{"id":182403,"date":"2025-01-13T18:40:04","date_gmt":"2025-01-13T18:40:04","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=182403"},"modified":"2025-01-13T18:40:09","modified_gmt":"2025-01-13T18:40:09","slug":"kmarks-profiles-tab-window-help","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/13\/kmarks-profiles-tab-window-help\/","title":{"rendered":"kmarks Profiles Tab Window Help"},"content":{"rendered":"\n

kmarks Profiles Tab Window Help<\/p>\n\n\n\n

Home – ?MyJaxState<\/p>\n\n\n\n

x||= ?Aktiv Link<\/p>\n\n\n\n

Aktiv Chemistry – ?Dimensional<\/p>\n\n\n\n

Question 1 ?of 19<\/p>\n\n\n\n

According to the balanced reaction below, calculate the quantity of<\/p>\n\n\n\n

gas<\/p>\n\n\n\n

that form when 4.20mol of N2H4 ?liquid completely reacts:<\/p>\n\n\n\n

3N2H4(l)?4,NH3(g)+N2(g)<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n

To calculate the quantity of gas produced when 4.20 mol of N2H4 (liquid) completely reacts, we need to analyze the balanced chemical equation and use stoichiometry.<\/p>\n\n\n\n

Step 1: Write the balanced chemical equation<\/h3>\n\n\n\n

The balanced chemical equation is:<\/p>\n\n\n\n

3N2H4(l)\u21924NH3(g)+N2(g)3N_2H_4(l) \\rightarrow 4NH_3(g) + N_2(g)<\/p>\n\n\n\n

This tells us that for every 3 moles of N2H4 (liquid), 4 moles of NH3 (gas) and 1 mole of N2 (gas) are produced.<\/p>\n\n\n\n

Step 2: Determine the mole ratio<\/h3>\n\n\n\n

We are given 4.20 mol of N2H4 (liquid), and we need to calculate the total moles of gases produced.<\/p>\n\n\n\n

From the balanced equation:<\/p>\n\n\n\n

    \n
  • 3 moles of N2H4 produce 4 moles of NH3 and 1 mole of N2.<\/li>\n<\/ul>\n\n\n\n

    The total number of moles of gas produced per 3 moles of N2H4 is: 4\u2009mol NH3+1\u2009mol N2=5\u2009mol of gas4 \\, \\text{mol NH}_3 + 1 \\, \\text{mol N}_2 = 5 \\, \\text{mol of gas}<\/p>\n\n\n\n

    Step 3: Set up a proportion to calculate the moles of gas produced<\/h3>\n\n\n\n

    If 3 moles of N2H4 produce 5 moles of gas, we can use a simple proportion to calculate the total moles of gas produced by 4.20 mol of N2H4. 3\u2009mol N2H45\u2009mol gas=4.20\u2009mol N2H4x\u2009mol gas\\frac{3 \\, \\text{mol N}_2H_4}{5 \\, \\text{mol gas}} = \\frac{4.20 \\, \\text{mol N}_2H_4}{x \\, \\text{mol gas}}<\/p>\n\n\n\n

    Solving for xx: x=5\u00d74.203=7.00\u2009mol of gasx = \\frac{5 \\times 4.20}{3} = 7.00 \\, \\text{mol of gas}<\/p>\n\n\n\n

    Step 4: Conclusion<\/h3>\n\n\n\n

    The total quantity of gas produced when 4.20 mol of N2H4 reacts completely is 7.00 mol. This gas is a combination of both NH3 (ammonia) and N2 (nitrogen gas), as described in the balanced equation. The total molar quantity of gas is simply the sum of the individual gases produced.<\/p>\n","protected":false},"excerpt":{"rendered":"

    kmarks Profiles Tab Window Help Home – ?MyJaxState x||= ?Aktiv Link Aktiv Chemistry – ?Dimensional Question 1 ?of 19 According to the balanced reaction below, calculate the quantity of gas that form when 4.20mol of N2H4 ?liquid completely reacts: 3N2H4(l)?4,NH3(g)+N2(g) The correct answer and explanation is: To calculate the quantity of gas produced when 4.20 […]<\/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-182403","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182403","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=182403"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182403\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=182403"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=182403"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=182403"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}