{"id":230915,"date":"2025-06-10T08:04:46","date_gmt":"2025-06-10T08:04:46","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=230915"},"modified":"2025-06-10T08:04:48","modified_gmt":"2025-06-10T08:04:48","slug":"how-many-molecules-are-there-in-4-00-moles-of-glucose-c6h12o6","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/10\/how-many-molecules-are-there-in-4-00-moles-of-glucose-c6h12o6\/","title":{"rendered":"How many molecules are there in 4.00 moles of glucose, C6H12O6"},"content":{"rendered":"\n

How many molecules are there in 4.00 moles of glucose, C6H12O6? 4.00 moles = 4.00 x 6.022 x 10^23 molecules = 2.4088 x 10^24 molecules When the units are set up properly, the unit you are converting FROM will cancel out: You are left with the desired unit you are converting TO. 3. How many moles are 20 x 10^23 atoms of phosphorus? 20 x 10^23 atoms = 20 x 10^23 \/ 6.022 x 10^23 = 3.32 moles How many atoms are in 0.750 moles of zinc? 0.750 moles = 0.750 x 6.022 x 10^23 atoms = 4.5165 x 10^23 atoms How many molecules are in 0.400 moles of NO2? 0.400 moles = 0.400 x 6.022 x 10^23 molecules = 2.4088 x 10^23 molecules 6. How many atoms are in 0.340 moles of sodium? 0.340 moles = 0.340 x 6.022 x 10^23 atoms = 2.04908 x 10^23 atoms How many moles are in 204 x 10^23 molecules of Bromine? 204 x 10^23 molecules = 204 x 10^23 \/ 6.022 x 10^23 = 3.388 moles How many molecules are in 0.75 moles of oxygen gas? 0.75 moles = 0.75 x 6.022 x 10^23 molecules = 4.5165 x 10^23 molecules How many moles are present in 2.45 x 10^23 molecules of CH4? 2.45 x 10^23 molecules = 2.45 x 10^23 \/ 6.022 x 10^23 = 0.406 moles How many moles are there in 3.4 x 10^23 molecules of NH3? 3.4 x 10^23 molecules = 3.4 x 10^23 \/ 6.022 x 10^23 = 0.564 moles<\/p>\n\n\n\n

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

Correct Answer:<\/h3>\n\n\n\n

How many moles are there in 3.4 \u00d7 10\u00b2\u00b3 molecules of NH\u2083?<\/strong>Moles of NH\u2083=3.4\u00d71023 molecules6.022\u00d71023 molecules\/mol\u22480.564 moles\\text{Moles of NH\u2083} = \\frac{3.4 \\times 10^{23} \\text{ molecules}}{6.022 \\times 10^{23} \\text{ molecules\/mol}} \\approx 0.564 \\text{ moles}Moles of NH\u2083=6.022\u00d71023 molecules\/mol3.4\u00d71023 molecules\u200b\u22480.564 moles<\/p>\n\n\n\n

\n\n\n\n

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

In chemistry, the concept of the mole<\/strong> allows scientists to count particles like atoms, ions, or molecules by weighing them. This is essential because individual particles are so small that counting them one by one isn’t practical. To bridge the gap between the microscopic world and measurable quantities, we use Avogadro\u2019s number<\/strong>, which is:6.022\u00d71023 particles\/mole6.022 \\times 10^{23} \\text{ particles\/mole}6.022\u00d71023 particles\/mole<\/p>\n\n\n\n

This number represents how many particles (atoms, molecules, etc.) are in one mole of a substance. When converting between number of particles and moles, Avogadro\u2019s number acts as a conversion factor.<\/p>\n\n\n\n

Let\u2019s apply this to the question: How many moles are in 3.4 \u00d7 10\u00b2\u00b3 molecules of ammonia (NH\u2083)?<\/strong><\/p>\n\n\n\n

To find the number of moles, divide the number of molecules by Avogadro\u2019s number:3.4\u00d710236.022\u00d71023\u22480.564 moles\\frac{3.4 \\times 10^{23}}{6.022 \\times 10^{23}} \\approx 0.564 \\text{ moles}6.022\u00d710233.4\u00d71023\u200b\u22480.564 moles<\/p>\n\n\n\n

This calculation shows that 3.4 \u00d7 10\u00b2\u00b3 molecules of NH\u2083 is equal to about 0.564 moles<\/strong>.<\/p>\n\n\n\n

Why It Works:<\/h3>\n\n\n\n
    \n
  • You\u2019re converting from molecules (a count)<\/strong> to moles (an amount of substance)<\/strong>.<\/li>\n\n\n\n
  • The unit \u201cmolecules\u201d cancels out<\/strong>, and you\u2019re left with the unit \u201cmoles\u201d.<\/li>\n\n\n\n
  • This type of dimensional analysis ensures accuracy and consistency.<\/li>\n<\/ul>\n\n\n\n

    Tip:<\/h3>\n\n\n\n

    Always remember:<\/p>\n\n\n\n

      \n
    • Multiply<\/strong> when converting from moles to particles<\/strong>.<\/li>\n\n\n\n
    • Divide<\/strong> when converting from particles to moles<\/strong>.<\/li>\n<\/ul>\n\n\n\n

      This simple rule helps avoid confusion and ensures correct application of Avogadro\u2019s number in any mole-particle conversion.<\/p>\n\n\n\n

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

      How many molecules are there in 4.00 moles of glucose, C6H12O6? 4.00 moles = 4.00 x 6.022 x 10^23 molecules = 2.4088 x 10^24 molecules When the units are set up properly, the unit you are converting FROM will cancel out: You are left with the desired unit you are converting TO. 3. How many […]<\/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-230915","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230915","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=230915"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230915\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=230915"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=230915"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=230915"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}