{"id":193569,"date":"2025-02-20T17:56:38","date_gmt":"2025-02-20T17:56:38","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=193569"},"modified":"2025-02-20T17:56:59","modified_gmt":"2025-02-20T17:56:59","slug":"how-many-molecules-are-there-in-2-3-grams-of-nh4so2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/20\/how-many-molecules-are-there-in-2-3-grams-of-nh4so2\/","title":{"rendered":"How many molecules are there in 2.3 grams of NH4SO2"},"content":{"rendered":"\n
How many molecules are there in 2.3 grams of NH4SO2?<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n
To determine the number of molecules in 2.3 grams of ammonium bisulfite (NH4SO2), we need to go through several steps involving molar mass and Avogadro’s number.<\/p>\n\n\n\n
Steps:<\/h3>\n\n\n\n\n
Determine the molar mass of NH4SO2.<\/strong> The formula for ammonium bisulfite is NH4SO2. We need to calculate the molar mass by adding the atomic masses of each element involved:<\/li>\n<\/ol>\n\n\n\n
Convert grams to moles.<\/strong> To find the number of moles in 2.3 grams of NH4SO2, divide the given mass by the molar mass: [ \\frac{2.3 \\, \\text{g}}{82.112 \\, \\text{g\/mol}} = 0.02805 \\, \\text{mol} ]<\/li>\n\n\n\n
Determine the number of molecules.<\/strong> Avogadro’s number (6.022 \u00d7 10\u00b2\u00b3 molecules per mole) tells us how many molecules are in one mole. To find the number of molecules, multiply the moles by Avogadro’s number: [ 0.02805 \\, \\text{mol} \\times 6.022 \\times 10^{23} = 1.69 \\times 10^{22} \\, \\text{molecules} ]<\/li>\n<\/ol>\n\n\n\n
Final Answer:<\/h3>\n\n\n\n
There are approximately (1.69 \\times 10^{22}) molecules in 2.3 grams of NH4SO2.<\/p>\n\n\n\n
Explanation:<\/h3>\n\n\n\n
The calculation involves first determining the molar mass of the compound and then converting the given mass into moles. By using Avogadro’s number, which defines the number of particles in one mole, we can convert moles into molecules. This approach is foundational in chemistry for converting between grams, moles, and molecules.<\/p>\n\n\n\n
I will now generate an image to illustrate this process.<\/p>\n\n\n\n
Here is an illustration of the steps involved in calculating the number of molecules in a given mass of ammonium bisulfite (NH4SO2). It visually breaks down the process, showing how to calculate the molar mass, convert from grams to moles, and then multiply by Avogadro’s number to find the number of molecules.<\/p>\n\n\n\n
Let me know if you’d like any further clarification or help!<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"
How many molecules are there in 2.3 grams of NH4SO2? The Correct Answer and Explanation is : To determine the number of molecules in 2.3 grams of ammonium bisulfite (NH4SO2), we need to go through several steps involving molar mass and Avogadro’s number. Steps: Final Answer: There are approximately (1.69 \\times 10^{22}) molecules in 2.3 […]<\/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-193569","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/193569","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=193569"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/193569\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=193569"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=193569"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=193569"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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