoding=\"async\" width=\"500\" height=\"500\" src=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-1-1-15.png\" alt=\"\" class=\"wp-image-6380\" srcset=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-1-1-15.png 500w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-1-1-15-300x300.png 300w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-1-1-15-150x150.png 150w\" sizes=\"auto, (max-width: 500px) 100vw, 500px\" \/><\/a><\/figure>\n<\/div>\n<\/div>\n","protected":false},"excerpt":{"rendered":"<p>Molecular Mass And Mole Concept Key notes : Molecular Mass: Molecular&nbsp;mass&nbsp;of&nbsp;H\u2082O = (2\u00d71) + (1\u00d716) = 18&nbsp;amu Mole Concept: Number&nbsp;of&nbsp;moles = Mass&nbsp;of&nbsp;substance&nbsp;(in&nbsp;grams) \/ Molar&nbsp;mass&nbsp;(g\/mol)\u200b Moles&nbsp;of&nbsp;H\u2082O = 18&nbsp;g \/ 18&nbsp;g \/ mol = 1&nbsp;mole Molar Mass: Avogadro\u2019s Number: Mole and Chemical Reactions: Conversions: Moles = Mass&nbsp;(g) \/ Molar&nbsp;mass&nbsp;(g\/mol) Number&nbsp;of&nbsp;molecules = Moles \u00d7 (6.022 \u00d7 1023) Application<a class=\"more-link\" href=\"https:\/\/9thclass.deltapublications.in\/index.php\/s-3-e-molecular-mass-and-mole-concept\/\">Continue reading <span class=\"screen-reader-text\">&#8220;S-3.e Molecular Mass And Mole Concept&#8221;<\/span><\/a><\/p>\n","protected":false},"author":1,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"om_disable_all_campaigns":false,"_monsterinsights_skip_tracking":false,"_monsterinsights_sitenote_active":false,"_monsterinsights_sitenote_note":"","_monsterinsights_sitenote_category":0,"footnotes":""},"class_list":["post-3649","page","type-page","status-publish","hentry","entry"],"aioseo_notices":[],"_links":{"self":[{"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/pages\/3649","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/pages"}],"about":[{"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/types\/page"}],"author":[{"embeddable":true,"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/comments?post=3649"}],"version-history":[{"count":21,"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/pages\/3649\/revisions"}],"predecessor-version":[{"id":16340,"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/pages\/3649\/revisions\/16340"}],"wp:attachment":[{"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/media?parent=3649"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}